Definitions And Mcqs Of Ninth Class Chemistry 28w5x
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Chapter 1 Introduction to Chemistry (Tungsten is not illuminating until given voltage; you are not beautiful until skilled)
Chemistry Def. & MCQs 1
Dr. Sajid Ali Talpur
Definitions 1. Chemistry: - It is the branch of science, which deals with the properties, composition, and the structure of matter. It also deals with the changes in matter and the principles, which govern these changes. OR “The scientific study of matter is called chemistry” 2. Matter: - Anything having mass and volume is called matter. 3. Mass: - The quantity of matter contained in a body is called mass. 4. Volume: - Volume is the quantity of three dimensional space occupied by the matter. OR
Chemistry Def. & MCQs 2
Dr. Sajid Ali Talpur
Volume (also called capacity) is quantification of how much space an object occupies. 5. Space: - The free area between two material objects is called space. 6. Hypothesis: - It is the intelligent guess of the scientist about any phenomenon. 7. Phenomenon: - Any observable event is called phenomenon. 8. Theory: -The scientifically acceptable idea or principle to explain a phenomenon is called theory. 9. Organic compounds:- Those compounds which contains carbon and hydrogen covalently bounded with each other are called organic compounds 10. Physical Chemistry: - The scientific study of the laws and the principles governing the combination of atoms and molecules in chemical reactions is called Physical Chemistry. 11. Organic Chemistry: - The scientific study of organic compounds is called organic chemistry. 12. Inorganic Chemistry: - The scientific study of inorganic compounds is called inorganic chemistry.
Chemistry Def. & MCQs 3
Dr. Sajid Ali Talpur
13. Analytical Chemistry: - The scientific study of kind, quantity and quality of various components in a given substance is called analytical chemistry. 14. Biochemistry: - The scientific study of the compounds and their reactions within the living organisms is called biochemistry. 15. Industrial Chemistry: - The scientific study of the chemical industries and the synthetic products like glass, cement, soap etc over there is called industrial chemistry. 16. Nuclear Chemistry: - The scientific study of the changes occurring in the nuclei of atoms, accompanied by the emission of invisible radiations is called nuclear chemistry. 17. Environmental Chemistry: - The scientific study of interaction of chemical materials and their effect on the environment is called environmental chemistry 18. Polymeric Chemistry: - The scientific study of polymerization and the products obtained through the process of polymerization such as plastics, synthetic fibers, papers etc is called polymeric chemistry.
Chemistry Def. & MCQs 4
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Multiple Choice Questions 1. Chemistry is the study of: a) matter b) energy c) both a & b d) life e) N.O.T 2. The Muslim period ranges from: a) 347 – 428 B.C b) 600 – 1600 A.D c) 600 – 1000 A.D d) 1600 to today 3. Known as the father of Al-Chemy. a) Jabir bin Hayan b) Al Razi c) Ibne Sina d) Al Beruni 4. Known as the father of Modern Chemistry a) Jabir bin Hayan b) Robert Boyle c) Mendeleef d) Cavendish Chemistry Def. & MCQs 5
Dr. Sajid Ali Talpur
5. First used opium as anaesthesia. a) Jabir Bin Hayan b) Al Razi c) Ibne Sina d) Al Beruni 6. ____,____,and____discovered oxygen, chlorine and hydrogen respectively. a) J. Black, J.Priesly, Scheele b) Scheele, J. Priesly, Cavendish c) Cavendish, Lavoiser, Scheele d) J.Priesly, Scheele, Cavendish 7. Introduced first the idea of symbols: a) Gay Lussac b) Mendeleef c) Faraday d) J.J. Berzilius 8. Cholera, Typhoid, and Desentry are the dangerous disease transmitted through the impure water drinking. a) true b) false 9. Al Razi divided chemical substances on the basis of living and non-living origin. a) true b) false 10. Biochemistry is the basis of medical sciences. a) true b) false 11. PVC stands for poly vinyl carbon a) true b) false 12. Fluorine is the best disinfectant: a) true b) false
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13. Periodic arrangement is the result of Mendeleef’s work: a) true b) false Questions 14 – 19 Select from the below: a) Organic Chemistry b) Inorganic chemistry c) Biochemistry d) Analytical Chemistry e) N.O.T 14. Wood is studied in: 15. Blood, urine, proteins are studied in: 16. Iron is studied in: 17. Hydrocarbons and their derivatives are studied in: 18. It is the study of polymerization 19. It deals with the determination of kind, quality and quantity of various components in a given substance. 20. A wise guess of scientists is called hypothesis a) true b) false Answer Key 1 4 7
A B B
2 5 8
C B A
Chemistry Def. & MCQs 7
3 6 9
A D A
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10 13 16 19
A A B D
11 14 17 20
B A A A
12 15 18
B C E
Chapter 2 Chemical Combinations (You can neither stop nor save the time but can make every moment historical if you
Chemistry Def. & MCQs 8
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know the value of time)
Definitions 1. Atomic mass: - Atomic mass is defined as the mass of one atom of the element compared with the mass of one atom of C12 (the stable light isotope of carbon). 2. Molecular mass: - It is defined as the sum of atomic masses of the atoms of all the elements present in a molecule shown by its molecular formula. 3. Empirical formula mass/ formula mass: - It is the sum of atomic masses as given in the simplest (empirical) formula of ionic compound Chemistry Def. & MCQs 9
Dr. Sajid Ali Talpur
4. Molecular formula: - The expression, showing types and actual number of atoms present in a compound, using symbols for component elements and numerals for number of atoms of each element per molecule, like C6H6 for benzene. 5. Empirical formula: - A chemical formula that indicates the relative proportions of the elements in a compound rather than the actual number of the atoms of the elements. 6. Mole: - One mole is gram atomic mass, gram molecular mass or gram formula mass of any substance (atoms, ions, molecules), which contains 6.02*1023 elementary entities. 7. Molar mass: - The mass of one mole is called molar mass. 8. Avagadro’s number: - The number of basic quantities as present in 12 grams of C12 i.e 6.02*1023
Multiple Choice Questions 1. Mass can not be created but can be destroyed. a) true b) false Chemistry Def. & MCQs 10
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2. Landolt experiment is performed to : a) law of conservation of mass b) law of definite proportions c) law of multiple proportions d) law of reciprocal proportions 3. The empirical formula of glucose is: a) CH b) CH2O c) C3H6O6 d) C6H12O6 4. The empirical formula mass of benzene is: a) 12 a.m.u b) 13 a.m.u c) 78 a.m.u d) N.O.T 5. Molecular mass of sodium is: a) 11 a.m.u b) 12 a.m.u c) 23 a.m.u d) N.O.T 6. ______moles are there In 50 g of CaCO3. a) 0.5 b) 1 c) 1.5 d) 1.5 7. 3 moles of Carbon are equal to: a) 4g b) 36g c) 132g d) 18.06*1023 8. Zn + HCl → ZnCl2 + H2. The reaction is an example of: a) decomposition reaction b) addition reaction c) single displacement reaction d) double displacement reaction e) combustion reaction
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9. Chemical equation is a short hand method for describing a compound. a) true b) false 10. Combustion reaction consumes heat: a) true b) false The book MCQs 11. mass is neither created nor destroyed during a chemical reaction is the statement of: a) law of conservation of mass b) law of definite proportions c) law of multiple proportions d) law of reciprocal proportions 12. a given compound always contains exactly the same proportion of elements by mass is the statement of: a) law of conservation of mass b) law of definite proportions c) law of multiple proportions d) law of reciprocal proportions 13. the average mass of natural mixture of isotopes, which is compared to the mass of one atom of C-12 a.m.u is called: a) atomic number b) atomic mass c) mass number d) molecular mass 14. a formula that gives only the relative number of each type of atoms in a molecule is called: Chemistry Def. & MCQs 12
Dr. Sajid Ali Talpur
a) empirical formula c) molecular mass
b) molecular formula d) formula mass
15. a formula that indicates actual number and type of atoms in a molecule is called: a) empirical formula b) molecular formula c) molecular mass d) formula mass 16. the sum of atomic masses of all atoms in a molecule is called: a) empirical formula b) molecular formula c) molecular mass d) formula mass 17. the sum of atomic masses of all atoms in a formula unit: a) empirical formula b) molecular formula c) molecular mass d) formula mass 18. the mass of one mole of a substance expressed in grams is called: a) empirical formula b) molecular formula c) molecular mass d) molar mass 19. 44 a.m.u of CO2 is equal to: a) formula mass b) atomic mass c) molecular mass d) molar mass 20. 5 moles of H2O are equal to: a) 80g b) 90g c) 100g d) 90a.m.u Answer Key
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1 4 7 10 13 16 19
B B B B B C C
Chapter 3
2 5 8 11 14 17 20
A D C A A D D
3 6 9 12 15 18
B A B B B D
Atomic Structure
(Neither take rest nor be the time waste, Because life is the test and only heaven is the rest) Chemistry Def. & MCQs 14
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Definitions 1. Atom: -The building block of the matter that takes part in the reaction. OR The smallest component of an element having the chemical properties of the element, consisting of a nucleus and surrounding shells. 2. Nucleus: -the central part of the atom comprising the mass of the atom conferred by protons and neutrons, initially discovered by RUTHERFORD.
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3. Shell or energy level: -according to Bohr these are the circular orbits at certain distance from the nucleus where electrons exist. 4. Atomic number (Z): -The number of protons in nucleus is called the atomic number of the element. 5. Atomic mass: - The total number of protons and neutrons in nucleus constitute its atomic mass. 6. Element: -The simplest matter whose all atoms have same atomic number and can not be further simplified is called element. 7. Crook’s discharge tube experiment: indicates the existence of protons and electrons in the atom 8. Cathode rays: -the rays which consist of electrons and are produced when the current is ed through gases at low pressure are called cathode rays. 9. Properties of cathode rays (electrons): Discovered by J.J THOSMSON Carry a negative charge equal to 1.6*1019 C=4.803*10-10 Their e/m ratio is 1.76*108 C/g Their mass is 9.11*10-31 kg = 0.00055a.m.u They can be deflected by electromagnetic field.
Chemistry Def. & MCQs 16
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These don’t depend upon the material of which the electrode is made nor of the gas which is enclosed inside the tube. 10. The properties of canal rays ( protons): GOLDSTIEN discovered them. These rays carry positive charge They travel in straight line The value of e/m depends upon the gas enclosed The mass is 1.67*10-27kg=1.0073amu They are composed of heavy particles than electrons. 11. The properties of neutrons: Discovered by CHADVICK. They are neutral, carrying no charge. The mass is same as that of proton but slightly heavier. i.e. 1.0087 a.m.u. It is highly energetic particle. 12. Radioactivity: -the spontaneous emission of radiations by certain elements is called radioactivit 13. Isotopes: - Atoms of the same elements, having the same atomic number but the different atomic masses are called isotopes. 14. Spectrum: -the band of colors formed through the dispersion of light is called spectrum.
