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Chemistry > PAPER 1 GCSE > Flashcards

PAPER 1 GCSE Flashcards

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1
Q

Arrangement of solids

A

Particles are close together and regularly packed

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2
Q

Movement of solids

A

Particles vibrate around a fixed point

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3
Q

Energy of solids

A

Particles have less kinetic energy than both liquids and gasses

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4
Q

Arrangement of liquid

A

Particles are close together but irregular.

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5
Q

Movement of liquids

A

Particles are free to move

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6
Q

Energy of liquids

A

Particles have less kinetic energy than gasses but more than solids

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7
Q

Arrangement of gas

A

Particles are far apart and there are no forces between them

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8
Q

Movement of gas

A

Particles are free to move

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9
Q

Energy of gas

A

Particles have more kinetic energy than liquids and solids.

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10
Q

Melting

A

When a solid is heated, the energy makes the particles vibrate fast enough so that the forces of attraction between the particles break

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11
Q

Freezing

A

When a liquid is cooled, the particles move slow enough so that the forces of attraction between them will hold them into a solid

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12
Q

Boiling

A

When a liquid is heated strongly, the energy makes the particles move fast enough so that all forces of attraction are broken

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13
Q

Condensing

A

When a gas is cooled, the particles move slow enough so that the forces of attraction between them will hold them as a liquid

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14
Q

understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained

A

Diffusion is the spreading out of particles in a gas or liquid. There is a net movement of particles from areas of high concentration to areas of low concentration until a uniform concentration is achieved

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15
Q

Solvent

A

the liquid in which it dissolves

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16
Q

Solute

A

the substance that dissolves

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17
Q

Solution

A

The liquid that forms after dissolving

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18
Q

Saturated solution

A

solution into which no more solute can be dissolved

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19
Q

What is the atom

A

An atom is the smallest part of an element.

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20
Q

Molecule

A

molecule is made of a fixed number of atoms covalently bonded together

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21
Q

Atomic number

A

The number of protons in an atom

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22
Q

Mass number

A

The number of protons and neutrons in an atom

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23
Q

Relative atomic mass

A

The average mass of an atom compared to 1/12th the mass of carbon-12

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24
Q

Isotopes

A

Atoms of the same element (same number of protons) but with a different number of neutrons

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25
Q

What is a mol

A

The mass of 1 mole of a substance is the relative formula mass (Mr) of the substance in grams

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26
Q

What is yield

A

Yield is how much product you get from a chemical reaction

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27
Q

Theoretical yield

A

the amount of product that you would expect to get

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28
Q

How to calculate the actual yield

A

Actual amount / theoretical amount

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29
Q

Finding the formula of a metal oxide experimentally

A

reacting a metal with oxygen and recording the mass changes.

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30
Q

Finding the formula of a salt containing water of crystallisation

A

When some substances crystallise from solution, water becomes chemically bound up with the salt. This is called water of crystallisation
The difference of mass before and after heating is the mass of the water lost

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31
Q

What is the empirical formula

A

shows the simplest whole-number ratio between atoms/ions in a compound

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32
Q

What is the molecular formula

A

shows the actual number of atoms of each type of element in a molecule.

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33
Q

What is a covalent bond

A

ESFOA between the nuclei and the shared pairs of electrons

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34
Q

How is covalent bond formed

A

A covalent bond is formed between two non - metal atoms by sharing a pair of electrons in order to fill the outer shell

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35
Q

Why do simple molecular substances have a low boiling point

A

between the molecules are weak intermolecular forces of attraction that require little energy to break

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36
Q

explain why the melting and boiling points of substances with simple molecular structures increase, in general, with increasing relative molecular mass

A

because larger molecules (molecules with more mass) have more forces of attraction between them. These forces, although weak, must be overcome if the substance is to boil, and larger molecules have more attractions which must be overcome.

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37
Q

why substances with giant covalent structures are solids with high melting and boiling points

A

it is a giant covalent structure with many strong covalent bonds that require a lot of energy to break.

