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OCR A Level Chemistry > Topic 3 - Periodic Table and Energy > Flashcards

Topic 3 - Periodic Table and Energy Flashcards

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1
Q

The relative mass of an electron

A

1/1836

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2
Q

The relative mass of a proton

A

1

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3
Q

The relative mass of a neutron

A

1

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4
Q

Charge of proton

A

+1

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5
Q

Charge of neutron

A

0

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6
Q

Charge of electron

A

-1

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7
Q

What is an isotope?

A

Isotopes are atoms of the same element, with a different number of neutrons (same number of protons/electrons)

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8
Q

In the periodic table, horizontal rows are called …

A

periods

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9
Q

In the periodic table, vertical collums are called …

A

groups

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10
Q

How many groups are there?

A

18

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11
Q

What is group 1?

A

Alkali metals

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12
Q

What is group 2?

A

Alkaline Earth Metals

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13
Q

What is groups 3-12/

A

Transition metals

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14
Q

What is group 15?

A

Pnictogens

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15
Q

What is group 16?

A

Chalcogens

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16
Q

What is group 17?

A

The halogens

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17
Q

What is group 18?

A

The noble gases

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18
Q

What are metalloids/semi metals? Why do they have that name?

A

Elements that touch the line between metal and non-metals, they have a combination of properties of metals and non-metals

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19
Q

Define ionisation

A

when an atom loses an electron from its outer shell.

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20
Q

Define first ionisation

A

The energy required to remove 1 mole of electrons from one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions.

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21
Q

What 3 things can affect ionisation energy?

A

Shielding, nuclear charge and atomic radius

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22
Q

Define shielding

A

Shielding is when inner electrons screen the outer electrons from the pull from the nucleus

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23
Q

Define nuclear charge

A

The positive charge of the nucleus

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24
Q

Define atomic radius

A

Atomic radius is radius of an atom, we measure atomic radius by measuring the distance between 2 nuclei of touching atoms and halving the distance

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25
Q

Describe and explain the trend of atomic radius size as you go along period 3

A

There is an increase in nuclear charge as you go along the period. The stronger the nuclear charge the more it can pull the electrons closer to the nucleus. The shielding is the same as you go along the period. The general trend for atomic radius is it decreases as you go along period 3 as the electrons are pulled closer to the nucleus.

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26
Q

Describe and explain the trend of period 3 first ionisation energy

A

First ionisation energy enthalpy increases across a period, the nuclear charge increases across a period, attraction of electrons to the nucleus increases, atomic radius decreases (so electrons are closer), it takes more energy to remove that first electron.

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27
Q

Why does first ionisation energy dip between magnesium and aluminium?

A

There is a decease between magnesium and aluminium as magnesium has a full sub-shell stability, as the highest occupied sub-shell is complete (3s). Aluminium has one electron in a higher sub-shell (3p), this one electron is removed more easily as it is further away from the nucleus, and therefore the first ionisation energy is lower than magnesium.

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28
Q

Why does first ionisation energy dip between phosphorus and sulphur?

A

There is a decrease between phosphorus and sulphur because phosphorus has a half subshell stability, sulphur has one 3p orbital that contains a pair of electrons. These paired electrons repel each other, so one of these electrons is easier to remove therefore sulphur has a lower fist ionisation energy then phosphorus.

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29
Q

Describe and explain the trend in first ionisation energy as you go down group 3

A

First ionisation energy decreases down a group.
This is because more inner shell electrons as you go down the group, so there is shielding of outer electrons, attraction of electrons to the nucleus decreases, atomic radius increases (so electrons are further away).

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30
Q

Where does metallic bonding occur?

A

Only in metals

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31
Q

Describe and explain the metallic structure

A

.Giant structure
.The atoms are in tightly packed layers, which form a regular lattice structure
.Each atom in a solid metal structure has donated its negative electrons from its outer shell forming an ion
.The outer electrons become delocalised and create a ‘sea of free electrons’
.The positive metal ion (cation) is fixed in a portion maintaining the structure of the metal
.The delocalised electrons are mobile and can move through the structure

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32
Q

Define metallic bonding

A

.Metallic bonding is the strong electrostatic attraction between the metal ions (cations) and the delocalised electrons

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33
Q

Where do metals conduct? Why?

A

.Most only conduct in solid and liquid states

.The delocalised electrons can move freely anywhere with the metal lattice allowing them to conduct electricity

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34
Q

Why do metals have large bp/mp?

A

.Strong electrostatic attraction between the metal ion and the delocalised electrons
.Needs a lot of energy to break

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35
Q

What does the strength of the metal depend on? What does this also affect?

A

.The strength of metal depends on the charge of the metal ion in the structure (the greater the charge, the greater the number of delocalized electrons, the stronger the attraction, the stronger the bond)
.This also affects the size of the ion (the smaller the ion, the closer the electrons to the nucleus, the stronger the bond)

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36
Q

Do metals dissolve in solvents?

