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Question #44323

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The Question

Consider Oxide $\mathbf{X}$ , a gaseous non-metal oxide that exists as a monomeric, planar molecule with zero dipole moment at $298\text{ K}$ . Upon complete hydration, it forms a strong dibasic oxoacid $\mathbf{X'}$ . Consider Oxide $\mathbf{Y}$ , a volatile solid that auto-ionizes into two distinct molecular ions. In the vapor phase, it exists as a covalent molecule. Hydration of $\mathbf{Y}$ yields a strong monobasic oxoacid $\mathbf{Y'}$ . Which of the following statements regarding the structural and electronic properties of these species is \textbf{INCORRECT}?

Options

A.
In the solid state of $\mathbf{Y}$ , the cationic and anionic central atoms are $sp$ and $sp^2$ hybridized respectively, and both possess a formal charge of $+1$ .
B.
The hydration of $\mathbf{X}$ to $\mathbf{X'}$ involves a change in the hybridization of the central atom from $sp^2$ to $sp^3$ , while its formal charge remains zero in the most stable Lewis structure.
C.
The higher acidity of $\mathbf{X'}$ compared to $\ce{H2SO3}$ is primarily due to the central sulfur in $\ce{H2SO3}$ retaining the $sp^2$ hybridization of its parent oxide $\ce{SO2}$ , which restricts the resonance stabilization of the conjugate base.
D.
The vapor phase of $\mathbf{Y}$ contains an $sp^3$ hybridized bridging oxygen atom, and its hydration to $\mathbf{Y'}$ involves no change in the $sp^2$ hybridization of the central nitrogen atoms.

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How the Examiner Thinks

Mechanism_Trap

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Concepts Behind This Question

Acid-Base Nature of Oxides|Hybridization and Geometry|Formal Charge Calculation

Why This Question Is Tricky

Common Mistakes

The question tests the 'Hidden Variable' of stereochemically active lone pairs during hydration and the 'Chemical Exception' regarding the formal charge of central atoms in polyatomic anions.

Students often memorize that $\ce{SO2}$ is $sp^2$ and incorrectly assume its hydrated form, $\ce{H2SO3}$ , remains $sp^2$ because it has one less oxygen than the $sp^3$ hybridized $\ce{H2SO4}$ .

They fail to account for the lone pair on the sulfur atom in $\ce{H2SO3}$ , which makes its electron geometry tetrahedral ( $sp^3$ ).

Furthermore, it tests the counter-intuitive fact that the central nitrogen in the nitrate anion ( $\ce{[NO3]-}$ ) carries a $+1$ formal charge, trapping students who assume the central atom of an anion must be negatively charged.

Quick Facts About This Question

Question Information

Subject	Chemistry
Chapter	Classification of Elements and Periodicity in Properties - Class 11 Part 1
Concept	Acid-Base Nature of Oxides
Difficulty	8
Cognitive Load	7
Target Solve Time	160 sec
Access	Free