Consider an atom of Krypton ( Z = 36 ) in its ground state. Find the number of electrons that satisfy the following two conditions respectively: (A) n + l = 4 (B) n = 3, m _ l = +1

Step-by-step solution

Write the ground state electronic configuration of Krypton ( Z = 36 ): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d¹⁰ 4p^6 For condition (A): n + l = 4 Identify the subshells in the configuration where the sum of n and l is 4 . These are 4s ( n =4, l=0 4+0=4 ) and 3p ( n =3, l=1 3+1=4 ). The number of electrons in the 4s subshell is 2 . The number of electrons in the 3p subshell is 6 . Total electrons satisfying condition (A) = 2 + 6 = 8 . For condition (B): n = 3, m _ l = +1 Identify the subshells in the n =3 shell: 3s, 3p, 3