A

no

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37
Q

Why are metals good conductors of heat?

A

.When a metal is heated the delocalised electrons gain kinetic energy and move faster
.This movement transfers the gained energy throughout the metal

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38
Q

Why are pure metals soft?

A

When a metal is hit, the layers of metal ions are able to slide over each other, and so the layers do not shatter

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39
Q

What is an alloy and why are they harder than pure metals?

A

.An alloy is a mixture of two metals, thereby distorting the layers so they can’t slide over each other and make a harder new metal

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40
Q

diamond structure

A 
.Giant covalent bonding
.Forms a lattice
.Made of carbon only
.Strong covalent bond between each atom
.Each carbon is bonded to 4 other carbons
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41
Q

Diamond properties

A

.Hard – a giant covalent structure and has lots of strong bonds
.Doesn’t conduct electricity – no delocalised electrons that can move
.High melting point – many strong covalent bonds between atoms , it needs a lot of energy to break

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42
Q

Graphite structure

A

.Giant covalent bonding
.Made of carbon only
.Hexagonal structure
.Strong covalent bonds between carbon atoms
.In parallel layers
.Weak intermolecular forces between layers
.Each carbon is bonded to 3 other carbons
.Delocalised electrons in each layer

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43
Q

Graphite properties

A

.Soft/slippery – the layers can slide over each other because there are weak forces between the layers
.Conduct electricity – delocalised electrons that can move through the whole structure
.High melting point – graphite has a giant structure with lots of strong covalent bonds between atoms, it needs lots of energy to break bonds

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44
Q

What is graphene? properties

A

.One layer of graphite

.Highly conductive and strong and flexible

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45
Q

What is a nanotube?

A

When graphene forms a tube like strutcure

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46
Q

What is a bucky ball?

A

When carbon forms a cage like structure

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47
Q

What are different physical forms of elements called?

A

allotropes

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48
Q

On a melting point across a period graph, how can you section the different points?

A

Metallic bonding, giant covalent structures, covalent molecules

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49
Q

Why does the melting point increase across period 3?

A

.The charge in the metal ions increase
.The number of delocalised electrons increases
.So the strength of the metallic bonding increases
.Need more energy to break stronger metallic bonds so the melting points and boiling points increase

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50
Q

Is silicon a metal or non-metal?

A

TRICK QUESTION

Its a metalloid

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51
Q

What is silicons structure like?

A

It has a giant covalent structure exactly the same as carbon in diamond (each silicon is bonded to four other silicon’s)

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52
Q

Why does silicon have a high melting point?

A

you have to break lots of string covalent bonds in order to melt it, and this requires a lot of energy to break.

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53
Q

How do phosphorus, sulphur and chlorine exist?

A

simple molecules, with strong covalent bonds between their atoms.

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54
Q

How does argon exist?

A

Argon exists as separate atoms (it is monatomic)

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55
Q

Why is Cl, Ar, S8 and P4’s melting points so low?

A
  • When these four substances melt or boil, it is the London forces between the molecules which are broken. These are very weak bonds. So little energy is needed to overcome them.
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56
Q

In what order do the melting points of Cl2, Ar, S8 and P4 decrease? Why?

A

The strength of the intermolecular forces increases with the number of electrons, so the melting point decreases in this order:
S8 > P4 > Cl2 > Ar

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57
Q

What happens to the size of the metal atoms down group 2?

A

increases

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58
Q

What happens to the shielding of the outer electrons down group 2?

A

Increases

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59
Q

Describe and explain reactivity down group 2?

A

.Reactivity increases down group 2
.The size of the metal atoms increases down group 2
.The shielding of the outer electrons increases
.The outer electrons require less energy to remove as the attraction to the nucleus is less
.Meaning the metal is more reactive

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60
Q

What happens to oxides of group 2 elements when they react with water?

A

they release hydroxide ions and make a metal hydroxide.

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61
Q

CaO(s) + H2O(l) 

A

Ca(OH)2(aq)

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62
Q

Why does alkalinity increase down group 2?

A

the metal hydroxides are more soluble

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63
Q

What happens when metal hydroxides react with water?

A

they make a white precipitate, which will dissolve into the water

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64
Q

Uses of group 2 compounds

A

to treat indigestion, agriculture and medicine

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65
Q

Uses of group 2 compounds in indegestion

A

e.g. Gaviscon and Rennies are made with calcium carbonate

Milk of Magnesia with magnesium hydroxide

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66
Q

Use of group 2 compounds in agriculture

A

in fields you get soil that has acidic conditions

treat the soil with an alkali, usually calcium hydroxide (lime)

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67
Q

Use of group 2 compounds in medicine

A

Barium meal made of barium sulphate, which is completely insoluble in water

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68
Q

What are halogens elemental forms like?

