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nat 5 chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

What are the properties of metals ?

A

Shiny
Malleable
Good conductors of heat and electricity

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2
Q

Why is it important we recycle metals ?

A

They are finite in nature

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3
Q

What is metallic bonding ?

A

The force of attraction between positively charged ions and delocalised electrons

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4
Q

What is an alloy?

A

Is a mixture of two or more elements, at least one of which is a metal

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5
Q

What do alloys have in comparison to pure elements ?

A

Different physical properties and are often more useful that pure metals

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6
Q

What is brass an alloy of ?

A

70% copper

30% zinc

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7
Q

What is 18 carat gold an alloy of?

A

75% gold

25% copper/other metals

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8
Q

What is the chemical formula for potassium permanganate ?

A

KMnO4

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9
Q

What does a metal + oxygen produce ?

A

Metal oxide

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10
Q

What metals do not readily react with oxygen ?

A

Mercury
Silver
Gold

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11
Q

What does a metal + water produce?

A

Metal hydroxide + hydrogen

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12
Q

Most metals don’t react with water but what do?

A

Only group 1 and group 2

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13
Q

Why do alkali metals have to be stored under oil?

A

They react violently with water

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14
Q

What do metal + acid produce?

A

Salt + hydrogen

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15
Q

What metals do not react with dilute acid?

A

Copper
Mercury
Silver
Gold

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16
Q

What is oilrig ?

A

Oxidation is loss

Reduction is gain

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17
Q

What metals react with oxygen to form metal oxide ? (11)

A 
Potassium 
Sodium
Lithium 
Calcium
Magnesium 
Aluminium 
Zinc 
Iron 
Tin
Lead

Copper

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18
Q

What metals react with water to form metal hydroxide and hydrogen? (5)

A 
Potassium
Sodium
Lithium
Calcium
Magnesium
19
Q

What metals react with acid to form a metal salt and hydrogen ?(10)

A 
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium 
Zinc 
Iron 
Tin
Lead
20
Q

How can less reactive metals (copper, Mercury, silver, gold) be found?

A

Uncombined in the earths crust

21
Q

What is the equation for the extraction of unreactive metals by heat alone ?

A

Metal oxide > metal+oxygen

22
Q

What type of reaction are the extractions of metals from ores ?

A

Reduction.

23
Q

How can slightly more reactive metals be removed from their oxides ?

A

By heating with carbon or carbon monoxide

24
Q

Give 2 examples of unreactive metals that can be extracted from their oxide by heating alone ?

A

Mercury and silver

25
Q

Give 2 examples of slightly more reactive metals that can be extracted from their oxide by heating with carbon or carbon monoxide ?

A

Copper and zinc

26
Q

By extracting slightly more reactive metals by heating carbon or carbon monoxide what do they produce ?

A

Metal atom and carbon dioxide

27
Q

Where can iron from iron ore be produced ?

A

In a blast furnace

28
Q

How can even more reactive metals be extracted from their compounds ?

A

By electrolysis

29
Q

Give examples of even more reactive metals that can be extracted from their compounds by electrolysis ?

A 
Potassium 
Sodium
Lithium
Calcium
Magnesium
Aluminium
30
Q

During electrolysis what happens to the metal ions ?

A

They gain electrons at the negative electrode to become metal atoms

31
Q

What are the 3 methods in which metals can be extracted from their ores if not found uncombined ?

A

Extraction by heating alone
Extraction by heating with carbon or carbon monoxide
Extraction by electrolysis

32
Q

What is oilrig ?

A

Oxidation is loss

Reduction is gain

33
Q

What reactions always occur together?

A

Oxidation and reduction

34
Q

What is the name given to oxidation and reduction reactions that occur at the same time ?

A

Redox reactions

35
Q

What can redox reactions be split into?

A

2 ion-electron equations

36
Q

What reaction produces a metal atom?

A

Reduction

37
Q

What reaction produces metal ion and electron?

A

Oxidation

38
Q

What are displacement reactions ?

A

If we place a metal into a solution of ions which are lower in the ECS, the higher metal will displace the lower metal

39
Q

Describe displacement reactions ?

A

The higher metal will lose electrons to become ions and go into the solution (oxidation) whereas the lower metal will gain electrons, become metal atoms and comes out of solution (reduction)

40
Q

What must the ion electron equation be for a oxidation?

A

Reversed

41
Q

What is not included in redox equations?

A

Electrons and spectator ions

42
Q

What is a reducing agent?

A

A chemical which causes another substance to reduce I.e. Donates electrons (oxidation)

43
Q

What metals in the ECS react with acids ?

A

Only metals above hydrogen

44
Q

Give 2 examples of energy sources that power objects through redox reactions ?

A

Fuel cells and rechargeable batteries

nat 5 chemistry (13 decks)

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