U1-2-1 - Quantum Numbers and Atomic Orbitals

Question 1

Principal quantum number, n

Answer 1

Energy level the electron resides in

Question 2

Angular momentum quantum number, l

Answer 2

Defines the shape of a subshell (e.g. spherical)

Question 3

Quantum number l can take values __________.

Answer 3

from 0 to n – 1

Question 4

When l = 0, the subshell is marked with the letter __.

Answer 4

s

Question 5

When l = 1, the subshell is marked with the letter __.

Answer 5

p

Question 6

When l = 2, the subshell is marked with the letter __.

Answer 6

d

Question 7

When l = 3, the subshell is marked with the letter __.

Answer 7

f

Question 8

Subshells are further split into energy levels known as orbitals.

What is an orbital?

Answer 8

An orbital describes where an e⁻ is likely to be found around a nucleus.

Question 9

Each orbital can hold a maximum of _____ e⁻.

Answer 9

two

Question 10

Shape of s orbital

Answer 10

Spherical

Question 11

Shape of p orbital

Answer 11

Dumbbell/8

Question 12

Shape of d orbital

Answer 12

Two intersecting p orbitals

Question 13

Arrange the subshells in order of increasing energy:

d, s, f, p

Answer 13

s, p, d, f

Question 14

In an isolated atom, all orbitals in a subshell are degenerate. This means they are ___________.

Answer 14

of equal energy

Question 15

Magnetic quantum number, m_ℓ

Answer 15

Defines orbital orientation in space (e.g. along y axis, or xy plane)

Question 16

m_ℓ can have values __________.

Answer 16

from −ℓ to +ℓ

(e.g. if ℓ = 1, m_ℓ = −1, 0, +1)

Question 17

Number of s orbitals in an s subshell

Answer 17

1

(1 orientation possible for a sphere)

Question 18

Number of p orbitals in a p subshell

Answer 18

3

(along x, y and z axes)

Question 19

Number of d orbitals in a d subshell

Answer 19

5

Question 20

Spin magnetic quantum number, m_s

Answer 20

Describes electron spin (+1/2 or –1/2)