Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

IGCSE CHEMISTRY MATS > 4 - Metals > Flashcards

4 - Metals Flashcards

1
Q

What is the state of metals at room temperature?

A
  • solids

- mercury is the exception as it is a liquid at room temperature

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

What are the melting points of metals?

A
  • high melting points
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How good is the electrical conductivity of metals?

A
  • very good electrical conductors
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How good is the thermal conductivity of a metal?

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

What is the appearance of most metals?

A
  • shiny

- metallic

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

What density do metals have?

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

What is the strength of metals?

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

Are metals malleable and ductile?

A

yes

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

Group 1 metals are ____ ________

A

very reactive

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

Group _ metals have relatively ___ _______ points

A

1, low melting

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Group 1 metals are ____ and can be cut ____ _ _____

A

soft, with a knife

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

Group 1 metals have a ___ _______ and some _____ on water

A

low density, float

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What do Group 1 metals form when reacting with water?

A
  • alkaline solution

- Hydrogen gas

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

Transition metals have ____ _______ points

A

high melting

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

Transition metals are not ____ ________

A

very reactive

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

Transition metals are useful as _________

A

catalysts

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

Transition metals are _____ and ____

A

strong, hard

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

Transition metals compounds are ________

A

coloured

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

Group 1 metals compounds are _____

A

white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Transition metals have a ____ density

A

high

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Transition metals and Group 1 metals form _____ compounds on reactions with ___-______

A

ionic, non-metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Transition metals and Group 1 metals are good _______ and __________ conductors

A

thermal, electrical

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Why are metals good conductors of electricity?

A

The delocalised electrons can flow and carry charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Why are metals mallaeble?

A

Their structure is in layers, layers can slide over each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What are the 3 types of bonding?
- ionic - covalent - metallic
26
Define ionic bonding
Two oppositely charged ions that are electrostatically attracted
27
Define covalent bonding
Shared pair of electrons electrostatically attracted to two positive nuclei.
28
Define metallic bonding
Regular arrangement of positive nuclei and delocalised electrons
29
When does an ionic bond happen?
metal + non-metal
30
When does a covalent bond form?
non-metal + non-metal
31
When does a metallic bond form?
metal + metal
32
What does an ionic bond form?
It forms giant ionic lattices (lots of very strong electrostatic attractions that take a lot of energy to break) 
33
What are giant ionic lattices?
Lots of very strong electrostatic attractions that take a lot of energy to break
34
Why do ionic bonds only conduct if liquid or aqueous?
Because the ions are free to move and carry charge
35
Do covalent bonds conduct electricity?
No
36
What is a giant covalent?
- graphite, diamond | - lots of strong covalent bonds so needs lots of energy to break
37
What is a simple molecular?
- carbon dioxide, ethane, water | - weak intermolecular bonds that do not need much energy to break
38
What do covalent bonds form?
- giant covalent | - simple molecular
39
Order of reactivity from least reactive to most reactive
- gold - silver - copper - iron - zinc - aluminium - magnesium - calcium - lithium - sodium - potassium
40
Describe the reaction between potassium and water
- purple flame - effervescence - dissolves/melts
41
Describe the reaction between sodium and water
- effervescence - dissolves - melts
42
Describe the reaction between lithium and water
- effervescence | - dissolves
43
Describe the reaction between calcium and water
- gentle effervescence | - dissolves
44
Describe the reaction between magnesium and water
- no reaction with cold water | - will react with steam (very bright white light)
45
Describe the reaction between aluminium and water
- no reaction with cold water | - will react with steam
46
Describe the reaction between zinc and water
- no reaction with cold water | - will react with steam
47
Describe the reaction between iron and water
- no reaction with cold water | - will react with steam
48
Describe the reaction between copper and water
- no reaction
49
Describe the reaction between silver and water
- no reaction
50
Describe the reaction between gold and water
- no reaction
51
Metal + acid = ____ + ________
Metal + acid = salt + hyrdogen
52
How to measure which metal is the most reactive?
- react metal + acid in conical flask - bung + gas syringe - the hydrogen will fill the gas syringe - the metal that produced the most hydrogen is the most reactive
53
Define displacement
When a more reactive metal displaces a less reactive metal from its other element in the compound
54
Define oxidation
The loss of electrons 
55
Define reduction
The gain of electrons 
56
How to find the percentage of mass of an element in a compound?
100 x atomic mass of element/atomic mass of compound
57
Which 4 metals react with water?
- potassium - sodium - lithium - calcium
58
Which 10 metals react with acids?
- potassium - sodium - lithium - calcium - magnesium - aluminium - zinc - iron - tin - lead
59
Which 13 metals react with oxygen?
- potassium - sodium - lithium - calcium - magnesium - aluminium - zinc - iron - tin - lead - copper - mercury - silver
60
Define rusting
When a metal (iron) reacts with oxygen to form a metal oxide. For this to happen you need water and oxygen 
61
What are the 5 ways to prevent/avoid rusting?
- painting - oiling or greasing - covering with plastic - galvanising - sacrificial protection
62
Why does painting prevent rusting? 
- paint covers the metal | - if paint is scratched, rusting starts as metal is exposed to oxygen and water
63
Why does oiling or greasing prevent rusting?
- moving parts of a machine cannot be protected by paint - instead of paint, grease or oil is used - helps lubricate the parts as well
64
Why does covering with plastic prevent rusting?
The water and oxygen cannot reach the metal. 
65
Why does galvanising prevent rusting?
- coat a less reactive metal with a more reactive metal - oxygen in the air and water will react with the more reactive metal first  - protection layer will form to protect the wanted metal 
66
Why does sacrificial protection prevent rusting?
More reactive metals are attached along the product (normally very big products) in intervals so that the water or oxygen reacts with it before it reacts with the protected metal. Once all the sacrificial metal is gone, it is replaced. 
67
What is a reducing agent?
- usually a metal or a negative ion - loses electrons to another element or ion - is itself oxidised
68
What is an oxidising agent?
- normally a non-metal or positive ion - causes oxidation reactions  - gains electrons from other atoms or ions (is itself reduced)
69
What do metal + water form?
metal + water = metal hydroxide + hydrogen

IGCSE CHEMISTRY MATS (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions