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C9 metals Flashcards

1
Q

general physical properties of metals

A
  • electrical conductor
  • thermal conductor
  • high melting/boiling point
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2
Q

observations of reaction of metal with dilute acids

A
  • metal gradually disappears (soluble salt formed)
  • effervescence
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3
Q

metal + acid –>

A

salt + hydrogen

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4
Q

metal + water –>

A

metal hydroxide + hydrogen

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5
Q

describe reaction between metal and cold water

A
  • slow to begin
  • exothermic, so reaction speeds
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6
Q

metal + steam –>

A

metal oxide + hydrogen

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7
Q

use of aluminium and why

A
  • aircraft: low density
  • overhead electrical cables: low density, good electrical conductivity
  • food containers: resistance to corrosion
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8
Q

use of copper and why

A
  • electrical wiring: good electrical conductivity
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8
Q

define alloy

A

mixtures of a metal with other elements

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9
Q

what is brass composed of

A

mixture of copper and zinc

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10
Q

what is stainless steel composed of

A

mixture of iron and other elements, eg
- chromium
- nickel
- carbon

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11
Q

why are alloys more useful than pure metals

A

can be harder and stronger than pure metals

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12
Q

use of stainless steel and why

A
  • cutlery
  • hardness and resistance to corrosion
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13
Q

why are alloys stronger and harder than pure metals

A
  • diff sized atoms
  • mean layers can no longer slide over each other
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14
Q

order of reactivity series

A

Please Stop Calling Me A Cunty Zebra, I Have Called SalGado

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

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15
Q

reaction of K, Na, Ca with cold water

A
  • react vigorously
  • strongly alkaline solutions formed
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16
Q

reaction of potassium with cold water (equation and observations)

A

2K + 2H2O –> 2KOH + H2
- floats on surface of water
- effervescence pushes metal around on surface
- strongly exothermic
- hydrogen ignites with lilac flame
- potassium quickly disappears, eventually explodes with pop

17
Q

reaction of sodium with cold water (equations and observations)

A

2Na + 2H2O –> 2NaOH + H2
- moves around on surface of water
- very exothermic, metal melts to form silvery ball, steadily disappears as reaction continues
- if sodium trapped, hydrogen may ignite with yellow flamerea

18
Q

reaction of calcium with cold water (equation and observations)

A

Ca + 2H2O –> Ca(OH)2 + H2
- metal sinks
- reaction slow to begin with, speeds as reaction is exothermic
- eventually cause rapid bubbling
- white suspension of calcium hydroxide forms

19
Q

reaction of magnesium with steam (equation and observation)

A

Mg + H2O –> MgO + H2
- reacts vigorously
- gives off very bright white flame
- powdery white MgO forms

20
Q

reaction of magnesium cold dilute acid

A

rapid bubbling

21
Q

reaction of magnesium in warm dilute acid

A

often not done as it may be unsafe

22
Q

reaction of zinc in cold dilute acid

A

slow bubbling

23
Q

reaction of zinc in warm dilute acid

A

rapid bubbling

24
reaction of iron in cold dilute acid
very slow bubbling
25
reaction of iron in warm dilute acid
slow bubbling
26
reaction of copper in dilute acid
do not react
27
reaction of silver in dilute acid
do not react
28
reaction of gold in dilute acid
do not react
29
describe what is meant by a displacement reaction
more reactive element replaces less reactive element in a compound
30
conditions required for rusting of iron
presence of oxygen and water
31
common barrier methods against rusting
- painting - greasing - coating with plastic
32
how do the common barrier methods prevent corrosion
excludes oxygen and water
33
metal + oxygen --> (also known as)
metal oxide (corrosion)
34
equation for rusting
iron + water + oxygen --> rust (iron(III) oxide)
35
explain sacrificial protectoin
- more reactive metal placed in contact with less reactive metal - more reactive metal loses electrons more easily - presence of these electrons prevents oxidation
36
37
how does ease in obtaining metals from ore relate to its position in the reactivity series
more reactive = harder to obtain
38
how is iron from hematite extracted (simple)
reduction of iron(III) oxide in blast furnace
39
describe the extraction of iron from hematite
1. burn carbon (coke) to provide heat and produce CO2 (C + O2 --> CO2) 2. reduce CO2 to CO (C + CO2 --> 2CO) 3. reduce iron(III) oxide by CO (Fe2O3 + 3CO --> @Fe + 3CO2) 4. thermal decomposition of calcium carbonate/limestone to produce calcium oxide (CaCO3 --> CaO + CO2 5. formation of slag (CaO + SiO2 --> CaSiO3)
40
what is the main ore of aluminium and how is it extracted
- bauxite - by electrolysis

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