1. Physical chemistry
  2. 1. The solid state
    2. Language of Chemistry
    3. Gaseous and Liquid states
    4. Stoichiometry
    5. Solutions
    6. Structure of Atom
    7. Chemical equilibrium
    8. Nuclear chemistry (Radioactivity)
    9. Ionic equilibrium
    10. Chemical Bonding
    11. Chemical kinetics
    12. Concepts of Acids, Bases and Salts
    13. Surface catalysis and Colloids
    14. Redox reactions
    15. Chemical energetics
    16. Volumetric analysis
    17. Electrochemistry
  3. Inorganic chemistry
  4. 18. Introduction
    19. Periodic table
    20. Hydrogen and its compounds
    21. General aspects of Metallergy
    22. Alkali metals
    23. Alkaline metals
    24. Boron family
    25. Carbon family
    26. Nitrogen family
    27. Oxygen family
    28. Fluorine family
    29. Inert gases
    30. Transition metals
    31. Coordination compounds
    32. Analytical chemistry
  5. Organic chemistry
  6. 33. Purification and analysis of organic compounds
    34. Nomenclature of Organic compounds
    35. Reaction Mechanisms
    36. Hydrocarbons
    37. Haloalkanes (Alkyl halides)
    38. Alcohol, Phenol and Ether
    39. Aldehyde and Ketones
    40. Carboxylic acids
    41. Compounds conatining Nitrogen
    42. Polymers
    43. Chemistry in daily life
Inorganic chemistry
19. Periodic table
1. Which one of the following has highest electronegativity?

[I.E.]

  • Cl
  • N
  • O
  • S
2. The element Uranium (At. No. 92) belongs to

[I.E. 2003]

  • Representative elements
  • Noble (inert) gases
  • Transition elements
  • Inner transition element
3. Atomic radius is nearly equal in

[I.E. 2006]

  • Na, K, Cs, Fr
  • B, C, N, O
  • Cr, Mn, Fe, Co
  • He, Ne, Ar, Kr
4. Lithium shows diagonal relationship with Magnesium because

[BPKIHS 2006]

  • They have same electromagnetic property
  • They have same atomic radius
  • They have same ionization energy
  • They have same electronegativity
5. The correct sequence of ionization energies is

[BPKIHS 2011]

  • Li < Be < B < C
  • Li < Be > B > C
  • Li < Be > B < C
  • Li < Be < B > C
6. Correct order of increasing ionization energy is

[I.E. 2006]

  • Na < P < N < Ne
  • Na < N < P < Ne
  • Rb < K < Na < Li
  • Na < Ne < P < N
7. Which of the following elements has the lowest ionization energy?

[I.E.]

  • Be
  • Mg
  • Ca
  • Rb
8. Which of the following is correct order of electron affinity?

[I.E.]

  • F > Cl > Br
  • Cl > F > Br
  • Br > Cl > F
  • F > Br > Cl
9. Alkali metal in each period has

[IOE]

  • Smallest size
  • Lowest ionization energy
  • Highest electronegativity
  • Highest ionization energy
10. Chemical and physical properties of an element are the function of their

[IOE]

  • Atomic size
  • Atomic energy
  • Atomic volume
  • Atomic number
11. According to Mendeleev, properties of elements are periodic function of their

[IOE]

  • Atomic number
  • Atomic size
  • Atomic weight
  • Atomic energy
12. Variable valency is generally shown by

[IOE]

  • Representative elements
  • Transitional elements
  • p-block elements
  • Non metals
13. Iron belongs to which block of periodic table?

[IOE]

  • s-block
  • p-block
  • d-block
  • f-block
14. Beryllium shows diagonal relationship with

[IOE]

  • Mg
  • Al
  • Si
  • Li
15. The ability of an atom to attract shared electron pair towards itself is called

[IOM 2002]

  • Electronegativity
  • Electron affinity
  • Ionization potential
  • Reducing power
16. Which of the following is the most electronegative atom?

