Orbitals

Question 1

What are the different types of orbitals

Answer 1

S p d f

Question 2

What shape is an s orbital

Answer 2

⚪️

Question 3

What is the maximum number of electrons can an s orbital hold

Answer 3

2

Question 4

What shape are p orbitals

Answer 4

⏳

Question 5

What is the maximum number of electrons a p orbital can hold

Answer 5

6

Question 6

How many electrons can a d orbital hold

Answer 6

10

Question 7

How many orbitals can an f orbital hold

Answer 7

14

Question 8

Which block are the transition metals in

Answer 8

D

Question 9

Which block are the noble gases in

Answer 9

P

Question 10

What 3 factors affect ionisation energy

Answer 10

Atomic radius
Nuclear charge
Electron shielding

Question 11

How would you write the second ionisation energy for helium

Answer 11

He+ (g) -> He2+ + e-

Question 12

What happens to ionisation energy down a group

Answer 12

Sharp decrease

Question 13

What happens to ionisation energy across a period

Answer 13

Increase

Question 14

How do you work out mean atomic number

Answer 14

Abundancy / 100

X relative atomic mass

Question 15

Why is each successive ionisation energy greater than the last

Answer 15

As each e- is removed there is less repulsion between electrons
Each shell is drawn in tighter to the nucleus
As distance decreases, nuclear attraction increases
Therefore more energy is required to remove each successive electron

Question 16

Why does ionisation energy decrease down a group as they have:

Answer 16

A greater atomic radius, each element has more electron shells, so outer e- is further from the nucleus
More electron shielding, more full electron shells between the outer electron and nucleus
More protons in the nucleus, but also more electrons. Lower electrostatic attraction to the nucleus due to less effective nuclear charge