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Chemistry Flashcards - OCR 21st Century > C3 - Chemicals of the Natural Environment > Flashcards

C3 - Chemicals of the Natural Environment Flashcards

1
Q

Describe the chemical bonds found in

metals

A

Describe the chemical bonds found in metals

  • Metallic bonding.
  • Many positive metal ions fixed in a giant regular
    structure surrounded by a sea of delocalised
    negative electron.
  • There is strong electrostatic attraction between
    opposite charges.
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2
Q

What are the general properties of

metals?

A

What are the general properties of metals?

  • High melting points
  • Solid at room temperature
  • Strong and hard
  • Malleable (can be pressed into shape)
  • Ductile (can be drawn into wires)
  • Good electrical and thermal conductors
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3
Q

Why do metals have high melting points?

A

Why do metals have high melting points?

Lots of energy is required to overcome
the many strong metallic bonds.

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4
Q

Why are metals hard?

A

Why are metals hard?

Very strong metallic bonds hold the giant
structure together.

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5
Q

Why are metals malleable and ductile?

A

Why are metals malleable and ductile?

Metals are made up of uniform layers of
atoms which can easily slide over one
another. So the shape of the metal can
be easily changed.

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6
Q

Why are metals good conductors?

A

Why are metals good conductors?

The delocalised electrons are free to
move to carry charge.

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7
Q

Write the general equation for the

reaction of metals with water

A

Write the general equation for the reaction of metals
with water

metal + water → metal hydroxide + hydrogen

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8
Q

Write the general equation for the

reaction of metals with dilute acid

A

Write the general equation for the reaction of metals
with dilute acid

metal + acid → salt + hydrogen

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9
Q

What is a displacement reaction in terms

of metals?

A

What is a displacement reaction in terms of metals
?
A reaction in which a more reactive metal
displaces (replaces) a less reactive
metal from a compound.

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10
Q

How can the order of the reactivity of
metals be deduced from the results of an
experiment?

A

How can the order of the reactivity of metals be
deduced from the results of an experiment?

More reactive metals can displace less
reactive metals from their compounds in a
displacement reaction. A series of
displacement reactions can be carried out to
compare the reactivities of metals.

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11
Q

What is meant by the reactivity of

metals?

A

What is meant by the reactivity of metals?

The tendency of a metal atom to lose
electrons and form its positive ion.

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12
Q

Which metal in the reactivity series

reacts with water most vigorously?

A

Which metal in the reactivity series reacts with water
most vigorously?

Potassium

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13
Q

Reactivity series

A 
Potassium              MOST REACTIVE
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Lead
(Hydrogen)
Copper
Silver                     LEAST REACTIVE
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14
Q

Using the reactivity series, which elements don’t

react with acids?

A

Which elements don’t react with acids?

Copper and silver because they are below hydrogen in
the reactivity series so are less reactive than hydrogen.

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15
Q

What is the principle of conservation of

mass?

A

What is the principle of conservation of mass?

A closed system has a constant mass
during a reaction, no matter is gained or
lost, so the mass of reactants is equal to
the mass of products.

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16
Q

Write a balanced symbol equation for the
displacement reaction between calcium
and copper(II) sulphate

A

Write a balanced symbol equation for the
displacement reaction between calcium and copper(II) sulphate

Ca(s) + CuSO4(aq)→ CaSO4(aq) +Cu(s)

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17
Q

Write the ionic equation for the reaction

between sodium and iron(II) carbonate

A

Write the ionic equation for the reaction between
sodium and iron(II) carbonate
2Na(s) + Fe2+(aq) → 2Na+(aq) + Fe(s)

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18
Q

What is an ore?

A

What is an ore?

A rock that contains a mineral that can
be extracted.

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19
Q

Which metals can be extracted from their

ores by heating with carbon?

A

Which metals can be extracted from their ores by
heating with carbon?

Metals which are below carbon in the reactivity series,
such as zinc

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20
Q

Describe how zinc can be extracted from

its ore

A

Describe how zinc can be extracted from its ore

Heat zinc oxide with carbon to reduce it
and form zinc. Carbon is the reducing
agent and is oxidised. Carbon displaces
zinc from its oxide.

