Question

Consider the following statements.

$S_1$: Fluorine does not form any polyhalide as it has low F - F bond energy
$S_2$: The chlorine has the most negative electron gain enthalpy.
$S_3$: The first ionization potential of N and 0 atoms are 14.6 and 13.6 eV respectively.

Which of the above statements are correct?

• A. $S_1,S_2$ and $S_3$
• B. $S_1$ and $S_2$
• C. $S_1$ and $S_3$
• D. $S_2$ and $S_3$

Answer 1

The correct option is A $S_1,S_2$ and $S_3$

$S_1:$ Fluorine does not form any polyhalide as other halogens because:- (1) It has maximum ionic character (2) It has low F-F bond energy (38.5 k cal mol–1) (3) Of the absence of d-orbitals in the valence shell of fluorine (4) It brings about maximum coordination number in other elements.

$S_2:$ The negative electron gain enthalpy of fluorine is less than that of chlorine. It is due to small size of fluorine atom. As a result, there are strong interelectronic repulsions in the relatively small 2p orbitals of fluorine and thus, the incoming electron does not experience much attraction.

$S_3:$ Consider the electronic configurations of Nitrogen and Oxygen.

N - $1s^{2}2s^{2}2p^3$

O - $1s^{2}2s^{2}2p^4$

We notice that if oxygen loses one electron, it will attain half-filled configuration. Hence it can lose an electron easily. Also, nitrogen is already in a half-filled configuration, and hence losing an electron will require more energy than that of oxygen.

Therefore The first ionization potential of N and 0 atoms are 14.6 and 13.6 eV respectively.

Hence , All are correct .

Therefore , option A is correct .