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Chemistry ovr Flashcards

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1
Q

What is the Definition Of Atomic Number

A

The atomic number represents the number of protons and indirectly shows the number of electrons (atoms are stable)

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2
Q

What is the Relative Atomic Mass

A

The Relative Atomic Mass represents the number of subatomic particles in the nucleus + electrons

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3
Q

What are the three subatomic particles

A

Protons, Neutrons and Electrons

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4
Q

Charge and Mass of Proton

A

Mass=1

The charge is positively charged

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5
Q

Charge and Mass of Neutron

A

Mass=1

The charge is neutral

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6
Q

Charge and Mass Of Electron

A

Mass= 1/1836

The Charge is negative

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7
Q

Charge of an Atom and Why?

A

No overall Charge because of Num Of Protons= Num of Electrons

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8
Q

How to Calculate RAM

A

Num of Protons + Num of Neutrons

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9
Q

How to calculate Num of Protons

A

Same as the Atomic Number

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10
Q

How to calculate the Num of Electrons

A

Same as the Atomic Number

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11
Q

How to Calculate the Num of Neutrons

A

RAM - ATOMIC NUMBER
Because RAM = protons and neutrons
ATOMIC NUMBER = protons

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12
Q

What is the Group Number?

A

Represents the Num of electrons in the outer shell

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13
Q

What is the Period Number?

A

Represents the Num of electron shells surrounding the nucleus

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14
Q

What is Ionic Bonding

A

Ionic Bonding is the electrostatic force of attraction between positively charged ions and negatively charged ions. (Metals and Non Metals)

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15
Q

What does the Compound of Ionic Bonding lead to?

A

Formation of Salts

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16
Q

What does it mean by the electrostatic force of attraction?

A

When 2 oppositley charged ions attract

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17
Q

Why do elements undergo Ionic Bonding?

A

This is because all elements want to acheive a full outershell.

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18
Q

How does it Ionic Bonding occur?

A

When a non metal combines with a metal the non metal has a stronger attraction for electrons than the metal so metals are transffered from the outer shell.

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19
Q

Why Are Non Metals Negatively Charged?

A

Because an Electron has a negative charge and when something gains an electron it will become negatively charged as there are more electrons than protons.

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20
Q

Why are Metals Positively Charged

A

Because an Electron has a negative charge and when it loses an Electron it will have more protons then electrons making it positively charged.

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21
Q

What is Covalent Bonding

A

When Electrons are shared between 2 non-metal atoms to acheive a full outershell.

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22
Q

What is Metallic Bonding

A

The Electrostatic Attraction between the sea of delocalised electrons and the positively charged metal atoms.

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23
Q

Properties Of Ionic Bonding in terms of electrostatic attraction

A

Very Strong Electrostatic Attraction

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24
Q

Properties of Ionic Bonding in terms of melting and boiling point

A

Ionic Compunds have a high melting and boiling points because the electrostatic force of attraction between the positive metal ions and the negative non metal ions is so strong that it requires a lot of energy to break therefore having a high melting and boiling point

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25
Q

Properties of Ionic Compounds in terms of Conductivity

A

Can Conduct when molten or when dissolved in water. This is because free movement of ions can lead to the generation of a current

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26
Q

Properties Of Ionic Compounds in terms of arrangement

A

Ionic Compounds generate a lattice arrangement. This is because oppositely charged ions, attract in all directions

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27
Q

What are the 2 main groups of covalent structures

A

Simple Molecular e.g. H20, CO2

Giant Covalent e.g. Diamond, Graphite, Fullerene

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28
Q

Is the melting/boiling point of simple molecular structures high or low?

A

Low Melting and Boiling points as small amounts of energy are needed to overcome the weak intermolecular
forces that exist between adjacent compounds

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29
Q

Properties Of Simple Molecular Structure in terms of conductivity?

