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chemsitry tests Flashcards

1
Q

Soluble salts

A
  • Ammonium, sodium, and potassium salts
  • Nitrate salts
  • Nearly all chloride, bromide, and iodide salts
  • Nearly all sulfates
  • Ammonium, sodium, potassium carbonate salts
  • Ammonium, sodium, potassium hydroxide salts
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2
Q

Insoluble salts

A
  • Silver chloride, silver bromide, silver iodide, lead chloride
  • Barium sulfate, calcium sulfate, lead sulfate
  • Most carbonates
  • Most hydroxides
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3
Q

Testing for cations using aqueous sodium hydroxide

Ammonium

A

Ammonia gas produced on heating - turns red litmus paper blue

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4
Q

Testing for cations using aqueous sodium hydroxide

Calcium

A

White percipitate, insoluble in excess

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5
Q

Testing for cations using aqueous sodium hydroxide

Copper(II)

A

Light blue percipitate, insoluble in excess

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6
Q

Testing for cations using aqueous sodium hydroxide

Iron (II)

A

Green percipitate, insoluble in excess

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7
Q

Testing for cations using aqueous sodium hydroxide

Iron (III)

A

Red-brown percipitate, insoluble in excess

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8
Q

Testing for cations using aqueous sodium hydroxide

Zinc (II)

A

White percipitate, soluble in excess, gives a colourless solution

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9
Q

Testing for cations using aqueous ammonia

Calcium

A

No percipitate, very slifhrly white percipate

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10
Q

Testing for cations using aqueous ammonia

Copper (II)

A

Light blue percipitate, soluble in excess, dark blue solution

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11
Q

Testing for cations using aqueous ammonia

Iron (II)

A

Green percipitate, insoluble in excess

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12
Q

Testing for cations using aqueous ammonia

Iron (III)

A

Red-brown percipitate, insoluble in excess

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13
Q

Testing for cations using aqueous ammonia

Zinc (II)

A

White percipitate, insoluble in excess, gives colourless solution

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14
Q

Flame test

Lithium

A

Red

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15
Q

Flame test

Sodium

A

Yellow

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16
Q

Flame test

Potassium

A

Lilac

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17
Q

Flame test

Copper (II)

A

Blue-green

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18
Q

Testing for anions

Carbonate

A

Test: Dilute acid
Result: Effervesence, carbon dioxide produced

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19
Q

Testing for anions

Chloride (in solution)

A

Test: Acidify with dilute nitric acid, then add aqeous silver nitrate
Result: White percipitate

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20
Q

Testing for anions

Bromide (in solution)

A

Test: Acidify with dilute nitric acid, then add aqeous silver nitrate
Result: Cream percipitate

21
Q

Testing for anions

Nitrate (in solution)

A

Test: Add aqueous sodium hydroxide then aluminium foil; warm carefully
Result: Ammonia gas produced

22
Q

Testing for anions

Sulfate (in solution)

A

Test: Acidift then add aqueous barium nitrate or barium chloride
Result: White percipitate

23
Q

Fuels

Small number of carbon atoms

A
  • Low boiling points
  • Evaporate and rise up first
24
Q

Fuels

Higher number of carbon

A
  • Higher boiling point
  • ## As they evaporate, they condense at a higher temperature - lower down the tower
25
Q

Fuels

Refinery gas

A
  • Used for bottled gas for cooking
  • 1-4 Carbon atoms
  • Boiling point of under 40 degrees
  • Gases at low temperatures
  • Very low viscosity (flows easily)
26
Q

Fuels

Gasoline

A
  • Used in cars
  • 5 - 6 Carbon atoms
  • Boiling point of 40-100
  • Very volatile
  • Very low viscosity
27
Q

Fuels

Naphtha

A
  • Feedstock for making chemicals
  • 5 - 9 Carbon atoms
  • Boiling point of 60-100
  • Volatile
  • Low viscosity
28
Q

Fuels

Diesel oil/gas

A
  • Fuel in diesel engines
  • 13-25 Carbon atoms
  • Boiling point: 250 - 350
  • Low volatility
  • High viscosity
29
Q

Fuels

Bitumen

A
  • Used for road surfaces
  • Carbon atoms of over 40
  • Boiling point over 500
  • Very low volatility
  • High viscosity
30
Q

Alkane general formula

31
Q

Alkene general formula

32
Q

Alkanes

A
  • Unreactive because C-H bonds are strong
  • Can be used as fuel because they combust
  • Saturated hydrocarbons (each molecule only has single covalent bonds)
  • Every atom has a full outer shell
33
Q

Alkenes

34
Q

Thermal cracking

A
  • Cracking long chain alkanes into smaller ones
  • High temperature (800 degrees)
  • Ethene and hydrogen gas produced
35
Q

Catalytic cracking

A
  • Another form of cracking
  • Uses aluminium and ceramic based catalysts that lower the temperature required to 500 degrees
  • Cheaper
  • Thermal cracking more useful fo rlonger chain hydrogcarbons
35
Q

Detecting alkenes

A
  • Bromine
  • Hydrogen
  • Steam
  • Confirm the presence of a double bond by testing the ability of an alkene to undergo additionr Reactions
35
Q

Detecting alkenes

Bromine

A
  • Alkenes react with halogens such as bromine
  • Brown to colourless
36
Q

Detecting alkenes

Hydrogen

A
  • Temperature of 200 degrees
  • Presence of a nickel catalyst
  • Also called hydrogenation
36
Q

Detecting alkenes

Steam

A
  • 300 degrees
  • Presence of steam and phoshoric acid, which acts as a catalyst to produce alcohol
  • Water splits into an H atom and an OH group
36
Q

Hydration of ethene

A
  • ## Synthetic ethanol
37
Q

Molten lead bromide

A

Product at cathode: Lead
Product at anode: Bromide
Observations: Silvery solid at the cathode, brown gas at the anode

38
Q

Concentrated aqueous sodium chloride

A

Product at cathode: Hydrogen
Product at anode: Chloride
Observations: Colourless gas at the cathode, pale yellow green gas at the anode which bleaches damp litmus paper

39
Q

Acid + metal

A

Observation:
* Effervescence
* Heat evolved
* Hydrogen gas formed

Reaction occurring:
Acid + Metal -> Salt + Hydrogen

40
Q

Acid + Base

A

Observation:
Indicator goes green
Reaction occurring:
Neutralisation
Acid + Base -> Salt + Water

41
Q

Bronze

A

Copper and tin

42
Q

Mild steel

A

Iron and about 0.25% carbon

43
Q

High carbon steel

A

Iron and up to 2.5% carbon

44
Q

Brass

A

Copper and zinc

45
Q

Stainless steel

A

Iron, carbon, chromium and nickel

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