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Year 11 Chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

1.1

How has copper been used throughout history?

A

Ornaments, tools, weapons, cooking pots
Bronze (+tin) - makes copper stronger and better for tools
Contemporary uses: related to conductivity, corrosion resistances and ability to form alloys

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2
Q

1.1

How has iron been used throughout history?

A

Weapons

Contemporary: steel alloys - bridges, car, machinery, appliances

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3
Q

1.2

What are the metals in STEEL, what are its properties and what is it used for?

A

Iron, Chromium, Nickel

Resists corrosion, hard - sinks, cutlery, nails, chains

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4
Q

1.2

What are the metals in BRASS, what are its properties and what is it used for?

A

Copper, Zinc

Resists corrosion, ductile, polishes well - door knobs, screws, instruments

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5
Q

1.2

What are the metals in SOLDER, what are its properties and what is it used for?

A

Tin, Lead

Low melting point - joining pipes and wires

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6
Q

1.3

Explain why energy input is necessary to extract metal from its ores

A
  1. to remove impurities in the ore

2. to break ionic bonds between the ore and the metal to obtain pure metal

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7
Q

1.4

Identify why there are more metals available now than 200 years ago

A

Because of the development of new extraction techniques and technology
e.g. even though Aluminium is the most abundant metal, it was not used until early 20th century because it was too difficult to extract from bauxite.

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8
Q

2.1

Describe the reaction of acids and metals

A

metal + acid -> salt + hydrogen (H2)

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9
Q

2.1

Describe the reaction of metals and oxygen (combustion)

A

metal + oxygen -> metal oxide

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10
Q

2.1

Describe the reaction of metals and water

A

metal + water -> hydrogen + metal hydroxide

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11
Q

2.2

Describe the criteria used to place metals in order of activity based on their ease of reaction

A

The more reactive a metal is, the more violent its reactions will be. Therefore, the ease of reaction tells you have active a metal is - the more reactive, the higher the metal is on the scale

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12
Q

2.3

Identify the reaction of metals with acids as requiring the transfer of electrons

A

reactions which involve the transfer of electrons are oxidation and reduction reactions

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13
Q

2.4

Outline examples of the selection of metals for different purposes based on their reactivity

A

Copper: use - water piping. reactivity - no reaction with oxygen or water
Magnesium: use - protect buried fuel tanks for corrosion
Aluminium: use - fireworks. reactivity - very active, release electrons readily to create white light

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14
Q

2.5

Outline the relationship between the relative activities of metals and their position on the periodic table.

A

The most reactive metals are in group one, with metals become more reactive down the group. The least active metals are in transition metals.

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15
Q

2.6

What is first ionisation energy?

A

The minimum energy required to remove and electron from an atom

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16
Q

2.6

Identify the importance of first ionisation energy in determining the relative reactivity of metals

A

As the reactivity increases, the energy needed to rearrange atoms of that element decreases. This means that if a metal has a low first IE, it is reactive.

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17
Q

3.1

Identify an appropriate model that has been used to describe atomic structure

A

Bohr’s model
nucleus is central and contains protons and electrons.
nucleus has positive charge equal to the number of protons
electrons move around the nucleus and are held by electro static forces

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18
Q

3.2

What was Lavoisier’s contribution to the development of the Periodic Table?

A

FIRST:
he recognised 33 “elements” (some of which were compounds) and divided them into metals and non-metals
- he began classification of elements

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19
Q

3.2

What was Döbereiner’s contribution to the development of the Periodic Table?

A

SECOND:
“triads” - several groups of 3 elements with similar properties -
- began the grouping of elements according to physical and chemical properties

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20
Q

3.2

What was Chancourtois’ contribution to the development of the Periodic Table?

A

THIRD:
helix - constructed vertical helix table with elements of similar properties arranged vertically
- suggested periodic recurrence of properties

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21
Q

3.2

What was Newlands’ contribution to the development of the Periodic Table?

A

FOURTH:
arranged all known elements according to atomic mass
- first to clearly recognise periodicity of properties

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22
Q

3.2

What was Mendeleev’s contribution to the development of the Periodic Table?

A

FIFTH:
arranged the elements in order of increased atomic mass
- recognisable that there were elements left to be discovered and left space in the table

23
Q

3.2

What was Meyer and Moseley’s contributions to the development of the Periodic Table?