Chemistry Def. & MCQs 17
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15. Electronic configuration: - the arrangement or distribution of electrons in the available orbitals is called electronic distribution. 16. Atomic radius: -the half of the bond length, taken between two homonuclear diatomic molecules. OR the distance from nucleus to the valence electron is called atomic radius. 17. Ionic radius: -the radius of an ion. 18. ion: -the charged atom is called ion
19. Cation: -the positively charged ion is called cation. 20. Anion: -the negative charged ion is called anion. 21. Ionization potential: -the energy required to make an atom ion is called ionization potential. 22. Electron affinity: -the amount of energy released when an electron is added to a neutral gaseous atom to form a negative ion is called electron affinity. 23. Electronegativity: - the force with witch an atom attracts the shared pair towards itself is called electronegativity.
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Multiple Choice Questions 1. The first atomic theory was proposed by: a) Democritus b) Greek Philosophers c) both a & b d) John Dalton 2. According to modern theory, all elements are made up of small, indivisible, indestructible particles called atoms a) true b) false
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3. Protons and neutrons were discovered by respectively: a) J.J Thomson, Chadwick b) Chadwick, J.J Thomson c) Goldstein, Chadwick d) Chadwick, Goldstein 4. Electrons are the constituent of all matter. a) true b) false 5. The incorrect statement regarding the cathode rays is: a) material particles b) e/m ratio is different c) possess K.E d) N.O.T 6. Electrons do not depend upon the the nature of the cathode and the gas inside the tube. a) true b) false 7. e/m ratio of electron is: a) 1.76*108 C/g b)1.76*1011C/g c) 1.602*10-19 C/g d) 1.672*10-27C/g 8. The Charge on electron is: a) 1.76*108 C b)1.76*1011C c) 1.602*10-19 C d) 1.672*10-27C 9. The charge on proton is: a) 1.76*108 b)1.76*1011C c) 1.602*10-19 C d) 1.672*10-27C Chemistry Def. & MCQs 20
Dr. Sajid Ali Talpur
10. 1 a.m.u =? a) 1.76*108 g c) 1.602*10-19 g
b)1.76*1011g d) 1.672*10-27g
11. Atom was proved divisible particle by: a) cathode rays b) radioactivity c) discharge tube exp. d) A.O.T 12. Electron is 1836 times heavier than proton. a) true b) false 13. Radioactivity was discovered by: a) Henry Bequeral b) Rutherford c) Bohor d) J.J Thomson 14. Rutherford used particles in his experiment. a) α – particles b) β – particles c) γ – particles d) A.O.T 15. The α-particles deflected back by striking the atom because of the presence of: a) shells b) nucleus c) protons d) electrons 16. Energy is …… when an electron jumps from higher energy level to lower energy level. a) absorbed b) released c) neither absorbed nor released d) both a & b
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17. This of the following particles takes part in the reaction. a) electron b) proton c) neutron d) A.O.T 18. The correct equation is: a) E2 - E1 = hυ b) E2 + E1 = hυ c) E2 * E1 = hυ d) E2 / E1 = hυ 19. Na has: a) 11 electrons c) 12 neutrons
b) 11 protons d) A.O.T
20. Mass number = a) protons + electrons b) protons + neutrons c) electrons + neutrons d) no. of protons.
21. Atomic number = a) protons + electrons b) protons + neutrons c) electrons + neutrons d) no. of protons. 22. The positively charged particles in radioactivity are protons. a) true b) false 23. Isotopes have different number of: Chemistry Def. & MCQs 22
Dr. Sajid Ali Talpur
a) electrons c) neutrons
b) protons d) A.O.T
24. Proteum has one proton and no neutron. a) true b) false 25. Isotopes are used in the treatment of diseases. a) true b) false 26. The formula to find out max number of electrons is: a) n2 b) 2n c) 2n2 d) N.O.T 27. When n=3 the max electrons in a shell should be. a) 3 b) 6 c) 9 d) 18 28. The max. number of electrons in 4th shell is: a) 4 b) 8 c) 16 d) 32 29. Find the mis match a) electrons : J.J Thomson b) protons : nucleus c) neutrons : atomic mass d) protons : atomic number 30. The correct statement is: a) A = Z+A b) A=Z-N c) A=N-Z d) Z=A-N 31. Which isotope of oxygen forms ozone Chemistry Def. & MCQs 23
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a) O16 c) O18
b) O17 d) O19 Answer Key
1 4 7 10 13 16 19 22 25 28 31
D A A D A B D C A D C
2 5 8 11 14 17 20 23 26 29
B A C B B B B A C A
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3 6 9 12 15 18 21 24 27 30
C B C B A A D A D D
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Chapter 4 Periodicity of Elements (People are bad enough to tease you but I am sure you are good enough to forgive them)
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Definitions 1. Periodicity: - The repetition of properties of elements after some interval is called periodicity. 2. Periods: - The horizontal rows in the periodic table are called periods. 3. Groups: - The vertical columns in the periodic table are called groups. 4. Metals: -Those elements which conduct heat and electricity and become positively charged by loosing electrons are called metals. 5. Non metals: -Those which do not conduct heat and electricity and become negatively charged by accepting electrons are called non metals 6. Metalloids: - These have the mixed properties of metalloids. 7. Atomic radius: -the half of the bond length, taken between two homonuclear diatomic molecules. OR the distance from nucleus to the valence electron is called atomic radius. 8. Ionic radius: -the radius of an ion. 9. ion: -the charged atom is called ion
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10. Cation: -the positively charged ion is called cation. 11. Anion: -the negative charged ion is called anion. 12. Ionization potential: -the energy required to make an atom ion is called ionization potential. 13. Electron affinity: -the amount of energy released when an electron is added to a neutral gaseous atom to form a negative ion is called electron affinity. 14. Electronegativity: - the force with witch an atom attracts the shared pair towards itself is called electronegativity.
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Multiple Choice Questions 1. Law of triads was proposed by: a) Doberinier b) Lother Mayer c) Newland d) Mendeleef 2. Modern classification is based on atomic number. a) true b) false 3. law of octaves was proposed by: a) Doberinier b) Lother Mayer c) Newland d) Mendeleef 4. Mg being eighth element from Be has the similar properties with it. The statement comes from: a) law of octaves b) law of triads c) Lother Mayer’s classification d) Mendeelev’s periodic table 5. atomic volume = ? a) gram atomic Weight * density b) gram atomic Weight / density c) gram atomic weight + density d) gram atomic weight – density 6. Mendeleev arranged the elements in order of increasing: a) atomic volume b) atomic mass c) atomic number d) periodicity
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7. Mendeleev’s periodic table was remarkable in having: a) columns b) rows c) both d) gaps for unknown elements 8. Mendeleev’s periodic table failed to give the idea of atomic structure. a) true b) false 9. regarding the periodic table the incorrect statement is: a) rows have similar properties b) it does not contain isotopes c) shows the periodicity of elements d) N.O.T 10. Eka boran was later termed as: a) boron b) scandium c) gallium d) germanium 11. …..proved atomic mass not as the fundamental property of elements: a) radioactivity b) isotopes c) electronic configurationd) periodicity 12. atomic number was discovered by: a) doberinier b) newland c) baquerel d) mosely 13. the longest period is: a) first c) sixth
b) second d) seventh
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14. the sixth period contains: a) 6 b) 8 c) 16 d) 32 15. the elements of sub group A are called transition elements. a) true b) false 16. group 1A and 2A contain alkali metals: a) true b) false 17. the most stable of the following elements is: a) Na b) N2 c) Ni d) Ne 18. the most reactive is: a) Na c) Na+
b) Mg d) F
19. The valency of seventh A group is : a) +1 b)-1 c) +2 d)-2 20. boron is metalloid: a) true
b) false.
21. it exists in tetameric form: a) K b) P c) N d) Sb 22. inert or noble gases are placed in the group: a) 3A b) 4A c) 7A d) 8A Chemistry Def. & MCQs 30
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23. electronegativity of fluorine is: a) 1 b) 2 c) 3 d) 4 24. the minimum energy required to remove an electron from an atom in gaseous state is called: a) electronegativity b) electron affinity c) ionization potential d) P.E 25. 1Å = ? a)10-8 c)10-7
b) 10-9 d) 10-10
26. atomic number depends upon the number of shells but does not depend upon the nuclear charge. a) true b) false 27. the energy change that occurs when an electron is gained by an atom in gaseous state is called: a) electron affinity b) ionization potential c) enthalpy d) electronegativity 28. the relative tendency of an atom in a molecule to attract shared pair of electrons towards itself is called: a) electron affinity b) ionization potential c) enthalpy d) electronegativity 29. electronegativity decreases down the group. a) true b) false
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30. the incomplete period is: a) first b) fourth c) sixth d) seventh 31. which period contains only gases a) first b) fourth c) sixth d) seventh 32. it is the radioactive element of 1A group. a) Li b) Rb c) Cs d) Fr 33. the valency of alkaline earth metals is: a) +1 b) +2 c) -1 d) -2 34. N and P are non metals. a) true b) false 35. which pair of elements is chemically similar: a) K, Cr b) Cu, Ca c) F, Cl d) N, O
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Answer Key 1 4 7 10 13 16 19 22 25 28 31 34
A A D B C B B D A D A A
2 5 8 11 14 17 20 23 26 29 32 35
A B A A D D A D B A D C
Chemistry Def. & MCQs 33
3 6 9 12 15 18 21 24 27 30 33
C B A D B C B C A D B
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Chapter 5 Chemical Bonding (The future will take revenge if you spoil the present)
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Definitions 1. Chemical bond: - The attractive force that holds atoms together in a compound is called chemical bond. 2. Ionic or electrovalent bond: - It is defined as the electrostatic force of attraction between positive and negative ions. 3. Covalent bond: - Achemical bond that involves the sharing of electrons is called covalent bond. 4. Single covalent bond (—): -such a bond is formed when one electron is contributed from each atom making one shared pair. E.g. Cl2 5. Double covalent bond: -in such a covalent bond each of the two atoms contribute two electrons as in O2 6. Triple covalent bond: -in triple covalent bond each atom contributes three electrons as in N2 7. Co-ordinate or dative covalent bond: -a covalent bond in witch one of the bonded atoms furnishes both of the shared electrons. 8. Hydrogen bond: - it is an electrostatic force of attraction between a partially positive hydrogen atom of one molecule and the electronegative atom of the other molecule Chemistry Def. & MCQs 35
Dr. Sajid Ali Talpur
9. Metabolic Bond: - It is defined as the force of attraction between electrons and the positive nuclei of atoms. 10. Dispersion Forces: The dispersion forces are the weak attractive forces between temporarily polarized atoms (or molecules) caused by the varying positions of the electrons during their motion about the nuclei 11. Dipole moment: - the measure of the degree of the polarity of a polar compound is called dipole moment. 12. Electronegativity: - It is the power of an atom to attract shared pair of electrons towards itself. 13. Bond pairs electrons: - also called active set of electrons they take part in bond formation and are incorporated as shared pair. 14. Lone pair of electrons: - also called non bonding pairs, are paired electrons but don’t take part in bonding.
