Which of the following electronic configurations has the lowest ionization enthalpy ?
(a) `1s^2 , 2s^2 , 2p^5`, ,(b) `1s^2 , 2s^2 , 2p^6`
(c) `1s^2 , 2s^2 , 2p^6 , 3s^1`.

Which of the following electronic configuration is/are wrong? 1. 1s^2 2s^(2)2p_(x)^(2)2p_(y)^(1) (for nitrogen) 2. 1s^(2)2s^(2)2p_(x)^(2)2p_(y)^(1)2p_(z)^(1) (for oxygen) 3. 1s^2 2s^2 2p^6 3s^(2)3p^(6)3d^(5)4s^(1) (for chromium) 4. 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(6)4s^(2) (for iron)

The atom having the outer electronic configuration 4s^(2)4p^(2) would be in:

Which of the following overlapping of atomic orbitals will not be allowed? 2s+2s

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

Consider the electronic configuration: 1s^(2)2s^(2)2p_(x)^(2) It violates

The electronic configuration of an element is 1s^2 2s^2 2p^6 3s^2 . It is most likely to have a valecy of :

Which of the following overlaping of atomic orbital will not be allowed ? (i) 2P_x + 2P_z (ii) 2P_x - 2P_x (iii) 2s + 2s