A

LAST:
recognised that properties related to atomic number, not mass
- organised modern periodic table

24
Q

3.3

Describe trends on the Periodic Table of electrical conductivity

A

Decreases from left to right

Increases down a group

25
Q

3.3

Describe trends on the Periodic Table of first ionisation energy

A

Increases from left to right

Decreases down a group

26
Q

3.3

Describe trends on the Periodic Table of atomic radius

A

Decreases from left to right

Increases down a group

27
Q

3.3

Describe trends on the Periodic Table of melting and boiling points

A

Increases from left to right until group 4, then decreases

28
Q

3.3

Describe trends on the Periodic Table of electronegativity

A

Increases from left to right

Decreases down a group

29
Q

3.3

Describe trends on the Periodic Table of reactivity

A

Metals
Decreases from left to right, increases down a group
Non-metals
Increases from left to right, decreases down a group

30
Q

4.1

What is the mole?

A

the number of atoms in exactly 12g of Carbon-12

31
Q

4.1

What is Avogadro’s number?

A

6.022x^23

32
Q

4.1

What is molar mass?

A

The mass of a mole of a substance

= molecular mass

33
Q

4.1

What is the formula for moles?

A 
moles = mass/molar mass
n = m/M
34
Q

4.2

Compare mass changes in samples of metals when the combine with oxygen

A

When a metal reacts with oxygen, the total mass of the product is more that the original mass of the metal, as oxygen solidifies to become an oxide

35
Q

4.3

What is Gay-Lussac’s Law?

A

Gay-Lussac’s Law:
When measured at a constant temperature and pressure, the volume of gases taking part in a chemical reaction show whole number ratios to each other

36
Q

4.3

How did Gay-Lussac contribute to an understanding of the mole? (3 points)

A
  1. The chemical formula represents one mole of the substance
  2. The formula mass represents one mole of that substance
  3. One mole of any gas, at STP conditions, occupies 22.71L of volume
37
Q

4.4

Recount Avogadro’s law

A

Equal volumes of gases, at the same temperature and pressure, contain equal numbers of molecules

38
Q

4.4

What is the formula for volumes of gases?

A 
moles = volume/molar volume
n = V/VM
39
Q

4.5

What is empirical formula?

A

the formula which tells us the ratio in which atoms are present in a substance

40
Q

4.5

What is molecular formula?

A

the formula which tells us how many of each atom are present in a molecule of a compound

41
Q

5.1

What is a mineral?

A

compound occurring naturally, containing commercial metal of value

42
Q

5.1

What is an ore?

A

a piece of rock containing minerals or metals

43
Q

5.1

What is an economic deposit?

A

a deposit which contains high percentages of valuable ore that is easily extracted

44
Q

5.1

What is a non-economic deposit?

A

a deposit which does not contain minerals which are economically viable to extract and produce

45
Q

5.2
Describe the relationship between commercial prices of common metals, their actual abundances and relative cost of production

A

A high cost of production and low abundance of a metal will result in an increase in the commercial price

46
Q

5.2

What factors influence the cost of production of a metal?

A

Reactivity: less active metals are more likely to be found uncombined
Location: more remote mines are more expensive to extract from
Production: complex refining techniques will cost more

47
Q

5.3

Explain why ores are non-renewable resources

A

They cannot be replaced, as they are formed by geological processes (over millions of years) that cannot be replicated to produce more ores

48
Q

5.4

Describe the separation processes involved in extracting copper from its ores

A

Mining and crushing
Froth flotation
Roasting and smelting
Electrolytic refining

49
Q

5.4

What is mining and crushing and what does it do?

A

It helps separate copper from unwanted rock

50
Q

5.4

What is froth floatation and what does it do?

A

Crushed ore is mixed wiht water and oils, and copper sticks to bubbles which float to the top and are collected.
creates a mixture of 30% copper

51
Q

5.4

What are roasting and smelting and what do they do?

A

High temperatures are applied to the copper, with coal combustion, which reacts and remove impurities.
creates a mixture of 98% pure copper

52
Q

5.4

What is electrolytic refining?

A

Copper from the smelter becomes an anode, and a pure sheet of copper becomes a cathode. In an electrolytic cell copper transfers from the impure anode and forms pure copper on the cathode.

53
Q

5.5

Recount the steps taken to recycle aluminium

A

Collection: through council initiatives and individual action
Sorting: steel is removed through magnetic separation
Preparation: aluminium is compressed for form bales
Remelting and refining: baled Al is fed to furnace at 700º to melt. Molten Al is cast into ingots which can create new products

54
Q

5.6

What is the formula for percentage yield?

A

% yield = amount obtained/amount expected

Year 11 Chemistry (3 decks)

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