TOPIC 9 - Magic Metals Flashcards

1
Q

Metallic bonding

A

As the outer electrons are delocalised; this produces an electrostatic force of attraction between the positively charged metal ions, and the negatively charged delocalised electrons.

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2
Q

How do metallic bonds allow conductivity?

A

The delocalized electrons are free to move therefore an electrical current can flow (through metallic materials.)

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3
Q

Many transition metals can be used as

A

catalysts.

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4
Q

Do metals combine to form compounds?

A

No

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5
Q

What do metals mix to form

A

alloys.

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6
Q

All metals are

A

insoluble.

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7
Q

Reaction of metal reacting with water

A

metal + water -> metal hydroxide + hydrogen

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8
Q

All metals above ______ react with acids

A

hydrogen

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9
Q

The first _ elements in the EM series react with water

A

4

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10
Q

All the metals above _____ react with oxygen

A

gold

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11
Q

Reaction of metal reacting with acid

A

metal + acid -> salt + hydrogen

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12
Q

Reaction of metal reacting with oxygen

A

metal + oxygen -> metal oxide

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13
Q

The first metals to be discovered were the most unreactive and remained uncombined, these are:

A

silver and gold

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14
Q

equation for extraction of metal through heat alone

A

metal oxide -> metal + oxygen

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15
Q

equation for extraction of metal through heat with carbon or carbon monoxide

A

metal oxide + carbon -> metal + carbon dioxide

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16
Q

equation for extraction of metal through electrolysis

A

metal ions -> metal + oxygen

17
Q

reducing agents; name 4

A

carbon, carbon monoxide, hydrogen and methane

18
Q

reducing agents remove ____ from a metal ____.

A

oxygen; oxide.

19
Q

ELECTROLYSIS: the positive metal ion is attracted to the ______ electrode where it _____ enough electrons to _______. This is a ______ reaction.

A

negative; gains; turn back into the metal atom; reduction

20
Q

ELECTROLYSIS: the non-metal ion is attracted to the ______ electrode where it _____ enough electrons to ________. This is a ______ reaction.

A

positive; loses; form the element; oxidation

21
Q

an electrolyte

A

ionic solution

22
Q

what does the electrolyte do

A

complete the circuit

23
Q

a basic electrochemical cell requires

A

two different metals connected by an external circuit and between the metals there is an electrolyte

24
Q

electricity is produced by

A

the flow of electrons from one metal to the other

25
Q

redox can also be known as

A

displacement reactions.

26
Q

what is a displacement reaction

A

where a metal ion is displaced from solution by a metal higher up the electromagnetic series

27
Q

reactions in fuel cells

A

2H₂ -> 4H⁺ + 4e⁻

O₂ + 4H⁺ + 4e⁻ -> 2H₂O

28
Q

when metals react with oxygen the process is called

A

corrosion / rusting for iron

29
Q

rusting in iron requires:

A

iron, oxygen and water

30
Q

a rusting indicator

A

ferroxyl

31
Q

ferroxyl goes ___ when iron ions are present

A

yellow to blue

32
Q

ferroxyl goes ___ when hydroxide ions are present

A

yellow to pink

33
Q

when iron rusts in ferroxyl indicator it goes dark blue because

A

the blue iron(2+) ions mask the pink hydroxide ones

34
Q

how to speed up rusting

A

increasing the concentration of the electrolyte

35
Q

how to prevent rusting (4)

A

paint, grease, plastic and metal plating with unreactive metals

36
Q

sacrificial protection is when

A

metals higher up in the electrochemical series than iron donate electrons that prevent the iron rusting.

37
Q

galvanising is when

A

iron is coated in a layer of zinc, which acts like a barrier against air and water, but if the zinc is damaged it acts like a sacrificial protector to the iron.

38
Q

what is the only problem with galvanising

A

expensive

39
Q

cathodic protection is where

A

iron is attached the negative terminal of a battery or electrical supply