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Types of reactions Flashcards

(68 cards)

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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
Most chlorides, bromides and iodides
soluble
26
most sulphates
soluble
27
Sodium,potassium and ammonium carbonates
soluble
28
Sodium,potassium and ammonium hydroxides
Soluble
29
Lead,silver,chloride,bromide and iodide
insoluble
30
Barium sulphate, calcium and lead sulphates and sulphate
insoluble
31
Most other carbonates except sodium,potassium and ammonium
insoluble
32
Most hydroxides except sodium, potassium and ammonium
insoluble
33
Precipitation reaction
a chemical reaction between two soluble salts where one of the products is an insoluble salt (a precipitate)
34
How to prepare insoluble salt by precipitation 1
Mix 2 soluble salts together , so they react together
35
How to prepare a insoluble salt by precipitation 2
Filter the mixture to separate products produced (soluble and insoluble salt produced)
36
How to prepare a insoluble salt by precipitation 3
Wash the insoluble salt on the filter paper
37
How to prepare an insoluble salt by precipitation 4
Dry the insoluble salt in a warm oven
38
Reactive metals+ cold water
potassium,sodium and calcium will react with cold water producing bubbles of hydrogen gas
39
All metals above hydrogen
will react with acids causing bubbles
40
The more reactive a metal
the faster/more vigourous the reaction will be- producing hydrogen gas quicker
41
Metals below hydrogen
will not react with acids
42
Please Stop Calling Me A Careless Zebra Instead Try Learning How Copper Saved Gold
Potassium,Sodium,Calcium,Magnesium,Aluminium,Carbon,Zinc,Iron,Tin , Lead , Hydrogen ,copper, Silver , Gold
43
Displacement reactions
A more reactive metal can displace a less reactive metal from a compound copper sulfate+magenesium -->Magnesium sulfate +Copper
44
Neutralisation reaction
Acids are neutralised by alkalis base + acid --> salt + water
45
metal carbonates + acid
also neutralise Acids metal carbonate+acid--> salt+water+carbon dioxide
46
Hydrochloric acid
produces chlorides
47
nitric acid
produces nitrates
48
Sulfuric acid
produces sulfates
49
Acids
Have H+ ions
50
alkalis
contain OH- ions
51
PH1-6
Acidic
52
PH 7
neutral
53
PH 8-14
Alkali
54
neutralisation equation
H+ + OH- ---> H2O
55
Titration results
have to be concordant (within 0.1 of each other)
56
Concentration
moles/volume
57
moles
concentration x volume
58
Loss of electrons
becomes positive
59
gain of electrons
becomes negative
60
Step 1 titration
Use the pipette and pipette filler to add 25 cm3 of alkali to a clean conical flask.
61
step 2 titration
Add a few drops of Phenolphthalein indicator and put the conical flask on a white tile.
62
step 3 titration
Fill the burette with acid and note the starting volume.
63
step 4 titration
Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix.
64
step 5 titration
Stop adding the acid when the colour changes from pink to colourless. Note the final volume reading.
65
what indicator is used in titration?
Phenolphthalein indicator
66
Why is phenopthalein indicator used in titration?
because it changes colour in alkali solutions
67
phenopthalein in alkali
pink
68
phenopthalein in acidic solutions
colourless

Chemistry (8 decks)

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