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Chemistry > Seperate Chemistry 1 > Flashcards

Seperate Chemistry 1 Flashcards

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1
Q

Transition metal properties

A 
High melting / boiling point
Good heat / electric conductor 
High density 
Ductile 
Malleable 
Shiny
Hard
Colourful compounds 
Compounds are good catalysts
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2
Q

Why alloys are stronger than pure metals

A

Allows contain different elements
Atoms of different elements have different sizes
Prevents layers of atoms from sliding over each other easily

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3
Q

Properties of steel

A

Harder than iron
Stronger than iron (if carbon < 1%)
Less likely to corrode than iron

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4
Q

How to make bronze

A

copper + tin

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5
Q

Properties and uses of bronze

A

Harder than copper
Medals
Decorative ornaments
Statues

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6
Q

How to make brass

A

copper + zinc

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7
Q

Properties and uses of brass

A

more malleable than bronze
used where lower friction is needed
water taps
door fittings

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8
Q

Properties and uses of gold alloys

A

Stronger than gold

Jewellery

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9
Q

Properties and uses of aluminium alloys

A

Lower density than other metals and alloys

Aircraft manufacture

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10
Q

How to make magnalium

A

aluminium + magnesium

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11
Q

Properties and uses of magnalium

A

(low magnesium percentage)
stronger, lighter and corrodes less than aluminium
Aeroplane and car parts
(high magnesium percentage)
reactive but more stable than pure magnesium
Fireworks

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12
Q

Corrosion definition

A

When something is slowly damaged or destroyed by a chemical process

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13
Q

Rusting definition

A

Corrosion of iron

Only happens when iron is in contact with both oxygen and water

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14
Q

How corrosion of metals is a redox reaction

A

Metal loses electrons (oxidised)

Oxygen gains electrons (reduced)

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15
Q

How to prevent rusting / corrosion

A

Barrier e.g. painting/oiling/greasing (keeps water and oxygen out)
Sacrificial protection e.g. galvanising (when more reactive metal is placed with iron so oxygen and water reacts to it instead of wanted metal)

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16
Q

Galvanisation definition

A

Coating iron objects with zinc to protect them from rusting

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17
Q

Electroplating definition

A

Coating the surface of a metal with another metal using electrolysis

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18
Q

Electroplating in preventing corrosion methods

A

Cathode = object to be electroplated
Anode = bar of metal used in plating
Solution = contains metal ions used in plating
Metal ions are deposited at cathode and anode “tops up” metal ions in solution

19
Q

Titration purpose

A

How much acid is needed to neutralise a set amount of alkali (or vice versa)

20
Q

Titration method

A

Measure out set volume of alkali using pipette
Add few drops of indicator with single colour change
Fill a burette with acid of known concentration
Use burette to slowly add acid to alkali, regularly swirling flask
Stop when indicator changes colour
Record volume of acid used to neutralise alkali

21
Q

How to use titration results to work out concentration of reactants

A

Work out how many moles of reactant with given concentration are used
Use ratio of equation to find out moles of reactant with unknown concentration
Using given volume of reactant with unknown concentration and moles, work out its concentration

22
Q

How to convert mol dm-3 to g dm-3

A

Multiply by RFM

23
Q

Percentage yield equation

A

percentage yield = actual yield / theoretical yield x 100

24
Q

Actual yield definition

A

mass of product actually made

25
Q

Theoretical yield definition

A

mass of product made if all reactants were converted to products

26
Q

Percentage yield method

A

Find RFM / RAM of reactant and product
Work out moles of reactant
Use ratio of equation to work out moles of product
Work out theoretical yield by multiplying moles and RFM / RAM of product
Divide actual yield by theoretical yield and multiply by 100 to get percentage yield

27
Q

Why 100% yield is impossible

A

Incomplete reactions
Practical losses e.g. transferring chemicals between containers
Unwanted reactions

28
Q

Atom economy definition

A

Percentage of reactants changed to useful products

29
Q

Atom economy formula

A

total RFM of desired products / total RFM of total products x 100

30
Q

Disadvantages of low atom economy

A

Uses up resources quickly
Lots of waste
Makes reactions unsustainable
Resources may be expensive so not even profitable with low economy

31
Q

Factors to consider in chemical industry

A

Percentage yield
Rate of reaction
Reversible reactions
Atom economy

32
Q

Factors to consider in an industrial process

A

Cost of extracting and refining raw materials

Energy costs to control the conditions

33
Q

Haber process

A

N2 + 3H2 <=> 2NH3 (+heat)

34
Q

Haber process conditions

A

Higher pressures favour forward reaction (more molecules on left side than right)
Pressure is set as high as possible without impacting costs too much (200 atmospheres)
Forward reaction is exothermic but more heat moves equilibrium position the wrong way
Lower temperatures means lower rate of reaction so temperature is 450°C to compromise

35
Q

How catalysts and conditions affect how quickly equilibrium is reached

A

By increasing rate of reaction, the rate at which equilibrium is reached is increased

36
Q

Fertiliser facts

A

Contains nitrogen, phosphorus and potassium

Helps plants increase growth and life processes

37
Q

Ammonia fertilisers benefits over traditional fertilisers

A

Can control compositions of chemicals
Control how much is made
Soluble so chemicals can dissolve down into soil to reach plants

38
Q

Ammonium salts reaction

A

Example:

NH3 + HNO3 -> NH4O3

39
Q

Molar volume equation

A

molar volume = gas volume / number of moles

40
Q

Avogadro’s Law on molar volumes

A

same number of moles of different gases occupy the same volume
24dm3 per mol at room temperature

41
Q

How fuel cells work

A

Type of chemical cell

Reacts fuel and oxygen to produce electrical energy efficiently

42
Q

Reaction in hydrogen-oxygen fuel cells

A

hydrogen + oxygen -> water

2H2 + O2 -> 2H2O

43
Q

Advantages of hydrogen-oxygen fuel cells

A

Much more efficient (80% if heat produced is used)
Electricity is generated directly in a fuel cell (fewer places to lose energy)
No moving parts (no energy lost through friction)
No conventional pollutants (only water and heat)

44
Q

Disadvantages of fuel cells

A

Hydrogen gas is hard to store and is very explosive

Hydrogen is made from hydrocarbon or electrolysis of water, both involving the finite resource fossil fuels

Chemistry (10 decks)

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