A

Diatomic molecules

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69
Q

What are halides?

A

Halogen ions with charge -1

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70
Q

What are halides like?

A

Monoatomic ions with full outer shells

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71
Q

F appearance at room temp

A

Pale yellow gas

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72
Q

Cl appearance at room temp

A

Pale green gas

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73
Q

Br appearance at room temp

A

Orange liquid

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74
Q

I appearance at room temp

A

Grey solid

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75
Q

Br appearance of vapour

A

Orange gas

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76
Q

I appearance of vapour

A

Purple gas

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77
Q

Trend in group 7 reactivity

A

lower as go down group

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78
Q

Describe and explain halogen boiling points

A

Halogen molecules increase in size as we go down the group, this leads to greater London forces between molecules, increasing the energy needed to separate the molecules and therefore higher melting and boiling points.

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79
Q

Fluorine boiling point

A

-118’C

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80
Q

Iodine boiling point

A

184’C

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81
Q

Describe and explain electronegativity trend in halogens

A

Electronegativity of the halogens decreases down the group due to an increase in atomic radius.
Increased nuclear charge is outweighed because there are more electron shells and more shielding. Iodine atoms therefore attract electron density in a covalent bond less strongly than fluorine.

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82
Q

Describe electron configuration in halogens

A

7 electrons in the outer shell, highest energy electrons in a p sub-shell
Each element has one fewer electrons than the next noble gas
Outer p subshell containing 5 electrons (needs one more to form a -1 ion)

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83
Q

Halogens are a strong oxidising agent, what does this mean?

A

They gain electrons

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84
Q

Why does reactivitity/oxidising power decrease down the halogens group?

A

.Atomic radius increases
.Electron shielding increases
.Ability to gain an electron decreases

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85
Q

Cl in water and cyclohexane

A

Pale green

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86
Q

Br in water and cyclohexane

A

Orange

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87
Q

I in water

A

Brown

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88
Q

I in cyclohexane

A

Violet

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89
Q

What is cyclohexane?

A

An organic solvent

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90
Q

Sodium chloride and chlorine water colour change, and with organic solvent (cyclohexane)

A

Stayed clear

Pale green

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91
Q

Sodium bromide and chlorine water colour change, and with organic solvent (cyclohexane)

A

Clear to pale yellow Reddy brown

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92
Q

Sodium iodine and chlorine water colour change, and with organic solvent (cyclohexane)

A

Clear to reddy brown Violet

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93
Q

Sodium chloride and bromine water colour change, and with organic solvent (cyclohexane)

A

Clear to pale yellow Orangey brown

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94
Q

Sodium bromide and bromine water colour change, and with organic solvent (cyclohexane)

A

Clear to pale yellow Orangey brown

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95
Q

Sodium iodide and bromine water colour change, and with organic solvent (cyclohexane)

A

Clear to reddy brown Violet

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96
Q

Sodium chloride and iodine water colour change, and with organic solvent (cyclohexane)

A

Clear to pale brown Violet

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97
Q

Sodium bromide and iodine water colour change, and with organic solvent (cyclohexane)

A

Clear to pale brown Violet

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98
Q

Sodium iodide and iodine water colour change, and with organic solvent (cyclohexane)

A

Clear to pale brown Violet

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99
Q

In displacement reactions between halogens and halides, what acts as an oxidising agent?

A

The halogen

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100
Q

If the halogen is an oxidising agent, what does this mean?

A

.Oxidises the halide ion to the halogen
.Gains electrons
.Is reduced to form the halide ion

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101
Q

Halogen oxidising ability order

A

BOTTOM I,  Br,  Cl,  F TOP

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102
Q

What does chlorine dissolve in water to form?

A

an acidic solution of hydrochloric acid and chloric (I) acid.

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103
Q

chloric(I) acid formula

A

HOCl

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104
Q

How is water and chlorine a disproportionation reaction?

A

chlorine is both oxidised and reduced, from 0 to -1 in HCl and from 0 to +1 in HOCl

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105
Q

What does chlorine react with cold dilute sodium hydroxide to form?

A

sodium chlorate (I) and sodium chloride and water

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106
Q

sodium chlorate (I) formula

A

NaOCl

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107
Q

How is chlorine and cold dilute sodium hydroxide a disproportionation reaction?

A

chlorine is both oxidised and reduced, from 0 to -1 in NaCl and from 0 to +1 in NaOCl

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108
Q

Why is chlorine used to purify water samples?

A

because it is toxic to bacteria, some of which may cause disease

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109
Q

What is the risk of using chlorine to purify water samples?

A

chlorine is also toxic to humans, so there are risks associated with gas leaks during the chlorination process. There is also a risk of the formation of chlorinated hydrocarbons, which are also toxic

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110
Q

Why does the chlorination of drinking water raise ethical questions?

