Question 53

The maximum number of lone pairs of electron on the central atom from the following species is _______ ClO$$_3^-$$, XeF$$_4$$, SF$$_4$$ and I$$_3^-$$

Correct Answer: 3

Solution

1. $$ClO^{3-}$$

Central Atom: Chlorine (Cl), which has 7 valence electrons.

Calculation: It gains 1 electron from the negative charge (7 + 1 = 8). Each of the 3 oxygen atoms forms a double bond, sharing 2 electrons (3 * 2 = 6).

Remaining electrons: 8 - 6 = 2 electrons.

Lone Pairs: 1

$$\text{}$$

2.$$XeF_4$$

Central Atom: Xenon (Xe), a noble gas with 8 valence electrons.

Calculation: It forms 4 single bonds with 4 fluorine atoms, using 4 electrons.

Remaining electrons: 8 - 4 = 4 electrons.

Lone Pairs: 2

3.$$SF_4$$

Central Atom: Sulfur (S), which has 6 valence electrons.

Calculation: It forms 4 single bonds with 4 fluorine atoms, using 4 electrons.

Remaining electrons: 6 - 4 = 2 electrons.

Lone Pairs: 1

4. $$I_{3}^{-}$$

Central Atom: The central Iodine (I) atom has 7 valence electrons.

Calculation: It gains 1electron from the negative charge (7 + 1 = 8). It forms single bonds with the 2 surrounding iodine atoms, using 2 electrons.

Remaining electrons: 8 - 2 = 6 electrons.

Lone Pairs: 3

hence Highest no. of loan pairs is 3

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