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GCSE Chemistry OCR A > C4 > Flashcards

C4 Flashcards

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1
Q

Describe the group 1 physical & chemical properties:

A

1️⃣shiny when freshly cut
1️⃣solid state at RT
1️⃣soft
1️⃣ conducts of electricity

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2
Q

What is the trend of group 1 metals going down the group?

A

1️⃣ density increases
1️⃣ melting point decreases
1️⃣ reactivity increases (fizzes —> flames)

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3
Q

Why do group 1 elements get more reactive down the group?

A

Want to loose 1 outer electron
Larger Atomic radius = weaker force of attraction
Shielding (more electron shells in way) = weaker force

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4
Q

What do group 1 metals produce when they react with water?

A

Hydrogen and an alkali (metal hydroxide)

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5
Q

What are some chemical and physical properties of group 7 elements?

A

7️⃣brittle
7️⃣poor conductors
7️⃣DIATOMIC

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6
Q

How does fluorine appear in RT?

A

A pale yellow gas (F2)

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7
Q

How does chlorine appear in RT?

A

Cl2
A green gas

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8
Q

How does bromine appear in RT?

A

An orange / brown liquid (Br2)
Vaporises easily

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9
Q

How does Iodine (I2) appear at RT?

A

A shiny grey- black crystalline solid

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10
Q

What are the trend of group 7 , going down the group?

A

7️⃣density increases
7️⃣MP/BP increase
7️⃣ reactivity decreases

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11
Q

What do halogens produce when reacting with metals?

A

Salt

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12
Q

Why does the reactivity decrease when going down the group?

A

Must gain 2 electrons
More atomic radius = weaker forces of attraction
More shielding = weaker forces of attraction
More shells , makes it harder to attract 2 electrons

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13
Q

Why do halogens displace other halogens?

A

If they are more reactive (more higher on in the group) then they kick the other out

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14
Q

What are some chemical and physical properties of group 0 elements

A

0️⃣all gasses at RT
0️⃣so un reactive (full outer shells)
0️⃣non metals
0️⃣monatomic
0️⃣low BPs

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15
Q

What is the trend of group 0 going down the group?

A

Boiling point increases (attractive forces between atoms are stronger)
Boiling point increases

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16
Q

What are some properties of transition metals?

A

Shiny when freshly cut
Good conductors of electricity
Strong
Malleable

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17
Q

Describe the transition metals in comparison to group 1

A

More dense
More stronger /harder
Higher melting points
Also less reactive

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18
Q

What are some chemical properties of transition metals?

A

💚Less reactive than group 1
💚Produce coloured ionic compounds
💚Can have multiple charges
💚Good catalyst
💚 resistant to corrosion (not so reactive)

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19
Q

What is the reactivity series?

A

Potassium
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Tin
Lead

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20
Q

What does the rate of reaction tell you?

A

The order of reactivity
More reactive = greater rate of hydrogen production

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21
Q

Do group 0 react?

A

NOPE
Full outer shell and so won’t easily give up or gain electrons

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22
Q

Which are least reactive out of group 1, group 2 and transition metals

A

Transition metals

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23
Q

How do you test for oxygen?

A

Place a glowing splint near the mouth of the container of gas
If oxygen is present the splint should relight

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24
Q

How do you test for hydrogen?

A

Place a lighted splint near the mouth of the container.
If hydrogen is present it should ignite with a squeaky pop

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25
Q

How do you test for carbon dioxide ?

A

Use limewater (calcium hydroxide).
If it turns cloudy when carbon dioxide is bubbled through then it is present.
White precipitate = calcium carbonate

26
Q

How do you test for chlorine?

A
  1. Dampen the blue litmus paper
  2. Put it near, should turn red then white(bleeches )
    Chlorine + water =acidic solution
27
Q

What colour is lithium in the flame test?

A

Red

28
Q

What colour is sodium in the flame test?

A

Yellow

29
Q

What colour is potassium in the flame test?

A

Lilac

30
Q

What colour is calcium in the flame test?

