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AA IGCSE Chemistry > Metals and the Reactivity Series > Flashcards

Metals and the Reactivity Series Flashcards

1
Q

Compare the general physical properties of metals and non-metals.

A
  • metals have high melting/boiling points, non-metals have low
  • metals are good electric conductors, non-metals are electric insulators
  • metals are good thermal conductors, non-metals are thermal insulators
  • metals are ductile/malleable, not non-metals
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2
Q

State the order of the reactivity series.

A

potassium
sodium
calcium
magnesium
aluminium
carbon
zinc
iron
tin
lead
hydrogen
copper
silver
gold

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3
Q

Where is hydrogen in the reactivity series?

A

below iron, above copper

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4
Q

Where is carbon in the reactivity series?

A

below aluminium, above zinc

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5
Q

Reaction of metals with water.

A

metal + water → metal hydroxide + hydrogen

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6
Q

Group I elements are ____ reactive than Group II.

A

more

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7
Q

Which elements are more reactive, group 1 or 2?

A

group 1

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8
Q

For metals, what does the group define about their reactivity?

A

the lower the group the more reactive

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9
Q

For metals, what does the mass of an element define about their reactivity?

A

heavier elements further down the group are more reactive

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10
Q

Mnemonic for reactivity series.

A

Please send cats, monkeys and zebras charging into hot countries,
Signed Greg

OR (para aluninhos do dicks - annuca):

please stop calling me a careless zebra, instead try learning how copper saves gold

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11
Q

Reaction of metals with dilute acids.

A

metal + acid → salt + hydrogen

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12
Q

Reaction of metals with oxygen.

A

metal + oxygen → metal oxide

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13
Q

What is aluminium used for and why?

A
  • manufacture of aircraft: low density
  • manufacture of overhead electrical cables: low density + good electrical conductivity
  • food containers: resistance to corrosion
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14
Q

What is copper used for and why?

A

electrical wiring: good electrical conductivity and ductility

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15
Q

Describe the reaction of potassium with cold water.

A
  • vigorous effervescence
  • hydrogen gas released
  • metal floats on water surface, gets smaller as it reacts
  • after a short while the gas given off will ignite and a lilac-coloured flame seen
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16
Q

Describe the reaction of sodium with cold water.

A
  • similar to potassium, but reaction is less vigorous so the hydrogen gas may not ignite
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17
Q

Describe the reaction of calcium with cold water.

A
  • solid metal sinks
  • bubbles produced on surface of the metal (much slower than K and Na)
  • as metal disappears, solution becomes cloudy as calcium hydroxide is insoluble
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18
Q

Describe the reaction of magnesium with cold water/steam.

A

no reaction with cold water, but reacts with steam to form hydrogen and white powder (magnesium oxide)

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19
Q

The solid metal sinks, bubbles produce on the surface of the metal, as the metal disappears solution turns cloudy. What reaction is this?

A

calcium and water

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20
Q

Describe the reaction of magnesium with dilute HCl.

A

strong: bubbles form quickly on the surface, metal slowly disappears

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21
Q

Describe the reaction of zinc with dilute HCl.

A

bubbles slowly form

22
Q

Describe the reaction of iron with dilute HCl.

A

very slow, must be powdered iron

23
Q

Describe the reaction of copper/silver/gold with dilute HCl.

A

none

24
Q

A metal reacts with dilute HCl. The reaction is slow and the metal must be powdered. What is the metal?

A

iron

25
Q

A metal reacts with dilute HCl. The reaction is bubbles forming slowly. What is the metal?

A

zinc

26
Q

Explain the apparent unreactivity of aluminium.

A

aluminium oxide forms quickly when aluminium is exposed to air, creating an oxide layer that creates a perfect barrier around the aluminium, preventing further metal reaction

27
Q

How can displacement reactions be used to extract metals?

A
  • carbon is more reactive than the metal, so it displaces the metal from its oxides
  • produces pure metal and carbon dioxide
28
Q

How can we extract metals less reactive than carbon?

A

mixing them with carbon (most likely as charcoal) and heating them to high temperatures

29
Q

A _____ reactive metal displaces a _____ reactive metal.

A

more/less

30
Q

What is a displacement reaction?

A

a more reactive element is taking the place of a less reactive element

31
Q

State the conditions required for the rusting of iron and steel.

A

oxygen and water in the air

32
Q

What is the chemical name for rust?

A

hydrated iron(III) oxide

33
Q

Word equation for rusting

A

iron + water + oxygen → hydrated iron(III) oxide

34
Q

Symbol equation for rusting

A

2Fe(s) + 2H2O(l) + O2(g) → Fe2O3·H2O(s)

35
Q

State some common barrier methods.

A
  • painting
  • greasing
  • coating with plastic
36
Q

Which metal quickly forms an oxide layer, appearing unreactive?

A

aluminium

37
Q

Describe how barrier methods prevent rusting.

A

by preventing oxygen or water from reaching the metal

38
Q

What is a barrier method?

A

set of techniques to prevent corrosion by preventing oxygen and water coming into contact with the metal surface

39
Q

What is zinc in galvanising an example of?

A

barrier method and sacrificial protection

40
Q

Describe the use of zinc in galvanising.

A

iron/steel objects are completely coated in a thin layer of zinc, the zinc forms a barrier between the iron and oxygen in the atmosphere

41
Q

What is sacrificial protection?

A

protecting a metal from corrosion by allowing another more reactive metal, to corrode instead

42
Q

What is sacrificial protection often used for?

A

hulls of ships, as salt water accelerates rusting

43
Q

Describe sacrificial protection.

A
  • iron/steel placed in contact with a more reactive metal
  • more reactive metals loses electrons more easily than iron
  • presence of electrons prevents iron from oxidising
  • while more reactive metals than iron remain in contact with the iron, it remains protected
44
Q

uses of aluminium

A
  • aluminium in the manufacture of aircraft because of its low density
  • aluminium in the manufacture of overhead electrical cables because of its low density and good electrical conductivity
  • aluminium in food containers because of its resistance to corrosion
45
Q

use of copper

A

electrical wiring because of its good electrical conductivity and ductility

46
Q

reactions of metals with water

A

potassium - most vigorous
sodium - vigorous
calcium- strong
magnesium - only reacts with steam
aluminium - no reaction

47
Q

word equation for metal reaction with dilute acid

A

metal + acid → salt + hydrogen

48
Q

word equation for metal reaction with water

A

metal + water → metal hydroxide + hydrogen

49
Q

word equation for metal reaction with oxygen

A

metal + oxygen → metal oxide

50
Q

metals reaction with dilute acid

A

potassium - explosive
sodium - violent
calcium - rapid with many bubbles
magnesium - rapid, steady bubbles
zinc - slow
iron - very slow
copper - nada

AA IGCSE Chemistry (18 decks)

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