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IGCSE CHEMISTRY MATS > 4 - Metals > Flashcards

4 - Metals Flashcards

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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

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2
Q

What are the melting points of metals?

A
  • high melting points
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3
Q

How good is the electrical conductivity of metals?

A
  • very good electrical conductors
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4
Q

How good is the thermal conductivity of a metal?

A
  • very good
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5
Q

What is the appearance of most metals?

A
  • shiny

- metallic

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6
Q

What density do metals have?

A
  • high density
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7
Q

What is the strength of metals?

A
  • very strong
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8
Q

Are metals malleable and ductile?

A

yes

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9
Q

Group 1 metals are ____ ________

A

very reactive

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10
Q

Group _ metals have relatively ___ _______ points

A

1, low melting

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11
Q

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

A

soft, with a knife

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12
Q

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

A

low density, float

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13
Q

What do Group 1 metals form when reacting with water?

A
  • alkaline solution

- Hydrogen gas

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14
Q

Transition metals have ____ _______ points

A

high melting

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15
Q

Transition metals are not ____ ________

A

very reactive

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16
Q

Transition metals are useful as _________

A

catalysts

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17
Q

Transition metals are _____ and ____

A

strong, hard

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18
Q

Transition metals compounds are ________

A

coloured

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19
Q

Group 1 metals compounds are _____

A

white

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20
Q

Transition metals have a ____ density

A

high

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21
Q

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

A

ionic, non-metals

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22
Q

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

A

thermal, electrical

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23
Q

Why are metals good conductors of electricity?

A

The delocalised electrons can flow and carry charge

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24
Q

Why are metals mallaeble?

A

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

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25
Q

What are the 3 types of bonding?

A
  • ionic
  • covalent
  • metallic
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26
Q

Define ionic bonding

A

Two oppositely charged ions that are electrostatically attracted

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27
Q

Define covalent bonding

A

Shared pair of electrons electrostatically attracted to two positive nuclei.

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28
Q

Define metallic bonding

A

Regular arrangement of positive nuclei and delocalised electrons

29
Q

When does an ionic bond happen?

A

metal + non-metal

30
Q

When does a covalent bond form?

A

non-metal + non-metal

31
Q

When does a metallic bond form?

A

metal + metal

32
Q

What does an ionic bond form?

A

It forms giant ionic lattices (lots of very strong electrostatic attractions that take a lot of energy to break)

33
Q

What are giant ionic lattices?

A

Lots of very strong electrostatic attractions that take a lot of energy to break

34
Q

Why do ionic bonds only conduct if liquid or aqueous?

A

Because the ions are free to move and carry charge

35
Q

Do covalent bonds conduct electricity?

A

No

36
Q

What is a giant covalent?

A
  • graphite, diamond

- lots of strong covalent bonds so needs lots of energy to break

37
Q

What is a simple molecular?

A
  • carbon dioxide, ethane, water

- weak intermolecular bonds that do not need much energy to break

38
Q

What do covalent bonds form?

A
  • giant covalent

- simple molecular

39
Q

Order of reactivity from least reactive to most reactive

A
  • gold
  • silver
  • copper
  • iron
  • zinc
  • aluminium
  • magnesium
  • calcium
  • lithium
  • sodium
  • potassium
40
Q

Describe the reaction between potassium and water

A
  • purple flame
  • effervescence
  • dissolves/melts
41
Q

Describe the reaction between sodium and water

A
  • effervescence
  • dissolves
  • melts
42
Q

Describe the reaction between lithium and water

A
  • effervescence

- dissolves

43
Q

Describe the reaction between calcium and water

A
  • gentle effervescence

- dissolves

44
Q

Describe the reaction between magnesium and water

A
  • no reaction with cold water

- will react with steam (very bright white light)

45
Q

Describe the reaction between aluminium and water

A
  • no reaction with cold water

- will react with steam

46
Q

Describe the reaction between zinc and water

A
  • no reaction with cold water

- will react with steam

47
Q

Describe the reaction between iron and water

A
  • no reaction with cold water

- will react with steam

48
Q

Describe the reaction between copper and water

A
  • no reaction
49
Q

Describe the reaction between silver and water

A
  • no reaction
50
Q

Describe the reaction between gold and water

A
  • no reaction
51
Q

Metal + acid = ____ + ________

A

Metal + acid = salt + hyrdogen

52
Q

How to measure which metal is the most reactive?

A
  • 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
Q

Define displacement

A

When a more reactive metal displaces a less reactive metal from its other element in the compound

54
Q

Define oxidation

A

The loss of electrons

55
Q

Define reduction

A

The gain of electrons

56
Q

How to find the percentage of mass of an element in a compound?

A

100 x atomic mass of element/atomic mass of compound

57
Q

Which 4 metals react with water?

A
  • potassium
  • sodium
  • lithium
  • calcium
58
Q

Which 10 metals react with acids?

A
  • potassium
  • sodium
  • lithium
  • calcium
  • magnesium
  • aluminium
  • zinc
  • iron
  • tin
  • lead
59
Q

Which 13 metals react with oxygen?

A
  • potassium
  • sodium
  • lithium
  • calcium
  • magnesium
  • aluminium
  • zinc
  • iron
  • tin
  • lead
  • copper
  • mercury
  • silver
60
Q

Define rusting

A

When a metal (iron) reacts with oxygen to form a metal oxide. For this to happen you need water and oxygen

61
Q

What are the 5 ways to prevent/avoid rusting?

A
  • painting
  • oiling or greasing
  • covering with plastic
  • galvanising
  • sacrificial protection
62
Q

Why does painting prevent rusting?

A
  • paint covers the metal

- if paint is scratched, rusting starts as metal is exposed to oxygen and water

63
Q

Why does oiling or greasing prevent rusting?

A
  • 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
Q

Why does covering with plastic prevent rusting?

A

The water and oxygen cannot reach the metal.

65
Q

Why does galvanising prevent rusting?

A
  • 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
Q

Why does sacrificial protection prevent rusting?

A

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
Q

What is a reducing agent?

A
  • usually a metal or a negative ion
  • loses electrons to another element or ion
  • is itself oxidised
68
Q

What is an oxidising agent?

A
  • normally a non-metal or positive ion
  • causes oxidation reactions
  • gains electrons from other atoms or ions (is itself reduced)
69
Q

What do metal + water form?

A

metal + water = metal hydroxide + hydrogen

IGCSE CHEMISTRY MATS (7 decks)

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