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Chemistry > Topic 4 / 5 > Flashcards

Topic 4 / 5 Flashcards

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1
Q

reactivity series mnemonic

A

please stop calling me a careless zebra instead try learning how copper saves gold

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2
Q

reactivity series

A

potassium sodium calcium magnesium aluminium carbon zinc iron tin lead hydrogen copper silver gold

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3
Q

more reactive metals

A

have a greater tendency to lose electrons and form positive ions

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4
Q

silver gold and platinum

A

found underground as uncombines metals as they are unreactive so don’t chemically join with any element to form a compound

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5
Q

phytoextraction

A

+ metals can be extracted from contaminated soils
- weather dependant
- requires high temperatures (burning)
- more expensive than mining ores

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6
Q

BIOLEACHING

A

+ doesn’t require high temperatures
- releases harmful gases like sulfur dioxide which damages the environment

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7
Q

both p and b

A
  • very slow process
    + preserves supplies of higher grade ores
    + less damage to environment
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8
Q

rusting is a _________ reaction

A

oxidation reaction

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9
Q

redox reactions

A

oxidation and reduction happen simultaneously
e.g. displacement reactions

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10
Q

extracted by heating with carbon

A

metals less reactive tha corbon

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11
Q

extracted by electrolysis

A

above carbon

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12
Q

making copper

A
  1. place copper oxide and carbon powder into a crucible
  2. put thin layer of carbon powder to ensure all the copper oxide reacts
  3. place the lid
  4. heat crucible strongly
  5. solid copper produced
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13
Q

cryolite

A

an aluminium cmpound with a much lower melting point than aluminium oxide so using this reduces the cost of extracting

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14
Q

economic advangates of recycling

A

less energy needed so lower lost than mining

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15
Q

enviromental advantages

A

natural reserves of metal ores will last longer
produces less pollution
less metls end up in landfill
doesn’t ruin habitats
less noise and dust

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16
Q

advantages of recycling

A
  • cheaper because no need to pay for electricity
  • less air pollution eg sulfr dioxide
  • doesn’t ruin teh environment habitats
  • requires less energy than extracting eb electricity is needed to extract aluminium
  • landfill sites don’t get full
  • reduces need to mine ores so don’t run out
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17
Q

transition metals

A

high melting and boiling point
high density - metal cations are densely packed together
conducts heat
conducts heat
malleable
ductile
colourful
can act as catalysts in different reactions

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18
Q

copper

A

blue

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19
Q

nickel

A

green

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20
Q

cobalt

A

pink

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21
Q

iron

A

yellow

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22
Q

harbour process to make ammonia

A

iron catalyst

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23
Q

catalytic converter in cars

A

platinum converter

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24
Q

rust…

A

a metal oxide layer that forms on the outside of the metal
we can prevent rusting by
- excluding oxygen
- excluding water
- sacrificial protection (galvanising)
- electroplating

25
Q

sacrificail protection

A

a method that doesn’t rely on excluding oxygen or water
instead, a piece of zinc or magnesium is attached to the iron or steel
will oxideise more easily so reacts with them instead of the iron/ steel object
this protection continues until the sacrificial method corrodes away

26
Q

electroplating

A

coating a metal with another metal for protective or aesthetic reasons
uses electrolysis to transfer the metal atoms onto the surface of teh other metal

27
Q

why are some objects electroplated

A
  • aesthetics e.g. shiny
  • to prevent corrosion as it wont react with oxygen or water
28
Q

silver ring

A

silver atoms lose electrons and become silver ions
silver ions go into electrolyte and move to negiv=tavely charged copper ring
silver ions gain electrons and left as silver atoms

29
Q

alloy

A

a mixture of one or more metal element, mostly metal
irregular arrangement in layers so less malleable and atoms arent able to easily slide over each other

