1
Q
How do you tell in a substance is a metal?
A
- high melting point
- malleable
- shiny
- electrical conductors
2
Q
What is a solute?
A
The substance which is going to be dissolved
3
Q
What is a solvent?
A
A liquid which is going to do the dissolving
4
Q
What is the relative mass and charge of a proton?
A
Mass - 1
Charge - +1
5
Q
What is the relative mass and charge of an electron?
A
Mass - 0.0005
Charge - -1
6
Q
What is the relative mass and charge of a neutron?
A
Mass - 1
Charge - 0
7
Q
What is the atomic number?
A
Number of protons
8
Q
What is the mass number?
A
The total number of protons and neutrons (on top)
9
Q
How do you work out the relative atomic mass?
A
(Abundance x mass number) + (abundance x mass number)
————————————————————————————
100
10
Q
What does OIL RIG stand for?
A
O xidisation
Is
Loss of electrons
Reduction
Is
Gain of electrons
11
Q
How are particles arranged in an ionic compound?
A
Giant ionic lattice
12
Q
What are ionic properties?
A
High melting points - ionic bonds are very strong and there are lots of them, lots of energy required to break bonds
Electrical conductivity - can only conduct if liquid or dissolved as particles are free to move
13
Q
Acid + base -> ?
A
Salt + Water
14
Q
What are the two components of a metallic structure?
A
- lattice of positive metal ions
- sea of delocalised ions
15
Q
Metal + water -> ?
A
Metal hydroxide + hydrogen
16
Q
What are the observations in a metal + water reaction?
A
- effervescence
- solid disappears
17
Q
What is the reactivity in group 1?
A
The group gets more reactive as you move down
18
Q
Acid + metal -> ?
A
Salt + hydrogen
19
Q
What are the observations in an acid + metal reaction?
A
- the metal disappears
- fizzing
20
Q
When a simple molecular substance boils, what’s bonds are breaking?
A
Inter molecular forces
21
Q
Why does diamond melt at really high temperatures?
A
Giant lattice structures contain lots of covalent bonds that require lots of energy to break the bonds
22
Q
What are the properties of diamond?
A
- giant structure, covalent bonds very strong, lots of energy needed
- does not conduct electricity as no electrons are free to move - they are stuck in the bonds
- used in cutting as it is hard to
23
Q
What are the properties of graphite?
A
- giant structure, covalent bonds, lots of energy required
- conducts electricity because it contains free electrons which are able to move
- every carbon bonded to 3 other carbons, 1 spare delocalised electron that can move + carry charge
- soft (solid lubricant), as weak forces between strong layers can be broken
24
Q
What are the trends in halogens?
A
- get darker as you move down the group
- less reactive down the group
- diatomic
- melting point increases down the group
25
What colours are chlorine, bromine and iodine in water?
Chlorine - pale yellow
Bromine - orange
Iodine - brown
26
What is activation energy?
The minimum amount of energy needed for a reaction to start
27
What is the collision theory?
Reactions can only happen when particles collide with sufficient kinetic energy and are in the correct orientation
28
How do you work out rate of reaction per second?
1
_________
Time (s)
29
How does increasing temperature increase the rate of reaction?
- particles have more kinetic energy
- they move faster
- more frequent collisions + larger proportion are successful
30
How does increasing the concentration increase the rate of reaction?
- More particles in the same volume
- more frequent successful collisions
31
How does reducing particle size increase rate of reaction?
- increase in surface area
- more contact between reactants
- more frequent successful collisions
32
How does using a catalyst increase rate of reaction?
- reduces activation energy
- more collisions are successful
- more frequent successful collisions
33
Carbonate + acid -> ?
Water + carbon dioxide + salt
34
Do catalysts get used up in a reaction + what state are they?
No
Solid or liquid
35
Hydrogen peroxide -> ?
Water + oxygen
36
How do you work out moles?
Use the relative formula mass and divide the grams by that
3G of H2O = 3/18 = 0.167 moles
37
How do you work out the relative formula mass?
Add the mass numbers (large one)
38
How do you work out the empirical formula?
Element. Element
Mass
RAM
Moles
Ratio
39
What is the difference between empirical and molecular formula?
Empirical - lowest ratio of elements CH2O
Molecular - actual elements C6H12O6
40
Mol = ?
Mass/RFM
41
What is crude oil?
A mixture of hydrocarbons (hydrogen + carbon)
42
Why does crude oil boil over a range of temperatures?
The different hydrocarbons have different boiling points because of the different shapes and sizes
43
What is fractional distillation?
