Periodic Classification of Elements & Periodicity (F.sc Part 2) Chemistry Mcqs

CHAPTER # 1
Periodic Classification of Elements & Periodicity

1. Which of the following pairs are chemically  
    dissimilar?

(A) Na and K     (B) Ba and Sr
(C) Zr and Hf     (D) Ca and Zn.

2. The total number of inner transition elements
is

(A) 10                 (B) 14
(C) 28                 (C) 30

3. The alkali metal which is liquid at 15oC is

(A) K                  (B) Cs
(C) Na                (D) None

4. Which of the following ion will form most water
    soluble hydroxide?

(A) K+                (B) Ni2+
(B) Zn2+             (C) Al3+

5. Which of the following has greatest tendency to lose electron?

(A) F                  (B) Fr
(B) S                  (C) Be.

6. The oxide of which of the following elements will be acidic in character

(A) Mg                (B) Rb
(C)  Li                 (C) CI

7. Which of the following is isoelectronic with carbon atom?

(A) Na+             (B) Al3+
(C) O2-              (D) N+
D
8. Which of the following ions are paramagnetic in character?

(A) Zn2+              (B) Cu+
(C) Ni2+              (D) Ag+

9. Ca2+ ion is isoelectronic with

(A) Mg2+            (B) Na+
(C) Ar                (D) Kr

10. Gradual addition of electronic shells in the noble gases causes a decrease in their

(A) Ionization energy        (B) atomic radius
(C) Boiling point                (D) density.




11. Which of the following has highest first ionization potential?

(A) Carbon                      (B) Oxygen
(C) Nitrogen                    (C) Boron.

12. Which of the following has the smallest size?

(A) Na+                          (B) Mg2+
(C) Al3+                          (D) CI

13. Which of the following element has the maximum  electron affinity?

(A) F                                  (B) S
(C) I                                   (D) CI.

14. Which of the following is isoelectronic as well as has the same structure as that of N2O ?

(A) N3H                               (B) H2O
(B) NO2                               (C) CO2

15. The atomic radius increases as we move down a group because

(A) Effective nuclear charge increases
                (B) Atomic mass increases
(C) Additive electrons are accommodated in
     new electron  level
(D) Atomic number increase.

16. Which one of the following is an incorrect
      statement?

(A)  The ionization potential of nitrogen is
      greater than that of chlorine
(B)  The electron affinity of fluorine is greater
       than that of chlorine
(C)  The ionization potential of beryllium is
       greater than that of boron
(D) The electronegativity of fluorine is greater
      than that of chlorine.

17. Electron affinity depends on

(A) Atomic size
(B) Nuclear charge
(C) Atomic number
(D) Atomic size and nuclear charge both.

18. Two elements whose eletronegativities are 1.2 and 3.0, the bond formed between them would
be

(A) Ionic                           (B) covalent
(C) Coordinate                  (C) metallic.








19. Ionic radii are

(A) Directly proportional to square of effective
      nuclear charges
(B) Inversely proportional to effective nuclear
      charge
(C) Inversely proportional to square of
       effective nuclear charge
(D) Directly proportional to effective nuclear
     charge.

20. Which of the following oxides is atmospheric in
      character?

(A) CaO                    (B) CO2
(C) SiO2                    (D) SnO2

21. Mark the correct statement:

(A) Na+ is smaller than Na atom
(B) Na+ is larger than Na atom
(C) CI- is smaller than CI atom
(D) CI- and CI are equal in size

22. Who introduced the zero groups?

(A) Lothar Meyer               (B) Lockery
(C) Mendleev                     (D) Ramsay

23. Element, of group I-B are called

(A) Representative elements
(B) Transition elements
(C) Rare earth
(D) Coinage metals

24. The element with Z = 24 is placed in the period

(A) 5                                    (B) 2
(C) 3                                    (D) 4

25. Which is the part of metalloids?

(A) NA and K                        (B) F and CI
(C) None of these                 (D) Cu and Au

26. Which one of the following has the maximum
      electron affinity?
(A) I                             (B) Br
(C) CI                           (D) F

27. On electrolysis of NaH, hydrogen is liberated

(A) At anode               (B) in the electrolyte
(C) At cathode            (D) none of them

28. Elements with greater number of electrons
have _________values of ionization energy.

a) Only one b) More than one
c) Zero d) Infinite




29.   Which of the following possess maximum
        hydration power?

a) Na+ b) K+
c) Mg+2 d) Ca+2

30.   Higher value of electron affinity means_________

Atom will lose electron easily
Atom will gain electron easily
Atom may form di-positive ion
The reason is unknown

31.   Melting points of VII-A group ___________ down the group

a.    Increase b     Decrease
c.    Remain constant d.    No regular trend

32.   Oxidation state of an atom represents______

No. of electrons gained
No. of electrons lost
No. of electrons gained or lost
                   d.   None of above correctly represent it

33. Mendeleev’s periodic table was based on

a) Atomic number    b) Atomic mass
c) Atomic volume     d) Electronic configuration

34. Elements present in a same group have the same

a) Atomic number
b) Molecular weight
c) Chemical properties
d) Electronic configuration

35. “s” and “p” block elements are also called

Transition elements
Inert elements
Typical elements
Rare earth elements

36. What is the symbol of the element with only three electrons and three protons?

a) Li b) C
c) Ag d) Cu

37. Elements with seven electrons in their valence shell are known as

a) Inert b) Lanthanides
c) Halogens d) Alkali metals






38. Which of the following pairs of elements are chemically most similar?

a) Na and Al b) Cu and Cu
c) S and F d) Sc and Zn

39. A student of chemistry will identify positively the following symbols as sodium
a) EMBED Equation.3   b) EMBED Equation.3  
c) EMBED Equation.3   d) EMBED Equation.3  

40. In the periodic table each period begins with a metal, which is

Most electronegative
Most electropositive
Less electropositive
Less electronegative

41. Which one of the following is not a coinage metal?

a) Au b) Cu
c) Ag d) Pd

42. Which is the most metallic element of 2nd period?

a) Lithium b) Beryllium
c) Boron d) Carbon

43. The outer most orbital involved in chemical bonding is called

a) Molecular orbital b) Complete orbital
c) Valence orbital d) Free orbital

44. Elements, which form basic oxides are

a) Electropositive b) Electronegative
c) Inert d) None of these

45. Which of the following has the most basic character?

a) Na2O b) MgO
c) Al2O3 d) P2O3

46. Which of the following is smallest in size?

a) K+1 b) O-2
c) F-1 d) Na+

47. Ionization energy is lowest for

a) Inert gases           b) Halogens
c) Alkali metals           d) Alkaline earth metals





48. An isotope of hydrogen is

a) Neptunium b) Plutonium
c) Thorium d) Tritium

49. With respect to chlorine, hydrogen will be

a) Electropositive b) Electronegative
c) Neutral d) None of these

50. Which of the following has the highest electron affinity?

a) 1S2 2S2 2P3 b) 1S2 2S2 2P6 3S1
c) 1S2 2S2 2P5 d) 1S2 2S2 2P5

51. Excluding hydrogen and helium, the smallest elements in the periodic table is

a) Lithium b) Fluorine
c) Cesium d) Iodine

52. Which halogen has the smallest electron affinity?

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

53. The element with atomic number 7 is likely to have same properties to the element whose atomic number is

a) 11 b) 2
c) 15 d) F

54. Which of the following will have largest size?

a) Br b) I -1
c) I d) F

55. In its chemical properties, calcium is most similar to

a) Cs b) Cu
c) Sc d) Sr

56. Which two of the following are iso electronic with one another?

a) Na+ and O b) Na+ and K+
c) Na+ and Ne d) Ne and O

57. Which of the following is a transuranic element?

a) Americium b) Plutonium
c) Neptunium d) All of these

58. The hydrogen, which is present in the atmosphere of sun and stars in a large amount, is
a) H2 b) H
c) H+ d) H-


59. Cesium and Francium are liquids above

a) 10oC b) 15oC
c) 20oC d) 30oC

60. In an aqueous solution the hydrides of alkali metals are

a) Stable b) Unstable
c) No change d) None of these

61. As the atomic number of the halogen increases, the halogens

Lose their outermost electrons less easily
Become less dense
Becomes lighter in color
Gain electrons less easily

62. The electron affinity of fluorine is

a) – 348.8 kj/mol b) – 337 kj/mol
c) 337 kj/mol d) 348.8 kj/mol

63. Which ionic halides have high m.p and b.p?

a) Fluoride b) Chloride
c) Bromide d) Iodide

64. Which gas is used in the making of tungsten bulb filaments?

a) H2 b) N2
c) O2 d) CO2

65. The ionic halides in order of decreasing m.p and b.p can be arranges as

Iodide>bromide>chloride> fluoride
Bromide>chloride>fluoride>iodide
Chloride>bromide>iodide>fluoride
Fluoride>chloride>bromide>iodide

66. A hydride ion and helium atom has same number of

a) Protons b) Neutrons
c) Electrons d) All of these

67. Ionic hydrides are also called

a) Saline hydrides b) Salt like hydrides
c) Both a & b d) None of these

68. The hydrides are acts as powerful reducing agents are

a) Ionic b) Covalent
c) Interstitial d) Complex





69. The hydrides which are non stoichiometric in nature are

a) Ionic b) Covalent
c) Interstitial d) Complex

70. Which one is the example of complex hydride?

a) PH3 b) NaH
c) LaH3 d) NaBH4

71. The adsorption of hydrogen by platinum is known as

a) Hydrogenation b) Dehydrogenation
c) Occlusion d) Substitution

72. From left to right in a periodic table charge to mass ratio increases therefore the hydration energy

a) Decreases b) Increases
c) Remains constant d) None of these

73. ______ elements have been discovered so
far.

a) 100 b) 110
c) 120 d) 150

74. _______ classified the then known elements
into metals, non metals and their derivatives.

a) Dobreiner b) Al – Razi
c) Newlands d) Mendeleeve

75. Dobreiner’s work led to the law of triads which states that ______

a) Atomic weight of any one element was
  found to be approximately the mean of the
  other two elements of triad.
b) Atomic weight of the middle element was
  found to be approximately the mean of the
  other two elements of a triad.
c) Atomic number of any one element was
  found to be approximately the mean of the
  other two elements of a triad.
d) Atomic number of the middle element was
  found t be approximately the mean of the
  other two elements of a triad.

76. The law of octaves was given by _______

a) Dobreiner b) Al – Razi
c) Newlands d) None of these









77. Law of octave states that ______

a) The properties of every 6th element from the
   given one were similar to the first.
b) The properties of every 9th element from the
   given one were similar to the first.
c) The properties of every 8th element from the
   given one were similar to the first.
d) The properties of every 7th element from the
   given one were similar to the second.

78. Mendeleev’s Periodic Table was based on _______

a) Atomic number    b) Atomic mass
c) Atomic volume     d) Electronic configuration

79. Moseley’s work led to the periodic law, which
states that _______

a) The number of the electrons in the 1st
   energy level increases as the atomic
   number increases.
b) The properties of the elements are a
   periodic function of their atomic mass.
c) The x – rays spectra of the elements are
   more complex than the optical spectra.
d) The properties of elements are the periodic
   function of their atomic number.

80. A pair of elements in the same family in the
periodic table classification is ________

a) Chlorine and carbon
b) Calcium and aluminum
c) Nitrogen and neon
d) Sodium and potassium

81. In the period, the elements are arranged in
strict sequence in order of _______

a) Increasing charges in the nucleus.
b) Increasing atomic weights.
c) Increasing number of electrons in valence
   shell.
d) Increasing valency.

82. Uranium is a member of

a) s – block b) p – block
c) d – block d) f – block

83. How many ionization energies can carbon
have?

a) 1 b) 2
c) 4 d) 6