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Chemistry > Unit 17, 18 & 19 - Groups in the Periodic Table/ Rates of Reaction/ Heat Energy Changes in Chemical Reactions > Flashcards

Unit 17, 18 & 19 - Groups in the Periodic Table/ Rates of Reaction/ Heat Energy Changes in Chemical Reactions Flashcards

1
Q

What and the group 1 elements called

A

Alkali metals

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2
Q

Give 2 properties of alkali metals that are different to normal metals

A

Low melting points, soft and easy to cut

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3
Q

What happens to alkali metals when they are burned in air

A

They are oxidised

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4
Q

Which way does the reactivity of alkali metals go?

A

More reactive further down

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5
Q

Why are alkali metals with more shells more reactive

A

It is easier for the electron to be lost

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6
Q

What are group 7 elements called

A

Halogens

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7
Q

What type of molecules do halogens exist as

A

Diatomic

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8
Q

Why do halogens need to be handled with care

A

They are toxic and corrosive

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9
Q

What does chlorine look like

A

A green has

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10
Q

What does iodine look like

A

Purple/ black solid

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11
Q

What does bromine look like

A

Brown liquid

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12
Q

What is formed when a halogen reacts with metals

A

Salts with halide ions

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13
Q

Give a halide salt and what it is used for

A

Sodium chloride, table salt

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14
Q

Why can all halogens be used as disinfectants and bleaches

A

They kill microorganisms and remove colour

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15
Q

What is the test for chlorine

A

Turns damp blue litmus paper red then bleached

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16
Q

What is formed when halogens react with hydrogen

A

Hydrogen halides which form an acid

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17
Q

How is HCl acid made

A

Hydrogen gas and chlorine gas react to form hydrogen chloride, when dissolved in water, the ions disassociate so the H+ ions make it an acid

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18
Q

Which way are the halogens more reactive

A

As you go up the table

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19
Q

How can the order of halogens be worked out

A

Using displacement reactions

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20
Q

Why do halogens with less shells react more

A

It is easier to gain an electron

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21
Q

What is a redox reaction

A

When a reaction has oxidation and reduction

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22
Q

What are group 0 elements called

A

Noble gases

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23
Q

Give 3 properties of noble gases

A

Colourless
Low melting points
Poor conductors

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24
Q

What is a unique property of noble gases

A

Inert, don’t react easily

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25
Q

Why do noble gases all exist as single atoms

A

Don’t form bonds easily

26
Q

What is krypton used for

A

Photography lighting because it produces a white light when electricity passes through it

27
Q

What is argon used for

A

Stops oxygen reacting with wine between cork and wine as it is dense than air

28
Q

What is helium used for

A

Weather balloons as it has a low density and is non flammable

29
Q

What is neon used for

A

Making illuminated signs as it produces red-orange light when electricity is passed through it

30
Q

Why are noble gases inter

A

They have full outer shells

31
Q

What is the rate of reaction?

A

The speed at which reactants are turns into products

32
Q

How can we control the rates of reaction

A

By altering variables

33
Q

Why do granules of magnesium react faster than a ribbon

A

Their surface area is bigger

34
Q

What is the activation energy

A

The minimum amount of energy needed for a reaction to occur

35
Q

What is an exothermic reaction

A

A reaction which releases energy

36
Q

What are endothermic reactions

A

Reactions where energy is taken in

37
Q

Give an example of an endothermic reaction

A

Electrolysis of copper chloride

38
Q

What 4 factors affect the rate of a reaction

A

Concentration, surface area, pressure of gases, temperature

39
Q

Why does the concentration affect the rate of reaction

A

When it increases, there are more particles so collisions occur more often

40
Q

How does surface area affect the rate of reaction

A

If it increases, the rate increases as there is more surface for collisions

41
Q

How does pressure of gases affect the rate of a reaction

A

Increased pressure means the particles are closer together so collide more

42
Q

How does temperature affect the rate of a reaction

A

Increased temperature means they particles move faster so collide more often

43
Q

Explain the core practical - Investigating reaction rates, measuring volumes of gases

A

Set up conical flask with bung and delivery tube
Attach the delivery tube to a set up for measuring gas
Add 40cm3 of hcl and 5g of marble chips to the conical flask
Note how much gas is produced every 30 seconds
Repeat with larger marble chips

44
Q

Explain the core practical - Investigating reaction rates, observing colour change

A

Place 50cm3 of sodium thiosulphate solution into a conical flask
Measure 5cm3 of dilute hcl in a test tube
Place both the conical flask and test tube in a water bath and note down temperature
After 5 mins, remove and place flask on paper with a cross drawn
Add acid and measure how long it takes for cross to disappear
Repeat with different temperatures

45
Q

What are catalysts

A

Substances that speed up chemical reactions without being permanently changed

46
Q

What catalyst is used in the manufacture of nitric acid from ammonia

A

Platinum

47
Q

Why don’t catalysts need to be replaced

A

They don’t get used up

48
Q

How do catalysts save costs

A

They allow reactions to occur at lower temperatures

49
Q

How does a catalyst make a reaction faster

A

The activation energy is lower so more molecules have enough energy to react

50
Q

What are enzymes

A

Biological catalysts made from proteins

51
Q

What is the active site

A

The specific shape in an enzyme where the substrate fits into

52
Q

What is the enzyme for alcoholic drinks

A

Yeast

53
Q

What does a reaction model show

A

The energy change during a chemical reaction

54
Q

How can you determine whether a reaction in a solution is exothermic or endothermic?

A

If it is exothermic, the temperature increases in the solution

55
Q

Which 2 types of reactions are always exothermic?

A

Neutralisation and displacement

56
Q

Give a type of reaction that has a low activation energy

A

Precipitation

57
Q

What yep of reaction has a high activation energy

A

Combustion

58
Q

What is bond energy

A

The average energy needed to break once mole of a particular bond

59
Q

Which part of a reaction is exothermic

A

Making the bonds

60
Q

Which part of a reaction is endothermic

A

Breaking the bonds

61
Q

How do you calculate energy change

A

Energy change = energy in - energy out

62
Q

What is bond energy measured in

A

KJ/ mol

Chemistry (12 decks)

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