Question

Does each of the configurations in FIGURE Q$41.6$represent a possible electron configuration of an element? If so,

(i) identify the element and

(ii) determine whether this is the ground state or an excited state. If not, why not?

Short answer

$2p$a. Yes, this is the ground state of nitrogen. The $p$subshells have $6$states, then they can accept three electrons without the Pauli exclusion principle.

b. No, the only two electrons are accessed in the $2s$state.

c. No, the $2s$states are the lowest energy than the $2p$states, then the ground state would be occupied before the $2p$state.

Step-by-step solution

Part (a) step 1: Given Information 

We need to find identify the element and determine whether this is the ground state or an excited state in diagram (a).

Part (a) step 2: Explanation

Yes, this is the ground state of nitrogen. The $p$subshells have $6$states, then they can accept three electrons without the Pauli exclusion principle.

Part (b) step 1: Given Information 

We need to find identify the element and determine whether this is the ground state or an excited state in diagram (b).

Part (b) step 2: Explanation

No, the only two electrons are accessed in the $2s$state.

Part (c) step 1: Given Information 

We need to find identify the element and determine whether this is the ground state or an excited state in diagram (c).

Part (c) step 2: Explanation

No, the $2s$states are the lowest energy than the $2p$states, then the ground state would be occupied before the $2p$state.