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Chemistry GCSE > Topics I need to improve on or weak topics > Flashcards

Topics I need to improve on or weak topics Flashcards

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1
Q

Who realised that electrons orbit in shells and were specific distances away?

A

Neil Bohr

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2
Q

What is the plum pudding model?

A

that the middle of an atom is positive and surrounded by negative charge

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3
Q

What conclusions did Rutherford draw from his alpha scattering experiment?

A

That an atom is mainly open space as most alpha particles passed straight through, centeral mass as some rebounded back, the nucleus is positive as some of the alpha particles (positive ions) were deflected in its path

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4
Q

Who first discovered electrons?

A

JJ Thompson

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5
Q

Who first said that everything is made up of particles called atoms?

A

John Dalton

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6
Q

What was fired at very thin gold
foil, which led to the nuclear
model of the atom?

A

Helium nuclei (alpha
particles).
These are positive ions.

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7
Q

What is the formula for propene?

A

C3H6

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8
Q

Do thermosetting or thermosoftening polymers melt when heated?

A

thermosoftening

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9
Q

What non metal makes up steel?

A

carbon

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10
Q

What two metal are in brass

A

copper and zinc

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11
Q

what two metals are in bronze

A

copper and tin

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12
Q

How to prevent corrosion

A

greasing, painting, electroplating, galvarising

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13
Q

How can we reduce use of worlds resources

A

reuse and recycle

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14
Q

What does LCA stand for

A

life cycle assesment

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15
Q

4 stages of process of sewage treatment

A
  1. screening 2. sedimentation 3.anaerbobic digestion of sludge 4. aerobic treatment
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16
Q

why is potable water not necassarily pure water?

A

contains dissolved substances

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17
Q

name a sterilising agent for sterilising potable water

A

chlorine, ozone, UV light

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18
Q

What pollutant causes acid rain?

A

sulfuric/nitric acid

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19
Q

What two things reduced the amount of carbon dioxide in the earths early atmosphere?

A

photosynthisis, formation o sedimentary rocks and fossil fuels

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20
Q

What happens to the reactivity of elements in the halogens as they get further down?

A

The reactivity decreases

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21
Q

What state is flourine at room temp

A

gas

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22
Q

What state is bromine at room temp

A

liquid

23
Q

What state is iodine at room temp

A

solid

24
Q

Why are group 1 called alkali metals

A

Because they react with water to form alkalis

25
Q

why do ions with a 1+ charge and a -1 charge form a bond

A

electrostatic attraction between oppisitely charged ions

26
Q

define giant ionic lattice

A

a 3d network of ions

27
Q

why do ionic substances conduct electricity when molten or dissolved in water

A

ions are free to move

28
Q

define an aqueous soloution

A

something dissolved in water

29
Q

What is the 3 main acids

A

hydrochloric nitric and sulfuric

30
Q

What is the formula for sulfuric acid

A

HSO

31
Q

What is the formula for nitric acid

A

HNO

32
Q

What ions does HCl form in a solution

A

H and Cl

33
Q

What ions does HSO form in a solution

A

H2 and SO2

34
Q

What ions does HNO form in a solution

A

H and NO

35
Q

How to measure pH

A

indicator or a pH probe

36
Q

What is a base

A

a metal oxide hydroxide or carbonate that reacts with an acid

37
Q

what is a salt

A

a compound when some or all of the hydrogen is replaced by a metal

38
Q

what are the products of a metal oxide and an acid

A

salt and water

39
Q

products of metal carbonate and an acid

A

salt and water and carbon dioxide

40
Q

How can metals be placed in order of their reactivity

A

add the metals to water or acid see which ones react the most on how much fizzing there is for example

41
Q

Why can gold and silver be found naturally in the earths crust

A

its very unreactive

42
Q

Define an ore

A

a material containing enough metal for it to be worthwhile to extract the metal from it

43
Q

for the extraction of metals when is electrolysis needed

A

when the metal is more reactive than carbon

44
Q

Why is aluminium oxide mixed with cryolite when extracting aluminium?

A

to lower the melting point

45
Q

Why does the anode need to be replaced in the electrolysis of aluminium oxide

A

because the oxygen reacts with the carbon to produce co2

46
Q

What is produced at the cathode in electrolysis of solutions

A

the metal is produced at the cathode if it is less reactive than hydrogen

47
Q

What is produced at the anode in electrolysis of solutions

A

either a halogen or oxygen if halogen is not present

48
Q

Give two examples of endothermic

reactions.

A

Thermal decomposition reactions, citric acid and

sodium hydrogencarbonate.

49
Q

State two uses of exothermic reactions

A

hand warmers and self heating cans

50
Q

State two uses of endothermic reactions

A

sports injury cool pack

51
Q

What is a reaction profile?

A

A diagram to see wether the reactants in a reaction have more or less energy than the products

52
Q

Is breaking bonds endothermic or

exothermic?

A

endothermic because energy is needed as bonds are strong

53
Q

How do we work out the overall energy

change of a reaction?

A

difference between energy needed to break all the bonds of the reactants and energy released to form all the bonds in the products

Chemistry GCSE (11 decks)

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