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additional chemistry > Topic 5 > Flashcards

Topic 5 Flashcards

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1
Q

What group are halogens in

A

Group 7

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2
Q

Halogens have…….properties

A

Similar

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3
Q

Name properties of chlorine(halogen)

A

Fairly reactive
Poisonous
Dense green gas

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4
Q

Name properties of bromine

A

Dense
Poisonous
Orange liquid

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5
Q

Name properties of iodine

A

Dark gray

Crystallised solid

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6
Q

What do halogens when react with metals form

A

Metal halides

E.g metals iron, aluminium

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7
Q

What do halogens form when reacted with hydrogen

A

Hydrogen halides

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8
Q

Are halogens soluble or insoluble and what do they form in water

A

Soluble

Form Acidic solutions

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9
Q

The higher up group 7 the…(halogens)

A

More reactive as outer shell nearer to nucleus

Pull apart from positive nucleus is greater which attracts extra electrons more strongly

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10
Q

How do more reactive halogens displace less reactive ones in reactions

A

When halides dissolve in water halide ions are free to react

More reactive halogen reacts with a solution containing halide ions it will “push out”(displace) less reactive halogen

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11
Q

How are Nobel gases seen at room temperature

A

Are all colourless gases

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12
Q

Why are very few Nobel gases reactive

A

Because have full outer shells

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13
Q

What happens to the boiling points as you go down the group

A

They increase

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14
Q

How where Nobel gases discovered

A

When chemists noticed that the density of nitrogen made in chemical reactions was different to that of nitrogen taken from the air

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15
Q

What is argon used for and why (Noble gas)

A

Is inert and non flammable so used in filament lamps to stop filament burning away
Protects metals being welded as inert atmosphere stops the hot metal reacting with oxygen

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16
Q

What is helium used for and why (noble gas)

A

In airships and party balloons because lower density than air so will float

17
Q

What happens in chemical reactions

A

Energy is usually transfused to and from the surroundings making and breaking bonds

18
Q

What is always needed to break bonds

A

Energy

19
Q

What happens in and exoteric reaction

A

Overall gives out energy to the surroundings intdhe form of heat shown in a rise in temperature

20
Q

Give an example of two reactions that give out heat (exothermic)

A

Burning fuels

Explosions

21
Q

What is an endothermic reaction

A

One which overall takes in energy shown in a fall in temperature

22
Q

Give two examples of endothermic reactions

A

Photosynthesis

Ammonium nitrate

23
Q

What is more common endothermic or exothermic

A

Exothermic

24
Q

What would an exothermic graph look like and why

A

Initial rise due to energy needed to break old bonds the decrease in temp as heat is given out in the reaction putting the product at a lower temp

25
Q

What would an endothermic reaction look like on a graph and why

A

Product at a higher energy than reactant showing the energy taken in during the reaction

26
Q

What are the four ways of measuring temperature change in a reaction

A

Dissolved salts
Neutralisation
Displacement
Precipitation reactions

27
Q

How would you reduce heat loss to surroundings in a reaction

A

Put polystyrene cup in beaker with wool to give insulation

Put lid on to reduce energy loss by evaporation

28
Q

Name the three different rates of reactions and examples of them

A

Slowest- rusting of iron
Moderate- a metal reacting with an acid
Fast- explosion

29
Q

What do the rates of reaction depend on

A

Temperature
Concentration or pressure(for gases)
Catalysts
Surface area

30
Q

What does the reaction of hydrochloric acid and marble chips produce and what is the catalyst

A

CO2

Marble chips

31
Q

Name two independent variable that would change the rate of reaction of marble chips and hydrochloric acid

A

Surface area do marble chips

Concentration of HCL

32
Q

What will a higher temp change of an experiment and give an example

A

Will produce quicker reaction
Will produce cloudy precipitate that will cause a black mark in test tube to disappear which you can time how long it takes to disappear
E.g Sodium thiosulfate and HCL or marble chip and HCL

33
Q

What is a catalyst

A

Something that speeds up the rate of reaction but is not used up in the reaction

34
Q

What is the advantages of using a catalysts

A

Lower energy required
Increase rate of reaction
Increase temp without rate of reaction dropping

35
Q

A use of catalysts

A

Catalytic converters in cars- vehicle exhausts can give of toxic gas Carbon monoxide
Increases the amount of time it takes for carbon monoxide to react with O2 in air to produce CO2 and H2O

36
Q

What is collision theory

A

Rate of reactions depend on how often and how hard reacting particles collide with each other

37
Q

Faster collisions are only caused by

A

Increase in temperature

38
Q

Name three collision to change the rate of reaction

A

Concentration (pressure for gases)
Temperature
Surface area
Catalyst

additional chemistry (4 decks)

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