gcse chemistry > metals > Flashcards

metals Flashcards

(65 cards)

Study These Flashcards
1
Q

typical metal properties (8)

A
  1. hard
  2. strong
  3. dense
  4. shiny
  5. ductile
  6. malleable
  7. good conductors (heat + electricity)
  8. sonorous
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

transition metal properties

A
  1. form coloured compounds (eg copper compounds = blue)
  2. good catalysts
  3. can form more than one type of atom
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

‘typical metal’ example

A

iron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

uses of metals

A
  • iron = construction (strong)
  • aluminum = pylon wires (good conductor and low density)
  • copper = electrical wires and hot water pipes (2nd best conductor)
  • gold and silver = jewlery (unreactive)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

metal + oxygen/ steam ->

A

metal oxide (solid)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

metal + water ->

A

metal hydroxide + hydrogen gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

metal +acids ->

A

salt + hyrdogen gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

how do metals from K to Fe react with oxygen? (2)

A
  • burn to from oxide
  • decrease in vigour
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what is the flame colour when burning potassium?

A

lilac

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what is the flame colour when burning sodium?

A

yellow

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what is the flame colour when burning lithium?

A

red

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what is the flame colour when burning calcium?

A

brick red

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what is the flame colour when burning magnesium?

A

bright white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what is tin, lead and copper’s reaction with oxygen?

A

react slowly to form a layer of oxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

how do silver, gold and platinum react with oxygen?

A

unreactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

how do potasium, sodium, lithium and calcium react with water/steam?

A

fast reaction, less vigorous as you go down

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

how does magnesium react with water/steam?

A

slowly with cold water, but fast with steam

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

how do aluminium, zinc and iron react with water/steam?

A
  • don’t react with water
  • react with steam
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

how do tin, lead, copper, silver, gold and platinum react with water/steam?

A

unreactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

how do potasium, sodium, lithium react with acid ?

A

violent, explosive reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

how do calcium - lead react with acid ?

A
  • give off h2 gas
  • decreasing vigour
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

how do silver, gold, platinum react with acid ?

A

ureactive to dilute acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

mnemomic to remember reactivity series of metals

A

Please Stop Literally Calling Me A (Cute) Zebra, I’m Tryna Learn (Higher) Chemistry, Said Gabe Parker

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

(remember the mnemonic)

reactivity series of metals
(most to least reactive)

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
(Carbon)
Zinc
Iron
Tin
Lead
(Hydrogen)
Copper
Silver
Gold
Platinum

