Inornganic Chem + periodic table

Question 1

What colour does sodium turn in a flame test?

Answer 1

yellow-orange

Question 2

What colour does caesium turn in a flame test?

Answer 2

blue-violet

Question 3

What colour does potassium turn in a flame test?

Answer 3

lilac

Question 4

What colour does lithium turn in a flame test?

Answer 4

red

Question 5

What colour does rubidium turn in a flame test?

Answer 5

reddish-purple

Question 6

What colour does magnesium turn in a flame test?

Answer 6

intense white flame

Question 7

What colour does strontium turn in a flame test?

Answer 7

red

Question 8

What colour does calcium turn in a flame test?

Answer 8

orange-red

Question 9

What colour does barium turn in a flame test?

Answer 9

pale green

Question 10

What happens to the atomic radius as you go down group 2 and why?

Answer 10

atomic radius increases
each extra electron shell is further away

Question 11

what happens to ionisation energy as you go down group 2?

Answer 11

ionisation energy decreases
outer electrons are further away and experience less attraction to the nucleus

Question 12

what happens to melting point as you go down group 2?

Answer 12

melting point decreases
ion cores have larger radii down the group
free electrons experience less attraction to the nuclei because of the larger radii
bonding is weaker, so the melting point is lower

Question 13

whats formed when group 2 metals react with water

Answer 13

a metal hydroxide and hydrogen gas is produced
reactivity increases going down group 2 because lower elements have lower ionisation energies

(beryllium is an exception, if it were to lose 2 electrons it would be tiny and have a very high charge density, this would make it unstable and so beryllium doesnt react with water)

Question 14

what happens to the solubility of salts going down group 2?

Answer 14

solubility of hydroxides increases going down
solubility of sulfates decreases going down

Question 15

whats formed when group 2 metals react with acids?

Answer 15

salt and hydrogen gas
salts produced become less soluble as you go down the group

Question 16

whats formed when group 1 and group 2 carbonates undergo thermal decomposition?

Answer 16

metal oxide & carbon dioxide

Question 17

whats formed when group 1 and group 2 nitrates undergo thermal decomposition?

Answer 17

metal oxide, nitrogen dioxide & oxygen

Question 18

what happens to the thermal decomposition of group 1 and 2 carbonates & nitrates going down the group?

Answer 18

they get more stable as you go down the group
more energy is required for thermal decomposition to occur

Question 19

what is the charge density like on a smaller charged particle?

Answer 19

they have a greater charge density compared to a larger charged particle

Question 20

what happens to the charge density of the elements going down group 1 and 2?

Answer 20

the charge density gets lower as the size of the ions get bigger

Question 21

what affect does polarisation have on a carbonate ion or a nitrate ion?

Answer 21

the more polarised the ion is, the easier it is for it to decompose

Question 22

describe the reactions of group 2 oxides and water

Answer 22

group 2 oxides steadily react with water
the reaction produces a metal hydroxide salt. the salt dissociates into metal ions and hydroxide ions, giving the solution an alkaline pH

Question 23

describe group 2 solubility down the group

Answer 23

group 2 hydroxides become more soluble down the group so the solutions become more strongly alkaline down the group

Question 24

does beryllium oxide react with water?

Answer 24

NO

Question 25

does magnesium oxide react with water?

Answer 25

yes, but very slowly

Question 26

what phase is fluorine in?

Answer 26

gas

Question 27

what phase is chlorine in?

Answer 27

gas

Question 28

what phase is bromine in?

Answer 28

liquid

Question 29

what phase is iodine in?

Answer 29

solid

Question 30

what happens to electronegativity down group 7

Answer 30

decreases - atomic radius increases and so electrons experience less attraction to the nucleus electrons become further away from the nucleus and so experience a lower attraction

Question 31

what happens to boiling point going down group 7

Answer 31

increases elements have more electron going down group 7 this causes an increase in LDF, stronger LDF means greater intermolecular forces

Question 32

which of the halogens is the most oxidising agent?