A

In general simple molecular compound, e.g. CO2 does not conduct electricity

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30
Q

What types Of Giant Covalent Network structures are there

A

Diamond, Graphite and Fullerene

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31
Q

What are Diamond, Graphite and Fullerene made from

A

Carbon atoms only

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32
Q

Explain the structure of a diamond in a Giant Covalent Network

A

Each carbon atoms forms a covalent bond with 4 oher carbon atoms. this generates a giant network of carbon atoms

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33
Q

Properties of Diamond in terms of Melting Point

A

The Melting and Boiling Point of Diamond is high because high amounts of energy is needed to overcome the weak intermolecular forces that exist between adjacent compounds

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34
Q

Properties of Diamond in terms of Toughness

A

Diamond is Tough because the covalent bonds are very strong

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35
Q

Properties of Diamond in terms of conductivity

A

Diamond does not conduct electricity as it does not have any available delocalised electrons to conduct a current

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36
Q

Explain the structure of Graphite in Covalent Bonding

A

Each Carbon atom forms a covalent bond with 3 other carbon atoms. because of this it will have free electrons that will become delocalised

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37
Q

Properties of Graphite in terms of conductivity

A

Can conduct electricity as the delocalised electrons are free to move in between the layers/ sheets of carbon atoms

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38
Q

Explain the structure of Fullerene

A

Molecular Structure - C60, forms a hollowsphere

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39
Q

Properties of Fullerene in terms of Conductivity

A

Fullerene does not Conduct electricty because it has no free delocalise electrons.

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40
Q

Properties of Fullerene in terms of Melting and Boiling points

A

High melting and Boiling points as the c-c bonds are strong and as it forms a giant covalent network.

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41
Q

Properties of Metals in terms of conductivity

A

Can conduct electricity since they have free delocalised electrons that can move to generate a current. They can also conduct heat

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42
Q

Properties of Metals in terms of malleability and ductility

A

Metals are malleable and ductile as they have layers of positive metal ions that can slide over each other

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43
Q

Properties Of Metals in terms of Melting and Boiling point

A

Metals have a high melting and boiling point because the electrostatic force of attraction between the positively charged metal ions and the sea of delocalised electrons is
so strong that a lot of energy is required to break this bond therefore having a high melting and boiling point

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44
Q

How does Metallic Bonding occur

A

Electrons become delocalised from metal atom generating metal ions due to imbalance of electrons and protons within the metal ion

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45
Q

Definition Of Metallic Bonding

A

Metallic Bonding refers to the electrostatic attraction between the sea of negatively charged delocalised electrons and the positively charged metal ions.

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46
Q

Definition Of Isotopes

A

Atoms of the same element (herefore they have the same number of protons) but they have a different relative atomic mass (therefore they have a different number of neutrons

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47
Q

What is the Definiton of an Element

A

only one type of atom

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48
Q

What is the definiton of a Compound

A

2 or more different types of atoms chemically bonded together

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49
Q

What is the Definition of A Mixture

A

2 or more different types of atoms not chemically bonded together

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50
Q

What is Filtration

A

Filtration is the seperation of an insoluble solid from a liquid

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51
Q

What is Crystillisation

A

Crystillisation is the seperation of an soluble solid from a liquid

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52
Q

What is Chromatography

A

Chromotography is the seperation of mixtures you can identify the mixtures by determining its Rf value.

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53
Q

How do you calculate the Rf value

A

Distance travelled by solute/Distance travelled by solvent

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54
Q

What is Distillation

A

Distillation is the seperation of liquids based upon the different boiling points

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55
Q

What is Crude Oil made up of

A

Crude Oil is a mixture of different hydrocarbons of different chainlengths

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56
Q

Why do all Group 1 elements react in the same way

A

This is because they have one electron in the outer shell

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57
Q

What is the order of reactivity in Group 1

A

As you descend in Group 1 reactivity increases this is because the size of the atom increases and therefore the number of electron shells surrounding the positively charged nucleus increases protecting the electrostatic attraction between the positively charged nucleus the negatively charged outer electron. This makes it easier for the outer electron to be transferred in reactions

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58
Q

One way to identify the order of reactivity is by (Group 1)

A

Alkali metal + Water -> Metal Hydroxide + Hydrogen
Hydrogen -> Squeaky Pop test
To carry out this test use a lighted splint and place it above the chamber in which the reaction has taken place

