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Chapter 3: Problem 27

What do you mean by regular and irregular geometry? Use VSEPR theory to illustrate your answer.

Short Answer

Expert verified
Regular geometry refers to structures with molecule shapes where all bonds and bond angles are equal, like linear or tetrahedral, while irregular geometry refers to structures where lone pairs of electrons on the central atom distort the shape resulting in unequal bond lengths or angles, like bent or pyramidal geometries.

Step by step solution

01

Explanation of VSEPR theory

VSEPR (Valence Shell Electron Pair Repulsion) theory states that the arrangement of electron pairs around a central atom is dictated primarily by minimizing electrostatic repulsion. It is based on the principle that groups of electrons surrounding an atom will arrange themselves in space to maximize the distance between them, resulting in specific molecular structures or geometries.
02

Definition and illustration of Regular Geometry

Regular geometry refers to the structures in which all the bond angles are equal and all the bonds are of equal length. Examples include linear (for example, \(CO_2\)), trigonal planar (\(BF_3\)), tetrahedral (\(CH_4\)), trigonal bipyramidal (\(PF_5\)), and octahedral (\(SF_6\)) geometries. In these structures, the electron pairs are evenly distributed around the nucleus, resulting in a symmetrical shape.
03

Definition and illustration of Irregular Geometry

Irregular geometry arises due to the presence of lone pair(s) of electrons on the central atom which occupy more space than bonding electrons and hence repel the bonding electron pairs more strongly. This results in a geometry where the bond angles are not all equal and/or the bonds are not of equal length. Examples are bent or V-shaped (\(H_2O\)), pyramidal (\(NH_3\)), see-saw (\(SF_4\)), T-shaped (\(ClF_3\)), and square pyramidal (\(BrF_5\)) geometries. The presence of lone pairs distorts the geometry from the regular arrangement.

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Most popular questions from this chapter

Compare the bond angles in the following molecules: (a) \(\mathrm{CH}_{4}\) (b) \(\mathrm{NH}_{3}\) (c) \(\mathrm{H}_{2} \mathrm{O}\)

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Use MO diagram to compare bond length and bond order of following species: \(\mathrm{O}_{2}^{+}, \mathrm{O}_{2}, \mathrm{O}_{2}^{-}, \mathrm{O}_{2}^{2-}\).

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Differentiate between covalent and coordinate bond.
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