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Chemistry Periodic Classification Of Elements & Periodicity Online Test

Malik TahirLast Updated: October 14, 2025

Important Periodic Classification Of Elements & Periodicity Question and Answer

Total Questions:	107
Time Allowed:	60 Minutes
Total Marks:	107
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Chemistry Periodic Classification Of Elements & Periodicity Practice Test Online With Explanation

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Page 1 of 5

Chemistry

1. Elements whose outer electronic configuration vary from ns²np¹ to ns¹np⁶ constitute

d – block elements

f – block elements

s – block elements

p – block elements

2. Higher value of electron affinity means

Atom will gain electron easily

Atom may form di-positive ion

Atom will lose electron easily

The reason is unknown

3. Best position of hydrogen in the periodic table is mainly due to

Both are electropositive

All

Similar electronic configuration

Both are not found in free state

4. Which one of the following is not a periodic property?

Coordination number of icons

BP of elements

Ionization energy of elements

MP of elements

5. Which one is the strongest reducing agent?

6. Which of the pairs belongs to the same group of periodic table?

Elements with atomic number 17 and 38

Elements with atomic number 17 and 53

Elements with atomic number 11 and 33

Elements with atomic numbers 20 and 40

7. The highly electronegativity atom is

8. Elements in the same vertical group of the periodic table have same

Atomic mass

Number of valence electrons

Atomic volume

Atomic number

9. The longest period in the modern periodic table is

5th

7th

2nd and 3rd both

6th

10. Which statement is correct?

Hydrogen resembles in properties with IIA, IIIA and VIIIA elements

Hydrogen resembles in properties with IIIA, IVA and VA elements

Hydrogen resembles in properties with IIA, IVA and VIA elements

Hydrogen resembles in properties with IA, IVA and VIIA elements

11. Which of these Period 3 element has lowest electronegativity?

12. Number of elements present in the fifth period of periodic table is

13. Oxidation state of an atomic represent

No of e lost

No of e gained or/lost

No of e gained

None

14. The element with atomic number 14 belongs to

3rd period

2nd period

4th period

5th period

15. Mark the correct statement

The ionization energy of calcium is lower than that of strontium

The ionization energy of calcium is lower than that of barium

The ionization energy of calcium is higher than that of magnesium

The ionization energy of calcium is than that of beryllium

16. The property which increases up to the middle of the period and then decreases is

Ionization energy

Atomic radii

m.P and B.P

Atomic volume

17. Modern periodic table has been divided in __________ block.

18. Alkali metals in each period have

Highest electronegativity

Highest IE

Lowest IE

Smallest size

19. Mark the elements that belong to same period:

H, He, F

Ca, Cr, Zn

Li, Na, K

Cr, In, Pb

20. Chemically the most similar pair of elements is

Na, Al

Zr, Hf

Cu, S

Ti, Zr

21. In modern periodic table all the elements are arranged in ascending order of

Valence electrons

Atomic number

Atomic mass

Valency

22. The atoms of same element having same atomic number bit different mass number are called

Isomers

Isotopes

Isobars

Isotropes

23. Metals form halides which are

All

Ionic

Covalent

Polymeric

24. Which of the following statements is most appropriate about effective nuclear charge? It depends upon?

The atomic number

The charge on the nucleus

The shielding constant

Both the nuclear charge and the shielding constant

25. The elements which behave as metalloid is:

Rb & Cs

Pt & I

AI & Zn

Br & I

Page 2 of 5

26. Which of the following set consist of all coinage metals?

Cu, Fe, Au

Cu, Hg, Au

Ag, Au, Hg

Cu, Ag, Au

27. Which of the following has highest electropositive character?

28. Which one has least ionization Potential?

29. The atomic radii decreases by increasing atomic number in

Alkaline earth metal

Alkali metal

Halogens

Elements from Li to Ne

30. Which set of elements is listed in order of increasing ionization energy?

As < Cl < P < S < Sb

Sb < As < Cl < S < P

Sb < As < S < P < Cl

Cl < Sb < P < As < S

31. Elements were classified into groups of three called as trades by

New lands

Rutherford

Lother Meyer

Dobereiner

32. Elements with similar chemical properties appear in 1 the

Same period

Right upper corner

Same family

p block elements

33. Which element was not known when Mendeleev proposed his classification?

Germanium