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Multiple Choice Questions: 1. The force which holds atoms together in a molecule or crystal is called a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 2. the energy in a molecule is less than the atoms. a) true b) false 3. the electrons in the innermost shell are called valence electrons. a) true b) false 4. the bond formed by sharing of electrons is called: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 5. the bond formed by the complete transfer of electrons: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 6. the gases like oxygen, nitrogen, are the result of: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 7. MgO is an example of: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent
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8. the idea of chemical bond was introduced in a) 1808 b) 1910 c) 1816 d) 1916 9. ionic compounds don’t possess molecular formula. a) true b) false 10. the atom that donates electrons becomes negatively charged: a) true b) false 11. which one is the stable: a) Na b) Na+ ++ c) Na d) Na12. ionic compounds are good conductors of electricity: a) true b) false 13. covalent compounds are soluble in water: a) true b) false 14. ionic compounds form the molecules of high molecular weight. a) true b) false 15. all are correct about ionic bond except: a) they conduct electricity in all the states b) they are soluble in polar solvents c) ionic compounds do not form molecules d) N.O.T
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Questions 16 – 18 •
Select from the below: A) single covalent bond B) double covalent bond C) triple covalent bond D) ionic bond E) N.O.T
16. the bond in hydrogen molecule is: 17. the bond in nitrogen molecule is: 18. the bond in CaCl2 is: 19. HCl is an example of: a) ionic bond b) covalent bond c) polar covalent bond d) non-polar 20. Cl- contains electrons in it: a) 1 b) 2 c) 7 d) 8
Questions 21 – 33 •
Select from the below
A) covalent bond B) polar covalent bond C) non polar covalent bond D) ionic bond E) co-ordinate covalent bond F) N.O.T
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21. The bond in oxygen molecule is 22. both the electrons are shared by one electrons: 23. also called electrovalent bond: 24. the bond in the table salt 25. the bond in NH4Cl 26. e.n > 1.7 27. the e.n = 0 28. involves the sharing of electrons: 29. formed by sharing of electrons between dissimilar atoms 30. formed by sharing of electrons between similar atoms. 31. lone pair of electrons is the indication of the bond 32. the attraction between electrons and nuclei. 33. the greatest electronegativity difference is present in: 34. metals are solids except bromine a) true b) false Chemistry Def. & MCQs 40
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35. metals conduct heat and electricity because of the presence of: a) fixed electrons b) free electrons c) fixed protons d) free protons 36. inter molecular forces hold atoms together in a molecule: a) true b) false 37. all of the following are wander wall’s forces except: a) dispersion forces b) covalent bond c) dipole-dipole forces d) H-bonding 38. inter molecular forces are much weaker than intra molecular forces. a) true b) false
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Answer Key 1 4 7 10 13 16 19 22 25 28 31 34 37
A B C B B A C E E A E B B
2 5 8 11 14 17 20 23 26 29 32 35 38
A C D B B C D D D B F B B
Chemistry Def. & MCQs 42
3 6 9 12 15 18 21 24 27 30 33 36 39
B B A B A D C D C C D B
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Chapter 6
States of matter
(Every action has reaction, yes exactly if you can not please your books how you will be
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pleased)
Definitions 24. Matter: - Any thing having mass and volume is called matter. 25. Solid: - The state of matter having specific shape and volume 26. Liquid: - The state of matter having specific volume but not the shape. 27. Gas: - It is the state of matter having neither specific volume nor the shape 28. Diffusion: - the distribution or spreading of the gas molecules throughout the vessel is known as Chemistry Def. & MCQs 44
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diffusion. OR the mixing and merging of the molecules with each other is called diffusion 29. Pressure: -force per unit area. 30. Temperature: - the degree of hotness or coldness of a body is called temperature. 31. Heat: - it is the form of energy that produces sense of warmth and flows from hot body to cold body. 32. Density: - the mass unit volume is called density. (d=M/V) 33. Vapour pressure: - it is the pressure exerted by the vapors on the surface of liquid when rate of condensation exceeds the rate of evaporation. 34. Boiling: - when vapour pressure of liquid equals the atmospheric pressure, the bubbles of vapour form easily and rise to the surface. The liquid is said to boil. 35. Boiling point: -it is the temperature at which boiling starts. 36. Melting: - conversion of a solid into liquid. 37. Melting point: - it is the temperature at which melting begins to take place.
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Dr. Sajid Ali Talpur
38. Sublimation: -the process of conversion of solids directly into gases form without ing through the liquid state is called sublimation. 39. Phenomenon: -an observable event. 40. The latent heat of fusion: - heat required during conversion of the state. OR the heat energy required converting 1g of a solid into liquid at its melting point. 41. Brownian motion: - A continuous, zigzag motion of suspended particles through the medium is called Brownian motion.
Multiple Choice Question 1. Any thing having mass and volume is not called called a) power b) energy c) both a & b d) matter 2. The quantity of matter in a body is called a) mass b) energy c) matter d) volume 3. According to K.M.T all are true except: a) molecules are always in motion: b) they possess K.E c) they possess P.E d) molecules are very tiny particles e) N.O.T Chemistry Def. & MCQs 46
Dr. Sajid Ali Talpur
4. The space occupied by an object is called a) mass b) energy c) volume d) matter 5. Regarding gases all are true except: a) K.E very low b) intermolecular space very high c) neither shape nor volume d) molecules move in all directions. 6. The liquids have constant shape but not volume. a) true b) false 7. The spreading of a substance through a medium is called: a) diffusion b) Brownian motion c) effusion d) fusion 8. A continuous, rapid, zigzag motion of suspended particles through the medium is called Brownian motion. a) true b) false 9. Water can exist in all the three states of matter. a) true b) false The Book MCQs 10. The number of common states of matter is: a) 3 b) 4 c) 5 d) N.O.T
Chemistry Def. & MCQs 47
Dr. Sajid Ali Talpur
11. Neither definite shape nor volume is the property of: a) solids b) liquids c) gases d) N.O.T 12. The temperature at which the vapour pressure of a liquid becomes equal to its external pressure is called: a) melting point b) boiling point c) triple point d) freezing point 13. The state of matter in which molecules are tightly packed and possess only vibratory motion is: a) solid state b) liquid state c) gaseous state d) N.O.T 14. The process in which molecules escape from the surface of liquid is called: a) sublimation b) evaporation c) boiling d) melting 15. the process in which solid directly changes to gas is called a) sublimation b) evaporation c) boiling d) melting
Answer Key 1 4
C C
2 5
A A
Chemistry Def. & MCQs 48
3 6
C B
Dr. Sajid Ali Talpur
7 10 13
A A A
8 11 14
B C B
9 12 15
A B A
Chapter 7 Solution and Suspension (Solving the problems is the solution of problems than increasing the problems by
Chemistry Def. & MCQs 49
Dr. Sajid Ali Talpur
worrying on the problems…!)
Definitions 1. Solution: -the homogeneous mixture of two or more things. 2. Solute: - It is the component of solution present in smaller amount and is dissolved by the solvent. 3. Solvent: - It is the component of solution present in greater amount and dissolves the solute. 4. Unsaturated solution: - It is that one solution which contains less solute than it has the capacity to dissolve. Chemistry Def. & MCQs 50
Dr. Sajid Ali Talpur
5. Saturated solution: - It is that one solution which contains maximum amount of solute and can not dissolve more solute at a given temperature 6. Super saturated solution: - It is that one solution which contains more solute than the normal capacity and this is done usually by increasing temperature. 7. Crystallization: - The process in which dissolved solute comes out of solution and forms crystals is called crystallization. 8. Molarity: - The number of moles of solute dissolved in 1 liter (1dm3) of a solution is called molarity. It is denoted by (M). 9. Molality : - The number of moles of solute dissolved in 1 kilogram of solution is called molality. It is denoted by (m). 10. Mole fraction: - Mole fraction of any component in a solution is the number of moles of the component divided by total number of moles making up solution. It is denoted by X. 11. Suspension: - It is defined as a heterogenous mixture consists of visible particles which remain suspended in the liquid.
Chemistry Def. & MCQs 51
Dr. Sajid Ali Talpur
Multiple Choice Questions 1. A heterogeneous mixture of two or more substances is called solution: a) true b) false 2. there are types of solutions a) 2 b) 3 c) 5 d) 9 3. The composition of air is as a) 78% N2, 21% O2, 1% Ar. b) 78% N2, 15% O2, 5% CO2, 1 other gases c) 78% N2, 21% O2, 1% other gases d) all are possible 4. alloys are the mixture of: a) solid-solid b) solid-liquid c) liquid-gas d) solid-gas Chemistry Def. & MCQs 52
Dr. Sajid Ali Talpur
5. which of the following does not affect the solubility: a) temperature b) size of particles c) pressure d) nature of solute e) nature of solvent 6. the solubility of gases increases with the increase in temperature. a) true b) false 7. Only the solubility of is affected by pressure. a) solids b) liquid c) gases d) plasma 8. ionic compounds are not dissolved in: a) polar solvent b) non-polar c) water d) A.O.T 9. A solution which has the capacity to dissolve more solute is called: a) saturated solution b) unsaturated solution c) super saturated d) N.O.T 10. the process in which the dissolved solute comes out of the solution is called: a) titration b) solubility c) crystallization d) N.O.T 11. what is the molarity of a solution when 10 g NaOH are dissolved in 1 liter solution: a) 0.25M b) 0.5M c) 1M d) 2M
Chemistry Def. & MCQs 53
Dr. Sajid Ali Talpur
The Book MCQs 12. the suspended particles in the suspensions are generally of the size: a) 10nm b) 100nm c) 1000nm d) 1200nm 13. the sum of mole fraction of solute and solvent is equal to: a) 1 b) 2 c) 3 d) 4 14. solubility is defined as the amount of solute in gram at a given temperature, dissolved in …… of the solvent. a) 10g b) 20g c) 100g d)1000g 15. the process in which solid directly changes to vapours is called. a) sublimation b) evaporation c) diffusion d) boiling 16. the solubility of gas …….with the rise in temperature. a) increase b) decrease Answer Key 1 4
B A
2 5
D B
Chemistry Def. & MCQs 54
3 6
C B
Dr. Sajid Ali Talpur
7 10 13 16
C C A B
Chapter 8
8 11 14
B A C
9 12 15
B C A
Thermochemistry
(To shine your face make nimaz (salah) base because life is race and in this case to fasten the pace don’t create mess)
Chemistry Def. & MCQs 55
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Definitions 12. Electrochemistry: - It is the branch of chemistry which deals with the relationship of electrical and chemical energies and their interconversion. 13. Electrolyte: -The substance capable of being dissociated into ions on the age of electricity in the molten state. 14. Non-eclectrolytes: - The chemical compounds which do not conduct electricity in molten or aqueous solutions are called non electrolytes.
