Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur $\left(\text{S}\right)$.

Answer to Problem 13E

The ionic charge for sulfur $\left(\text{S}\right)$ is $2-$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge $2-$.

Conclusion:

Therefore, the ionic charge for sulfur $\left(\text{S}\right)$ is $2-$.

(b)

To determine

The ionic charge for the given element potassium $\left(\text{K}\right)$.

Answer to Problem 13E

The ionic charge for potassium $\left(\text{K}\right)$ is $1+$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge $1+$.

Conclusion:

Therefore, the ionic charge for potassium $\left(\text{K}\right)$ is $1+$.

(c)

To determine

The ionic charge for the given element bromine $\left(\text{Br}\right)$.

Answer to Problem 13E

The ionic charge for bromine $\left(\text{Br}\right)$ is $1-$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge $1-$.

Conclusion:

Therefore, the ionic charge for bromine $\left(\text{Br}\right)$ is $1-$.

(d)

To determine

The ionic charge for the given element nitrogen $\left(\text{N}\right)$.

Answer to Problem 13E

The ionic charge for nitrogen $\left(\text{N}\right)$ is $3-$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge $3-$.

Conclusion:

Therefore, the ionic charge for nitrogen $\left(\text{N}\right)$ is $3-$.

(e)

To determine

The ionic charge for the given element magnesium $\left(\text{Mg}\right)$.

Answer to Problem 13E

The ionic charge for magnesium $\left(\text{Mg}\right)$ is $2+$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge $2+$.

Conclusion:

Therefore, the ionic charge for magnesium $\left(\text{Mg}\right)$ is $2+$.

(f)

To determine

The ionic charge for the given element neon $\left(\text{Ne}\right)$.

Answer to Problem 13E

The ionic charge for neon $\left(\text{Ne}\right)$ is $0$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of $0$.

Conclusion:

Therefore, the ionic charge for neon $\left(\text{Ne}\right)$ is $0$.

(g)

To determine

The ionic charge for the given element carbon $\left(\text{C}\right)$.

Answer to Problem 13E

The ionic charge for carbon $\left(\text{C}\right)$ is $0$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of $0$.

Conclusion:

Therefore, the ionic charge for carbon $\left(\text{C}\right)$ is $0$.

(h)

To determine

The ionic charge for the given element aluminium $\left(\text{Al}\right)$.

Answer to Problem 13E

The ionic charge for aluminium $\left(\text{Al}\right)$ is $3+$.

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge $3+$.

Conclusion:

Therefore, the ionic charge for aluminium $\left(\text{Al}\right)$ is $3+$.