`{:(,"ColumnI",,"ColumnII"),((A),"The d-orbital which has two angular nodes",(P),3d_(x^(2)-y^(2))),((B),"The d-orbitial with two nodal surfaced from conce",(Q),3d_(s^2)),((C),"The orbital without angular node",(R),4f),((D),"The orbital which has three angular nodes",(S),3s):}`

{:(,"ColumnI",,"ColumnII"),((A),"The radial node of 5s atomic orbital is",(P),1),((B),"The angular node of" 3d_(yz) "atomic orbital is",(Q),4),((C),"The sum of angular node and radial node of" 4d_(xv) "atomic orbital",(R),2),((D),The "angular node of 3patomic orbital is",(S),3):}

{:(,"ColumnI",,"ColumnII"),((A),"Number of orbitials in then" n^(th)"sheel",(P),2(2l+1)),((B),"Maximum number of electrons in a subshell",(Q),n),((C),"Number of subshell in" n^(th)"sheel",(R),2l+1),((D),"Number of orbitals in a subshell",(S),n^(2)):}

{:(,"ColumnI",,"ColumnII"),((A),"Orbital angular momentum of an electron",(P),sqrt(s(s+1))(h)/(2pi)),((B),"Angular momentum of an electron in an orbit",(Q),sqrt((n(n+2)))),((C),"Spin angular momentum of an electron",(R),(nh)/(2pi)),((D),"Magnetic moment of atom",(S),sqrt((l(l+1)(h)/(2pi)))):}

{:("ColumnI (shell)","ColumnII (value of l)"),((A)2nd,(P)1),((B)3rd,(Q)2),((C)4th,(R)3),((D)1st,(S)0):}

{:(,"ColumnI",,"ColumnII"),((A),"Lyman series",(P),"Visible region"),((B),"Humphery series",(Q),"Ultraviolen region"),((C),"Paschen series",(R),"Infrared region"),((D),"Balmer series",(S),"Far infared region"):}

Using s, p, d and f notations, describe the orbital with the quantum number. n = 3 , l = 2

The correct order of closeness of 3s,3p,3d orbitals of nucleus is :

Using s, p, d and f notations, describe the orbital with the quantum number. n = 5 , l = 3

Using s, p, d and f notations, describe the orbital with the quantum number. n = 3 , l = 0

Using s, p, d notations, describe the orbital with the quantum number. n = 4, l = 3