A

raises questions about individual freedom because it makes it difficult for individuals to opt out.

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111
Q

What does household bleach commonly contain?

A

the chlorate(I) ion in the form of sodium chlorate(I), NaOCl.

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112
Q

What does the chlorate(I) ion act as, what does it do?

A

It oxidises the organic compounds in food stains, bacteria and dyes.

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113
Q

Test for carbonate ions

A
  1. Add dilute nitric acid to the solid or solution
  2. Bubble any gas made into limewater
  3. If ions present the lime water will turn milky
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114
Q

Test for sulphate ions

A
  1. Add dilute hydrochloric acid
  2. Followed by aqueous barium chloride solution
  3. You will see a white precipitate being formed if sulphate ions were present as BaSO4 is made
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115
Q

Sulphate ions test ionic equation

A

Ba2+ + SO42-  BaSO4

116
Q

Halide ions test

A
  1. Add dilute nitric acid

2. Followed by aqueous silver nitrate solution

117
Q

Why, in the halide ions test, do you have to use nitric acid?

A

since chloride is present in HCl

118
Q

Colour of precipitate for Cl- anion

A

White

119
Q

Colour of precipitate for Br- anion

A

Cream

120
Q

Colour of precipitate for I- anion

A

Yellow

121
Q

What do you do if you can’t tell the difference after the halide ion test?

A

you then add aqueous ammonia (NH3).

122
Q

What does aqueous ammonia do to the different halide anions, why?

A

Chloride ions are soluble and the precipitate redissolves.
Bromide ions are soluble and the precipitate redissolves.
Iodide ions are insoluble so the precipitate will stay.

123
Q

Sequence of anion tests

A

CaSH = Carbonate, sulphate then halides

124
Q

Ammonium ion test

A
  1. Add aqueous sodium hydroxide
  2. Gently warm
  3. Hold moist pH paper above, turns blue
125
Q

What contains enthalpy?

A

Elements and compounds

126
Q

What is enthalphy (H)?

A

the heat that is stored in a chemical system

127
Q

What is a chemical system?

A

The system refers to the atoms, molecules and ions making up the chemicals

128
Q

Enthalpy cannot be measured, what can?

A

Enthalpy change

129
Q

What is enthalpy change (ΔH)?

A

the difference in enthalpy between the products and reactants in a reaction

130
Q

What happens in an exothermic reaction?

A

.In an exothermic chemical reaction heat energy is transferred from the system to the surroundings
.Any energy loss by the system is balanced by the energy gain by the surroundings
.The temperature of the surroundings increases, so we see a temperature increase

131
Q

What happens in an endothermic reaction?

A

.In an endothermic chemical reaction heat energy is absorbed from the surroundings into the system
.Any energy gain by the system is balanced by the energy loss of the surroundings
.The temperature of the surroundings decreases, so we see a temperature decrease

132
Q

Burning fuel, exo or endo?

A

Exo

133
Q

Condensing a vapour, exo or endo?

A

Exo

134
Q

Evaporation, exo or endo?

A

Endo

135
Q

Neutralising an acid, exo or endo?

A

Exo

136
Q

Thermal decomposition of copper carbonate, exo or endo?

A

Endo

137
Q

Rapid oxidation of iron, exo or endo?

A

Endo

138
Q

Shop bought hand warmers, exo or endo?

A

Exo

139
Q

Sports injury cool packs, exo or endo?

A

Endo

140
Q

Enthalpy change equation

A

H(Products) – H(Reactants)

141
Q

Sign for exothermic reaction

A

negative

142
Q

Sign for endothermic reaction

A

positive

143
Q

Define activation energy

A

The minimum amount of energy required to start a reaction by breaking the bonds

144
Q

Draw an exothermic activation energy graph

A

Check notes

145
Q

Draw an endothermic activation energy graph

A

Check notes

146
Q

Draw an exothermic enthalpy profile

A

Check notes

147
Q

Draw an endothermic enthalpy profile

A

Check notes

148
Q

Define Enthalpy change of reaction (ΔHr) with example

A

the enthalpy change when the reaction occurs in the molar quantities shown in the chemical reaction
e.g. Zn(s) + Cu2+(aq)  Cu(s) + Zn2+(aq)

149
Q

Define Enthalpy change of formation (ΔHf) with example

A

the enthalpy change when 1 mole of compound is formed from its elements
e.g. C(s) + O2(g)  CO2(g)

150
Q

Define combustion change of reaction (ΔHc) with example

A

the enthalpy change when 1 mole of substance is burnt

e.g. CH4(g) + O2(g)  CO2(g) + H2O(g)

151
Q

Define Enthalpy change of neutrilisation (ΔHneut) with example

A

the enthalpy change when solutions of an acid and an alkali react together under standard conditions to produce 1 mole of water. It is always measured per mole of water formed.
e.g. HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)

152
Q

What symbol is used for standard conditions?

A

ϴ

153
Q

What conditions are used for enthalpy change values?

A

Standard conditions:
Standard pressure = 100KPa
Standard temperature = 298K (25’C)
Standard concentration = 1 moldm-3

154
Q

Two equations for calculating enthalpy changes

A 
q = mcΔT
ΔH = q/n
155
Q

What is each part of ΔH = q/n?

A 
q = heat energy (J)
n = number of moles (mol)
156
Q

What is each part of q = mcΔT?

A 
q = heat energy (J)
m = mass of substance heated or cooled (g)
c = specific heat capacity of water (4.18 Jg-1K-1)
ΔT = change in temperature (‘C or K)
157
Q

What is the final step of calculating enthalpy change equations?

A

Multiply the answer by the co-efficient of the reagent not in excess

158
Q

When doing enthalpy change calculations, and you dont have a weight for the solution, what do you use?

A

The volume of it in cm^3, Cm^3 = g

159
Q

When doing enthalpy change calculations with an equation and bond energy values, how do you get the final answer after finding the values of either side of the equation?

A

bonds broken - bonds made

left - right

160
Q

Define average bond enthalpy

A

the average enthalpy change when one mole of gaseous covalent bonds is broken

161
Q

Why might the calculated average bond enthalpy different from the actual?

A

.The bond enthalpies used in the calculations are averages from different compounds, the exact bond enthalpy depends on the particular compound in which it is either formed or broken
.The bond enthalpies are not determined under standard conditions. Bond enthalpies are determined by molecules in a gaseous state. But at 298K not all compounds are a gas, such as water.

162
Q

In terms of enthalpy, what is breaking of bonds always? Why?

A

Always endothermic, as you need to add energy to break bonds

163
Q

What can average bond enthalpy also be called?

A

Mean bond enthalpy

164
Q

Where is average bond enthalpy taken from?

A

the average is taken over a wide range of compounds containing that type of bond

165
Q

State the standard conditions

A

Standard pressure = 100kPa (1 atmosphere)
Standard temperature = 298K (25’C)
Standard concentration = 1moldm-3
Standard states of all substances (carbons is a solid, hydrogen is a gas and water is a liquid)

166
Q

Define standard enthalpy change of reaction

A

The enthalpy change for a reaction as shown by the molar quantities in the chemical equations
Measured under standard conditions

167
Q

Define standard enthalpy change of combustion

A

Enthalpy change when 1 mole of a substance reacts completely with oxygen under standard conditions`

168
Q

Define standard enthalpy change of formation

A

The enthalpy change when 1 moles of substance is formed from its elements under standard conditions

169
Q

Enthalpy change of formation of elements is always …

A

zero

170
Q

What to remember for Hess’ Law Cycles Involving Enthalpies of Formation

A

Using delta H f it’s p-r!

171
Q

Formula for hess’ law cycles involving enthalpies of formation

A

sum of ΔHf products - sum of ΔHf reactants

172
Q

Why does oxygen have no enthalpy of combustion value?

A

Oxygen can’t be combusted

173
Q

What does Hess’ law state?

A

Hess’ law states that the overall enthalpy change of the two routes is the same

174
Q

Equation for Hess’ Law Cycles involving enthalpies of combustion

A

sum of enthalpy of combustion of reactants - sum of enthalpy of combustion of products

175
Q

Does breaking bonds require or release energy?

A

Require

176
Q

Does forming bonds require or release energy?

A

Release

177
Q

Define exothermic

A

the energy required to break bonds is less than the energy given out when new bonds form

178
Q

Define endothermic

A

the energy required to break bonds is more than the energy given out when new bonds form

179
Q

Define average bond enthalpy

A

the average enthalpy change when one mole of gaseous covalent bonds is broken

180
Q

Equation for enthalpy change

A

enthalpy of bonds broken – enthalpy of bonds formed

181
Q

Why might calculated bond enthalpies not be right?

A
  1. The bond enthalpies used in the calculations are averages from different compounds, the exact bond enthalpy depends on the particular compound in which it is either formed or broken
  2. The bond enthalpies are not determined under standard conditions. Bond enthalpies are determined by molecules in a gaseous state. But at 298K not all compounds are a gas, such as water
182
Q

Draw a general diagram for Hess’ law

A

CHECK NOTES

183
Q

Enthalpy change of reaction –

A

This is the enthalpy change when the reaction occurs in the molar quantities shown in the chemical equation

184
Q

Enthalpy change of formation –

A

This is the enthalpy change when 1 mole of compound is formed from its elements

185
Q

Enthalpy change of combustion –

A

This is the enthalpy change when 1 mole of substance is burned

186
Q

Enthalpy change of neutralisation –

A

The enthalpy change when solutions of an acid and an alkali react together under standard conditions to produce 1 mole of water. It is always measured per mole of water formed.