[IOM 1996]

  • Oxygen
  • Nitrogen
  • Fluorine
  • Sodium
17. The outermost electronic configuration of most electronegative atom is

[IOM 1995]

  • ns²np⁴
  • ns²np⁵
  • ns¹
  • ns²np³
18. The most homogenous family in the periodic table is

[IOM 1995]

  • Alkaline metals
  • Alkaline Earth metals
  • Volatile metal
  • Coinage metals
19. Moving from top towards bottom in periodic table

[IOM 1995]

  • Basic nature of oxide decreases
  • Basic nature of oxide increases
  • Electronegativity increases
  • None of the above
20. Electron attracting tendency of an element is called

[BPKIHS]

  • Electron affinity
  • Electronegativity
  • Lattice energy
  • Ionic potential
21. Newland is famous for giving

[BPKIHS]

  • Long form of periodic table
  • Octave law
  • Law of triads
  • Unitary hypothesis
22. Increasing order of size is

[BPKIHS]

  • Ca²⁺ < Cl⁻ < S²⁻ < P³⁻
  • Ca²⁺ < S²⁻ < Cl⁻ < P³⁻
  • P³⁻ < S²⁻ < Cl⁻ < Ca²⁺
  • P³⁻ < Cl⁻ < S²⁻ < Ca²⁺
23. Correct order of electron affinity

[BPKIHS]

  • Cl > S > O > N
  • O > Cl > S > N
  • Cl > N = S > O
  • N > O > S > Cl
24. In periodic table, the element which comes after calcium is

[BPKIHS]

  • Scandium
  • Titanium
  • Manganese
  • Cobalt
25. Mendeleev proposed his periodic law on the basis of

[IOM 1992]

  • Atomic number
  • Atomic weight
  • Valency
  • Equivalent weight
26. Which of the following represents the correct order of ionic radii?

[MOE 2065]

  • Li⁺ < Na⁺ < K⁺ < Rb⁺
  • Li⁺ > Na⁺ > K⁺ > Rb⁺
  • Li⁺ = Na⁺ = K⁺ = Rb⁺
  • Rb⁺ > K⁺ < Na⁺ > Li⁺
27. Which sequence is correct if elements are arranged by ascending atomic number?

[IOM 2008]

  • Fe, Co, Ni, Cu
  • Co, Fe, Ni, Cu
  • Fe, Ni, Co, Cu
  • Cu, Fe, Co, Ni
28. Atomic number 27 belongs to which block?

[MOE 2008]

  • s
  • p
  • d
  • f
29. The character of hydrogen which is different from halogen is

[Bangladesh 2008]

  • Ionisation energy
  • Electropositive nature
  • Electronegativity
  • Reaction with alkali metals
30. Atomic number of calcium is

[IOM 2000]

  • 11
  • 20
  • 40
  • 19
ADDITIONAL QUESTIONS
1. The first attempt to classify elements was made by
  • Mendeleeff
  • Newlands
  • Lothar Meyer
  • Dobereiner
2. Mendeleeff's periodic law is based on
  • Atomic number
  • Atomic weight
  • Number of neutrons
  • None of these
3. In the modern periodic table, elements are arranged in
  • Increasing mass
  • Increasing volume
  • Increasing atomic number
  • Alphabetically
4. Eka-aluminium and Eka-silicon are known as
  • Gallium and Germanium
  • Aluminium and Silicon
  • Iron and Sulphur
  • Proton and Silicon
5. Aluminium is diagonally related to
  • Li
  • Be
  • C
  • B
6. If the valence shell electronic structure for an element is ns²np⁵, this element will belong to the group of
  • Alkali metals
  • Inert metals
  • Noble gases
  • Halogens
7. An atom with atomic number 21 belongs to the category of
  • s-block elements
  • p-block elements
  • d-block elements
  • f-block elements
8. Chloride of an element A gives neutral solution in water. In the periodic table, the element A belongs to
  • First group
  • Third group
  • Fifth group
  • First transition series
9. Which one of the following belongs to representative element of a group in the periodic table?
  • Lanthanum
  • Argon
  • Chromium
  • Aluminium
10. The lightest metal is
  • Li
  • Fe
  • Cu
  • Ag
11. Which of the following is the smallest cation?
  • Na⁺
  • Mg²⁺
  • Ca⁺
  • Al³⁺
12. Which of the following is largest ion?
  • Na⁺
  • Mg²⁺
  • O²⁻
  • F⁻
13. Which of the following is smallest in size?
  • Na⁺
  • Mg²⁺
  • Cl⁻
  • F⁻
14. Which of the following is not isoelectronic?
  • Na⁺
  • Mg²⁺
  • O
  • Cl⁻
15. Which one is the correct order of the size of the iodine species?
  • I⁻ > I > I⁺
  • I > I⁺ > I⁻
  • I⁺ > I > I⁻
  • I⁻ > I⁺ > I
16. The size of the following species increases in the order
  • Mg²⁺ < Na⁺ < F⁻ < Al
  • F⁻ < Al < Na⁺ < Mg²⁺
  • Al < Mg < F⁻ < Na⁺
  • Na⁺ < Al < F⁻ < Mg²⁺
17. Al³⁺ has a lower ionic radius than Mg²⁺ because
  • Mg atom has less number of neutrons than Al
  • Al³⁺ has a higher nuclear charge than Mg²⁺
  • Their electronegativities are different
  • Al has a lower ionisation potential than Mg atom
18. The energy required to remove an electron of a gaseous atom from its ground state is called
  • Potential energy
  • Ionization energy
  • Electrode potential
  • Activation energy
19. Which of the following elements will have the lowest first ionisation energy?
  • Mg
  • Rb
  • Li
  • Ca
20. The first ionisation energy of lithium will be
  • Greater than Be
  • Less than Be
  • Equal to that of Na
  • Equal to that of F
21. Which of the following electronic configuration corresponds to an element having lowest ionisation energy?
  • 1s², 2s²2p⁶
  • 1s², 2s²2p⁶, 3s¹
  • 1s², 2s²2p¹
  • 1s¹, 2s²2p³
22. Which has maximum first ionization potential?
  • C
  • N
  • B
  • O
23. Which has lowest first ionization potential?
  • N
  • O
  • F
  • Ne
24. Which has the highest second ionisation potential?
  • Nitrogen
  • Carbon
  • Oxygen
  • Fluorine
25. Which one of the following elements has the highest ionisation energy?
  • [Ne]3s²3p¹
  • [Ne]3s²3p²
  • [Ne]3s²3p³
  • [Ar]3d¹⁰4s²4p¹
26. Which of the following order is correct for ionisation energy?
  • B < Be < C < O < N
  • B < Be < C < N < O
  • B < Be < N < C < O
  • Be > B > C > N > O
27. The correct order of second ionisation potential of carbon, nitrogen, oxygen and fluorine is
  • C < N > O > F
  • O > N > F > C
  • O > F > N > C
  • F > O > N > C
28. Of the following elements, which one has the highest electronegativity?
  • I
  • Br
