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Science Year 9 > Acid and Metal Reactions > Flashcards

Acid and Metal Reactions Flashcards

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1
Q

What is formed when a metal reacts with water?

A

Metal hydroxide+ Hydrogen.

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2
Q

What metals in the reactivity series do not react with dilute acids?

A

Metals below Hydrogen do not react with dilute acids.

Unreactive towards the hydrogen atoms in the solution.

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3
Q

What does a metal + dilute acid produce?

A

Metal+ Dilute acid - Salt + Hydrogen

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4
Q

What is oxidation?

A

Gain of oxygen, loss of electrons in a chemical reaction.

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5
Q

Give an example of an oxidation reaction?

A

Magnesium + oxygen - Magnesium oxide

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6
Q

Give an example of a reduction reaction?

A

Copper oxide+ carbon - copper + carbon dioxide.

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7
Q

If something has reduced, what ion will it produce?

A
  • Gain electrons.

- Form negative ion.

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8
Q

If something has oxidised, what ion will it produce?

A
  • Loss of electrons.

- Form positive ions.

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9
Q

What is a displacement reaction?

A

A displacement reaction is when a more reactive metal displaces a less reactive metal from its compounds.

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10
Q

Give an example of a displacement reaction?

A

Magnesium + copper sulphate - Magnesium sulphate + copper.

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11
Q

What happens when magnesium displaces copper sulphate solution?

A
  • The magnesium becomes coated with copper.

- Blue colour fades and colourless into colourless magnesium sulphate solution.

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12
Q

How can you deduce a reactivity series?

A
  • Metal dipped in salt solution to see displacement reaction.
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13
Q

What is a redox reaction?

A

A redox reaction is when oxidation and reduction happen at the same time.

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14
Q

How do you work out the formula of an ionic compound?

A
  • Make sure the charges are equal to 0.
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15
Q

What is the formula of Sulphuric acid?

A

H2SO4

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16
Q

What is the charge on a nitrate ion?

A

NO3 -

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17
Q

What is meant by pH?

A

The level of hydrogen ions in an acid.

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18
Q

What is the formula for ammonium?

A

NH4 (+)

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19
Q

What is the charge on a sulphate ion?

A

SO4 2-

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20
Q

What is the charge on a carbonate ion?

A

CO3 2-

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21
Q

What is the charge on a hydroxide ion?

A

OH-

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22
Q

Where are most metals extracted from?

A
  • Most metals are extracted from an ore.

- Ore: A rock that contains enough metal to make extracting it worthwhile.

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23
Q

How can a substance be extracted from its compounds by heating with carbon?

A
  • Any elements less reactive than carbon.
  • Heated with carbon.
    Eg. Copper oxide + Carbon —– Carbon dioxide + copper.
  • Molten copper is formed.
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24
Q

What does molten mean?

A

Molten is a term to describe a liquid substance.

25
Q

What is a mineral?

A

A mineral is a naturally occurring element or compound.

26
Q

What does malachite ore have in it?

A
  • Malachite ore has copper(II Carbonate) in it.
27
Q

What does cinnabar have in it?

A
  • Cinnabar ore has mercury(II sulphide) in it.
28
Q

What do most metals exist as?

A
  • Sulphides.
  • Oxides.
  • Carbonates.
29
Q

What does limestone have in it?

A
  • Calcium carbonate.
30
Q

What does hematite contain?

A
  • Iron (III) Oxide.
31
Q

What are electrolytes?

A
  • Electrolytes are substances, when melted/ dissolved, will conduct an electric current.
32
Q

Why is aluminium oxide mixed with cryolite before the electrolysis process?

A
  • It lowers the melting point so less energy is needed.

- Reduced energy, saves money.

33
Q

What is the positive electrode in electrolysis?

A
  • The positive electrode in electrolysis is the graphite anode.
  • This attracts the negative ions (eg. O2-, from aluminium oxide.)
34
Q

What is the negative electrode in electrolysis?

A
  • The negative electrode in electrolysis is the graphite cathode.
  • This attracts positive ions eg. (Al 3+, from aluminium oxide.)
35
Q

What is electrolysis?

