C7 Metals Flashcards

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
in REDOX rxn, more reactive metals are ...?
oxidized // reducing agent
26
in REDOX rxn, less reactive metals are ...?
reduced // oxidizig agent
27
the reactivity series?
``` Potassium Sodium Calcium Magnesium Aluminum (Carbon) Zinc Iron Tin Lead (Hydrogen) Copper Silver Gold ```
28
metals more reactive than what element can react with cold water+steam+acid?
calcium
29
metals more reactive than what element can react with steam+acid but not cold water?
hydrogen
30
how are the most reactive metals extracted? what is the disadvantage of it?
electrolysis | expensive and takes up lots of energy
31
how are metals less reactive than carbon extracted?
heat their oxides with carbon → REDUCED by carbon
32
how are the least reactive metals extracted?
they are found as pure elements
33
mixtures from which metals can be extracted are called?
ores
34
why do ores need to be recycled? | what are good+bad sides of recycling?
they are finite resources - less landfill - expensive
35
how is iron extracted?
blast furnace
36
describe the process of IRON EXTRACTION in BLAST FURNACE | equations
iron extraction: 1. C + O2 → CO2 2. C + CO2 → CO 3. CO + Fe2O3 → Fe (l) + CO2 slag removal: 4. CaCO3 → CaO + CO2 5. CaO + SiO2 → CaSiO3 (l)
37
what are the materials needed for iron extraction in blast furnace?
iron ore - Fe2O3 limestone - CaCO3 coke - C
38
BLAST FURNACE: | what happens to the SLAG?
REMOVED → make CEMENT
39
BLAST FURNACE: | what happens to the MOLTEN IRON?
SINK to bottom (dense) → tapped off → turned into steel
40
what is zinc's ore called?
zinc blende (ZnS)
41
what is iron's ore called?
hematite (Fe2O3)
42
what are the conditions for rusting?
water | oxygen
43
what happens to the rate of rusting if there's impurity in water?
faster
44
why does iron need to be protected from rusting?
rust weakens its structure and strengths
45
what is physical protection of rust? what are the drawbacks?
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
what is sacrificial/galvanizing protection of rust? give an example
cover with more reactive metal → reactive metal reacts with oxygen first → leaves iron unreacted e.g. zinc
47
why does aluminum not corrode?
aluminum oxide layer → prevents metal from contact with oxygen/air