Answer
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Work Step by Step
The electron configuration of the given oxygen atom is \( 1 s^{2} 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{2} \). In this configuration, there are two unpaired electrons in the 2p subshell. The 2p subshell has three orbitals, each of which can hold a maximum of two electrons. In the given configuration, two of the three orbitals are singly occupied, and the third orbital is empty. Therefore, there are two unpaired electrons.
This is an excited state of oxygen because the ground state electron configuration of oxygen is \( 1 s^{2} 2 s^{2} 2 p_{x}^{1} 2 p_{y}^{1} 2 p_{z}^{1} \). In the ground state, all three 2p orbitals are singly occupied by electrons with parallel spins.
In going from the excited state to the ground state, energy would be released because the ground state is the lowest energy state. The energy released would be in the form of electromagnetic radiation, such as visible light or ultraviolet radiation.
