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IP Secondary 4 Chemistry > Chapter 2 - Metal Activity Series > Flashcards

Chapter 2 - Metal Activity Series Flashcards

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1
Q

Metal reactivity series :)

A 
potassium (K)
sodium (Na)
calcium (Ca)
magnesium (Mg)
aluminium (Al)
  carbon (C)
zinc (Zn)
iron (Fe)
tin (Sn)
lead (Pb)
  hydrogen (H)
copper (Cu)
silver (Ag)
gold (Au)
platinum (Pt)
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2
Q

General properties of metals: appearance

A

Shiny (lustrous)

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3
Q

General properties of metals: physical state

A

Solid at room temperature and pressure

except Hg

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4
Q

General properties of metals: density

A

Usually high

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5
Q

General properties of metals: strength

A

Strong

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6
Q

General properties of metals: ease of shaping

A

Malleable (can be bent) and ductile (can be stretched without breaking)

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7
Q

General properties of metals: melting & boiling points

A 
Usually high
(except Hg and Group I metals)
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8
Q

General properties of metals: heat conductivity

A

Good conductors of heat

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9
Q

General properties of metals: Electrical conductivity

A

Good conductors of electricity

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10
Q

Why are pure metals not widely used?

A

They are often too soft and have a low resistance to corrosion

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11
Q

What is an alloy?

A

A mixture of a metal with one or a few other elements

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12
Q

Why are alloys made?

A
  • To improve the appearance of the metal
  • To lower the melting point of the metal
  • To improve the strength and hardness of the metal
  • To improve the resistance of the metal against corrosion
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13
Q

Why are alloys stronger (less malleable and ductile) than its pure metals?

A
  • In pure metals, layers of atoms with equal size can slip over each other easily
  • In alloys, layers of atoms cannot slip over each other easily as atoms of alloying elements with different sizes distort the orderly arrangement of the metal atoms
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14
Q

What determines the reactivity of a metal?

A

The ease at which the metal atoms lose electrons

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15
Q

What characterises highly reactive metals?

A
  • They have a greater tendency to lose electrons to form cations
  • They are more likely to be found as positive ions rather than neutral atoms
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16
Q

The more easily the electrons are lost, the ________ reactive is the metal

A

more

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17
Q

What is the general equation for reaction of metals with cold water?

A

metal + cold water → metal hydroxide + hydrogen gas

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18
Q

What are the metals that react with cold water?

A

potassium (K)
sodium (Na)
calcium (Ca)
magnesium (Mg)

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19
Q

What is the general equation for reaction of metals with steam?

A

metal + steam → metal oxide + hydrogen gas

20
Q

What are the metals that react with steam?

A

aluminium (Al)
zinc (Zn)
iron (Fe)
tin (Sn)

21
Q

What is the general equation for reaction of metals with dilute acid?

A

metal + dilute acid → metal salt + hydrogen gas

22
Q

What are the metals that react with dilute acid?

A 
potassium (K)          zinc (Zn)
sodium (Na)             iron (Fe)
calcium (Ca)             tin (Sn)
magnesium (Mg)     lead (Pb)
aluminium (Al)
23
Q

What happens in the reaction of metals with other metal oxides?

A

A more reactive metal can displace (reduce) a less reactive metal oxide
(displacement reaction)

24
Q

What happens in the reaction of metals with other metal solutions?

A

A more reactive metal can displace (reduce) a less reactive metal ion from its solution
(displacement reaction)

25
Q

What happens in the heating of metal carbonates?

A

A more reactive metal forms a more stable carbonate that is more difficult to decompose by heating
(thermal decomposition)

26
Q

What are the observations for potassium + cold water?

A

Reacts explosively

Burns with a lilac flame

27
Q

What are the observations for sodium + cold water?

A

Reacts violently

Burns with a yellow flame

28
Q

What are the observations for calcium + cold water?

A

Reacts readily with lots of bubbles

29
Q

What are the observations for magnesium + cold water?

A

Reacts very slowly with only a few bubbles

30
Q

What are the observations for magnesium + steam?

A

Reacts violently

Burns with a bright white glow

31
Q

What are the observations for zinc + steam?

A

Reacts readily

Zinc oxide is yellow when hot and white when cold

32
Q

What are the observations for iron + steam?

A

Reacts slowly

Iron must be heated constantly

33
Q

What are the observations for potassium + dilute acid?

A

Reacts explosively

34
Q

What are the observations for sodium + dilute acid?

A

Reacts explosively

35
Q

What are the observations for calcium + dilute acid?

A

Reacts violently

36
Q

What are the observations for magnesium + dilute acid?

A

Reacts rapidly

37
Q

What are the observations for zinc + dilute acid?

A

Reacts moderately

38
Q

What are the observations for iron + dilute acid?

A

Reacts slowly

39
Q

What are the observations for lead + dilute acid?

A

Reacts slowly

reaction stops quickly with hydrochloric acid as insoluble lead(II) chloride is formed

40
Q

What is reduction used for with metals?

A

Used to extract metals from their ores

41
Q

What are metal ores?

A
  • A naturally occurring compound of the metal

- Most are metal oxides mixed with large amount of impurities

42
Q

How are oxides of metals below carbon in the reactivity series reduced?

A

Heated with carbon to form the metal and carbon dioxide

43
Q

How are oxides of metals above carbon in the reactivity series reduced?

A

By electrolysis to decompose the molten metal oxides

44
Q

How are oxides of metals below zinc in the reactivity series reduced?

A

Hydrogen is passed over the metal oxides to form the metal and water

45
Q

Metals higher in the reactivity series form more ________ compounds which require more ________ to reduce the compounds to the metals

A

stable

energy

IP Secondary 4 Chemistry (3 decks)

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