187
Q

Hess’ Law

A

If a reaction can take place by more than one route, and the initial and final concentrations are the same, the total enthalpy change is the same regardless of the route taken

188
Q

Things to remember when using Hess’ law

A

If you have more than one compound, then you have to add the enthalpy of formation for each compound together
Enthalpy of formation is given for 1 mole of compound formed. If there is more than one mole, you multiply it

189
Q

What is Hess’ law used for?

A

Hess’ Law determines enthalpy changes indirectly, for when determining them directly isn’t possible

190
Q

Where does Hess’ law come from?

A

Hess’ Law comes from the idea of the conservation of energy

191
Q

For elements, enthalpy change of formation is ALWAYS ____

A

zero

192
Q

Enthalpy change of reaction equation =

A

sum of the enthalpy change of formation of products - sum of the enthalpy change of formation of reactants OR sum of the enthalpy change of combustion of reactants - sum of the enthalpy change of combustion of products

193
Q

equation for rate of reaction

A

change in concentration (of products or reactants) / time

194
Q

Units of rate of reaction

A

moldm^-3s^-1

195
Q

Draw a graph of conc of reactants against time

A

check notes

196
Q

Draw a graph of conc of products against time

A

check notes

197
Q

What does the gradient of rates of reaction graphs show?

A

the rate of the reaction at that point

198
Q

In collision theory, what must you remember?

A

Not all collisions are successful

199
Q

High rate of reaction = what in terms of collision theory?

A

high number of successful collisions per second

200
Q

A successful collision is

A

any collision that reaches the activation energy

201
Q

Factors which alter rate of reaction:

A
  • Temperature
  • Surface area (solids)
  • Catalysts
  • Concentration
  • Pressure (gases)
202
Q

How does temperature affect ror?

A

At a higher temperature the particles have more kinetic energy, so more collisions are successful, and more frequent collisions, so higher rate of reaction

203
Q

How does surface are affect ror?

A

At higher surface areas the particles have more places to collide into, so more successful collisions occur per second, so it’s a higher rate of reaction

204
Q

How do catalysts affect ror?

A

Provide an alternative route for the reaction which lowers the activation energy, while remaining chemically unchanged. Lower activation energy, meaning more successful collisions per second, so faster rate of reaction

205
Q

How does concentration affect ror?

A

Higher concentration, more particles per unit volume, so more successful collisions per second as more particles hitting into each other, so higher rate of reaction

206
Q

How does pressure affect ror?

A

Higher pressure, more particles per unit volume, so more successful collisions per second as more particles hitting into each other, so higher rate of reaction

207
Q

Describe general botzmann distribution curve

A 
Every particle has energy
No particles with no energy
Most particles have medium energy
A few particles have high energy
Can’t touch x axis, must have an asymptote
208
Q

Why must the boltzmann distribution curve have an asymptote?

A

cannot assume no particles with higher energy

209
Q

Total area under boltzmann distribution curve is

A

the number of particles in the sample

210
Q

Draw normal boltzmann distribution curve

A

Check notes

211
Q

Show affect of catalyst on boltzmann distribution curve

A

Check notes

212
Q

Show affect of temp (hot and cold) on boltzmann distribution curve

A

Check notes

213
Q

Increase in concentration or pressure …

A

 more particles in same volume  more frequent collisions  collisions over EA are more frequent  rate of reaction increases

214
Q

For a reaction to occur …

A

particles need to collide with sufficient energy and the correct orientation

215
Q

Show affect of concentration on Boltzmann curve

A

check notes

216
Q

A catalyst is

A

a substance that changes the rate of chemical reaction without undergoing a permanent change. It lowers the activation energy of the reaction by providing an alternative reaction pathway.

217
Q

What is Effect of temperature on boltzmann curve

A
  • As we increase the temperature the amount of energy increases so the curve moves to the right
  • However we have no extra particles so the curve gets lower
  • The area underneath the curve is the same as the number of particles hasn’t changed
  • More particles now have sufficient energy to react
218
Q

WHat is effect of concentration on boltzmann curve

A
  • As we raise the concentration the amount of energy stays the same so the curve doesn’t move left or right
  • However we have extra particles so the curve gets higher
  • More particles now have sufficient energy to react
219
Q

What is effect of catalyst on boltzmann curve

A
  • If we introduce a catalyst an alternative reaction pathway with a lower activation energy is available
  • More particles now have sufficient energy to react
220
Q

Draw a diagram of how a catalyst works generally

A

Check notes

221
Q

Draw potential energy diagram including catalyst

A

Check notes

222
Q

Draw how catalyst works for ethene and hydrogen

A

check notes

223
Q

Draw how catalyst works for hydrogen and carbon monoxide

A

check notes

224
Q

Draw how catalysts work for ammonia in the haber process

A

check notes

225
Q

How does a catalyst work?

