Chapter 4.2, Problem 4.17P

Interpretation Introduction

Interpretation:

Geometry of all the atoms in the given compound has to be identified.

Concept Introduction:

Geometry of a compound is how the atoms that are present in the compound is connected in a 3D space.  In order to find the geometry of the compound, the first thing that must be known was how the atoms bond with each other.  Each and every atom in a compound is connected through bonds and the bonds are formed by overlapping orbitals.

Simple atomic orbitals are s and p orbitals.  Generally in organic chemistry we don’t consider or deal with d and f orbitals.  The second row elements ($\text{C,}\text{N,}\text{O}\text{and}\text{F}$) have a single s orbital and three p orbitals in their valence shell.  The s orbital mix with three p orbitals to form three types of hybridized orbital, and they are $s{p}^3,s{p}^2\text{and}sp$.  These hybridized orbital are involved in forming bonds with other atoms.

To find the hybridization state of atom we start by counting the number of bonds the atom has and the lone pair of electrons present.  The below table can be used to find the hybridization of atom,

Sum of bonded atoms and lone pairs	Number of hybridized orbitals
4	4 $s{p}^3$ orbitals
3	3 $s{p}^2$ orbitals and one p orbital
2	2 $sp$ orbitals and two p orbitals

From the hybridization state of the atoms we can identify the geometry of the same.  For finding the geometry, the lone pair of electrons also has to be considered.  This complete details are given in the following table,

Hybridization along with lone pair	Geometry
$s{p}^3$ with 0 lone pair of electrons	Tetrahedral
$s{p}^3$ with 1 lone pair of electrons	Trigonal pyramidal
$s{p}^3$ with 2 lone pair of electrons	Bent
$s{p}^2$ with 0 lone pair of electrons	Trigonal planar
$s{p}^2$ with 1 lone pair of electrons	Bent
$sp$ with 0 lone pair of electrons	Linear