Chemistry Def. & MCQs 56
Dr. Sajid Ali Talpur
15. Electrolysis: -The breakage of a solution on the age of electric current. 16. Anode: -the positively charged electrode where oxidation occurs. 17. Cathode: -the negatively charged electrode where reduction takes place is called cathode. 18. Ampere: - It is the S.I unit of current which is defined as the current when ed through a circuit for one second. 19. Columb: - It is the S.I unit of electric charge and is defined as the quantity of charge when one ampere of current is ed for one second. 20. Electroplating: - It is the process of electrolysis which is used to coat one metal onto the other. 21. Electrochemical cell: - The cell which is used to convert electrical energy into chemical energy and vice versa is called electrochemical cell. Multiple Choice Questions 1. Chemical and electrical energies are inter convertible: a) true b) false 2. all acids, bases and salts are electrolytes in aqueous solutions or fused state. Chemistry Def. & MCQs 57
Dr. Sajid Ali Talpur
a) true
b) false
3. all the conductors are electrolytes. a) true b) false 4. which of the following does not conduct electricity. a) salt b) water c) sugar d) N.O.T 5. all are true about cathode except: a) is negatively charged b) positive ions move towards it c) oxidation takes place over it d) Na+ ions become Na e) N.O.T 6. all are true about anode except: a) is positively charged b) oxidation takes place c) Cl becomes Cld) negative ions moves towards it e) N.O.T 7. Columb= ? a) current * time c) current + time
b) current / time d) current – time
8. 1F = ? a) 500C c) 96500C
b) 6500C d) 1000 C
Chemistry Def. & MCQs 58
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9. What is the charge when 2 A current es for 2 seconds: a) 1 b) 2 c) 3 d) 4 10. electrolysis is used for the extraction of certain metals from their ores. a) true b) false 11. coating of metal by non metal is called plating a) true b) false 12. a cell which converts electrical energy into chemical energy is called voltaic cell a) true b) false 13. lead storage battery is a reversible cell. a) true b) false Answer Key 1 4 7 10 13
A C A A A
2 5 8 11
A C C B
Chemistry Def. & MCQs 59
3 6 9 12
B C D B
Dr. Sajid Ali Talpur
Chapter 9 Acids, Bases and Salts (I do not own any business but the entire world is my own where Almighty Allah is to Chemistry Def. & MCQs 60
Dr. Sajid Ali Talpur
be felt and Muhammad (s.a.w) to be followed)
Definitions 22. Acid: -A compound having usually sour taste and capable of neutralizing alkalis and reddening blue litmus paper, containing hydrogen that can be replaced by a metal or any other electropositive atom to form salt, or containing an atom that can accept electrons from a base. 23. Base: - A base is a substance that can accept hydrogen ions or more generally, donates electrons pairs.
Chemistry Def. & MCQs 61
Dr. Sajid Ali Talpur
24. Salt: -the ionic substance that result from the neutralization of an acid with a base. 25. Ph: - A measure of the acidity or alkalinity of a solution, numerically equal to 7 for neutral solutions, increasing with increasing alkalinity and decreasing with increasing acidity. 26. Arrhenius Theory: It states that an acid can be defined as a substance that yields hydrogen ions when dissolved in water. A base can be defined as a substance which yields hydroxide ions when dissolved in water. 27. Bronsted Lowery Theory: It states that an acid is a substance having a tendency to donate one or more protons and a base is a substance having a tendency to accept protons. 28. Lewis Theory: It states that an acid is any species (molecule or ion) which can accept a pair of electrons and a base is any species (molecule or ion) which can donate a pair of electrons. 29. Titration: -titration is the quantitative measurement of an analyte in solution by completely reaction with reagent solution. Indicators: -color showing organic compounds. OR for acid-base titrations, organic compounds that exhibit different colors in solution of different acidities; used to determine the point at
Chemistry Def. & MCQs 62
Dr. Sajid Ali Talpur
which the reaction between two solutes is complete. 30. Buffer: -any substance that prevents changes in pH is known as buffer. 31. Neutralization: -when the two substances (acid and base) having opposed properties are allowed to react, salt and water are produced. The reaction is known as neutralization.
Multiple Choice Questions: 1. Ascorbic acid is the other name of: a) Vitamin A b) Vitamin B c) Vitamin C d) Vitamin D 2. all are the properties of acids except: a) sour in taste b) smooth in touch c) proton donor d) electrons acceptor 3. the common acid in stomach is: a) HCl b) H2SO4 c) HNO3 d) H3PO4 Chemistry Def. & MCQs 63
Dr. Sajid Ali Talpur
4. The consumption of …… is an index to the state of civilization and prosperity of a country: a) HCl b) H2SO4 c) HNO3 d) H3PO4 5. the important acid for making explosive materials and fertilizers is: a) HCl b) H2SO4 c) HNO3 d) H3PO4 6. the souring of milk produces. a) citric acid b) lactic acid c) acetic acid d) fumaric acid 7. lemon, oranges, grape fruits contain: a) citric acid b) lactic acid c) acetic acid d) fumaric acid 8. all are the properties of bases except: a) bitter in taste b) aqueous solution conducts electricity c) undergo neutralization with acids d) turn litmus paper to red. Q 9 – 14 Select from the below: a) Arrhenius Theory b) Bronsted –lowery c) Lewis concept d) N.O.T 9. Bases are proton acceptors. 10. acids are sour in taste Chemistry Def. & MCQs 64
Dr. Sajid Ali Talpur
11. acids are H+ ions donor 12. bases turn litmus paper to blue 13. ammonia is base 14. bases are electron donors 15. all are weak acids except: a) sulphuric acid b ) acetic acid c) formic acid d) phosphoric acid 16. which one is the normal salt: a) NaCl b) NaHSO4 c) KHCO3 d) Mg(OH) Cl 17. which one is not double salt: a) potash alum b) chrome alum c) Mohor’s salt d) table salt Q18 -22 Select from the below: a) Sodium carbonate b) backing soda c) copper sulphate d) Epsom salt e) potash alum f) N.O.T 18. it is a common double salt 19. used as antiacid and fire extinguishers 20. used as germicide, insecticide and in paint and varnish industry
Chemistry Def. & MCQs 65
Dr. Sajid Ali Talpur
21. it is used in softening of water, glass industry and as cleaning agent 22. used as anticeptic and mouth wash 23. water is not: a) universal solvent c) present in urine e) N.O.T
b) liquid d) amphoteric molecule
24. The number of moles of solute dissolved per liter of solution is: a) molarity b) molality c) titration d) pH 25. negative logarithm of hydrogen ion concentration is: a) molarity b) molality c) titration d) pH 26. it is important for an analytical chemist a) molarity b) molality c) titration d) pH Q 27 – 32 Select from the below a) 0 b) 5-7 c) 7 d) 7.4 e) 14 27. it is the neutral pH
Chemistry Def. & MCQs 66
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28. the pH of water is : 29. it is the highly acidic Ph 30. the pH of urine is: 31. the pH of blood is 32. pH + p OH = ? 33. Methyl orange produce…. Color in acidic solution a) red b) green c) yellow d) pink 34. a solution whose molarity or strength is known is called standard solution: a) true b) false 35. low p H of blood causes diabetes, diarrhea, vomiting. a) true b) false 36. water and CO2 are produced as a result of neutralization: a) true b) false Answer Key 1 4 7
C B A
2 5 8
B C D
Chemistry Def. & MCQs 67
3 6 9
A B B
Dr. Sajid Ali Talpur
10 13 16 19 22 25 28 31 34
D B A B E C D D A
11 14 17 20 23 26 29 32 35
A C D C E A E C B
12 15 18 21 24 27 30 33 36
D A E A C B A A B
Chapter 10 Chemical Energetics Chemistry Def. & MCQs 68
Dr. Sajid Ali Talpur
(The failure is the result of disobedience of first parents then teachers and finally of the Almighty Allah)
Definitions 1. Thermodynamics: -The study of conversion and conservation of heat and other forms of energy is called thermodynamics. 2. Thermochemistry: - it deals with the measurement or calculation of heat absorbed or abandoned in chemical reactions. 3. Thermo chemical reactions: - the chemical reactions which are accompanied by energy
Chemistry Def. & MCQs 69
Dr. Sajid Ali Talpur
changes along with the material changes are generally known as thermochemical reactions. 4. Exothermic reactions: -the chemical reactions which are accompanied by the liberations or emission of energy are called exothermic reactions. 5. Endothermic reactions: -the chemical reactions which are accompanied by the absorption of energy are called endothermic reactions. 6. system: -the collection of matter having certain boundaries is called system 7. Surroundings:- the environment of a system or the thing that affect on a system are included in surroundings. 8. Heat of formation: - the change of enthalpy when one gram mole of a substance is formed from its elements 9. Standard heat of formation: -the change of enthalpy when one gram mole of a substance is formed from its elements at 25oC and 1 atm is called standard heat of formation. 10. Enthalpy: -the total heat content of a system is called enthalpy..
Chemistry Def. & MCQs 70
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11. Heat of neutralization: - The amount of heat released during the neutralization process when one mole of water is produced by the reaction of acid and base.
Multiple Choice Questions 1. Thermochemical reactions involve: a) material changes b) energy changes c) both a & b d) heat changes 2. EXO means: a) out of or to evolve c) outside
b) into or to absorb d) heat
3. ∆H negative represents which reaction: a) thermochemical b) exothermic Chemistry Def. & MCQs 71
Dr. Sajid Ali Talpur
c) endothermic
d) chemical
4. Formation of water from hydrogen and oxygen produces energy: a) -286 K.J/mole b) +286 K.J/mole c) -393 K.J/mole d) +393 K.J/mole 5. ∆H positive represents neutralization: a) true b) false 6. Acid Base reaction is called neutralization reaction: a) true b) false
Questions 7 – 12 • Select from the below: A) endothermic reaction B)exothermic reaction 7. photosynthesis 8. respiration 9. decomposition reaction 10. bond formation 11. combustion 12. melting of ice The Book MCQs 13. in an exothermic reaction: a) heat energy is lost b) heat energy is gained Chemistry Def. & MCQs 72
Dr. Sajid Ali Talpur
c) both a & b
d) N.O.T
14. In an exothermic reaction: a) container becomes hot b) container becomes cold c) the temperature of container remains same d) N.O.T 15. During an endothermic reaction: a) container becomes cold b) container becomes hot c) the temperature of container remains same d) N.O.T Answer Key 1 4 7 10 13
C A A B A
2 5 8 11 14
A B B B A
3 6 9 12 15
B A A A A
By the same Author:
Chemistry Def. & MCQs 73
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Ninth Class Biology MCQs
How to be successful?
Definitions of chemistry
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Definitions and MCQs on branches of Biology
Definitions and MCQs of matric (10th class) Physics
Scientific Biological Reasons
Definitions, Scientific Reasons and MCQs on Chemistry
Skeletal muscles Physiology BCQs
What are goodness and badness?
