Prepared By G Naseer (Lecturer Chemistry Leeds College)

MCQs of Chemistry FSc Level

Chap No 1: Fundamental of chemistry


1. The period of Muslim is almost __________ years.

a. 600 b. 1000 c. 1600 d. None

2. The Muslim discovered __________element.

a. Sodium b. Arsenic c. Chlorine d. Magnesium

3. The period of __________is called period of Al-Chemist.

a. Romans b. Muslim c. Greek d. Latin

4. Muhammad Ibn-e-zakaria Al-Razi wrote __________ books.

a. 50 b. 26 c. 56 d. 56

5. __________ is know father of old chemistry.

a. Boyle b. Jabber-Ibn-Haiyan c. Ruther ford d. None

6. __________ is known as Aristotle of the Muslim world.

a. Al-Beruni b. Al-Razi c. Ibn-e-Sina d. None

7. The qualitative and quantitative analysis of matter is called

a. Physical Chemistry b. Nuclear Chem

c. Analytical Chem d. None

8. The theory of dual nature of matter was given

a. 1824 b. 1724 c. 1924 d. None

9. In 1914 __________ suggested the system for representing elements with

a. Neil Bohr b. Broyle c. Berzelius d. Symbols

10. The Latin name of sodium is __________

a. Natronium b. Nacrium c. Natrium d. None

11. __________ Metal would melt from the warmth of your hand.

a. Na b. Mg c. Ca d. Ga

12. The formula of lime stone is __________

a. Cao b. Ca(oH)2 c. Caocl2 d. CaCo3

13. We used formula A-Z to find no of __________

a. Electron b. Proton c. Both b-c

d. Neutron

14. Atoms having same mass no but different atomic no are called __________

a. Isotopes b. Isobares c. Both d. None

15. __________ Formula Show the actual No of atoms in a molecule formula

a. Chemical b. Empirical c. Molecular d. Unit

16. __________ compound have identical empirical and molecular formula.

a. NH3 b. H2So4 c. C6H6 d. H2O2

17. Ionic Compounds are represented by __________

a. Formula Unit b. Molecular formula

c. Empirical Formula d. None

18. Which element is represented by formula units.

a. Nacl b. Co2 c. HCL d. CCl4

19. The molecular mass of H2So4 is __________

a. 63 b. 98 c. 100 d. 38

20. An atom is __________ particle.

a. Positive Charge b. Negative Charge

c. Neutral Charge d. None

21. The charge particle is called __________

a. Atom b. Ion c. Molecular d. None

22. The atom which gain a electron is called __________

a. Element b. Cation c. Anion d. None

23. The smallest unit of ionic compound is __________

a. Atom b. Element c. Ion d. None

24. Which one is free radical

a. Cl2 b. Nat c. CHo3 d. None

25. Free Radical is formed by __________ Fission.

a. Hemolytic b. Heterolytic c. None d. Both b & C

26. The smallest unit of element is called __________

a. Ion b. Free radical c. Atom d. Molecule

27. The smallest unit of substance is __________

a. Atom b. Element c. Molecule d. None

28. Which one is Mono atomic molecule

a. H2 b. Co2 c. Ne d. Na

29. Which one is Homo atomic molecule

a. Hcl b. H2O c. H2 d. C6H12O6

30. Which one is Heteronuclear Molecule

a. HCL b. H2 c. Cl2 d. S8

31. The number of particles present in one mole of a substance

a. Atomic No b. Mass No c. Avogadro No d. None

32. The value of Avogadro No is

a. 6.023x1024 b. 6.023x10-23 c. 6.023x1023 d. None

33. Mole is represented as __________

a. Mole b. M c. Mol d. Ml

34. 12grams of carbon is equal to __________ moles.

a. 12 b. 1 c. 2 d. None

35. The mass of an atom is expressed in grams is called

a. Molecular mass b. Molar mass c. Mole d. b & c

36. The No of molecule in 88g of Co2 are __________

a. 1 b. 2 c. 88 d. 44

37. How many moles are there in 90 grams of H2O

a. 18 b. 90 c. 5 d. None

38. The pure form of matter is called

a. Substance b. Molecule c. Mixture d. None

39. The atomic no of an atom is represented by

a. A b. Z c. A & Z d. None

40. Which one is not a compound

a. N2o b. N2 c. No d. No2

41. Which one is equal to Two mules of H2o

a. 1.084x1025 b. 6.023x1023 c. 1.204x1024

42. Which one is the example of polyatomic molecules

a. Co2 b. H2 c. C6H12O6 d. Hcl

43. Which branch of chemistry is used to determine the amount of impurities in drinking water.

a. Physical b. Organic c. Analytical d. Nuclear

44. The branch which deals with the study of cement is_____

a. Nuclear b. Industries c. Biochemistry

45. The symbolically Representation of the elements was given in __________ by Berzelius.

a. 1816 b. 1814 c. 1914 d. None

46. The symbol of Gold is __________

a. Ag b. G c. Au d. None

47. The formula of Marsh gas is __________

a. C6H6 b. C2H4 c. CH4 d. None

48. The average atomic of oxygen is __________ a mass

a. 15 b. 15.8994 c. 16

49. Cationic Molecular ions are __________ than anionic molecular ions

a. Less Common b. More Common c. Equal

d. None

50. Hemoglobin is a __________ molecule

a. Homo atomic b. Micro c. Macro d. None

Answer Keys

1. b 15. c 29. c 43. c

2. b 16. a 30. a 44. b

3. b 17. a 31. c 45. b

4. b 18. a 32. c 46. c

5. c 19. a 33. c 47. c

6. c 20. c 34. b 48. b

7. c 21. c 35. d 49. b

8. c 22. c 36. b 50. c

9. c 23. b 37. c

10. c 24. c 38. a

11. d 25. a 39. b

12. d 26. c 40. b

13. d 27. b 41. c

14. b 28. c 42. c

Chap No 2: Structure Of Atom


1) The word atom was derived from _______ Language.