  • C
  • F
29. Which of the following is the most electronegative?
  • Oxygen
  • Chlorine
  • Fluorine
  • Nitrogen
30. The electronegativity of Be is same as that of
  • Al
  • Mg
  • Na
  • Li
31. Which of the following represents the electronic configuration of d-block elements?
  • (n-1)s² nd¹⁻¹⁰
  • (n-1)d⁰⁻¹⁰ns⁰
  • (n-1)d¹⁻¹⁰ ns²np
  • (n-1)p⁰⁻¹⁰ns
32. Which one of the following elements has the maximum electron affinity?
  • F
  • Cl
  • Br
  • I
33. Electron affinity depends on
  • Atomic size
  • Nuclear charge
  • Atomic number
  • Atomic size and nuclear charge both
34. Elements of which group form anions most readily?
  • Oxygen family
  • Nitrogen group
  • Halogens
  • Alkali metals
35. Oxidizing action increases from top to bottom in the following order
  • Cl < Br < I < F
  • Cl < I < Br < F
  • I < F < Cl < Br
  • I < Br < Cl < F
36. Which is the weakest base among NaOH, Ca(OH)₂, KOH and Zn(OH)₂?
  • NaOH
  • KOH
  • Ca(OH)₂
  • Zn(OH)₂
37. Variable valency is generally exhibited by
  • Transition elements
  • Gaseous elements
  • Non-metals
  • s-Block elements
38. Paramagnetism is exhibited by molecules
  • Not attracted in a magnetic field
  • Containing only paired electrons
  • Carrying a positive charge
  • Carrying unpaired electrons
39. Which of the following ion is paramagnetic?
  • Zn²⁺
  • Ni²⁺
  • Cu²⁺
  • None of these
40. Which of the following shows highest magnetic moment?
  • N³⁻
  • Cr²⁺
  • Fe²⁺
  • Co²⁺
41. Variable valency is due to
  • Lone pair effect
  • Inert pair effect
  • High melting point
  • High boiling point
42. Which one of the following electronic configuration is not possible?
  • 1s¹, 2s²2p²
  • 1s², 2s²2p²
  • 1s¹, 2s¹2p¹
  • 1s², 2s⁵
43. One would expect proton to have very large
  • Ionization potential
  • Radius
  • Hydration energy
  • Charge
44. In the long form of the periodic table all the non-metals are placed in
  • s-block
  • p-block
  • d-block
  • f-block
45. The long form of periodic table is based on
  • Shape of the atom
  • Mass of the atom
  • Atomic number of the atom
  • Electronegativity
46. The correct order of first ionization potential of the elements is
  • Na > Mg > Al
  • Mg > Na > Al
  • Al > Mg > Na
  • Mg > Al > Na
47. Which of the following has maximum ionisation potential?
  • Mg
  • Si
  • Al
  • P
48. With reference to ionization potential which one of the following sets is correct?
  • Li > K < Cs
  • B > Li > K
  • Cs > Li > B
  • Cs < Li < K
49. Highest ionization potential is shown by
  • Alkali metals
  • Transition elements
  • Halogens
  • Inert gases
50. The atomic radius of elements of which of the following series should be nearly the same?
  • Na, K, Rb, Cs
  • Li, Be, B, C
  • Fe, Co, Ni, Cu
  • F, Cl, Br, I
51. The decreasing order of the size of the following ions is
  • Li⁺ > H⁺ > H
  • H⁺ > H > Li⁺
  • F⁻ < O²⁻ < N³⁻
  • Fe³⁺ < Fe²⁺ < Fe⁴⁺
52. The correct order of radii is
  • N < Be < B
  • Na < Li < K
  • Na < Li < K
  • Li < Na < K
53. Which has the smallest size?
  • Na
  • Mg²⁺
  • Al³⁺
  • P⁵⁺
54. Which one of the following represents the correct order of size?
  • Na < Mg < K
  • P < Cl < B
  • O²⁻ < F⁻ < Mg²⁺
  • I⁻ < Br⁻ < Cl⁻
55. On going from right to left in a period in the periodic table, the electronegativity of the elements
  • Increases
  • Decreases
  • Remains unchanged
  • Decreases first then increases
56. The correct order of electron affinity of B, C, N and O is
  • O > C > N > B
  • B > N > C > O
  • O > C > B > N
  • O > B > C > N
57. Fluorine has low electron affinity than chlorine because of
  • Smaller radius of fluorine, high density