Chemistry Def. & MCQs 74
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Biology MCQs test for entry test
Chemistry MCQs test for entry test
Cardiovascular system anatomy quiz
Lower limb anatomy quiz
Lower limb Anatomy MCQs
Spiritual successful life quotations
Why should one love the Prophet Muhammad (s.a.w)
Quotations on the Prophet Muhammad (s.a.w)
Chemistry Def. & MCQs 75
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The origin and future of human life
Endocrinology – Hormones MCQs
Islam, science, success and wisdom quotes
Chemistry Def. & MCQs 76
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Chemistry Def. & MCQs 1
Dr. Sajid Ali Talpur
Definitions 1. Chemistry: - It is the branch of science, which deals with the properties, composition, and the structure of matter. It also deals with the changes in matter and the principles, which govern these changes. OR “The scientific study of matter is called chemistry” 2. Matter: - Anything having mass and volume is called matter. 3. Mass: - The quantity of matter contained in a body is called mass. 4. Volume: - Volume is the quantity of three dimensional space occupied by the matter. OR
Chemistry Def. & MCQs 2
Dr. Sajid Ali Talpur
Volume (also called capacity) is quantification of how much space an object occupies. 5. Space: - The free area between two material objects is called space. 6. Hypothesis: - It is the intelligent guess of the scientist about any phenomenon. 7. Phenomenon: - Any observable event is called phenomenon. 8. Theory: -The scientifically acceptable idea or principle to explain a phenomenon is called theory. 9. Organic compounds:- Those compounds which contains carbon and hydrogen covalently bounded with each other are called organic compounds 10. Physical Chemistry: - The scientific study of the laws and the principles governing the combination of atoms and molecules in chemical reactions is called Physical Chemistry. 11. Organic Chemistry: - The scientific study of organic compounds is called organic chemistry. 12. Inorganic Chemistry: - The scientific study of inorganic compounds is called inorganic chemistry.
Chemistry Def. & MCQs 3
Dr. Sajid Ali Talpur
13. Analytical Chemistry: - The scientific study of kind, quantity and quality of various components in a given substance is called analytical chemistry. 14. Biochemistry: - The scientific study of the compounds and their reactions within the living organisms is called biochemistry. 15. Industrial Chemistry: - The scientific study of the chemical industries and the synthetic products like glass, cement, soap etc over there is called industrial chemistry. 16. Nuclear Chemistry: - The scientific study of the changes occurring in the nuclei of atoms, accompanied by the emission of invisible radiations is called nuclear chemistry. 17. Environmental Chemistry: - The scientific study of interaction of chemical materials and their effect on the environment is called environmental chemistry 18. Polymeric Chemistry: - The scientific study of polymerization and the products obtained through the process of polymerization such as plastics, synthetic fibers, papers etc is called polymeric chemistry.
Chemistry Def. & MCQs 4
Dr. Sajid Ali Talpur
Multiple Choice Questions 1. Chemistry is the study of: a) matter b) energy c) both a & b d) life e) N.O.T 2. The Muslim period ranges from: a) 347 – 428 B.C b) 600 – 1600 A.D c) 600 – 1000 A.D d) 1600 to today 3. Known as the father of Al-Chemy. a) Jabir bin Hayan b) Al Razi c) Ibne Sina d) Al Beruni 4. Known as the father of Modern Chemistry a) Jabir bin Hayan b) Robert Boyle c) Mendeleef d) Cavendish Chemistry Def. & MCQs 5
Dr. Sajid Ali Talpur
5. First used opium as anaesthesia. a) Jabir Bin Hayan b) Al Razi c) Ibne Sina d) Al Beruni 6. ____,____,and____discovered oxygen, chlorine and hydrogen respectively. a) J. Black, J.Priesly, Scheele b) Scheele, J. Priesly, Cavendish c) Cavendish, Lavoiser, Scheele d) J.Priesly, Scheele, Cavendish 7. Introduced first the idea of symbols: a) Gay Lussac b) Mendeleef c) Faraday d) J.J. Berzilius 8. Cholera, Typhoid, and Desentry are the dangerous disease transmitted through the impure water drinking. a) true b) false 9. Al Razi divided chemical substances on the basis of living and non-living origin. a) true b) false 10. Biochemistry is the basis of medical sciences. a) true b) false 11. PVC stands for poly vinyl carbon a) true b) false 12. Fluorine is the best disinfectant: a) true b) false
Chemistry Def. & MCQs 6
Dr. Sajid Ali Talpur
13. Periodic arrangement is the result of Mendeleef’s work: a) true b) false Questions 14 – 19 Select from the below: a) Organic Chemistry b) Inorganic chemistry c) Biochemistry d) Analytical Chemistry e) N.O.T 14. Wood is studied in: 15. Blood, urine, proteins are studied in: 16. Iron is studied in: 17. Hydrocarbons and their derivatives are studied in: 18. It is the study of polymerization 19. It deals with the determination of kind, quality and quantity of various components in a given substance. 20. A wise guess of scientists is called hypothesis a) true b) false Answer Key 1 4 7
A B B
2 5 8
C B A
Chemistry Def. & MCQs 7
3 6 9
A D A
Dr. Sajid Ali Talpur
10 13 16 19
A A B D
11 14 17 20
B A A A
12 15 18
B C E
Chapter 2 Chemical Combinations (You can neither stop nor save the time but can make every moment historical if you
Chemistry Def. & MCQs 8
Dr. Sajid Ali Talpur
know the value of time)
Definitions 1. Atomic mass: - Atomic mass is defined as the mass of one atom of the element compared with the mass of one atom of C12 (the stable light isotope of carbon). 2. Molecular mass: - It is defined as the sum of atomic masses of the atoms of all the elements present in a molecule shown by its molecular formula. 3. Empirical formula mass/ formula mass: - It is the sum of atomic masses as given in the simplest (empirical) formula of ionic compound Chemistry Def. & MCQs 9
Dr. Sajid Ali Talpur
4. Molecular formula: - The expression, showing types and actual number of atoms present in a compound, using symbols for component elements and numerals for number of atoms of each element per molecule, like C6H6 for benzene. 5. Empirical formula: - A chemical formula that indicates the relative proportions of the elements in a compound rather than the actual number of the atoms of the elements. 6. Mole: - One mole is gram atomic mass, gram molecular mass or gram formula mass of any substance (atoms, ions, molecules), which contains 6.02*1023 elementary entities. 7. Molar mass: - The mass of one mole is called molar mass. 8. Avagadro’s number: - The number of basic quantities as present in 12 grams of C12 i.e 6.02*1023
Multiple Choice Questions 1. Mass can not be created but can be destroyed. a) true b) false Chemistry Def. & MCQs 10
Dr. Sajid Ali Talpur
2. Landolt experiment is performed to : a) law of conservation of mass b) law of definite proportions c) law of multiple proportions d) law of reciprocal proportions 3. The empirical formula of glucose is: a) CH b) CH2O c) C3H6O6 d) C6H12O6 4. The empirical formula mass of benzene is: a) 12 a.m.u b) 13 a.m.u c) 78 a.m.u d) N.O.T 5. Molecular mass of sodium is: a) 11 a.m.u b) 12 a.m.u c) 23 a.m.u d) N.O.T 6. ______moles are there In 50 g of CaCO3. a) 0.5 b) 1 c) 1.5 d) 1.5 7. 3 moles of Carbon are equal to: a) 4g b) 36g c) 132g d) 18.06*1023 8. Zn + HCl → ZnCl2 + H2. The reaction is an example of: a) decomposition reaction b) addition reaction c) single displacement reaction d) double displacement reaction e) combustion reaction
Chemistry Def. & MCQs 11
Dr. Sajid Ali Talpur
9. Chemical equation is a short hand method for describing a compound. a) true b) false 10. Combustion reaction consumes heat: a) true b) false The book MCQs 11. mass is neither created nor destroyed during a chemical reaction is the statement of: a) law of conservation of mass b) law of definite proportions c) law of multiple proportions d) law of reciprocal proportions 12. a given compound always contains exactly the same proportion of elements by mass is the statement of: a) law of conservation of mass b) law of definite proportions c) law of multiple proportions d) law of reciprocal proportions 13. the average mass of natural mixture of isotopes, which is compared to the mass of one atom of C-12 a.m.u is called: a) atomic number b) atomic mass c) mass number d) molecular mass 14. a formula that gives only the relative number of each type of atoms in a molecule is called: Chemistry Def. & MCQs 12
Dr. Sajid Ali Talpur
a) empirical formula c) molecular mass
b) molecular formula d) formula mass
15. a formula that indicates actual number and type of atoms in a molecule is called: a) empirical formula b) molecular formula c) molecular mass d) formula mass 16. the sum of atomic masses of all atoms in a molecule is called: a) empirical formula b) molecular formula c) molecular mass d) formula mass 17. the sum of atomic masses of all atoms in a formula unit: a) empirical formula b) molecular formula c) molecular mass d) formula mass 18. the mass of one mole of a substance expressed in grams is called: a) empirical formula b) molecular formula c) molecular mass d) molar mass 19. 44 a.m.u of CO2 is equal to: a) formula mass b) atomic mass c) molecular mass d) molar mass 20. 5 moles of H2O are equal to: a) 80g b) 90g c) 100g d) 90a.m.u Answer Key
Chemistry Def. & MCQs 13
Dr. Sajid Ali Talpur
1 4 7 10 13 16 19
B B B B B C C
Chapter 3
2 5 8 11 14 17 20
A D C A A D D
3 6 9 12 15 18
B A B B B D
Atomic Structure
(Neither take rest nor be the time waste, Because life is the test and only heaven is the rest) Chemistry Def. & MCQs 14
Dr. Sajid Ali Talpur
Definitions 1. Atom: -The building block of the matter that takes part in the reaction. OR The smallest component of an element having the chemical properties of the element, consisting of a nucleus and surrounding shells. 2. Nucleus: -the central part of the atom comprising the mass of the atom conferred by protons and neutrons, initially discovered by RUTHERFORD.
Chemistry Def. & MCQs 15
Dr. Sajid Ali Talpur
3. Shell or energy level: -according to Bohr these are the circular orbits at certain distance from the nucleus where electrons exist. 4. Atomic number (Z): -The number of protons in nucleus is called the atomic number of the element. 5. Atomic mass: - The total number of protons and neutrons in nucleus constitute its atomic mass. 6. Element: -The simplest matter whose all atoms have same atomic number and can not be further simplified is called element. 7. Crook’s discharge tube experiment: indicates the existence of protons and electrons in the atom 8. Cathode rays: -the rays which consist of electrons and are produced when the current is ed through gases at low pressure are called cathode rays. 9. Properties of cathode rays (electrons): Discovered by J.J THOSMSON Carry a negative charge equal to 1.6*1019 C=4.803*10-10 Their e/m ratio is 1.76*108 C/g Their mass is 9.11*10-31 kg = 0.00055a.m.u They can be deflected by electromagnetic field.
Chemistry Def. & MCQs 16
Dr. Sajid Ali Talpur
These don’t depend upon the material of which the electrode is made nor of the gas which is enclosed inside the tube. 10. The properties of canal rays ( protons): GOLDSTIEN discovered them. These rays carry positive charge They travel in straight line The value of e/m depends upon the gas enclosed The mass is 1.67*10-27kg=1.0073amu They are composed of heavy particles than electrons. 11. The properties of neutrons: Discovered by CHADVICK. They are neutral, carrying no charge. The mass is same as that of proton but slightly heavier. i.e. 1.0087 a.m.u. It is highly energetic particle. 12. Radioactivity: -the spontaneous emission of radiations by certain elements is called radioactivit 13. Isotopes: - Atoms of the same elements, having the same atomic number but the different atomic masses are called isotopes. 14. Spectrum: -the band of colors formed through the dispersion of light is called spectrum.
