Maximum number of electrons present in these orbitals having at least "'2'" nodes is (I) "n=1,l=0,m_(l)=0],[(II)n=3,l=2,m_(l)=+1],[(III)n=5,l=1,m_(l)=+1],[(IV)n=3,l=2,m_(l)=-1],[" ( "V)n=2,l=1,m_(l)=0]]

Describe the orbital having n=2,l=1 and m=0 .

Give the possible value for the missing quantum number (s) in each of the following sets. (a) n=3, l=0, m_(l)=? , (b) n=3, l=?, m_(l)=-1 (c) n=?, l=1, m_(l)=+1 , (d) n=?, l=2, m_(l)=? .

Arrange the electrons represented by the following sets of quantum numbers in decreasing order of energy. (i) n=4, l=0, m_(l)=0, s=+1//2 , (ii) n=3, l=1, m_(l)=1, s=-1//2 (iii) n=3, l=2, m_(l)=0, s=+1//2 , (iv) n=3, l=0, m_(l)=0, s=-1//2

The quantum number of electrons are given below: Arrange then in order of increasing energies a. n= 4,l= 2,m_(1)= -2, m_(s)= -(1)/(2) b. n= 3,l= 2,m_(1) = 1, m_(s)= +(1)/(2) c. n= 4,l= 1,m_(1) = 0, m_(s)= +(1)/(2) e.n= 3,l= 2,m_(1)= -2, m_(s)= +(1)/(2) f. n= 4,l= 1,m_(1) = +1, m_(s)= +(1)/(2)

Name the orbitals corresponding to given set of quantum numbers (i() n=3, l=2, m=+-2 (ii) n=4, l=0, m=0 (iii) n=3, l=1, m+-1 (iv) n=2, l=1, m=1

From the following sets of quantum numbers, state which are possible. Explain why the others are not possible. (a) n=0, l=0, m_(l)=0, s=+1//2 , (ii) n=1, l=0, m_(l)=0, s=-1//2 (iii) n=1, l=1, m_(1)=0, s=+1//2 , (iv) n=1, l=0, m_(l)=+1, s=+1//2

In a multi - electron atom , which of the following orbitals described by the three quantum numbers will have the same energy in the absence of magnetic and electric fields ? (A) n=l, l=0,m=0 (B) n = 2, l =0 , m= 0 (C) n = 2 , l = 1 , m = 1 (D) n = 3, l =2 , m=1 (E) n=3,l=2,m=0.