A
  • Electrolysis is the decomposition of a compound using an electric current.
  • Large amounts of it can be expensive.
36
Q

Why are the cathodes and anodes made of graphite?

A
  • It can conduct electricity.

- High melting points (withstand high temperatures.)

37
Q

Explain, with the half equation, how oxide ions are oxidised during the electrolysis of aluminium oxide?

A

The half equation is: 2O2- → O2 + 4e-. It shows that oxide ions lose electrons, and oxidation is loss of electrons.

38
Q

Explain, with the help of a half equation, how aluminium ions are reduced during the electrolysis of aluminium oxide?

A

The half equation is: Al3+ + 3e- → Al

It shows that aluminium ions gain electrons, and reduction is gain of electrons.

39
Q

Why do you need to double the oxygen half equation?

A
  • The oxygen atoms pair up to make an oxygen molecule at the anode.
40
Q

How do you test for hydrogen?

A
  • Light a split, put it in a sample of wherever hydrogen is present.
  • A squeaky pop noise means hydrogen is present.
  • If not, there will be no change.
41
Q

What is a base?

A
  • A base is a substance that reacts with an acid to form salt and water.
42
Q

What types of bases are also alkali?

A
  • Bases that are soluble in water.
43
Q

Give the neutralisation reaction.

A
  • Acid +base — Salt +water
44
Q

Explain why all alkalis are bases, but not all bases are alkali.

A
  • Only bases that are soluble (dissolve in water) are alkali.
  • All alkalis are bases
45
Q

What is produced when an acid reacts with a carbonate?

A

Acid + carbonate — salt + water + carbon dioxide

46
Q

How can you make a soluble salt?

A
  • You can make a soluble salt by having an insoluble reactant react with an acid.
47
Q

Give examples of insoluble reactants that produce salt.

A
  • Metal
  • Metal oxide
  • Metal hydroxides
  • Carbonates
48
Q

What is the method of producing a soluble salt from an insoluble reactant?

A
  • Add powdered insoluble reactant to a beaker with acid. Keep adding until it is in excess. All the acid mixed with reactant.
  • Filter the mixture in the beaker to get rid of any solid. Now should be salt+ water only.
  • Heat the solution in an evaporating basin over a water bath. Stop heating when it is halfway. Small crystals should form. It is now saturated.
  • Pour the rest of the solution in a watch glass
  • Leave the saturated solution for two days to allow crystals to form.
49
Q

What does saturated mean?

A
  • Saturated means unable to have any liquid.
50
Q

What is an endothermic reaction?

A
  • One that takes in energy from its surroundings.
  • The energy of surroundings decrease.
  • Feels cold
  • Energy of products is more than energy of reactants.
51
Q

What is an exothermic reaction?

A
  • One that releases energy into its environment.
  • The temperature of the surrounding increase.
  • Energy of reactants more than products.
  • Feel hot.
52
Q

What is an energy level diagram?

A
  • The energy level diagram shows the energy of reactants and products, and the difference between them.
53
Q

What are the metals in the reactivity series?

A

Lithium, Potassium, Barium, Calcium, Sodium, Magnesium, Aluminium, CARBON, Zinc, Iron, Nickel, Tin, Lead, HYDROGEN, Copper, Mercury, Silver, Gold, Platinum.

54
Q

What is meant by “concentration?”

A
  • Concentration is the mass per unit volume.
55
Q

What happens if the pH of a solution decreases by 1 unit?

A
  • If the pH of a solution decreases by 1 unit it means that the concentration of ions increases by a factor of 10. Eg. x100 x 1000
56
Q

Why does copper not react with sulphuric acid?

A
  • Copper is lower than HYDROGEN in the reactivity series.

- It will be unable to displace the HYDROGEN in a reaction.

57
Q

What is a salt?

A
  • A salt is the substance formed when the hydrogen ion in an acid is replaced by a metal ion.
58
Q

When can you measure the pH of a substance?

A
  • You can measure pH when the substance is dissolved in water.

Science Year 9 (25 decks)

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