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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

Study These Flashcards
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

Study These Flashcards
A

increases
london forces increase
size increases
Mr increases

25
what happens to the electronegativity down G7 and why
decreases down larger atoms distance from nucleus to bonding electrons increases more sheilding
26
what happens when potassium chloride solution reacts with chloride water, bromine water and iodine solution with colours of organic and aq
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
what happens when potassium bromide solution reacts with chloride water, bromine water and iodine solution with colours of organic and aq
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
what happens when potassium iodide solution reacts with chloride water, bromine water and iodine solution with colours of organic and aq
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
how does G7 react with group 1 and G2 with Cl2 as the example with Mg and Li
forms metal halides Mg + Cl2 --> MgCl2 2Li + Cl2 --> 2LiCl
30
what is the oxidation state of chloride/bromide
Cl-/Br- -1
31
what is the oxidation state of chlorine/bromine
Cl/Br 0
32
what is the oxidation state of chlorate(I)
ClO- +1
33
what is the oxidation state of bromate(I)
BrO- +1
34
what is the oxidation state of bromate (III)
BrO2 - +3
35
what is oxidation state of iodate (V)
IO3 - +5
36
what is the oxidation state of iodate (VII)
IO4 - +7
37
how do halogens react with cold alkalis
X2 + 2NaOH --> NaOX + NaX + H20 0 --> +1 and -1
38
how do halogens react with hot alkalis
3X2 + 6NaOH --> NaXO3 + 5NaX + 3H2O 0-->+5 and -1
39
how is bleach made
chlorine + sodium hydroxide --> sodium chlorate (I) Cl2 (g) + 2NaOH (aq) --> NaClO (aq) +NaCl (aq) +H2O (l) disproportionation reaction
40
what is bleach used for
treating water bleaching paper and fabrics cleaning agents
41
what happens during water sterilisation
produces chlorate (I) ions which kill bacteria H2O + Cl2 --><-- HCl + HClO HClO + H2O --><-- ClO- + H3O+
42
what happens to the reducing powerof halide ions down the group and why
increases down increased ionic radius more sheilding decreased attractive force outer electrons more readily lost
43
how to test the reducing power of the halide ions
reaction with sulfuric acid reaction with silver nitrate solution
44
how does Cl- react with surfuric acid
H2SO4 + NaCl --> NaHSO4 + HCl produces white misty fumes
45
how does Br- react with sulfuric acid
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
how does I- react with sulfuric acids
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 3. 3. 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
what observation happens when hydrogen halides react with water in the air
form white misty fumes
48
what observation happens when hydrogen halides react with amomonia gas
white fumes of ammonium halides
49
what happens when iodide ions react with silver nitrate then ammounia
add dilute nirtic acid then silver nitrate yellow precipitate insoluble in all ammonia
50
what happens when you react bromide ions with silver nitrate
add dilute nitric acid the silver nitrate cream precipitate dissolves in conc. ammonia
51
what happens when you react silver nitare with chloride ions
add dilute nitric acid the silver nitrate white precipitate dissolves in dilute ammonia
52
how to test for carbonates
HCl reacts to make CO2 gas which turns limewater cloudy
53
how to test for sulfates
add HCl to remove carbonates add barium chloride white precipitate
54
how to test for ammonium compounds
add NaOH and heat damp red litmus paper turns blue
55
how to test for hydroxides
turn red litmus paper blue

chemistry (15 decks)

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