How does the orbital energy change as the nuclear charge increases from $Ne$ to $Ca$?

The unpaired electrons in $Al$ and $Si$ are present in the $3p$ orbital. Which electrons will experience a higher effective nuclear charge from the nucleus?

Between $2s$ and $2p$ electrons,which one experiences a greater shielding effect from inner shells?

For the valence shell of $Na$,screening is provided by:

Arrange $s, p, d,$ and $f$ subshells of a shell in the increasing order of effective nuclear charge $(Z_{eff})$ experienced by the electron present in them.

The bromine atom possesses $35$ electrons. It contains $6$ electrons in $2p$ orbital,$6$ electrons in $3p$ orbital and $5$ electrons in $4p$ orbital. Which of these electrons experiences the lowest effective nuclear charge?