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Chemistry > Third Year > Flashcards

Third Year Flashcards

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1
Q

Element

A

A substance containing only 1 type of atom

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2
Q

Compound

A

A substance contains 2 or more types of atoms chemically combined

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3
Q

Mixture

A

Two or more types of atoms mixed together but not chemically combined

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4
Q

What is simple distillation?

A

Obtaining water from a solution

Boil the water then condense the vapours

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5
Q

What is fractional distillation?

A

Separating mixtures of liquids

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6
Q

What is filtration?

A

Obtaining a solid from a suspension

Solid left on the paper is called the residue, the liquid that passes through the filtrate paper is called the filtrate

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7
Q

What is crystallisation?

A

As the water from a solution evaporates, the solution can no longer hold as much dissolved solute and so some of the solute crystallises out

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8
Q

Why doesn’t the temperature rise when boiling ethanol?

A

The energy is used to overcome forces rather than heat it up

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9
Q

What is paper chromatography?

A

Separating mixtures of different coloured dyes from each other

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10
Q

What 3 things does paper chromatography show?

A

How many dyes there are

How soluble each dye is

Whether a pen is permanent

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11
Q

How to calculate the rf value ?

A

Measure to the middle of the spot

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12
Q

Chromatography process

A

1) draw a pencil line 2cm from the bottom of the paper
2) draw a spot on the paper for each pen
3) label each spot
4) place 1cm depth of water in the beaker
5) place chromatography paper in bracket
6) leave paper in the beaker until the water is near the top

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13
Q

Atom

A

A particle of matter containing a single nucleus (number of protons is balanced by equal number of electrons)

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14
Q

Molecule

A

Two or more atoms joined together with covalent bonds

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15
Q

Atomic number

A

Number of protons in the nucleus

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16
Q

Mass number

A

Number of protons and neutrons in the nucleus

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17
Q

Isotopes

A

Atoms of the same element with different numbers of neutrons

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18
Q

Relative atomic mass

A

The average mass of all the different isotopes of an element on a scale where 12C atoms have a mass of exactly 12

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19
Q

How to calculate the relative atomic mass?

A

Times the mass number by the abundance % for each element, add, then divide by 100

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20
Q

Groups

A

Columns - how many are in the outer shell

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21
Q

Periods

A

Rows - how many shells are occupied

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22
Q

Metal oxides that dissolve in water form ?

A

Alkaline solutions

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23
Q

Non metal oxides that dissolve in water form ?

A

Acidic solutions

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24
Q

What are ions?

A

Contain full outer shells of electrons - in reactive

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25
Q

Metal atoms lose electrons to form ?

A

Cations

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26
Q

Non metal atoms gain electrons to form?

A

Anions

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27
Q

What is ionic bonding

A

The force of attraction between oppositely charged ions

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28
Q

Why do compounds with giant ionic lattices have high melting and boiling points?

A

Oppositely charged ions attract each other
Strong force of attraction
Lots of these ions in a solid, therefore lots of energy is needed to overcome these forces
MP and BP very high

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29
Q

Why don’t ionic compounds conduct electricity when solid?

A

No freedom to move - only conduct electricity when molten and in aqueous solutions

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30
Q

Diamond ?

A

Covalent bonding
Giant covalent structure (each carbon atom is covalently bonded to 4 other atoms)
Very poor conductivity - no ions, no electrons capable of moving away from atoms
Very hard - very rigid lattice

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31
Q

Graphite ?

A

Covalent bonding
Giant covalent (each carbon atom is covalently bonded to 3 other atoms )
Very good conductivity - extra electron can move
Very soft - only weak forces between layers, layers can slide over each other easily

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32
Q

C60 fullerene ?

A

Covalent bonding
Simple molecular (each molecule has 60 carbon atoms joined together, forces between molecules are weak, but forces within molecules are strong)
Very poor conductivity - no ions, no electrons capable of moving away
Not very hard - only weak force between molecules, forces are easy to break

33
Q

What is covalent bonding between

A

Non metals and non metals

34
Q

What happens in covalent bonding

A

Electrons are shared between the atoms to produce full outer shells
Atoms join together to make a molecule
Each pair of shared electrons is a covalent bond
The compound formed is made of molecules (molecules arent joined together)

35
Q

What is the ‘bond’?

A

The bond is the electrostatic attraction between the negatively charged pair of electrons shared between the 2 atoms and the positively charged nucleus

36
Q

What are the diatomic elements with single bonds?