30
Q

pure metals

A

regular layers of metal ions, layers can easily slide over each other

31
Q

cartas

A

mass of pure gold/ 24 parts of the alloy

32
Q

alloy proteries

A
  • decreases malleability
  • increases hardness
  • increases corrosion resistance
33
Q

wedding ring

A

platinum used which is expensive and unreactive will stay shiny

34
Q

concentration in g dm-3

A

mass of solte / volume of solution

35
Q

concentration in mols

A

concentration g dm-3 / ram

36
Q

titration accuracy

A
  • use an indicator so we see the end point of teh reaction by a colour change
  • glass pipette to maintain an accurate volume
  • read from bottom of miniskus
  • use a white tile to more easily see the colour change
  • add solution drop by drop near the end point to identify exactly when teh colour changes
  • make sure there are no bubbles in teh burrito / pipette
  • consistintky SWIRL teh flask to ensure mixing of alkali and acid
  • wash pipette to avoid contamination
37
Q

chemical and fuel cells

A
  • two different metals can undergo a redox reaction if they are in contact with salt solution of therir own metal
  • greater different in reactivity between teh two metal teh higher the voltage produced
  • the curicit must be completed with a salt bridge which allows ions to flow from one half of the cell to the other chemical cells
38
Q

the daniel cells

A
39
Q

alkaline batteries

A

non rechange

40
Q

what happens when one of the reactants run out batteries

A

modern batteries contain solution mixed with a powder to form a paste
we call the call these dry cells

41
Q

hydrogen fuel vs petrol

A

+ only water product is H2O non-pollution
+ 40-60% efficient
+ requires less maintenance
+ oxygen readily available
+ doesn’t produce CO2
- expensive to make
- slightly flammable so have to be stored carefully
- few rechargeable stations
- hydrogen not easily purchased
- heavy and costly to transport

42
Q

petrol/ disel

A

+ easier to store, many filling stations
- noisy in use, CO2 waste product, many moving parts

43
Q

iron + water + oxygen

A

hydrated iron oxide

44
Q

Explain why iron rod rather than stainless steel rod is used in this experiment.

A

they would take too long to corrode as stainless steel is more resistant to corrosion, doesn’t react with water/ oxygen

45
Q

actual yield

A

yeild made in a reaction

46
Q

theoretical yeild

A

maximum yield calculated using the balanced equation with no losses

47
Q

State two reasons why the actual yield of a reaction is usually less than the
theoretical yield

A
  • side reactions
  • some reactants remained unreacted
48
Q

Adding catalyst

A

rate of attainment increases
yeild attained stays the same

49
Q

Explain what effect a pressure higher than 200 atmospheres would have on the rate of
attainment of equilibrium and on the equilibrium yield of ammonia.

A
  • equilibrium shifts to the right
  • rate of attainment is quicker
  • yeild increases
  • moves to fewer molecules
50
Q

Stage 1 takes in heat energy, it is endothermic.
Explain the effect of increasing the temperature on the yield of the products of stage 1.

A

equilibrium shifts to the right
higher yeild

51
Q

The overall equation for the process is
0.40 g of methane were fully reacted with steam to form carbon dioxide and hydrogen.
Calculate the maximum volume of hydrogen in dm3
, measured at room temperature and
pressure, that could be made in this reaction.
(relative formula mass: CH4 = 16, 1 mol of any gas at room temperature and pressure
occupies 24 dm3
)

A

2.4

52
Q

Explain what is meant by a dynamic equilibrium

A

rate of foward and backward reactions is the same with no overall change (no chnage in volume)

53
Q

increasing concentartion

A

equilibrium reached faster

54
Q

When there are alternative methods of producing a product, the final pathway is
chosen by considering atom economy, cost of energy, yield of product and rates
of reactions.
State another factor that should also be considered.

A

equilibrium position/usefulness of by-products

55
Q

What is the source of the hydrogen used in the Haber process?

A

natural gas

56
Q

Explain why the amount of ammonia remains constant.

A

forward and back reactions take
place / reversible / dynamic (1)
at the same rate / equilibrium (1)

57
Q

The voltage of a cell is 1.5 V.
Give a reason why this voltage of the cell decreases when the cell is left connected in a
circuit.

A

reactants are used up

58
Q

Give one advantage of using a hydrogen-oxygen fuel cell, rather than using a chemical cell,
to power a vehicle.

A

constant voltage as long as reactants provided

59
Q

Explain what is meant by a dynamic equilibrium.Explain what is meant by a dynamic equilibrium.

A

Chemistry (9 decks)

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