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59
Q

What are Group 7 elements regarded as

A

Halogens

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60
Q

What is the state of Cl at room temp

A

Cl is a green reactive and poisonous gas

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61
Q

What is the state of Bromine at room temp

A

Br is a poisonous red-brown liquid that produces orange vapour

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62
Q

What is the state of Iodine at room temp

A

forms a dark grey crystalline solid that produces purple vapour

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63
Q

What is the trend in the Boiling Point in the group (Group 7)

A

Boiling Point increases as you go down the group. This is because the size of the atom increases

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64
Q

What is the trend of reactivity in group 7

A

As you descend down the group reactivity decreases, this is because the size of the atom increaaes and the amount of electron shells protecting the electrostatic attraction between the positively charged nucleus and the negative charged external electron increases. This makes it much more difficult for the halogen to attract an electron and therefore react in a chemical reaction

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65
Q

What is a Displacement Reaction

A

A displacement reaction is where a more reactive element pushes out a less reactive element from a compound

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66
Q

What are the three states of matter

A

Solid Liquid Gas

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67
Q

Describe the arrangement of a Solid

A

Packed, Strong and regular arrangement
Vibrating around its own position
Connected to each other by strong molecular bonds

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68
Q

Describe the arrangement of a Liquid

A

Less regular arrangement

Particles have slightly greater kinetic energy compared to particles at solid state

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69
Q

Describe the arrangement of A Gas

A

Have large amounts of Kinetic Energy

Move in all random directions

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70
Q

What are Isotopes?

A

Atoms of the same element that have a different number of neutrons
(Same atomic number but different RAM)

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71
Q

What is the trend of Group 7 halogens in the group? In terms of Boiling Point?

A

Boiling Points of the halogens increase as you descend down the group. We know this as Fluorine and Chlorine are gases at room temperature, bromium is liquid at room temperature and iodine and astatatine are both solids at room temperature.

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72
Q

What is the trend of Group 7 halogens in the group in terms of reactivity?

A

The order of reactivity descends as you go down the group because the size of the atom increases. Therefore the number of shells protecting the electrostatic attraction between the positively charged nucleus and the negatively charged external electrons decreases. This makes it much more difficult for the halogen to accept the external electron and therefore to participate in a chemical reaction.

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73
Q

If you start with Potassium Chloride (Kcl (aq) colourless)

and add Cl2 water what will you observe

A

No reaction

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74
Q

If you start with Potassium Chloride (Kcl (aq) colourless) and add Br2 water, what will you observe?

A

No reaction

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75
Q

If you start with Potassium Chloride (Kcl (aq) colourless) and add I2 water, what will you observe)

A

No reaction

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76
Q

If you start with Potassium Bromide (KBr (aq) colourless) and add Cl2 water what will you observe?

A

Orange Solution (Br2)

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77
Q

If you start with KBr aq colourless and add Br2 water, what will you observe?

A

No reaction

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78
Q

If you start with KBr aq colourless and I2 water, what will you observe?

A

No reaction

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79
Q

If you start with KI (aq) and add Cl2 water, what will you observe?

A

Brown

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80
Q

If you start with KI and add Br2 water, what will you observe?

A

Brown

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81
Q

If you start with KI and add I2 water, what will you observ?

A

No reaction

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82
Q

What is a redox Reaction?

A

A redox reaction is where a substance in a chemical reaction is reduced or oxidised

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83
Q

What happens to a substance if it is Oxidised and Reduced?

A

Oxidiation- Loss of Electrons and gains O2

Reduction-Gains Electrons and loses O2

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84
Q

What is an Oxidising agent?

A

A substance that has the abillity to oxidise other substances.

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85
Q

What is a Reducing agent?

A

A substance that has the abillity to reduce other substances

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86
Q

How much Nitrogen is in the atmosphere? (%)

A

78

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87
Q

How much Oxyen is in the atmosphere? (%)

A

21

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88
Q

How much Argon is in the atmosphere? (%)

A

1

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89
Q

How much Carbon Dioxide is in the atmosphere? (%)

A

0.04

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90
Q

What happens to Magnesium when Burnt?

A

Produces Magnesium Oxide which forms a white powder

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91
Q

What colour flame does Mg produce when Burnt?

A

White Flame

92
Q

What happens when you dissolve Mg in water?

A

It produces a slight Alkaline Solution

93
Q

What happens when burning Hydrogen in water? Represent this in an equation? What kind of flame does it produce?

