Question

Write the electron configuration for the monatomic ions formed from the following elements (which form the greatest concentration of monatomic ions in seawater): (a) \({\rm{Cl}}\) (b) \({\rm{Na}}\) (c) \({\rm{Mg}}\)(d) \({\rm{Ca}}\) (e) \({\rm{K}}\) (f) \({\rm{Br}}\) (g) \({\rm{Sr}}\) (h) \({\rm{F}}\).

Short answer

1. The electron configuration is obtained as: \(\left[ {{\rm{Ne}}} \right]{\rm{3s^{2}3}}{{\rm{p}}^{\rm{6}}}\).
2. The electron configuration is obtained as: \(\left( {{\rm{Ne}}} \right)\).
3. The electron configuration is obtained as: \(\left( {{\rm{Ne}}} \right)\).
4. The electron configuration is obtained as: \(\left( {{\rm{Ar}}} \right)\).
5. The electron configuration is obtained as: \(\left( {{\rm{Ar}}} \right)\).
6. The electron configuration is obtained as: \(\left( {{\rm{Kr}}} \right)\).
7. The electron configuration is obtained as: \(\left( {{\rm{Kr}}} \right)\).
8. The electron configuration is obtained as: \(\left( {{\rm{Ne}}} \right)\).

Step-by-step solution

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

Writing the electron configuration for monoatomic ion

a. The ion formed is: \({\rm{C}}{{\rm{l}}^{\rm{ - }}}\).

Then, it’s electron configuration will be: \(\left[ {{\rm{Ne}}} \right]{\rm{3s^{2}3}}{{\rm{p}}^{\rm{6}}}\).

Therefore, electron configuration is: \(\left[ {{\rm{Ne}}} \right]{\rm{3s^{2}3}}{{\rm{p}}^{\rm{6}}}\).

Writing the electron configuration for monoatomic ion

b.

The ion formed is: \({\rm{N}}{{\rm{a}}^{\rm{ + }}}\).

Then, it’s electron configuration will be:\(\left( {{\rm{Ne}}} \right)\).

Therefore, electron configuration is: \(\left( {{\rm{Ne}}} \right)\).

Writing the electron configuration for monoatomic ion

c.

The ion formed is: \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\).

Then, it’s electron configuration will be:\(\left( {{\rm{Ne}}} \right)\).

Therefore, electron configuration is: \(\left( {{\rm{Ne}}} \right)\).

Writing the electron configuration for monoatomic ion

d.

The ion formed is: \({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}\).

Then, it’s electron configuration will be:\(\left( {{\rm{Ar}}} \right)\).

Therefore, electron configuration is: \(\left( {{\rm{Ar}}} \right)\).

Writing the electron configuration for monoatomic ion

e.

The ion formed is: \({{\rm{K}}^{\rm{ + }}}\).

Then, it’s electron configuration will be:\(\left( {{\rm{Ar}}} \right)\).

Therefore, electron configuration is: \(\left( {{\rm{Ar}}} \right)\).

Writing the electron configuration for monoatomic ion

f.

The ion formed is: \({\rm{B}}{{\rm{r}}^{\rm{ - }}}\).

Then, it’s electron configuration will be:\(\left( {{\rm{Kr}}} \right)\).

Therefore, electron configuration is: \(\left( {{\rm{Kr}}} \right)\).

Writing the electron configuration for monoatomic ion

g.

The ion formed is: \({\rm{S}}{{\rm{r}}^{{\rm{2 + }}}}\).

Then, it’s electron configuration will be:\(\left( {{\rm{Kr}}} \right)\).

Therefore, electron configuration is: \(\left( {{\rm{Kr}}} \right)\).

Writing the electron configuration for monoatomic ion

h.

The ion formed is: \({{\rm{F}}^{\rm{ - }}}\).

Then, it’s electron configuration will be:\(\left( {{\rm{Ne}}} \right)\).

Therefore, electron configuration is: \(\left( {{\rm{Ne}}} \right)\).