Chemistry Def. & MCQs 17
Dr. Sajid Ali Talpur
15. Electronic configuration: - the arrangement or distribution of electrons in the available orbitals is called electronic distribution. 16. Atomic radius: -the half of the bond length, taken between two homonuclear diatomic molecules. OR the distance from nucleus to the valence electron is called atomic radius. 17. Ionic radius: -the radius of an ion. 18. ion: -the charged atom is called ion
19. Cation: -the positively charged ion is called cation. 20. Anion: -the negative charged ion is called anion. 21. Ionization potential: -the energy required to make an atom ion is called ionization potential. 22. Electron affinity: -the amount of energy released when an electron is added to a neutral gaseous atom to form a negative ion is called electron affinity. 23. Electronegativity: - the force with witch an atom attracts the shared pair towards itself is called electronegativity.
Chemistry Def. & MCQs 18
Dr. Sajid Ali Talpur
Multiple Choice Questions 1. The first atomic theory was proposed by: a) Democritus b) Greek Philosophers c) both a & b d) John Dalton 2. According to modern theory, all elements are made up of small, indivisible, indestructible particles called atoms a) true b) false
Chemistry Def. & MCQs 19
Dr. Sajid Ali Talpur
3. Protons and neutrons were discovered by respectively: a) J.J Thomson, Chadwick b) Chadwick, J.J Thomson c) Goldstein, Chadwick d) Chadwick, Goldstein 4. Electrons are the constituent of all matter. a) true b) false 5. The incorrect statement regarding the cathode rays is: a) material particles b) e/m ratio is different c) possess K.E d) N.O.T 6. Electrons do not depend upon the the nature of the cathode and the gas inside the tube. a) true b) false 7. e/m ratio of electron is: a) 1.76*108 C/g b)1.76*1011C/g c) 1.602*10-19 C/g d) 1.672*10-27C/g 8. The Charge on electron is: a) 1.76*108 C b)1.76*1011C c) 1.602*10-19 C d) 1.672*10-27C 9. The charge on proton is: a) 1.76*108 b)1.76*1011C c) 1.602*10-19 C d) 1.672*10-27C Chemistry Def. & MCQs 20
Dr. Sajid Ali Talpur
10. 1 a.m.u =? a) 1.76*108 g c) 1.602*10-19 g
b)1.76*1011g d) 1.672*10-27g
11. Atom was proved divisible particle by: a) cathode rays b) radioactivity c) discharge tube exp. d) A.O.T 12. Electron is 1836 times heavier than proton. a) true b) false 13. Radioactivity was discovered by: a) Henry Bequeral b) Rutherford c) Bohor d) J.J Thomson 14. Rutherford used particles in his experiment. a) α – particles b) β – particles c) γ – particles d) A.O.T 15. The α-particles deflected back by striking the atom because of the presence of: a) shells b) nucleus c) protons d) electrons 16. Energy is …… when an electron jumps from higher energy level to lower energy level. a) absorbed b) released c) neither absorbed nor released d) both a & b
Chemistry Def. & MCQs 21
Dr. Sajid Ali Talpur
17. This of the following particles takes part in the reaction. a) electron b) proton c) neutron d) A.O.T 18. The correct equation is: a) E2 - E1 = hυ b) E2 + E1 = hυ c) E2 * E1 = hυ d) E2 / E1 = hυ 19. Na has: a) 11 electrons c) 12 neutrons
b) 11 protons d) A.O.T
20. Mass number = a) protons + electrons b) protons + neutrons c) electrons + neutrons d) no. of protons.
21. Atomic number = a) protons + electrons b) protons + neutrons c) electrons + neutrons d) no. of protons. 22. The positively charged particles in radioactivity are protons. a) true b) false 23. Isotopes have different number of: Chemistry Def. & MCQs 22
Dr. Sajid Ali Talpur
a) electrons c) neutrons
b) protons d) A.O.T
24. Proteum has one proton and no neutron. a) true b) false 25. Isotopes are used in the treatment of diseases. a) true b) false 26. The formula to find out max number of electrons is: a) n2 b) 2n c) 2n2 d) N.O.T 27. When n=3 the max electrons in a shell should be. a) 3 b) 6 c) 9 d) 18 28. The max. number of electrons in 4th shell is: a) 4 b) 8 c) 16 d) 32 29. Find the mis match a) electrons : J.J Thomson b) protons : nucleus c) neutrons : atomic mass d) protons : atomic number 30. The correct statement is: a) A = Z+A b) A=Z-N c) A=N-Z d) Z=A-N 31. Which isotope of oxygen forms ozone Chemistry Def. & MCQs 23
Dr. Sajid Ali Talpur
a) O16 c) O18
b) O17 d) O19 Answer Key
1 4 7 10 13 16 19 22 25 28 31
D A A D A B D C A D C
2 5 8 11 14 17 20 23 26 29
B A C B B B B A C A
Chemistry Def. & MCQs 24
3 6 9 12 15 18 21 24 27 30
C B C B A A D A D D
Dr. Sajid Ali Talpur
Chapter 4 Periodicity of Elements (People are bad enough to tease you but I am sure you are good enough to forgive them)
Chemistry Def. & MCQs 25
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Definitions 1. Periodicity: - The repetition of properties of elements after some interval is called periodicity. 2. Periods: - The horizontal rows in the periodic table are called periods. 3. Groups: - The vertical columns in the periodic table are called groups. 4. Metals: -Those elements which conduct heat and electricity and become positively charged by loosing electrons are called metals. 5. Non metals: -Those which do not conduct heat and electricity and become negatively charged by accepting electrons are called non metals 6. Metalloids: - These have the mixed properties of metalloids. 7. Atomic radius: -the half of the bond length, taken between two homonuclear diatomic molecules. OR the distance from nucleus to the valence electron is called atomic radius. 8. Ionic radius: -the radius of an ion. 9. ion: -the charged atom is called ion
Chemistry Def. & MCQs 26
Dr. Sajid Ali Talpur
10. Cation: -the positively charged ion is called cation. 11. Anion: -the negative charged ion is called anion. 12. Ionization potential: -the energy required to make an atom ion is called ionization potential. 13. Electron affinity: -the amount of energy released when an electron is added to a neutral gaseous atom to form a negative ion is called electron affinity. 14. Electronegativity: - the force with witch an atom attracts the shared pair towards itself is called electronegativity.
Chemistry Def. & MCQs 27
Dr. Sajid Ali Talpur
Multiple Choice Questions 1. Law of triads was proposed by: a) Doberinier b) Lother Mayer c) Newland d) Mendeleef 2. Modern classification is based on atomic number. a) true b) false 3. law of octaves was proposed by: a) Doberinier b) Lother Mayer c) Newland d) Mendeleef 4. Mg being eighth element from Be has the similar properties with it. The statement comes from: a) law of octaves b) law of triads c) Lother Mayer’s classification d) Mendeelev’s periodic table 5. atomic volume = ? a) gram atomic Weight * density b) gram atomic Weight / density c) gram atomic weight + density d) gram atomic weight – density 6. Mendeleev arranged the elements in order of increasing: a) atomic volume b) atomic mass c) atomic number d) periodicity
Chemistry Def. & MCQs 28
Dr. Sajid Ali Talpur
7. Mendeleev’s periodic table was remarkable in having: a) columns b) rows c) both d) gaps for unknown elements 8. Mendeleev’s periodic table failed to give the idea of atomic structure. a) true b) false 9. regarding the periodic table the incorrect statement is: a) rows have similar properties b) it does not contain isotopes c) shows the periodicity of elements d) N.O.T 10. Eka boran was later termed as: a) boron b) scandium c) gallium d) germanium 11. …..proved atomic mass not as the fundamental property of elements: a) radioactivity b) isotopes c) electronic configurationd) periodicity 12. atomic number was discovered by: a) doberinier b) newland c) baquerel d) mosely 13. the longest period is: a) first c) sixth
b) second d) seventh
Chemistry Def. & MCQs 29
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14. the sixth period contains: a) 6 b) 8 c) 16 d) 32 15. the elements of sub group A are called transition elements. a) true b) false 16. group 1A and 2A contain alkali metals: a) true b) false 17. the most stable of the following elements is: a) Na b) N2 c) Ni d) Ne 18. the most reactive is: a) Na c) Na+
b) Mg d) F
19. The valency of seventh A group is : a) +1 b)-1 c) +2 d)-2 20. boron is metalloid: a) true
b) false.
21. it exists in tetameric form: a) K b) P c) N d) Sb 22. inert or noble gases are placed in the group: a) 3A b) 4A c) 7A d) 8A Chemistry Def. & MCQs 30
Dr. Sajid Ali Talpur
23. electronegativity of fluorine is: a) 1 b) 2 c) 3 d) 4 24. the minimum energy required to remove an electron from an atom in gaseous state is called: a) electronegativity b) electron affinity c) ionization potential d) P.E 25. 1Å = ? a)10-8 c)10-7
b) 10-9 d) 10-10
26. atomic number depends upon the number of shells but does not depend upon the nuclear charge. a) true b) false 27. the energy change that occurs when an electron is gained by an atom in gaseous state is called: a) electron affinity b) ionization potential c) enthalpy d) electronegativity 28. the relative tendency of an atom in a molecule to attract shared pair of electrons towards itself is called: a) electron affinity b) ionization potential c) enthalpy d) electronegativity 29. electronegativity decreases down the group. a) true b) false
Chemistry Def. & MCQs 31
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30. the incomplete period is: a) first b) fourth c) sixth d) seventh 31. which period contains only gases a) first b) fourth c) sixth d) seventh 32. it is the radioactive element of 1A group. a) Li b) Rb c) Cs d) Fr 33. the valency of alkaline earth metals is: a) +1 b) +2 c) -1 d) -2 34. N and P are non metals. a) true b) false 35. which pair of elements is chemically similar: a) K, Cr b) Cu, Ca c) F, Cl d) N, O
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Answer Key 1 4 7 10 13 16 19 22 25 28 31 34
A A D B C B B D A D A A
2 5 8 11 14 17 20 23 26 29 32 35
A B A A D D A D B A D C
Chemistry Def. & MCQs 33
3 6 9 12 15 18 21 24 27 30 33
C B A D B C B C A D B
Dr. Sajid Ali Talpur
Chapter 5 Chemical Bonding (The future will take revenge if you spoil the present)
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Definitions 1. Chemical bond: - The attractive force that holds atoms together in a compound is called chemical bond. 2. Ionic or electrovalent bond: - It is defined as the electrostatic force of attraction between positive and negative ions. 3. Covalent bond: - Achemical bond that involves the sharing of electrons is called covalent bond. 4. Single covalent bond (—): -such a bond is formed when one electron is contributed from each atom making one shared pair. E.g. Cl2 5. Double covalent bond: -in such a covalent bond each of the two atoms contribute two electrons as in O2 6. Triple covalent bond: -in triple covalent bond each atom contributes three electrons as in N2 7. Co-ordinate or dative covalent bond: -a covalent bond in witch one of the bonded atoms furnishes both of the shared electrons. 8. Hydrogen bond: - it is an electrostatic force of attraction between a partially positive hydrogen atom of one molecule and the electronegative atom of the other molecule Chemistry Def. & MCQs 35
Dr. Sajid Ali Talpur
9. Metabolic Bond: - It is defined as the force of attraction between electrons and the positive nuclei of atoms. 10. Dispersion Forces: The dispersion forces are the weak attractive forces between temporarily polarized atoms (or molecules) caused by the varying positions of the electrons during their motion about the nuclei 11. Dipole moment: - the measure of the degree of the polarity of a polar compound is called dipole moment. 12. Electronegativity: - It is the power of an atom to attract shared pair of electrons towards itself. 13. Bond pairs electrons: - also called active set of electrons they take part in bond formation and are incorporated as shared pair. 14. Lone pair of electrons: - also called non bonding pairs, are paired electrons but don’t take part in bonding.
