Question

A metal forms ionic compounds with the following non-metals.

(A) Bromine

(B) Oxygen

(C) Iodine

(D) Fluorine

(E) Sulphur

Arrange these non-metals in the decreasing order of the strength of the ionic bonds.

• A. DBEAC
• B. CAEBD
• C. BDEAC
• D. CBEAD

Answer 1

The correct option is A

DBEAC

Explanation of correct option:

• The strength of an ionic metal-non-metal bond depends upon the tendency of the non-metal to accept electrons from metal.
• This tendency can be estimated from the value of electron affinity which is defined as the amount of energy released when an electron is added to the valence shell of an isolated gaseous atom in its ground state.
• Electron affinity increases along the period and decreases down the group.
• Keeping all this in mind we get the order of electron affinity of the non-metals given in the question as Fluorine ($\mathrm{F}$) $>$Oxygen ($\mathrm{O}$)$>$Sulphur ($\mathrm{S}$)$>$Bromine ($\mathrm{Br}$)$>$Iodine ($\mathrm{I}$).

So, the correct order is DBEAC.

Hence, the correct option is (A).