AQA GCSE Trilogy Chemistry Paper 1 Foundation November 2020 question paper 8464/C/1F

This question is about acids and bases.

What is the pH of sulfuric acid? Tick (✓) one box.

An acid reacts with zinc to produce zinc chloride and hydrogen. Which acid reacts with zinc to produce zinc chloride? Tick (✓) one box.

What type of substance is zinc chloride? Tick (✓) one box.

An alkali is a base in solution. Which compound is an alkali? Tick (✓) one box.

The formula of the copper ion is Cu²⁺ The formula of the oxide ion is O^2– What is the formula of copper oxide? Tick (✓) one box.

A student reacts an acid with copper oxide.

The reaction between the acid and copper oxide is very slow at room temperature. How could the student speed up the reaction?

Complete the sentence to show how the student makes sure that all the acid reacts. Choose the answer from the box.

The student adds copper oxide to the acid until the copper oxide is.

The student filters the unreacted copper oxide from the solution. Which apparatus does the student use? Tick (✓) one box.

What process is used to produce crystals of a salt from a salt solution?

A student investigated the temperature change when metal X was added to copper sulfate solution. This is the method used.

1. Add 25 cm³ of copper sulfate solution to a beaker.

2. Measure the temperature of the copper sulfate solution.

3. Add 1.0 g of metal X and stir.

4. Measure the highest temperature reached when metal X is added to copper sulfate solution.

5. Repeat steps 1 to 4 with different metals.

Figure 1 shows the apparatus used.

Figure 2 shows the thermometer reading of the copper sulfate solution at the start of the investigation.

The highest temperature reached when metal X was added to copper sulfate solution was 35.5 °C Determine the temperature change when metal X is added to copper sulfate solution. Use Figure 2. Highest temperature = 35.5 °C

Give two variables the student should keep the same in this investigation.

The student repeated the experiment with metal Y. Table 1 shows four results for metal Y.

Calculate the mean temperature change for metal Y. Do not include the anomalous result in your calculation.

The more reactive the metal added to copper sulfate solution, the greater the temperature change. Figure 3 shows a reactivity series.

Figure 3

Calcium Magnesium Zinc Copper Silver least reactive

The student repeated the experiment. The student added:

• magnesium to copper sulfate solution

• an unknown metal A to copper sulfate solution.

Table 2 shows the results.

The student concludes metal A is zinc. Give one reason why the student is correct. Use Figure 3 and Table 2.

The student did the experiment with silver and copper sulfate solution. What happens to the temperature of the mixture? Use Figure 3. Tick (✓) one box.

Suggest one reason why the student should not add potassium metal to copper sulfate solution.

100 cm³ of the copper sulfate solution contains 1.8 g of copper sulfate. Calculate the mass of copper sulfate in 25 cm³ of this copper sulfate solution.

This question is about gold and compounds of gold. In the alpha particle scattering experiment alpha particles are fired at gold foil. Alpha particles are positively charged. Figure 4 shows the results.

Some alpha particles are deflected. Complete the sentence. Choose the answer from the box.

Some alpha particles are deflected because the nucleus of the atom is.

Why are most alpha particles not deflected? Tick (✓) one box.

What was one conclusion from the alpha particle scattering experiment? Tick (✓) one box.

Gold reacts with the elements in Group 7 of the periodic table.

What are Group 7 elements known as? Tick (✓) one box.

Fluorine, chlorine and bromine react with gold. Which element will be the most reactive with gold?

Tick (✓) one box.

3.94 g of gold reacts with chlorine to produce 6.07 g of gold chloride. The word equation for the reaction is: gold + chlorine → gold chloride Calculate the mass of chlorine that reacts with 3.94 g of gold.

Calculate the relative formula mass (M_r) of gold chloride (AuCl₃). Relative atomic masses (A_r): Cl = 35.5 Au = 197

This question is about elements and compounds.

Figure 5 shows the proportion of elements in the periodic table that are metals and non-metals.

Determine the percentage of the elements in Figure 5 that are metals.

Give two physical properties of metals.

Sodium reacts with chlorine to produce sodium chloride. Balance the equation for the reaction.

Figure 6 shows part of the structure of sodium chloride (NaC l).

What holds the particles together in sodium chloride? Use Figure 6. Tick (✓) one box.

Solid sodium chloride does not conduct electricity. Give two ways in which sodium chloride can be made to conduct electricity.

This question is about elements in the periodic table.

What property was used to arrange elements in early periodic tables? Tick (✓) one box.

In early periodic tables, iodine (I) was placed before tellurium (Te). Mendeleev placed iodine after tellurium. Figure 7 shows part of Mendeleev’s periodic table.

Suggest one reason why Mendeleev placed iodine in the column shown in Figure 7.

Table 3 shows the melting points of three Group 1 metals.

What state is lithium at 100 °C? Use Table 3. Tick (✓) one box.

Complete the graph in Figure 8. Use Table 3. You should:

• complete the scale on the y-axis

• draw bars to show the melting points of sodium and potassium.

Figure 8

Lithium reacts with chlorine to produce lithium chloride. Figure 9 shows what happens to the electrons in the outer shells when a lithium atom reacts with a chlorine atom. The dots (o) and crosses (x) represent electrons.

Describe what happens to a lithium atom and to a chlorine atom when they react. Use Figure 9 to answer in terms of electrons.

Lithium and potassium are in the same group of the periodic table. Figure 10 represents the electronic structures of a lithium atom and of a potassium atom.

Give two reasons why potassium is more reactive than lithium.

This question is about the extraction of aluminium.

An aluminium atom is represented as: 27 A l 13 Give the number of electrons and neutrons in the aluminium atom.

Aluminium is extracted by the electrolysis of a molten mixture of aluminium oxide and cryolite. Figure 11 shows the cell used for the electrolysis.

Aluminium is produced by the reduction of aluminium oxide (Al₂O₃). What is meant by the term reduction?

Oxygen is formed at the positive carbon electrodes. Explain why the positive carbon electrodes must be continually replaced.

A substance conducts electricity because of free moving, charged particles. What are the free moving, charged particles in a:

• carbon electrode (made from graphite)

• molten mixture of aluminium oxide and cryolite

• metal wire?

Molten mixture of aluminium oxide and cryolite

This question is about substances with covalent bonding.

Figure 12 shows a ball and stick model of a water molecule (H₂O).

Suggest one limitation of using a ball and stick model for a water molecule.

Ice has a low melting point. Water molecules in ice are held together by intermolecular forces. Complete the sentence. Ice has a low melting point because the intermolecular forces are.

Figure 13 shows the structure of a molecule.

What is the molecular formula of the molecule in Figure 13 ?

Diamond has a giant covalent structure.

What is the number of bonds formed by each carbon atom in diamond? Tick (✓) one box.

Give two physical properties of diamond.

Name two other substances with giant covalent structures.

Some students investigated the thermal decomposition of metal carbonates. The word equation for the reaction is: metal carbonate → metal oxide + carbon dioxide The students made the following hypothesis: ‘When heated the same mass of any metal carbonate produces the same mass of carbon dioxide.’

The students heated a test tube containing copper carbonate. Table 4 shows their results.

Plan a method the students could use to test their hypothesis. You should show how the students use their results to test the hypothesis. You do not need to write about safety precautions.