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21
Q

Write a word and symbol equation for the

reduction of zinc oxide with carbon

A

Write a word and symbol equation for the reduction
of zinc oxide with carbon

zinc oxide + carbon → zinc + carbon monoxide
ZnO(s) + C(s) → Zn(l) + CO(g)

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22
Q

Why must electrolysis be used to extract

some metals from their ores?

A

Why must electrolysis be used to extract some
metals from their ores?

Metals above carbon in the reactivity series are more reactive than carbon so they will not be displaced from their ores by carbon.

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23
Q

Why is electrolysis not used to extract

zinc from its ore?

A

Why is electrolysis not used to extract zinc from its
ore?

  • Zinc is less reactive than carbon so can
    be extracted by heating with carbon.
  • Electrolysis is expensive and requires a
    lot of energy.
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24
Q

How can plants be used as an

alternative metal extraction method?

A

How can plants be used as an alternative metal
extraction method?

Phytoextraction:
Plants are grown in areas with metals in the soil. The
plants take up metals through their roots and
concentrate them in their shoots and leaves. These
plants are burned and the metals are removed from the
ash.

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25
How can bacteria be used as an | alternative metal extraction method?
How can bacteria be used as an alternative metal extraction method? Bacterial extraction: Some bacteria absorb metal compounds. These bacteria produce solutions called leachates containing the metals. Scrap iron can be used to remove the metal from the leachate.
26
What are the limitations of biological | methods of extraction?
What are the limitations of biological methods of extraction? - Produces smaller quantities of metals. - Slow processes. - Require displacement or electrolysis for the final step. - Bacteria require acidic conditions and may introduce toxic substances to the environment.
27
When do ionic compounds conduct | electricity? Why?
When do ionic compounds conduct electricity? Why? When molten or aqueous (dissolved in water) because the ions are free to move. When solid, the ions are fixed in the lattice so they can’t move to carry a charge.
28
What is an electrolyte?
What is an electrolyte? A molten or aqueous ionic compound that conducts electricity.
29
What is electrolysis and what can it be | used for?
What is electrolysis and what can it be used for? Electrolysis is the decomposition of an electrolyte using an electric current. It can be used to extract metals from their ores.
30
When using inert electrodes, what | happens at the cathode?
When using inert electrodes, what happens at the cathode? Cations (positive ions) move towards the cathode (negative electrode). Positive metal ions gain electrons to form metal atoms. If the metal is more reactive than hydrogen, hydrogen will form at the cathode instead and the metal will remain in the electrolyte.
31
When using inert electrodes, what | happens at the anode?
When using inert electrodes, what happens at the anode? Anions (negative ions) move towards the anode (positive electrode). Negative non-metal ions lose electrons to form non-metal atoms.
32
Predict what will form when molten | lead(II) bromide is electrolysed
Predict what will form when molten lead(II) bromide is electrolysed Lead atoms (Pb) at cathode. Bromine molecules (Br2) at anode.
33
Write half equations for the reactions that take place when calcium chloride undergoes electrolysis
Write half equations for the reactions that take place at each electrode when calcium chloride undergoes electrolysis Cathode: Ca2+ + 2e- → Ca Anode: 2Cl- → Cl2 + 2e-
34
Describe oxidation and reduction in | terms of electrons
``` Describe oxidation and reduction in terms of electrons Oxidation is loss of electrons. Reduction is gain of electrons. OILRIG ```
35
How can electrolysis be used to extract | aluminium from its ore bauxite?
How can electrolysis be used to extract aluminium from its ore bauxite? - Purified to form aluminium oxide. - Dissolved in molten cryolite. - Insert inert electrodes and connect to power supply. - Aluminium ions gain electrons at cathode to produce pure aluminium and oxide ions lose electrons to form oxygen at anode.
36
Why is aluminium oxide dissolved in | cryolite during electrolysis?
Why is aluminium oxide dissolved in cryolite during electrolysis? - Cryolite has a lower melting point than aluminium oxide. - Aluminium oxide is insoluble in water. - Reduces energy use and cost.
37
Why must the inert graphite electrodes be replaced regularly when aluminium is being extracted from its ore?
Why must the inert graphite electrodes be replaced regularly when aluminium is being extracted from its ore? The oxygen produced at the anode reacts with carbon in the electrode forming carbon dioxide meaning carbon is lost from the anode.
38
When would oxygen not be produced at the anode during the electrolysis of an aqueous ionic compound? What would form instead?
When would oxygen not be produced at the anode during the electrolysis of an aqueous ionic compound? What would form instead? When halide ions are present (chloride, bromide or iodide ions). A halogen would form (chlorine, bromine or iodine).
39
Write the balanced half equation for the formation of oxygen from hydroxide ions at the anode
Write the balanced half equation for the formation of oxygen from hydroxide ions at the anode 4OH- → 2H2O + O2+ 4e-
40
Describe how to carry out electrolysis on | an aqueous salt solution
Electrolysis on aq salt solution 1. Pour the salt solution into a beaker. 2. Insert 2 graphite electrodes and connect to a power supply. 3. Fill 2 test tubes with salt solution and place over the electrodes to collect any gas produced. 4. Turn on the power supply, ensuring the electrodes don’t touch. 5. Turn off power and test gases.
41
What is a hydrocarbon?
What is a hydrocarbon? A compound made up of only hydrogen and carbon atoms.
42
Crude oil is the main source of _________
Crude oil is the main source of hydrocarbons
43
What is crude oil a feedstock for?
What is crude oil a feedstock for? The petrochemical industry
44
Is crude oil finite or infinite?
Is crude oil finite or infinite? Finite
45
Why is modern life dependent on | hydrocarbons?
Why is modern life dependent on hydrocarbons? Hydrocarbons are a source of fuel which is relied on heavily for modern life.
46
What is a homologous series?
What is a homologous series? A series of organic molecules with the same general formula. Successive members in the series differ by -CH2. Molecules in a homologous series have similar chemical properties because they have the same general formula.
47
What is the general formula for the | alkane homologous series?
What is the general formula for the alkane homologous series? CnH2n+2
48
What is a fraction of crude oil?
What is a fraction of crude oil? A mixture of similar-sized hydrocarbon molecules with similar boiling points. These compounds are generally members of the alkane homologous series and have the formula CnH2n+2.
49
Why can crude oil be separated by | fractional distillation?
Why can crude oil be separated by fractional distillation? Because the different hydrocarbons have different boiling points so condense at different temperatures.
50
Describe the fractional distillation of | crude oil
Describe the fractional distillation of crude oil - Crude oil is heated and evaporates. - Crude oil vapours enter and rise up a fractionating column which is hot at the bottom and cold at the top. - Vapours condense when the temperature is below its boiling point. - Separated liquids leave the column at different heights.
51
Do the longest hydrocarbons leave the fractionating column at the top or bottom?
Do the longest hydrocarbons leave the fractionating column at the top or bottom? Bottom
52
Which forces must be overcome for alkanes to turn from liquid to gas? What other bond is found in alkane molecules?
Intermolecular forces must be overcome for an alkane to evaporate. Covalent bonds are found between carbons and between carbon and hydrogen. These are not broken during boiling.
53
Why do different alkanes have different | boiling points?
Why do different alkanes have different boiling points? - Longer hydrocarbons have stronger intermolecular forces. - More energy is required to overcome the stronger forces. - Longer hydrocarbons have higher boiling points.
54
What is meant by the term empirical | formula?
What is meant by the term empirical formula? The simplest whole number ratio of atoms of each element in a compound.
55
What is the empirical formula of C4H10?
What is the empirical formula of C4H10? C2H5
56
What is a covalent bond?
What is a covalent bond? A bond formed from a shared pair of electrons between atoms.
57
What are the limitations of using dot and cross diagrams to represent covalent compounds?
What are the limitations of using dot and cross diagrams to represent covalent compounds? - Don’t show the 3D arrangement of atoms in space. - Doesn’t show the size of atoms relative to one another.
