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GCSE Chemistry > C5 > Flashcards

C5 Flashcards

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1
Q

In the table of ions what os the forst column

A

+1
Simple ions( group 1 ): Na+, Li+, K+, H+
Polyatomic ions: NH4+ ( ammonium )

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2
Q

Innthe table of ions what is in column 2

A

+2

Simple ions: Mg2+, Ca2+, Cu2+, Zn2+

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3
Q

In the table of ions what is in column 3

A

3+

Simple ions: Al3+

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4
Q

In the table of ions what is in collumn 4

A 
1-
Simple ions ( group 7 ): Cl-, Br-, I-

Polyatomic: NO3- ( nitrate )

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5
Q

In the table of ions what is in collumn 5

A

2-
Simple ions: O2-

Polyatomic: SO4 2- ( sulphate ), CO3 2- (carbonate )

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6
Q

What has happened to the metals in many of these ores?

A

They have been chemically bonded to other elements in compounds. Many have been oxidised to form their oxides.

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7
Q

Give an example of oxidation..

A

Iron + oxygen -> iron (III) oxide

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8
Q

What must you do to extract metals from their oxide form?

A

You must reduce them (oxygen is removed).

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9
Q

What is the reactivity series?

A

This is a list of metals in order of their reactivity, the most reactive are at the top and least reactive are at the bottom.

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10
Q

What can you use to help find the reactivity of metals?

A

Water or dilute acid

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11
Q

What happens when you react the metals with water?

A

The most reactive will give off a slight fizz, then a slow reaction, slight reaction with steam and finally the least reactive won’t react with water

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12
Q

How to find which metals are most reactive with dilute acid?

A 
Most reactive:
Explosion 
Fizz, giving of Hydrogen gas + salt
React slowly
No reaction - least reactive
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13
Q

How can you find if hydrogen gas is given of from an equation?

A

You can use the squeaky pop test with a lighted splint

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14
Q

What are Ores?

A

These are rocks from which you can extract the metals found in the periodic table from.

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15
Q

What happens in a displacement reaction?

A

A more reactive metal will displace a less reactive metal from its aqueous solution

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16
Q

When would nothing happen in a displacement reaction?

A

When the more reactive metal is already in solution

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17
Q

What can copper and hydrogen be used for in displacement reactions?

A

They can be used for seeing what metals are more and less reactive than them for the reactivity series

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18
Q

What does OILRIG mean?

A

Oxidation is loss (of electrons), reduction is gain (of electrons)

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19
Q

What is an ionic equation?

A

This is only showing the atoms that gained or lost electrons with another reactant

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20
Q

What is a half equation?

A

This is where you only show what happened in terms of electrons to each reactant

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21
Q

Why do we extract metal from ores?

A

Because there’s enough metal inside to make it economic to do so.

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22
Q

Why is gold and some other metals found in its native state?

A

Because it is so unreactive it didn’t even react with anything to make the ore.

23
Q

How does carbon help extract metal from ores?

A

Anything less reactive than carbon can be extracted through a displacement reaction with it.

24
Q

How are metals more reactive than carbon extracted?

A

Electrolysis (we don’t need to know this yet)

25
Q

What is a metal + acid turn into?

A

Metal + acid -> salt + hydrogen

26
Q

What salts are formed from HCl?

A

Chloride salts (Cl-)

27
Q

What salts are formed from H2SO4?

A

Sulphates (SO4 ^2- ions)

28
Q

What salts are formed from Nitric acid (HNO3)?

A

Nitrates (NO3 ^- ions)

29
Q

Metal + water =

A

Metal hydroxide + hydrogen

30
Q

Metal + oxygen =

A

Metal + oxygen = metal oxide ( if reactive enough )

31
Q

Metal + acid

A

Metal + acid = salt + hydrogen ( if reactive enough )

32
Q

Metal + water

A

Metal + water = metal hydroxide + hydrogen ( if reactive enough )

33
Q

Metal oxide + acid

A

Metal oxide + acid = salt + water

34
Q

Metal hydroxide + acid

A

Metal hydrixide + acid = salt + water

35
Q

Metal carbonate + acid

A

Metal carbonate + acid = salt + water + carbonate

36
Q

Ammonia + acid

A

Ammonia + acid = ammonium salt

37
Q

Base + acid

A

Base + acid = salt + water

38
Q

Alkali + acid

A

Alkali + acid = salt + water

39
Q

How is an alkali different to a base

A

An alkali is a base that is soluble in water

40
Q

What is a base

A

A base is a metal that neutralises acid to form salt and water

41
Q

What colour of universal indicator is strong acid

A

Red ( 0 - 1)

42
Q

What colour of universal indicator is strong alkali

A

Purple ( 13 - 14)

43
Q

What is the definition of an acid

A

A substance that produces H+ ( aq) ( hydrogen ) ions when added to water

44
Q

What do alkalis prodice when you add them to water

A

They produce OH- ( aq) ions ( hydroxide ) when added to water

45
Q

What is the chemical equation for what happens to HCl ( hydrochloric ackd )when it is added to water

A

HCl ( g)= H+ ( aq ) + Cl- ( aq )

46
Q

What is the chemical equation for what happens to sodium hydroxide when it is added to water

A

NaOH ( s) = Na+ ( aq ) + OH- ( aq )

47
Q

What do strong acids do when they are added to water

A

They ionise COMPLETELY e.g HCl ( g)= H+ ( aq ) + Cl- ( aq ) - all ions have been spit up, reaction is not reversible

48
Q

What do weak acids do when they are added to water

A

They only ionise PARTIALLY e.g CH3COOH = CH3COO- ( aq) + H+(aq) - only the hydrogen acid has ionised, the reaction can be reversible ( arrows going both ways )

49
Q

What can pH stand for

A

Power of hydrogen, this relates that the more acidic the substance is, the more powerul hydrogen is in the compound

50
Q

What happens when the concentration of the H+ ion is reduced by a factor of 10

A

The pH value goes up a unit ( indicating is has got less acidic )

51
Q

Recite the chart of how the pH value changes with the concentration of hydrogen

A 
Concentration of H+ ions ( mol/dm^3):
1x10^-1 : 1 - pH value 
1x10^-2 : 2 - pH value 
1x10^-3 : 3 - pH value 
1x10^-4 :  4 - pH value 
etc
52
Q

What is the rule for H+ ions and the change in pH

A

As the concentration of H+ ions decreases, the pH value increases ( get less acidic )

53
Q

One way to remember reactivity series

A 
Peggy: potassium
Sue: sodium
Cooks: calcium
Meat: magnesium
At: aluminium
Cool: carbon
Zoos: zinc
In: iron
Tropical: tin
London: lead
Hence: hydrogen
Causing: copper
Severe: silver
Gut: gold
Pain: platinum
54
Q

C5 required practical method: making a copper salt

A

1) measuring cylinder, measure 20cm^3 or acid into beaker
2) stand beaker on tripod and gauze and warm gently until almost boiling, turn off Bunsen burner
3) add half spatula of copper(II) oxide powder into acid and stir using glass rod
4) continue adding copper oxide until no more dissolves. When copper oxide disappears the solution is clear blue
5) allow apparatus to cool completely and then filter mixture and discard residue
6) pour filtrate into evaporating basin and use water bath ( 250 cm^3 beaker with boiling water ) in tripod and gauze. Stop heating when crystals start to form

GCSE Chemistry (15 decks)

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