Quantum number worksheet

Quantum number is important concept for understanding structure of atom. Here is worksheet on Quantum number to excel in examination

Question 1. What is the total number of orbitals associated with the principal quantum number n = 3 ?

Question 2. Using s, p, d, f notations, describe the orbital with the following quantum numbers
(a) n = 2, l = 1
(b) n = 4, l = 0
(c) n = 5,l = 3
(d) n = 3, l = 2
(e) n=1 , l-0
(g) n=4, l=3

Question 3. Which of the following sets of Quantum is not possible

(a) n = 0, l = 0, m = 0, m = 1/2
(b) n = 1, l = 0, m = 0, m = -1/2
(c) n = 1, l = 1, m = 0, m = -1/2
(d) n = 2, l = 1, m = 0, m = -1/2
(e) n = 3, l = 3, m = –3, m = 1/2
(f) n = 3, l = 2, m = 0, m = 1/2
(g) n = 1,l = 1,m = 0,s = +1/2

 

Question 4. The quantum numbers of six electrons are given below.

i. n = 4, l = 2, ml = –2 , ms = –1/2
ii. n = 3, l = 2, ml = 1 , ms = +1/2
iii. n = 4, l = 1, ml = 0 , ms = +1/2
iv. n = 3, l = 2, ml = –2 , ms = –1/2
v. n = 3, l = 1, ml = –1 , ms = +1/2
vi. n = 4, l = 1, ml = 0 , ms = +1/2

Answer below questions
a) which of the electrons are in same energy level
b) which of the electron is having lowest energy
c) which of the electron is having highest energy

Question 5. The total number of electrons that can be accommodated in all the orbitals having principal quantum number 3 azumuthal quantum number 1 is
a) 2
b) 4
c) 6
d) 8

Question 6. The principal quantum number of an atom represents
a. Spin Angular momentum
b.Size of the Orbital
c.Orbital Angular momentum
d. Space orientation of the orbital

 

Question 7. A p-orbital can accommodate
a. 4 electrons
b. 6 electrons
c.2 electron with opposite spins
d. 2 electron with parallel spins

 

Question 8. What are n,l,m values for electrons in below orbitals
a. 2px
b 4py
c. 3pz

Question 9. An electron is in one of the 3d orbitals. Give the possible values of n, l and ml for
this electron.

 

Question 10. Principal,azimuthal and magnetic quantum numbers are respectively related to
a. Size,shape and orientation
b.Shape,size and orientation
c.Size,orientation and shape
d.None of the above

 

 



Solutions

1.For n = 3, the possible values of l are 0, 1 and 2. Thus there is one 3s orbital (n = 3, l = 0 and ml = 0); there are three 3p orbitals (n = 3, l = 1 and ml = –1, 0, +1); there are five 3d orbitals (n = 3, l = 2 and ml = –2, –1, 0, +1+, +2). Therefore, the total number of orbitals is 1+3+5 = 9
The same value can also be obtained by using the relation; number of orbitals
= n2, i.e. 32 = 9.

2.
a) 2p
b) 4s
c) 5f
d) 3d
e) 1s
f) 4f

3. (e) (a) (c)

4.

a) 2 and 4 electron, 3rd and sixth electron
b) 5th electron
c) Ist electron

5. (c)

6. ( b)

7. (c)

8.a n=2, l=1 ,m=-1
b. n=2,l=1,m=0
c. n=3,l=1,m=1

9.

Principal quantum number (n) = 3

Azimuthal quantum number (l) = 2

Magnetic quantum number (ml) = – 2, – 1, 0, 1, 2

10.  (a)

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