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IGCSE Chemistry > C7 Metals > Flashcards

C7 Metals Flashcards

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1
Q

what is METALLIC BONDING?

A

lattice of cations

in a sea of delocalized electrons

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2
Q

properties of METALS?

A

good conductor of heat and electricity
high m/b point
malleable and ductile

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3
Q

why do metals conduct heat and electricity?

A

delocalized electrons

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4
Q

why do metals have high m/b points?

A

strong force of attraction between metal ions and delocalized electrons
→ more energy needed to break the bonds

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5
Q

why are metals malleable and ductile?

A

LAYERS OF ION in lattice structure SLIDE PAST one another due to delocalized electrons

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6
Q

properties of TRANSITION METALS?

A

high density
high melting point
form colored compounds

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7
Q

why do transition metals have high melting points?

A

each atom is bonded to electrons
each ion is bonded to other ions
→ more energy to break the bonds

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8
Q

what are transition metals often used as?

A

catalysts

e.g. Fe in haber process to make NH3

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9
Q

what are ALLOYS?

A

mixtures of metals

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10
Q

why do alloys have different properties from the metals they contain?
what are the different properties?

A
  • difference atoms distort regular lattice structure
  • harder for layers to slide past one another
    → stronger, less flexible
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11
Q

properties and uses of ALUMINUM?

A

resistant to corrosion + strong + light → aircraft

conduct heat + non-toxic → saucepan

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12
Q

properties and uses of ZINC?

A

cheap, reactive → coating iron (galvinizing)

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13
Q

properties and uses of COPPER?

A

conduct electricity → electrical wires

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14
Q

properties and uses of BRONZE?

A

doesn’t corrode → medals

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15
Q

properties and uses of BRASS?

A

doesn’t corrode → music instruments

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16
Q

composition, properties and uses of STEEL?

A

Fe+C

very hard → cutting tool

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17
Q

properties and uses of MILD STEEL

A

easily shaped → car body

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18
Q

properties and uses of DURIRON?

A

not affected by acid → pipes in chemical factories

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19
Q

properties and uses of STAINLESS STEEL?

A

doesn’t rust → car parts, cutlery

20
Q

what is REDOX reaction?

A

loss/gain of electrons (oxidation, reduction)

21
Q

an element is oxidized when it

… electrons?

A

loses electrons

OIL - Oxidation Is Loss of electrons

22
Q

an element is reduced when it

… electrons?

A

gains electrons

RIG - Reduction Is Gain of electrons

23
Q

what can more reactive metals do to less reactive metals?

A

DISPLACE them from their salt solution

24
Q

write the
1. SYMBOL EQUATION
2. HALF EQUATION
for copper reacting w/ silver nitrate

A

Cu (s) + 2AgNO3 (aq) → Cu(NO3)2 (aq) + 2Ag (s)

Cu(s) → Cu2+ (aq) + 2eˉ

Ag+ (aq)+ 1eˉ →Ag(s)

25
Q

in REDOX rxn, more reactive metals are …?

A

oxidized // reducing agent

26
Q

in REDOX rxn, less reactive metals are …?

A

reduced // oxidizig agent

27
Q

the reactivity series?

A 
Potassium
Sodium
Calcium
Magnesium
Aluminum
(Carbon)
Zinc
Iron
Tin
Lead
(Hydrogen)
Copper
Silver
Gold
28
Q

metals more reactive than what element can react with cold water+steam+acid?

A

calcium

29
Q

metals more reactive than what element can react with steam+acid but not cold water?

A

hydrogen

30
Q

how are the most reactive metals extracted? what is the disadvantage of it?

A

electrolysis

expensive and takes up lots of energy

31
Q

how are metals less reactive than carbon extracted?

A

heat their oxides with carbon → REDUCED by carbon

32
Q

how are the least reactive metals extracted?

A

they are found as pure elements

33
Q

mixtures from which metals can be extracted are called?

A

ores

34
Q

why do ores need to be recycled?

what are good+bad sides of recycling?

A

they are finite resources

  • less landfill
  • expensive
35
Q

how is iron extracted?

A

blast furnace

36
Q

describe the process of IRON EXTRACTION in BLAST FURNACE

equations

A

iron extraction:

  1. C + O2 → CO2
  2. C + CO2 → CO
  3. CO + Fe2O3 → Fe (l) + CO2

slag removal:

  1. CaCO3 → CaO + CO2
  2. CaO + SiO2 → CaSiO3 (l)
37
Q

what are the materials needed for iron extraction in blast furnace?

A

iron ore - Fe2O3
limestone - CaCO3
coke - C

38
Q

BLAST FURNACE:

what happens to the SLAG?

A

REMOVED → make CEMENT

39
Q

BLAST FURNACE:

what happens to the MOLTEN IRON?

A

SINK to bottom (dense) → tapped off → turned into steel

40
Q

what is zinc’s ore called?

A

zinc blende (ZnS)

41
Q

what is iron’s ore called?

A

hematite (Fe2O3)

42
Q

what are the conditions for rusting?

A

water

oxygen

43
Q

what happens to the rate of rusting if there’s impurity in water?

A

faster

44
Q

why does iron need to be protected from rusting?

A

rust weakens its structure and strengths

45
Q

what is physical protection of rust? what are the drawbacks?

A

keeping air and oxygen away from surface:

  • cover with oil, plastic, paint (easy to rub/peel off)
  • cover with less reactive metal (loses protection and rusts faster once coating is scratched)
46
Q

what is sacrificial/galvanizing protection of rust? give an example

A

cover with more reactive metal → reactive metal reacts with oxygen first → leaves iron unreacted
e.g. zinc

47
Q

why does aluminum not corrode?

A

aluminum oxide layer → prevents metal from contact with oxygen/air

IGCSE Chemistry (9 decks)

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