Answer 32

fluorine as it is the most electronegative

Question 33

what happens if an elemental halogen is added to a halide solution?

Answer 33

the heavier halide will be displaced this is because the lighter halide has a greater preference to be the halide ion as its more electronegative

Question 34

describe halide reactions with sulfuric acis

Answer 34

halides react differently with sulfuric acid depending on the reducing ability

Question 35

what colour precipitate do chloride ions and silver nitrate form

Answer 35

white

Question 36

what colour precipitate do bromide ions and silver nitrate form?

Answer 36

cream

Question 37

what colour precipitate do iodide ions and silver nitrate form

Answer 37

yellow

Question 38

what happens when silver chloride is added to ammonia

Answer 38

silver chloride should redissolve

Question 39

what happens when silver bromide is added to ammonia

Answer 39

silver bromide should redissolve slowly and will need a lot of ammonia

Question 40

what happens when silver iodide is added to ammonia

Answer 40

silver bromide should not dissolve

Question 41

whats formed when fluoride reacts with sulfuric acid

Answer 41

produces HF

Question 42

whats formed when chloride reacts with sulfuric acid

Answer 42

produces HCl

Question 43

whats formed when bromide reacts with sulfuric acid

Answer 43

produces Br2 and some SO2

Question 44

whats formed when iodide reacts with sulfuric acid

Answer 44

produces I2 immediately and then will reduce the sulfur to H2S

Question 45

whats formed when chlorine reacts with water

Answer 45

HCl + HClO then can go to: 2H + ClO- + Cl- this reaction is used in water treatment to kill bacteria

Question 46

what happens when chlorine reacts with water in sunlight

Answer 46

the chlorate ion produced will decompose to produce hydrochloric acid and oxygen

Question 47

what are the risks of adding chlorine to water

Answer 47

chlorine gas is toxic liquid chlorine that touches eye or skin will burn chlorine may react with organic compounds and form carcinogenic hydrocarbons

Question 48

how is bleach made?

Answer 48

by adding chlorine to sodium hydroxide

Question 49

describe how you would test for carbonates

Answer 49

hydrochloric acid reacts with carbonates and hydrogencarbonates to make carbon dioxide gas when bubbled through limewater it turns cloudy

Question 50

describe how you would test for sulfates

Answer 50

add hydrochloric acid to remove any carbonates in. these could precipitate out after adding barium chloride giving a false result add barium chloride you will observe a white precipitate if there are sulfates

Question 51

describe how you would test for ammonium compounds

Answer 51

add sodium hydroxide, gently heat, and if the ammonium compound is present ammonia gas will be produced use damp red litmus. ammonia will dissolve in the water and turn litmus blue

Question 52

describe how you would test for hydroxides

Answer 52

hydroxides are alkaline and they will turn red litmus blue

Question 53

describe how you would test for the thermal stability of nitrates

Answer 53

measure how long it take a specific amount of oxygen is produced. using a gas syringe or the amount needed to relight a glowing splint the length of time it takes until a specific amount of nitrogen dioxide is produced. nitrogen dioxide is a brown gas so is easily observed. it is TOXIC though so must be done in a fume cupboard

Question 54

give the oxidation state of a chloride ion

Answer 54

-1

Question 55

give the oxidation state of chlorine

Answer 55

0

Question 56

give the oxidation state of a chlorate(I) ion

Answer 56

+1

Question 57

give the oxidation state of a bromate(I) ion

Answer 57

+1

Question 58

give the oxidation state of a bromate(III) ion

Answer 58

+3

Question 59

give the oxidation state of a iodate(V) ion

Answer 59

+5

Question 60

give the oxidation state of a iodate(VII) ion

Answer 60

+7

Question 61

give the equation of how bleach is made

Answer 61

2NaOH(aq) + Cl2(g) --> NaClO(aq) + NaCl(aq) + H2O(l)