Reactivity Series

Question 1

Explain why rubidium is more reactive than potassium

Answer 1

Rubidium is further down group 1 so reactivity increases

There is more electrons or atoms gets larger

Attraction between outer electrons and positive nucleus gets weaker

Easier to lose outer electrons

Question 2

Explain the trend in boiling points of halogens as you go down group 7

Answer 2

As u go down, boiling point increases

Gets more reactive as there is more shells

Attraction between nucleus and outer electrons is stronger

Harder to lose electrons and more energy needed to break attraction

Question 3

Explain one observation you would see that shows rubidium is more reactive than potassium

Answer 3

It will float

It will fizz

It will be more vigorous

Lights in flame

Question 4

Explain how metals conduct electricity

Answer 4

Metals have delocalised electrons

Carries a charge

Free to move through the structure

Question 5

Iodine is group 7, why does liquid iodine not conduct electricity

Answer 5

Iodine has no delocalisation electrons

Have no ions

Can’t carry a charge

Question 6

Describe the trend in reactivity of group 7

Answer 6

The further down, the less reactive

Elements at top have few electron shells

So have strong attraction

Electrons gained more easily

Question 7

Explain why Caesium is more reactive than sodium.

Answer 7

Caesium has more energy levels or shells as it’s further down

So outer electron is further from nucleus

There is weaker attraction between outer electron and nucleus

Outer electron more easily lost

Question 8

Explain the trend in boiling point in group 7

Answer 8

Molecules Get larger going down the group

Intermolecular forces increase

Therefore boiling points increase going down

Question 9

Why are boiling points low in group 7

Answer 9

Weak forces between molecules

Weak intermolecular forces

Little energy needed to break forces