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CSEC CHEMISTRY > C7: Metals > Flashcards

C7: Metals Flashcards

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1
Q

Physical properties of metals

A

A -common to all metals

  • good conductors of electricity
  • good conductors of heat
  • malleable
  • ductile
  • lustrous(shiny)
  • solids at room temperature

B - transition metals

  • high melting and boiling points
  • sonorous
  • high density
  • hard
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2
Q

exceptions to physical properties of metals

A
  • group 1 metals have low denisty and are soft
  • tin and lead are fairly soft.
  • mercury is a liquid at rtp
  • copper is pinkish brown in colour when freshly cut
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3
Q

Chemical Properties of metals

A
  • react with oxygen to form oxides
  • react with water if above hydrogen in the electrochemical series
  • react with dilute acids to form salt and hydrogen gas.
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4
Q

which metals do not react with oxygen?

A

metals low in the elctrochemical series eg gold

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5
Q

metals higher in the electrochemical series react with water to form__________

A

a metal hydroxide + hydrogen

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6
Q

which metals do not react with dilute acids?

A

those that are below hydrogen in the electrochemical series

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7
Q

why is it that calcium and sodium are never used to react with acids in the school lab?

A

the reaction can be very explosive

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8
Q

reactive metals lower in the electrochemical series react with hot water or steam to form__________

A

metal oxide and hydrogen

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9
Q

metal oxide + dilute acid gives:

A

salt + water

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10
Q

metal hydroxide + dilute acid gives (1)________. This type of reaction is called a (2)_____________

A
  1. salt + water
  2. neutralization reaction
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11
Q

metal cabonate + dilute acid gives

A

salt + water + carbon dioxide

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12
Q

heat + group 1 metal nitrate ===>

A

metal nitrite + oxygen

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13
Q

Heat + metal nitrate(except group 1) ——>

A

metal oxide + nitrogen dioxide + oxygen

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14
Q

If the nitrate of an unreactive metal is heated the products are:

A

unreactive metal + nitrogen dioxide + oxygen

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15
Q

a metal nitrate is heated and only oxygen gas is given off. From which goup is the metal?

A

group 1

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16
Q

a metal nitrate is heated and a brown gas is seen + the pure metal remains. Where is the metal in the reactivity series?

A

very low and below hydrogen

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17
Q

metal nitrate + heat ——> metal oxide + NO2 + O2

Where whould the metal be in the reactivity series?

A

above hydrogen and below the group 1 metals

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18
Q

when a compound is broken down by heat

A

thermal decomposition

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19
Q

group 1 carbonate(except lithium) + heat —–>

A

no reaction

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20
Q

carbonate(not group 1) + heat ——>

A

metal oxide + carbon dioxide

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21
Q

which metal carbonates do not decompose on heating? what is the exception?

A

group 1

exception - lithium carbonate

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22
Q

group 1 (except lithium) metal hydroxide + heat ——>

A

no reaction

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23
Q

metal oxide + heat —->

A

no reaction , except a few unreactive metal oxides such as silver oxide.

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24
Q

the nitrates and carbonatesof (1)______________ metals undergo thermal decoomposition more easily than those of (2)______________ metals

A
  1. less reactive
  2. more reactive
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25
Q

relationship between the reducing power of a metal and its position in the electrochemical series

A

the higher in the electrochemical series, the greater reducing power and vice versa.

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26
Q

what is meant by the reducing power of a metal?

A

ability to give away electrons (remember OIL RIG)

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27
Q

Metals that are (1)_____________ in the reactivity series are (2)_______________ reactive and therefore give away electrons (3)__________ to become (4)_____________. A more reactive metal will (5)___________ a less reactive metal form its (6)___________ by (7)_____________ it.

A
  1. higher
  2. more
  3. easily
  4. cations
  5. displace
  6. salt/compound
  7. reducing
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28
Q

In the following pairs say if the metal on the right will displace the one on the left:

  1. Zn(s) + Cu2+(aq) ——>
  2. Mg(s) + Zn2+ ———–>
  3. Ca(s) + Al3+————–>
  4. Ag(s) + Cu2+ ———–>
  5. Pb(s) + Al3+ —————>
A
  1. yes
  2. yes
  3. yes
  4. no
  5. no
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29
Q

How is thermal decomposition of carbonates, nitrates and hydroxides related to the electrochemical or reactivity series?

A

the ease of decomposition increases down the reactivity series. compounds of sodium and potassium are stable or only decompose slightly(nitrates)

30
Q

where is carbon in reactivity series

A

between aluminium and zinc

31
Q

what is the reactivity series of metals based on?

A
  • how vigorous the metals react with dilute acids
  • how easily metal compounds undergo thermal decomposition
  • whether or not a metal will displace another metal from its compounds
32
Q

On going up the reactivity series, the ability to give away electrons (1)____________ , therefore the metal becomes a stronger (2)____________, and forms compounds that are more (3)____________, because their (4) ______________ are more stable.

A
  1. more easily
  2. reducing
  3. stable
  4. ions
33
Q

Method of extraction of metals depends on:

A

Position of the metal in the electrochemical series

34
Q

extraction of metals above carbon in the electrochemical series

A

Electrolysis of their molten ores

35
Q

Extraction of metals below carbon (zinc and below)

A

Reduction by heating with a reducing agent such as carbon

36
Q

reducing agents used in extracting metals

A

Carbon, carbon monoxide, hydrogen

37
Q

which metals require more energy to extract from their ores and why?

A
  • Aluminium and above
  • because they form very stable compounds and as such eletrolysis in needed to extract them and this process requires large amounts of energy
38
Q

Main methods of extraction of metals

A
  • direct physical separation from the earths crust
  • electrolysis
  • reduction
39
Q

suggest a method for the extraction of each metal below

  1. gold
  2. aluminium
  3. iron
  4. silver
A
  1. direct physical separation
  2. electrolysis
  3. reduction
  4. direct physical separation
40
Q

the extraction of metals from their ores is a ________________ process

A

reduction

41
Q

what are the 2 ores of aluminium?

A
  1. impure hydrated aluminium oxide(bauxite)
  2. sodium aluminium fluoride , Na3AlF
42
Q

Label the diagram of the electrolytic cell for the extractio of aluminium

A

W - graphite anode (+)

R - Cathode(-)

V - Molten aluminium oxide(alumina)

P - Molten Aluminium

43
Q

what is alumina?

A

pure anhydrous aluminium oxide

44
Q

why is alumina dissolved in cryolite?

A
  • reduces the melting temperature of alumina and energy required to melt it.
  • the mixture is a better conductor than alumina by itself
45
Q

what are the products of the electrolysis of alumina?

A

cathode: aluminium ions reduced to aluminium
anode: oxide ions oxidized to exygen gas

46
Q

what happens to the aluminium that is formed at the cathode?

A

it collects at the bottom of the electrolytic cell and is tapped off

47
Q

the chemical formula or cryolite?

A

Na3AlF6

48
Q

what is the use of cryolite in the extraction of Al?

A

reduce melting point and increase conuctivity of molten Al2O3

49
Q

overall reaction for the electrolysis of Aluminium Oxide:

A

2Al2O3 =====> 4Al + 3O2

50
Q

what kind of electrodes are use in the extraction of aluminium?

A

graphite

51
Q

what happens at the cathode during the electrolysis of aluminium oxide?

what is the half equation?

A

Aluminium ions reduced to elemental aluminium

half equation: Al3+(l) + 3e ======> Al(l)

52
Q

what happens at the anode during the electrolysis of aluminium oxide?

what is the half equation?

A

Oxide ions oxidised to oxygen gas

half equation: 2O2- (l)====> O2(g) + 4e

53
Q

what are the ores of iron?

A
  • haematite - impure iron(III) oxide - Fe2O3
  • magnetite - impure iron(II, III) oxide - Fe3O4
54
Q

what are the raw materials used in the extraction of iron?

A

iron ore, coke, limestone and air

55
Q

Name of the structure used to exract iron

A

blast furnace

56
Q

General equation for the reduction of iron from its ore

A

Fe2O3(s) + 3CO(g) ====> 2Fe(l) + 3CO2(g)

57
Q

ldentify the different substances in the diagram of the blast furnace

A

M - mixture of metal ore (haematite), coke and limestone

G - gas waste

X - hot air

Y - slag (calcium silicate)

Z - molten iron

58
Q

what reaction takes place in each zone. Show equations for the reactions

A

Zone 1: Hot air reacts with carbon(coke) to form CO2:

C(s) + Os(g) ===> CO2(g)

Zone 2: CO2 reacts with Carbon to form CO:

CO2(g) + C(s) ====> 2CO(g)

Zone 3: CO reduces Iron Odixe to iron:

Fe2O3(s) + 3CO(g) ====> 2Fe(l) + 3CO2(g)

59
Q

Role of limestone in the extraction of iron

A

limestone is added to the blaast furnace to remove the main impurity in the iron ore, Silicon dioxide. The reaction produces liquid calcium silicate(slag) which is tapped off.

