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Y11 Chem 2025 > Bonding - Metals and Ionic Compounds > Flashcards

Bonding - Metals and Ionic Compounds Flashcards

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1
Q

Cation

A

A positive ion

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2
Q

Alloy

A

A mixture of elements, at least one of which is a metal.

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3
Q

Malleable (definition and reason for metals being malleable)

A

Can be beaten into sheets. Layers of cations can slide past each other relatively easily, while delocalised electrons can move to maintain their electrostatic attractions with cations.

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4
Q

Ductile (definition and reason for metals being ductile)

A

Can be drawn into wires. Layers of cations can slide past each other relatively easily, while delocalised electrons can move to maintain their electrostatic attractions with cations.

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5
Q

Why do metals have a high melting and boiling point?

A

The strong electrostatic attractions between cations and delocalised electrons require lots of heat energy to break, in order to melt or boil the material.

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6
Q

Why can metals conduct electricity effectively?

A

Delocalised electrons can move through the metal easily, carrying charge and enabling current to flow.

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7
Q

Why do metals conduct heat efficiently?

A

The lattice arrangement of cations enables heat energy (in the form of vibrations) to be transferred efficiently through the metal, while delocalised electrons can also move through the metal and transfer heat energy.

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8
Q

What is metallic bonding?

A

The electrostatic force of attraction between a lattice of metal cations and a sea of delocalised electrons.

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9
Q

Which electrons are delocalised from metal atoms?

A

Only the valence electrons.

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10
Q

Name one metallic property that cannot be explained using the metallic bonding model

A

Magnetism of elements such as iron, cobalt and nickel.

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11
Q

Why are alloys harder than pure metals?

A

The lattice arrangement of cations is disrupted in alloys, so layers of metal cations cannot slide past each other as easily as in pure metals.

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12
Q

Give a general word equation for the reaction between a metal and a non-metal

A

Metal + Non-Metal –> Salt

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13
Q

Give a general word equation for the reaction between a metal and oxygen

A

Metal + Oxygen –> Metal Oxide (can be thought of as MOMO)

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14
Q

Give a general word equation for the reaction between a metal and an acid

A

Metal + Acid –> Salt + Hydrogen (can be thought of as MASH)

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15
Q

Give a general word equation for the reaction between a metal and water

A

Metal + Water –> Metal Hydroxide + Hydrogen

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16
Q

Give a general word equation for the reaction between a metal and steam

A

Metal + Steam –> Metal Oxide + Hydrogen (this is ‘nice to know’, rather than ‘need to know’ - but ensure you do know the reaction of metal with water)

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17
Q

In what situation will a metal be able to displace another metal ion from a compound?

A

Where the metal that is reacting is more reactive than the one in the compound - in either case the more reactive metal will end up in the compound.

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18
Q

What is a circular economy?

A

One where the resources from a product are returned back into the economy which is a closed product cycle

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19
Q

What is a linear economy?

A

When a product is essentially disposed of in landfill (or equivalent) after it has been used

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20
Q

What are the aims of a circular economy?

A

To maximise sustainability of resource use; to reduce environmental impacts of production and consumption while using resources more productively and creating less waste.

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21
Q

What is the main difference between recycling a product compared to reusing or repurposing the same product?

A

Recycling a product requires converting the individual components so that they can be used in new products, whereas reusing and repurposing utilise the essentially unchanged product again.

22
Q

Why can iron be extracted using carbon in a blast furnace, while aluminium requires electrolysis, a more expensive technique?

A

Iron is less reactive than carbon, whereas aluminium is more reactive than carbon.

23
Q

In ionic compounds, what does the formula unit show?

A

The simplest whole number ratio of atoms/ions in the compound

24
Q

What is ionic bonding?

A

The electrostatic force of attraction between cations and anions in a giant ionic lattice.

25
Q

What charge does a silver ion have?

A

1+

26
Q

What charges can an iron ion have?

A

2+ or 3+

27
Q

What charges can a copper ion have?

A

1+ or 2+

28
Q

Describe how an ionic compound is formed in a reaction between potassium and sulfur, including what happens to valence electrons, the name and formula of the compound and the basis for ionic bonding.

A

Two potassium atoms each lose their one valence electron, forming two potassium ions (1+). These electrons are transferred to one sulfur atom, forming a sulfide ion (2-).
The ions in the potassium sulfide compound, K2S, are oppositely charged so they attract each other electrostatically.

29
Q

Describe the meaning of the word giant as used in the description giant ionic lattice

A

The actual number of particles is undefined

30
Q

Describe the meaning of the word lattice as used in the description giant ionic lattice

A

The structure is regular and repeating

31
Q

Why do ionic compounds have high melting and boiling points?

A

The electrostatic attraction between oppositely charged ions is very strong, and requires lots of heat energy to disrupt.

32
Q

Why do ionic compounds conduct electricity as liquids or in solution, but not as solids?

A

In a solid ionic compound, the ions are held in fixed positions within the lattice and are not free to move. This means the solid is not electrically conductive as electric current requires free-moving charged particles. However, when the ionic compound is liquid or dissolved, the ions are free to move through the structure and carry electric charge.

33
Q

Why are ionic compounds hard but brittle?

A

Due to their lattice arrangement, the electrostatic attraction between positive and negative ions is very strong and so the crystals are hard. However, when enough force is applied, layers of ions can become mis-aligned, introducing repulsion. This causes the ionic lattice to split or shatter.

34
Q

What is the formula of the ethanoate ion?

A
35
Q

What is the formula of the nitrate ion?

A
36
Q

What is the formula of the hydroxide ion?

A
37
Q

What is the formula of the permanganate ion?

A
38
Q

What is the formula of the cyanide ion?

A
39
Q

What is the formula of the sulfate ion?

A
40
Q

What is the formula of the carbonate ion?

A
41
Q

What is the formula of the chromate ion?

A
42
Q

What is the formula of the dichromate ion?

A
43
Q

What is the formula of the phosphate ion?

A
44
Q

What is the formula of the ammonium ion?

A
45
Q

What is the name of the ionic compound CuCl?

A

Copper (I) chloride

46
Q

What are the main state symbols and what do they represent?

A

(s) - solid, (l) - liquid, (g) - gas, (aq) - aqueous

47
Q

What is a precipitate?

A

A solid product formed from the reaction of two dissolved substances

48
Q

How can a precipitate be separated from a mixture?

A

Filtration

49
Q

What name is given to ions that do not participate in a reaction?

A

Spectator ions

50
Q

Name five types of ionic compound that are always soluble

A

Sodium salts, Nitrates, Ammonium salts, Potassium salts and Ethanoate salts (think SNAPE)

51
Q

Chlorides, bromides and iodides are usually soluble. Name two positive ions that will cause these ions to precipitate

A

Silver and Lead (although lead chloride is sparingly soluble)

52
Q

Sulfates are usually soluble. Name two positive ions that will cause them to precipitate.

A

Lead and Barium

Y11 Chem 2025 (14 decks)

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