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Alevel > topic 4 > Flashcards

topic 4 Flashcards

1
Q

flame test procedure

A

place nichrome wire in conc HCL
place wire in roaring bunsen flame
place wire in sample then back into flame
observe colour

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2
Q

Li+

A

bright red

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3
Q

Na +

A

bright yellow

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4
Q

k+

A

lilac

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5
Q

Be 2+

A

no colour

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6
Q

mg2+

A

colourless

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7
Q

ca 2+

A

brick red

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8
Q

sr 2+

A

bright red

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9
Q

ba 2+

A

pale green

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10
Q

what could cause yello contamination

A

Na + presence

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11
Q

what causes colour

A

e excited to higher energy level

e relaxes back to lower energy level, emitting photon of light whose energy is equal to the energy difference between the shells e has moved from

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12
Q

thermal decomposition

A

breaking down using heat = lot of energy required to break strong bond between atoms

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13
Q

group 1 hydroxide solubility

A

soluble

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14
Q

group 1 sulfate solubility

A

soluble

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15
Q

group 1 nitrate solubility

A

soluble

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16
Q

group 1 carbonate solubility

A

soluble

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17
Q

group 2 hydroxide solubility

A

solubility increases down group

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18
Q

group 2 sulfate solubility

A

solubility decreases down group

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19
Q

group 2 nitrate solubility

A

soluble

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20
Q

group 2 carbonate solubility

A

insoluble

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21
Q

which chloride aren’t soluble

A

silver and lead chloride

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22
Q

which sulfates arent soluble

A

barium and lead sulfates

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23
Q

reactivity trend in group 2

A

reactivity increases down group

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24
Q

barium plus water observation

A

lots of bubbles

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25
Mg plus water observation
nothing much occurs
26
calcium oxide plus water
CaO plus H2O -----> Ca(OH)2
27
why dont BeO and MgO react with water well
BeO is insoluble and | MgO isnt very soluble
28
Group 1 nitrates decomposition
partially decompose to form metal nitrate plus oxygen exception lithium undergoes complete decomposition to form lithium oxide (white solid), NO2 (red brown gas) and oxygen
29
group1 carbonates decomposition
do not decompose except lithium carbonate to give lithium oxide plus CO2
30
group 2 nitrates
all nitrates fully decompose to form metal oxide, NO2 and oxygen becomes harder to decompose down group = more thermally stable
31
group 2 carbonates
decompose to form metal oxide and CO2
32
measuring rates of decomposition
change in mass colorimetry gas formation
33
positives and negatives of change in mass
+ = accuate measurements, mass balance to 2 d.p - = non continuous measurement and toxic no2 produced, skin eye burns, fatal if inhaled
34
positives and negatives of colorimetry
+ = continous monitoring - = product is involved in furhter reaction (2NO2 ----> N2O4)
35
positives and negatives of gas formation
+ = continous monitoring, toxic No2 captured - = potential for NaOH solution to be drawn back into test tube after heating = pressure difference so glass could break
36
comparing MgCO3 and SrCO3 decomposition
Mg 2+ has higher charge density than sr2+ Mg 2+ strongly polarises the carbonate ion more than the sr2+ so the Mg- O bond is strengthened results in the C- O bond weakening less energy required to break C- O bond so less energy to decompose MgCO3
37
group 7 MP trend and why
increases down group due to increased london forces as the molecules get larger
38
group 7 electronegativity trend and why
decrease as you go down the group due to increased shielding and atomic radius so weaker attraction to bonded electrons
39
Fluorine
pale yellow gas
40
chlorine
pale green gas
41
bromine
brown/red liquid
42
iodine
grey solid | violet vapour
43
astatine
black solid
44
colour of chlorine dissolved in water
pale green
45
colour of bromine dissolved in water
orange
46
colour of iodine dissolved in water
brown
47
colour of chlorine dissolved in organic solvent
pale green
48
colour of bromine dissolved in organic solvent
orange
49
colour of iodine dissolved in organic solvent
purple
50
Cl2 plus Br- ---->? colour change
orange solution produced
51
Cl2 plus I- ---->? colour change
brown solution produced
52
Br2 plus I- ------>? colour change
brown solution produced
53
oxidising agent strength trend group 7
decreases down group chlorine strongest oxidising agent as it has smallest atomic radius and less shielding so able to attract incoming e more easily
54
reducing agent strength (donates e) trend
reducing agent strength increases down group as atomic radius get larger and increased shielding means there's less attraction between valence e and nucleus so electrons lost more easily
55
test for halides procedure and results
dissolve sample add nitric acid to remove carbonates add silver nitrate (silver complex ions) cl- white ppt br- cream ppt I- yellow ppt
56
how to test ppt from above
AgCl dissolves in dilute and conc NH3 AgBr dissolves in conc NH3 but not in Dilute NH3 AgI doesn't dissolve in either dilute or conc NH3
57
chlorine plus water
Cl2 (g) + H2O ----> HClO (aq) + HCl (aq)
58
chlorine plus cold KOH
Cl2 (g) + 2KOH (aq) ------> KClO (aq) + KCl (aq) +H2O
59
chlorine plus hot KOH
3Cl2 (g) + 6KOH (aq) ------> KClO3 (aq) + 5KCl +5H20
60
HBr + NH3 ----->
HBr + NH3 -----> NH4Br
61
HBr +H20 ----->
HBr +H20 -----> H3O+ + Br-
62
metal plus halogen procedure
in fume hood so cl2 doesnt escape iron is in wool not in blocks to increase surface area iron heated to increase rate of reaction halogen vapour is dry otherwise cl2 reacts with H20 to form acidic gas excess gas allowed to escape so no pressure build up
63
does iodine with fe2+ ion
no bc iodine isnt strong enough oxidisng agent
64
Cl2 + H2 ----->
Cl2 + H2 -----> 2HCl violent reaction
65
Br2 plus H2
creates HBr react with calm pale blue flame
66
iodine plus hydrogen
produces HI and reaction is reversible
67
H2SO4 + NaBr ----->
H2SO4 + NaBr -----> Br2 (g) + SO2 (g) + H2O (g) br2 is orange and so2 is acidic choking
68
H2SO4 + NaI ---->
H2SO4 + 6NaI ----> 3 I2(s) + 2 H2O (s) + H2S(g) +NaHSO4 i2 is grey solid s is yellow solid and H2s has egg smell
69
H2SO4 + NaCl ---->
H2SO4 + NaCl ----> HCl + NaHSO4
70
test for carbonate ions
disslove carbonate add hcl to solution bubble gas through limewater if carbonate present - limewater turns cloudy
71
equation for test carbonate
CO3- + H+ -------> H20 + C02
72
test for sulphate ions
disslove compound and add dilute HCl to remove carbonate ions add few drops of barium chloride if sulphate ion present - white ppt of barium sulfate forms
73
equation for testing of sulphate ions
SO42- + Ba2+ ----> BaSO4(s)
74
testing for NH4+ ions
dissolve NH4+ add dilute NaOH heat gently IF ion present damp red litmus paper turns blue

Alevel (30 decks)

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