Question

5. These sets of quantum numbers are each supposed to specify an orbital. One set, however, is erroneous. Which one and why?

a. n = 3; l = 0; ml = 0

b. n = 2; l = 1; ml = –1

c. n = 1; l = 0; ml = 0

d. n = 4; l = 1; ml = –2

Answer 1

option (d) is not possible

a) n=3;l=0;ml=0

for n=3, l=0, the orbital is 3s

for l=0, ml=0(1)

so 3s orbital is possible with the given quantum numbers

b) n=2; l=1 ; ml=-1

For n=2; l=1, the orbital is 2p

for l=0, ml=-1,0,+1(3)

so, 2p orbital is possible with the given quanyum numbers

c) n=1; l=0; ml=0

For n=1; l=0, the orbitsl is 1s

for l=0, ml=0(1)

1s orbital is possible with the given quantum numbers

d) n=4; l=1; ml=-2

For n=4; l=1, the orbital is 4p

for l=1, the possible orientations of ml= -1,0,+1(3)

but given ml=-2, so the orbital is not possible with the givenquantum numbers

Note: ml= 2l+1