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
what do displacement reactions involve?
reacting a metal with a COMPOUND of ANOTHER metal
26
how can you determine the reactivity series?
- displacement reactions - if the metal displaces the metal ion in the compound, it is more reactive - if no reaction happens, it is less reactive
27
what is oxidation?
- gain of oxygen - loss of electrons (o2-)
28
what is reduction?
- loss of oxygen - gain of electrons (o2-)
29
what are oxidizing agents?
- substances that cause something else to be oxidised (ie provide oxygen to other substance) - oxidising agents are reduced in a redox reaction
30
what are reducing agents?
- substances that cause something else to be reduced (ie remove oxygen to other substance) - reducing agents are oxidised in a redox reaction
31
what are redox reactions?
- a reaction during which both oxidation and reduction happen - oxygen is lost by one reactant and taken by another reactant
32
3 observations when an iron nail is placed in copper sulfate solution?
- iron nails gets coated by copper (becomes orange/brown) - copper sulfate solution decolourizes - test tube gets hotter
33
how do electrochemical cells work?
- electrons do useful work as the electrons are passed from the more reactive metal to the less reactive metal (the metal ion in the compound)
34
what does the voltage show in an electrochemical cell?
- difference in reactivity between the 2 metals - larger the voltage, greater the difference in reactivity
35
which metal is the positiveelectrode and why?
- the more reactive metal bc it loses electrons (is oxidised)
36
which metal is the negative electrode and why?
the less reactive metal bc the electrons released by the oxidized metal flow to the less reactive metal (which is reduced), making it negative
37
why does the more reactive metal wear away in the reaction in an electrochemical cell?
- the more reactive metal atoms lose electrons to become metal cations and these move into the solution (are lost) M(s) -> M^n+ (aq) + ne-
38
what is an ore?
metal rich compound
39
how are potassium - aluminium metal ores extracted and why?
- electrolysis (electricity) of molten compound - too reactive to use carbon
40
how are zinc-lead metal ores extracted and why?
reduction by carbon (SMELTING) /carbon monoxide (less reactive than carbon)
41
how are copper-platinum metal ores extracted and why?
- mining - found native (uncombined) as they are very unreactive
42
how does smelting/ reduction by carbon work in extracting ores ?
- carbon is reducing agent - causes metal in the metal compound to lose oxygen and it iself in oxidized
43
what is the name of the ore that contains iron?
haematite (Fe2O3)
44
how is haemitite (iron ore) extracted?
smelting in a blast furnace
45
what ions are metals and which charge?
positive cations eg Mg2+
46
what ions are non-metals and which charge?
negative anion eg O2-
47
what is the positive electrode called?
anode (attracts negative anions)
48
what is the negative electrode called?
cathode (has surplus electrons) (attracts positive cations)
49
how does electrolysis to obtain a metal from an ionic compound work?
- metal compound meted - electric current passed through via 2 electrodes +ve cations attracted to -ve cathode - metal ions reduced (gain electrons) to make metals -ve anions attracted to +ve anode - non-metal ions oxidised (lose electrons) to make non-metals
50
difference between electrochemical cells and electrolysis
electrochemical cells - use chemical reaction to produce voltage vs electrolysis - apply voltage to drive a chemical reaction
51
what is phytomining?
grow a plant (hyperaccumaltors) that will absorb chosen metal from the soil and store it in the leaves, which can be burnt (ash contains chosen metal)
52
pros of phytomining
- low energy cost - less waste than traditional methods - smaller carbon footprint - metals can be extracted from low concentrations of soil
53
cons of phytomining
- time-consuming to grow - lots of plants for not much metal - in areas where mineral ores are plentiful, smelting is cheaper and faster
54
what is bioleaching?
uses bacteria to produce leachate solutions that contain metal compounds
55
pros of bioleaching
- less pollution than conventional bleaching - metals can be extracted from low grade ores - low energy cost
56
cons of bioleaching
- in cold climate, bacteria takes longer to grow -> time-consuming - in areas where mineral ores are plentiful, smelting is cheaper and faster
57
what are alloys?
mixtures of metals to change/enhance their original properties
58
how can alloying a metal make it harder?
- metal ions from other metal disrupt structure - layers can't slide across each other - less maleable and requires more force to break it apart (harder)
59
what is steel?
alloy of iron many types eg mild steel, stainless steel, tugsten steel
60
what is corrosion?
the process by which metals are slowly broken down by reactig with substances in their environment
61
what is rusting?
- corrosion of iron caused by water AND oxygen - presence of ionic compound in water makes it rust faster - rust = hydrated iron oxide = red/brown solid
62
what are the types of methods of rust prevention?
1. barrier (paint, oil/grease, electroplating) 2. sacrificial (adding a more reactive metal to iron) work by provoding barrier between iorn and water, oxygen and ionic compounds (salts)
63
what is galvanising
covering steel with zinc, still works even if zinc is chipped away in some places to prevent rusting
64
how does electroplating work?
object to be plated is made the cathode, desired metal is made electrode and the electrolyte is a solution with ions of the desired plating metal
65
what kind of cell uses displacement?
electrochemical cell
gcse chemistry
flashcards
Decks in class (19)
# Cards
Brainscape helps you reach your goals faster, through stronger study habits.
© 2026 Bold Learning Solutions. Terms and Conditions