Match Column-I with Column-II and Column-III: Column-I...

Match Column-I with Column-II and Column-III: Column-I Column-II Column-III (a) $\mathrm{XeF}_{2}$ (p) $90^{\circ}$ (i) Tetrahedral (b) $\mathrm{XeF}_{4}$ (q) $109.5^{\circ}$ (ii) Pyramidal (c) $\mathrm{XeO}_{4}$ (r) $103^{\circ}$ (iii) Linear (d) $\mathrm{XeO}_{3}$ (s) $180^{\circ}$ (iv) Square planar

Match Column-I with Column-II and Column-III:
Column-I Column-II Column-III
(a) $\mathrm{XeF}_{2}$
(p) $90^{\circ}$
(i) Tetrahedral
(b) $\mathrm{XeF}_{4}$
(q) $109.5^{\circ}$
(ii) Pyramidal
(c) $\mathrm{XeO}_{4}$
(r) $103^{\circ}$
(iii) Linear
(d) $\mathrm{XeO}_{3}$
(s) $180^{\circ}$
(iv) Square planar

Key Concepts

VSEPR Theory

VSEPR (Valence Shell Electron Pair Repulsion) theory is a fundamental concept that predicts the shape of molecules based on the repulsions between electron pairs surrounding a central atom. It explains how electron pairs—both bonding and non-bonding—arrange themselves to minimize repulsion, thereby dictating the overall molecular geometry.

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms in a molecule. It considers the positions of both bonding pairs and lone pairs of electrons. This concept is essential for understanding shapes such as linear, tetrahedral, square planar, and pyramidal in various molecular structures.

Bond Angles

Bond angles are the angles between adjacent bonds around a central atom in a molecule. They are determined by the idealized geometry predicted by VSEPR theory, with common angles such as 180°, 109.5°, 90°, and others. These angles help in identifying specific molecular geometries and understanding deviations caused by lone pairs.

Hypervalency

Hypervalency refers to the ability of atoms, particularly those in the third period and beyond like xenon, to expand their octet and accommodate more than eight electrons. This concept is relevant for predicting the structure and bonding in compounds with central atoms that form more bonds than the traditional octet rule would allow.

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