3.5 - Metals Flashcards

1
Q

how metal can be extracted from its ore

A

using a blast furnace
reacting with more reactive material
electrolysis

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2
Q

reactivity series positions

A
  • tendency to become oxidised is linked to how reactive a metal is
  • metals higher up are less resistant to oxidation than
  • metals placed lower down which are more resistant to oxidation, reacts with water
  • position of the metal on the reactivity series determines the method of extraction
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3
Q

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium

PSL CMA

A
  • extracted by ELECTROLYSIS of the molten chloride or oxide
  • large amounts of ELECTRICITY are required, which makes this an EXPENSIVE process
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4
Q

Zinc
Iron
Copper

ZIC

A
  • extracted by heating with a reducing agent such as carbon or carbon monoxide in a BLAST FURNACE
  • cheap process as carbon is CHEAP and can also be a source of heat
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5
Q

Silver
Gold

A
  • found as PURE elements
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6
Q

reactivity series from most to least reactive

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Copper
Silver
Gold

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7
Q

uses of aluminium and its properties

A

aircraft bodies - high strength-to-weight ratio (low density)

saucepans - very good conductor of heat and unreactive

overhead electrical cables - very good conductor of electricity

food cans - non-toxic, resistant to corrosion and resistant to acidic food stuffs

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8
Q

uses of copper

A

electrical wiring - very good conductor of electricity and ductile

saucepans - very good conductor of heat, unreactive, malleable

water pipes - unreactive (does not react with water), non-toxic and malleable

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9
Q

uses of iron

A

building material - good strength, malleable and ductile, relatively inexpensive

catalyst - increases the rate of reaction without being used up

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10
Q

steels alloys its uses: mild

A

alloyed with - 0.25% carbon

  • car body panels and wiring
  • soft and malleable
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11
Q

steels alloys and its uses: high carbon

A

alloyed with - 0.5-1.4% carbon

  • tools, e.g. chisels
  • hard
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12
Q

steels alloys and its uses: stainless steel

A

alloyed with - 20% chromium and 10% nickel

  • cutlery, sinks and chemical plants
  • strong and resistant to corrosion
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13
Q

alloy and example

A

a mixture of two or more metals or metal with a non-metal such as carbon
e.g. steel is made from iron and carbon

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14
Q

alloy properties

A
  • stronger and harder
  • resistant to corrosion or extreme temperatures
  • makes it more useful than pure metals
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15
Q

why is an alloy harder than a pure metal

A
  • pure metal has layers so the atoms can slide over more easily
  • alloy has different sized atoms which are randomly arranged which prevents layers sliding over
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16
Q

brass is a common example of an alloy which contains

A

70% copper and 30% zinc

17
Q

metallic lattice by a 2-D diagram

A
  • outer electrons become ‘delocalised’ which means they are free to move throughout the whole structure
  • metals have a giant regular arrangement of layers of positive ions surrounded by a sea of delocalised electrons
18
Q

metal + acid ⟶

A

salt + hydrogen
__(s) + H2SO4 (aq) → __SO4 (aq) + H2 (g)

19
Q

rusting equation

A

iron + water + oxygen ⟶ hydrated iron(III)oxide

20
Q

what must be present for rusting to occur

A

Oxygen and water

21
Q

oxidation is any reaction which

A

a substance gains oxygen
- lose electrons

22
Q

reduction is any reaction which

A

a substance loses oxygen
- gain electrons

23
Q

oxidising agent

A

what supplies the oxygen

24
Q

reducing agent

A

removes the oxygen

25
Q

investigate the reactions between dilute hydrochloric and sulfuric acids with the metals magnesium, iron and zinc

A
  • add 5 cm3 of dilute hydrochloric acid to each of three test tubes
  • add 1 cm length of magnesium ribbon to the first tube, observe and note down what you see
  • use a lighted splint to test for any gases given off
  • to the second test tube add a few pieces of iron filings and to the third some zinc turnings
  • observe what happens, test for any gases and note down your observations
  • repeat the experiment with dilute sulfuric acid
26
Q

magnesium reacting with dilute hydrochloric acid dilute sulfuric acid

A

hydrochloric acid - dissolves quickly, gets hot, gas given off which goes pop with a lighted splint, colourless solution left

sulfuric acid - bubbling, splint goes pop, metal dissolves

27
Q

magnesium reacting with dilute hydrochloric acid dilute sulfuric acid

A

hydrochloric acid - very slow bubbling sulfuric acid - slow reaction, small bubbles seen

28
Q

magnesium reacting with dilute hydrochloric acid dilute sulfuric acid

A

hydrochloric acid - bubbles given off, metal slowly dissolves
sulfuric acid - metal dissolves forming colourless solution, gas given off slowly

29
Q

metal​ ​+​ ​oxygen​ ​→​ ​

A

metal​ ​oxide

30
Q

rusting​ ​can​ ​be​ ​prevented​ ​by​ ​excluding​ ​oxygen​ ​and​ ​water​ ​e.g.​ by:

A

o painting
o coating​ ​with​ ​plastic
o using​ ​oil​ ​or​ ​grease

31
Q

reaction between different metals and acids (hydrochloric acid and sulphuric acid)

A

you​ ​can​ ​observe​ ​the​ ​reaction​ ​of​ ​different​ ​metals​ ​with​ ​acids,​ ​as​ ​the​ ​most​ ​reactive
will​ ​give​ ​off​ ​large​ ​amounts​ ​of​ ​H​2​​ ​gas​ ​bubbles​ ​and​ ​the​ ​least​ ​reactive​ ​will​ ​not​ ​give off​ ​any​ ​at​ ​all

● metal​ ​+​ ​acid​ ​→​ ​hydrogen​ ​+​ ​salt