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1
Q

Factors that increase the rate of reaction

A

Catalyst
Smaller particles
Higher temperature

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2
Q

How to get average rate

A

Change in quantity
—————————
Change in time

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3
Q

Structure of the periodic table

A

Elements in the same group have similar chemical properties and the same number of outer electrons

Below the black line are metals

Above the black line are non metals

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4
Q

The name of group 1

A

Alkali metals

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5
Q

Name group 7

A

Halogens

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6
Q

Name group8/0

A

Noble gases

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7
Q

Why is an atom neutral

A

Atoms are neutral as Number of protons=number of electrons

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8
Q

How to find the atomic number

A

Number of protons

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9
Q

Mass number

A

Number of protons + number of neutrons.

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10
Q

How to find number of neutrons

A

mass number- number of protons

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11
Q

Definition of isotope

A

Same element but different mass number

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12
Q

Definition of covalent bond.

A

Shared pair of outer electrons (non metals)

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13
Q

Diatomic molecules

A

Bromine, oxygen, fluorine, nitrogen, Iodine, Chlorine, hydrogen

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14
Q

Properties of a covalent molecular substance

A

Low melting and boiling points
Don’t conduct

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15
Q

Properties of a covalent network

A

High boiling/melting points
Don’t conduct

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16
Q

How positive and negative ions are made

A

Positive ions are formed when atoms LOSE their outer electrons

Negative ions are formed when atoms gain outer electrons

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17
Q

What is an ionic bond

A

The transfer of electrons between a positive metal ion and negative non metal ion

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18
Q

Properties of ionic compound

A

Dont Conduct when solid
Conduct when liquid as ions are free to move
High melting/ boiling points

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19
Q

Difference between suffix -ite/-ate and ide

A

Ite/ate is the presence of oxygen
Ide is the bond between two elements

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20
Q

How to find the mass

A

M=NxGFM

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21
Q

How to find the moles

A

N=CXV

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22
Q

How to find concentration

A

C=N/V

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23
Q

How to find the volume

A

V=N/C

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24
Q

How to find %mass

A

%m= M/GFM x 100

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25
Ph scale features
Below 7 = acidic 7= neutral Over 7 =alkaline
26
What are The two ions in water
Hydroxide Hydrogen
27
Why is water neutral
Hydrogen ions =hydroxide ions
28
What happens when you dilute an acid
The ph goes up The acidity goes down Hydrogen ions concentration decreases
29
What happens when a soluble Non metal oxide dissolves in water
an acidic solution is formed
30
Are acids a metal or non metal solution
Non metal
31
What happens when soluble metal oxide dissolves in water
Forms alkaline solution
32
What happens if an insoluble oxide is added to water
PH stays the same
33
Name the three types of chemicals we call bases
Metal oxides Metal hydroxide Metal carbonate
34
nitric acid + sodium hydroxide=??
Sodium nitrate + water
35
Propanoic acid + sodium oxide = ????
Sodium propanoate
36
Methanoic acid + sodium carbonate =????
Sodium methanoate + Carbon dioxide + water
37
What is the function of a pipette
To extract, dispense and transfer liquid samples
38
Function of a burette
To measure the volume of liquid and gases
39
What does concordant results mean
Results within 0.2 of each other
40
Why must we add an indicator in titration
To be able to view the end result
41
Why must we add an indicator in titration
To be able to view the end result
42
Titration equation
C1V1. = C2V2 ——- ——— N1. N2
43
Explain how to obtain a solid sample of the salt produced in a neutralisation experiment
Filter the mixture Evaporate the filtrate
44
Define a homologous series
Same general formula, similar chemical properties
45
WHATS a hydrocarbon
A compound that is made of only hydrogen and carbon atoms
46
Define saturated
Only single carbon to carbon bonds
47
Define unsaturated
At least one Carbon to carbon double bond
48
How to test for unsaturation
Decolorises bromine solution
49
General formula for alkane
CnH2n+2
50
General for alkenes
CnH2n
51
General formula for cycloalkanes
CnH2n
52
Definition of isomers
Same general formula but different structural formula
53
Give examples of addition reactions
Hydration Hydrogenation Halogenation
54
What is a hydration reaction
The addition of water into an alkene forming alcohol and an alkane
55
Hydrogenation
The addition of hydrogen to an alkene producing an alkane
56
The functional group of alcohols
Hydroxyl (OH)
57
General formula for alcohols
CnH2n+OH
58
Why does melting/boiling points increase with an increase in molecular mass
Stronger intermolecular bonds/ attractions
59
Properties of alcohol
Very Soluble in water Higher boiling/melting points than alkane Alcohols with lower molecular weights, like methanol, ethanol, propanol, and butanol, are miscible with water
60
Carboxylic acids functional group
Carboxyl group (COOH)
61
Properties of carboxylic acid
Smaller acids are soluble in water High melting/ boiling points Reacts with metal to form hydrogen and water
62
Define exothermic reactions
When heat energy is given out
63
Define endothermic
When heat energy is absorbed
64
What is combustion
When a fuel is burned and reacts with oxygen to release heat energy
65
Products of complete combustion
Carbon dioxide and water
66
How to calculate energy release
Eh=cm🔺T
67
What is a metallic bond
The force of attraction between the delocalised electrons of a metal and the positive metal ions
68
Why do metals always conduct electricity
Due to metallic bonding, Delocalised electrons are free to move
69
Metal + oxide= ?
Metal oxide
70
Metal + water =???
Metal hydroxide
71
Metal + oxygen=???
Metal carbonate
72
First four elements on metal reactivity series and what do they react with
Potassium Sodium Lithium Calcium They react with water as they are very reactive
73
Middle 6 elements on reactivity series and what they react with
Magnesium Aluminium Zinc Iron Tin Lead They react with acids
74
3 elements that react with oxygen on the reactivity series
Copper Mercury Silver
75
Bottom element of the reactivity series
Gold

Chemistry (2 decks)

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