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Prelim Chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

Why did the use of metals increase 7000 years ago?

A

Humans began to extract metals from compounds.

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2
Q

Why does metal extraction require energy?

A

It breaks chemical bonds.

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3
Q

What order did the bronze, iron and copper ages come in, and how were they extracted?

A

Copper Age - Heating copper oxide with carbon
Bronze Age - Heating copper and tin, first alloy
Iron Age - Heating iron ore with bellows

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4
Q

List 5 metals and their uses in relation to their physical and chemical properties.

A

Iron is strong, and used in construction and vehicles
Aluminium is malleable and light, and used in aeroplane parts
Copper is highly conductive and ductile, and is used in wiring
Zinc is reactive and forms alloys, and is used in battery casings
Lead is reactive and forms alloys, and is used in electrodes

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5
Q

List five inventions that have lead to a huge increase the amount of metals available today since 200 years ago.

A

Batteries, circuits, electrolysis, nuclear power and particle accelerators.

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6
Q

What is an alloy?

A

A homogenous mixture of one or more elements.

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7
Q

What metals is steel made from, what are its properties, and what is it used in?

A

Iron and Carbon
Strength
Construction and Vehicles

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8
Q

What metals is brass made from, what are its properties, and what is it used in?

A

Copper and Zinc
Unreactive, Ductile, Lustre
Musical Instruments, Door Knobs

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9
Q

What metals is solder made from, what are its properties, and what is it used in?

A

Lead and Tin
Low Melting Point, Strong
Welding

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10
Q

What metals is bronze made from, what are its properties, and what is it used in?

A

Copper and Tin
Unreactive, Malleable, Strong
Tools and Ornaments

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11
Q

What metals is sterling silver made from, what are its properties, and what is it used in?

A

Silver and Copper
Malleable, Unreactive,
Lustrous, Harder than Silver
Jewellery

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12
Q

Acid + Metal = ?

A

Hydrogen + Salt

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13
Q

Water + Metal = ?

A

Hydrogen + Hydroxide

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14
Q

Steam + Metal = ?

A

Hydrogen + Oxide

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15
Q

Oxygen + Metal = ?

A

Metal Oxide

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16
Q

What is the order of reactivity of metals by group?

A 
Group 1
Group 2
Group 3
Some Transition Metals
Group 4
Remaining Transition Metals
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17
Q

Describe trends in reactivity on the periodic table.

A

The reactivity of a metal increases down and to the left of the periodic table.

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18
Q

What does a more reactive metal do to another metal compound in solution?

A

It displaces it.

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19
Q

What do redox reactions involve?

A

The transfer of electrons.

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20
Q

Reactions between metals and acids, water, steam or oxygen are all an example of what type of reaction?

A

Redox reactions.

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21
Q

Does oxidation involve losing or gaining electrons?

A

Losing electrons.

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22
Q

Does reduction involve losing or gaining electrons?

A

Gaining electrons.

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23
Q

Is the following an oxidation or reduction net ionic half equation?

2H(+) + 2e —–> H2

A

Reduction

The Result on the Right is R-Lone

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24
Q

Is the following an oxidation or reduction net ionic half equation?

2Zn —–> Zn(2+) + 2e

A

Oxidation

The Result on the Right is not R-Lone

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25
Q

What is ionisation energy?

A

The amount of energy required to remove the loosest electron from an atom.

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26
Q

What is the relationships between the reactivity and ionisation energy of a metal?

A

The higher the reactivity, the lower the ionisation energy.

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27
Q

Explain the trends in ionisation energy on the periodic table.

A

It increases to the right because electrons are pulled closer to the nucleus by more protons.
It decreases down the periodic table as the electrons are on rings further out from the nucleus, decreasing its pull on them.

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27
Q

Describe Rutherford’s model of the atom.

A

Rutherford’s model featured a tiny, positively charged nucleus orbited by negatively charged electrons.

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28
Q

What did Antoine Lavoisier contribute to the periodic table?

A

He classified 33 elements into metals and non-metals in 1789.

29
Q

What did Johann Dobereiner contribute to the periodic table?

A

He classified elements with similar properties into triads in 1829.

30
Q

What did De Chancourtrois contribute to the periodic table?

A

He listed the elements by wrapping them around a screw so that elements with similar properties were in the same column in 1862.

31
Q

What did John Newlands contribute to the periodic table?

A

He invented the theory of octaves, that states every eighth element has similar properties in 1864.

32
Q

What did Lothar Meyer contribute to the periodic table?

A

He arranged elements into groups based on valency in 1869.

33
Q

What did Dimitri Mendeleev contribute to the periodic table?

A

He arranged the elements horizontally by mass and vertically by properties in 1869.

34
Q

What did Ramsay contribute to the periodic table?

A

He discovered five noble gases by 1898.

35
Q

What did Henry Moseley contribute to the periodic table?

A

He suggested the atomic number in 1913.

36
Q

List 8 scientists that have contributed to the periodic table, in the order they did.

A 
Antoine Lavoisier
Johann Dobereiner
De Chancourtrois
John Newlands
Lothar Meyer
Dimitri Mendeleev
Ramsay
Henry Moseley
37
Q

Describe the trend in conductivity on the periodic table.

A

Increases down and to the left.

38
Q

Explain the trend in ionisation energy on the periodic table.

A

Increases up because electrons are closer and more attracted to the nucleus.
Increases to the right because the electrons are pulled closer to the extra protons in the nucleus.

39
Q

Explain the trend in atomic radius on the periodic table.

A

Increases down because the electrons are on wider shells.

Increases to the left because the electrons are less attracted to the nucleus.

40
Q

Describe the trend in melting and boiling point on the periodic table.

A

Increases up and to the outside.

41
Q

Explain the trends in electronegativity on the periodic table.

A

Increases up because the electrons are being attracted more by the nucleus because they are in closer shells.
Increases to the right because the nucleus has more protons and hence a stronger pull on electrons.

42
Q

Describe the trends in reactivity on the periodic table.

A

Increases down and to the left in metals.

Increases up and to the right in non-metals.

43
Q

Define a mole.

A

The number of atoms in 12g of carbon 12.

44
Q

What is Avogadro’s number?

A

6.02 x 10^23

45
Q

How many atoms are in one mole?

A

6.02 x 10^23

46
Q

How do you find the mass of one mole of a molecule?

A

Find the sum of the atomic weights of its atoms.

47
Q

What does it mean if an equation has ‘excess’ of a reactant?

A

That reactant is infinite.

48
Q

What is the name of molecules on either side of a chemical equation.

A

Reactants —–> Products

49
Q

What is the weight of one mole of oxygen molecules?

A

32g

Remember to check whether molecules or atoms.

50
Q

What is the weight of one mole of oxygen atoms?

A

16g

Remember to check whether molecules or atoms.

51
Q

Describe the contributions of Gay-Lussac in relation to the mole.

A

He discovered when gases react, their volumes have simple whole number ratios.

52
Q

State Avogadro’s Law, and its implications in relation to the mole.

A

Equal volumes of gases contain the same number of molecules when at a constant temperature and pressure.

This means one mole of any gas has the same volume as one mole of any other gas at the same temperature and pressure.

53
Q

What is the molecular formula of a molecule?

A

The actual number of atoms within the molecule.

54
Q

What is the empirical formula of a molecule?

A

The ratio of atoms in a molecule.

55
Q

What determines whether an ore deposit is economic?

A

Whether it can be mined to produce a net profit.

56
Q

What is the definition of a rock?

A

A naturally occurring mixture of minerals.

57
Q

What is the definition of a mineral?

A

A naturally occurring compound.

58
Q

What is the definition of an ore?

A

A mineral deposit that is economic to extract from.

59
Q

What is a yield?

A

The amount of metal expected to be extracted from an ore.

60
Q

What is the definition of an ore body?

A

A collection of ore worth extracting.

61
Q

Are ores renewable resources?

A

No, they were formed as part of the original Earth and are no longer being formed.

62
Q

What four factors influence the cost of metals?

A

Abundance
Demand
Production Cost
Transportation Cost

63
Q

Describe the process of copper extraction.

A

A ball mill crushes the ore.
Froth flotation concentrates ore.
Silicon Dioxide added to remove Iron and form Copper Oxide.
Air is injected to remove the Sulphur.
Blister Copper placed as an anode in electrolysis.
Pure Copper deposits on cathode, impurities are insoluble.

64
Q

What two copper ores are concentrated during froth flotation?

A

Cu2S and CuFeS2

65
Q

Write a chemical equation for when Silicon Dioxide is smelted with CuFeS2.

A

2 CuFeS2(l) + 5 O2(g) + 2 SiO2(s) —-> 2 Cu(l) + 4 SO2(g) + 2 FeSiO3(l)

66
Q

Write a chemical equation for when Cu2S is smelted.

A

2 CuS(l) + 3 O2(g) —–> 2 Cu2O(l) + 2 SO2(g)

67
Q

Write a chemical equation for when air is injected into the smelting of Cu2O and Cu2S.

A

2 Cu2O(l) + Cu2S(l) —–> 6 Cu(l) + SO2(g)

68
Q

Write a chemical equation for when blister copper goes through electrolysis.

A

Cu(s) —–> Cu(2+)(aq) + 2 e(-)

69
Q

Compare how much energy is required to extract aluminium from its ore to how much energy is required to recycle aluminium.

A

200kJ required to extract 1kg

7kJ required to recycle 1kg

70
Q

Justify the recycling of aluminium.

A

It takes far less energy to recycle aluminium than to extract it from its ore, making it cheaper and better for the environment.
Also, aluminium ore is non-renewable, and will eventually run out.

Prelim Chemistry (3 decks)

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