Consider the following sets of quantum numbers:

$Set$	$(n)-(l)-(m)-(s)$
$(i)$	$(3)-(2)-(1)-(+1/2)$
$(ii)$	$(2)-(2)-(1)-(+1/2)$
$(iii)$	$(4)-(3)-(-2)-(-1/2)$
$(iv)$	$(1)-(0)-(-1)-(-1/2)$
$(v)$	$(3)-(2)-(3)-(+1/2)$

Which of the following sets of quantum numbers is not possible?

The total number of electrons present in all the $p$-orbitals of bromine is

The electronic configuration of a nitrogen atom in its ground state is represented as follows:

Although no currently known element contains electrons in $g$ orbitals in the ground state,it is possible that such an element will be found or that electrons in excited states of known elements could be in $g$ orbitals. For $g$ orbitals,$l = 4$. What is the lowest value of $n$ for which $g$ orbitals could exist? What are the possible values of $m_l$? How many electrons could a set of $g$ orbitals hold?

The electronic configurations of four elements are given in brackets: $L\,(1s^2, 2s^2 2p^1)$; $M\,(1s^2, 2s^2 2p^5)$; $Q\,(1s^2, 2s^2 2p^6, 3s^1)$; $R\,(1s^2, 2s^2 2p^2)$. Which element would most readily form a diatomic molecule?

The correct order of increasing energy of atomic orbitals is