Prepared By G Naseer (Lecturer Chemistry Leeds College)
MCQ
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
MCQ
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. πΌ b. π½ c. π
9) He used a radioactive source of _______ Metal.
a. Gold Foil b. Polonium c. Zinc
10) Rutherford Bombored _______ πΌ 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 π’ 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 2β 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
MCQ
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
MCQ
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. β -bond b. Sigma bond c. Both d.None
13. The sigma bond is _______ than β bond
a. Weaker b. Equal c. Stronger d. None
14. Sigma bond is represent by _______
a. β b. Δ c. o d. πΌ
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. 100π b. 85 π c. −85 π d. −95 π
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
MCQ
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 atoπ 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. -103π b. -252π c. -272π 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 π 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 25π 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 100π
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. Oπ b. 4π c. 25π
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
MCQ
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 _______ π a. 20π b. 22.2π c. 32.4π 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. _______ = π€π‘ ππ π πππ’π‘πππ‘ ππ π πππ£πππ‘ x 100 a. Molarity b. Solubility c. Viscoscity d. None
34. At 32.4π 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.
None
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.
0.002M
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
MCQ
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. 40π b. 50π c. 60 d. 100π
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. 600π c. 801π 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
MCQ
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 _______π
a. 100π b. 97π c. 97.6π 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 _______ π
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. 38.87π b. 29.76π c. 50.49π d. 7.2π
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