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chemistry a level > 4. inorganic chem and periodic table (as) > Flashcards

4. inorganic chem and periodic table (as) Flashcards

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1
Q

group two IE down group + reactivity

A

IE decreases down group
extra electron shell
inner shell shield outer e from attraction of nucleus
reduces electrostatic attraction between nucleus and outer e
easier to remove outer e
,, reactivity increases down group

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2
Q

group 2 reaction w water: metal + water

A

= metal hydroxide + hydrogen

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3
Q

group 2 metals burn in oxygen
metal burns in oxygen forms
metal + oxygen

A

solid white oxides formed

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4
Q

group 2 reacts with chlorine
metal + chlorine

A

forms solid white chlorides

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5
Q

oxides of group 2 metals react with water to form

A

metal hydroxides which dissolve the hydroxide ions make solutions strongly alkaline

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6
Q

what is an exception as a base as g1 and g2

A

magnesium oxide and beryllium oxide

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7
Q

oxides and hydroxides are

A

bases

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8
Q

because oxides and hydroxides are both bases they will

A

neutralise dilute acids forming salts

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9
Q

oxides as you go down the group

A

form more strongly alkaline solutions because hydroxides get more soluble

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10
Q

oxides reaction w water
MO + H2O

A

metal hydroxides formed
M(OH)2

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11
Q

oxides reaction with dilute acids
MO + 2HCl

A

form salt and water
MCl2 + H2O

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12
Q

hydroxides reaction with water
M(OH)2 + H2O

A

metal hydroxides
M(OH)2

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13
Q

hydroxide reaction w dilute acids
m(OH)2 + 2HCl

A

salt + water
MCl+ 2H2O

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14
Q

solubility trends depend on

A

compound anion

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15
Q

compounds of group 2 elects contain… and what does it do

A

singly charged negative ions
it increases in solubility down the group

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16
Q

compounds that contain doubly charged negative ions

A

decrease solubility down the group

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17
Q

hydroxides of group 2 elements and their solubility order

A

least soluble: magnesium hydroxide
calcium hydroxide
strontium hydroxide
most soluble: barium hydroxide

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18
Q

sulfates and their solubility of group 2 elements

A

most soluble: magnesium sulphate
calcium sulphate
strontium sulphate
least soluble: barium sulphate (insoluble)

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19
Q

thermal decomposition def

A

when a substance breaks down when heated

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20
Q

the more thermally stable a substance is …

A

the more heat it will take to break it down

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21
Q

carbonate and nitrates are large negative ions (anions) and can be unstable by

A

positively charged ions (cations) and they polarise the anion, and distorts it

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22
Q

the greater the distortion what happens to the compound

A

the less stable the compound

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23
Q

large cations cause

A

less distortion than small cations because they have lower charge density

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24
Q

charge density def

A

the areas covered by the charge of of an ion

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25
thermal stability down a group
thermal stability increases
26
what happens down a group and link to thermal stability
down the group the larger the cations ,, the lower the charge density ,, less distortion caused ,, more stable the carbonate and nitrate compound
27
group 2 compounds are what thermally stable than group 1 compounds
less thermally stable
28
explain the diff in g1 and g2 compounds and their thermal stability
g2 less thermally stable because greater charge greater distortion ,, less stable the compound g2 causes +2 charges ,, less stable
29
group 1 carbonates thermal stability
thermally stable- can’t make them decompose w a bunsen burner
30
group 1 nitrates thermal stability
decompose to form nitrogen and oxygen
31
group 2 carbonates thermal stability
decompose to from oxide and carbon dioxide
32
group 2 nitrates thermal stability
form oxide, nitrogen dioxide, and oxygen
33
how to test thermal stability of nitrates
.measure how long it takes until certain amount of oxygen produced . how long it takes until an amount of brown gas (nitrogen dioxide) produced but in a fume cupboard because it’s toxic
34
how to test carbonates
. how long it takes to produce carbon dioxide using limewater
35
lithium colour flame
red
36
sodium flame colour
yellow
37
potassium flame colour
lilac
38
rubidium flame colour
red
39
caesium flame colour
blue
40
calcium flame colour
brick red
41
strontium flame colour
crimson
42
barium flame colour
green
43
how to do a flame test
- mix small amount of compound w a few drops of HCl - heat a piece of nichrome/ platinum wire in a bunsen flame to clean it - dip wire into compound/ acid mixture - hold into flame + note colour produced
44
explanation of flame colour test
.energy absorbed from flame causes electron to move to higher energy levels . colours seen are electrons falling back down to lower energy levels releasing energy in form of light
45
fluorine colour + physical state at room temp
pale yellow gas
46
chlorine colour + physical state
green and gas
47
bromine colour and state
red brown and liquid
48
iodine colour and physical state
grey and solid
49
halogens solubility in water explained
low solubility in water because they’re non polar
50
chlorine colour in water and hexane
water- colourless hexane- colourless
51
bromine colour in water and hexane
water- yellow/orange hexane- orange/ red
52
iodine colour in water and hexane
water- brown hexane- pink/violet/purple
53
electronegativity down the halogens
decreases down the group
54
halogens reactivity down group explains
reactivity decreases . atoms is large down the group ,, outer e further from nucleus ,, more shielded ,, less electronegative ,, reactivity decreases
55
melting and boiling points down the halogens group
. increase down group increase electron shells ,, more electrons ,, more London forces are stronger between molecules more london forces ,, harder to overcome intermolecular forces ,, mp increases
56
displacement reactions def
a reaction wheee one element replaces another element in a compound
57
what ions can chlorine/ fluorine/ iodine displace
Cl: Br ion + I ion Br: I ion I:
58
displacement reaction between halogens and halides in a redox reactions
displaced element is oxidised and displacing element is reduced
59
potassium chloride solution reaction w chlorine water
no reaction
60
potassium chloride solution reaction with bromine water
no reaction
61
potassium chloride solution reaction with iodine solution
no reaction
62
potassium bromide reactions w chlorine water
bromine produced and chlorine ion produced
63
potassium bromide reaction w bromide water
no reaction
64
potassium bromide reaction w iodine water
no reaction
65
potassium iodide solution reaction with chlorine water
iodine atoms produced and chlorine ion
66
potassium iodide solution reaction w bromine water
bromide ion + iodine atom
67
potassium iodide solution reaction w iodine water
no reaction
68
if bromine formed then what colours formed
orange
69
if iodine formed what colour will be present
brown
70
when halogens reacts
they’re reduced
71
when halogens react with cold alkalis they
undergo disproptionation
72
what is produced when I2 + 2NaOH—>
(sodium iodate) NaOI + NaI + H2O
73
chlorine and sodium hydroxide reacts to produce
bleach
74
2NaOH (aq) + Cl2 (g) —>
(sodium chlorite) NaClO (aq) + NaCl (aq) + H2O (l)
75
when you mix chlorine w water ( cl2 + h2o) it produces
HCl+ HClO hydrochloric acid + hypochlorous acid hypochlorous acids ionises to make chlorate (I) ions that kill bacteria ,, adding chlorine to water makes water safe to drink
76
reducing power of halides down a group
increases down a group
77
KF/ KCl reaction with H2SO4 (sulphuric acid)
KHSO4 (s) + HF (g) KHSO4 + HCl
78
KBr + H2SO4
.—> KHSO4 (s) + HBr (g) . 2HBr (aq) + H2SO4 —> Br (g) ( orange fumes) + SO2 (g) + 2H2O
79
KI + H2SO4 —>
KI(s) + H2SO4 —> KHSO4 (s) + HI(g) 2HI (g) + H2SO4 —> I2 + SO2 (g) + 2H2O (l) 6HI(g) + h2so4 (g) —> s (s) + 3I2 (s) + 4H2O (l) 8hi + h2so4 arrow 4i2 + h2s + 4h2o h2s gas smells of rotten eggs
80
hydrogen halides are
acidic gases - colourless gasss
81
hydrogen halides can dissolve in water and produce
misty fumes of acidic gas ( turn damp litmus paper blue to red)
82
hydrogen chloride/ bromide / iodide forms
hydrochloric acid hydrobromic acid hudroiodic acid
83
hydrogen halides ( HCl) + ammonia gas ( NH3) react to produce + what type of reaction
NH4Cl ammonium chloride ( white fumes) acid base reaction
84
test for halides
- add dilute nitric acid - silver nitrate solution
85
colours of halides precipitate formed after
AgF- no peecipitate AgCl- white peecipitate AgBr- cream peecipitate AgI- yellow peecipitate
86
1 AgCl 2 AgBr 3 AgI reactions with dilute ammonia solution
1- precipitate dissolves in ammonia solution to give a colourless solution 2- precipitate remains unchanged if dilute ammonia solution added ,, colourless solution 3- peecipitate does not dissolve even in concentrates ammonia solution
87
carbonates test
- add dilute HCl ,, carbon dioxide produces run through limewater
88
sulfates test
- add dilute HCl - add barium chloride solution white peecipitate will be formed
89
test for ammonium compounds
- add sodium hydroxide and heat gently - use a damp red litmus paper will turn blue if ammonia present
90
why do we add concentrated HCl to metal compounds in flame tests
conc HCl would produc chlorides and this would increase volatility and ,, better colour produced
91
sulfate ions test + false positive
add nitric acid drops add barium chloride white precipitate formed nitric acid is used to neutralise solution if carbonates present to prevent a falsie positive

chemistry a level (20 decks)

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