  • Smaller radius of chlorine, high density
  • Bigger radius of fluorine, less density
  • Smaller radius of chlorine, less density
58. Which of the following is not paramagnetic?
  • Cl
  • Be
  • Ne⁺
  • As³⁺
59. Which of the following is not paramagnetic?
  • S
  • N₂
  • O₂
  • NO
60. Lanthanides contraction is due to increase in
  • Shielding by 4f-electrons
  • Atomic number
  • Effective nuclear charge
  • Size of 4f-orbital
61. According to modern periodic law, variations in the properties of elements is related to their
  • Atomic weights
  • Nuclear weights
  • Atomic numbers
  • Neutron-proton ratios
62. Increasing order of density is
  • Li < Na < K < Rb < Cs
  • Li < K < Na < Rb < Cs
  • Cs < Rb < K < Na < Li
  • K < Li < Na < Rb < Cs
63. The lanthanide contraction is responsible for the fact that
  • Zr and Y have about the same radius
  • Zr and Nb have similar oxidation states
  • Zr and Hf have about the same radius
  • Zr and Zn have the same oxidation state
64. Increasing order of electron affinity is
  • N < O < Cl < Al
  • O < N < Al < Cl
  • Al < N < O < Cl
  • Cl < N < O < Al
65. Outer electronic configuration of K, Cu and Cr are respectively
  • 4s¹, 3d¹⁰, 3d⁵
  • 4s¹, 3d¹⁰, 3d¹
  • 4s¹, 3d¹, 3d¹
  • 4s¹, 3d³, 3d¹
66. Lanthanides and actinides are also called as
  • Short periods
  • Inner transition elements
  • Long periods
  • Main transition elements
67. Which of the following sets is of coinage metal?
  • Cu, Ag, Au
  • Zn, Cd, Hg
  • Au, Ag, Zn
  • Li, Na, K
68. The group of elements in which the differentiating electron enters the antepenultimate shell are called
  • f-block elements
  • p-block elements
  • s-block elements
  • d-block elements
69. Which is not soluble in water?
  • PbSO₄
  • CuSO₄
  • Bi₂(SO₄)₃
  • Na₂SO₄
70. Which of the following is second most electronegative element?
  • Chlorine
  • Oxygen
  • Sulphur
  • Fluorine
71. In the periodic table, metals usually used as catalysts belong to
  • d-block
  • f-block
  • s-block
  • p-block
72. Which is correctly arranged in increasing size?
  • F < O < C < Cl < B
  • C < O < F < Cl < Br
  • Cl < Br < F < C < O
  • O < F < C < Cl < Br
73. Ionization energy decreases down the group due to
  • Increase in charge
  • Increase in atomic size
  • Decrease in atomic size
  • Decrease in shielding effect
74. Increase in atomic size down the group is due to
  • Increase in number of electrons
  • Increase in number of protons and neutrons
  • Increase in number of protons
  • Increase in number of protons, neutrons and electrons
75. The only non-metal which is liquid at room temperature is
  • NH₃
  • Br₂
  • Hg
  • None of these
76. Lanthanides contraction is due to increase in
  • Shielding by 4f-electrons
  • Atomic number
  • Effective nuclear charge
  • Size of 4f-orbital
77. Lanthanides and Actinides are also called as
  • Short periods
  • Inner transition elements
  • Long periods
  • Main transition elements
78. In the periodic table, metals usually used as catalysts belong to
  • d-block
  • f-block
  • s-block
  • p-block
79. Increase in atomic size down the group is due to
  • Increase in number of electrons
  • Increase in number of protons and neutrons
  • Increase in number of protons
  • Increase in number of protons, neutrons and electrons
80. The long form of the periodic table is based on
  • Atomic number
  • Atomic mass
  • Electronic configuration
  • Effective nuclear charge
81. The only non-metal which is liquid at room temperature is
  • NH₃
  • Br₂
  • Hg
  • None of these
SAURAV QUESTION
1. Technetium is named by Mendeleev as

[2022]

  • Eka boron
  • Eka aluminium
  • Eka manganese
  • Eka silicon
2. Increasing order of metallic character

[2022]

  • Na, Li, K
  • Be, Mg, Ca
  • P, Mg, Cl
  • N, Mg, S
3. X belongs to group IIA and Y belongs to group VIIA. The formula of the compound formed by them is

[2022]

  • X₂Y
  • XY₂
  • XY
  • X₂Y₃
4. Mg²⁺ is isoelectronic with

[2021]

  • Na⁺
  • Li⁺
  • Ca²⁺
  • Ba²⁺
5. Electronic configuration having highest first I.E is

[2017 Re-exam]

  • 1s² 2s² 2p³
  • 1s² 2s² 2p⁴
  • 1s² 2s² 2p⁵
  • 1s² 2s² 2p⁶
6. If the electronic configuration of an element ends at (n-1)d¹⁰ ns² then it falls in

[2017]

  • IIB
  • VIB
  • IVB
  • VIII
7. The atom with highest 2ⁿᵈ ionization potential is

[2016]

  • Sulphur
  • Argon
  • Sodium
  • Magnesium
8. The VII A group of the periodic group is known as halogen family due to the property of forming

[2016]

  • Acid
  • Salt
  • Ores
  • Amphoteric nature
9. Which of the following has the highest ionization energy?

[2014]

  • 1s² 2s² 2p³
  • 1s² 2s² 2p⁶ 3s² 3p⁴
  • 1s² 2s² 2p⁴
  • 1s² 2s² 2p⁶ 3s² 3p³
10. Which of the following electronic configuration given for some neutral atoms would be expected to have highest second ionization energy IE₂?

[2010]

  • 1s² 2s² 2p⁴
  • 1s² 2s² 2p⁵
  • 1s² 2s² 2p³
  • 1s² 2s² 2p⁶
11. Arrange these in increasing Atomic Size

[2000]

  • Na, K, P, N
  • N, P, Na, K
  • P, Na, K, N
  • K, Na, N, P
12. Moving from top towards bottom in periodic table

[1995]

  • Basic nature of oxide decreases
  • Basic nature of oxide increases
  • Electronegativity increases
  • None
13. Al is diagonally related to

[1994]

  • Be
  • Br
  • B
  • Sr
14. Which property of element is always a whole number?

[2071 Mangsir 20]

  • Atomic weight
  • Equivalent weight
  • Atomic Number
  • Atomic Volume
15. Sodium and potassium have similar chemical and physical properties. This is best explained by the fact that both elements are

[2070 Poush]

  • Active elements
  • Are in period one of the periodic table
  • Have the same outer electronic configuration
  • Have relatively low first ionization energies
16. Which of the following elements have least value for electronegativity?

[2069 Kartik]

  • Oxygen
  • Boron
  • Carbon
  • Nitrogen
17. The decreasing order of atomic radii for Be, Na and Mg is

[2068 Kartik]

  • Na > Mg > Be
  • Mg > Na > Be
  • Be > Na > Mg
  • Be > Mg > Na
18. While moving from left to right in a periodic table which of the following variable decreases?

[2067 Kartik]

  • Ionization affinity
  • Ionization potential
  • Atomic radius
  • Electronegativity
19. Element with atomic number 19 belongs to which block of the periodic table?

[2066 Poush]

  • s
  • p
  • d
  • f
20. Which of the following represents the correct order of ionic radii in aqueous medium?

[2065 Marg]

  • Li⁺ < Na⁺ < K⁺ < Rb⁺
  • Li⁺ > Na⁺ > K⁺ > Rb⁺
  • Li⁺ = Na⁺ = K⁺ = Rb⁺
  • Rb⁺ > K⁺ > Na⁺ > Li⁺
21. Atomic number 27 belong to which block?

[2065 Baisakh]

  • s
  • p
  • d
  • f
22. Oxidation number of Nitrogen ranges from

[2055 Bhadra]

  • -3 to +5
  • 3 to 5
  • +3 to -5
  • None of the above
23. Which element was not included in Mendeleev's periodic table?

[2018]

  • Lithium
  • Gallium
  • Francium
  • Helium
24. It is impossible for any two electrons in the same atom to have all the four quantum numbers identical. It states

[2017]

  • Hund's rule
  • Uncertainty rule
  • Pauli's exclusion principle
  • Aufbau rule
25. Which one of the following ion has the largest radius?