Hydrogen

Copper

34. Seventh period contains ____________ normal elements

35. An element having low value of ionization energy and low value of electron affinity is likely to belong to

Group IA

Group VIII

Group IB

Group VII A

36. Which one is more acidic?

As₂O₃

Wa₂O₂

Al₂O₃

Cl₂O₇

37. The element with atomic number 26 will be found in group

38. Which of the following groups of period table has entirely metals?

VII

39. Among the following elements which one has the highest value of first ionization potential?

Barium

Oxygen

Argon

Cesium

40. Elements whose atoms have two outermost shells incomplete are called

d – block elements

f – block elements

s – block elements

p – block elements

41. Which of the following groups may contain a metalloid?

IIIA

VIA

IIA

42. The element with atomic number 55 belongs to which block of the periodic table

p-block

s-block

d-block

f-block

43. Which element was not known when Mendeleev proposed his classification?

Copper

Germanium

Hydrogen

Sodium

44. Which of the following pair of atomic numbers represents s-block element?

6, 12

3, 20

7, 15

9, 17

45. The electronegativity of Si is

1.2

2.1

1.8

1.5

46. The electron affinity values (in kJ mol¯¹) of three halogens X, Y and Z are respectively – 349, -333 and -325. Then X, Y and Z respectively are:

Cl, F and Br

F, Cl and Br

Br, Cl and F

Cl, Br and F

47. Best position of hydrogen in the periodic table is above I.A Group which is mainly due to

All

Both form ionic compounds

Both are electropositive

Similar outer most shell electronic configuration

48. The formation of the oxide ion O²¯ (g) requires first a exothermic and then and endothermic step – as shown below:
O(g) +e – → O
∆Ho = – 142 k3 mol – 1
O– (g) + e– →O2 –(g)
∆Ho = + ∆H° = + 844 kJ mol¯¹
This is because:

Oxygen is more electronegative

Oxygen has high electron affinity

O– ion has comparatively larger size oxygen atom

O– ion will tend to resist the addition of another electron

49. Non-metals usually form ________ oxides.

Acidic

All of the above

Amphoteric

Neutral

50. The attempt of classification of elements by plotting the atomic weight of elements against their volumes was made

Dobereiner

Newlands

Lother Meyer

Bohr

Page 3 of 5

51. The 14 elements have been placed in VI period and II group of periodic table. These are called

Rare earth metals

Alkaline earth metals

Inert gases

Alkali metals

52. The number of elements in fourth period of periodic table is

53. The atomic radii decrease by increasing atomic number in

Alkaline earth metal

Elements from Li to Ne

Alkali metal

Halogens

54. Variable valency is generally exhibited by

Normal elements

None of these

Transition elements

Metallic elements

55. Many of the properties of elements and its compounds can be predicted from the position of element in the periodic table. Which property cannot be predicted?

Charge on its ions

The number of isotopes it has

Acidic or basic nature of oxides

The formula of its oxides

56. The valency of noble gases, in general, is

Zero

Two

One

Three

57. Which of the pair of metalloids?

As and Sb

F and U

Na and K

Cu and Au

58. An element has electronic configuration 1s2 2s2 2p2. It belongs to

Group IV-A

Group VI-A

Group VII-A

Group II-A

59. Noble gases are named so because they are

All

Zero group element

Inert

Having completely filled valence shell

60. The alkali metal which is liquid at 15°C is

None

61. Among the elements given below, the one with highest electro positivity is

62. The valence shell electronic stricture of an element is ns²np⁵. The element will belong to the group of

Alkali metals

Noble gases

Inert metals

Halogens

63. Of the given alkali metals, the one with smallest size is

64. The periodic table consists of

8 horizontal and 7 vertical series

7 horizontal and 18 vertical series

7 horizontal and 7 vertical series

8 horizontal and 18 vertical series

65. Which discovery caused a revision in periodic law as predicted by Mendeleev?

x-rays by Roentgen

Location of nucleus by Rutherford

Henry Becquerel’s natural radioactivity

Atomic number by Moseley

66. Which of the following pairs are chemically dissimilar?

Zr and Hf

Ca and Zn

Na and K

Ba and Sr

67. The correct arrangement of increasing order of atomic radius among Na, K, Mg, Rb is

Mg < Na < Rb < K

Mg < K < Na < Rb

Na < K < Rb < Mg

Mg < Na < K < Rb

68. The defects in the Mendeleev’s Periodic table is/are

K (at, wt.39.1) has been placed after argon (at, wt. 39.9)

All above statements are correct

In spite of their different properties, alkali metals and coinage metals have been grouped together

Similar elements like Cu and Zn have been placed in different groups

69. Which among the following elements have lowest value of IE₁?

70. Oxidation state of an atom represent

Number of electrons lost

Number of electrons gained

Apparent charge I compound

Its vacancies

71. Which of the following represents element s in order of increasing atomic size?

C, N, O

Na, Mg, C

I, Br, CI

Li, Na, K

72. Californium is the member of

Actinide series

Alkali metals

Lanthanide series

Alkaline earth metals

73. Which of the following does not reflect the periodicity of elements?

Electronegativity

Bonding behavior

Neutron/proton ration

Ionization potential

74. Keeping in view the size of atoms, which order in correct one

Cl > I

B > Ga

Ba > Mg

Lu > Ce

75. Mark the correct statement

Na⁺ is larger than Na atom

Cl⁺ is smaller than Cl atom

Na⁺ is smaller than Na atom

Cl⁺ (ions are equal in size)

Page 4 of 5

76. The element with highest first ionization energy is

77. Which order of ionization energy is correct?

Mg > A1

Mg < A1

Si > P

Both b & c

78. Periodic table provides a basic framework to study elements with respect to their

All

Chemical properties

Physical properties

Properties of their compounds

79. White enamel of our teeth is

CaBr₂

CaU₂

Ca₃ (PO4)₂

CaF₂

80. Metallic characters of alkali metals

Remain same

Increase down the group

Decrease down the group

No regular trend

81. Which of the following ion is stable in aqueous solution?

Cl-

H+

All are stable

H-

82. Magnesium keeps on burning in

Co₂

N₂O

N₂

N₂ as well as Co₂

83. Which of the following metal requires radiation of highest frequency to cause emission of electrons?

84. Which of the p-block elements are not representative elements?

Alkali metals (I-A)

Group-14 elements (IV-A)

Group-18 elements (VIII-A)

Halogens (VII-A)

85. Mark the correct statement

Melting points of halogens decrease down the group

Melting points of halogens increases down the group

Melting point of halogens first increase and then decrease down the group

Melting points of halogens remains the same throughout the group

86. Which of the following elements is/are not liquid at 30°C?

87. Addition of 2nd e to uni-negative ion is always

Exothermic

Data is insufficient

A or b

Endothermic

88. Inner transition elements are called

Lanthanides

Rare earth metals

All

Actinides

89. Among O, C, F, Cl, Br, the correct order of increasing radii is

F Cl Br O C

F C O Cl Br

F O C Cl Br

C O F Cl Br

90. An element has electronic configuration IS2, 2S2, 2P2 with which group does this element belong to

Group IIA

Zero

IVA

VIIA

91. IN the light of Mendeleev’s periodic law,. the properties of elements are periodic function of their

Density

Atomic numbers

Volume

Atomic masses

92. The property which increases up to group IV-A then decreases onwards

Ionization energy

Atomic radii

Atomic volume

Melting & boiling points

93. The discovery of which of the following group of elements give below to the Newland’s law of octaves?

Inert gases

Alkaline earths

Actinides

Rare earths

94. Which of the following possess maximum hydration power?

K⁺

Na⁺

Ca⁺²

Mg⁺²

95. Which of these Period 3 elements have highest electronegativity?

96. Which of the following has greatest tendency lose electron?

97. Which of the following elements is most electronegative?

Oxygen

Nitrogen

Chlorine

Fluorine

98. Shielding effect across the period

Increases

Decreases

Cannot be predicted

Remains constant

99. Mark the correct statement

All halogens are present in the same period

All lanthanides are present in the same group

All the noble gases are present in the same period

All the alkali metals are present in the same period

100. Inner transition elements are called

Actinides

Rare earth metals

All

Lanthanides

Page 5 of 5

101. The electronegativity of Sodium is

1.5

1.2

0.9

1.8

102. Hydrogen resembles with carbon because of having

Remarkable reducing properties

Similar physical state

Homovalent (show same valency)

Same number of electrons in the valence shell

103. Modern periodic table has been divided in _________ blocks.

104. The attraction that an atom exerts on a pair of electrons that are being shared with another atom for forming covalent bond is referred to as its

Electron affinity

Electronegativity

Ionization energy

Valency

105. Which one is not an ionic hydride?

LiH

NaH

CsH

106. Mark the Dobereiner triad

B, C, Si

Ne, Ar, K

Cl, Br, I

Zn, Cr, Na

107. Which has largest first ionization energy?

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Malik TahirLast Updated: October 14, 2025

Chemistry Periodic Classification Of Elements & Periodicity Online Test

Important Periodic Classification Of Elements & Periodicity Question and Answer

Chemistry Periodic Classification Of Elements & Periodicity Practice Test Online With Explanation

Chemistry

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