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38
Q

Why is diamond hard

A

is a giant covalent structure with many strong covalent bonds that require a lot of energy to break

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39
Q

Why can graphite conduct electricity

A

because the delocalised electrons are free to move

each carbon atom has one electron not involved in a covalent bond, and these electrons form a sea of delocalised electrons between the layers

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40
Q

Why is graphite soft and slippery

A

Each layer is a giant structure, with weak forces of attraction between the layers. These layers can easily slide over each other

41
Q

Why do covalent compounds usually not conduct electricity

A

Electric current is a flow of charged particles that can move.

Covalent compounds do not conduct electricity.

42
Q

Percentage of nitrogen in air

A

78 percentage

43
Q

Percentage of oxygen in air

A

21 percent

44
Q

Percentage of argon in air

A

0.9

45
Q

Percentage of CO2 in air

A

0.04

46
Q

How to use carbon to determine the percentage of oxygen in air

A

The copper is in excess and uses up the oxygen to form copper oxide (CuO).
All the oxygen in the air is therefore used up, and so the volume of the air decreases by about 20% (the percentage of oxygen in air).

47
Q

How to use iron to determine the percentage of oxygen in air

A

The iron reacts with the oxygen in the air (rusting).

As long as the iron and water are in excess, the total volume of air enclosed by the apparatus decreases by about a fifth (20%) over several days.

48
Q

How to use phosphorus to determine the percentage of oxygen in air

A

The phosphorus is lit with a hot wire.

It reacts with the oxygen in the air and causes the water level in the bell jar to rise by about 20%.

49
Q

How does magnesium react with oxygen (combustion)

A

producing a bright white flame leaving behind a white ash of magnesium oxid

50
Q

How does hydrogen react with oxygen (combustion)

A

in an explosive reaction. This is the basis of the ‘squeak pop’ test for hydrogen in test tube. With larger quantities of hydrogen this explosion can be dangerous.

51
Q

How does sulphur react with oxygen (combustion)

A

reacts with oxygen producing a blue flame

52
Q

What happens if you heat metal carbonates

A

On heating metal carbonates thermal decompose into metal oxides and carbon dioxide.

53
Q

CO2 is a greenhouse gas which

A

absorbs infra-red radiation and therefore warms the atmosphere. This leads to global warming.

This may cause climate change.

54
Q

Test for hydrogen

A

Use a lit splint

gas pops

55
Q

Test for oxygen

A

use a glowing splint

relights

56
Q

Test for CO2

A

Bubble the gas through limewater

limewater turns cloudy

57
Q

Test for ammonia

A

Turns damp red litmus paper blue

58
Q

Test for chlorine

A

Bleaches moist litmus paper

59
Q

How to carry out a flame test

A

A platinum or nichrome wire is dipped into hydrochloric acid to remove any impurities.
The wire is dipped into the salt being tested
The wire and salt are held in a (roaring) bunsen burner flame.
The colour is observed

60
Q

Lithium flame colour

A

red

61
Q

Sodium flame colour

A

yellow

62
Q

Potassium flame colour

A

lilac

63
Q

Calcium flame colour

A

orange - red

64
Q

Copper II flame colour

A

blue - green

65
Q

Describe tests for the cation NH4+ (ammonium)

A

add sodium hydroxide and warm

will turn damp litmus paper blue

66
Q

Describe tests for the cations Cu2+, Fe2+ and Fe3+ (copper, iron)

A

First, add sodium hydroxide (NaOH), then observe the colour:
blue precipitate forms
green precipitate forms
brown precipitate forms

67
Q

Describe tests for Halide ions (Cl–, Br– and I–)

A 
add nitric acid to remove impurities
then add silver nitrate solution
Chloride - white precipitate
Bromide - cream precipitate
Iodine - yellow precipitate
68
Q

Describe tests for anions: Sulfate ions (SO42–)

A

Add hydrochloric acid to remove impurities
add barium chloride solution
white precipitate will form

69
Q

Describe tests for anions: Carbonate ions (CO32-)

A

add hydrochloric acid

fizzing will occur

70
Q

describe a test for the presence of water using anhydrous copper(II) sulfate

A

Add anhydrous copper (II) sulfate (CuSO4) to a sample.

