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Chemistry

9th

382 Terms

1

Rate of reaction definition

a measure of how quickly a reactant is used up, or a product is formed.

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2

To be successful when particles collide they need

the minimum activation energy

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3

Rate of reaction equation

change in concentration, volume or mass/change in time

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4

Volume units

dm³ (1 litre)

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5

steepest part of graph

highest rate of reaction

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6

gradient on a graph

rate of reaction

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7

Effect steepness of curve

temperature, concentration, surface area and catalyst

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8

effect height of curve

mass of product/reactant

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9

collision theory

reactants in a solution must collide withe the particles on the solid surface area and have the activation energy for a reaction to occur and make the products

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10

If a collision is not succsefull

they will bounce off each other

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11

factors affecting rate

temperature, surface area, concentration, presence of a catalyst and pressure (of gas)

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12

activation energy

the minimum amount of energy required to start a chemical reaction

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13

equation to figure out rates on a graph

to find rate at a specific time draw a tangent then use that to figure out the gradient - this is the rate of reaction at that time

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14

Average rate on a graph

product produced/reactant lost / time

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15

methods for determining rates of reaction

mass lost with time, volume of gas produced or cross to disappear (if producing a solid)

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16

metal carbonate reacts with acid to form

a salt, water and carbon dioxide

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17

calcium carbonate (s) + Hydrochloric acid (aq) →

calcium chloride (aq) + water (l) + carbon dioxide (g)

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18

CaCO₃ (s) + 2HCl (aq)→

CaCl₂ (aq)+ H₂O (l)+ CO₂ (g)

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19

measuring the mass lost with time

Loses mass because the gas escapes the conical flask

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20

cotton wool plug use

so the gas can escape but the other products (like the acid) can't

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21

measuring gas produced measuring cylinder inaccurate

not all gas goes into the inverted measuring cylinder

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22

Mg (s) + 2HCl (aq) →

MgCl₂ (aq) +H₂ (g)

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23

CO₂ (g) + Ca(OH)₂ (limewater) (aq) →

CaCO₃ (aq) + H₂O (l) test for carbon dioxide

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24

CuCO₃ (s) + 2HNO₃ (aq) →

Cu(NO₃)₂ (aq) + H₂O (l) + CO₂ (g)

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25

Concentration of solutions affecting rate of reaction

Increasing the concentration of solutions means the particles are closer together, so there are more particles in a given volume. This increases the frequency of successful collisions which increases the rate of reaction.

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26

Surface area of solids affecting rate of reaction

Increasing the surface area of solids means more particles, on the surface of the solid, are in contact with the other reactant making it so there is a higher frequency of successful collisions which increases the rate of reaction

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27

Temperature affecting rate of reaction

Increasing the temperature means increasing the particles kinetic energy. this means that the particles move faster and collide more often. It also means more particles have the activation energy which increases the frequency of successful collisions and therefore the rate of reaction.

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28

Catalyst affecting rate of reaction

Catalysts provide an alternative energy pathway with a lower activation energy without loosing mass (getting used up). This means a greater proportion of the particles have the activation energy which increases the frequency of successful collisions and therefore the rate of reaction.

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29

mass rate of reaction graph

will end at a lower amount

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30

Na₂S₂O₃ (aq) + 2HCl (aq) →

2NaCl (aq) + H₂O (l) + SO₂ (g) + S (s)

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31

Catalyst

substances that speed up chemical reactions but aren't used up in the process - they are chemically unchanged

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32

homogenous catalysts

in the same state as what they speed up (enzymes are proteins that speed up protein reactions)

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33

How do catalysts find an alternative pathway

they (A) react with one product (B) and using that new product (AB) then reacts with the other product (C)

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34

hydrogen peroxide (aq) →

water (l) + oxygen (g)

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35

2H₂O₂ (aq) →

2H₂O (l) + O₂ (g)

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36

Solute

A substance that is dissolved in a solution.

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37

Solvent

the liquid in which a solute is dissolved to form a solution.

