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chemistry > Chemistry In Society #1: Metals > Flashcards

Chemistry In Society #1: Metals Flashcards

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1
Q

What does each atom in a metal do?

A

Loses its outer electrons to form positive ions

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2
Q

What do these positive metal ions do?

A

They form a regular, 3 dimensional lattice of positively charged ions

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3
Q

The outer electrons of metal ions can be described as… why?

A

Delocalised
They are not attached to a particular atom and are free to move around

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4
Q

What does the electrostatic attraction do positive metal ions for the delocalised electrons do?

A

They BIND the positive ions together

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5
Q

What is electric current?

A

A flow of charged particles (ions, electrons)

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6
Q

Why can metals conduct electricity?

A

Because electrons can flow through them without chemical changes taking place

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7
Q

Why is electrolysis the opposite case of metals conducting electricity?

A

Electrons cannot flow through without chemical changes taking place

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8
Q

What is the reactivity series?

A

A list of metals in order of reactivity, eg with oxygen, water, and dilute acids

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9
Q

What metals do not react?

A

Gold, silver

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10
Q

What metals will combine with oxygen when heated?

A

All ABOVE silver

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11
Q

What is the equation for metals combining with oxygen when heated?

A

Metal + oxygen -> metal oxide

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12
Q

The higher the metal is in the series,

A

The more violent the reaction

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13
Q

Metals high in the table are good at…

A

Losing electrons, therefore are more reactive

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14
Q

What metals react with water?

A

All above ALUMINIUM

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15
Q

What is the equation for metal reacting with water?

A

Metal + water -> metal hydroxide + hydrogen

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16
Q

What metals react with a DILUTE ACID?

A

All above copper

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17
Q

What is the word equation for metals reacting with a dilute acid?

A

Metal + acid -> salt + hydrogen

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18
Q

Oxidation reaction

A

One in which electrons are lost or oxygen is gained

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19
Q

Reduction reaction

A

One in which electrons are gained

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20
Q

What are redox reactions

A

Ones which involve both reduction and oxidation taking place at the same time

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21
Q

What do you do if the ion-electron equations do not contain equal numbers of electrons?

A

Balance them. Multiply one or both of the ion-electron equations

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22
Q

What is a displacement reaction?

A

It involves the formation of a metal from a solution containing its ions by reaction with a metal higher in the ECS

23
Q

How do you know where to place hydrogen in the ECS?

A

According to its reaction with dilute hydrochloric acid

24
Q

Metals can displace hydrogen ions to

A

Produce hydrogen gas

25
Q

Where is hydrogen in the ECS?

A

between lead and copper

26
Q

What are ores?

A

Naturally occurring compounds of metals
Most ores are oxides

27
Q

Why were gold, silver, and copper the first metals to be discovered?

A

They are found uncombined in the earth’s crust

28
Q

The extraction of gold, silver, copper metal ores …

A

Does NOT involve a chemical reaction

29
Q

What do we have to do to more reactive metals unlike CU AG AU?

A

extract them from their ores

30
Q

The method of extraction depends on…

A

The reactivity of the metal

31
Q

The more reactive the metal,

A

The stronger the bonds which hold the compound together, the more energy required to extract it

32
Q

What type of reaction is the extraction of any metal from its ore?

A

A reduction one

33
Q

How can we extract metals below copper?

A

Using heat alone

34
Q

Equation for extraction using heat alone

A

Metal oxide -> metal + oxygen

35
Q

How can we extract oxides of metals above MERCURY and below aluminium in the reactivity series?

A

Heating with carbon or carbon monoxidw

36
Q

Equation for extraction with heat and carbon / carbon monoxide

A

Metal oxide + carbon -> metal + carbon dioxide
Metal oxide + carbon monoxide -> metal + carbon dioxide

37
Q

How do extraction reactions with carbon (monoxide) work?

A

Because the carbon bonds stronger with the oxygen than the metal dows

38
Q

Carbon and carbon monoxide are

A

Reducing agents

39
Q

Why does heating with carbon not work as an extraction method for oxides of metals above zinc?

A

The metal bonds more strongly with the oxygen than carbon does

40
Q

How are oxides of metals above zinc extracted?

A

Electrolysis of molten compounds using a direct current

41
Q

What is electrolysis?

A

The decomposition of an ionic compound into its elements

42
Q

Why must a direct current (DC) suple be used in electrolysis?

A

If the products are ti be identified

43
Q

Why does electrolysis work?

A

When the compound becomes molten, the ionic lattice breaks and the ions are free to move

44
Q

Where are the positive metal ions attracted to in electrolysis? What do they do there?

A

The negative electrode
They gain electrons and form metals ions

45
Q

Ions flow through…

A

Solutions

46
Q

Electrons flow through…

A

Metal wires

47
Q

Electrochemical cells: (3)

A
  • convert chemical cells into electric energy
  • contain one substance which gives up electrons
  • contain another substance which accepts electrons
48
Q

What is an electrolyte?

A

A substance which completes the circuit by allowing ions to move through it

49
Q

What does a cell consist of?

A
  • 2 different metals
  • an electrolyte to complete the circuit
50
Q

Why does NaCl solution work as an electrolyte?

A

It is an ionic solution, so ions can move through it

51
Q

The voltage between different pairs of metals…

A

Varies

52
Q

Metals can be sorted by their voltages. How?

A

In the ECS

53
Q

In conclusion, the ECS is

A

A list of metals (&hydrogen) in order of their ability to lose electrons and form ions in solution

chemistry (5 decks)

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