Question 71

According to Lewis theory, the total number of $$\sigma$$ bond-pairs and lone pair of electrons around the central atom of $$\text{XeO}_6^{4-}$$ ion is _____.

Correct Answer: 6

Solution

The central atom is xenon. Xenon belongs to group 18, so it possesses $$8$$ valence electrons.

Xenon forms bonds with 6 oxygen atoms, which means there are exactly 6 $$\sigma$$ bonds.

To satisfy the stable structure of the ion, 4 oxygens carry a negative charge and form single bonds ($$\text{Xe}-\text{O}^-$$), while the remaining 2 oxygens form double bonds ($$\text{Xe}=\text{O}$$).

Electrons used for 6 $$\sigma$$ bonds = 6 electrons

Electrons used for 2 $$\pi$$ bonds = 2 electrons

Total valence electrons utilized by Xe = $$6 + 2 = 8$$ electrons

Therefore, the total of “σ bond-pairs + lone pair of electrons’’ around the central xenon atom is $$6 + o = 6$$.

Answer: 6

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