Chemistry Def. & MCQs 36
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Multiple Choice Questions: 1. The force which holds atoms together in a molecule or crystal is called a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 2. the energy in a molecule is less than the atoms. a) true b) false 3. the electrons in the innermost shell are called valence electrons. a) true b) false 4. the bond formed by sharing of electrons is called: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 5. the bond formed by the complete transfer of electrons: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 6. the gases like oxygen, nitrogen, are the result of: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent 7. MgO is an example of: a) chemical bond b) covalent bond c) ionic bond d) co-ordinate covalent
Chemistry Def. & MCQs 37
Dr. Sajid Ali Talpur
8. the idea of chemical bond was introduced in a) 1808 b) 1910 c) 1816 d) 1916 9. ionic compounds don’t possess molecular formula. a) true b) false 10. the atom that donates electrons becomes negatively charged: a) true b) false 11. which one is the stable: a) Na b) Na+ ++ c) Na d) Na12. ionic compounds are good conductors of electricity: a) true b) false 13. covalent compounds are soluble in water: a) true b) false 14. ionic compounds form the molecules of high molecular weight. a) true b) false 15. all are correct about ionic bond except: a) they conduct electricity in all the states b) they are soluble in polar solvents c) ionic compounds do not form molecules d) N.O.T
Chemistry Def. & MCQs 38
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Questions 16 – 18 •
Select from the below: A) single covalent bond B) double covalent bond C) triple covalent bond D) ionic bond E) N.O.T
16. the bond in hydrogen molecule is: 17. the bond in nitrogen molecule is: 18. the bond in CaCl2 is: 19. HCl is an example of: a) ionic bond b) covalent bond c) polar covalent bond d) non-polar 20. Cl- contains electrons in it: a) 1 b) 2 c) 7 d) 8
Questions 21 – 33 •
Select from the below
A) covalent bond B) polar covalent bond C) non polar covalent bond D) ionic bond E) co-ordinate covalent bond F) N.O.T
Chemistry Def. & MCQs 39
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21. The bond in oxygen molecule is 22. both the electrons are shared by one electrons: 23. also called electrovalent bond: 24. the bond in the table salt 25. the bond in NH4Cl 26. e.n > 1.7 27. the e.n = 0 28. involves the sharing of electrons: 29. formed by sharing of electrons between dissimilar atoms 30. formed by sharing of electrons between similar atoms. 31. lone pair of electrons is the indication of the bond 32. the attraction between electrons and nuclei. 33. the greatest electronegativity difference is present in: 34. metals are solids except bromine a) true b) false Chemistry Def. & MCQs 40
Dr. Sajid Ali Talpur
35. metals conduct heat and electricity because of the presence of: a) fixed electrons b) free electrons c) fixed protons d) free protons 36. inter molecular forces hold atoms together in a molecule: a) true b) false 37. all of the following are wander wall’s forces except: a) dispersion forces b) covalent bond c) dipole-dipole forces d) H-bonding 38. inter molecular forces are much weaker than intra molecular forces. a) true b) false
Chemistry Def. & MCQs 41
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Answer Key 1 4 7 10 13 16 19 22 25 28 31 34 37
A B C B B A C E E A E B B
2 5 8 11 14 17 20 23 26 29 32 35 38
A C D B B C D D D B F B B
Chemistry Def. & MCQs 42
3 6 9 12 15 18 21 24 27 30 33 36 39
B B A B A D C D C C D B
Dr. Sajid Ali Talpur
Chapter 6
States of matter
(Every action has reaction, yes exactly if you can not please your books how you will be
Chemistry Def. & MCQs 43
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pleased)
Definitions 24. Matter: - Any thing having mass and volume is called matter. 25. Solid: - The state of matter having specific shape and volume 26. Liquid: - The state of matter having specific volume but not the shape. 27. Gas: - It is the state of matter having neither specific volume nor the shape 28. Diffusion: - the distribution or spreading of the gas molecules throughout the vessel is known as Chemistry Def. & MCQs 44
Dr. Sajid Ali Talpur
diffusion. OR the mixing and merging of the molecules with each other is called diffusion 29. Pressure: -force per unit area. 30. Temperature: - the degree of hotness or coldness of a body is called temperature. 31. Heat: - it is the form of energy that produces sense of warmth and flows from hot body to cold body. 32. Density: - the mass unit volume is called density. (d=M/V) 33. Vapour pressure: - it is the pressure exerted by the vapors on the surface of liquid when rate of condensation exceeds the rate of evaporation. 34. Boiling: - when vapour pressure of liquid equals the atmospheric pressure, the bubbles of vapour form easily and rise to the surface. The liquid is said to boil. 35. Boiling point: -it is the temperature at which boiling starts. 36. Melting: - conversion of a solid into liquid. 37. Melting point: - it is the temperature at which melting begins to take place.
Chemistry Def. & MCQs 45
Dr. Sajid Ali Talpur
38. Sublimation: -the process of conversion of solids directly into gases form without ing through the liquid state is called sublimation. 39. Phenomenon: -an observable event. 40. The latent heat of fusion: - heat required during conversion of the state. OR the heat energy required converting 1g of a solid into liquid at its melting point. 41. Brownian motion: - A continuous, zigzag motion of suspended particles through the medium is called Brownian motion.
Multiple Choice Question 1. Any thing having mass and volume is not called called a) power b) energy c) both a & b d) matter 2. The quantity of matter in a body is called a) mass b) energy c) matter d) volume 3. According to K.M.T all are true except: a) molecules are always in motion: b) they possess K.E c) they possess P.E d) molecules are very tiny particles e) N.O.T Chemistry Def. & MCQs 46
Dr. Sajid Ali Talpur
4. The space occupied by an object is called a) mass b) energy c) volume d) matter 5. Regarding gases all are true except: a) K.E very low b) intermolecular space very high c) neither shape nor volume d) molecules move in all directions. 6. The liquids have constant shape but not volume. a) true b) false 7. The spreading of a substance through a medium is called: a) diffusion b) Brownian motion c) effusion d) fusion 8. A continuous, rapid, zigzag motion of suspended particles through the medium is called Brownian motion. a) true b) false 9. Water can exist in all the three states of matter. a) true b) false The Book MCQs 10. The number of common states of matter is: a) 3 b) 4 c) 5 d) N.O.T
Chemistry Def. & MCQs 47
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11. Neither definite shape nor volume is the property of: a) solids b) liquids c) gases d) N.O.T 12. The temperature at which the vapour pressure of a liquid becomes equal to its external pressure is called: a) melting point b) boiling point c) triple point d) freezing point 13. The state of matter in which molecules are tightly packed and possess only vibratory motion is: a) solid state b) liquid state c) gaseous state d) N.O.T 14. The process in which molecules escape from the surface of liquid is called: a) sublimation b) evaporation c) boiling d) melting 15. the process in which solid directly changes to gas is called a) sublimation b) evaporation c) boiling d) melting
Answer Key 1 4
C C
2 5
A A
Chemistry Def. & MCQs 48
3 6
C B
Dr. Sajid Ali Talpur
7 10 13
A A A
8 11 14
B C B
9 12 15
A B A
Chapter 7 Solution and Suspension (Solving the problems is the solution of problems than increasing the problems by
Chemistry Def. & MCQs 49
Dr. Sajid Ali Talpur
worrying on the problems…!)
Definitions 1. Solution: -the homogeneous mixture of two or more things. 2. Solute: - It is the component of solution present in smaller amount and is dissolved by the solvent. 3. Solvent: - It is the component of solution present in greater amount and dissolves the solute. 4. Unsaturated solution: - It is that one solution which contains less solute than it has the capacity to dissolve. Chemistry Def. & MCQs 50
Dr. Sajid Ali Talpur
5. Saturated solution: - It is that one solution which contains maximum amount of solute and can not dissolve more solute at a given temperature 6. Super saturated solution: - It is that one solution which contains more solute than the normal capacity and this is done usually by increasing temperature. 7. Crystallization: - The process in which dissolved solute comes out of solution and forms crystals is called crystallization. 8. Molarity: - The number of moles of solute dissolved in 1 liter (1dm3) of a solution is called molarity. It is denoted by (M). 9. Molality : - The number of moles of solute dissolved in 1 kilogram of solution is called molality. It is denoted by (m). 10. Mole fraction: - Mole fraction of any component in a solution is the number of moles of the component divided by total number of moles making up solution. It is denoted by X. 11. Suspension: - It is defined as a heterogenous mixture consists of visible particles which remain suspended in the liquid.
Chemistry Def. & MCQs 51
Dr. Sajid Ali Talpur
Multiple Choice Questions 1. A heterogeneous mixture of two or more substances is called solution: a) true b) false 2. there are types of solutions a) 2 b) 3 c) 5 d) 9 3. The composition of air is as a) 78% N2, 21% O2, 1% Ar. b) 78% N2, 15% O2, 5% CO2, 1 other gases c) 78% N2, 21% O2, 1% other gases d) all are possible 4. alloys are the mixture of: a) solid-solid b) solid-liquid c) liquid-gas d) solid-gas Chemistry Def. & MCQs 52
Dr. Sajid Ali Talpur
5. which of the following does not affect the solubility: a) temperature b) size of particles c) pressure d) nature of solute e) nature of solvent 6. the solubility of gases increases with the increase in temperature. a) true b) false 7. Only the solubility of is affected by pressure. a) solids b) liquid c) gases d) plasma 8. ionic compounds are not dissolved in: a) polar solvent b) non-polar c) water d) A.O.T 9. A solution which has the capacity to dissolve more solute is called: a) saturated solution b) unsaturated solution c) super saturated d) N.O.T 10. the process in which the dissolved solute comes out of the solution is called: a) titration b) solubility c) crystallization d) N.O.T 11. what is the molarity of a solution when 10 g NaOH are dissolved in 1 liter solution: a) 0.25M b) 0.5M c) 1M d) 2M
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The Book MCQs 12. the suspended particles in the suspensions are generally of the size: a) 10nm b) 100nm c) 1000nm d) 1200nm 13. the sum of mole fraction of solute and solvent is equal to: a) 1 b) 2 c) 3 d) 4 14. solubility is defined as the amount of solute in gram at a given temperature, dissolved in …… of the solvent. a) 10g b) 20g c) 100g d)1000g 15. the process in which solid directly changes to vapours is called. a) sublimation b) evaporation c) diffusion d) boiling 16. the solubility of gas …….with the rise in temperature. a) increase b) decrease Answer Key 1 4
B A
2 5
D B
Chemistry Def. & MCQs 54
3 6
C B
Dr. Sajid Ali Talpur
7 10 13 16
C C A B
Chapter 8
8 11 14
B A C
9 12 15
B C A
Thermochemistry
(To shine your face make nimaz (salah) base because life is race and in this case to fasten the pace don’t create mess)
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Definitions 12. Electrochemistry: - It is the branch of chemistry which deals with the relationship of electrical and chemical energies and their interconversion. 13. Electrolyte: -The substance capable of being dissociated into ions on the age of electricity in the molten state. 14. Non-eclectrolytes: - The chemical compounds which do not conduct electricity in molten or aqueous solutions are called non electrolytes.
