Reactivity of metals

This question is about copper and copper compounds.

A teacher demonstrated the reaction of copper with silver nitrate.

Figure 16 shows the apparatus:

at the start

after a few minutes.

The word equation for the reaction is:

solution solution

What type of reaction happens between copper and silver nitrate?

Tick () one box.

Combustion

Displacement

Neutralisation

Give two observations that can be made when copper reacts with silver nitrate solution.

Use Figure 16 and the word equation.

Copper reacted with silver nitrate solution.

The teacher then added copper to nickel nitrate solution.

Copper did not react with nickel nitrate solution.

Write the order of reactivity for copper, nickel and silver.

A student reacted solid copper oxide with nitric acid to produce a solution of copper nitrate.

This is the method used.

1. Add 25 cm³ of nitric acid to a beaker.

2. Warm the nitric acid.

3. Add solid copper oxide to the nitric acid.

4. Stir the mixture.

5. Repeat steps 3 and 4 until solid copper oxide is in excess.

Give one safety precaution the student should use.

The nitric acid was warmed in step 2 of the method.

Suggest how the reaction was affected by warming the nitric acid.

After the reaction finished, the beaker contained a mixture of solid copper oxide and copper nitrate solution.

Describe a method to obtain pure, dry copper nitrate crystals from the mixture.

This question is about metals and metal compounds.

A teacher demonstrated the reaction of copper with silver nitrate.

Figure 6 shows the apparatus:

at the start

after a few minutes.

The word equation for the reaction is:

copper + silver nitrate copper nitrate + silver

Silver ions are reduced to silver atoms in the reaction.

What is meant by ‘reduced’ in this reaction?

Complete the ionic equation for the reaction between copper and silver nitrate solution.

You should balance the equation.

Copper nitrate is made up of Cu²⁺ ions and NO₃⁻ ions.

What is the formula of copper nitrate?

Tick () one box.

CuNO₃

Cu(NO₃)₂

Cu₂NO₃

Cu₂(NO₃)₃

Figure 7 shows the order of reactivity for three metals.

Table 2 shows the colours of three metal nitrate solutions.

The teacher added an excess of each metal to each metal nitrate solution.

Complete Table 3 to show the colours of the resultant solutions.

Copper is a good conductor of electricity.

Explain how copper conducts electricity.

Pure copper is too soft for many uses.

Copper is mixed with other metals to make copper alloys.

Explain why copper alloys are harder than pure copper.

A student investigated the reactivity of four metals with sulfuric acid.

Figure 13 shows the apparatus.

Give two variables the student should control.

Write the order of reactivity from least reactive to most reactive for the four metals.

Use Figure 13.

The gas produced in Figure 13 is hydrogen.

Describe the test for hydrogen gas.

Give the result if hydrogen is present.

The student repeated the investigation using different apparatus to determine the rate of reaction.

Figure 14 shows part of the apparatus.

Complete Figure 14 so that the apparatus can be used to determine the rate of reaction.

Give two measurements the student should make to determine the rate of reaction.

What is the unit for the rate of reaction determined using the apparatus in Figure 14

A student investigated the reactivity of four metals with sulfuric acid.

Figure 5 shows the apparatus.

Give two variables the student should control.

Write the order of reactivity from least reactive to most reactive for the four metals.

Use Figure 5.

The gas produced in Figure 5 is hydrogen.

Describe the test for hydrogen gas.

Give the result if hydrogen is present.

The student repeated the investigation using different apparatus to determine the rate of reaction.

Figure 6 shows part of the apparatus.

Complete Figure 6 so that the apparatus can be used to determine the rate of reaction.

Give two measurements the student should make to determine the rate of reaction.

What is the unit for the rate of reaction determined using the apparatus in Figure 6?

This question is about reactions of metals.

A student investigated the reactivity of three metals.

Figure 1 shows the order of reactivity of the three metals.

The student added each metal to three different metal sulfate solutions.

Table 1 shows some of the results.

A more reactive metal displaces a less reactive metal from a compound.

Complete Table 1.

Use: where a reaction occurs where there is no reaction.

Use Figure 1.

What type of solution is formed when potassium reacts with water?

Tick (✓) one box.

Acidic

Alkaline

Neutral

Which gas is produced when potassium reacts with water?

Tick (✓) one box.

Carbon dioxide

Hydrogen

Oxygen

Give one observation seen when potassium is added to water.

Sodium is above potassium in Group 1 of the periodic table.

How does the reactivity of sodium compare with the reactivity of potassium?

Tick (✓) one box.

Sodium is less reactive than potassium.

Sodium has the same reactivity as potassium.

Sodium is more reactive than potassium.

Figure 3 shows the electronic structure of two different atoms.

A sodium atom forms a Na + ion.

Which ion does a magnesium atom form?

Tick (✓) one box.

Mg⁺ Mg⁻ Mg²⁺ Mg²⁻

This question is about the extraction of metals.

Traditional mining methods extract copper from high-grade copper ores.

