Question

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:

1. K and S 
2. Ca and O 
3. Al and N.

Answer 1

(a) \(K\) and \(S\): 
The electronic configurations of \(K\) and \(S\) are as follows:
\(K\) : \(2, 8, 8, 1\) 
\(S\) : \(2, 8, 6\)

Sulphur \((S)\) requires \(2\) more electrons to complete its octet. Potassium \((K)\) requires one electron more than the nearest noble gas i.e., \(Argon\). Hence, the electron transfer can be shown as:

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(b) \(Ca\) and \(O\):
The electronic configurations of \(Ca\) and \(O\) are as follows:
\(Ca\) : \(2, 8, 8, 2\)
\(O\) : \(2, 6\) 
Oxygen requires two electrons more to complete its octet, whereas calcium has two electrons more than the nearest noble gas i.e., \(Argon\). Hence, the electron transfer takes place as:

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(c) \(Al\) and \(N\): The electronic configurations of \(Al\) and \(N\) are as follows:
\(Al\): \(2, 8, 3\) 
\(N\) : \(2, 5\) 
Nitrogen is three electrons short of the nearest noble gas (Neon), whereas aluminium has three electrons more than Neon. 
Hence, the electron transference can be shown as: