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new science > C9 metals > Flashcards

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
Q

reaction of iron in cold dilute acid

A

very slow bubbling

25
Q

reaction of iron in warm dilute acid

A

slow bubbling

26
Q

reaction of copper in dilute acid

A

do not react

27
Q

reaction of silver in dilute acid

A

do not react

28
Q

reaction of gold in dilute acid

A

do not react

29
Q

describe what is meant by a displacement reaction

A

more reactive element replaces less reactive element in a compound

30
Q

conditions required for rusting of iron

A

presence of oxygen and water

31
Q

common barrier methods against rusting

A
  • painting
  • greasing
  • coating with plastic
32
Q

how do the common barrier methods prevent corrosion

A

excludes oxygen and water

33
Q

metal + oxygen –> (also known as)

A

metal oxide (corrosion)

34
Q

equation for rusting

A

iron + water + oxygen –> rust (iron(III) oxide)

35
Q

explain sacrificial protectoin

A
  • more reactive metal placed in contact with less reactive metal
  • more reactive metal loses electrons more easily
  • presence of these electrons prevents oxidation
36
Q
A
37
Q

how does ease in obtaining metals from ore relate to its position in the reactivity series

A

more reactive = harder to obtain

38
Q

how is iron from hematite extracted (simple)

A

reduction of iron(III) oxide in blast furnace

39
Q

describe the extraction of iron from hematite

A
  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
Q

what is the main ore of aluminium and how is it extracted

A
  • bauxite
  • by electrolysis

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