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A2 Chem > Inorganic > Flashcards

Inorganic Flashcards

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1
Q

trend of 1st ionisation energy across period 3

A

generally requires more energy
increase in nuclear charge
atoms become smaller so closer distance
same shielding

2->3 decrease as p orbital is higher in energy than s
5->6 decrease as extra electron-electron repulsion means less energy required to remove electron from p4 than p3

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2
Q

trend of electronegativies across period 3

A

increases

increase nuclear charge, smaller atomic radius, same shielding

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3
Q

Na + H2O

A

floats, moves and fizzes with water

2Na + H2O -> 2NaOH + H2

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4
Q

Mg + H2O

A

in cold water very slow reaction
in water water it forms a white precipitate Mg(s) + 2H2O(l) -> Mg(OH)2(s) + H2(g)
in steam it burns with a white flame and forms a white powder
Mg + H2O -> MgO + H2

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5
Q

Al + H2O

A

do not react with water as they are non-polar molecules so no interactions

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6
Q

Si + H2O

A

do not react with water as they are non-polar molecules so no interactions

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7
Q

P4 + H2O

A

do not react with water as they are non-polar molecules so no interactions

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8
Q

S8 + H2O

A

do not react with water as they are non-polar molecules so no interactions

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9
Q

Cl2 + H2O

A

dissolves to give a pale green colour

Cl2 + H2O ↔ HCl + HClO (chloric acid)

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10
Q

Na + O2

A

yellow flame
white powder
4Na + O2 -> Na2O (s)

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11
Q

Mg + O2

A

bright white flame
white powder
2Mg + O2 -> 2MgO (s)

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12
Q

Al + O2

A

oxide layer with air prevents further reaction with air
when pure: white flame
white powder
4Al + 3O2 -> 2Al2O3 (s)

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13
Q

Si + O2

A

unable to ignite alone: white flame
slowly form a white powder
Si + O2 -> SiO2 (s)

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14
Q

P4 + O2

A

spontaneously flammable: bright white flame
white powder
P4 + 5O2 -> P4O10 (s)

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15
Q

S8 + O2

A

blue flame
acidic colourless choking gas
S + O2 -> SO2 (g)

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16
Q

Na2O + H2O

A

dissolves and reacts vigorous exothermic reaction
pH 14
Na2O + H2O -> 2NaOH

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17
Q

MgO + H2O

A

slightly soluble as ionic bonding is strongest
pH 10
MgO + H2O -> Mg(OH)2

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18
Q

Al2O3 + H2O

A

insoluble as not enough interaction and high ionic lattice enthalpy
pH7

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19
Q

SiO2 + H2O

A

insoluble as macromolecular structure consisting of strong covalent bonds
pH 7

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20
Q

P4O10 + H2O

A

big simple molecule so reacts violently, vigorous exothermic reaction
pH 0
P4O10 + 6H2O -> 4H3PO4
H2O releases H+ when attached to δ+ P atoms

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21
Q

SO2 + H2O

A

dissolves and then reacts
pH 3
SO2 + H2O -> H2SO3
H2O releases H+ when attached to δ+ S atoms

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22
Q

SO3 + H2O

A

reacts violently
pH 0
SO3 + H2O -> H2SO4
H2O releases H+ when attached to δ+ S atoms

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23
Q

uses of magnesium

Study These Flashcards
A

Extract titanium from the ore rutile (TiO2)
TiO2 +2C + 2Cl2 -> TiCl4 + 2CO
TiCl4 + 2Mg -> Ti + 2MgCl2

