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Chemistry A Level > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

(55 cards)

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1
Q

Groups 1 and 2

A

All have the highest energy electron in the s subshell

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2
Q

Group 2 reacting with O2

A
  • except Be, they all react vigorously, producing a bright flame
  • 2M + O2 -> 2MO
  • Ba + O2 -> 2BaO2
  • contains a peroxide ion
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3
Q

Peroxide ion

A

(O2)2-

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4
Q

2Mg + O2 -> 2MgO

A
  • bright white flame

* used in fireworks and flames

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5
Q

Ca + Sr with O2

A

red flames

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6
Q

Ba + O2 -> 2BaO2

A

Green flame

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7
Q

Group 2 reactions with water

A
  • less reactive than the corresponding group 1 elements
  • Be does not react with steam
  • Mg reacts v. slowly w/ cold water and does react w/ steam
  • Ca, Sr and Ba all react w/ cold water with increasing vigour
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8
Q

Mg (s) + H2O (g)

A

-> MgO(s) + H2 (g)

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9
Q

Ca (s) + 2H2O

A

-> Ca(OH)2 + H2(g)

Calcium hydroxide is only sparingly soluble in water, so a thick white suspension accompanies the effervescence

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10
Q

Sr(s) + 2H2O (l)

A

-> Sr(OH)2 + H2 (g)

Strontium hydroxide is slightly soluble in water

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11
Q

Ba(s) + 2H2O (l)

A

-> Ba(OH)2 + H2 (g)

Barium hydroxide is soluble in water

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12
Q

Group 2 reactions with chlorine

A

All form chlorides

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13
Q

Group 2 oxide reacting with water

A
  • BeO is not attacked by water

* others are ionic; react to form hydroxides

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14
Q

Group 2 oxides reacting with dilute acids

A

All produce salt and water

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15
Q

Group 2 hydroxides (bases)

A

React with acids in neutralisation to form salt and water

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16
Q

Group 2 sulphate solubility

A

Solubility decreases down the group

MgSO4 -> soluble
CaSO4 -> slightly soluble
SrSO4 -> insoluble
BaSO4 -> insoluble

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17
Q

Testing for sulphate ions

A
  • used because BaSO4 is highly insoluble
  • if BaCl2 is added to a solution containing sulphate ions, a white ppt is produced

Ba2+(aq) + (SO4)2-(aq) -> BaSO4(s)

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18
Q

Group 2 hydroxide solubility

A
  • solubility increases down the group
  • Ca(OH)2 is not very soluble in water; much more soluble than CaCO3
  • when CO2 is passed through Ca(OH)2, it forms insoluble CaCO3 suspension, turning limewater cloudy
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19
Q

Indicator of carbonate thermal stability

A

Time taken for gas evolved to turn limewater cloudy

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20
Q

All group 1 carbonates are…

A

… thermally stable up to Bunsen temperatures; smaller charge density; lower polarising power

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21
Q

Lithium and group 2 carbonates thermally decompose to form

A

Metal oxide + CO2

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22
Q

Stability trend down Group 2

A
  • more stable
  • charge density decreases
  • smaller polarising power
  • cannot draw oxygen towards it as easily
  • does not distort the C-O bond to the same extent
  • need more vibrational energy as the bond has not been as weakened
  • harder to release the CO2 and form the metal oxide
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23
Q

