Question

Classify the bonding in each of the following molecules as ionic, polar covalent, or nonpolar covalent.

a. ${\mathbf{H}}_{\mathbf{2}}$

b. ${\mathbf{K}}_{\mathbf{3}}\mathbf{P}$

c.$\mathbf{Nal}$

d.${\mathbf{SO}}_{\mathbf{2}}$

e.$\mathbf{HF}$

f.${\mathbf{CCl}}_{\mathbf{4}}$

g.${\mathbf{CF}}_{\mathbf{4}}$

h. ${\mathbf{K}}_{\mathbf{2}}\mathbf{S}$

Short answer

a) Non-polar covalent

b) Ionic

c) Ionic

d) Polar covalent

e) Polar covalent

f) Non- polar covalent

g) Non- polar covalent

h) Ionic

Step-by-step solution

Define ionic bond and id entify the ionic compounds:

Ionic bond is an electrovalent bond formed from electrostatic attraction between oppositely charged cations and anions. It is formed by transfer of electrons.

For ionic bond to form, one atom has to lose electrons while the other has to gain.

So the ionic compounds are ${\mathrm{K}}_3\mathrm{P}$, $\mathrm{Nal}$, and ${\mathrm{K}}_2\mathrm{S}$.

Define non- polar covalent bonds and identify the non- polar covalent molecules:

It is a type of bond formed when the electrons are equally shared between two atoms. These molecules are non-polar due negligible electro negativity difference or by cancellation of the dipole moment.

So the non- polar covalent molecules are ${\mathrm{H}}_2$, ${\mathrm{CCl}}_4$and ${\mathrm{CF}}_4$.

There is electronegativity difference between carbon and chlorine or carbon and fluorine. But the molecules being symmetric, the dipole moments cancel out to give zero net dipole moment.

Describe polar covalent bond and identify the polar covalent molecules:

A polar covalent bond is formed when atoms have different electro negativities and they share electrons in a covalent bond. Due to electro negativity differences, electrons are not equally shared.

So, the polar covalent molecule is $S{O}_2$and $\mathrm{HF}$.