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Introduction to Noble Gases

The electroni...

Question

The electronic configuration of few elements is given below. Mark the statement which is not correct about these elements.
(i) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$
(ii) $1 s^{2} 2 s^{2} 2 p^{5}$
(iii) $1 s^{2} 2 s^{2} 2 p^{6}$
(iv) $1 s^{2} 2 s^{2} 2 p^{3}$

(i) is an alkali metal.

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(iii) is a noble metal.

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(i) and (ii) form ionic compounds.

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(iv) has high ionisation enthalpy.

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Solution

The correct option is B (iii) is a noble metal.
(i) is an alkali metal. It readily loses an electron to attain a noble gas configuration.
(iii) is a noble gas. It has completed its octet.
Highly electropositive (i) and highly electronegative (ii) form ionic compounds.
(iv) has high ionization enthalpy as removal of an electron will break half-filled 2p subshell.

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Similar questions

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}

1 s^{2} 2 s^{2} 2 p^{3}

1 s^{2} 2 s^{2} 2 p^{5}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

1 s^{2}

1 s^{2} 2 s^{2} 2 p^{2}

1 s^{2} 2 s^{2} 2 p^{5}

1 s^{2} 2 s^{2} 2 p^{6}

Arrange the elements with the following electronic configurations in the increasing order of electron affinity

(i) $1 s^{2} 2 s^{2} 2 p^{3}$ (ii) $1 s^{2} 2 s^{2} 2 p^{4}$ (iii) $1 s^{2} 2 s^{2} 2 p^{5}$ (iv) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}$

A, B, C

D

1 s^{2} 2 s^{2} 2 p^{6}

1 s^{2} 2 s^{2} 2 p^{4}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

1 s^{2} 2 s^{2} 2 p^{5}

(i) [X e] {6 s}^{1}

(i i) [X e] {4 f}^{14}, {5 d}^{1} {6 s}^{2}

(i i i) [A r] {4 s}^{2} {4 p}^{3}

(i v) [A r] {3 d}^{7}, {4 s}^{2}

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