Drawing Orbitals: Chapter 12

Question 1

S orbital

Answer 1

Circle

Question 2

P-orbital

Answer 2

Dumbell

Question 3

D-orbital

Answer 3

Four-leaf clover

Question 4

How to calculate number of nodes?

Answer 4

nodes = n-1

Question 5

What do the subscripts of orbitals mean?

Answer 5

They signify the plane on which the orbital lies
dxy would be on the xy plane
dyz would be on the yz plane

Question 6

How does a squared subscript affect an orbital?

Answer 6

The lobes of the orbital lie on the axis (so the lobes would be on x,y,z = 0

Question 7

How do you draw an orbital without a squared subscript?

Answer 7

Diagonal to/off the axes

Question 8

What does the 3dz^2 orbital look like?

Answer 8

A p-orbital with the lobes lying on the z-axis, then a donut/hoola hoop surrounds those lobes on the xy axis

Question 9

What does the 3p(x,y,z) orbital look like?

Answer 9

A p-orbital with a normal angular node and a radial node circumscribed inside the orbital

Question 10

What does the 4d(x,y,z) orbital look like?

Answer 10

A d-orbital with two normal angular nodes and a radial node circumscribed inside the orbitals

Question 11

What is the lowest level each orbital can have?

Answer 11

1s
2p
3d
4f

Question 12

Pauli Exclusion Principle

Answer 12

No two electrons can have the same quantum numbers. This is the reason why orbitals can only hold two electrons, each of different spin (ms)

Question 13

Hund’s rule

Answer 13

Fill orbitals singly first

Electrons are filled in one to each orbital at first, then a second electron with opposite spin will be added once each orbital has been taken up