Question

what are the possible subshell when n=4?How many orbitals are contained by each of these shells?? explain it a bit plz​

Answer 1

Answer:

Therefore in n=4, number of subshells=4, orbitals=16 and number of electrons =32.

Explanation:

For n

th

orbital possible values of azimuthal quantum number (subshell), l are from 0 to (n-1). Total of 'n' values.

In n=4, l=0,1,2,3 thus there are 4 subshells i.e.s,p,d,f respectively.

Magnetic quantum number m

l

have values from -l to +l and total of 2l+1 values.

For n=4, possible values of l and m

l

are:

m

l

=0 for l=0; total m

l

values =1

m

l

=−1,0,1 for l=1; total m

l

values =3

m

l

=−2,−1,0,1,2 for l=2; total m

l

values =5

m

l

=−3,−2,−1,0,1,2,3 for l=3; total m

l

values =7

Total number of orbitals = total values of m

l

for n=4,

∴1+3+5+7=16 orbitals

Each orbital can occupy maximum of two electron

Number of electrons =2×16=32

Therefore in n=4, number of subshells=4, orbitals=16 and number of electrons =32.

Answer 2

Answer:

shell number=n=4

subshell number=l=n-1=4-1=3

so subshell number would be 0,1,2,3

and subshells in 4th shell would be 4s,4p,4d and 4f

now orbital number=-l to +l

so in subshell number 0(4s)

number of orbitals =-0 to +0 =0

so 4s subshell has 1 orbital

now in subshell number 1(4p):

number of orbitals=-1 to +1=3

so 4p subshell has 3 orbitals

now in subshell number 2(4d):

number of orbitals=-2 to +2=5

so 4d subshell has 5 orbitals

now in subshell number 3(4f):

number of orbitals=-3 to +3=7

so 4f subshell has 7 orbitals

so at last in total shell number 4 has

1+3+5+7=16 orbitals

4 subshells

16 orbitals

32 electrons