If water is present the anhydrous copper (II) sulfate will change from white to blue.

71
Q

how can the rate of reaction be measured

A

The rate of a chemical reaction can be measured either by how quickly reactants are used up or how quickly the products are formed.

72
Q

if surface area increases

A

rate of reaction increases
increases surfaces for collisions
more frequent successful collisions

73
Q

if concentration increases

A

rate of reaction increases
increases number of particles in a given area
more frequent successful collisions

74
Q

if temperature increases

A

rate of reaction increases
particles have more energy so move quicker
more particles have the required activation energy
more frequent successful collisions

75
Q

what is a catalyst

A

a substances that increases the rate of reaction but remains chemically unchanged at the end by providing an alternate pathway with lower activation energy

76
Q

what is crude oil

A

a mixture of hydrocarbons

77
Q

how does fractional distillation work

A

Crude oil is separated by fractional distillation.
Crude oil is heated and the oil evaporates.
It then goes into the tower. As the vapours rise up the tower the temperature falls.
Different sized fractions condense at different heights because they have different boiling points.
Smaller molecules condense high up the tower. Larger molecules condense low down in the tower.
The fractions are collected

78
Q

refinery oil

A

bottled gas

79
Q

gasoline

A

fuel for cars

80
Q

kerosene

A

fuel for planes

81
Q

diesel oil

A

fuel for lorries

82
Q

fuel oil

A

fuel for ships

83
Q

bitumen

A

road surfacing

84
Q

The boiling point increases as

A

the number of carbon atoms (chain length) increases.

85
Q

The viscosity increases as

A

the number of carbon atoms (chain length) increases.

86
Q

the darker in colour that fraction is

A

The greater the number of carbon atoms (chain length)

87
Q

what is a fuel

A

a substance that when burned releases heat energy

88
Q

Complete Combustion happens when

A

there is enough oxygen available, producing carbon dioxide (CO2) and water (H2O)

89
Q

Incomplete Combustion happens when

A

there is not enough oxygen available, with possible products being carbon monoxide (CO), carbon (C, soot), carbon dioxide (CO2) and water (H2O)

90
Q

Carbon monoxide is poisonous because

A

it reduces the capacity of the blood to carry oxygen.

91
Q

nitrogen oxides are produced when

A

in car engines the temperature reached is high enough to allow nitrogen and oxygen in the air to react

92
Q

sulfur dioxides are produced when

A

some impurities in hydrocarbon fuels combust

93
Q

how sulfur dioxide and oxides of nitrogen oxides contribute to acid rain

A

sulfue dioxide and nitrogen oxides can react with water to make acids
Acids formed in the atmosphere can fall as acid rain. killing trees and fish in lakes.
the acid rain also corrodes limestone buildings and marble statues since these are both made of calcium carbonate
some metals such as iron are also attacked by acid rain.

94
Q

cracking is

A

the thermal decomposition of long-chain alkanes into shorter-chain alkanes and alkenes:

95
Q

the conditions of cracking

A

600 - 700 degrees

catalyst - silica/alumina

96
Q

why cracking is necessary

A

Crude oil contains a surplus long chains.
Shorter chain hydrocarbons are in greater demand, e.g. petrol.
Cracking also produces alkenes which are used in making polymers and ethanol.

97
Q

the general formula for alkanes

A

CnH2n+2

98
Q

saturated hydrocarbons

A

A molecule containing only single bonds between carbon atoms (alkanes)

99
Q

Alkanes react with bromine (halogens)

A

In the presence of UV light, e.g. sunlight.
A hydrogen atom in the alkane is replaced by a bromine atom.
This is known as substitution.
methylbromine + hydrogen bromide

Chemistry (15 decks)

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