Asked Jan 15, 2020

For each of the following electron configurations determine whether it is ground state, excited state or impossible.

a. 1s22s32p1

b. 1s22s2

c. 1s22s2

d. 1s22s22p54f1

e. 1s22p2

f. 1s22s2

g. 2p63s13d1

h. 1s11p1


Expert Answer

Step 1

Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If you want remaining sub-parts to be solved, then please resubmit the whole question and specify those sub-parts you want us to solve.


The given electronic configuration is 1s22s32p1.

According to the Pauli exclusion principle, a maximum of 2 electrons can be added in a single orbital due to which 2s subshell can hold only 2 electrons as it contains only 1 orbital. But in the given electronic configuration, 2s orbital contains 3 electrons which is not possible. Hence, this electronic configuration is impossible.

Step 2



The given electronic configuration is 1s22s2.

In this electronic configuration both 1s and 2s orbitals contains two electrons and no excitation of electrons to the higher energy level occurs. Therefore, it represents the ground state electronic configuration.

Step 3


The given electronic configuration is 1s22s22p54f1.

In this electronic configuration both 1s and 2s orbitals contains two electrons and the excitation of one 2p electron occurs direc...

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