Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > 3.5 - Metals > Flashcards

3.5 - Metals Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What does the structure of a metal look like?

A
  1. A lattice of positive metal ions.
  2. Delocalized electrons.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is metallic bonding?

A

Metallic bonding is the very strong electrostatic attraction between the positive metal ions and the negative
delocalized electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Why do metals have high melting points?

A

This is because the metallic bonding is very strong so lots of energy is needed to break it.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Why can metals conduct electricity?

A

Delocalized electrons are free to move through the lattice.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Why are metals malleable?

A

The layers of metal ions can slide over each other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What happens when metal carbonates thermally decompose?

A

Metal carbonate → Metal oxide + Carbon dioxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Give an example of and metal carbonate decomposition?

A

Copper carbonate → Copper oxide + Carbon dioxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Observations in the thermal decomposition of copper carbonate?

A

The green copper carbonate turns black.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What happens when a metal reacts with water?

A

Metal + Water → Metal hydroxide + Hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What observations can be seen when Li, Na and K react with water?

A
  • Solid floats - it is less dense than water.
  • Effervescence - hydrogen gas is produced.
  • Solid moves - the effervescence propels it around the surface of the water.
  • Solid disappears - it is used up in the reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What happens to the reactivity of group one metals as you go down the group?

A

The group 1 metals get more reactive as you go down the group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Why do metals get more reactive?

A
  1. The atoms get bigger and have more shells
  2. The outer-electron is further from the nucleus
  3. The attraction between the nucleus and the outer-electron is weaker
  4. So less energy is needed to break the attraction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What happens when metal reacts with steam?

A

Metal + Steam → Metal oxide + Hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why do metals react with cold water and hot steam to produce different products?

A

Steam has more energy, so both bonds in the water molecule can break.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What happens when metal reacts with acid?

A

Acid + Metal → Salt + Hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Why is a salt compound formed when and acid reacts with a metal?

A

A salt is a compound formed when H is displaced from an acid.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Is sodium soluble in water?

A

yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Is potassium soluble in water?

A

yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Is ammonium soluble in water?

A

yes

20
Q

Is nitrate soluble in water?

A

yes

21
Q

Is chloride soluble in water?

A

yes - except with silver (Ag) and lead (Pb)

22
Q

Is sulphate soluble in water?

A

yes - except with calcium (Ca), barium (Ba) and lead (Pb)

23
Q

Are carbonates soluble in water?

A

no - except with sodium (Na), potassium (K) and ammonium (NH4)

24
Q

Are hydroxides soluble in water?

A

no - except with sodium (Na), potassium (K) and calcium (Ca)

25
Q

Are oxides soluble in water?

A

no - except with sodium (Na), potassium (K) and ammonium (NH4)

26
Q

What are the two key observations in a acid + metal reaction?

A
  • The metal disappears:
  • There is fizzing:
27
Q

Order of the reactivity series from most to least reactive?

A

K - potassium
Na - sodium
Li - lithium
Ca - calcium
Mg - magnesium
Al - aluminium
C - carbon
Zn - zinc
Fe - iron
Pb - lead
H - hydrogen
Cu - copper
Ag - silver
Au - gold

28
Q

What is a metal displacement reaction?

A

When more reactive metals displace less reactive metals from their compounds.

29
Q

What observations are usually seen in a metal displacement reaction?

A
  • Solid colour change
  • Solution colour change
30
Q

Key metal displacement reaction and the colour changes?

A

Magnesium + Copper sulphate → Copper + Magnesium sulphate

  1. Solid - turns from grey to pink-orange.
  2. Solution - turns from blue to colourless.
31
Q

What are ores?

A

The rocks containing specific metal compounds.

32
Q

What methods can be used to extract metals from ores?

A
  1. Using Electricity:
    Metals more reactive than carbon cannot be displaced by carbon.
    Instead, we have to use electricity to break down their ore compounds.
  2. Carbon Extraction
    Metals less reactive than carbon can be displaced by carbon.
33
Q

What is rusting?

A

Rusting is a chemical process by which iron is oxidized to form rust.

34
Q

How does rusting happen?

A
  1. Iron is oxidized by oxygen to form iron(III) oxide
  2. Iron(III) oxide is hydrated by water
35
Q

How can rusting be prevented?

A
  1. Using barriers
  2. Sacrificial protection
  3. Galvanising
36
Q

What is using barriers?

A

Coating the iron in paint, oil, grease or plastic prevents the iron from coming into contact with oxygen or water.

This only works as long as the coating is intact - as soon as it breaks, rusting happens

37
Q

What is sacrificial protection?

A

Attach a block of a more reactive metal to the iron. This works by displacing the iron from rust as soon as the rust form.

The down-side to this method is that the block of metal has to be replaced often

38
Q

What is galvinising?

A

This method specifically involves coating the iron in zinc.

It works both ways:
* Coating prevents O2 and H2O from coming in contact with the iron, but even if a crack appears zinc is more reactive than iron so acts as sacrificial protection as well.

39
Q

What is an alloy?

A

Alloys are mixtures of a metal with one or more other elements, usually other metals or carbon

40
Q

Why are alloys harder than pure metals?

A

Alloys are harder than pure metals because the different-sized atoms/ions prevent the layers of metal ions from sliding over each other.

41
Q

What is the use of iron?

A

Making steel because steel is more useful than iron

42
Q

What is the use of low-carbon steel?

A

Ships, cars, bridges.

43
Q

What is the use of high-carbon steel?

A

Tools e.g. knives, screwdrivers.
(High-carbon so less malleable and
stiffer than low-carbon steel.)

44
Q

What is the use of stainless steel?

A

Cutlery, cooking utensils, kitchen sinks.

45
Q

What is the use of copper?

A

Wires, Cooking pans, Water pipes

46
Q

What is the use of aluminium?

A

Aircraft bodies, Power cables

Chemistry (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions