Classification of Elements Test

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Classification of Elements Test - 2

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Weekly Quiz Competition

Question 1
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The first ionisation energy of Ar is less than that of Ne. An explanation of this fact is that

A
The effective nuclear charge experienced by a valence electron in Ar is much smaller than in Ne.

B
The effective nuclear charge experienced by a valence electron in Ar is much larger than in Ne.

C
The atomic radius of Ar is larger than that of Ne.

D
Both (A) and (C)

Solution

The 1^st IE of noble gases follows the order He > Ne > Ar > Kr. Ionisation energy increases down the group as size increases.
Also higher the number of electron shells, greater will be the shielding effect experienced by the outermost electrons.
Higher the shielding effect, lower will be the effective nuclear charge experienced by the valence electron in outermost shell. Thus, it is easier to remove electron from Ar than from Ne.
Question 2
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Which of the following sets of elements have almost same atomic radii.

A
Fe, Co, Ni, Cu

B
He, Ne, Ar, Xe

C
Be, Mg, Ca, Sr

D
Cl, Br, I

Solution

The atomic radii of one series of transition metals do not vary greatly because inner 3d atomic orbitals are being filled, although there is a general decrease across a series of transition elements
Question 3
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Which of the following has the least ionic radius?

A
N^3–

B
Mg²⁺

C
Na⁺

D
Al³⁺

Solution

Higher the charge on the cation, smaller will be its ionic radius. Among the given options, Al³⁺ has the smallest size due to its highest charge.
Question 4
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The increasing order of the first ionization enthalpies of the elements B, P, S and F (lowest first) is

A
B < P < S < F

B
B < S < P < F

C
F < S < P < B

D
P < S < B < F

Solution

IP increases from left to right in the period and decreases down the group in the periodic table. Also phosphorus has higher ionisation enthalpy than sulphur because phosphorus has stable half-filled electronic configuration. Thus, the correct order of ionisation enthalpy is B < S < P < F.
Question 5
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The ionic radii (in Å) of N^3-, O^2- and F^- are respectively :

A
1.36, 1.40 and 1.71

B
1.36, 1.71 and 1.40

C
1.71, 1.40 and 1.36

D
1.71, 1.36 and 1.40

Solution

These are isoelectronic species.
As negative charge increases, ionic radius increases.
Hence, option C is correct
Question 6
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According to the peridoic law of elements the variatiion in properties of elements is related to their

A
Atomic masses

B
nucelear masses

C
atomic numbers

D
nuclear neutron-proton number ratios

Solution

All physical and chemical properties of elements are perioidic function of atomic number. Modern periodic law.
Hence, option C is correct.
Question 7
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The increasing order of the ionic radii of the given isoelectronic species is :

A
Cl^–, Ca²⁺, K⁺, S^2–

B
S^2–, Cl^–, Ca²⁺, K⁺

C
Ca²⁺, K⁺, Cl^–, S²–

D
K⁺, S^2–, Ca²⁺, Cl^–

Solution

For isoelectronic species, as the z/e decreases, ionic radius increases. Higher the positive charge smaller will be the ionic radius. Higher the negative charge, larger will be the ionic radius. Hence, the correct increasing order is Ca²⁺< K⁺ < Cl^–< S^2–.
Hence, option C is correct.
Question 8
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Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar?

A
S < Se < Ca < Ba < Ar

B
Ba < Ca < Se < S < Ar

C
Ca < Ba < S < Se < Ar

D
Ca < S < Ba < Se < Ar

Solution

Increasing order of first ionization enthalpy is
Ba < Ca < Se < S < Ar
Hence, option B is correct.

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Classification of Elements Test - 2

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Classification of Elements Test - 2

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Question 1

The effective nuclear charge experienced by a valence electron in Ar is much smaller than in Ne.

The effective nuclear charge experienced by a valence electron in Ar is much larger than in Ne.

The atomic radius of Ar is larger than that of Ne.

Both (A) and (C)

Solution

Question 2

Fe, Co, Ni, Cu

He, Ne, Ar, Xe

Be, Mg, Ca, Sr

Cl, Br, I

Solution

Question 3

N3–

Mg2+

Na+

Al3+

Solution

Question 4

B < P < S < F

B < S < P < F

F < S < P < B

P < S < B < F

Solution

Question 5

1.36, 1.40 and 1.71

1.36, 1.71 and 1.40

1.71, 1.40 and 1.36

1.71, 1.36 and 1.40

Solution

Question 6

Atomic masses

nucelear masses

atomic numbers

nuclear neutron-proton number ratios

Solution

Question 7

Cl–, Ca2+, K+, S2–

S2–, Cl–, Ca2+, K+

Ca2+, K+, Cl–, S2–

K+, S2–, Ca2+, Cl–

Solution

Question 8

S < Se < Ca < Ba < Ar

Ba < Ca < Se < S < Ar

Ca < Ba < S < Se < Ar

Ca < S < Ba < Se < Ar

Solution

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N^3–

Mg²⁺

Na⁺

Al³⁺

Cl^–, Ca²⁺, K⁺, S^2–

S^2–, Cl^–, Ca²⁺, K⁺

Ca²⁺, K⁺, Cl^–, S²–

K⁺, S^2–, Ca²⁺, Cl^–