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Chemistry P1 > C5 - Chemical Changes > Flashcards

C5 - Chemical Changes Flashcards

1
Q

What do metals and oxygen produce?

A

Metal oxides
- Metal OXIDISED
- Oxygen REDUCED

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2
Q

What is OILRIG?

A
  • Oxidation Is Loss, Reduction is Gain
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3
Q

What do metals do when they react with other substances?

A

Produce positive ions

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4
Q

What is reactivity of a metal?

A
  • Related to its tendency(how often)to form positive ions
  • Higher reactivity = quicker loss of electrons
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5
Q

What is the reactivity series? (PLEASE SEND LIONS, CATS, MONKEYS..)

A
  • Potassium
  • Sodium
  • Lithium
  • Calcium
  • Magnesium
  • Aluminium
  • Carbon
  • Zinc
  • Iron
  • Hydrogen
  • Copper
  • Gold
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6
Q

What does the reactivity series help us figure out?

A
  • A more reactive metal can displace a less reactive metal from a compound
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7
Q

What would happen if a metal reacts with water?

A
  • Metals above hydrogen produce hydrogen gas alongside metal hydroxide
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8
Q

What does metal and water produce?

A

Metal + Water –> Metal Hydroxide + Hydrogen

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9
Q

How can metals more reactive than carbon be extracted?

A

Electrolysis

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10
Q

How can metals less reactive than carbon be extracted? Give an example

A

Reduction(LOSS of oxygen) with carbon
e.g iron(III) oxide + carbon monoxide → iron + carbon dioxide

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11
Q

What would an ionic equation for displacement reactions look like?

A

Metal ions are reacting (in terms of electrons being transferred)

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12
Q

What is the ionic equation for the displacement reaction
Zn(s) + CuSO4(aq) → Cu(s) + ZnSO4(aq)?

A

Zn + Cu 2+ → Cu + Zn 2+ (ionic equation)

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13
Q

What happens in terms of electrons for zinc?

A
  • Zinc has lost electrons - so has oxidised
  • Half equation: Zn → (Zn 2+) + 2e-
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14
Q

Explain what you would observe when a metal is added to an acid

A
  • Only those above hydrogen
  • More reactive the metal = more vigorous reaction; producing hydrogen gas quicker
  • Bubbles because hydrogen gas is produced
  • Container is warm - exothermic reaction
  • Metal disappears - salt dissolves
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15
Q

What happens in terms of electrons for copper?

A
  • Copper has gained electrons - so has reduced
  • (Cu 2+) + 2e- → Cu
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16
Q

What does metal and acid produce?

A

Metal + Acid = Salt + Hydrogen

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17
Q

What would be oxidised and reduced in a reaction of acid with metal? E.G. Magnesium

A
  • Mg → (Mg 2+) + 2e-
  • magnesium is oxidised as it is losing electrons
  • (2H+) + 2e- → H2
  • hydrogen is reduced as it is gaining electrons
18
Q

What are acids neutralised by and what do they produce?

A
  • Alkalis - soluble metal hydroxides
  • Bases - insoluble metal hydroxides and metal oxides
  • Produce salts and water
  • Also metal carbonates
19
Q

What do acids and metal carbonates produce?

A

Metal Carbonate + Acid –> Salt + Water + CO2

20
Q

What does the name of the salt produced depend on?

A
  • Acid used
  • Metal in base/alkali/carbonate
21
Q

What salt would be produced in a neutralisation reaction if HYDROCHLORIC acid is used? HCl

A

____ Chloride

22
Q

What salt would be produced in a neutralisation reaction if NITRIC acid is used? HNO3

A

____ Nitrate

23
Q

What salt would be produced in a neutralisation reaction if SULFURIC acid is used? H2SO4

A

____ Sulfate

24
Q

How can soluble salts be made from acids?

A
  • Reacting them with solid insoluble substances (e.g metals, metal oxides, hydroxides or carbonates)
  • Solid is added to acid until no more reacts and excess solid is filtered off to produce a solution
25
How can you produce solid salts?
Salt solutions can be crystallised
26
RP1 - Preparation of a Pure Dry Salt 8 STEPS
1. Measure 50 cm3 acid in beaker 2. Warm the acid using bunsen burner 3. Add spatula of solid base or metal and keep adding solid until no more reacts and base is in excess 4. Filter off excess solid base using filter funnel and filter paper 5. Pour solution into evaporating basin 6. Evaporate solution using bunsen burner until crystals start to form 7. Leave to crystallise in cool place 8. Pat dry crystals on filter paper
27
What is an acid?
Produces H+ ions in aqueous solutions
28
What is an alkali?
- Produce hydroxide ions (OH-) in aqueous solutions - They are soluble hydroxides
29
What is a base?
- Neutralise acids - Metal oxides and hydroxides
30
What is the pH scale?
- Measure 0-14 of the acidity or alkalinity of a solution
31
Explain what happens in terms of ions when any acid reacts with an alkali
H+ ions react with OH- ions to make water H+(aq)+OH-(aq) --> H2O(l)
32
Describe the use of universal indicator to measure the approximate pH of a solution
- Substance which changes colour depending on the pH of the solution - Only a few drops needed
33
RP2 - Neutralisation/Titration 10 STEPS
1. Use pipette to measure 25cm3 of alkali into conical flask 2. Place conical flask on white tile 3. Fill the burette with sulphuric acid using a funnel 4. Record the initial reading of acid in the burette 5. Add 5 drops of indicator in this case phenolphthalein to the conical flask 6. Slowly open the burette tap while swirling the conical flask 7. Add acid drop-by-drop near the endpoint 8. Close the burette when a colour change occurs in phenolphthalein 9. Record the final reading of acid in the burette and calculate the titre - this is volume of acid used to neutralise the alkali 10. Repeat and calculate a mean
34
RP2 - How to calculate concentration of one of the solutions in mol/dm3
1. Calculate amount of moles (volume and concentration given) 2. Find the amount of other substance in moles(LOOK AT RATIO) 3. CONCENTRATION = MOLES/VOLUME
35
RP2 - How would you calculate the concentration in g/dm3
Mass = relative formula mass × moles
36
RP2 - Why are pipettes and burettes used in this titration practical
Pipettes - measured fixed volume accurately Burettes - measures variable volume
37
What is a strong acid? 3 examples
- Completely ionised in aq solutions - e.g hydrochloric, nitric, sulfuric
38
What is a weak acid? 3 examples
- Only partially ionised in aq solutions - Usually reversible reaction - e.g ethanoic, citric, carbonic
39
How does pH vary with strength of acid?
The stronger the acid or the higher the concentration of H+ ions, the lower the pH
40
What is a dilute solution?
- One that contains a relatively small amount of dissolved solute
41
What is a concentrated solution?
- One that contains a relatively large amount of dissolved solute

Chemistry P1 (7 decks)

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