A

H2, F2, Cl2, Br2, I2

37
Q

What are the diatomic element le with double or triple bonds?

A

O2, N2

38
Q

What are the diatomic compounds

A

HCl

39
Q

What are the inorganic molecules

A

H2O
NH3
CO2

40
Q

What are the organic molecules

A

CH4, C2H6 (ethane), C2H4 (Ethene)

41
Q

What are the organic molecules containing halogen atoms?

A

C2H5Cl (chloroethane)

C2H3Cl (chloroethene)

42
Q

Simple molecular substances

A

Melting or boiling of them does not involve braking strong covalent bonds
Only weak forces are broken
Not much energy is required to overcome the forces, therefore the MP and BP is low

43
Q

Giant covalent

A

No molecules - all atoms are linked via a series of covalent bonds
Large number of bonds have to be broken in order to melt or boil
High mp and bp

44
Q

General word equation for Alkali metals

A

Metal + water = metal hydroxide + hydrogen

45
Q

When metals react and lose electrons, they become?

A

Oxidised

46
Q

What happens in group 1

A

The atoms of each element get larger going down the group
The outer shell of electrons gets further away from the nucleus - shielded by more shells
Yeh further the electron is from the positive nucleus, the easier it can be lost in reactions

Reactivity of alkali metals increases going down group 1

47
Q

Down group 1

A

Element becomes more reactive, MP decreases (suggesting the metabolic bonding becomes weaker)
Element becomes denser

48
Q

Lithium

A

Fizzes and floats

49
Q

Sodium

A

Melts into a ball, fizzes and floats

50
Q

Potassium

A

Burns with lilac flame

Fizzes and floats

51
Q

Rubidium

A

Sinks, vigorous reaction

52
Q

Caesium

A

Sinks

Explosive

53
Q

Metal + oxygen

A

= metals oxide

54
Q

Metal + acid

A

= salt + hydrogen

55
Q

Reactivity series

A 
Potassium 
Sodium 
Lithium 
Calcium 
Magnesium 
Aluminium 
Zinc 
Iron 
Nickel 
Tin 
Lead 
Copper 
mercury 
Silver 
Gold 
Platinum
56
Q

Displacement

A

A more reactive element will displace the positive ion of a less reactive element from a compound

57
Q

Practical for displacement

A

Add a small amount of each metal on the spotting tile
Add each solution of metal salt to each of the metals
Record the results

58
Q

What does iron need to rust

A

Oxygen and water

59
Q

What are 3 ways to prevent rusting

A

Galvanising
Sacrificial protection
Barrier methods

60
Q

What is galvanising

A

Iron is coated in thin layer of zinc

61
Q

What is sacrificial protection

A

Magnesium and zinc are used as sacrificial protection
Should be periodically replaced
They are more reactive than iron

62
Q

What is barrier methods ?

A

Coating iron in oil or paint

63
Q

What is oxidation

A

Loss of electrons and gain or oxygen

64
Q

What is reduction

A

Gain of electrons and loss of oxygen

65
Q

Oxidising agent

A

= reduction (usually a non metal)

66
Q

What is reducing agent

A

=oxidation (usually a metal or negative ion)

67
Q

What are group 7 non metals called

A

Halogens

68
Q

Colours of halogens

A 
F - pale green gas 
Cl - green gas 
Br - brown/red liquid 
I - grey solid (sublimates to purple vapour)
At - black solid (radioactive)
69
Q

What happens going down group 7

A

Melting and boiling points increase
Molecules become larger
Intermolecular forces get stronger
More energy is needed to overcome these forces

70
Q

Halogen + metal

A

= salt

71
Q

Halogens become …… reactive going down the group?

A

Less reactive

72
Q

Displacement reactions for halogens

A

A more reactive halogen can displace a less reactive halogen from solutions of its salt

Add bromide water to each test tube containing KCl, KBr, KI

73
Q

% gases in atmosphere

A

Nitrogen - 78
Oxygen - 21
Argon - 0.9/1
Carbon dioxide - 0.04

74
Q

Element + air

A

Volume always decreases to 79%

21% is used up for oxygen

75
Q

Mg in oxygen

A

Bright blue flame

76
Q

Sulfur in oxygen

A

Bright blue flame, smoke created

77
Q

Hydrogen in oxygen

A

Louder explosion than in air

78
Q

Equation for thermal decomposition

A

Metal carbonate - metal oxide + carbon dioxide

Chemistry (17 decks)

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