Chapter 12, Problem 32E

(a)

To determine

The shape of the molecule ${\text{N}}_{\text{2}}\text{O}$ and its polar or nonpolar nature.

Answer to Problem 32E

The shape of the molecule ${\text{N}}_{\text{2}}\text{O}$ is linear as shown:

The molecule ${\text{N}}_{\text{2}}\text{O}$ is polar.

Explanation of Solution

Given Info: Refer to Table 12.6 in the textbook to predict the shape of the molecule.

Explanation:

The shape of the molecule ${\text{N}}_{\text{2}}\text{O}$ is linear as shown:

The central atom has two surrounding regions.

The polarity of a molecule depends on the electronegativity of atoms in that molecule and the shape of the molecule. A molecule which has one polar bond is polar.

A molecule which has all nonpolar bonds is nonpolar.

The symmetric molecule will be nonpolar because the polarity of bonds is canceled out. Thus an asymmetric molecule is polar because the polarity of bonds is not canceled.

Therefore, the asymmetric molecule ${\text{N}}_{\text{2}}\text{O}$ is polar.

Conclusion:

Therefore, the shape of the molecule ${\text{N}}_{\text{2}}\text{O}$ is linear as shown:

The molecule ${\text{N}}_{\text{2}}\text{O}$ is polar.

(b)

To determine

The shape of the molecule ${\text{SO}}_4{}^{2-}$ and its polar or nonpolar nature.

Answer to Problem 32E

The shape of the molecule ${\text{SO}}_4{}^{2-}$ is tetrahedral as shown:

The molecule ${\text{SO}}_4{}^{2-}$ is nonpolar.

Explanation of Solution

Given Info: Refer to Table 12.6 in the textbook to predict the shape of the molecule.

Explanation:

The shape of the molecule ${\text{SO}}_4{}^{2-}$ is tetrahedral as shown:

The central atom has four surrounding regions.

The polarity of a molecule depends on the electronegativity of atoms in that molecule and the shape of the molecule. A molecule which has one polar bond is polar.

A molecule which has all nonpolar bonds is nonpolar.

The symmetric molecule will be nonpolar because the polarity of bonds is canceled out. Thus an asymmetric molecule is polar because the polarity of bonds is not canceled.

Therefore, the symmetric molecule ${\text{SO}}_4{}^{2-}$ is nonpolar.

Conclusion:

Therefore, the shape of the molecule ${\text{SO}}_4{}^{2-}$ is tetrahedral as shown:

The molecule ${\text{SO}}_4{}^{2-}$ is nonpolar.

(c)

To determine

The shape of the molecule ${\text{GaH}}_{\text{3}}$ and its polar or nonpolar nature.

Answer to Problem 32E

The shape of the molecule ${\text{GaH}}_{\text{3}}$ is trigonal planar as shown:

The molecule ${\text{GaH}}_{\text{3}}$ is nonpolar.

Explanation of Solution

Given Info: Refer to Table 12.6 in the textbook to predict the shape of the molecule.

Explanation:

The shape of the molecule ${\text{GaH}}_{\text{3}}$ is trigonal planar as shown:

The central atom has three surrounding regions.

The polarity of a molecule depends on the electronegativity of atoms in that molecule and the shape of the molecule. A molecule which has one polar bond is polar.

A molecule which has all nonpolar bonds is nonpolar.

The symmetric molecule will be nonpolar because the polarity of bonds is canceled out. Thus an asymmetric molecule is polar because the polarity of bonds is not canceled.

Therefore, the symmetric molecule ${\text{GaH}}_{\text{3}}$ is nonpolar.

Conclusion:

The shape of the molecule ${\text{GaH}}_{\text{3}}$ is tetrahedral as shown:

The molecule ${\text{GaH}}_{\text{3}}$ is nonpolar.

(d)

To determine

The shape of the molecule ${\text{NH}}_{\text{2}}\text{Cl}$ and its polar or nonpolar nature.

Answer to Problem 32E

The shape of the molecule ${\text{NH}}_{\text{2}}\text{Cl}$ is trigonal pyramidal as shown:

The molecule ${\text{NH}}_{\text{2}}\text{Cl}$ is polar.

Explanation of Solution

Given Info: Refer to Table 12.6 in the textbook to predict the shape of the molecule.

Explanation:

The shape of the molecule ${\text{NH}}_{\text{2}}\text{Cl}$ is trigonal pyramidal as shown:

The central atom has four surrounding regions.

The polarity of a molecule depends on the electronegativity of atoms in that molecule and the shape of the molecule. A molecule which has one polar bond is polar.

A molecule which has all nonpolar bonds is nonpolar.

The symmetric molecule will be nonpolar because the polarity of bonds is canceled out. Thus an asymmetric molecule is polar because the polarity of bonds is not canceled.

Therefore, the asymmetric molecule ${\text{NH}}_{\text{2}}\text{Cl}$ is polar.

Conclusion:

Therefore, the shape of the molecule ${\text{NH}}_{\text{2}}\text{Cl}$ is trigonal pyramidal as shown:

The molecule ${\text{NH}}_{\text{2}}\text{Cl}$ is polar.