A
  1. One of the reactants approaches the catalysts surface and settles onto an active site – adsorption
  2. Another reactant approaches the catalyst
  3. Re-arrangement of electrons takes place – reaction
  4. The products are released from the surface – desorption
226
Q

Which metals are found in a catalytic converter?

A

Platinum, palladium and rhodium

227
Q

What does a catalytic converter turn nitrogen oxide into?

A

Nitrogen and oxygen

228
Q

What does a catalytic converter turn carbon monoxide molecules into?

A

Carbon dioxide

229
Q

Heterogeneous catalysis is most frequently used in

A

industrial production processes

230
Q

.Heterogeneous means that

A

the catalysts and starting molecules are present in different phases – for example, solid and gaseous – the gaseous starting particles react on the solid catalyst particles

231
Q

Describe the process of heterogeneous catalysis

A

.The molecules approach the surface of the catalyst and stick to it in a defined arrangement
.The chemical bonds are cleaved with the aid of a catalyst
.The desired molecular bonds are formed, on completion of the reaction, the products leave the catalyst

232
Q

A nickel catalyst can be used to

A

hydrogenate double bonds in an alkene

233
Q

What does hydrogenating double bonds in an alkene do?

A

turn unsaturated fats, into saturated fats (vegetable oil into margarine)

234
Q

A palladium catalyst can be used in a catalytic converter to combine what to produce what?

A

to combine 2 x CO molecules with a molecule of O2 to make 2 molecules of CO2

235
Q

An iron catalyst is used in the _____ process

A

Haber

236
Q

Why is a catalyst needed in the Haber process?

A

This ‘fixes’ nitrogen from the air using hydrogen and turns it into ammonia. This is very difficult to do without a catalyst as N2 has a triple bond and so has a high bond enthalpy (takes a lot of energy to break).

237
Q

Explain why many industrial manufacturing processes use catalysts

A

Enables reactions to occur with less waste, enable reactions to happen with less toxic solvents/reactants, reactions can happen at room temperature, saves energy/cost, reduce carbon dioxide emissions, enable reactions to occur with more specify

238
Q

Two methods can be used to determine the rate of reaction from gases, what are they?

A
  • Monitoring the volume of gas produced at regular time intervals using gas collection
  • Monitoring the loss of mass reactants using a balance at regular time intervals
239
Q

When do you stop recording results when determining the rate of reaction?

A

You stop recording when the measured value does not change with time, this means the reaction is complete

240
Q

How can catalysts work?

A

The catalyst may react with a reactant to form an intermediate or may provide a surface on which the reaction can take place
At the end of the reaction the catalyst is regenerated

241
Q

What is a homogenous catalyst and how does it work?

A

A homogenous catalyst has the same physical state as the reactants. The catalyst reacts with the reactants to form an intermediate, the intermediate then breaks down to give the product and regenerates the catalyst.

242
Q

Give an example of a homogenous catalyst

A

An example would be making esters with sulfuric acid as the catalyst, all ethanol, ethanoic acid and sulfuric acid are liquids.

243
Q

What does the honeycomb mesh in catalytic converters do?

A

.Honeycomb mesh provides a large surface area for the reaction to take place

244
Q

The economic costs of using a catalyst outweigh …

A

any costs associated with developing a catalytic process

245
Q

How do you know when it is a reversible reaction?

A

The double arrows

246
Q

What is a reversible reaction?

A

When the reaction can go forwards and backwards

247
Q

What are reversible reactions described as?

A

dynamic, they are continuous

248
Q

There comes a point where the rate of the rate of the forward reaction equals the rate of the backwards reaction, this is called …

A

Dynamic equilibrium

249
Q

The concentrations of all the particles in the system remain constant, this is because …

A

the rate of reaction in one direction is equal to the rate of reaction in the other direction

250
Q

Dynamic equilibrium’s must remain in a closed system, why?

A

matter cannot enter or exit, as if it did it would ruin the equilibrium

251
Q

What conditions change the position of equilbrium?

A

.Concentration of the substances
.Temperature of system
.Pressure of system for gasses
.Presence of a catalyst

252
Q

What is le chatelier’s principle?

A

‘When a system in dynamic equilibrium, is subjected to a change, the position of the equilibrium will shift to minimise the change’

253
Q

Shifting the reaction to the left means to …

A

Increase the concentration of the reactants

254
Q

Shifting the reaction to the right means to …

A

Increase the concentration of the products

255
Q

If you increase the concentration of one of the products, the reaction …

A

shifts to the left and increases the amount of reactants being formed, thereby increasing their concentration and keeping the concentration of all particles in the system constant

256
Q

If you increase the concentration of one of the reactants, the reaction …

A

shifts to the right and increases the amount of products being formed, thereby increasing their concentration and keeping the concentration of all particles in the system constant

257
Q

If you decrease the concentration of one of the products, the reaction …

A

shifts to the right and increases the amount of products being formed, thereby increasing their concentration and keeping the concentration of all particles in the system constant

258
Q

If you decrease the concentration of one of the reactants, the reaction …

A

shifts to the left and increases the amount of reactants being formed, thereby increasing their concentration and keeping the concentration of all particles in the system constant

259
Q

Changing the pressure only works for which state?

