JEE Main Chemistry question

If the IP of Na is 5.48 eV, the ionisation potential of K will be

(A)Same as that of Na
(B)4.34 eVCorrect
(C)5.68 eV
(D)10.88 eV

Answer: (B)

Solution

Ionisation potential decreases down a group as atomic size increases, so K (below Na in Group 1) must have a lower IP than Na's 5.48 eV. The literature value for potassium's first

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Question ID VK-133263