A

Orange-red

31
Q

What colour is copper in the flame test?

A

Green-blue

32
Q

Why do metal ions create a colour when heated?(excitation)

A

Energy is transferred to the electrons
They move to higher shells , and then move back down
As they do radiation is emitted in the form of visible light

33
Q

How do you carry out a flame test?

A

Clean Nichrome wire loop in HCL and distilled water, hold it in the flame until it stops changing colour.
1.dip the loop into the test powder.
2. Hold it in the blue roaring flame
3. note the colour

34
Q

Why is sodium hydroxide solution used in experiments?

A

Group 1 hydroxides are soluable in water

35
Q

What colour does iron (ll) make in the sodium hydroxide tests?

A

Green

36
Q

What colour does iron (lll) make in the sodium hydroxide tests?

A

Orange - brown

37
Q

What colour does copper(ll) make in the sodium hydroxide tests?

A

Blue

38
Q

What colour does calcium make in the sodium hydroxide tests?

A

A white precipitate that does NOT a dissolve in excess
*remains white

39
Q

What colour does zinc make in the sodium hydroxide tests?

A

A white precipitate that DOES dissolve in excess.
Goes from white to colourless

40
Q

How do you detect sulfate ions?

A

Add HCL
Add barium chloride

If present then should get an insoluble white precipitate (barium sulphate)

41
Q

How do you detect carbonate ions?

A

Add a few drops of dilute hydrochloric acid
*should produce bubbles

If present there should be bubbling of carbon dioxide being released

2H+ (aq) + CO3 2-(aq) —> CO2 (g) + H2O (l)

42
Q

How do you detect halide ions?

A

Add a few drops of nitric acids
Then add a few drops of silver nitrate solution

43
Q

What colour Is the precipitate of silver chloride?

A

Whitw

44
Q

What is the colour of silver bromide?

A

Cream

45
Q

What is the colour of silver iodide precipitate ?

A

Yellow

46
Q

What is the reaction for the copper hydroxide(product)?

A

CuSo4 (aq) + 2NaOH(aq) —> Cu(OH)2 (s) + Na2SO4 (aq)

Net ionic equation:
Cu 2+ (aq) + OH- (aq) —> cu(OH)2 (s)

47
Q

What are the advantages of instrumental methods of analysis?

A

🟢speed
🟢accuracy : more decimal points
🟢sensitivity: a small amount can be used

48
Q

How do you interpret a mass spectrometer?

A

The x axis (mass to charge ratio) is just the mr
1. Look at the last peak on the graph, this is the relative formula of the entire substance

49
Q

What is formed when a metal and water react?

A

Metal + water —> metal hydroxide + hydrogen

50
Q

Why might a precipitate reaction occur really fast?

A

The collision frequency is high

51
Q

What would you observe if a Grp 1 metal is added to water?

A

🟣floats on surface
🟣fizzing
🟣the flame of hydrogen ignites
🟣melts as reacts

52
Q

What is a metal and steam form?

A

🤨
Metal+ steam —> metal oxide + hydrogen
Metal + H20–> metalO + H2

Weird coz it’s water but no hydroxide

53
Q

Why might some experiments be made in a fume cupboard?

A

The gas produced could be TOXIC

¥toxic by Britney Spears 💋

54
Q

Why does the reactivity increase going down group 1 (2marks)?

A

🟢more shielding
🟢’outer electron’ is lost more easily

55
Q

Why is nitric acid added before silver nitrate?

A

To make sure there are no carbonate ions present

56
Q

Which metals react with acids and water and why are their reactions?

A

Metals that are more reactive than hydrogen can displace the hydrogen

57
Q

HOw would you know if a metal is more reactive?

A

Greater RATE of hydrogen production

58
Q

Why must the blue litmus paper be dampened for a chlorine test?

A

So that the water can dissolve the chlorine, allowing it to react with the indicator

59
Q

Mass spectrometer

A
60
Q

Gas chromatograph

A

GCSE Chemistry OCR A (10 decks)

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