group 1

Question 1

What happens to size down group 1

Answer 1

Increases down group as electrons in shells further from the nucleus

Question 2

What happens to reactivity down group 1?

Answer 2

Increases as ionisation energy decreases

Question 3

What is the bonding like in group 1?

Answer 3

Metallic bonding, they aren’t very electronegative

Question 4

What happens to basicity in group 1 hydroxides down the group?

Answer 4

Basicity increases down the group because increased metallic character (down group atoms aren’t as electronegative)

Question 5

Are group 1 hydroxides Acidic or Basic?

Answer 5

Basic

Question 6

What is the bonding between group 1 and the oxides?

Answer 6

strong Ionic lattice. smaller ions can get closer together and therefore have really strong bonds

Question 7

Why do larger group 1 cations usually form superoxides and not stronger ionic lattices with smaller anions?

Answer 7

The ionic lattices with large ions are weaker and therefore it isn’t favourable for the peroxide to undergo an energy cost reaction into a smaller oxide.

Question 8

N2 is a very stable gas, but it reacts with Li, none of the other group 1 metals do this, why?

Answer 8

Lithium can become such a small densely charged cation which can form a really strong ionic lattice making the energy cost of breaking the N2 bond favourable

Question 9

Why does only Li react with N2 and not the other group 1 atoms?

Answer 9

They are too big, the ionic lattice would not be favourable and wouldn’t offset the energy used to break the N2 bond

Question 10

Why is Li similar to Mg

Answer 10

The diagonal relationship, they both have very high charge density small cations

Question 11

What bonding is in group 1 hydrides?

Answer 11

Ionic lattices as a big difference in electronegativity, group 1 electropositive

Question 12

As metal ions get bigger down group one what happens to the ionic lattice?

Answer 12

Gets weaker as the ions are further apart from each other, therefor the thermal stability is also weaker.

Question 13

What bonds are in the group 1 halides?

Answer 13

Ionic as big electronegativity difference. Strength is greatest between smallest ions

Question 14

What is this O^2- called?

Answer 14

Oxide

Question 15

What is O2^2- called?

Answer 15

Peroxide

Question 16

what is O2- called?

Answer 16

Superoxide

Question 17

Products of group 1 metals with oxygen are?

Answer 17

Basic

Question 18

What structure does Na form with halides?

Answer 18

Rocksalt crystal structure

Question 19

Why is solubility of group 1 halides complex?

Answer 19

There are two competing factors, hydration enthalpy and lattice enthalpy. As the halide ion gets bigger the dominant factor changes from lattice energy to hydration enthalpy.

Question 20

For group 1 halides why does the dominant solubility factor shift from lattice energy to hydration enthalpy as the halide ion gets bigger?

Answer 20

As the ion gets bigger it cant overlap as well with the group 1 elements, therefore the lattice enthalpy isn’t as high. This weak lattice energy doesn’t change much with the cation size if anion is small so hydration becomes dominant factor

Question 21

What happens to the solubility of group 1 halides if the anion is large?

Answer 21

Decreases down the group 1. As hydration enthalpy is the dominant factor over lattice enthalpy. Hydration E decreases as cation gets bigger it is less favourable to hydrate.

Question 22

What happens to the solubility of group 1 halides if the anion is small?

Answer 22

Increases down group 1. Small anion means the lattice energy could be strong, as the cation gets bigger this energy rapidly decreases meaning it can get broken easier.