60
Q

reaction between limestone and silicon dioxide to form calcium silicate(slag)

A

the reacion comprises two stages:

  1. Thermal decomposition of limestone to form Calium Oxide and CO2:

CaCO3(s) ===> CaO(s) + CO2(g)

  1. Reaction betweeen CaO and Silicon dioxide to form calcium silicate:

CaO(s) + SiO(g) ===> CaSiO3(l)

61
Q

what is slag used for?

A
  • an ingredient in cement production
  • mixed with asphalt to build roads
  • used as aggregate in concrete for construction
62
Q

Uses of aluminium

A
  • overhead electrical cables
  • window frames and doors
  • cans to store drinks
  • cooking utensils
  • aluminium foil
63
Q

uses of lead

A
  • making car batteries
  • soldering
  • joining metal pipes
  • radiation shields eg Xray shield
  • Keel for sailboats
  • lead weights eg fishing and diving weights
64
Q

uses of iron

A
  • pure iron too weak to be useful. instead it is mixed with other metals to form steel alloys
  • making car bodies
  • contruction
  • making aircraft
  • makinf food and drink cans
  • tools
  • surgical instruments
  • indistrial chemical vessels
65
Q

what is an alloy?

A

Mixture of two or more metals or mixture of one or more metals with a non-metal such as carbon.

66
Q

examples of iron alloys and their uses

A
  • stainles steel - surgical iinstruments, cooking utensils, sinks.
  • mild steel - construction of bridges, oil rigs, ships, trains and motor vehicles, tin cans coated with tin.
  • high carbon steel - cutting tools such as chisels, knives, dril bits, masonry nails
  • cast iron - engine parts, railings, gates, manhole covers, hinges and cast iron cookware
67
Q

examples and uses of aluminium alloys

A
  • Duraluminum - aircraft construction, bodies of motor vehicles
  • Magnalium - aircraft and motor vehicle parts
68
Q

why are alloys sometimes stronger and harder than the metals from which they are made?

A

The regular metal lattice is disrupted by the presence of different sized atoms present in an alloy. Therefore the layers cannot slide over each other so easily. this makes the metal alloy stronger and/or harder

69
Q

List some toxic metals and the damage they can cause

A

lead: -

  • damages body tissues and organs
  • harms nervous system especially in childre leading to low IQ
  • interferes with production

Arsenic-

  • Damages the skin
  • causes skin cancer

Mercury - damages nervous system leading to problems with coordination, hearind gloss, impaired vision and speech - Minamata disease

Cadmium -

  • weakens bones leading to oteoporosis
  • damages the kidneys, liver and lungs
70
Q

How do toxic metals harm the evironment?

A
  • improper disposal of waste containing heavy metals is a major source of pollution.
  • Think bioaccumlation. As the toxic metal moves up the food chain its concentration in the rganism increases thereby increasng its toxic effects
  • Heavy metals remain in the environment for a long time
  • Toxic metals can reach underground water and contaminate water sources
  • Toxic metals can be inhaled such as from car exhausts, burning of fossil fuels such as coal.
71
Q

list some useful metals

A

magnesium - important for plants to make chlorophyll in order to carry out photosynthesis

Iron - important for animals to produce haemoglobin in order to carry oxygen needed for respiration

Calcium - imporant for forming healthy bones and teeth of animals

Zinc - important for growth and repair of tissues as well the normal functioning of the immune sytem.

Sodium and potassium - important for the transmission of nerve impulses and for muscles t contract

72
Q

Difference between corrosion and rusting

A

corrosion is the gradual dissolving away of a metal from its surface inwards. rusting is a special form of corrosion where iron(III) oxide is formed from the reaction between iron and oxygen in the presence of water.

CSEC CHEMISTRY (17 decks)

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