$(13$ points, $2$ points each parts a$-$d$,5$ points part $e)$ All parts refer to the same neutral atom.

A student attempted to draw an excited state electron configuration for a neutral atom, and their work is shown here as an orbital box diagram. Note that the relative energies of each subshell are indicated but their exact energies are not listed.

$($a$)$ There is exactly one error in this electron configuration. This error makes the configuration impossible according to quantum mechanics. Identify the one error and state why it is impossible: be specific.

$($b$)$ Draw the orbital box $n$ subshell labels.

$($c$)$ What is the total number of orbitals that are occupied $($contain any electrons$)$ in your configuration from part $($b$)?$

$($d$)$ How many unpaired electrons are represented in your configuration from part $($b$)?$

$($e$)$ Classify each statement as accurate or inaccurate: write ONLY accurate or inaccurate for each answer.

All of the s orbitals have the same shape.

All of the s orbitals have the same energy.

Comparing the $2s$ and $3$ s orbitals, an electron in the $2s$ orbital experiences weaker attractions to the nucleus and require less energy to remove from the atom.

Comparing the $2s$ and $3$ s orbitals, the $3s$ orbital does not exist in the ground state.

The ground state configuration for the neutral atom implies that this is

$2$

$3$

$4.$ a paramagnetic atom.

$5.$