Math, asked by STINKINGSLUG, 1 year ago


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
a) All the statements are correct
b) All the statements are incorrect
c) A, B are correct and C is incorrect
d) A, B are incorrect and C is correct ​

Answers

Answered by arpanbhowmick2
5

Answer:

b) is the correct answer

Answered by anushikaprabhu77
0

Answer:

A,B are correct and C is incorrect

Step-by-step explanation:

Statement-A:  Al <Mg   is correct because Al -13, electronic configuration is 1s2 2s22p63s23p1  electron has to be removed from 3p1  where as in Mg-

12,1s2 2s22p63s2 , similarily the electron has to be removed from the completely filled stable s-orbital.

Statement -B: Na-11, electronic configuration is 1s2 2s22p63s1 electron has to be removed from3s1 , for Mg-12,1s2 2s22p63s2 , similarly the electron has to be removed from the completely filled stable s-orbital.

Statement-C:  Mg>Na   is incorrect because Mg2+  electronic configuration is 1s22s22p63s1  here the electron has to be removed from 3s1   similarly for Na+  electronic configuration is 1s22s22p6  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.

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