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Nat 5 Chemistry > Unit 3 - Chemistry in Society > Flashcards

Unit 3 - Chemistry in Society Flashcards

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1
Q

What are properties of metals?

A
  • They are very strong and this is why they are used in construction.
  • They are very malleable - they can be hammered or rolled into flat sheets.
  • They are very ductile - they can be stretched into thin wires.
  • They are very good at conducting heat - they allow heat to pass through them.
  • They are very good at conducting electricity - allow a charge to flow through it.

They have a high density

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2
Q

What is the structure of metallic bonding?

A

positive nuclei of metal atoms are structured with a sea of delocalised electrons surrounding them.

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3
Q

What is metallic bonding?

A

The electrostatic force of attraction between positively charged ions/atoms and delocalised negative outer electrons.

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4
Q

What are melting an boiling points like in metallic bonding?

A

Very high due to the strong attraction.

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5
Q

Why are metallic elements conductors of electricity?

A

Metallic elements are conductors of electricity because they contain delocalised electrons.

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6
Q

How does metallic elements conduct electricity?

A

If an electron is inserted into the metal, another electron is ejected at the other end.This means that charge can flow and they conduct electricity.

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7
Q

What does a reaction between a metal and oxygen produce?

A

A metal oxide

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8
Q

What does a reaction between a metal and water produce?

A

A metal hydroxide

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9
Q

What does a reaction between a metal and an acid produce?

A

A salt + hydrogen

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10
Q

What metals from the electrochemical series react with water?

A

Lithium (Li), Potassium (K), Calcium (Ca), Sodium (Na), Magnesium (Mg).
ANY ELEMENT ABOVE ALUMINIUM ON THE ELECTROCHEMICAL SERIES DOES!!!!

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11
Q

What metals from the electrochemical series do not react with water?

A

Aluminium (Al), Zinc (Zn), Iron (Fe), Nickel (Nl), Tin (Sn), Lead (Pb), Copper (Cu), Silver (Ag), Mercury (Hg), Gold (Au).
ANY ELEMENT BELOW MAGNESIUM ON THE ELECTROCHEMICAL SERIES DOES NOT!!!!

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12
Q

What metals from the electrochemical series react with acid?

A

Lithium (Li), Potassium (K), Calcium (Ca), Sodium (Na), Magnesium (Mg), Aluminium (Al), Zinc (Zn), Iron (Fe), Nickel (Nl), Tin (Sn), Lead (Pb).
ANY ELEMENT ABOVE COPPER ON THE ELECTROCHEMICAL SERIES.

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13
Q

What metals from the electrochemical series do not react with acid?

A

Copper (Cu), Silver (Ag), Mercury (Hg), Gold (Au).

ANY ELEMENT BELOW LEAD ON THE ELECTROCHEMICAL SERIES.

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14
Q

What metals from the electrochemical series do react with oxygen?

A

Lithium (Li), Potassium (K), Calcium (Ca), Sodium (Na), Magnesium (Mg), Aluminium (Al), Zinc (Zn), Iron (Fe), Nickel (Nl), Tin (Sn), Lead (Pb), Copper (Cu).
ANY ELEMENT ABOVE SILVER ON THE ELECTROCHEMICAL SERIES.

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15
Q

What metals from the electrochemical series do not react with oxygen?

A

Silver (Ag), Mercury (Hg), Gold (Au).

ANY ELEMENT BELOW COPPER ON THE ELECTROCHEMICAL SERIES.

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16
Q

How does metal extraction work and why is there multiple methods to extract the metal?

A

During the extraction of metals, metal ions are reduced forming metal atoms. The method used to extract a metal from its ore depends on the position of the metal in the reactivity series. (Different methods are required, depending on how reactive the metal is).

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17
Q

What metals are found uncombined in the earth?

A

Silver (Ag), Gold (Au).

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18
Q

What metals require heat alone to extract them from their ores?

A

Silver (Ag), Gold (Au), Mercury (Hg).

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19
Q

What is the overall reaction for the extraction of metals using heat?

A

Heat

Metal oxide —-> Metal + Oxygen

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20
Q

What metals require heating with carbon/carbon monoxide to extract them from their ores?

A

Zinc (Zn), Iron (Fe), Tin (Sn), Lead (Pb), Copper (Cu).

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21
Q

What is the overall reaction of heating a metal with carbon?

A

Metal Oxide Metal
+ —-> +
Carbon Carbon dioxide

Carbon when heated will combine with oxygen from the air to form carbon dioxide. The carbon dioxide then decomposes to carbon monoxide which reacts with ore to form carbon dioxide.

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22
Q

What metals require electrolysis to extract them from their ores?

A

Lithium (Li), Potassium (K), Calcium (Ca), Sodium (Na), Magnesium (Mg), Aluminium (Al). Most metals ending in ium.

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23
Q

What is a reduction reaction?

A

A gain of electrons by a reactant in any reaction

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24
Q

What is an oxidation reaction?

A

A loss of electrons by a reactant in any reaction.

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25
Q

What happens in a REDOX reaction?

A

Reduction and oxidation take place at the same time.

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26
Q

Why Why do most metals that end in ium require electrolysis to extract hem from their ore?

A

These metals are very reactive and form metal oxides with very strong bonds that require more energy to break them down.

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27
Q

What happens during the extraction of metals?

A

During the extraction of metals, metal ions are reduced forming metal atoms

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28
Q

What is electrolysis?

A

The decomposition of an ionic compound into its elements using electricity.

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29
Q

What must be used if the products of electrolysis are to be identified?

A

A D.C supply.

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30
Q

What happens during electrolysis?

A

Positive ions gain electrons at the negative electrode and negative ions lose electrons at the positive electrode.

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31
Q

What is an electrolyte?

A

An electrically conducting solutions containing ions.

32
Q

What do metals at the top of the ECS want to be more than the other metals?

A

An ion.

33
Q

How does a displacement reaction occur?

A

A metal displacement reaction occurs when a metal high up in the electrochemical series displaces a metal in solution which is lower than itself.

34
Q

What are the two types of electrochemical cells?

A

Simple cell and half cell.

35
Q

How can a simple cell be made?

A

A simple cell can be made by placing two metals in an electrolyte.

36
Q

How do simple cells work?

A

Simple cells work because there is one metal higher up in the electrochemical series and will lose its electrons and push them round the circuit to the other metal.

37
Q

What is more efficient: a simple cell and a half cell?

A

A half cell,

38
Q

How is a half cell made?

A

By placing 2 metals in a solution of their own ions and connecting them with an ion bridge?

39
Q

What is an ion bridge and what does it do?

A

A length of filter paper soaked in a salt solution. It is used to link the half-cells as ions can move across the
bridge to complete an electrical circuit.

40
Q

What is the direction of electron flow in a half cell?

A

From the higher metal to the lower metal in the electrochemical series.

41
Q

What happens if the ion bridge is removed from a half-cell?

A

The circuit is broken and no electricity is made.

42
Q

When will a half-cell stop producing energy?

A

When there is no chemicals left/the metal higher up has more or less disintegrated/disappeared.

43
Q

How can the voltage produced in half-cells and simple cells be increased?

A

By increasing the distance between the two metals in the ECS.

44
Q

What is the electrode used for half-cells with non-metals?

A

Graphite/carbon rods.

45
Q

What are the five steps to working out the half-cell equation for non-metals?

A

1) Identify the ions present
2) Work out what is producing the electrons - If ions are positive they have already lost electrons so can’t lose any more (will normally be the metals). The negative electrons have excess electrons so are more likely to lose them (these are normally non-metals), figure out what one is higher up in the electrochemical series ant this should be the ion producing the electrons.
3) Work out where the electrons are going - Electrons must flow through the wire to the other half cell. In the other half cell the positive ion will be picking up the electrons.
4) Write the ion-electron equations for the half-cell - The oxidation of the negative ion producing the electrons and the reduction of the positive ion that is picking up the electrons.
5) Combine the ion-electron equation into a REDOX reaction - THIS IS OPTIONAL/MAY NOT ASK YOU TO DO.

46
Q

What are plastics an example of?

A

Materials known as polymers.

47
Q

What are polymers?

A

Polymers are long chain molecules formed by joining together a large number of small molecules called monomers.

48
Q

What is addition polymerisation?

A

Addition polymerisation is the name given to a chemical reaction in which unsaturated monomers (like alkenes ) are joined, forming a polymer by breaking down the double bond.

49
Q

What is the difference between a monomer and a repeating unit?

A

The monomer is the alkene before the double bond is broken. The repeating unit is when the double bond is broken down and thew dash of the bond goes through the bracket.

50
Q

How do you name a polymer?

A

Put the name of the monomer in brackets and put poly in front of the bracket. E.g. poly(…..)

51
Q

What are the 3 nutrients plants need?

A

Nitrogen, phosphorus, potassium.

52
Q

What are fertilisers?

A

Fertilisers are substances which restore elements, essential for healthy plant growth, to the soil.

53
Q

What are important compounds used to produce soluble, nitrogen containing salts that can be used as fertilisers?

A

Ammonia and nitric acid.

54
Q

What is ammonia?

A

Ammonia is a pungent, clear, colourless gas which dissolves in water to produce an alkaline solution.

55
Q

What is produced when ammonium reacts with an acid?

A

Soluble salts

Ammonium solution An ammonium salt
+ —-> +
An acid water

56
Q

What is the Haber process used to produce?

A

Ammonia required for fertiliser production.

57
Q

What is the overall reaction of the Haber process?

A

N2(g) + 3H2 (g) 2NH3 (g)

58
Q

What is the catalyst in the Haber process?

A

Iron

59
Q

Is the Harper process more efficient at higher temperatures?

A

No it is more efficient at lower temperatures.

60
Q

Is the Harper process more efficient at a higher pressure?

A

Yes the Haber process is more efficient at a high pressure.

61
Q

What doe the Ostwald process do?

A

Uses ammonia, oxygen and water to produce nitric acid.

62
Q

What doe the Haber process use to produce the Ammonia?

A

Nitrogen from the air and hydrogen from methane.

63
Q

What is the catalyst in the Ostwald process?

A

Platinum

64
Q

What dopes the Ostwald process use to produce the nitric acid at the start of the process?

A

Air and ammonia

65
Q

What is added during the Ostwald process?

A

Oxygen and water

66
Q

what does radioactive decay involve?

A

Changes in the nuclei of atoms. Unstable nuclei (radioisotopes) can become more stable nuclei by giving out alpha, beta or gamma radiation which changes the proton/neutron ratio.

67
Q

What is half-life?

A

Half-life is the time for half of the nuclei of a particular isotope to decay.

68
Q

Can the half-life of an isotope be changed?

A

NO!!!!

69
Q

What can flame tests identify?

A

The metals present in a sample.

70
Q

What is the test for Hydrogen?

A

Burns with a squeaky pop

71
Q

What is the test for Oxygen?

A

Relights a glowing splint

72
Q

What is the test for Carbon dioxide?

A

Turns lime water cloudy

73
Q

What is a precipitation reaction?

A

The reaction of two solutions to form an insoluble salt called a precipitate.

74
Q

How can you identify a precipitate?

A

The products will be insoluble

75
Q

What is a solution of accurately known concentration more commonly known as?

A

A standard solution

Nat 5 Chemistry (3 decks)

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