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Chemistry GCSE > Chemical Changes 1+2 > Flashcards

Chemical Changes 1+2 Flashcards

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1
Q

what are the three most common acids?

A
  • hydrochloric acid (HCl)
  • Sulfuric acid (H2SO4)
  • nitric acid (HNO3)
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2
Q

Types of salt that can form from the acids

A
  • nitrate
  • cholide
  • sulfate
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3
Q

What can salts be used for?

A
  • seasoning food
  • dissolved in drinking water
  • perserve food
  • fertilizers (sulfate and nitrate salts)
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4
Q

What kind of reaction is the reaction between acids and metals?

A
  • redox reaction
  • (oxidation and reduction reaction taking place at the same time)
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5
Q

What is oxidation?

A
  • gain of oxygen or losing of electrons of a substance in a reacton
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6
Q

What is reduction?

A
  • losing of oxygen, gaining of electrons or gaining hydrogen by a substance in a reaction
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7
Q

what do all acids have?

A

hydrogen ions

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8
Q

What is the difference between an alkali and a base?

A
  • alkalis are soluble, they can dissolve in water
  • all alkalis are bases but not all bases are alkali
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9
Q

How do you identify a base?

A
  • name ends with carbonate or oxide
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10
Q

How do you identify an alkali?

A
  • if the metal is in group 1/2 ending with hydroxide
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11
Q

How do you identify a salt?

A
  • ends with sulfate/ nitrate/ chloride
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12
Q

compound ions names

A
  • hydroxide (OH-)
  • nitrate ion (NO3-)
  • sulfate ion (SO4 2-)
  • carbonate ion (CO3 2-)
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13
Q

What is neutralisation?

A

When acids are neutralised by alkalis and bases to produce salt and water, and by metal carbonates to produce salts, water and carbon dioxide

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14
Q

What does alkalis and bases produce when they neutralise acids?

A

Water and salt

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15
Q

What do metal carbonates produce when they react with acid?

A

Salt, water, and carbon dioxide

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16
Q

What salt does the three most common acids make

A

Hydrochloric acid - chloride
Sulfuric acid - sulfate
Nitric acid - nitrite

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17
Q

How do you make pure, dry samples of soluble salts?

A
  • measure aicd using measuring cylinder and pour it into beaker
  • gently heat the acid by placing it on a bunsen burner and a tripod (speeds up reaction)
  • take acid off bunsen and add spatulas of the alkali/ base until the powder at the bottom of the beaker. (to make sure that the alkali/ base is in excess) the solution should turn into a different colour (blue for copper sulfate)
  • remove the excess copper oxide by filtering it using a funnel and filitering paper (to remove excess copper oxide)
  • pour the solution into evaporating basin and heat over a beaker of boiling water(if the solution is heated directly the crystals will break down)
  • take evaporating basin off the water bath once half of the solution is gone and leave it out at room temp to let it evaporate naturally (larger crystals can form)
  • after water has evaporated entirely, put crystals on filiter paper (to make sure that it is completely dry)
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18
Q

Why do we not use an oven to dry out the crystals?

A
  • the cyrstals would turn into powder
  • removes the water molecules from the crystal (needs water to remain crystal)
19
Q

describe the colour of universal indicator from acid to alkali

A

acid - red, orange, yellow
neutral - green
alkali - blue, purple

20
Q

what are strong acids in an aqueous solution?

A

completely ionised

21
Q

what are weak acids in an aqueous solution?

A

partially ionised

22
Q

how much does the concentration of hydrogen ions need to be diluted by to increase the pH by 1?

A

10 times, the less hydrogen ions, the higher the pH

23
Q

Write a half equation of sodium for the reduction of sodium ions

A

2Na -> 2Na+ + 2e-

24
Q

Write a half equation for the reduction of chloride ions

A

Cl2 + 2e -> 2Cl-

25
Q

reactivity series

A

group 1
(potassium, sodium etc)
aluminium
carbon
zinc
iron
tin
hydrogen
copper
silver
gold
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26
Q

What is given off when a metal reacts with water or acid and what can react with them?

A
  • hydrogen gas
  • metals > hydrogen in reactivity can react with dilute acids
27
Q

How do displacement reactions work?

A
  • more reactive metal displaces less reactive metal from compound
28
Q

How are unreactive metals (gold, silver, platinum etc) found?

A
  • in the earth’s crust
  • as pure metals
  • mined
29
Q

How are metals that are less reactive than carbon extracted?

A
  • found as ores
  • heating with carbon
  • reduction
30
Q

How are metals that are more reactive than carbon extracted?

eg. aluminium

A
  • electrolysis
31
Q

Steps for writing an ionic equation

A

1) check symbol equation is balanced
2) identify all aqueous ionic compounds
3) write those compounds out as ions
4) remove spectator ions

32
Q

What can be used to show pH?

A
  • universal indicator
  • electronic pH probes (gives exact pH)
33
Q

What is the reactivity of a metal?

A
  • its tendency to form positive ions
34
Q

What do metals produce when they react with oxygen and what reaction is it?

A
  • metal oxides
  • oxidation, metal gains oxygen
35
Q

What do reactive metals do when they react with oxygen?

A
  • burn with a flame
  • eg. magnesium
36
Q

What do unreactive metals do when they react with oxygen?

A
  • they tarnish and change colour without a flame
  • eg iron
37
Q

What do potassium, sodium and lithium do when they react with acid?

A
  • they explode
  • produce hydrogen gas
  • reacts more vigorously
38
Q

What do calcium, magnesium, zinc and iron do when they react with acid?

A
  • they fizz and give off hydrogen gas
39
Q

What does copper do when it reacts with acid?

A
  • no reaction
40
Q

What happens when potassium, sodium, lithium, and calcium do when they react with water?

A
  • they fizz and give off hydrogen gas
41
Q

What do magnesium and zinc do when they react with water?

A
  • they react very slowly
42
Q

What happens when copper reacts with water?

A
  • no reaction
43
Q

How are metals oxides that are less reactive than carbon extracted?

A
  • by reduction with carbon
  • produces carbon dioxide

Chemistry GCSE (9 decks)

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