a. Latin b. Greek c. English

2) The word atoms means _______

a. Indivisible b. Divisible c. Name of these

d. Both a & b

3) The word atom was used in _______

a. 1808 A.D b. 400 Bc c. 370 B.C

4) The word atom was used by _______

a. Democritus b. Neil Bohr c. John Dalton

5) A new system of chemical philosophy is the title of _______

a. Neil Bohr Model b. Rutherford Model

c. John Dalton Model

6) Atoms of same elements have properties

a. Same b. Different c. Both

7) Father of nuclear physics is _______

a. Neil Bohr b. Rutherford c. Dalton

8) Rutherford Bum bored _______ particles

a. 𝛼 b. 𝛽 c. π‘Ÿ

9) He used a radioactive source of _______ Metal.

a. Gold Foil b. Polonium c. Zinc

10) Rutherford Bombored _______ 𝛼 particles.

a. 19990 b. 2000 c. 20,000

11) The Positively Charged center portion is called _______

a. Proton b. Nucleus c. Neutron

12) The Electrons are Revolving around nucleus due to _______

a. Columbic force b. Intermolecular Force

c. Centripetal Force

13) _______ is responsible for mass and energy

a. Atom b. Nuclear c. Proton

14) The size of nucleus is _______ to the atoms s size

a. Equal b. Greater c. Smaller

15) Law of motion is applicable to _______ bodies

a. Neutral b. Charged c. Both

16) If electron radiate energy continuously it will give _______

a. Line spectrum b. Continuous Spectrum c. None

17) Bohr Consider _______ atom as a model

a. Carbon b. Gold Foil c. Hydrogen

18) Each orbit have _______ energy

a. Less b. Greater c. Fixed

19) Energy of shell is _______ proportional to distance from the nucleus

a. Directly b. Inversely c. Equal

20) Energy of M shell is _______ than L-Shell

a. Higher b. Lower c. Equal

21) ΔE = hu where 𝑒 is the _______ of electron.

a. Velocity b. Speed c. Frequency

22) The product of mass and velocity is _______

a. Frequency b. Momentum c. Angular momentum

23) The value of 2βŒ… is _______

a. 90o b. 180o c. 360o

24) Electron was discovered by _______

a. J.W. Dobrioner b. J.J. Thomson c. New land

25) The mass of proton is _______ kg

a. 9.11x10-31 b. 1.6726x10-27kg c. 1.6749x10-27

26) Neutron was discovered in _______

a. 1808 b. 1897 c. 1932

27) In 2n2 formula "n" show the No of _______

a. Electron b. Shell c. Sub shell

28) The electrons are found to be in _______

a. Shell b. Sub shell c. Orbital

29) The place where maximum chances for an electron to be found is called _______

a. Shell b. Sub shell c. Orbital

30) There are _______ Sub shell

a. Five b. Two c. Four

31) The d-sub shell have _______ orbital's.

a. 2 b. 5 c. 7

32) Which orbital have complicated shape

a. S b. P c. d d. f

33) According to Auf Bua principal electron will fill first _______

a. Lowest energy sub shell b. Higher energy sub shell

34) 45 is filled first than 3d because _______ energy

a. High b. Low c. Equal

35) ISO means _______

a. Different b. Same c. Not equal

36) Isotopes have different No of _______

a. Neutrons b. Protons c. Electrons

37) Isotopes have different _______ No

a. Atomic b. Mass c. Name of these

38) The rare isotopes of hydrogen is

a. Protium b. Dutrium c. Tritium

39) The formula of heaving water is _______

a. H2o b. D2o c. T2o

40) Heavy water is called heavy because of high

a. Molecular mass b. Density c. B.P d. All of these

41) There are _______ isotopes of chlorine

a. Two b. Three c. Four

42) The No of neutrons in 136C is _______

a. 6 b. 13 c. 14 d. 7

43) Protium has abundance of _______ %

a. 90 b. 99.985 c. 0.015%

44) The molecular mass of D2o is _______

a. 18 a.m.u b. 19 a.m.u c. 20.03 a.m.u d. None

45) Iodine-123 used for _______

a. Cancer Treatment b. Brain Imaging c. Tracer d None

46) _______ is used for identification of blood circulation problems.

a. 614 b. Na2u c. Kr85 d. None

47) _______ is used in smoke detector

a. Californium 252 b. Americium 241 c. Na-24 d. None

48) _______ is used in electrical cloth washer.

