Chapter 10.4, Problem 1RC

Interpretation Introduction

Interpretation:

The reason for non-existence of  ${\text{sp}}^4$ hybrid orbitals has to be explained.

Concept Introduction:

Hybridization:

Hybridization is defined as intermixing of atomic or molecular orbital.  The valance orbitals of an atom is allowed to combine with valence orbital of another orbital.  The resulting orbitals forms a bond and these orbitals are known as hybridized orbital.

Principal Quantum Number (n):  The energy of an electron becomes lower when the value of n is smaller.  The orbital size also depends on n.  The size of orbital increases with increase in value of principal quantum number (n).  It relates to distance between electron and nucleus in particular orbital.

Angular Momentum Quantum Number (l): It helps to differentiate different shapes of orbitals for given n.  For a given n, there are n different shapes of orbitals are present and are denoted as l.  The possible values of angular momentum quantum number is between $\text{0}\text{to}\text{(n-1)}$.  If the n is $3$, then l value is $0,1,2$

Magnetic Quantum Number (${\text{m}}_{\text{l}}$): It helps to distinguish orbitals having various orientation in space.  Any integer between $\text{-l,}\text{(-l+1),}\mathrm{..}\text{0,}\mathrm{..}\text{(+l-1)},\text{+l}$ is the probable values of magnetic quantum number.   For s subshell the $\text{l}\text{=}\text{0}$, then ${\text{m}}_{\text{l}}$ is zero.   For p subshell the $\text{l}\text{=}1$, then ${\text{m}}_{\text{l}}=-1,0,+1$.