Chemistry Def. & MCQs 56
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15. Electrolysis: -The breakage of a solution on the age of electric current. 16. Anode: -the positively charged electrode where oxidation occurs. 17. Cathode: -the negatively charged electrode where reduction takes place is called cathode. 18. Ampere: - It is the S.I unit of current which is defined as the current when ed through a circuit for one second. 19. Columb: - It is the S.I unit of electric charge and is defined as the quantity of charge when one ampere of current is ed for one second. 20. Electroplating: - It is the process of electrolysis which is used to coat one metal onto the other. 21. Electrochemical cell: - The cell which is used to convert electrical energy into chemical energy and vice versa is called electrochemical cell. Multiple Choice Questions 1. Chemical and electrical energies are inter convertible: a) true b) false 2. all acids, bases and salts are electrolytes in aqueous solutions or fused state. Chemistry Def. & MCQs 57
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a) true
b) false
3. all the conductors are electrolytes. a) true b) false 4. which of the following does not conduct electricity. a) salt b) water c) sugar d) N.O.T 5. all are true about cathode except: a) is negatively charged b) positive ions move towards it c) oxidation takes place over it d) Na+ ions become Na e) N.O.T 6. all are true about anode except: a) is positively charged b) oxidation takes place c) Cl becomes Cld) negative ions moves towards it e) N.O.T 7. Columb= ? a) current * time c) current + time
b) current / time d) current – time
8. 1F = ? a) 500C c) 96500C
b) 6500C d) 1000 C
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9. What is the charge when 2 A current es for 2 seconds: a) 1 b) 2 c) 3 d) 4 10. electrolysis is used for the extraction of certain metals from their ores. a) true b) false 11. coating of metal by non metal is called plating a) true b) false 12. a cell which converts electrical energy into chemical energy is called voltaic cell a) true b) false 13. lead storage battery is a reversible cell. a) true b) false Answer Key 1 4 7 10 13
A C A A A
2 5 8 11
A C C B
Chemistry Def. & MCQs 59
3 6 9 12
B C D B
Dr. Sajid Ali Talpur
Chapter 9 Acids, Bases and Salts (I do not own any business but the entire world is my own where Almighty Allah is to Chemistry Def. & MCQs 60
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be felt and Muhammad (s.a.w) to be followed)
Definitions 22. Acid: -A compound having usually sour taste and capable of neutralizing alkalis and reddening blue litmus paper, containing hydrogen that can be replaced by a metal or any other electropositive atom to form salt, or containing an atom that can accept electrons from a base. 23. Base: - A base is a substance that can accept hydrogen ions or more generally, donates electrons pairs.
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24. Salt: -the ionic substance that result from the neutralization of an acid with a base. 25. Ph: - A measure of the acidity or alkalinity of a solution, numerically equal to 7 for neutral solutions, increasing with increasing alkalinity and decreasing with increasing acidity. 26. Arrhenius Theory: It states that an acid can be defined as a substance that yields hydrogen ions when dissolved in water. A base can be defined as a substance which yields hydroxide ions when dissolved in water. 27. Bronsted Lowery Theory: It states that an acid is a substance having a tendency to donate one or more protons and a base is a substance having a tendency to accept protons. 28. Lewis Theory: It states that an acid is any species (molecule or ion) which can accept a pair of electrons and a base is any species (molecule or ion) which can donate a pair of electrons. 29. Titration: -titration is the quantitative measurement of an analyte in solution by completely reaction with reagent solution. Indicators: -color showing organic compounds. OR for acid-base titrations, organic compounds that exhibit different colors in solution of different acidities; used to determine the point at
Chemistry Def. & MCQs 62
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which the reaction between two solutes is complete. 30. Buffer: -any substance that prevents changes in pH is known as buffer. 31. Neutralization: -when the two substances (acid and base) having opposed properties are allowed to react, salt and water are produced. The reaction is known as neutralization.
Multiple Choice Questions: 1. Ascorbic acid is the other name of: a) Vitamin A b) Vitamin B c) Vitamin C d) Vitamin D 2. all are the properties of acids except: a) sour in taste b) smooth in touch c) proton donor d) electrons acceptor 3. the common acid in stomach is: a) HCl b) H2SO4 c) HNO3 d) H3PO4 Chemistry Def. & MCQs 63
Dr. Sajid Ali Talpur
4. The consumption of …… is an index to the state of civilization and prosperity of a country: a) HCl b) H2SO4 c) HNO3 d) H3PO4 5. the important acid for making explosive materials and fertilizers is: a) HCl b) H2SO4 c) HNO3 d) H3PO4 6. the souring of milk produces. a) citric acid b) lactic acid c) acetic acid d) fumaric acid 7. lemon, oranges, grape fruits contain: a) citric acid b) lactic acid c) acetic acid d) fumaric acid 8. all are the properties of bases except: a) bitter in taste b) aqueous solution conducts electricity c) undergo neutralization with acids d) turn litmus paper to red. Q 9 – 14 Select from the below: a) Arrhenius Theory b) Bronsted –lowery c) Lewis concept d) N.O.T 9. Bases are proton acceptors. 10. acids are sour in taste Chemistry Def. & MCQs 64
Dr. Sajid Ali Talpur
11. acids are H+ ions donor 12. bases turn litmus paper to blue 13. ammonia is base 14. bases are electron donors 15. all are weak acids except: a) sulphuric acid b ) acetic acid c) formic acid d) phosphoric acid 16. which one is the normal salt: a) NaCl b) NaHSO4 c) KHCO3 d) Mg(OH) Cl 17. which one is not double salt: a) potash alum b) chrome alum c) Mohor’s salt d) table salt Q18 -22 Select from the below: a) Sodium carbonate b) backing soda c) copper sulphate d) Epsom salt e) potash alum f) N.O.T 18. it is a common double salt 19. used as antiacid and fire extinguishers 20. used as germicide, insecticide and in paint and varnish industry
Chemistry Def. & MCQs 65
Dr. Sajid Ali Talpur
21. it is used in softening of water, glass industry and as cleaning agent 22. used as anticeptic and mouth wash 23. water is not: a) universal solvent c) present in urine e) N.O.T
b) liquid d) amphoteric molecule
24. The number of moles of solute dissolved per liter of solution is: a) molarity b) molality c) titration d) pH 25. negative logarithm of hydrogen ion concentration is: a) molarity b) molality c) titration d) pH 26. it is important for an analytical chemist a) molarity b) molality c) titration d) pH Q 27 – 32 Select from the below a) 0 b) 5-7 c) 7 d) 7.4 e) 14 27. it is the neutral pH
Chemistry Def. & MCQs 66
Dr. Sajid Ali Talpur
28. the pH of water is : 29. it is the highly acidic Ph 30. the pH of urine is: 31. the pH of blood is 32. pH + p OH = ? 33. Methyl orange produce…. Color in acidic solution a) red b) green c) yellow d) pink 34. a solution whose molarity or strength is known is called standard solution: a) true b) false 35. low p H of blood causes diabetes, diarrhea, vomiting. a) true b) false 36. water and CO2 are produced as a result of neutralization: a) true b) false Answer Key 1 4 7
C B A
2 5 8
B C D
Chemistry Def. & MCQs 67
3 6 9
A B B
Dr. Sajid Ali Talpur
10 13 16 19 22 25 28 31 34
D B A B E C D D A
11 14 17 20 23 26 29 32 35
A C D C E A E C B
12 15 18 21 24 27 30 33 36
D A E A C B A A B
Chapter 10 Chemical Energetics Chemistry Def. & MCQs 68
Dr. Sajid Ali Talpur
(The failure is the result of disobedience of first parents then teachers and finally of the Almighty Allah)
Definitions 1. Thermodynamics: -The study of conversion and conservation of heat and other forms of energy is called thermodynamics. 2. Thermochemistry: - it deals with the measurement or calculation of heat absorbed or abandoned in chemical reactions. 3. Thermo chemical reactions: - the chemical reactions which are accompanied by energy
Chemistry Def. & MCQs 69
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changes along with the material changes are generally known as thermochemical reactions. 4. Exothermic reactions: -the chemical reactions which are accompanied by the liberations or emission of energy are called exothermic reactions. 5. Endothermic reactions: -the chemical reactions which are accompanied by the absorption of energy are called endothermic reactions. 6. system: -the collection of matter having certain boundaries is called system 7. Surroundings:- the environment of a system or the thing that affect on a system are included in surroundings. 8. Heat of formation: - the change of enthalpy when one gram mole of a substance is formed from its elements 9. Standard heat of formation: -the change of enthalpy when one gram mole of a substance is formed from its elements at 25oC and 1 atm is called standard heat of formation. 10. Enthalpy: -the total heat content of a system is called enthalpy..
Chemistry Def. & MCQs 70
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11. Heat of neutralization: - The amount of heat released during the neutralization process when one mole of water is produced by the reaction of acid and base.
Multiple Choice Questions 1. Thermochemical reactions involve: a) material changes b) energy changes c) both a & b d) heat changes 2. EXO means: a) out of or to evolve c) outside
b) into or to absorb d) heat
3. ∆H negative represents which reaction: a) thermochemical b) exothermic Chemistry Def. & MCQs 71
Dr. Sajid Ali Talpur
c) endothermic
d) chemical
4. Formation of water from hydrogen and oxygen produces energy: a) -286 K.J/mole b) +286 K.J/mole c) -393 K.J/mole d) +393 K.J/mole 5. ∆H positive represents neutralization: a) true b) false 6. Acid Base reaction is called neutralization reaction: a) true b) false
Questions 7 – 12 • Select from the below: A) endothermic reaction B)exothermic reaction 7. photosynthesis 8. respiration 9. decomposition reaction 10. bond formation 11. combustion 12. melting of ice The Book MCQs 13. in an exothermic reaction: a) heat energy is lost b) heat energy is gained Chemistry Def. & MCQs 72
Dr. Sajid Ali Talpur
c) both a & b
d) N.O.T
14. In an exothermic reaction: a) container becomes hot b) container becomes cold c) the temperature of container remains same d) N.O.T 15. During an endothermic reaction: a) container becomes cold b) container becomes hot c) the temperature of container remains same d) N.O.T Answer Key 1 4 7 10 13
C A A B A
2 5 8 11 14
A B B B A
3 6 9 12 15
B A A A A
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Chemistry Def. & MCQs 73
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