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38

Solution

a mixture of solute and solvent

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39

aqueous solution

a mixture of a solute and water

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40

saturated solution

a solution that contains the maximum amount of dissolved solute

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41

Solubility

The mass of a solute that will dissolve in 100g of water to form a saturated solution

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42

Atom

the simplest particle of an element that can still be recognised as that element

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43

Element

a substance which cannot be split into anything simpler by chemical means, and contains atoms of the same atomic number

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44

Molecule

two or more atoms covalently bonded together

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45

Relative atomic mass

The average mass of an atom relative to 1/12 of an atom of carbon-12

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46

Anion

A negatively charged ion

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47

cation

Positively charged ion

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48

Oxidation

Gain of oxygen or loss of electrons

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49

Reduction

Loss of oxygen or gain of electrons

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50

Oxidising agent (oxidant)

Oxygen donor or electron acceptor

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51

reducing agent (reductant)

oxygen acceptor or electron donor

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52

Ionic type of bonding

Metal and non metal

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53

Covalent type of bonding

Non-metal and non-metal

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54

metallic bond

metal and metal

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55

Nitrate

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56

Sulfate

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57

Hydroxide

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58

Ammonium

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59

Carbonate

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60

Zinc valency

2

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61

Silver valency

1

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62

ionic bond

a strong electrical attraction between oppositely charged ions

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63

Isoelectronic

atoms with the same electron configuration

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64

ionic: dot cross diagram

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65

A positive ion will be attracted to

any negative ion

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66

An ionic bond between chloride ions and a sodium ion

Only one is formed by share of electrons, the other by forces

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67

Why don't molecules of ionic compounds exist

because they are a giant structure (giant ionic lattice)

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68

How can a negative ion bond to any positive ion

If they are close enough

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69

properties of ionic compounds

high melting and boiling points, lack of electric conductivity when solid, brittle

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70

High melting and boiling points of ionic compounds

The strong electrostatic force of attraction between the oppositely charged ions holds the structure together. It takes a huge amount of energy to break the ionic bonds to produce a molten compound.

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71

Electric conductivity of ionic compounds

Do not react when solid because ions are fixed in place. Conducts electricity in molten or aqueous because ions can move carrying charge

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72

Brittle ionic compounds

a small distortion of the lattice structure causes like charges to repel, and the compounds to break apart.

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73

Electrostatic attraction in covalent bonds

the positively charged nuclei of both atoms are attracted to the negative electrons.

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74

Covalent bonding

The sharing of a pair or multiple pairs of electrons holds the nuclei together in a covalent bond, overcoming the repulsion of the two nuclei

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75

covalent bond

an electrostatic force of attraction between the nuclei of the atoms making up the bind and the shared pair of electrons

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76

covalent compound structure

simple molecular

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77

electricity in simple molecular

Do not conduct electricity

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78

simple molecular boiling and melting point

low

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79

Simple molecular at room temperature

liquids or gasses

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80

Simple molecular when heated

The strong covalent bonds are not broken, it is the weak intermolecular forces of attraction that are broken

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81

molecular mass increases

increases boiling and melting point

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82

more electrons in a molecule

stronger molecular forces

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83

Diamond structure type

Giant covalent

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84

Graphite structure type

Giant covalent

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85

c60 structure type

simple molecular

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86

Diamond formula

c

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87

Graphite formula

C

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88

Buckminsterfullerene formula

C60

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89

Diamond number of covalent bonds each C atom forms

4

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90

Graphite number of covalent bonds each C atom forms

3

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91

C60 number of covalent bonds each C atom forms

3

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92

Diamond melting and boiling point

very high (higher than graphite)

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93

graphite melting and boiling point

very high

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94

c60 melting and boiling point

Low but relatively high for simple molecular

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95

Diamond reason for melting and boiling points

carbon - carbon covalent bonds are very strong and require lots of energy to break

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96

Graphite reason for melting and boiling points

Carbon - carbon covalent bonds in each layer must be broken but the IMF's between layers are easier to break

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97

c60 reason for melting and boiling points

only have to break IMF's instead of covalent bonds

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98

Diamond Electrical Conductivity

None

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99

Graphite Electrical Conductivity

conductor

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100

C60 Electrical Conductivity

None

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