A

We produce Water
2H2 + O2 –> 2H2O
It produces an orange/ yellow flame

94
Q

What is the test for the presence of H?

A

We use a lighted splint and should obtain a squeaky pop

95
Q

If we burn Sulfur with Oxygen what do we obtain? What colour flame do we obtain? What will obtain if we mix it in water?

A

Sulfur Dioxide
Blue Flame
We will produce Sulfuric Acid in water

96
Q

What does thermal decomposition of metal carbonate produce? Represent this in an equation?

A

CuCO3 __> CuO + Co2

We will produce Co2 and Metal Oxide as well

97
Q

What is the Greenhouse Effect?

A

We release Greenhouse Gases which traps Infrared Radiation emmited by the sun (some of Ir radiation escapes) which leads to Global Warming

98
Q

Consequences of Greenhouse Effect?

A

Global Warming –> Climate Change __> Sea Levels Rising __> Flodding __> Habitat Loss __> Extinction loss of Biodiversity __> Loss of Agricultural areas (crops) affects economy

99
Q

What are the Major Contributions of Rising Co2 levels?

A

Combustion of Fossil Fuels

Deforestattion

100
Q

What is the order of the reactivity series?

A 
K
Na
Li
Ca
Mg
Al
Zn
Fe
Cu
Ag
Au
101
Q

How can we determine the Reactivity of Metals?

A

When comparing the reactions of two or more different metals we can add Hydrochloric Acid to the metals, This is because which ever metal produces bubbles much more frequentley in the test tube will be more reactive.

102
Q

What Metals can we add acid to in order to find their reactivity? And why can we not use acid to find out other metals reactivity?

A

K, Li, Na and Al. We cant use acid to find out the reaction of other metals as other metals wont be able to react with acid at all meaning that we will not be able to determine which metal out of the metals that have no reaction with acid are more reactive.

103
Q

Metal + Water

A

Metal Hydroxide + Hydrogen

104
Q

Metal + Steam

A

Metal Oxide + Hydrogen

105
Q

What are the two ways to prevent rusting?

A

Barrier Methods: Painting, Coating with plastic, Oiling and greasing
Galvanising: Coat a more reactive metal instead of iron. We do this so that Iron does not react with Oxygen (Oxdiation)

106
Q

What is rusting?

What is the equation that is shown for this?

A

Iron + Oxygen + Water __> Hydrated Iron (iii) Oxide

. The process in which Iron is oxidised

107
Q

What is Electrolysis?

A

The breakdown of a substance using electricity

108
Q

What can Electrolysis be used for?

A

It can be used to extract metals from metal oxide

109
Q

What are common metals that are extracted?

A

Copper, Iron and aluminium. These tend to exist in their metal oxide form within their metal ores.

110
Q

What is one way of gaining a reactive metal? and what is another way of gaining an unreactive metal

A

Seperation as they form compounds

Non reactive metals can be dug up

111
Q

Why is it worse for a company to try and dig up a reactive metal?

A

The more reactive a metal is, the harder it is to extract it from its compound as the electrostatic force off attraction between the ionic compound or metallic compound is so strong that it requires a lot of energy to break.

112
Q

What can we use as a reducing agent if metals are found in their oxide form? What is the equation shown for this?

A

Carbon (reducing agent)

2CuO + C –> Co2 + 2Cu

113
Q

Why cant Carbon be used all the time for the extraction of metals? What are some examples of Metals that cant be displaced by Carbon?

A

Some metals are more reactive than carbon so therefore carbon cant displace the metal. Eg: K, Na, Ca, Mg and Al

114
Q

What can we do instead of displacement reactions in order to gain the metal that is more reactive than carbon?

A

Electrolysis

115
Q

How does electrolysis work?

A

In electrolysis youll have a tank filled with an ionic compound that you wish to extract (Molten) as well as a cathode and an anode. Since Cathodes are PAWsitive ions the Cations willl move towards the negative elctrode (cathode). Since Anions are negatively charged ions, Anions move towards the positive electrode (Anode). Then electrons flow across the Anode to the Cathode making the Cation reduced to form an Atom. The atom then sinks to the bottom of the electrolysis to be scraped.

116
Q

How can we classify substances as strong or weak acid and strong or weak alkalis?

A

pH Scale

117
Q

What are the four 4 different types of indicators?

A

Litmus
Methyl Orange
Phenolphathlein
Universal Indicator

118
Q

What is Neutralisation? What is the equation shown for this?

A

When acids and alkalis react forming a salt with a pH of 7

H+ (aq) + OH- (aq) —> H2O (l)

119
Q

How does Neutralisation work?

A

Acid donates protons which are then accepted by the base.

120
Q

What colour does Phenophaelin turn when acidic and alakaline?

A

Acid: Colourless
Alkali: Pink

121
Q

What colour does Litmus turn when Acid or Alkali?

A

Acid: Red
Alkali: Blue

122
Q

What colour does Methyl Orange turn when acid or alkali?

A

Acid:Red
Alkali:Yellow

123
Q

Metal Oxide + Acid

A

Salt + Water

124
Q

Metal Hydroxide + Acid

A

Salt + Water

125
Q

Acid + Ammonia

A

Ammonia Salt

126
Q

Acid + Metal + Carbonate

A

Salt + Water + Hydrogen

127
Q

What is the equation of atom economy?

A

Mass of Atoms of desired product/Mass of Atoms in reactants

x100

128
Q

What are the three anions you need to test for?

A

Carbonates, Sulfates, Halide Ions (Group 7 halogens)

129
Q

How do you test for carbonates?

A

.You need to react Hcl or any acid to the Carbonate
.Then you can test for Co2 (If limewater turns cloudy in the presence of Co2)
As 2Hcl + Co3 –> Co2 + H2O

130
Q

How do you test for Sulfates?

A

We test for sulfates using Hydrochloric Acid and Barium Chloride (Barium Chloride is more important).
We should then get Barium Sulfate which forms a white precipitate which tells that sulfate is present.
XSo4 (2-) + BaCl2 –> BaSO4

131
Q

How do you test for Halide Anions?

A

You must add (Nitric acid and Silver Nitrate to the Halide anion). The Silver Nitrate (AgNo3) then disperses which allows Silver to react with the Halide anion. If this performs a precipitate colour according to the certain halide anion, it is an anion.

132
Q

What colour should Agcl turn in a Halide anion test?

A

White Precipitate

133
Q

What colour should AgBr turn in a Halide anion test?

A

Creamy Precipitate

134
Q

What colour should AgI turn in a Halide anion test?

A

Yellow Precipitate

135
Q

What are the three tests for Cations?

A

Flame tests
Reaction with Sodium Hydroxide
Ammonium Ions

136
Q

How to detect Cations with flame tests?

A

To detect cations, flame tests can be used to detect positive metal ions.

137
Q

What colour what Li turn in a flame test?

A

Red flame

138
Q

What colour would Na turn in a flame test?

A

Yellow flame

139
Q

What colour would K turn in a flame test?

A

Lilac flame

140
Q

What colour would Ca turn in a flame test?

A

Orange/Red flame

141
Q

What colour would Cu turn in a flame test?

A

Blue/Green flame

142
Q

How to detect Cations by reactiong wih Sodium Hydroxide?

A

because many metal hydroxides are insoluble, they will form out of the solution to produce crystals (colours of crystals will differ).

143
Q

What are three examples of equations of Metal Ions with Sodium hydroxide ions?

A

Cu 2+ + 2OH- –> CuOH
OH- + Fe2+ –> Fe 2+ (OH)-2
Fe3+ OH- –> Fe3+ (OH)-3

144
Q

What colours should form when Sodium Hydroxide reacts with Metal ions?

A

CuOH –> Blue Precipitate
Fe 2+ (OH)-2 –> Sludgy green precipitate
Fe 3+ (OH)-3 –> Red/Brown

145
Q

How to test for Ammonium Ions?

A

Ammonia - NH3, meaning that N needs 3 electrons to become N3-. When Ammonium combines with another H it becomes an Ammonium Ion (NH4+). To detect for ammonium compounds, you nust react it with NaOH, This produces Ammonia (gas) meaning that it is an alkali. The we can test for Alkalis using Litmus paper which should be blue.

146
Q

What is the Colour Change of Copper Carbonate in Decomposition?

A

Green –> Black

147
Q

What are Properties that make Co2 suitable for use as a fire extuingisher

A

Unflammable (doesn’t support combstion)

Can be compressed into the extuingisher

148
Q

Observations when Na reacts with Water?

A

Na gets smaller
Na starts to move around
White Tail
Causes Litmus Paper/ Solution to turn blue

149
Q

Observations when Lithium reacts with water?

A

Not very reactive

150
Q

Observations when Potassoum reacts with water?

A

Lilac Flame

151
Q

Sodium + Water

A

Sodium hydroxide + Hydrogen

152
Q

What is the Periodic Table based on?

A

Atomic Number

153
Q

Are Group 8/0 Halogens reactive?

A

No

154
Q

Why is a glass rod used rather than a metal spatula?

A

Glass won’t react with metal. Metal spatula will react. Metal can conduct heat leading to burn

155
Q

What is a Precipitation reaction?

A

When Two soluble solutions react to create a solid

156
Q

How will a student know when the X stops reacting with HCL?

A

When it is fully saturated causing the X to stop dissolving in the Hcl

157
Q

Tests for Cu2+, Fe2+ and Fe3+?

A

Add Sodium Hydroxide

Observe Colour of Precipitate

158
Q

What colour of precipitate will Cu2+ turn when reacting with Sodium Hydroxide? Give the Chemical Equation?

A

Copper (II) Blue Precipitate

Cu2+ (aq) + 2OH (aq)–> Cu(OH)2 (s)

159
Q

What Colour of Precipitate will Fe2+ turn when reacting with Sodium Hydroxide? Give the Chemical Equation?

A

Iron (II) Green Precipitate

Fe2+ + 2OH- –> Fe(OH)2

160
Q

What Colour of Precipitate will Fe3+ turn when reacting with Sodium Hydroxide? Give the Chemical Equation?

A

Iron (III) Brown Precipitate

Fe3+ + 3OH- –> Fe(OH)3

161
Q

What is the use of titration?

A

To calculate the Vol of acid needed to neutralise an alkaline of known quantity and concentration

162
Q

How do you carry out a Titration experiment?

A

Calculate how much acid is nedded to neutralise an alkali (vice versa)
Add a known Quantity of known Conc. of Alkali into a Conical Flask using a pipette and a pipette filter.
Add a few drops of phenolphalein indicator (Vice Versa)
Fill burette with acid (Vice Versa)
Using Burette add acid into the conical flask a little bit at a time (Vice Versa)
Add slowly when measuring near the end point
Indicator will change colour when an alkali is neutralised (Vice Versa)
Record the Volume used (Acid)
Stop when you get Concordant Results

163
Q

How do you carry out a Titration experiment?

A

Calculate how much acid is nedded to neutralise an alkali (vice versa)
Add a known Quantity of known Conc. of Alkali into a Conical Flask using a pipette and a pipette filter.
Add a few drops of phenolphalein indicator (Vice Versa)
Fill burette with acid (Vice Versa)
Using Burette add acid into the conical flask a little bit at a time (Vice Versa)
Add slowly when measuring near the end point
Indicator will change colour when an alkali is neutralised (Vice Versa)
Record the Volume of acid needed to neutrlise all thealkail (vice versa). Repeat a few times for concordant results.

164
Q

Phenolphalein indicator

A

Acid: Colourless
Alkali: Pink

165
Q

Methyl Orange

A

Acid: Red
Akali: Yellow

166
Q

Are all Na+, K+, NH4+, NO3- Soluble?

A

Yes Sodium, Potassium, AMmoniun and Nitrates are all soluble

167
Q

Are CL-,

SO4 2- Soluble?

A

All soluble apart from AgCl, PbCl2

All Soluble except from PbSO4, BSO4, CaSO4

168
Q

Are CO3 2- and

OH- Soluble?

A

All insoluble except for Na, K, NH4

All Insoluble except for NaOH-, Ca(OH-)2, KOH-

169
Q

Describe how the student could produce a pure, dry sample of crystals from the filtrate in Step 5?

A

Heat up the filtrate, until crystallisation takes place
Leave the Solution to cool and filter the solution to remove crystals
Wash the crystals with a small amount of deionised water
Dry the crystals using a tissue paper

170
Q

Give a reason for a an anomaly?

