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Types of reactions Flashcards

1
Q

Combustion of elements in Oxygen

A

Elements burn more brightly and rapidly in pure oxygen than in air because air contains only 21% oxygen

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2
Q

Burning magnesium

A

burns with a white,bright flame to give a white powdery ash. Only soluble in small amounts

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3
Q

Burning sulfur

A

burns in oxygen with a blue flame.poisonous,colourless sulfur dioxide gas is produced

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4
Q

Burning Hydrogen

A

burns with a pale blue flame.Product is water

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5
Q

Oxidation

A

gain of oxygen

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6
Q

Reduction

A

Loss of oxygen

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7
Q

redox

A

Where both reduction and oxidation are happening at the same time

magnesium+copper (ii) oxide —> magnesium oxide + copper

magnesium has been oxidised
Copper has been reduced

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8
Q

Reducing agent

A

Substance that reduces something else and loses oxygen

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9
Q

oxidising agent

A

Substances that takes oxygen

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10
Q

OIL RIG

A

Oxidation
Is
Loss
Reduction
Is
Gain

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11
Q

Oxidation in terms of electrons

A

loss of electrons

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12
Q

Reduction in terms of electrons

A

is gain of electrons

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13
Q

metals

A

lose electrons to become metal ions

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14
Q

Non-metals

A

gain electrons to become non metal ions. and are negative

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15
Q

Thermal decomposition

A

breakdown of a compund into simpler substance using heat

CaCO3 —>CaO + CO2

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16
Q

Combustion equation

A

fuel +oxygen –>CO2 + H2o

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17
Q

Soluble salts step 1

A

warm acid

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18
Q

Soluble salts step 2

A

Add excess CuO

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19
Q

Soluble salts step 3

A

filter (remove excess CuO)

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20
Q

soluble salts step 4

A

Heat to drive off water

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21
Q

soluble salts step 5

A

leave to crystallise (under windowsill)

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22
Q

Precipitation

A

2 soluble salts —> insoluble salt + soluble salt

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23
Q

All sodium,potassium and ammonium salts

A

soluble

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24
Q

All nitrates

A

soluble

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25
Q

Most chlorides, bromides and iodides

A

soluble

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26
Q

most sulphates

A

soluble

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27
Q

Sodium,potassium and ammonium carbonates

A

soluble

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28
Q

Sodium,potassium and ammonium hydroxides

29
Q

Lead,silver,chloride,bromide and iodide

30
Q

Barium sulphate, calcium and lead sulphates and sulphate

31
Q

Most other carbonates except sodium,potassium and ammonium

32
Q

Most hydroxides except sodium, potassium and ammonium

33
Q

Precipitation reaction

A

a chemical reaction between two soluble salts where one of the products is an insoluble salt (a precipitate)

34
Q

How to prepare insoluble salt by precipitation 1

A

Mix 2 soluble salts together , so they react together

35
Q

How to prepare a insoluble salt by precipitation 2

A

Filter the mixture to separate products produced (soluble and insoluble salt produced)

36
Q

How to prepare a insoluble salt by precipitation 3

A

Wash the insoluble salt on the filter paper

37
Q

How to prepare an insoluble salt by precipitation 4

A

Dry the insoluble salt in a warm oven

38
Q

Reactive metals+ cold water

A

potassium,sodium and calcium will react with cold water producing bubbles of hydrogen gas

39
Q

All metals above hydrogen

A

will react with acids causing bubbles

40
Q

The more reactive a metal

A

the faster/more vigourous the reaction will be- producing hydrogen gas quicker

41
Q

Metals below hydrogen

A

will not react with acids

42
Q

Please Stop Calling Me A Careless Zebra Instead Try Learning How Copper Saved Gold

A

Potassium,Sodium,Calcium,Magnesium,Aluminium,Carbon,Zinc,Iron,Tin , Lead , Hydrogen ,copper, Silver , Gold

43
Q

Displacement reactions

A

A more reactive metal can displace a less reactive metal from a compound

copper sulfate+magenesium –>Magnesium sulfate +Copper

44
Q

Neutralisation reaction

A

Acids are neutralised by alkalis

base + acid –> salt + water

45
Q

metal carbonates + acid

A

also neutralise Acids

metal carbonate+acid–> salt+water+carbon dioxide

46
Q

Hydrochloric acid

A

produces chlorides

47
Q

nitric acid

A

produces nitrates

48
Q

Sulfuric acid

A

produces sulfates

49
Q

Acids

A

Have H+ ions

50
Q

alkalis

A

contain OH- ions

51
Q

PH1-6

52
Q

PH 7

53
Q

PH 8-14

54
Q

neutralisation equation

A

H+ + OH- —> H2O

55
Q

Titration results

A

have to be concordant (within 0.1 of each other)

56
Q

Concentration

A

moles/volume

57
Q

moles

A

concentration x volume

58
Q

Loss of electrons

A

becomes positive

59
Q

gain of electrons

A

becomes negative

60
Q

Step 1 titration

A

Use the pipette and pipette filler to add 25 cm3 of alkali to a clean conical flask.

61
Q

step 2 titration

A

Add a few drops of Phenolphthalein indicator and put the conical flask on a white tile.

62
Q

step 3 titration

A

Fill the burette with acid and note the starting volume.

63
Q

step 4 titration

A

Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix.

64
Q

step 5 titration

A

Stop adding the acid when the colour changes from pink to colourless. Note the final volume reading.

65
Q

what indicator is used in titration?

A

Phenolphthalein indicator

66
Q

Why is phenopthalein indicator used in titration?

A

because it changes colour in alkali solutions

67
Q

phenopthalein in alkali

68
Q

phenopthalein in acidic solutions

A

colourless

Chemistry (8 decks)

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