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Chemistry - Y10 + Y11 > Chemical Changes > Flashcards

Chemical Changes Flashcards

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1
Q

OIL RIG

A

Oxidation is loss of electrons. Reduction is gain of electrons

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2
Q

Where do metals go to?

A

Cathode

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3
Q

Where do non metals go to?

A

Anode

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4
Q

What charge is the anode?

A

Positive

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5
Q

What charge is the cathode?

A

Negative

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6
Q

What is the electrolyte?

A

Molten/ dissolved ionic compound where lots of ions float.

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7
Q

What is present when a lighted splint pops?

A

Hydrogen

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8
Q

What is present when a splint relights?

A

Oxygen

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9
Q

What is present when damp blue litmus paper bleaches?

A

Chlorine

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10
Q

What does native mean? Give an example

A

When something is found naturally and pure - they don’t need to be extracted e.g gold/silver

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11
Q

Characteristics of a giant ionic lattice

A
  • V high melting points - lots of energy to overcome strong electrostatic force of attraction
  • Brittle - Break easily due to repulsion (like charges repel)
  • Conduct electricity when they are dissolved/molten as ions can move
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12
Q

Ionic Formula

What charge is an ionic compound, why?

A

Neutral because the charges cancel each other out

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13
Q

Where does reduction happen?

A

Cathode - gain electrons

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14
Q

Where does oxidation happen?

A

Anode - lose electrons

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15
Q

What state should an element/compound be in to split up in ionic equations?

A

Aqueous

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16
Q

Which is easier to discharge, less or more reactive?

A

Less reactive

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17
Q

+Ions - What is the rule for what is discharged at the cathode?

A

Metals of lower reactivity > hydrogen
Metals of higher reactivity < hydrogen

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18
Q

-Ions - What is the rule for what is discharged at the anode?

A

Halide ions (Group 7) > oxygen
Other ions (e.g SO4) < oxygen

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19
Q

How can you measure the pH of a solution?

A
  • pH probe
  • Universal indicator
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20
Q

Reaction for neutralisation (word)

A

Acid + Alkali -> Salt + Water

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21
Q

Reaction for neutralisation (symbol) include state symbols

A

H⁺₍ₐq₎+OH⁻₍ₐq₎ –> H₂O₍ₗ₎

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22
Q

What are titrations and what do they do?

A

Method of analysing concentrations of solutions, tells you exactly how much acid/alkali is needed to neutralise

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23
Q

8 steps

Explain the steps for titrations

A
  1. Use pipette and pipette filler and set a volume of alkali to a conical flask with 2/3 drops of indicator
  2. Use a funnel and fill a burette with acid of known concentration - BELOW EYE LEVEL
  3. Record acid level in burette
  4. Add acid to alkali a bit at a time - give conical flash regular swirls
  5. Go slowly when you think it’s near the end-point (colour change)
  6. Record final volume of acid in burette
  7. Repeat
  8. Calculate mean ignoring anamolies
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24
Q

Why should you repeat titrations?

A

The first reading is a rough reading - gives you an idea of where the solution changes colour. Repeat the whole thing a few times to get the same answer

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25
Q

By what factor does the concentration of H⁺ increase when you go down the pH scale?

A

10

26
Q

5 Steps

Soluble salts practical

A
  1. Gently warm dilute acid using a Bunsen Burner
  2. Add insoluble base to acid a bit at a time, until no more reacts (add excess so all acid reacts - excesss sinks to base)
  3. Filter out excess solid to get the salt solution
  4. Gently heat the solution using a water bath to evaporate water (make it more concentrated) and then stop heating and let it cool
  5. Crystals form which can be filtered out and then dried - crystallisation
27
Q

Electrolysis Practical

A
  1. Pour solution into beaker
  2. Place petri dish over beaker
  3. Insert carbon graphite rods into each hole in petri dish
  4. Electrodes shouldn’t touch each other or else it will produce a short-circuit
  5. Attach crocidle leads to rods
  6. Connect rods to terminals of a low-voltage power supply (4V)
  7. Check for hydrogen (squeaky pop), chlorine (blue litmus paper bleaches)
28
Q

What is cryolite?

A

Aluminium compound with lower melting point than aluminium oxide - reduces cost

29
Q

Where is alumnium extracted from?

A

The ore bauxite by electrolysis

30
Q

How can we test for metal hydroxide?

A

Litmus paper turns blue OR universal indicator turns purple

31
Q

What is a use of chlorine?

A

To make bleach

32
Q

Why should carbon anodes be replaced regularly?

A

Oxygen produced at hot anodes reacts with carbon to produce carbon dioxide that burns away anodes

33
Q

What happens when iron reacts with copper sulfate?

A

Copper turns brown and solution turns pale green

34
Q

In electrolysis, which direction do the electron travel?

A

Anode to cathode

35
Q

Why is electrolysis expensive, 2 reasons?

A
  • Melting compounds like AlO2 needs a lot of energy
  • Lot of energy is needed to produce the electric current
36
Q

Cathode half equation for copper sulfate (aq)

A

Cu²⁺ + 2e⁻ -> Cu

37
Q

Anode half equation for copper sulfate (aq)

A

4OH⁻ -> O₂ + 2H₂O + 4e⁻

38
Q

Formula for calcium carbonate

A

CaCO3

39
Q

Formula for sodium hydroxide

A

NaOH

40
Q

Formula for sulfuric acid

A

H2SO4

41
Q

Formula for nitric acid

A

HNO3

42
Q

What does litmus paper turn into in acidic and alkaline solutions?

A

Acidic = red
alkaline = blue

43
Q

What does phenolphthalein turn into in acidic and alkaline solutions?

A

Acidic = colourless
Alkaline = pink

44
Q

What does methyl orange turn into in acidic and alkaline solutions?

A

Acidic = red
Alkaline = yellow

45
Q

true or false? The dissociation of weak acids is a reversible reaction, which means that the products can react together to reform the acid.

A

true

46
Q

For a weak acid, does the position of equilibrium lie to the left or the right?

A

left

47
Q

What are strong acids?

A
  • Ionise completely in water
    *
48
Q

What are weak acids?

A
  • They do not fully ionise in solution
  • Only small prop of acid particles dissociate to release hydrogen ions
49
Q

What is important about the ionisation of weak acid?

A

Its reversible, which sets up an equilibrium between undissociated and dissociated aicd
since only a few acid particles release H ions, equilibrium lies on the left

50
Q

Are strong acids more reactive than weak acids of the same conc.?
Why?

A

Yes, if the conc H ions is higher, the rate of reaction will be faster

51
Q

What is acid strength?

A

Tells you what prop. of the acid molecules ionise in water

52
Q

What is acid conc?

A

Tells you how much acid there is in a certain volume of water

53
Q

Acid + metal oxide =

A

salt + water

54
Q

acid + metal hydroxide =

A

salt + water

55
Q

acid + carbonate

A

salt + water + carbon dioxide

56
Q

Reactivity series

A
  • Potassium
  • Sodium
  • Lithium
  • Calcium
  • Magneisum
  • Carbon
  • ZInc
  • Iron
  • Hydrogen
  • Copper
57
Q

Acid + Metal

A

Salt + hydrogen

58
Q

How can you measure the reactivity of metals by measuring what?

A
  • Number of bubbles
  • Temp change - most reactive = most heat
  • Make sure it has the same mass/sa
59
Q

metal + water

A

metal hydroxide + hydrogen

60
Q

What metals dont react with water

A

zinc, iron, cu

61
Q

Do metals react more violently with water or acid?

A

acid

62
Q

Why do we find pure gold in the ground, but not pure iron?

A
  • Gold is unreactive, so doesnt react with other elements
  • Iron is reactive enough to react with oxyen so is oxidised to iron oxide

Chemistry - Y10 + Y11 (9 decks)

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