Phytomining is a method used to extract copper from low-grade copper ores.

Explain one advantage of using phytomining compared with using traditional mining methods to extract copper.

Do not refer to cost in your answer.

Describe how copper compounds are obtained by phytomining.

Electrolysis is one method of obtaining copper from solutions of copper compounds.

Figure 6 shows the apparatus used.

Graphite is a good conductor of electricity.

Give one other reason why graphite is used for the electrodes.

A gas is produced at the positive electrode. The gas is tested with damp litmus paper. The gas bleaches the damp litmus paper.

Identify the copper compound in solution.

Give one reason for your answer.

Scrap iron is used in a reaction to obtain copper from solutions of copper compounds.

Name this type of reaction.

Aluminium is extracted by the electrolysis of a molten mixture of aluminium oxide and cryolite.

Explain why a mixture rather than pure aluminium oxide is electrolysed.

The positive electrodes are made of carbon.

Explain why the positive electrodes wear away during the process.

This question is about the reaction of metals with sulfuric acid.

The word equation for the reaction of zinc with sulfuric acid is:

zinc + sulfuric acid → zinc sulfate + hydrogen

What type of substance is zinc sulfate?

Tick (✓) one box.

Calculate the relative formula mass (M_r) of zinc sulfate (ZnSO₄).

Relative atomic masses (A_r): Zn = 65 S = 32 O = 16

A student investigated the temperature increase when the same mass of different metals were added to 0.1 M sulphuric acid.

The student used four different metals.

The student did the experiment three times for each metal and calculated the mean temperature increase for each metal.

Table 5 shows the results for nickel.

Calculate value X.

Table 6 shows the mean values for the four metals.

The student plotted the results on a bar chart.

Figure 9 shows the bar chart.

The student made some errors when plotting the bar chart.

Give three errors the student made.

Use Table 6 to place the metals in order of reactivity.

This question is about the reactions of metals.

A student investigated the temperature change when a metal was added to 25 cm³ of dilute sulfuric acid.

The student repeated the investigation with different metals.

The student kept all other variables constant.

Table 1 shows the results.

Figure 6 shows an incomplete bar chart for the data in Table 1.

Complete Figure 6.

You should:

• write the correct scale on the y-axis

• plot the bar for magnesium.

Another student investigated displacement reactions of metals.

The student added magnesium, nickel and zinc to different metal sulfate solutions and recorded when a reaction occurred.

Predict which metals will react with each metal sulfate solution.

Complete Table 2.

You should:

• use a tick (✓) to show where a reaction will occur

• use a cross (×) to show where no reaction will occur.

Table 1 is repeated here to help you.

The student dissolved 0.0025 moles of nickel sulfate in water to make 5 cm³ of nickel sulfate solution.

Calculate the concentration of the nickel sulfate solution in g/dm³

Relative formula mass (M_r) of nickel sulfate = 155

A teacher extracted copper from copper oxide.

This is the method used.

1. Mix 1.30 g of zinc and 1.59 g of copper oxide.

2. Heat the mixture strongly.

3. When the mixture starts to glow, stop heating.

4. Let the glow spread through the mixture.

5. Leave the mixture to cool.

This reaction is exothermic.

Which part of the method shows the reaction is exothermic?

Tick one box.

The equation for the reaction between zinc and copper oxide is:

1.30 g of zinc fully reacted with 1.59 g of copper oxide to produce 1.62 g of zinc oxide.

What mass of copper was produced?

What is the physical state of zinc oxide in the reaction?

Tick one box.

Which substance has been oxidised in the reaction?

Tick one box.

What type of reaction takes place when zinc reacts with copper oxide?

Tick one box.

Copper is a metal.

Which structure represents the arrangement of atoms in pure copper?

Tick one box.

Copper is used in electrical wiring.

Give one reason why.

In the UK, 40% of the copper we use is recycled copper.

The other 60% is copper obtained by mining.

What is the simplest ratio of recycled copper to copper obtained by mining?

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What are two advantages of recycling copper?

Tick two boxes.

A teacher demonstrated the extraction of copper from copper oxide.

This is the method used.

1. Mix 1.30 g of zinc and 1.59 g of copper oxide.

2. Heat the mixture strongly.

3. When the mixture starts to glow, stop heating.

4. Let the glow spread through the mixture.

5. Leave the mixture to cool.

6. Add hydrochloric acid to the cooled mixture.

7. Filter the mixture obtained in step 6.

A student concluded that an exothermic reaction had taken place.

Explain how an observation made during the demonstration shows this.

The equation for the reaction between zinc and copper oxide is:

1.59 g of copper oxide reacted.

Calculate the mass of copper produced.

Relative atomic masses (A_r): Cu = 63.5 O = 16 Zn = 65

Explain why steps 6 and 7 result in only copper being obtained as the residue.

The ionic equation for the reaction is:

Which statement about the reaction between zinc and copper ions is correct?

Tick one box.