The ionization energy of Argon $(A r)$ is greater than:
I. Chlorine $(C l)$
II. Phosphorous $(P)$
III. Neon $(N e)$

I, II, and III

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I and II only

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II and III only

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I only

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Solution

The correct option is B I and II only
The IE of elements increases towards the right in a period and decrease down the group. Hence the IE of Argon ( $A r$ ) is greater than that of $C l$ (Chlorine) and $P$ (Phosphorous) but less than $N e$ (Neon). Hence answer is option B.

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The ionization energy of Argon (Ar) is greater than:I. Chlorine (Cl)II. Phosphorous (P)III. Neon (Ne)

The correct option is B I and II onlyThe IE of elements increases towards the right in a period and decrease down the group. Hence the IE of Argon (Ar) is greater than that of Cl (Chlorine) and P(Phosphorous) but less than Ne (Neon). Hence answer is option B.

The ionization energy of Argon $(A r)$ is greater than:
I. Chlorine $(C l)$
II. Phosphorous $(P)$
III. Neon $(N e)$

The correct option is B I and II only
The IE of elements increases towards the right in a period and decrease down the group. Hence the IE of Argon ( $A r$ ) is greater than that of $C l$ (Chlorine) and $P$ (Phosphorous) but less than $N e$ (Neon). Hence answer is option B.