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Chemistry > 9 - Metals > Flashcards

9 - Metals Flashcards

1
Q

Why is Aluminium almost as reactive as Magnesium, yet takes much longer to react?

A

It has a thin protective layer of Aluminium Oxide that take time to wear away

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2
Q

Name all the metals and hydrogen in their order of reactivity from highest to lowest

A

Potassium

Sodium

Lithium

Calcium

Magnesium

Aluminium

(Carbon)

Zinc

Iron

(Hydrogen)

Copper

Silver

Gold

Please Send Little Charlies Monkeys And Zebras In Hinged Cages Guarded Safely

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3
Q

What is the reactivity series?

A

The order of reactivity of a few selected metals and hydrogen

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4
Q

Which metals react with cold water?

Name them in order of reactivity from higherst to lowest

A
  • Potassium
  • Sodium
  • Lithium
  • Calcium
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5
Q

Which metals react with steam and acids only?

Name them in order of reactivity from higherst to lowest

A
  • Magnesium
  • Aluminium
  • Zinc
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6
Q

Which substances react with acids only?

Name them in order of reactivity from highest to lowest

A
  • Iron
  • Hydrogen
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7
Q

Which substances do not react?

Name them in order of reactivity from higherst to lowest

A
  • Copper
  • Silver
  • Gold
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8
Q

When does a displacement reaction occur?

A

When a metal reacts with an ion of another metal, and the metal is more reactive than the ion.

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9
Q

What is a displacement reaction (for metals)?

A

A reaction where a more reactive metal reduces a metal ion, making it gain electrons and form a metal atom as well

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10
Q

What is the link between displacement and redox reactions?

A

Displacement reaction are always redox reactions

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11
Q

In which states do metals conduct electricity?

A

Solids and liquids

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12
Q

What is the word equation for the corrosion of iron?

Aka Rusting

A

Iron + Oxygen gas + Water —> Hydrated Iron (III) Oxide

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13
Q

What are the methods to prevent rusting?

A
  • Painting
  • Greasing
  • Plastic covering
  • Electroplating
  • Galvanisation
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14
Q

What is Galvanisation?

A

Iron to be protected is coated with a layer of zinc.

This can be done by electroplating or dipping it into molten zinc

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15
Q

Def. Barrier Method

A

Physical barrier to prevent corrosion

|Eg. Greasing, painting, or plastic coating

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16
Q

Def. Sacrificial protection

A

A more reactive metal is oxidised in preference; it loses its electrons easier

This means another meal can be used to prevent the first from rusting

17
Q

Def. Alloy

A

A mixture of a metal with other elements

18
Q

What alloys are you required to know?

A

Brass - Mixture of copper and zinc

Stainless Steel - Mixture of iron with other elements such as chromium, nickel and carbon

19
Q

What are the advantages of alloys?

A
  • They can be harder and stronger than pure metals
  • They can be more useful than normal metals e.g resistant to corrosion
20
Q

Why is stainless steel used in cutlery?

A
  • Hardness
  • Resistance to rusting
21
Q

Why are alloys harder and stronger than pure metals?

A

They have ions of different sizes so layers of ions can’t slide over each other as easily

Meaning they aren’t as malleable

22
Q

What are the uses of aluminium?

Explain the properties that allow it to be useful

A
  • Food Containers - Corrosion resistant
  • Aircraft - Low density
  • Overhead cables - Good electrical conductor & low density
23
Q

What are the uses of stainless steel?

Explain the properties that allow it to be useful

A
  • Cutlery - Corrosion resistant
24
Q

What are the uses of Zinc?

Explain the properties that allow it to be useful

A
  • Galvanising steel - To prevent corrosion through sacrificial protection
  • Making brass - Increases hardness
25
Q

What are the uses of Copper?

Explain the properties that allow it to be useful

A
  • Making brass - Increases hardness
  • Electrical wires - Good electrical conductor

Chemistry (12 decks)

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