Question

Which of the following statement is INCORRECT with p-block elements?

• A. p-Block elements comprise of Group \( 13 \) to Group \( 18 \).
• B. The outer electronic configuration of p-block elements is \( ns^2\,np^{1-6} \).
• C. Halogens belongs to Group \( 16 \).
• D. Gallium and Bromine are liquids.
• E. The zero group elements having general formula \( ns^2p^6 \) are inert, because their energy levels are completely filled.

Hint:

Remember the p-block groups: \[ 13,14,15,16,17,18 \] and specifically: \[ \text{Group 17 = Halogens}, \qquad \text{Group 18 = Noble gases} \]

Answer 1

The Correct Option is C

Step 1: Recall what p-block elements are.
The p-block elements are those in which the last electron enters the p-subshell.
They occupy Groups \[ 13 \text{ to } 18 \] in the modern periodic table.
So statement (1) is correct.

Step 2: Recall the general outer electronic configuration.
The general valence shell configuration of p-block elements is: \[ ns^2\,np^{1-6} \] This matches statement (2), so it is also correct.

Step 3: Identify the halogen group correctly.
Halogens are the elements: \[ \text{F, Cl, Br, I, At} \] These belong to \[ \text{Group }17 \] not Group \( 16 \).
Therefore the statement \[ \text{Halogens belongs to Group 16} \] is incorrect.

Step 4: Examine statement (4).
Gallium has a very low melting point and can melt near room temperature, while bromine is a liquid at room temperature.
This statement is generally taken as correct in such objective questions.

Step 5: Examine statement (5).
Noble gases, except helium, have the general configuration: \[ ns^2 p^6 \] Their valence shell is completely filled, which makes them chemically inert.
So statement (5) is also correct in essence.

Step 6: Compare all options.
Among all given statements, the only clearly incorrect one is: \[ \text{Halogens belongs to Group 16} \] because halogens are actually in Group \( 17 \).

Step 7: Final conclusion.
Hence, the incorrect statement is \[ \boxed{\text{Halogens belongs to Group 16}} \] Therefore, the correct option is \[ \boxed{(3)} \]