Which of the following arrangements of electrons is most likely to be stable?

Match the following laws with their correct statements:

Laws	Statements
$(1)$ Hund's Rule	$(A)$ No two electrons in an atom can have the same set of all four quantum numbers.
$(2)$ Aufbau Principle	$(B)$ Half-filled and fully-filled orbitals have greater stability.
$(3)$ Pauli Exclusion Principle	$(C)$ Electrons prefer to remain unpaired in degenerate orbitals first.
$(4)$ Heisenberg's Uncertainty Principle	$(D)$ It is impossible to determine simultaneously the exact position and exact momentum of an electron.
	$(E)$ In the ground state of atoms,orbitals are filled in the order of increasing energy.

Match the items in List-$I$ with the items in List-$II$.

List-$I$	List-$II$
$A$. Nodes	$I$. Three dimensional shape of the orbital
$B$. Subsidiary quantum number	$II$. Significant only for motion of microscopic objects
$C$. White light	$III$. $|\psi|^2$ is zero
$D$. Heisenberg uncertainty principle	$IV$. Spin state of electron
	$V$. Continuous spectrum

Which of the following graphs is correct for the kinetic energy $(K.E.)$ of an electron in the $n^{th}$ orbit of a hydrogen-like atom?

In $H$ atom,an orbit has a diameter of about $16.92 \ \mathring{A}$. What is the maximum number of electrons that can be accommodated in this orbit?

Consider the following statements:
$(a)$ Photon is a positively charged nuclear particle
$(b)$ Size of nucleus is very small as compared to the size of atom
$(c)$ Photoelectric effect and diffraction show particle nature of light
$(d)$ Planck's constant has same dimensions as angular momentum
The correct statements is/are: