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NAT5 Chemistry > UNIT 3 - Metals > Flashcards

UNIT 3 - Metals Flashcards

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1
Q

what binds the ions together in metals?

A

The electrostatic attraction of positive metal ions for the delocalised electrons

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2
Q

what is electrolysis?

A

It is the decomposition of an ionic compound into its elements using electricity

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3
Q

What is required if the products are to be identified in electrolysis?

A

A direct current (dc) supply

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4
Q

what does each atom in a metal lose, and why?

A

its outer electrons, to form positive ions

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5
Q

what do the ions form after the metal has lost its outer electrons to become an ion?

A

a regular three dimensional lattice of positively charged ions

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6
Q

describe the outer electrons of a metal atom.

A

they are not attached to a particular atom and are free to move around, therefore they are delocalised

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7
Q

what is an electrical current?

A

a flow of charged particles (e-, ions)

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8
Q

why do metals conduct electricity?

A

because electrons can flow through them without chemical changes taking place

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9
Q

what is the reactivity series in order?

A
  1. pottasium
  2. sodium
  3. lithium
  4. calcium
  5. magnesium
  6. aluminium
  7. zinc
  8. iron
  9. tin
  10. lead
  11. copper
  12. mercury
  13. silver
  14. gold
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10
Q

what is the least reactive element?

A

gold (does not react at all)

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11
Q

what do all metals above silver in the reactivity series combine with?

A

they combine with oxygen when heated to form a metal oxide

metal + oxygen –> metal oxide

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12
Q

what happens the higher up the reactivity series the element is?

A

the higher the metal is in the reactivity series, the more violent the reaction

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13
Q

what do all of the metals above aluminium react with in the reactivity series?

A

they react with water to form a metal hydroxide and hydrogen.

metal + water –> metal hydroxide + hydrogen

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14
Q

what do all of the metals above copper in the reactivity series react with?

A

they react with a dilute acid to create salt and hydrogen.

metal + acid –> salt + hydrogen

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15
Q

how can metals be placed in order of reactivity?

A

by comparing the rates at which they react

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16
Q

what is an oxidation reaction?

A

one in which electrons are lost or oxygen is gained

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17
Q

what is a reduction reaction?

A

one in which electrons are gained or oxygen is lost

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18
Q

what is a Redox reaction?

A

a reaction which involves both reduction and oxidation reactions taking place at the same time

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19
Q

what must be removed at the end of a redox reaction?

A

the electrons

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20
Q

how do you balance redox equations?

A

by multiplying one or both of the ion-electron eqautions

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21
Q

what does a displacement reaction involve?

A

it involves the formation of a metal from a solution containing its ions by reaction with a metal higher in the electrochemical series

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22
Q

what non metal appears in the ECS?

A

hydrogen

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23
Q

what does ECS stand for?

A

electrochemical series

24
Q

how can you place hydrogen in the ECS?

A

you can place it according to its reaction with dilute hydrochloric acid

25
Q

what is produced when metals displace hydrogen ions?

A

hydrogen gas

26
Q

where is hydrogen in the ECS?

A

between LEAD and COPPER

27
Q

what are ores?

A

they are naturally occurring compounds of metals, and most ores are oxides

28
Q

what were the first metals to be found and why?

A

gold, silver, and copper, because they are found uncombined in the earths crust, therefore their extractions do not require a chemical reaction - they are inert

29
Q

what dictates how strong a metals bonds are?

A

the reactivity of the metal, if the metal is very reactive then more energy is required to seperate or extract it

30
Q

what type of reaction is any metal from its ore?

A

a reduction reaction

31
Q

what can metals below copper in the reactivity series be extracted with?

A

heat alone

32
Q

what can be reduced to their metal by heating with carbon or carbon monoxide?

A

oxides of metals above mercury and below aluminium in the reactivity series

33
Q

what does a metal oxide + carbon create?

A

metal oxide + carbon –> metal + carbon dioxide

34
Q

what does a metal oxide + carbon monoxide create?

A

metal oxide + carbon monoxide –> metal + carbon dioxide

35
Q

why do metal oxide + carbon(monoxide) take place?

A

because the carbon bonds more strongly with the oxygen than the metal does

36
Q

why does heating with carbon not work for oxides of metals above zinc?

A

because the metal bonds more strongly with the oxygen than the carbon does

37
Q

how are all metals above zinc in the reactivity series obtained?

A

by the electrolysis of molten compounds using a direct current

38
Q

what happens when metal compounds are in the molten state?

A

the ionic lattice breaks and the ions are free to move around.

39
Q

how are metals formed from electrolysis?

A

the positive metal ions are attracted to the negative electrode, where they gain electrons and form metal atoms

40
Q

what do ions flow through?

A

solutions

41
Q

what do electrons flow through?

A

metal wires

42
Q

what do electrochemical cells convert chemical energy into?

A

electrical energy

43
Q

what do electrochemical cells contain?

A

they contain one substance which gives up electrons and another substance that takes in electrons

44
Q

what does a cell consist of?

A

-two different metals
-an electrolyte to complete the circuit

45
Q

what is an electrolyte?

A

a substance which completes the circuit by allowing ions to flow through it

46
Q

how can metals be sorted?

A

they can be sorted accorded to their voltage in a league table - the ECS

47
Q

what is the ECS?

A

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

48
Q

the higher a metal is in the ECS….

A

the more readily it loses electrons

49
Q

what will electrons flow from in a cell?

A

the metal higher in the ECS to the metal lower down through the wires and meter

50
Q

the further apart the metals are in the ECS…

A

the larger the voltage produced

51
Q

What does a half cell consist of?

A

A metal in contact with a solution of it’s ions

52
Q

When can electricity be produced?

A

Only when half two cells are joined together

53
Q

How do ions move between half cells?

A

Using an ion bridge (salt bridge) which completes the curcuit

54
Q

When can non-metals be used in half-cells?

A

If a graphite rod is used to make electrical contact with the solution

55
Q

What will the ion higher in the ECS do?

A

Give away electrons

56
Q

What will the ion lower in the ECS do?

A

Will gain the electrons given out by the ion higher in the ECS

57
Q

What does a redox reaction produce?

A

An electric current

NAT5 Chemistry (11 decks)

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