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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

(62 cards)

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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
Why do noble gases all exist as single atoms
Don’t form bonds easily
26
What is krypton used for
Photography lighting because it produces a white light when electricity passes through it
27
What is argon used for
Stops oxygen reacting with wine between cork and wine as it is dense than air
28
What is helium used for
Weather balloons as it has a low density and is non flammable
29
What is neon used for
Making illuminated signs as it produces red-orange light when electricity is passed through it
30
Why are noble gases inter
They have full outer shells
31
What is the rate of reaction?
The speed at which reactants are turns into products
32
How can we control the rates of reaction
By altering variables
33
Why do granules of magnesium react faster than a ribbon
Their surface area is bigger
34
What is the activation energy
The minimum amount of energy needed for a reaction to occur
35
What is an exothermic reaction
A reaction which releases energy
36
What are endothermic reactions
Reactions where energy is taken in
37
Give an example of an endothermic reaction
Electrolysis of copper chloride
38
What 4 factors affect the rate of a reaction
Concentration, surface area, pressure of gases, temperature
39
Why does the concentration affect the rate of reaction
When it increases, there are more particles so collisions occur more often
40
How does surface area affect the rate of reaction
If it increases, the rate increases as there is more surface for collisions
41
How does pressure of gases affect the rate of a reaction
Increased pressure means the particles are closer together so collide more
42
How does temperature affect the rate of a reaction
Increased temperature means they particles move faster so collide more often
43
Explain the core practical - Investigating reaction rates, measuring volumes of gases
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
Explain the core practical - Investigating reaction rates, observing colour change
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
What are catalysts
Substances that speed up chemical reactions without being permanently changed
46
What catalyst is used in the manufacture of nitric acid from ammonia
Platinum
47
Why don’t catalysts need to be replaced
They don’t get used up
48
How do catalysts save costs
They allow reactions to occur at lower temperatures
49
How does a catalyst make a reaction faster
The activation energy is lower so more molecules have enough energy to react
50
What are enzymes
Biological catalysts made from proteins
51
What is the active site
The specific shape in an enzyme where the substrate fits into
52
What is the enzyme for alcoholic drinks
Yeast
53
What does a reaction model show
The energy change during a chemical reaction
54
How can you determine whether a reaction in a solution is exothermic or endothermic?
If it is exothermic, the temperature increases in the solution
55
Which 2 types of reactions are always exothermic?
Neutralisation and displacement
56
Give a type of reaction that has a low activation energy
Precipitation
57
What yep of reaction has a high activation energy
Combustion
58
What is bond energy
The average energy needed to break once mole of a particular bond
59
Which part of a reaction is exothermic
Making the bonds
60
Which part of a reaction is endothermic
Breaking the bonds
61
How do you calculate energy change
Energy change = energy in - energy out
62
What is bond energy measured in
KJ/ mol

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