All nitrates…

Study These Flashcards
A

… decompose

24
Q

Group 1 nitrates except Li

Study These Flashcards
A

Break down to form

Metal nitrite + oxygen

25
Lithium and group 2 elements...
... break down to a greater extent (because they have higher polarising power) to form Metal oxide + nitrogen dioxide + oxygen
26
Flame test theory
Electrons are pushed to a higher energy level when heated; when they drop back down, they give out their energy in the form of light
27
Flame colours
``` Lithium = red Sodium = yellow Potassium = lilac Calcium = brick red Strontium = crimson Barium = apple green ```
28
MP and BP trend down halogen group Don’t confuse with relativity!!!
* increases * more electrons * more idids * more energy needed to overcome the forces
29
Trend for electronegativity down halogen group
* decreases * atomic radius increases * bonding pair is further from nucleus with greater inner shielding * harder to pull the electron towards the nucleus
30
Reactivity of the halogens depends upon
How strongly the electron is drawn into the vacant position in their outer-shell
31
Reactivity trend down halogen group
* decreases * atomic radius increases * greater distance and more shielding between incoming electron and the nucleus * attraction decreases * illustrated by displacement reactions
32
Cl2 + 2KBr -> Br2 + 2KCl
``` Cl2 = chlorine water; colourless 2KBr = potassium bromide; colourless Br2 = bromine water; orange 2KCl = potassium chloride; colourless ``` Bromine présence is proven by adding an organic solvent into which bromine dissolves preferentially, turning red
33
Trend in oxidising capacity going down the halogen group
* chlorine is the strongest oxidising agent * wants to gain electrons! * smallest atomic radius * least distance and shielding * attraction of incoming e-s to the nucleus is greater As halogens tend to gain electrons (electronegative); they tend to be oxidising agents
34
Trend in reducing capacity going down the halogen group
* iodine is the best reducing agent * wants to lose e- * largest atomic radius * greatest distance and shielding * easily loses outer e-
35
Halogen reactions with metals
* tend to be reactive * vigour decreases with reduced reactivity * less exothermic as atomic number increases
36
Cl2 + H2
-> 2HCl Explosive in sunlight
37
Br2 + H2
-> 2HBr Requires heat + platinum catalyst
38
I2 + H2
V slow- reaction does not go to completion
39
Disproportionation of chlorine
Cl2 + H2O <=> HOCl + HCl Used in water treatment as HOCl contains chlorate(I)ion, which has strong anti-bac action, sterilising the water Reversible; quantités of chlorate(I)ions are quite small -> it is safe to drink the water Shifted right by removing acid products, using NaOH alkali
40
Cl2 + NaOH Cold!
* -> NaOCl + NaCl * produces a much higher concentration of chlorate(I) * used in bleach
41
3Cl2 + 6NaOH
-> NaOCl3+ 5NaCl + 3H20 • 5 chlorine atoms take an electron to form ions (in NaCl) • chlorine losing 5 electrons goes to 5+ (in NaClO3)
42
Iron is a ...
... transition metal; can form compounds of iron(II) and iron(III)
43
Solutions containing iron(II)
Pale green
44
Solutions containing iron(III)
Yellow
45
Cl2 + Fe2+
-> 2Cl- + 2Fe2+ Pale green -> yellow Could also use bromine as oxidising agent, but not iodine
46
Conc. H2SO4
* oxidising agent | * when added to potassium Hamite, hydrogen halide is formed
47
KCl(s) + H2SO4 (aq)
-> KHSO4 (aq) + HCl (g) Steamy white fumes Effervescence Wet litmus turns blue -> red Chloride is not a very strong reducing agent -> holds e-s
48
KBr (s) + H2SO4 (aq)
-> KHSO4 (aq) + HBr (g) H2SO4 (aq) + 2HBr (g) -> Br2 (l) + SO2 (g) + 2H2O (l)
49
KI (s) + H2SO4 (aq)
-> KHSO4 (aq) + HI H2SO4 (aq) + 2HI (g) -> I2 (s+g) + SO2 + 2H2O
50
Halide test
1) dissolve in water 2) acidity with dilute HNO3 3) add AgNO3 (aq) 4) identify silver halide precipitate by colour Ag+ (aq) + X- (aq) -> AgX (s)
51
Hydrogen halides + water
* soluble * dissociate into ions, forming acidic solutions * HX (aq) -> H+ (aq) + X- (aq)
52
Hydrogen halides + ammonia
* when gaseous hydrogen halides come into contact with gaseous ammonia, ammonium halide (dense white smoke) is produced * HX (g) + NH3 (g) -> NH4X (g)
53
Carbonate and hydrogencarbonate chemical test
• adding dilute acid forms CO2 (effervescence) * (CO3)2- (aq) + 2H+ (aq) -> H2O (l) + CO2 (g) * HCO3- (aq) + H+ (aq) -> H2O (l) + CO2 (g) * when CO2 is bubbled through limewater, it goes cloudy due to CaCO3(s) formation * Ca(OH)2 (aq) + CO2 (g) -> CaCO3(s) + H2O (l)
54
Sulphate test
* add dilute HCl * if no reaction, add a few drops of BaCl2 (aq) * forms a white precipitate • Ba2+ (aq) + (SO4)2- (aq) -> BaSO4 (s)
55
Ammonium test
* warm with NaOH(aq) -> produces NH3 * NH3 dissolves * test w/ damp red litmus * turns blue • NH3(g) + H2O(l) -> NH4+ + OH- Alkali!

Chemistry A Level (12 decks)

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