The electronic configuration with the highest ionization enthalpy is:
`[Ne]3s^(2)3p^(1)`
`[Ne]3s^(2)3p^(2)`
`[Ne]3s^(2)3p^(3)`
`[Ne]3d^(10)4s^(2)4p^(3)`

Which of the following has the hihest electron gain enthalpy. Give reasons. (a) [Ne]3s^(2)3p^(3) (b) [Ne]3s^(2)3p^(4) ( c) [Ne]3s^(2)3p^(5) , (d) [Ne]3s^(2)3p^(6)

Elements A to E have the following electronic configuration: A: [He]2s^(2) 2p^(2) , B: [Ne]3s^(2) 3p^(2) , C: [Ne]3s^(2) 3p^(3) , D: [Ne]3s^(2) 3p^(4) , E: [Ar]4s^(2) . Which of the above will belong to the same group in the periodic table?

Consider the first ionization energies of the elements whose electronic configurations correspond to the following. I. [He]2s^(2) 2p^3 II. [He]2s^(2) 2p^4 III. [Ne]3s^(2)3p^(1) [Ar]3d^(10)4p^1 Which of the above have almost the same first ionization energies?

The electronic configuration 1s2 ,2s2,2p6,3s2,3p6 corresponds to

The electronic configuration for some neutral atoms are given below : (i) 1s^(2),2s^(2),2p^(6),3s^(2) (ii) 1s^(2),2s^(2)2p^(6),3s^(1) (iii) 1s^(2),2s^(2)2p^(6),3s^(2)3p^(2) (iv) 1s^(2),2s^(2)2p^(6),3s^(2)3p^(3) Which of these is expected to have the highest second 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 of an element is 1s^(2)2s^(2)2p^(2)3s^(2)3p^(6)3d^(5)4s^(1) This represents its

The electronic configuration of an element is 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(5)4s^(1) .This represents its

The number of valence electrons in an atom with the configuration 1s^(2)2s^(2)2p^(6)3s^(2)3p^(2) is:

The increasing order of electron affinity of the electronic configurations of element is :- (I) 1s^(2) 2s^(2)2p^(6)3s^(2)3p^(5) (II) 1s^(2) 2s^(2)2p^(3) (III) 1s^(2)2s^(2)2p^(5) (IV) 1s^(2)2s^(2)2p^(6) 3s^(1)