Which of the following electronic configurations has the maximum total spin multiplicity?

The set of quantum numbers $n = 3$,$l = 0$,$m = 0$,$s = -1/2$ belongs to the element

What is the maximum number of electrons that can be accommodated in a single $p$ orbital?

For a $4p$-orbital,the number of radial and angular nodes,respectively,are

"Pairing of electrons in the orbitals belonging to the same subshell does not occur unless each orbital belonging to that subshell has got one electron each." This statement is known as

The number of correct statements from the following:
$A.$ For $1s$ orbital,the probability density is maximum at the nucleus.
$B.$ For $2s$ orbital,the probability density first increases to maximum and then decreases sharply to zero.
$C.$ Boundary surface diagrams of the orbitals enclose a region of $100\%$ probability of finding the electron.
$D.$ $p$ and $d$-orbitals have $1$ and $2$ angular nodes respectively.
$E.$ Probability density of $p$-orbital is zero at the nucleus.