Statement (A) : The first ionization energy of Al is less than the first ionization energy of Mg.
Statement (B) : The first ionization energy of Na is less than the first ionization energy of Mg.
Statement (C) : The second ionization of Mg is greater than the second ionization energy of Na.

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All the above statements are correct

All the above statements are incorrect

A and B are correct but C is incorrect

All the above statements are incorrect

answer is C.

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Detailed Solution

Statement-A: $Al <Mg$ is correct because $Al$ -13, electronic configuration is ${1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2} {3p}^{1}$ electron has to be removed from ${3p}^{1}$ where as in Mg-

12, ${1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2}$ , similarly the electron has to be removed from the completely filled stable s-orbital.

Statement -B: Na-11, electronic configuration is ${1s}^{2} {2s}^{2} {2p}^{6} {3s}^{1}$ electron has to be removed from ${3s}^{1}$ , for Mg-12, ${1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2}$ , similarly the electron has to be removed from the completely filled stable s-orbital.

Statement-C: $M g > N a$ is incorrect because ${Mg}^{2+}$ electronic configuration is ${1s}^{2} {2s}^{2} {2p}^{6} {3s}^{1}$ here the electron has to be removed from ${3s}^{1}$ similarly for ${Na}^{+}$ electronic configuration is ${1s}^{2} {2s}^{2} {2p}^{6}$ which is a stable electronic configuration.. Therefore the correct statement is the second ionization of Mg is less than the second ionization energy of Na.