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GCSE Chemistry > C5- Chemical Changes > Flashcards

C5- Chemical Changes Flashcards

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1
Q

What is the reactivity series?

A

A list of metals in order of their reactivity with the most reactive metals at the top and the least reactive ones at the bottom

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2
Q

Order of reactivity

A

Potassium, sodium, Lithium, Calcium, magnesium, aluminium, Zinc, Iron, Tin, lead, copper, Silver, Gold

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3
Q

Potassium, Sodium, Lithium, Calcium reaction with water

A

Fizz, giving off hydrogen gas, leaving an alkaline solution of metal hydroxide

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4
Q

Magnesium, Aluminium, Zinc, Iron reaction with water

A

Very slow reaction

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5
Q

Tin and lead reaction with water

A

Slight reaction with steam

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6
Q

Copper, Silver, Gold reaction with water

A

No reaction

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7
Q

Potassium, sodium, lithium reaction with dilute acid

A

Explode

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8
Q

Calcium, magnesium, aluminium, zinc, iron reaction with dilute acid

A

Fizz, giving off hydrogen gas and forming a salt

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9
Q

Tin and lead reaction with dilute acid

A

React slowly with warm acid

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10
Q

Copper, silver, gold reaction with dilute acid

A

No reaction

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11
Q

Reactivity of metals and displacement

A

A more reactive metal will displace a less reactive metal from an aqueous solution of one of its salts

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12
Q

Magnesium + copper sulfate ~>

A

Magnesium sulfate + copper
This is a displacement reaction which happens because Magnesium is more reactive than copper

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13
Q

Where do non metals carbon and hydrogen fit in the reactivity series?

A

Carbon is between aluminium and zinc
Hydrogen is between lead snd copper

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14
Q

What needs to happen to most metals in the Earth’s crust in order for them to be used?

A

The metals need to be chemically separated from other elements

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15
Q

Whether it is worth extracting a metal depends on…

A

How easy it is to extract from its ore
How much metal the ore contains
The changing demands for a particular metal

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16
Q

What is chemical reduction?

A

The removal of oxygen from a compound

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17
Q

Metal + acid ~>

A

Salt + hydrogen

18
Q

Salts formed when you react metals with different acids

A

Hydrochloric acid forms chlorides
Sulfuric acid forms sulfates
Nitruc acid forms nitrates

19
Q

What is a redox reaction ?

A

A reaction where reduction (gain of electrons) and oxidation (loss of electrons) both occur

20
Q

Acid + base

A

Salt + water

21
Q

Ions of group 1 metals

A

+1

22
Q

Ions of group 2 metals

A

+2

23
Q

Aluminium ion

A

+3

24
Q

Ammonium ion

A

+1 e.g NH4^+

25
Q

Transition metals ions (dependent on roman numeral)

A

E.g Copper (II) ion = +2

26
Q

Ions of group 7 non metals

A

-1

27
Q

Nitrate ions

A

-1

28
Q

Sulfate ions

A

-2

29
Q

Making salts practical (basic steps)

A
  1. Add copper oxide in excess to sulfuric acid. Warm gently on a tripod and gauze
  2. When the reaction is complete filter the solution to remove excess copper oxide.
  3. Evaporate half the water from the solution using a water bath. Leave the solution to form crystals in a warm room for a day.
  4. Pat dry if any solution remains on the crystals
30
Q

Acid + alkali

A

Salt + water

31
Q

Acid + carbonate

A

Salt + water + carbon dioxide

32
Q

What are alkalis?

A

Soluble hydroxides. An example is sodium hydroxide solution

33
Q

What are bases?

A

Substances that can neutralise acids

34
Q

What can you use to find the PH of a solution?

A

Universal indicator

35
Q

pH scale

A

0 - most acidic
7 - neutral
14 - most alkaline

36
Q

Where is pure water on the pH scale ?

A

pH 7

37
Q

What do strong acids do in solution?

A

Ionise completely

38
Q

What do weak acids do in solution?

A

Do not fully ionise in solution

39
Q

Examples of strong acids

A

Hydrochloric acid
Nitric acid
Sulfuric acid

40
Q

Examples of weak acids

A

Ethanoic acid
Citric acid
Carbonic acid

41
Q

Concentration of Hydrogen ions (H+) in relation to pH values

A

As the concentration decreases by a factor of 10 the pH value increases by one unit
e.g
0.10 to 0.010
1 to 2 on pH scale

GCSE Chemistry (11 decks)

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