Orbital Theory: Electron Quantum Numbers

Question 1

Shells (n) - Orbital number(n²) Define

Answer 1

For any shell with a Quantum number “n”, there will be an “n²” number of Orbitals

SQUARES (region within an atom containing 2 electrons with opposite spins)

Work out n= 1,2,3,4 Think about the electron config

Question 2

Principal Quantum Number (n)

Answer 2

is Orbital size/ Shell number (which period on the periodic table).

Small n values imply lower energy orbitals
- How far away an electron is from the Nucleus

Restriction of values: n ≥ 1 (whole numbers/ integers)

Question 3

Orbital Angular Quantum Number (ℓ )

Answer 3

is Orbital Type/Shape. ℓ = (n-1)

s orbitals have NO Angular Component/ Only radial

Restriction of values: ℓ ≥ 0

s orbitals - ℓ = 0
p orbitals - ℓ = 1
d orbitals - ℓ = 2
f orbitals - ℓ = 3

Question 4

Magnetic Quantum Number (mℓ)

ℓ is slightly lower

Answer 4

is the orientation in space ????? (HELP)
it is the Directional Component the orbital has

Direction of Orbital (xyz)

e.g. px Orbital points towards the x axis

Restriction of values: All numbers Positive or Negative

p orbital - mℓ = +1, 0 ,-1
p(x, y , z)

d orbital - mℓ = +2, +1, 0, -1, -2
d(x²-y², xz, z², yz, xy)

f orbital - mℓ = +3,+2,+1, 0 ,-1,-2,-3

Draw / Visualize the Shapes of “p and d” orbitals

Question 5

Spin Quantum Number (ms)

s is slightly lower

Answer 5

is the Spin of an electron

Clockwise = +½

Anticlockwise = -½