58
What are the limitations of using 3D | diagrams to represent covalent compounds?
``` What are the limitations of using 3D diagrams to represent covalent compounds? - They are not show to scale. - Don’t show how the bond formed. - Don’t show the shared pair of electrons. ```
59
Which is stronger: covalent bonds or | intermolecular forces?
Which is stronger: covalent bonds or intermolecular forces? Covalent bonds
60
Why do alkanes have low melting and | boiling points?
Why do alkanes have low melting and boiling points? During melting and boiling, intermolecular forces are overcome but covalent bonds aren’t broken. Intermolecular forces are relatively weak compared to covalent bonds so require little energy to overcome.
61
What is cracking?
What is cracking? Breaking long chain hydrocarbon molecules into smaller hydrocarbons.
62
What are the products of cracking?
What are the products of cracking? Alkanes and alkenes Alkenes are a different homologous series containing a carbon to carbon double bond.
63
Hexane is cracked to form butane and ethene. Write a word and symbol equation for this reaction.
Hexane is cracked to form butane and ethene. Write a word and symbol equation for this reaction. hexane → butane + ethene C6H14 → C4H10 + C2H4
64
Describe what happens during cracking
Describe what happens during cracking An alkane is heated. The vapours pass over a catalyst and the covalent bonds break and reform.
65
Why is cracking important?
Why is cracking important? - The shorter chained alkanes and alkenes are in higher demand than long chained alkanes. - Can match the supply of fractions with demand. Typically fractional distillation of crude oil produces too many long chain hydrocarbons. - Alkenes can be produced for use as a feedstock in the petrochemical industry.
66
Alkanes are saturated hydrocarbons. | Explain what this means
Alkanes are saturated hydrocarbons. Explain what this means Hydrocarbon - contains only hydrogen and carbon. Saturated - carbon atoms are all joined by single bonds.
67
What is an alkene? Include the general | formula and functional group
What is an alkene? Include the general formula and functional group An unsaturated hydrocarbon. General formula: CnH2n Functional group: C=C
68
Give examples of molecules that alkenes | react with in an addition reaction
Give examples of molecules that alkenes react with in an addition reaction React with water when heated with a catalyst to form alcohols. React with bromine to form bromoalkanes. React with other alkenes to form addition polymers.
69
What are the general formula and | functional group of an alcohol?
What are the general formula and functional group of an alcohol? (Chemistry only) General formula: CnH2n+1OH Functional group: OH
70
What are the common reactions of | alcohols?
What are the common reactions of alcohols? - Complete combustion, producing water and carbon dioxide. - Oxidation to produce carboxylic acids (needs an oxidation agent).
71
What are the general formula and | functional group of a carboxylic acid?
What are the general formula and functional group of a carboxylic acid? General formula: CnH2n+1COOH Functional group: COOH
72
What do carboxylic acids react with?
``` What do carboxylic acids react with? - Metals (forms salt and hydrogen). - Bases (forms salt and water). - Carbonates (forms salt, water and carbon dioxide). ```
73
Why do members of a homologous | series react similarly?
Why do members of a homologous series react similarly? Because they all contain the same functional groups.
74
Predict the formula of the products when | pentane is completely combusted
Predict the formula of the products when pentane is completely combusted H2O and CO2
75
Write a balanced symbol equation for the | incomplete combustion of ethane
Write a balanced symbol equation for the incomplete combustion of ethane C2H6 + 2O2 → 3H2O + C + CO C2H6 + 2½O2 → 3H2O + C + CO2 C2H6 + 2½O2 → 3H2O + 2CO Or any other balanced symbol equation where the products include H2O and C or CO. Products may also contain CO2 with C or CO.
76
Predict the formula of the product when | propene reacts with bromine
Predict the formula of the product when propene reacts with bromine C3H6Br2
77
Predict the formula of the products when | ethanol is oxidised
Predict the formula of the products when ethanol is oxidised Alcohols are oxidised to form carboxylic acids. Ethanoic acid: CH3COOH
78
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Chemistry Flashcards - OCR 21st Century (9 decks)

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