A 
Wrong Quantity 
Parallax Error
Equipment may be faulty
Some of the solution may be lost transferring to a beaker
Lack of precision
171
Q

What happens when an element goes from a gas to a liquid?

A

Kinetic Energy of particles increases. Intermolecular forces become broken resulting in Particles moving further apart.

172
Q

Suggest reasons why the actual mass obtained is less than the maximum theoretical mass?

A

Some of it is impure

Some Product was lost during transfer between apparatuses

173
Q

What is the definition of Electrolysis?

A

The Breakdown of an Ionic Compound using electricity

174
Q

What are the colours of Group 7 Halogens at room temperature?

A

F2 - Yellow Gas
Cl2 - Green Gas
Br2 - Red-Brown Liquid (Orange Brown Vapour)
I2 - Grey Solid (Purple Vapour)

175
Q

What is Polymerisation?

A

The joining up of lots of little molecules (monomers) to make one big molecule (polymer).

176
Q

What is Addition Polymerisation?

A

When Molecules simply add onto each other without anything else being formed

177
Q

What is the use Poly(ethene)?

A

Low Density - Thin film to make Polythene Bags
(Flexible and not very strong)

High Density- Plastic Bottles and Milk bottles

178
Q

Uses of Poly(Propene)?

A

Makes Ropes and Crates

179
Q

Uses of Poly(Chloroethene)?

A

(PVC)
Used for water pipes or replacement windows

Can be made flexible by adding plasticisers

Useful for sheet floor coverings, and even clothing.

Can be used for electrical insulation as they don’t conduct electricity

180
Q

Uses of Polytetrafluoroethene?

A

Often used as a non-stick coating for pots and pans because it is very unreactive due to the strong carbon-fluorine bonds, and can be found lining containers for corrosive chemicals.

181
Q

What do Some Microorganisms use as an energy resource for the oxidation of alcohol?

A

Can use microbes as an energy resource

Carry out aerobic respiration

Use O2 from open air to oxidise to the alcohol

182
Q

What happens when Alcohols are Oxidised?

A

Turn into Carboxylic acids

Conditions:

Potassium (VII) Dichromate in Sulfuric Acid is the Oxidising agent needed for this reaction.

Heat the ethanol with potassium dichromate in sulfuric acid –> Ethanoic acid

183
Q

Is a positive Delta H endothermic or exothermic?

A

Endothermic

184
Q

Fuel + Oxygen

A

Fuel + Oxygen –> Carbon Dioxide + Water

185
Q

What are the Fractions of Hydrocarbons from small to big? and Uses?

A 
Refinery Gases - Bottled Gas
Gasoline - Cars
Kerosene - Jet Fuel
Diesel - Lorries
Fuel Oil- Ships 
Bitumen - Roads
186
Q

In a Typical Fractionating column? How does the colour, boiling point and visocity differ in the fractionating column?

A

The bottom of the fraction has the larger crude oil chainlengths

Larger fractions of crude oil

.have higher boiling points
.are darker (in colour)
.have higher viscosities / are
more viscous

187
Q

Definition of Bioddegrade?

A

(polymer) breaks down / decomposes /
decays

M2 by bacteria / microbes / microorganisms /
decomposers /enzymes

188
Q

Is magnesium oxide a basic oxide or an acidic oxide?

A

Basic oxide formed from a non-metal

189
Q

Two observations when Magnesium reacts with O2?

A

White Solid

bright / white / blinding AND flame / light

190
Q

Why does Ammonia travel faster than HCl?

A

Lower Molar mass

191
Q

Are the Common Salts of Sodium, Potassium and Ammonium Soluble or Insoluble?

A

Soluble

192
Q

Advantages of Using Landfills to remove plastics?

A

No greenhouse gases or toxic gases produced from plastics

Cheap

193
Q

Disadvantages of using Landfills to remove plastics?

A

Ugly, Smelly and noisy; no one wants to live next to a landfill site

Uses large areas of land

Will be there for thousands of years

194
Q

Advantages of using Incineration as a method of removing Addition Polymers

A

Requires little space

Can produce for local homes and/or produce electricity

195
Q

Disadvantages of using Incineration as a method of removing Addition Polymers?

