Question

Which of the following elements is expected to show non-metallic character?

• A. $As$
• B. $Be$
• C. $B$
• D. $Br$

Answer 1

The correct option is D

$\mathrm{Br}$

The explanation for correct option:

(D) $\mathrm{Br}$

• Metals show a tendency to lose electrons, hence are electropositive.
• Non-metals show tendency to accept or share electrons, hence are electronegative.
• The trend for non-metallic character is discussed below:

The non-metallic character increases across a period. As one moves down the group, the non-metallic character decreases due to an increase in atomic size.

Since, $\mathrm{Br}$ shows the non-metallic character as an electronegative atom tends to accept electrons. Thus, Option (D) is correct.

The explanation for incorrect options:

(A) $\mathrm{As}$ has intermediate properties between metal and non-metal. Thus, it will have both metallic and non-metallic characters.

(B) $\mathrm{Be}$ shows metallic character since it belongs to Group-2.

(C) $\mathrm{B}$ is the only non-metal of group-13. Thus, it will show non-metallic character. In comparison to $\mathrm{Br}$, $\mathrm{B}$ is less electronegative and $\mathrm{Br}$ comes after $\mathrm{B}$ in the periodic table.

Therefore, the correct option is (D).