a. Cobalt-60 b. D2o c. Kr85 d. None

49) Electrons in its ground state does not

a. Spin b. Revolve c. Radiate energy d. None

50) L-Shell Has Sub-Shell

a. S b. S & P c. S.P.D d. None

Answer Keys

1. b 11. b 21. c 31. b 41. a

2. a 12. c 22. b 32. d 42. d

3. b 13. b 23. c 33. a 43. b

4. a 14. c 24. a 34. b 44. c

5. c 15. a 25. b 35. b 45. b

6. a 16. b 26. c 36. a 46. b

7. b 17. c 27. b 37. b 47. b

8. a 18. c 28. c 38. c 48. c

9. b 19. a 29. c 39. b 49. c

10. c 20. a 30. c 40. d 50. b

Chap No 3: Periodic Table & Periodicity of Properties


1. In 1800 there were_______ elements known

a. 118 b. 34 c. 105

2. In _______ there were 105 elements discovered

a. 1800 b. 1974 c. 1870

3. With Passage of time no of element was _______

a. Increased b. Decreased c. Remain constant

4. The most successful classification was given by

a. Newland b. Mendeleev c. Debierner

d. Mosely

5. Initiative elements was divided into _______ groups

a. Two b. Three c. Four

6. In _______ J.W Dobrenier gives his triads classification

a. 1869 b. 1864 c. 1817

7. The Classification of octaves was given by

a. Mendeleev b. Newland c. Laniser

8. Mendeleev arranged _______ elements in G & P

a. 34 b. 65 c. 105

9. The vacant spaces were left in P.T by _______

a. Moseley b. Newland c. Mendeleev

10. The entire crust contain _______ g of astatine

a. 20 b. 28 c. 36

11. The rarest naturally accruing elements is _______

a. Carbon b. Hydrogen c. Astatine d. None

12. The Horizontal rows in P.T are called _______

a. Group b. Period c. None

13. Modren Periodic table was given by _______

a. Moseley b. Mendeleev c. New land d. None

14. Modren P.T was based on _______ No

a. Increasing b. Decreasing c. Constant d. None

15. By Increasing No of shell _______ will be increased from top to bottom

a. Period b. Group c. Both d. None

16. There are _______ periods in P.T

a. 8 b. 7 c. 18 d. None

17. Atoms having same No of valence electrons are present in_______ group

a. Same b. Different c. None

18. _______ period is called shortest period

a. seven b. Two c. None d. 1st

19. Elements having variable oxidation state (valiancy) _______

a. Transition b. Representative c. Metals

20. Group 1 elements are called _______ metal

a. alkaline earth metal b. Alkali c. None

21. All element of group 1 are metals except

a. Li b. Na c. H

22. Groups viii elements have _______ electrons in valence shell

a. 6 b. 8 c. 2

23. Transition elements are also called _______ block elements

a. S b. P c. f d. d

24. In period II and group II which elements is

a. F b. cl c. Br

25. Metals alway _______ electron

a. Lose b. Gain c. Share

26. Group VIII elements are also called _______

a. Nitrogen family b. Halogens c. Noble gases

27. _______ are salt forming elements

a. Oxygen family b. Halogens c. Noble Gases

28. Group I and II elements are also called _______ block

a. P b. S c. d

29. Modern periodic table was based on _______

a. Atomic mass b. Atomic No c. Isotopes

30. _______ are also called Rare earth elements

a. S-block b. d-block c. f-block

31. There are _______ groups in P-Block

a. 2 b. 10 c. 6 d. 8

32. There are _______ gases which found in natural atmosphere

a. 8 b. 17 c. 25

33. The concentration of oxygen below _______ is considered unsafe for human

a. 20% b. 16% c. 12%

34. The size of an atom is _______

a. Fixed b. Not fixed c. Rigidly

35. The atomic radius is _______ to the No of shell

a. Directly proportional b. Inversely proportional

36. The atomic radius is expressed by _______

a. Kilometer b. Nanometer c. Picometer d. Band c

37. When an atom gain electron it get _______ charge

a. Positive b. Negative c. No

38. First I.E is always _______ than 2nd I.E

a. Smaller b. Greater c. Equal

39. The value of I.E is Positive because energy is _______

a. Released b. Absorbed c. None

40. The 2nd E.A values are +tive because of _______

a. Electron-Electron Attraction b. E.E Repulsion

41. The E.N is inversely proportional to _______

a. Atomic size b. Shielding Effect c. Both

42. Shielding Effect is produced due to _______ electron

a. Inner b. Outer most c. First Shell

43. Atomic size and shielding effects are _______

a. Directly proportional b. Inversely proportional

c. Constant d. None

44. I.E, E.N, E.A are _______ to atomic size and S.E

a. Inversely proportional b. Directly Proportional

c. Constant d. None

45. The ability of an atom to attract the shared pair of electron is called _______

a. Ionization energy b. Electron affinity

c. Electron affinity d. None

46. E.A is decreased from _______ to _______

a. Top to bottom b. Left to right c. Both and b

d. None

47. The unit of I.E is _______

a. Jule b. KJ c. KJ/mol d. None

48. The more electronegative element is _______

a. Fe b. F c. cl d. None

49. The least electronegative element is _______

a. F b. Na c. Cs d. None

50. Elements in _______ have similar chemical properties

a. Periods b. Group c. Both d. None

Answer Keys

1. b 11. c 21. c 31. c 41. c

2. b 12. b 22. b 32. b 42. a

3. a 13. a 23. d 33. b 43. a

4. a 14. a 24. a 34. b 44. a

5. b 15. a 25. a 35. a 45. c

6. c 16. b 26. c 36. d 46. a

7. b 17. a 27. b 37. b 47. c

8. b 18. d 28. b 38. a 48. b

9. c 19. a 29. b 39. b 49. c

10. b 20. b 30. c 40. b 50. b


Chap No 4: Structure of Molecules


1. The force of attraction between two atoms is called_______

a. Bond b. Non-bond c. None

2. Every system in universe tends to _______ its energy

a. Lower b. Higher c. Constant d. None

3. Atoms also want to _______ their energy

a. Decrease b. Increase c. Constant d. None

4. The energy of isolated hydrogen atom is _______ than two bonded hydrogen atoms

a. Higher b. Lower c. Equal d. None

5. The chemical bonding is explain by _______ concepts

a. Two b. Three c. Four d. None

6. The electronic valence theory was given in _______

a. 1916 b. 1919 c. 1816 d. 1716

7. Oxygen follows _______ rules to get stability

a. Duplet b. Octet c. Both d. None

8. Noble gases are also called _______

a. Noble metals b. Inert gases c. salt forming

9. Helium (He) have _______ electrons in last shell.

a. Two b. Eight c. Three d. None

10. The region around the nucleus where maximum chances of an electron to be found is called _______

a. Orbit b. Sub-shell c. Orbital d. None

11. Atomic orbital have _______ electron

a. Two b. Three c. One d. None

12. The endwise overlapping produce _______ bond

a. βŒ…-bond b. Sigma bond c. Both d.None

13. The sigma bond is _______ than βŒ… bond

a. Weaker b. Equal c. Stronger d. None

14. Sigma bond is represent by _______

a. βŒ… b. Δ c. o d. 𝛼

15. The electron which present in valence shell is called _____

a. Bonding Electron b. Valence Electron c. Non-Bonding

16. By the decomposition of a compound bond is _______

a. Formed b. Break c. Remains Constant d. None

17. There are _______ types of bond

a. Two b. Three c. Four d. None

18. The bond which is formed b/w metal and non-metal _____

a. Covalent b. Ionic c. Dative d. Metallic

19. Non-Metals always _______ to form anion

a. Gain b. Lose c. Both d. None

20. _______ bond is also called Electrovalent bond

a. Covalent b. Ionic c. Dative d. Metallic

21. An atom having high E.N will _______ electron

a. Gain b. Lose c. Neither gain nor loss d. None

22. Ca → ca+2+2e. In THis equ ca _______ electron.

a. Loss two b. Gain Tow c. Neither Gain nor loss d. None

23. Which one show trivalent in nature

a. Na b. Ca c. Al d. None

24. Covalent bond is formed b/w two _______

a. Metals b. Non-Metals c. Noble gase d. None

25. The shared pair of electron is represented by _______

a. ____ b. −→ c. ↔ d. None

26. The shared pair of electrons is called _______ electron

a. Delocalized b. Localized c. None

27. The bond b/w Hcl is _______ bond

a. Ionic b. Covalent c. Dative d. None

28. If the E.N difference is greater than 1.7 _______ will be formed

a. Polar Covalent b. Non-polar bond c. Ionic Bond d.None

29. Which one of the following is uncombined atom

a. O2 b. Hcl c. O3 d. None

30. In Dative bond the atom which donates shared pair of electron _______

a. Accepter b. Donner c. Both d. None

31. The dative bond is represented by _______

a. ______ b. → c. ↔ d.

32. Which one have co-ordinate covalent bond _______

a. Hcl b. CH4 c. NH+4 d. None

33. the H+ ions is electron _______ species

a. Rich b. Deficient c. Neither rich nor deficient

34. In lewis structure the unshared pair es are shown by_______

a. Dots b. Cross c. Lines d. None

35. The bond between O2 Molecule is _______ bond

a. Polar b. Non-Polar c. Ionic

36. The angle b/w H2o atoms is _______

a. 120o b. 180o c. 104.5o d. 107o

37. Metals are formed from _______ not from molecules

a. Atoms b. Elements c. Compounds d. None

38. The bond in pure gold is _______ bond

a. ionic b. Covalent c. Dative d. Metalic

39. The electron is neither shared nor transfer in _______ bond

a. Ionic b. Dative c. Covalent d. Metalic

40. The electron which donot take part in bonding_______

a. Localized b. Valence electron c. Delocalized d.None

41. The steructure of Co2 molecule is _______

a. Angular b. Linear c. Tetrahydrol d. None

42. _______ kj/mol energy is required to break H-O bond

a. 464 b. 19 c. 3 d. None

43. The B.P of hydrogen chloride is _______

a. 100𝑖 b. 85 𝑖 c. −85 𝑖 d. −95 𝑖

44. The bond In HF is _______

a. Hydrogen bond b. Covalent bond c. Polar bond d. None

45. The adhesive action of paints is due to _______

a. Ionic Bond b. Metalic bond c. Hydrogen Bond d.None

46. Greater the charge on the ions _______ will be M.P

a. Higher b. Lower c. Constant d. None

47. The formed of fluorine oxide is _______

a. FO b. F2O c. FO2 d. F2O2

48. Which two element will form covalent bond

a. Na and O2 b. Cll and O2 c. C and O2

d. Mg and O2

49. Which one do not have electronic configuration argon atom

a. Ca+2 b. S2 c. K+1 d. O-2

50. The ion of group Vi A element will be represented by

a. x+2 b. x-2 c. x-1 d. x+1

Answer Keys

1. a 11. c 21. a 31. b 41. b

2. a 12. b 22. a 32. c 42. a

3. a 13. c 23. c 33. b 43. c

4. a 14. c 24. b 34. a 44. d

5. a 15. b 25. a 35. b 45. c

6. a 16. b 26. b 36. c 46. a

7. b 17. c 27. b 37. a 47. b

8. b 18. b 28. c 38. d 48. c

9. a 19. a 29. d 39. d 49. d

10. c 20. b 30. b 40. c 50. b



Chap No 5: State Of Matter


1. _______ have weak intermolecular forces

a. Solid b. Liquid c. Gas

2. Gases molecules are in _______ motion

a. Slow b. Faster c. Constantd. None

3. Gases molecules are diffuse very quickly because of _______

a. Rest b. Motion c. Strong IMF d. None

4. The gases molecules form _______ mixture

a. Homogenous b. Heterogeneous c. Constant

d. None

5. The spontaneous Mixing of gas molecules _______

a. Effusion b. Diffusion c. Mobility d. None

6. The rate of diffusion of gases is various from gas to _______

a. Solid b. Liquid c. Gas d.None

7. Heavier gases can diffuse much _______ than lighter gases

a. Slow b. Faster c. Constant d.None

8. The smell of onion is spread due to _______

a. Effusion b. Diffusion c. Mobility c. None

9. Force per unit area is called _______

a. Work b. Volume c. Pressure d. None

10. The SI unit of force is _______

a. Jule b. M c. Newton d. None

11. Pascal is very _______ unit of pressure

a. large b. Rare c. Small d. None

12. At sea level ato𝑖 the atmospheric pressure_______

a. 760 Torr b. 760 mmHg c. a & b both d. None

13. The pressure and volume are _______ proportional

a. Directly b. Inversely c. equal d. None

14. By increasing force on a gas pressure and volume are ____

a. Increased b. Decreased c. Constantd. None

15. The change in volume per unit change in pressure

a. Mobility b. Pressure c. Compressibility

16. The density of gases is _______ than liquid

a. Greater b. Lower c. Equal d. None

17. The density of solid oxygen is 1.49 g/cm3 at _______ CO

a. -103𝑖 b. -252𝑖 c. -272𝑖 d. Nine

18. Robert boyle give his law in _______

a. 1962 b. 1662 c. 1762 d. None

19. _______ is called boyle constant

a. Kc b. Kb c. Ka d. None

20. The product of volume and pressure is _______ at constant temperature

a. Increased b. Decreased c. Constant d. None

21. J Charles give his law in _______

a. 1787 b. 1867 c. 1762 d. None

22. According charles law

a. VxT b. Vx≠ c. Vx1 𝑝 d. None

23. Absolute temperature means temperature on ______ Scale

a. Celisious b. Kelvin c. Foren Hight d. None

24. The keliven scale is equal to _______

a. K=c+273 b. C−273 c. F+273 d. None

25. Kelvin scale is also called _______

a. Celisious b. Adsdute c. Forenhight

26. Which one have more K.E

a. Solid b. Liquid c. gas

27. The surface of liquid Is always

a. Roush b. Smooth c. Leveled

28. The liquid have no definite shape b/ of

a. STMF b. INIMF c. Motion of molecules

29. The molecules of liquids have _______ K.E

a. Same b. Different c. High

30. Higher the K.E _______ will be the IMF

a. Higher b. Lower c. Equal

31. Greater the surface area _______ will be R of evaporation

a. Higher b. Lower c. Equal

32. The rate of evaporation is _______to IMF

a. Directly Proportional b. Inversely c. Equal

33. Alcohol evaporate _______ than water

a. Slow b. Quickly c. Equal

34. Rate of evaporation is _______ to condensation

a. Same b. Directly Proportional c. Inversely

35. The vapour pressure of liquids does not depends on ____

a. IMF b. Surface area c. Condensation

36. Water have _______ V.P than acetone at constant

a. Greater b. Less c. Equal

37. The vapour pressure of water at 25𝑖 is _______

a. 87mmHg b. 100mmHg c. 18

38. The Temperature at which the V.P of liquid become equal to the atmospheric pressure _______

a. M.P b. B.P c. F.P

39. Polar liquid have _______ B.P than non-polar

a. High b. Low c. Equal

40. At hilly areas the B.P of water is _______ than 100𝑖

a. Greater b. Less c. Equal

41. A device for the measurement of pressure is _______

a. Thermometer b. Ammeter c. Monometer

42. The maximum density of water is at _______


a. O𝑖 b. 4𝑖 c. 25𝑖

43. Solid molecules have _______ motion

a. Free b. Vibrational c. Rotational

44. Molecules are not move freely in _______

