Question

An element having configuration $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}4{\mathrm{s}}^1$ will form:

• A. Acidic oxide
• B. Amphoteric oxide
• C. Basic oxide
• D. None of these

Answer 1

The correct option is C

Basic oxide

Explanation for the correct option:

(c) Basic oxide

• The last electron in the arrangement $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}4{\mathrm{s}}^1$ belongs to the s subshell.
• An element having configuration $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}4{\mathrm{s}}^1$ is Potassium $\left(\mathrm{K}\right)$
• As a result, it belongs to the s block elements and it belongs to Group 1 i.e. Alkali metals.
• Metals usually create basic oxides.
• Metals react with oxygen and form a basic oxide.

Explanation for the incorrect options:

(a) Acidic oxide

• Acidic oxide is formed when non-metal reacts with oxygen.
• Hence this option is not correct.

(b) Amphoteric oxide

• Amphoteric oxide is formed when metals having many oxidation states reacts with oxygen.
• Hence this option is not correct.

Hence, the correct option is (C) i.e. Basic oxide