[2017]

  • Ca²⁺
  • S²⁻
  • K⁺
  • Cl⁻
26. Nitrogen is more stable than oxygen because of

[2012]

  • More stable ½ filled orbitals
  • Penetration effect
  • Low electron affinity
  • Electronegativity
27. In any given orbital electron fill up in increasing order of energy is it known as

[2006]

  • Aufbau principle
  • Pauli's exclusion principle
  • Hund's rule
  • Uncertainty principle
28. In periodic table the element which comes after calcium is

[2006]

  • Scandium
  • Titanium
  • Manganese
  • Cobalt
29. On moving from top to down in group IV

[2011]

  • Non-metallic property goes on increasing
  • +2 oxidation state becomes less stable than +4 oxidation state
  • Density goes on increasing
  • Covalent compounds become more stable
HYDROGEN
1. H2O2 is formed when a compound is reacted with H₂SO4. The compound is

[2022]

  • MnO₂
  • BaO
  • PbO₂
  • Na₂O₂
2. Ortho and para isomer of hydrogen are separated by

[2017]

  • Paper chromatography
  • Gas chromatography
  • Exchange reaction
  • Solvent extraction
3. Ortho and para hydrogen are distinguished by

[2011]

  • Spin of electron
  • Spin of proton
  • Atomic number
  • Spin of nucleus
4. Hydrogen cannot be obtained by

[2005]

  • Zn and dil. H₂SO₄
  • Zn + dil. HNO₃
  • Mg + H₂SO₄
  • Mg and H₂O
5. Calgon is used as a water softener is

[2004]

  • Na₂[Na₄(PO₃)₆]
  • Na₄[Na₂(PO₃)₆]
  • Na₆[Na₂(PO₃)₆]
  • Na₄[Na₄(PO₃)₆]
6. Given colourless liquid will be determined whether it is water or not by

[1998]

  • Evaporation
  • Litmus paper
  • Adding a pinch of anhydrous copper sulphate
  • Adding a few drops of phenolphthalein
7. In which of the following compounds does hydrogen have negative valency?

[1998]

  • NH₃
  • H₂O
  • NaH
  • HCl
8. Which of the following is not a water softener?

[2070 Poush]

  • Calgon
  • Permutit
  • Sodium carbonate
  • Sodium sulphate
9. Calgon process for purification of water involves

[2065 Baisakh]

  • Ion-exchange
  • Formation of soluble complex
  • Scum
  • Precipitation
10. The character of hydrogen which is different from halogen is

[2009 MOE Banga]

  • Ionisation energy
  • Electropositive nature
  • Electronegativity
  • Reaction with alkali metals
11. The exhausted Zeolite in a water softener is regenerated with 10% solution of

[2007]

  • Sodium chloride
  • Potassium chloride
  • Aluminum chloride
  • Hydrogen chloride
12. The permanent hardness of water is due to dissolved

[2006]

  • Carbonate of K and Na
  • Bicarbonate of Ca and Mg
  • Sulphate of K and Na
  • Nitrate of Na and Mg
13. Which option is false regarding ortho and para hydrogen?

[2018]

  • Ortho form is more stable than para form
  • Ortho form has higher pressure than para form
  • Ortho form is more conductive than para form
  • Ortho form has more specific heat than para form
14. Froth floatation process is used for

[2021]

  • Wetting process
  • Bessemerization
  • Calcination
  • Liquation
15. Metals in german silver

[2019]

  • Cu + Sn
  • Cu + Zn
  • Cu + Zn + Ni
  • Cu + Al
16. Auto reduction is used to extract

[2017 Re-exam]

  • Cu and Hg
  • Cu and Ag
  • Cu and Au
  • Hg and Ag
17. During metallurgy fused metal is obtained during

[2017]

  • Smelting
  • Roasting
  • Calcination
  • Froth floatation
18. Heating of pyrites to remove sulphur is

[2015]

  • Bessemerization
  • Roasting
  • Calcination
  • None
19. Hydrated Alumina is converted to anhydrous form by

[2009]

  • Roasting
  • Calcinations
  • Smelting
  • Leaching
20. Acid flux is
  • SiO₂
  • CaO
  • CaCO₃
  • MgO
21. Deposition of the layer of Zn over iron is called
  • Vulcanization
  • Galvanization
  • Annealing
  • Tempering
22. In the blast furnace iron ore is reduced by

[2071 Mangsir]

  • Carbon
  • Carbon dioxide
  • Carbon monoxide
  • Lime stone
23. Which of the following is the most abundant element in the Earth's Crust?