a. Gas b. Solid c. Liquid

45. Solids rests _______ due to hard structure

a. IMF b. Deforming force c. Columbic Force

46. Amorphus means_______

a. Volumeless b. Dimension less c. Shapless

47. Three dimensional arrangment of solid is called _______

a. Amorphus Solid b. Crystaline c. Moleculer

48. Wich one is amorphus solid _______

a. Nacl b. Butter c. Stone

49. The temperature at which one allotrophy form is changed to other form is called _______

a. Absolute temperature b. Room Temp

c. Transition Temperature d. None

50. Bucky ball consists of _______ carbons atoms

a. 10-100 b. 20-200 c. 20-100 d. None

Answer Keys

1. c 11. c 21. a 31. a 41. c

2. c 12. c 22. a 32. b 42. b

3. b 13. b 23. b 33. b 43. b

4. a 14. a 24. a 34. b 44. b

5. b 15. c 25. b 35. b 45. b

6. c 16. b 26. c 36. b 46. c

7. a 17. b 27. c 37. c 47. b

8. a 18. b 28. c 38. b 48. b

9. c 19. b 29. b 39. a 49. c

10. c 20. c 30. b 40. b 50. c



Chap No 6: Solution


1. A solution is a _______

a. Substance b. Homogeneous mixture

c. Heterogeneous d. None

2. Alloy is a _______ solution

a. Solid b. Liquid c. Gaseous d. None

3. A solution is made of _______ components

a. Four b. Two c. Three d. None

4. Binary solution is the solution of _______ components

a. One b. Two c. Three d. None

5. Aqua means _______

a. Milk b. Solution c. water d. None

6. A component of solution which is present in smaller amount is called _______

a. Solvent b. Solute c. Solution d. None

7. A solution which can Dissolved More amount of solute by changing temperature is called_______

8. A component of solution present in larger amount _______

a. Solute b. Solvent c. Suspension d. None

9. A solution which can dissolved more amount of solute _______

a. Saturated b. Unsaturated c. Super Saturated

d. None

10. Pepsi is the example of _______ solution

a. Gas in Gas b. Gas in Liquid c. Gas in solid

d. None

11. Bronze is an alloy of copper and _______

a. Zinic b. Silver c. Tin d. None

12. The example of solid in gas solution is _______

a. Vapours b. Pepsi c. Smoke d. None

13. Larger the amount of solute _______ will be concentration

a. Larger b. Lower c. Constant d. None

14. A solution contain larger amount of solute is called _____

a. Dilute solution b. Concentrated c. Standard

d. None

15. A solution of known concentration is called _______ solution

a. Concentrated b. Dilute c. Standard d. None

16. Which one is the unit of concentration of solution

a. a.m.u b. Grams c. Mole d. Molarity

17. Molarity is represented by _______

a. Concentration b. Molarity c. Both d. None

18. Molarity is represented by _______

a. m b. n c. M d. N

19. The molarity will be ______ in 90 grams of water in 1dm3

a. 5mol b. 5grams c. 5M d. None

20. The 0.5dm3 is _______ cm3

a. 5/1000 b. 5000 c. 500 d. None

21. How many moles of H2So4 are present in 0.500 dm3 pf 0.150 M H2So4 solution

a. 75moles b. 0.75 moles c. 0.075 moles d. None

22. By increasing temperature the solubility of gas will be ___

a. Increased b. Decreased c. Constant d. None

23. By increasing temperature of gases the average K.E of molecules will be _______

a. decreased b. Increased c. constant d. None

24. Lathium chloride is _______ in Benzene

a. Soluble b. Not soluble c. Highly soluble

d. None

25. Water and benzene form _______ solution

a. Miscible b. Immiscible c. Both d. None

26. Liquid solute and solvent that are soluble in each other are form _______ solution

a. Miscible Solution b. Immiscible Solution

c. Both d. None

27. The amount of solute in grams dissolved in 100 grams of a solvent to prepare saturated solution _______

a. Molarity b. Solubility c. Viscosity d. None

28. Solubility of _______ is not affected by pressure

a. Solid b. Liquid c. Gas d. Both a & b

29. Greater the pressure _______ will be solubility of gas

a. Higher b. Lower c. Constant d. None

30. Sodium sulphate form deca-hydrate at _______ 𝑖 a. 20𝑖 b. 22.2𝑖 c. 32.4𝑖 d. None

31. The solubility of _______ is decreases with increases into a. CaCl2 b. Cao c. Nacl d. None

32. The solubility of _______ is not affected by increasing or decreasing temperature a. Cao b. Cacl2 c. Nacl d. None

33. _______ = 𝑀𝑑 π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘’π‘Šπ‘‘ π‘œπ‘“ π‘ π‘œπ‘™π‘£π‘’π‘›π‘‘ x 100 a. Molarity b. Solubility c. Viscoscity d. None

34. At 32.4𝑖 the solubility of Na2So4 is _______ a. Maximum b. Minimum c. Constant d. None

35. Milk is the example of _______ a. Solution b. Suspension c. Collids d. None

36. Benzene (C6H6) is more likely to dissolved a. H2o b. C6H12 c. Agcl d. Nacl

37. The process in which paricles are setteldown at the bottom is called _______ a. Suspension b. Sedimentation c. Collids

d. None

38. The heterogeneous mixture of undisclosed particles in mixture a. Solution b. Suspension c. Collids d. None

39. The size of particle in collids is _______ a. 0.01-1nm b. 10-100m c. 1-1000nm d. None

40. _______ donot seatter light _______ a. Solution b. Suspension c. Collids d. None

41. Water is universal solvent due to its _______ a. Hydrogen Bonding b. Polarity c. Dielectric Constant d. All

42. The number of parts of solute present in 100 parts ______ a. Percentage b. Average c. Molarity d. None

43. The particles of _______are not seen with eyes a. Solution b. Suspension c. Collids d. a & c

44. The particles of _______ are separated by filtration a. Solution b. Suspension c. Collids d. None

45. Which one is more dilute solution a. 1.0 M b. 0.5M c. 0.003M d. 0.005M

46. 2 moles of Na2So4 are dissolved in 1 dm3. Molarity wil be a. 1M b. 2M c. 3M d. 0.5M

47. When kcl is dissolved in water _______ will be product a.K and cl b. K and cl2 c. K--+cl+ d. K++cl--

48. Molarity is the number of moles of solute dissolved in ___ a. 1kg of solvent b. 1dm3 of solvent c. 1dm3 of solution d.


49. The molarity of NaoH solution by dissolving 4g of it in 250dm3 of water is _______ a. 0.4M b. 0.004M c. 0.2M d.


50. The percentage composition of solution is expressed in _______ ways a. Two b. Three c. Four d.None

Answer Keys

1. b 11. c 21. c 31. b 41. d

2. a 12. c 22. b 32. c 42. a

3. a 13. a` 23. b 33. b 43. d

4. b 14. b 24. b 34. a 44. b

5. c 15. c` 25. b 35. c 45. c

6. b 16. d 26. a 36. b 46. b

7. c 17. b 27. b 37. b 47. d

8. b 18. c 28. d 38. b 48. c

9. b 19. c 29. b 39. c 49. b

10. b 20. c 30. c 40. a 50. c



Chap No 7: Electrochemistry


1) Gain of electron is called _______

a. Oxidation b. Reduction c. Redex d. None

2) In N2+3H2→ 2NH3 , N is _______

a. Oxidized b. Reduced c. constant d. None

3) In redax reaction No of lose electron are _______ to no of gain electron

a. Greater b. Smaller c. Equal d. None

4) The oxidation No of oxygen in H2O2

a. −2 b. +2 c. −1 d. +1

5) The oxidation No of Mn in KMno4 is _______

a. +4 b. −7 c. +7 d. −4

6) The maximum oxidation No of Sulpher is _______

a. +2 b. +4 c. +6 d. +7

7) The doner of hydrogen is called _______

a. Oxidizing Agent b. Reducing Agent c. Both d. None

8) Which one is oxidizing agent

a. cl2 b. O2 c. H25 d. None

9) There are _______ Types of electrochemical cell

a. Four b. Three c. Two d. None

10) Which one is strong electrolyte

a. NH4oH b. C6H6 c. None d. a and b

11) Cations are gathers at _______

a. Anode b. Cathode c. None d. Both a & b

12) Anode is _______ charge electrode

a. Positive b. Negative c. Neutral d.

13) The Reduction take place at _______

a. Anode b. Cathode c. None d. Both a & b

14) The chemical decomposition of an electrolyte is _______

a. Electrolytic cell b. Electrolysis c. Dancil cell d. None

15) 2cl →cl2+2e there is _______

a. Oxidation b. Reduction c. Both d. None

16) For the refining of cu temperature is _______

a. 40𝑖 b. 50𝑖 c. 60 d. 100𝑖

17) Which one is good conductor of electricity

a. 2n b. cu c. Gold d. None

18) Nelson cell is the example of _______

a. Electrolytic cell b. Voltaic cell c. Galvanic cell d. None

19) By electro-refining _______ % pure copper is obtained

a. 90 b. 99 c. 99.99 d. 95

20) Which one is less reactive metals amoung these

a. gold b. Mg c. Cll d. None

21) Salt bridge is used in _______

a. Nelson Cell b. Daniel cell c. Down cell

22) The slat bridge is filled with electrolytic gel called

a. Sludge b. Agar c. Sagar

23) Voltmeter is used to measure _______

a. Voltage b. Current c. temperature

24) In daniel cell cathode is _______ and Anode is _______

a. Positive & Negative b. Negative Positive c. None

25) The batteries used in toys are work on _______ principle

a. Nelson cell b. Down cell c. Daneil Cell

26) Battery was invented in _______

a. 1749 b. 1849 c. 1949 d. None

27) The dry cell is made of _______ container

a. Non-Metalic b. Zn c. Metalic d. None

28) _______ cell is water proofed with wax

a. Nelson cell b. Dry cell c. Down cell d. None

29) The Deposition of one metal on other is called _______

a. Electrolysis b. Purification of metal c. Electroplater d. None

30) _______ Anode is used to maintain the temperature of cell and not allow the molten Nacl to solidify

a. C4 b. 2n c. Graphite d. None

31) Sodium Metal was first discovered in _______

a. 1800 b. 1807 c. 1822 d. None

32) In down cell cathode is _______ shape

a. Rod b. Circular c. Square d. None

33) In down cell molten Na was collected in _______

a. Anode b. Cathode c. Both d. None

34) The M.P of Nacl is _______

a. 97.6i b. 600𝑖 c. 801𝑖 d. None

35) To Reduce/Decrease the M.p of Nacl _______ is added

a. Cacl2 b. CaCo3 c. Mgcl2 d. None

36) For the stable oxide layer the PH range _______

a. 7-9 b. 6-8 c. 6-9 d. 9-7

37) Fe2O3 is the chemical formula of _______

a. Ferrous oxide b. Feric Oxide c. Iron oxide d. None

38) _______ cell is perforated

a. Daneil cell b. Dry Cell c. Nelson d. None

39) Asbestos is toxic and caused _______

a. T.B b. Cancer c. Malaria d. None

40) The necessary condition for rusting is _______

a. Moisture & Air b. Moisture & Co2 c. Air 7 Co2

41) The process of Rusting is start from _______

a. Dents b. Plane surface c. Both d. None

42) The _______ of electron demage the metals.

a. Gain b. Lose c. Share

43) The rust mass is _______ and porouc in nature

a. Hard b. Paste form c. Soft d. None

44) _______ is act as corresion inhibitors.

