Question

which of the following is the correct orbital spin diagram of carbon (c)?

Explanation:

Step1: Determine carbon's electron - configuration

Carbon has an atomic number of 6, so its electron - configuration is \(1s^{2}2s^{2}2p^{2}\).

Step2: Apply Hund's rule for \(2p\) orbitals

According to Hund's rule, electrons in degenerate orbitals (the three \(2p\) orbitals in this case) first occupy separate orbitals with parallel spins before pairing up.
The \(1s\) orbital is filled with 2 electrons with opposite spins (\(\uparrow\downarrow\)), the \(2s\) orbital is also filled with 2 electrons with opposite spins (\(\uparrow\downarrow\)), and the two \(2p\) electrons occupy separate \(2p\) orbitals with parallel spins (\(\uparrow\ \uparrow\)).

Answer:

The fourth option (with \(\uparrow\downarrow\) in \(1s\), \(\uparrow\downarrow\) in \(2s\), and \(\uparrow\ \uparrow\) in \(2p\) with one empty \(2p\) orbital) is the correct orbital - spin diagram of carbon.