Ionic bonding and ionic compounds

This question is about atoms and ions.

The model of the atom has changed over time.

In an early model, scientists thought the atom was a tiny sphere that could not be divided.

Figure 1 represents this early model of the atom.

The discovery of a subatomic particle led to a change in the model in Figure 1.

Which was the first subatomic particle to be discovered?

Tick () one box.

In a later model of the atom, most of the mass was concentrated in the centre of the atom.

What is the name of the centre of an atom?

Atoms contain three types of subatomic particle.

Draw one line from each subatomic particle to the relative charge of the particle.

What is meant by the ‘atomic number of an atom’?

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Table 1 shows information about two isotopes of an element.

Calculate the relative atomic mass (A_r) of the element.

Use the equation:

A = (mass number × percentage) of isotope A + (mass number × percentage) of isotope B

Give your answer to 1 decimal place.

An oxygen atom has eight electrons.

Complete Figure 2 to show the electronic structure of an oxygen atom.

Figure 2

Figure 3 represents two models of sodium chloride.

What are two advantages of model B compared with model A ?

Tick () two boxes.

Lithium, carbon, nitrogen, fluorine and neon are elements in the same row of the periodic table.

What is the chemical symbol of lithium?

Use the periodic table.

Lithium has metallic bonding.

Which electrons are involved in metallic bonding?

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Lithium reacts with fluorine to produce lithium fluoride.

Draw one line from each substance to the particle diagram that represents the substance.

Table 2 shows the electrical conductivity of three substances.

Lithium fluoride is an ionic compound.

Which substance is lithium fluoride?

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Carbon can exist in different forms.

Figure 4 represents one form of carbon.

What is the name of the form of carbon in Figure 4 ?

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Carbon and fluorine form a compound with the formula CF₄

Calculate the relative formula mass (M_r) of CF₄

Relative atomic masses (A_r): C = 12 F = 19

Figure 5 represents a molecule of nitrogen.

What is the total number of shared electrons in the covalent bond shown in Figure 5 ?

Lithium and nitrogen form a compound with the formula Li₃N

Complete the sentence.

Choose the answer from the box.

Neon does not react with other elements to form compounds.

Why is neon unreactive?

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This question is about bonding and structures.

Figure 10 represents two models of sodium chloride.

Give two limitations of model A compared with model B.

Aluminium sulfate consists of the ions:

What is the formula of aluminium sulfate?

Metals have metallic bonding.

Suggest one reason why aluminium metal conducts electricity better than sodium metal.

Silicon dioxide and the polymer poly(ethene) are solid substances.

Compare silicon dioxide with the polymer, poly(ethene).

Answer in terms of structure and bonding.

Table 2 shows diagrams which represent the structures of two substances.

Compare the structure and bonding of sodium chloride and oxygen.

Halogens are elements in Group 7 of the periodic table.

Calcium reacts with chlorine to produce calcium chloride.

Explain what happens to calcium atoms and to chlorine atoms when calcium reacts with chlorine to produce calcium chloride.

Explain why chlorine is more reactive than bromine.

Table 4 shows the boiling points of four hydrogen halides.

Describe how the boiling points of the hydrogen halides change as the relative formula mass changes.

Structure and bonding is used to explain properties of compounds.

Metal atoms react with non-metal atoms to form ions.

Which group of elements does not form ions? Tick (✓) one box.

Potassium reacts with chlorine to produce potassium chloride (KC l). Figure 6 shows what happens to the electrons in the outer shells when a potassium atom reacts with a chlorine atom.

Describe what happens when a potassium atom reacts with a chlorine atom to produce potassium chloride. Answer in terms of electrons.

In solid ionic compounds, oppositely charged ions attract to form a giant structure. Which structure represents the arrangement of ions in solid potassium chloride? Tick (✓) one box.

Non-metal atoms share electrons to form covalent bonds.

Water (H₂O) is a covalent molecule. Table 2 shows the number of electrons in the outer shells of hydrogen atoms and

Figure 7 shows part of a dot and cross diagram for a molecule of water. Complete the dot and cross diagram. You should only show electrons in the outer shells.

Figure 7

Silica has a giant covalent structure. Figure 8 represents the structure of silica.

Determine the ratio of silicon (Si) atoms to oxygen (O) atoms in silica. Use Figure 8.

