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Chemistry > Third Year > Flashcards

Third Year Flashcards

(78 cards)

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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
Metal atoms lose electrons to form ?
Cations
26
Non metal atoms gain electrons to form?
Anions
27
What is ionic bonding
The force of attraction between oppositely charged ions
28
Why do compounds with giant ionic lattices have high melting and boiling points?
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
29
Why don’t ionic compounds conduct electricity when solid?
No freedom to move - only conduct electricity when molten and in aqueous solutions
30
Diamond ?
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
31
Graphite ?
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
32
C60 fullerene ?
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
What is covalent bonding between
Non metals and non metals
34
What happens in covalent bonding
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
What is the ‘bond’?
The bond is the electrostatic attraction between the negatively charged pair of electrons shared between the 2 atoms and the positively charged nucleus
36
What are the diatomic elements with single bonds?
H2, F2, Cl2, Br2, I2
37
What are the diatomic element le with double or triple bonds?
O2, N2
38
What are the diatomic compounds
HCl
39
What are the inorganic molecules
H2O NH3 CO2
40
What are the organic molecules
CH4, C2H6 (ethane), C2H4 (Ethene)
41
What are the organic molecules containing halogen atoms?
C2H5Cl (chloroethane) | C2H3Cl (chloroethene)
42
Simple molecular substances
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
Giant covalent
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
General word equation for Alkali metals
Metal + water = metal hydroxide + hydrogen
45
When metals react and lose electrons, they become?
Oxidised
46
What happens in group 1
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
Down group 1
Element becomes more reactive, MP decreases (suggesting the metabolic bonding becomes weaker) Element becomes denser
48
Lithium
Fizzes and floats
49
Sodium
Melts into a ball, fizzes and floats
50
Potassium
Burns with lilac flame | Fizzes and floats
51
Rubidium
Sinks, vigorous reaction
52
Caesium
Sinks | Explosive
53
Metal + oxygen
= metals oxide
54
Metal + acid
= salt + hydrogen
55
Reactivity series
``` Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Nickel Tin Lead Copper mercury Silver Gold Platinum ```
56
Displacement
A more reactive element will displace the positive ion of a less reactive element from a compound
57
Practical for displacement
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
What does iron need to rust
Oxygen and water
59
What are 3 ways to prevent rusting
Galvanising Sacrificial protection Barrier methods
60
What is galvanising
Iron is coated in thin layer of zinc
61
What is sacrificial protection
Magnesium and zinc are used as sacrificial protection Should be periodically replaced They are more reactive than iron
62
What is barrier methods ?
Coating iron in oil or paint
63
What is oxidation
Loss of electrons and gain or oxygen
64
What is reduction
Gain of electrons and loss of oxygen
65
Oxidising agent
= reduction (usually a non metal)
66
What is reducing agent
=oxidation (usually a metal or negative ion)
67
What are group 7 non metals called
Halogens
68
Colours of halogens
``` F - pale green gas Cl - green gas Br - brown/red liquid I - grey solid (sublimates to purple vapour) At - black solid (radioactive) ```
69
What happens going down group 7
Melting and boiling points increase Molecules become larger Intermolecular forces get stronger More energy is needed to overcome these forces
70
Halogen + metal
= salt
71
Halogens become ...... reactive going down the group?
Less reactive
72
Displacement reactions for halogens
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
% gases in atmosphere
Nitrogen - 78 Oxygen - 21 Argon - 0.9/1 Carbon dioxide - 0.04
74
Element + air
Volume always decreases to 79% | 21% is used up for oxygen
75
Mg in oxygen
Bright blue flame
76
Sulfur in oxygen
Bright blue flame, smoke created
77
Hydrogen in oxygen
Louder explosion than in air
78
Equation for thermal decomposition
Metal carbonate - metal oxide + carbon dioxide

Chemistry (17 decks)

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