`A=1s^(2)2s^(2)2p^(4) B=1s^(2)2s^(2)2p^(5)`
`C=1s^(2)2s^(2)2p^(6)`
(One of A/B/C is neutral atoms)
A,B&C are atoms/anion of same element.
Then :-

The electronic configuration for some neutral atoms are given below. A: 1s^(2) 2s^(2) , B: 1s^(2) 2s^(2)2p^(3) C: 1s^(2) 2s^(2)2p^(4) , D: 1s^(2) 2s^(2)2p^(6) 3s^(1) In which of this electronic configuration would you expect to have highest (a) IE_(1) and (b) IE_(2) .

The electronic configuration for some neutral atoms are given below. A: 1s^(2) 2s^(2) , B: 1s^(2) 2s^(2)2p^(3) C: 1s^(2) 2s^(2)2p^(4) , D: 1s^(2) 2s^(2)2p^(6) 3s^(1) In which of this electronic configuration would you expect to have highest (a) IE_(1) and (b) IE_(2) .

The electronic configuration for the following neutral atoms are given for use in question. (a) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (b) 1s^(2) 2s^(2) 2p^(6) 3s^1 (c ) 1s^(2) 2s^(2) 2p^(4) (d) 1s^(2) 2s^(2) 2p^(5) (e) 1s^(2) 2s^(2) 2p^(6) Which of the electronic configurations given above would you expect to have the lowest ionization enthalpy?

The electronic configuration for the following neutral atoms are given for use in question. (a) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (b) 1s^(2) 2s^(2) 2p^(6) 3s^1 (c ) 1s^(2) 2s^(2) 2p^(4) (d) 1s^(2) 2s^(2) 2p^(5) (e) 1s^(2) 2s^(2) 2p^(6) Which of the electronic configuration given above would you expect for the noble gas?

The electronic configuration for the following neutral atoms are given for use in question. (a) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (b) 1s^(2) 2s^(2) 2p^(6) 3s^1 (c ) 1s^(2) 2s^(2) 2p^(4) (d) 1s^(2) 2s^(2) 2p^(5) (e) 1s^(2) 2s^(2) 2p^(6) Which of the electronic configuration given above would you expect for the noble gas?

The electronic configuration for the following neutral atoms are given for use in question. (a) 1s^(2) 2s^(2) 2p^(6) 3s^(2) (b) 1s^(2) 2s^(2) 2p^(6) 3s^1 (c ) 1s^(2) 2s^(2) 2p^(4) (d) 1s^(2) 2s^(2) 2p^(5) (e) 1s^(2) 2s^(2) 2p^(6) List the above configurations in order of increasing ionization enthalpy.

The electronic structure of four element A, B, C and D are, A. 1s^(2) , B. 1s^(2)2s^(2) 2p^(2), C. 1s^(2) 2s^(2)2p^(5), d. 1s^(2)2s^(2)2p^(6) The tendency to from electrovalent bonds are greatest in

Consider the ground state electronic configuration given below: A: 1s ^(2) 2s ^(2) 2p ^(5) B: 1s ^(2) 2s ^(2) 2p ^(4) C: 1s ^(2) 2s ^(2) 2p ^(6) 3s ^(2) 3p ^(5) D: 1s ^(2) 2s ^(2) 2p ^(6) 3s ^(1) E: 1s ^(2) 2s ^(2) 2p ^(3) Which of the above configuration corresponds to element having (A) largest atomic size. (B) having highest ionisation enthalpy.

Electronic configuration of four elements A, B ,C and D are given below A) 1s^(2), 2s^(2), 2p^(6) B) 1s^(2), 2s^(2), 2p^(4) C) 1s^(2), 2s^(2), 2p^(6), 3s^(1) D) 1s^(2), 2s^(2), 2p^(5) Which of the following is the correct order of increasing tendency to gain electron?