Polymers have very large molecules. Figure 9 represents part of the structure of a polymer.

What holds polymer molecule 1 and polymer molecule 2 together in a polymer? Tick (✓) one box.

Describe the trend shown in Figure 10.

Sodium is in Group 1 of the periodic table. Sodium reacts with oxygen to produce sodium oxide.

Balance the equation for the reaction.

Explain what happens to sodium atoms and to oxygen atoms when sodium reacts with oxygen to produce sodium oxide (Na₂O). Answer in terms of electrons.

Sodium burns in a gas jar of oxygen. Figure 3 shows the apparatus.

Give two observations seen during the reaction.

Describe two differences in the observations if potassium is used instead of sodium.

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 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.

This question is about substances with covalent bonding.

Figure 2 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 3 shows the structure of a molecule.

What is the molecular formula of the molecule in Figure 3 ?

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.

This question is about elements. Caesium is in Group 1 of the periodic table.

Explain what happens to caesium atoms and to oxygen atoms when caesium reacts with oxygen to produce caesium oxide. You should answer in terms of electrons.

Explain why caesium is more reactive than sodium. You should answer in terms of electrons.

Figure 6 shows part of Mendeleev’s periodic table.

Explain why the early periodic tables placed iodine (I) before tellurium (Te), but then Mendeleev placed tellurium before iodine.

This question is about Group 1 elements.

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

4.6 g of sodium reacts with chlorine to produce 11.7 g of sodium chloride. What mass of chlorine reacted?

A teacher puts hot sodium into a gas jar of chlorine. The changes seen before, during and after this reaction were observed. Complete the sentences. Choose the answers from the box.

Sodium chloride (NaC l) is an ionic compound. Write the formulae of the ions in sodium chloride.

Complete the sentence. Choose the answer from the box.

Potassium is more reactive than sodium.

How does the size of a potassium atom compare with the size of a sodium atom? Give a reason for your answer.

This question is about sodium.

Sodium reacts with chlorine. What is the balanced equation for the reaction?

Tick (✓) one box.

Hot sodium is put in a gas jar of chlorine. Describe the observations made before, during and after the reaction.

Explain why sodium is less reactive than potassium.

Chlorine reacts with sodium and with hydrogen. Compare the structure and bonding in sodium chloride and hydrogen chloride.

This question is about structure and bonding.

Figure 1 shows part of the structure of calcium oxide (CaO).

What type of bonding is present in calcium oxide?

Tick one box.

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Figure 2 shows a particle of methane (CH₄).

What type of particle is present in Figure 2 ?

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Figure 3 shows the structure of C₆₀

Complete the sentence. Choose the answer from the box.

Figure 4 shows the structure of graphite.

What type of bond is labelled A in Figure 4 ? Tick one box.

In graphite, each carbon atom forms bonds with other carbon atoms as shown in

Figure 4

How many electrons does one carbon atom use to form one bond? Tick one box.

An electric current is passed through copper. Figure 5 shows the apparatus used.

Complete the sentence. Choose the answer from the box.

Complete the sentence. Choose the answer from the box.

Figure 6 shows the apparatus used to investigate the effect of electricity on sodium chloride solution.

Complete the sentence. Choose the answer from the box.

Sodium chloride is made up of ions. Figure 7 shows the apparatus used to investigate the effect of electricity on solid sodium chloride and molten sodium chloride.

Table 1 shows the results.

Draw one line from each statement to the correct reason.

This question is about sodium and chlorine. Figure 13 shows the positions of sodium and chlorine in the periodic table.

State one difference and one similarity in the electronic structure of sodium and of chlorine.

Sodium atoms react with chlorine atoms to produce sodium chloride (NaCl). Describe what happens when a sodium atom reacts with a chlorine atom. Write about electron transfer in your answer.

The reaction between sodium and chlorine is an exothermic reaction. Complete the reaction profile for the reaction between sodium and chlorine.

This question is about sodium and chlorine. Figure 2 shows the positions of sodium and chlorine in the periodic table.

State one difference and one similarity in the electronic structure of sodium and of chlorine.

Sodium atoms react with chlorine atoms to produce sodium chloride (NaCl). Describe what happens when a sodium atom reacts with a chlorine atom. Write about electron transfer in your answer.

The reaction between sodium and chlorine is an exothermic reaction. Complete the reaction profile for the reaction between sodium and chlorine.