Consider the below statements and identify the correct answer.
Statement I: Atomic radius increases in moving from left to right along a period.
Statement II: Nuclear charge increases in moving from left to right along a period.

Correct option is A

Sol: The correct answer is (a) Only Statement II is correct.

Analyze the given statements:

Statement I: Atomic radius increases in moving from left to right along a period.

• We move from left to right across a period in the periodic table, the atomic radius decreases.
• This is because, while electrons are added to the same energy level, the nuclear charge (protons in the nucleus) increases, which attracts the electrons more strongly and pulls them closer to the nucleus, resulting in a smaller atomic radius. This is Incorrect 

​Statement II: Nuclear charge increases in moving from left to right along a period.

• As we move from left to right across a period, protons are added to the nucleus, which increases the nuclear charge.
• This increase in nuclear charge leads to a stronger attraction between the nucleus and the electrons. This is correct 
  

Statement I is incorrect, and Statement II is correct.