a. Nickle b. Paints c. Glyaine d. None

45) A concentrated aqueous of Nacl is called

a. Brine b. Electrolytic solution c. Both d. None

46) Which organic acid is act as presentative of food

a. Hcl b. H2So4 c. CH3CooH d. None

47) The oxidation No of C in Co2 is _______

a. -2 b. -1 c. 0 d. +4

48) Caustic soda is prepared by _______ cell

a. Daniel cell b. Nelson c. Down

49) _______ cell is used for extraction of numerical

a. Nelson b. Down c.Daniel

50) How many Types of electrolytic cell

a. 2 b. 5 c. 7 d. None

Answer Keys

1. b 11. b 21. b 31. b 41. a

2. b 12. a 22. b 32. b 42. b

3. c 13. b` 23. a 33. b 43. c

4. c 14. b 24. b 34. c 44. c

5. c 15. a` 25. c 35. a 45. a

6. a 16. b 26. a 36. a 46. c

7. b 17. b 27. d 37. b 47. d

8. a 18. a 28. b 38. c 48. b

9. c 19. b 29. c 39. b 49. b

10. a 20. a 30. c 40. a 50. a


Chap No 8: Chemical Reactivity


1) Which one catch fire when placed in air

a. Na b. Fe c. Al d. Gold

2) The oxides of metals are _______

a. Acids b. Bases c. Neutrals d. None

3) Which metal is found in liquid state

a. Au b. Hg c. Fe d. Ag

4) Tin is _______

a. Metal b. Non metal c. Metalloid d. None

5) Earth is made of 8% of _______

a. Fe b. Al c. Ca d. K

6) Metallic character is increased with increases in _______

a. Electro negativity b. Electron affinity c. Electro positivity

7) Non Metallic character is _______ in periods

a. decreases b. Increases c. Constant d. None

8) The alkali comes from _______ language

a. Greek b. Arabic c. Latin d. English

9) The _______ metals form mono positive ions

a. Alkali b. Alkaline earth c. Non d. Metaliods

10) Which one is found in the form of spodumene

a. Na b. Ca c. Mg d. Al

11) Which one of group I metal is not found in nature

a. Rb b. Cs c. Fr d. K

12) The I.E of alkali metals is very _______

a. High b. Low c. Constant d. None

13) Which one is stored in kerosene oil

a. Na b. Li c. K d. Mg e. a& c

14) There are _______ alkaline earth metals

a. Five b. Six c. Seven d. None

15) The second name of calcium sulphate is _______

a. Gypsum b. Epsomite c. Barite d. None

16) Which one is radio active element

a. Cs b. Rb c. Ra d. Be

17) Which one have highest I.E Values

a. K b. Na c. Li d. Cs

18) In periods from left to right B.P of the element is _______

a. Increased b. Decreased c. Constant d. None

19) The sodium metal was first discovered in _______

a. 1807 b. 1707 c. 1607 d. 1907

20) The M.P of Na is _______𝑖

a. 100𝑖 b. 97𝑖 c. 97.6𝑖 d. None

21) na act as powerful _______ agent

a. Oxidizing b. Reducing c. Both d. None

22) The formula of sodium bicarbonate is _______

a. Na2Co3 b. NaNH2 c. NaHCo3 d. None

23) In desulphurization _______ metals is removed

a. Na b. Oxygen c. Supher d. None

24) The permanent hardness of water is due _______

a. Na b. Mg c. K d. Li

25) The B.P of Mg is _______ 𝑖

a. 880 b. 651 c. 1106 d. None

26) The atomic No of calcium is _______

a. 40 b. 20 c. 30 d. None

27) The formula of magnesa is _______

a. MgH2 b. Mgcl c. Mgo d. None

28) Balanced this equation Mg+ N2→MgN

a. 3mg+H2→ Mg3N2 b. 2Mg+N2 →2MgN c.2Mg+N2→ Mg2N2

29) It is used in steel making

a. Na b. Mg c. Ca d. K

30) The density of Ca is _______ glcm3

a. 1.55 b. 1.74 c. 0.971 d. None

31) The metals of group 1 and 2 are called _______

a. Hard metals b. Soft metals c. Noble d. None

32) Hard metals have _______ I.E values

a. High b. Low c. Constant d. None

33) The soft metals have _______ B.P than H.M

a. High b. Low c. Equal d. None

34) Those metals which are chemically insert _______

a. Hard metal b. Soft metal c. Noble metal d. None

35) Which one is precious metal _______

a. Ag b. Au c. Pt d. All of these

36) Pure silver is very _______

a. Soft b. Hard c. Noble d. None

37) Platinum is the _______ most common element in earth

a. 72th b. 82th c. 92th d. 62th

38) Which metal is used for coins

a. Platinum b. Copper c. Silver d. None

39) Bromine is non-metal in _______ state

a. solid b. Liquid c. Gaseous d. Plasma

40) Alkali metals are _______ Agents

a. Oxidizing b. Reducing c. Dehydrating d. All

41) The halogen present in solid form is _______

a. Cl b. F c. I d. Br

42) The oxides of calcium Cao is _______

a. Acidic b. Basic c. Amphoteric d. Neutron

43) Which one of following is not an alkali metal

a. Francium b. cesium c. Rubidum d. Redium

44) Which one is more reactive

a. Cl b. Br c. I d. F

45) Bleaching powder is formed by Ca((oH)2+?

a. F2 b. Br2 c. Cl2 d. I2

46) Which one is react in the presence of sunlight

a. F b. Cl c. Br d. I

47) Which one have lowest M.P

a. Hg b. Ca c. CS d. Br

48) There are _______ non metalic in P.T

a. 17 b. 26 c. 18 d. 27

49) The M.P Of bromine is

a. 38.87𝑖 b. 29.76𝑖 c. 50.49𝑖 d. 7.2𝑖

50) Halogens consists of _______ elements

a. Five b. Six c. Seven d. Eight

Answer Keys

1. a 11. c 21. b 31. b 41. c

2. b 12. a 22. c 32. a 42. b

3. b 13. e` 23. c 33. b 43. d

4. a 14. b 24. b 34. c 44. d

5. b 15. a` 25. c 35. d 45. c

6. a 16. c 26. b 36. a 46. b

7. b 17. c 27. c 37. a 47. d

8. b 18. a 28. a 38. c 48. d

9. a 19. a 29. c 39. b 49. d

10. a 20. c 30. a 40. b 50. a


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MCQs of Chemistry FSc Level