[2069 Marg]

  • Hydrogen
  • Oxygen
  • Iron
  • Carbon
24. Leaching of ores is a process of

[2067 Ashad]

  • Concentration
  • Refining
  • Reduction
  • Calcinations
25. Which of the following oxide can be reduced by carbon atom?

[2063 Falgun]

  • Al₂O₃
  • Na₂O
  • CuO
  • ZnO
26. Hall's process is used for

[2017]

  • Extraction of sodium
  • Extraction of barium
  • Purification of bauxite
  • Extraction of corundum
27. Froth floatation is applied for all except which ore

[2010]

  • Argentite
  • Galena
  • Copper pyrite
  • Pitchblende
28. Abundance of the following elements in the Earth's crust is in order of

[2007]

  • Si > O > Al
  • O > Si > Al
  • Al > O > Si
  • Al > Si > O
FROM SLIDES
1. What is the screening effect in atoms?
  • The increase in nuclear charge due to inner electrons
  • The reduction in effective nuclear charge due to inner electrons
  • The increase in atomic radius due to electron shielding
  • Decrease in Ionization energy due to repulsion
2. Which of the following factor increase screening effect?
  • Increase in number of protons
  • Increase in number of neutrons
  • Increase in number of inner shell electrons
  • Increase in electronegativity
3. The effective nuclear charge
  • Increases down the group
  • Increases in the periodic table (towards right)
  • Depends upon the screening effect
  • All of the above
4. In third row of periodic table from Na to Cl [MP PET 1986]

[1986]

  • Electronegativity increases
  • Electronegativity decreases
  • Ionisation energy decreases
  • Atomic volume increases
5. An atom with high electronegativity has [Kerala PMT 2003]

[2003]

  • Large size
  • High ionisation potential
  • Low electron affinity
  • Low ionisation potential
6. Between HF, HCl, HBr and HI, HF has the highest ionic character because [MP PMT 2007]

[2007]

  • F has the highest electron affinity
  • In HF, electronegativity difference is highest
  • F⁻ ion has the highest value of ionic radius
  • Atomic orbitals of H and F have almost similar energy
7. The most polar bond is [IIPMT 2005]

[2005]

  • N–Cl
  • O–F
  • N–N
  • N–F
8. On going from right to left in a period in the periodic table the electronegativity of the elements [MP PET/PMT 1998; MP PMT]

[1998]

  • Increases
  • Decreases
  • Remain unchanged
  • Decreases first then increases
9. Which one of the following represents the electronic configuration of the most electropositive element [AIIMS 1982; CPMT 1994; MP PMT 2000]

[1982, 1994, 2000]

  • [He]2s¹
  • [Xe]6s²
  • [He]2s²
  • [Xe]6s¹
10. Which element having following electronic configurations has minimum ionisation potential [KCET 1991; CBSE PMT 1991; Pb. PET 1999; BHU 2000]

[1991, 1991, 1999, 2000]

  • 1s¹
  • 1s², 2s² 2p⁶
  • 1s², 2s² 2p⁶, 3s¹
  • 1s², 2s² 2p²
11. A sudden large jump between the values of second and third ionisation energies of an element would be associated with the electronic configuration [CBSE PMT 1992; AFMC 1998; CPMT 1999; DCE 2006]

[1992, 1998, 1999, 2006]

  • 1s², 2s², 2p⁶, 3s¹
  • 1s², 2s², 2p⁶, 3s², 3p¹
  • 1s², 2s², 2p⁶, 3s², 3p²
  • 1s², 2s², 2p⁶, 3s²