A

Expensive to build and maintain

Produces greenhouse gases

Releases Toxic Gases

The ash produced must still be disposed of in landfill sites

196
Q

What conditions are required for the Hydration of Ethene?

A

Starting Matierals: Ethene and Steam

Temperature: 300 C’

Pressure: 60-70 atmospheres

Catalysts: Phosphoric Acid

197
Q

What conditions are required for Fermentation?

A

Starting Matierals: Glucose

Temp: 30 C’

Catalyst: Enzymes in yeast

Other Conditions: Anaerobic

Slow, inefficent and produces very impure ethanol which needs further processing

198
Q

Properties of Aluminium?

A 
Light Weight
Corrosion Resistant
Conductive
Ductile
Non-Magnetic
Reflective
Strong at Low temp
199
Q

Uses of Aluminium?

A 
Construction 
Aeroplanes
Powerlines
Al foil
Kitchen utensils
200
Q

Properties of Copper

A 
Malleable and Ductile
Low Reactivity
Good Conductor
softer than Zinc
can be polished
201
Q

Uses of Copper?

A

Hospitals
Wires
Water Pipes
Pots and Pans

202
Q

Properties of Mild Steel?

A 
High Tensile Strength
High Impact Strength
Good Ductility
Magnetic
Malleable
203
Q

Uses of Mild Steel?

A 
Steel from buildings 
Constructions
Long Pipes
Bridges and Construction
Metal fences
204
Q

Properties of High Carbon Steel

A

Very High Strength
Very hard and resistant
Moderate Ductility
Hard but Brittle

205
Q

Uses of High Carbon Steel?

A

Cutting tools

Utensils

206
Q

Properties of Stainless Steel?

A 
Hot Strength
Corrosion Resistant
Cryigenic
Magnetic Response
Ductile
High Strength
Does not Rust
207
Q

Uses of Stainless Steel?

A

Surgical Tools
Architecture
Automotive and aerospace applications

208
Q

BENDO

MEXO

A

Making bonds releases energy (Exo)

Breaking bonds needs energy (Endo)

209
Q

Examples of Exothermic reactions?

A

Neutralisation

Combustion

210
Q

Examples of Endothermic Reactions?

A

Thermal Decomposition

211
Q

Reactivity series

A 
K
Na
Ca
Mg
Al
C
Zn
Fe
Sn
Pb
H
Cu
Ag
Au
Pt
212
Q

Which Ions would be all soluble?

A

Sodium, potassium, ammonium and nitrates

213
Q

Solvent meaning?

A

usually liquid substance capable of dissolving or dispersing one or more other substances

214
Q

Solute meaning?

A

A solute is a substance, usually a solid, that is dissolved in a solution, which is usually a liquid.

215
Q

Solution meaning?

A

A homogenous mixture of two or more substances in relative amounts that can be varied continuously up to what is called the limit of solubility.

216
Q

Solubility meaning?

A

the degree to which a substance dissolves in a solvent to make a solution

217
Q

The explanation for the Movement of Bromine Gas?

A

The air and bromine particles are moving randomly and there are large gaps between particles.
The particles can therefore easily mix together.

218
Q

Explanation for the Diffusion of potassium manganate in water over time?

A

The water and potassium manganate (VII) particles are moving randomly and the particles can slide over each other.
The particles can therefore easily mix together.

219
Q

Why is Diffusion SLower in Liquids than Gases?

A

Diffusion in liquids is slower than in gases because the particles in a liquid are closely packed together and move more slowly.

220
Q

Examples of Solvent?

A

the water in seawater

221
Q

Examples of Solute?

A

The Salt in Seawater

222
Q

Saturated Solution?

A

A solution with the maximum concentration of solute dissolved in the solvent

223
Q

What affects the Solubility of Solids?

A

Solubility of solids is affected by temperature. As temperature increases, solids become more soluble

224
Q

What affects the Solubility of Gases?

A

The solubility of gases is affected by temperature and pressure. As pressure increases, gases become more soluble. As temperature increases, gases become less soluble, in general.

225
Q

How is Solubillity Expressed?

A

g per 100 g of solvent

Chemistry (8 decks)

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