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chemistry > topic 4 > Flashcards

topic 4 Flashcards

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1
Q

what happens to the atomic radius down a group and why

A

increases
extra shells added

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2
Q

what do all group 2 metals have at the end of electronic configuration

A

S2

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3
Q

what happens to ionisation energy down group 2 and why

A

decreases
more shielding
increase in protons overriden by sheilding

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4
Q

how do G2 react with water

A

form bases
metal hydroxides
Sr + H2O –> Sr(OH)2 + H2

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5
Q

what happens to reactivity with water down group 2 and why

A

increases
atoms get larger
more shielding

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6
Q

how does Mg react with cold water and steam

A

slowly with cold water

more vigorously with steam producing magnesium oxide

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7
Q

how do G2 react with oxygen using Mg as example

A

metal oxides

2Mg + O2 –> “MgO

Mg oxidised
O reduced

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8
Q

how does G2 react with chlorine using Mg as example

A

metal chlorides

Mg + Cl2 –> MgCl2

Mg oxidised
Cl2 reduced

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9
Q

how do G2 oxides react with water

A

form bases

SrO + H2O –> Sr(OH)2

more alkaline down group and hydroxides become more soluble

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10
Q

how do group 2 oxides react with HCl using calcium oxides as example

A

neuralisation

CaO+ 2HCl –> CaCl2 + H20

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11
Q

how do group 2 hydroxides react with HCl using calcium hydroxide as example

A

Ca(OH)2 + 2HCl –> CaCl2 + 2H2O

neutralisation

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12
Q

what happens to the solubility of G2 sulfates and G2 hydroxides down the group

A

sulfates SO4 2-
less soluble

hydroxides OH-
more soluble

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13
Q

how do G2 carbonates decompose using calcium carbonates as example

A

metal oxides + carbon dioxide

CaCO3 –> CaO + CO2

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14
Q

how do G2 nitrates decompose using calcium nitrate as an example

A

metal oxides + nitrogen dioxide + oxygen
2Ca(NO3)2 –> CaO + 4NO2 + O2

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15
Q

what is the trend in thermal stability down group 2 and why

A

more thermally stable down
lower charge density so less distortion

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16
Q

are G1 compounds more or less thermally stable than G2 and why

A

more

+1 charge so less distortion

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17
Q

do G1 carbonates decompose

A

no thermally stable except lithium
Li2CO3 –> Li2O + NO2 + O2

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18
Q

how do G1 nitrates decompose with lithium nitrate and potassium nitrate as examples

A

for nitrites and oxygen

LiNO3 –> Li2O + NO2 + O2
2KNO3 –> 2KNO2 + O2

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19
Q

how to measure thermal stability of nitrates

A

NO3 -
how long it takes for specific amount of O2
gas syringe or relight glowing splint

length of time for specific amount of NO2
brown toxic gas

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20
Q

how to measure thermal stability of carbonates

A

CO3 2-
length of time for specific volume of CO2
turns lime water cloudy
gas syringe

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21
Q

how to carry out a flame test

A
  1. dip nichrome wire in conc. hydrochloric acid
  2. dip into sample
  3. place loop into blue busen flame and observe colour change
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22
Q

why do you get different colours on the flame tests

A

electrons move to higher energy levels as they absorb energy from the flames
when they drop back down light is released
difference in energt levels determines wavelength of light energy released

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23
Q

what are the flame colours of lithium, sodium, potassium, rubidium, caesium, calcium, strontium, barium

A

lithium - crimson
sodium - yellow orange
potassium - lilac
rubidium - red
ceasium - blue
calciul - brick red
strontium - crimson
barium - green

24
Q

what happens to the boiling points of G7 down and why

A

increases
london forces increase
size increases
Mr increases

25
Q

what happens to the electronegativity down G7 and why

A

decreases down
larger atoms
distance from nucleus to bonding electrons increases
more sheilding

26
Q

what happens when potassium chloride solution reacts with chloride water, bromine water and iodine solution with colours of organic and aq

A

chloride water - no reaction
aq - colourless
org - colourless

bromine water - no reaction
aq - yellow
org - orange

iodine solution - no reaction
aq - brown
org - purple

27
Q

what happens when potassium bromide solution reacts with chloride water, bromine water and iodine solution with colours of organic and aq

A

chloride water -
Cl2 + 2Br- –> 2Cl- + Br2
aq - yellow
org - orange

bromine water - no reaction
aq - yellow
org - orange

iodine solution - no reaction
aq - brown
org - purple

28
Q

what happens when potassium iodide solution reacts with chloride water, bromine water and iodine solution with colours of organic and aq

