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OCR H032 AS Chemistry > Orbitals > Flashcards

Flashcards in Orbitals Deck (16)
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1
Q

What are the different types of orbitals

A

S p d f

2
Q

What shape is an s orbital

A

⚪️

3
Q

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

A

2

4
Q

What shape are p orbitals

A

5
Q

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

A

6

6
Q

How many electrons can a d orbital hold

A

10

7
Q

How many orbitals can an f orbital hold

A

14

8
Q

Which block are the transition metals in

A

D

9
Q

Which block are the noble gases in

A

P

10
Q

What 3 factors affect ionisation energy

A

Atomic radius
Nuclear charge
Electron shielding

11
Q

How would you write the second ionisation energy for helium

A

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

12
Q

What happens to ionisation energy down a group

A

Sharp decrease

13
Q

What happens to ionisation energy across a period

A

Increase

14
Q

How do you work out mean atomic number

A

Abundancy / 100

X relative atomic mass

15
Q

Why is each successive ionisation energy greater than the last

A

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

16
Q

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

A

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