24
Q

uses of magnesium hydroxide

Study These Flashcards
A

milk of magnesia (Mg(OH)2) taken for indigestion

25
uses of calcium hydroxide
Slaked lime (Ca(OH)2) is alkaline so can neutralise acidity (raise pH) in soil Limewater is used to test for presence of CO2 Ca(OH)2(aq) + CO2(g) -> CaCO3(s) + H2O(l)
26
uses of calcium oxide
CaO removes SO2 in flue gas by desulphurisation | CaO + SO2 -> CaSO3 (calcium sulphite)
27
uses of calcium carbonate
CaCO3 also removes SO2 in flue gas by desulphurisation 2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2 Limestone used as a building material
28
uses of barium sulphate
``` Barium meal (BaSO4) allows soft tissue to be seen through X-rays as it is insoluble Toxic but insoluble so body does not absorb ```
29
uses of acidified barium chloride
Used to test for sulphate ions (produce BaSO4 white precipitate) Must be acidified to remove any other ions which could give a precipitate with BaCl2 E.g. BaCl2 + NaHCO3 -> BaCO3 + NaCl + HCl
30
strongest to weakest halogen oxidising agent
Strongest green Cl2 > yellow Br2 > brown I2 Weakest
31
displacement reaction Cl2 + Br-
Cl2 + 2Br- -> 2Cl- + Br2 | forms yellow solution
32
displacement reaction Cl2 + I-
Cl2 + 2I- -> 2Cl- + I2 | forms brown solution
33
displacement reaction Br2 + Cl-
no reaction, remains yellow solution
34
displacement reaction Br2 + I-
Br2 + 2I- -> 2Br- + I2 | forms brown solution
35
displacement reaction I2 + Cl-
no reaction, remains brown solution
36
displacement reaction I2 + Br-
no reaction, remains brown solution
37
strongest to weakest halide reducing agent
Strongest I- > Br- > Cl- Weakest
38
NaCl + c.H2SO4
NaCl + c.H2SO4 -> NAHSO4 + HCl | Acid-base (displacement), steamy fumes (HCl)
39
NaBr + c.H2SO4
NaBr + c.H2SO4 -> NAHSO4 + HBr Acid-base (displacement), steamy fumes (HBr) 2Br- + H2SO4 + 2H+ -> Br2 + SO2 + 2H2O Redox: Oxidation of Br- to brown fumes (Br2) and Reduction of H2SO4 to colourless gas (SO2)
40
NaI + c.H2SO4
NaI + c.H2SO4 -> NAHSO4 + HI Acid-base (displacement), steamy fumes (HI) 2I- + H2SO4 + 2H+ -> I2 + SO2 + 2H2O Redox: Oxidation of I- to purple fumes (I2) and Reduction of H2SO4 to colourless gas (SO2) 6I- + H2SO4 + 6H+ -> 3I2 + S + 4H2O Reduction of H2SO4 to yellow solid (S) 8I- + H2SO4 + 8H+ -> 4I2 + H2S + 4H2O Reduction of H2SO4 to bad smell from gas (H2S)
41
Cl2 + H2O in bright light
2Cl2 + 2H2O -> 4H+ + 4Cl- + O2
42
chlorine and cold dilute NaOH
Cl2(aq) + 2NaOH(aq) -> NaCl(aq) + NaClO(aq) + H2O(l)
43
transition metals
elements with an incomplete d sub-shell in its atom or ion
44
why is zinc classed as a d block element but not a transition metal
Outer electrons are in 3d sub-shell | Doesn’t have incomplete d sub-shell either in elemental or ionic form
45
ligand
central ion linked to a number of molecules/ ions called ligands by donating a lone pair of electrons
46
example of heterogenous catalyst
V2O5 in Contact process to produce H2SO4 Overall: SO2 + ½O2 -> SO3 V2O5 + SO2 -> V2O4 + SO3 V2O4 + ½O2 -> V2O5
47
catalysts adsorb the reactant onto the surface and held in place by weak bonds
Adsorption of reactant on its surface increases concentration so increases likelihood to collide with second reactant Weaken bonds in the reactant so decreases activation energy Adsorption causes reactant molecule to break up into more reactive fragments so decreases activation energy
48
example of homogenous catalyst
Reaction between iodide and persulphate ions catalysed by Fe2+ Overall: S2O82- + 2I- -> 2SO42- + I2 S2O82- + 2Fe2+ -> 2SO42- + 2Fe3+ oxidised 2I- + 2Fe3+ -> I2 + 2Fe2+ reduced
49
why are transition metals good catalysts
variable oxidation states and partially filled d-subshells so able to accept and donate electrons easily
50
example of autocatalysis
reaction between ethanedioate ions and manganite (VII) ions catalysed by Mn2+ overall: 2MnO4- + 16H+ + 5C2O42- -> 2Mn2+ + 10CO2 + 8H2O alternative catalysed route 4Mn2+ + MnO4- + 8H+ -> 5Mn3+ + 4H2O 2Mn3+ + C2O42- -> 2Mn2+ + 2CO2
51
Na2O + acid/ alkali
acids | Na2O + 2H+ -> 2Na+ + H2O
52
MgO + acid/ alkali
acids | MgO + 2H+ -> Mg2+ + 3H2O
53
Al2O3 + acid/ alkali
amphoteric Al2O3 + 6H+ -> 2Al3+ + 3H2O Al2O3 + 2OH- + 3H2O -> 2Al(OH)4 -
54
SiO2 + acid/ alkali
very concentrated NaOH | SiO2 + 2NaOH -> Na2SiO3 + H2O
55
P4O10 + acid/ alkali
alkali | P4O10 +12OH- -> 4PO43- + 6H2O
56
SO2 + acid/ alkali
alkali | SO2 + 2OH- -> SO32- + H2O
57
SO3 + acid/ alkali
alkali | SO3 + 2OH- -> SO42- + H2O

A2 Chem (5 decks)

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