A

chlorine water -
Cl2 + 2I- –> 2Cl- + I2
aq - brown
org - purple

bromine water
Br2 + 2I- –> 2Br- + I2
aq - brown
org - purple

iodine solution - no reaction
aq - brown
org - purple

29
Q

how does G7 react with group 1 and G2 with Cl2 as the example with Mg and Li

A

forms metal halides

Mg + Cl2 –> MgCl2

2Li + Cl2 –> 2LiCl

30
Q

what is the oxidation state of chloride/bromide

A

Cl-/Br-
-1

31
Q

what is the oxidation state of chlorine/bromine

A

Cl/Br
0

32
Q

what is the oxidation state of chlorate(I)

A

ClO-
+1

33
Q

what is the oxidation state of bromate(I)

A

BrO-
+1

34
Q

what is the oxidation state of bromate (III)

A

BrO2 -
+3

35
Q

what is oxidation state of iodate (V)

A

IO3 -
+5

36
Q

what is the oxidation state of iodate (VII)

A

IO4 -
+7

37
Q

how do halogens react with cold alkalis

A

X2 + 2NaOH –> NaOX + NaX + H20
0 –> +1 and -1

38
Q

how do halogens react with hot alkalis

A

3X2 + 6NaOH –> NaXO3 + 5NaX + 3H2O
0–>+5 and -1

39
Q

how is bleach made

A

chlorine + sodium hydroxide –> sodium chlorate (I)
Cl2 (g) + 2NaOH (aq) –> NaClO (aq) +NaCl (aq) +H2O (l)
disproportionation reaction

40
Q

what is bleach used for

A

treating water
bleaching paper and fabrics
cleaning agents

41
Q

what happens during water sterilisation

A

produces chlorate (I) ions which kill bacteria

H2O + Cl2 –><– HCl + HClO
HClO + H2O –><– ClO- + H3O+

42
Q

what happens to the reducing powerof halide ions down the group and why

A

increases down

increased ionic radius
more sheilding
decreased attractive force
outer electrons more readily lost

43
Q

how to test the reducing power of the halide ions

A

reaction with sulfuric acid
reaction with silver nitrate solution

44
Q

how does Cl- react with surfuric acid

A

H2SO4 + NaCl –> NaHSO4 + HCl
produces white misty fumes

45
Q

how does Br- react with sulfuric acid

A
  1. H2SO2 + NaBr –> NaHSO4 + HBr
    white misty fumes
  2. 2Br- –> Br2 +2e-
    orange vapour
    H2SO4 + 2H+ +2e- –> SO2 + 2H2O
    = H2SO4 + 2H+ + 2Br- –> Br2 + SO2 + 2H2O
46
Q

how does I- react with sulfuric acids

A
  1. H2SO4 + NaI –> NaHSO4 + HI
    white misty fumes
  2. 2I- –> I2 + 2e-
    organge vapour
    H2SO4 + 2H+ + 2e- –> SO2 + 2H2O
    = H2SO4 + 2H+ + 2I- –> I2 + SO2 + 2H2O
    1. 6I- –> 3I2 + 6e-
      H2SO4 + 6H+ + 6e- –> S + 4H2O
      yellow solid S
      = H2SO4 + 6H+ + 6I- –> 3I2 + S + 4H2O
  4. 8I- –> 4I2 + 8e-
    H2SO4 + 8H+ + 8e- –> H2S + 4H20
    rotton egg smell
    = H2SO4 + 8H+ + 8I- –> 4I2 + H2S + 4H2O
47
Q

what observation happens when hydrogen halides react with water in the air

A

form white misty fumes

48
Q

what observation happens when hydrogen halides react with amomonia gas

A

white fumes of ammonium halides

49
Q

what happens when iodide ions react with silver nitrate then ammounia

A

add dilute nirtic acid then silver nitrate

yellow precipitate

insoluble in all ammonia

50
Q

what happens when you react bromide ions with silver nitrate

A

add dilute nitric acid the silver nitrate

cream precipitate

dissolves in conc. ammonia

51
Q

what happens when you react silver nitare with chloride ions

A

add dilute nitric acid the silver nitrate

white precipitate

dissolves in dilute ammonia

52
Q

how to test for carbonates

A

HCl reacts to make CO2 gas which turns limewater cloudy

53
Q

how to test for sulfates

A

add HCl to remove carbonates
add barium chloride
white precipitate

54
Q

how to test for ammonium compounds

A

add NaOH and heat
damp red litmus paper turns blue

55
Q

how to test for hydroxides

A

turn red litmus paper blue

chemistry (15 decks)

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