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
Answer:
b) is the correct answer
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.