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Chemistry > Unit 4 - Chemical Changes > Flashcards

Unit 4 - Chemical Changes Flashcards

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1
Q

What is oxidation/reduction?

A

Oxidation - When a substance gains oxygen
Reducation - When a substance loses oxygen

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2
Q

What is the reactivity series of metals? What are the trends in
reactivities of metals in reactions with acids/water?

A

The series shows the metals in order of their reactivity.
Metals above H2 in reactivity series react with acid to produce H2. The more
reactive the metal is, the quicker and more violent reaction with acid occurs.
Metals below H2 don’t react with acids.
Not all metals above H2 react with water - mostly Group I and II metals. Aluminium
is the borderline case.

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3
Q

How are unreactive metals found in Earth?

A

In their natural state (well, they are unreactive…)

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4
Q

What is a displacement reaction?

A

A reaction where a more reactive metal displaces a less reactive metal from a
compound

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5
Q

How can metals less reactive than carbon be extracted?

A

Reduction with carbon. Carbon displaces the metal in a metal oxide - gets
oxidised to carbon oxides. Metal from the metal oxide gets reduced to the pure
metal.

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6
Q

How are metals more reactive than carbon extracted?

A

By electrolysis

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7
Q

How are oxidation and reduction defined in terms of electron
transfer?

A

Oxidation – loss of electrons
Reduction – gain of electrons

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8
Q

What is the general equation for a reaction between metals
and acids? What type of reaction is this?

A

Metal + acid → salt + hydrogen
Redox reaction, also a displacement reaction

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9
Q

Which metals in the reactivity series will react with acid?

A

Those above hydrogen

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10
Q

What is the general equation for a neutralisation reaction?

A

Base + acid → salt + water

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11
Q

What is the general equation for the reaction between metal
carbonate and acid?

A

Metal carbonate + acid → salt + water + carbon dioxide

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12
Q

What is the general equation for the reaction between metal oxides
and acids?

A

Metal oxide + acid → a salt + water

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13
Q

What is a redox reaction?

A

A reaction where both oxidation and reduction occurs

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14
Q

Explain in terms of gain or loss of electrons which species
has been oxidised and which species has been reduced
when magnesium reacts with hydrochloric acid

A

Magnesium has lost electrons and thus has been oxidised (Mg to Mg2+)
The hydrogen in HCl has gained electrons and thus has been reduced (H+ to H2)

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15
Q

How is a soluble salt formed?

A

a) React the excess acid with some insoluble chemical (e.g. metal oxide)
b) Filter off the leftovers
c) Crystallise the product

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16
Q

What do acids and alkalis produce in aqueous solutions?

A

Acids produce hydrogen ions, alkalis produce hydroxide ions

17
Q

What are bases, acids and alkalis?

A

Bases are compounds that neutralise acids, acids produce hydrogen ions in
aqueous solutions, alkalis are soluble bases - produce hydroxide ions in aqueous
solutions

18
Q

What is the pH scale and what does a pH of 7 show?

A

The measure of acidity/alkalinity of a solution; neutral solution

19
Q

State the general equation for a neutralisation
reaction in a short, ionic form.

A

H+ + OH− → H2O

20
Q

What is a strong acid and weak acid?

A

Strong acid is completely ionised in aqueous solution; weak acid is only partially
ionised in aqueous solution

21
Q

What happens to pH as concentration of H+ increases?

A

The pH decreases

22
Q

What is a concentrated acid and what is a diluted acid? Is this the same
as a strong and weak acid?

A
  • Concentrated acid has more moles of acid per unit volume than dilute (dilute
    refers to solutions of low concentrations)
  • It is not the same - concentration is not the same thing as strength of an acid.
  • Strength refers to whether the acid is completely ionised in water (strong) or
    only partially (weak).
23
Q

As the pH is decreased by one unit, what change is seen in the
hydrogen ion concentration?

A

Increases by a factor of 10

24
Q

Name the following salts: LiNO3, K2CO3, MgBr2,
BaSO4

A

Lithium nitrate
Potassium carbonate
Magnesium bromide
Barium sulfate

25
Q

What is electrolysis?

A

The passing of an electric current through ionic substances that are molten or in
solution to break them down into elements; ions are discharged (they lose/gain
electrons) at electrodes to produce these

26
Q

What is an electrolyte?

A

The liquid/solution which conducts electricity

27
Q

What is a cathode and what is an anode?

A

Cathode is the negative electrode, anode is the positive electrode

28
Q

What occurs at the cathode and what occurs at the anode during
electrolysis?

A

Reduction occurs at the cathode
Oxidation occurs at the anode

29
Q

In aqueous electrolysis, which element is
discharged at the cathode? Oxygen is produced
at the anode unless what?

A

The less reactive element discharges at the cathode. Hydrogen is produced unless
there is a less reactive metal, in which case the said metal is produced. Oxygen is
produced at the anode unless the solution contains halide ions, in which case
halogen molecules are produced.

30
Q

How is aluminium manufactured? Why is it expensive?

A

Aluminium is made through the electrolysis of aluminium oxide and cryolite.
Lots of energy is needed to produce the current in electrolysis which makes this
process expensive.

31
Q

What are the half equations in the extraction of aluminium?

A

Al3+ + 3 e− → Al (cathode)
2 O2− → O2 + 4 e− (anode)
Oxygen reacts with C of the anode producing CO2.

32
Q

Why is cryolite used in manufacturing of aluminium?

A

It lowers the melting point of aluminium oxide, reducing energy costs

33
Q

What are the half equations in electrolysis of the
aqueous Na2SO4?

A

2 H+ + 2 e− → H2 (cathode)
4 OH− → 2 H2O + O2 + 4 e− (anode)

34
Q

What are the half equations in electrolysis of the
molten and aqueous KCl?

A

K+ + e− → K (cathode)
2 Cl− → Cl2 + 2 e− (anode)
2 H+ + 2 e− → H2 (cathode)
2 Cl− → Cl2 + 2 e− (anode), respectively

35
Q

What are the half equations in electrolysis of the
aqueous CuBr2?

A

Cu2+ + 2 e− → Cu (cathode)
2 Br− → Br2 + 2 e− (anode)

36
Q

What are the half equations in the extraction of aluminium?

A

It lowers the melting point of aluminium oxide, reducing energy costs

Chemistry (10 decks)

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