JEE MAIN - Chemistry (2022 - 27th July Evening Shift - No. 5)
Outermost electronic configurations of four elements A, B, C, D are given below :
(A) $$3 s^{2}$$
(B) $$3 s^{2} 3 p^{1}$$
(C) $$3 s^{2} 3 p^{3}$$
(D) $$3 s^{2} 3 p^{4}$$
The correct order of first ionization enthalpy for them is :
(A) < (B) < (C) < (D)
(B) < (A) < (D) < (C)
(B) < (D) < (A) < (C)
(B) < (A) < (C) < (D)
Explanation
Orbitals with fully filled and half-filled electronic configuration are stable, and require more energy for ionization
Elements with greater electronegativity require more energy for ionisation
Hence the correct order is $C>D>A>B$
Elements with greater electronegativity require more energy for ionisation
Hence the correct order is $C>D>A>B$
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