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Chemistry - Y10 + Y11 > Chemical Changes > Flashcards

Chemical Changes Flashcards

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

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

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

19
Q

How can you measure the pH of a solution?

A
  • pH probe
  • Universal indicator
20
Q

Reaction for neutralisation (word)

A

Acid + Alkali -> Salt + Water

21
Q

Reaction for neutralisation (symbol) include state symbols

A

H⁺₍ₐq₎+OH⁻₍ₐq₎ –> H₂O₍ₗ₎

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

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
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

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

Chemistry - Y10 + Y11 (5 decks)

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