A

Gasses

260
Q

For working out the favoured reaction with pressure changes and le chateliers principle, what must you do first? What equation do you do this with?

A

First you must establish which side of the reaction has the greater volume
moles = volume / 24

261
Q

An increase in pressure responds by shifting the reaction to …

A

The side with the fewest moles

262
Q

A decrease in pressure responds by shifting the reaction to

A

The side with the most moles

263
Q

Regarding le chateliers principle, if moles/volume equal on both sides, a change in pressure would

A

not cause an increase in one reactions rate of reaction, both would have an increase in rate of reaction

264
Q

What does a catalyst do for le chateliers reaction?

A

The catalyst increases the rate of the forward and backwards reaction by the same amount, so the position of equilibrium not effected

265
Q

When using temperature for le chateliers reaction, what must we do first?

A

We need to know which reaction is exothermic and which reaction is endothermic

266
Q

For le chateliers principle, an increase in temperature causes …

A

an increase in the rate of the endothermic reaction, the endothermic reaction is favoured

267
Q

For le chateliers principle, a decrease in temperature causes …

A

an increase in the rate of the exothermic reaction, the exothermic reaction is favoured

268
Q

Describe how a dynamic equilibrium comes about?

A

.At the start of the reaction, the concentrations of A and B were at their maximum
.This means that the rate of reaction was at its fastest
.As A and B react, their concentrations fall
.That means that they are less likely to collide and react, and so the rate of the forward reaction falls as time goes on
.In the beginning there isn’t any C and D so there can’t be any reaction between them
.As time goes on, though, their concentrations in the mixture increase and they are more likely to collide and react
.With time, the rate of reaction between C and D increases
.Eventually the rates of the two reactions will become equal
.A and B will be converting into C and D at exactly the same rate as C and D convert back into A and B again
.At this point there won’t be any further change in the amounts of A, B, C and D in the mixture
.As fast as something is being removed, it is being replaced again by the reverse reaction
.We have reached a position of dynamic equilibrium

269
Q

Dynamic equilibrium is reached when …

A

the rate of the forward reaction is the same as the backwards reaction, concentrations of reactants and products remain constant

270
Q

The Haber process takes place at 350’c-500’c and 100-200 atm, why?

A

these conditions produce the most ammonia in the dynamic equilibrium, but are also the most cost efficient

271
Q

Haber Process, pressure conditions, ideal, problem and actual

A

Ideal - high
problem - high danger
actual - 200ATM

272
Q

Haber Process, temperature conditions, ideal, problem and actual

A

Ideal - low
problem - rate low
actual - 400-500’C

273
Q

What catalyst is used in the Haber process?

A

Fe

274
Q

What are the actual conditions of the haber process called? Why?

A

These actual conditions are called compromise conditions, as they are compromising on the yield but they will be able to gain this product in shorter time frame

275
Q

What is the yield of the haber process?

A

15%

276
Q

What happens to unsused nitrogen and hydrogen in the haber process?

A

it is recycled through the process again

277
Q

Kc =

A

[products] / [reactants]

278
Q

[ ] =

A

equilibrium concentrations in moldm-3

279
Q

If the equation was aA + bB cC + dD, what would Kc equal?

A

([C]c x [D]d) / ([A]a x [B]b)

280
Q

What is Kc?

A

The equilibrium, constant but it is temperature dependant

281
Q

An increase in temperature does what to Kc in the case of a forward exothermic reaction?

A

An increase in the temperature increases the concentration of reactants and lessens that of the products so Kc decreases

282
Q

A decrease in temperature does what to Kc in the case of a forward exothermic reaction?

A

A decrease in the temperature decreases the concentration of the reactants and increases that of the products so Kc increases

283
Q

What does a large Kc mean?

A

equilibrium is favouring the right hand side

284
Q

What does a small Kc mean?

A

equilibrium is favouring the left hand side

285
Q

The magnitude of Kc indicates what?

A

the relative proportions of reactants and products in the equilibrium system

286
Q

A rough guide as to what the magnitude of Kc indicates

A
  • A Kc value of 1 indicates a position of equilibrium that is halfway between reactants and products
  • A Kc value > 1 indicates a position of equilibrium that is towards the products
  • A Kc value < 1 indicates a position of equilibrium that is towards the reactants
287
Q

So the larger the Kc value, the further the …

A

… position of equilibrium lies to the right-hand side and the greater the concentrations of the products compared to the reactants

OCR A Level Chemistry (17 decks)

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