- Separating flukes by boiling them as they have different BP
- They drain out of separate places as the top is cooler than the bottom
- Smaller hydrocarbons go out the top
44
Do small or large hydrocarbons have a low boiling point?
Small hydrocarbons
45
Are small or large hydrocarbons more flammable?
Small
46
Do small or large hydrocarbons have the Smokey flame?
Large
47
Do small or large hydrocarbons have a high viscosity?
Large
48
What is the formula for carbonate?
CO3 (2-)
49
What is the formula for a nitrate?
NO3 (-)
50
What is the formula for sulphate?
SO4 (2-)
51
What is the formula for ammonium ion?
NH4(+)
52
What are halides?
A chemical compound that contains a halogen ion
53
How do you work out an rf value?
Divide the distance the spot moved by the solvent line
54
What is the formula for ammonia gas?
NH3
55
Moles = volume/ ?
24 (dm3) or 24000 (cm3)
56
What is the equation for concentration involving moles?
Moles = concentrations x volume
57
How do you convert cm3 to dm3?
Divide by 1000
58
Acid + alkali -> ?
Salt + water
59
What do all acids produce?
Hydrogen ions
60
What happens if a base neutralises an acid?
Releases hydroxide ions
61
What is an alkali?
A soluble base
62
Acid + metal oxide -> ?
Salt + water
63
Acid + metal hydroxide -> ?
Salt + water
64
Acid + metal carbonate -> ?
Salt + water + carbon dioxide
65
Is the atomic number on the bottom or top?
Bottom
66
What is a neutralisation reaction?
Acid + alkali -> salt + water
67
How do you convert cm3 to dm3?
Divide by 1000
68
What is an endothermic process?
Breaking bonds
69
What is an exothermic process?
Making bonds
70
When is it an endothermic reaction?
If the bonds you break are stronger than the bonds you make
71
When is it an exothermic reaction?
When the bonds you break are weaker than the bonds you make
72
What is the equation for combustion calorimetry?
Q=mc∆t
73
What does everything stand for in Q=mc∆t?
Q = heat in joules (J)
M = mass in grams (g), volume of water
∆t = change in temperature
C = specific heat capacity
74
What is the test for displacement calorimetry?
- weight out 1g of the metal (iron,magnesium or zinc)
- add 25cm3 of copper sulphate into a polystyrene cup
- measure the temperature of the copper sulphate
- add the metal and store
- record the highest temperature
- use the equation Q=mc∆t
75
What does ∆h stand for and what is it measured in?
Enthalpy change
Kj/mol or Jmol-1
76
∆h = ?
-Q
77
What is an example of a basic oxide?
Copper
78
What is iodines state at room temperature?
Solid
79
How do you obtain pure water from a sugar solution?
Simple distillation
80
What pH are metals?
Alkali
81
Why is sulfuric acid not suitable in the marble chip experiment?
Insoluble calcium sulphate will form
Which will form a coating on the chips
Stopping the reaction
82
What are the characterstics of a reaction at dynamic equilibrium? - paper 2
Forward+backwards reactions occur at the same rate
Concentration of products and reactants remain constant
83
Why does a catalyst not affect the yield of dynamic equilibrium? - paper 2
It increases the rate of reaction equally on both sides
84
What is a solid turning into a gas called?
Sublimation
85
What is the chemical name for rust?
Hydrated iron (III) oxide
86
What gas is not usually found in the atmosphere?
Hydrogen
87
What colour is methyl orange in an hydroxide solution?
Yellow
88
What observations are seen when magnesium burns in oxygen?
Bright white light
White powder forms
89
How do magnesium and magnesium chloride conduct differently?
Magnesium has free delocalised electrons which are able to move
Magnesium chloride can only conduct when molten - needs ions which are free to move
90
What is the ionic half equation for the formation of chlorine at a positive electrode? - paper 2
Cl2 -> 2e- + cl
91
Why can the calculation for ∆H be much lower?
Some of the heat will be lost to surroundings
Incomplete combustion
Ethanol may be impure
92
Why does heating a liquid cause it to evaporate more quickly?
Particles have more kinetic energy
More particles have enough energy to escape
93
Why is it not possible to deduce the rfm of air?
It is a mixture
94
When copper carbonate is heated to form copper oxide and co2 what is the colour change?
Green to black
95
What is the chemical formula for copper carbonate?
CuCO3
96
Why is Ethane saturated?
Only contains single bonds
So no addition reactions can occur
Chemistry
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