Ch9.10

Question 1

What happens going down the group
In radius

Answer 1

The radius increases as there’s more shielding so further from nucleus so less nuclear attraction

Question 2

What happens going down the group
First ionization

Answer 2

It decreases

Less nuclear attraction as more shielding

Question 3

What happens going down the group in reactivity and MP

Answer 3

reactivity increases down the group and MP decreases down the group

Easier to lose electrons

And metal ions get bigger going down the group and the delocalised electrons are further apart so less attraction

So less energy to break bonds

Question 4

Joys is extraction of titanium work

Answer 4

Titanium ore is converted to titanium chloride by heating with carbon in a steam of chlorine gas

Then it’s purified by fractional distillation before being reduced by mg in a furnace at 1000 degrees

Question 5

How does CaO and CaCo3 remove sulphur dioxide

Answer 5

Removed by flue gases by reacting with an alkali this is wet scrubbing

Powdered CaO and calcium oxide can be both used

A slurry is made by mixing them with water and is then sprayed on flue gases

Sulfur dioxide reacts with alkaline slurry and produces waste product

Question 6

what are the colours and states of the halogen

Answer 6

fluorine is gas and it’s pale yellow

chlorine is gas and it’s green

bromine is liquid and it’s brownish red

iodine is grey and is solid

fluorine most electronegative

Question 7

how do electrognegativity and Bp work and reactivity going down the group for halogens

Answer 7

boiling points — increase down the group

cuz of increase in strength of VDW forces. as molecule increases

electronegativity — decreases down the group

there’s less nuclear attraction cuz electrons further from nucleus

reactivity — decreases down the group

because the halogens become less oxidising down the group

Question 8

how do you know what halogen is present in a solution (KCl)

Answer 8

chlroine — no reaction

bromine — no

iodine — no

Question 9

how do you know what halogen is present in a solution (KBr)

Answer 9

chlroine — orange solution (br2 formed)

bromine — no

iodine — no

Question 10

how do you know what halogen is present in a solution (KI)

Answer 10

chlroine — brown solution (I2 formed)

bromine — brown solution (I2 formed)

iodine — no reaction

Question 11

what’s the risk of using chlorine to treat water

Answer 11

chlorine gas is very harmful if breathed in — irritates respiratory system

liquid chlorine on eyes or skin causes severe chemical burns

chlroine reacts with other compounds in water to make chlorinated hydrocarbons which are carcinogenic

Question 12

what happens to the reducing powers of halides going down the group

Answer 12

it increases

ions are bigger so the electrons are further away from positive nucleus

more sheilds

it’s easier to lose electrons

Question 13

nitrate test colours on halogens

Answer 13

fluorine — no ppt

chlorine — white ppt

bromine — cream ppt

iodine — yellow ppt

Question 14

when adding ammonia to silver halide what happens

Answer 14

chlorine — dissolves in dilute NH3

bromine — dissolves in conc NH3

iodide — insoluble

Question 15

how to do flame test

Answer 15

dip nichrome wire loop in conc HCL

then dip wire loop into unknown compound

then hold loop in the clear blue flame of a bunsen burner

observe colour change

Question 16

what are the colours of metal ions

calcuum
strontium
barium

Answer 16

ca — brick red

Sr — red

barium — pale green

Question 17

what’s the ppt that comes out when adding drops of NaOH into a solution of a metal ion
in naOh and excess NaOH
Mg ca sr ba

Answer 17

mg — slight white ppt then white ppt

ca — slight white ppt then slight white ppt

sr — slight white ppt then slight white ppt

ba — no change

Question 18

how to test for ammonium ions

Answer 18

putting damp red litmus paper near ammonia gas it should turn blue

add hydroxide ions to a solution with ammonium ions they will react to produce ammonia gas and water

Question 19

how to test for sulphate

Answer 19

add a little dilute HCl followed by barium chloride solution

if white ppt or barium sulphate forms it means the original compound has sulphate in it

Question 20

how to test for hydroxides

Answer 20

by using a pH indicator

dip piece of red litmus paper into solution if hydroxide ions are present the paper will be blue

Question 21

how to test for carbonates

Answer 21

add dilute HCI to a solution with carbonate ions it present it will fizz
and give out CO2

test for CO2 using lime water if it turns cloudy then solution contains carbonate ions