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2.2 Bonding structure - How bonds relate to structure - High demand – Questions

Q1.This question is about ammonia.

(a) Figure 1 shows the outer electron shells in an ammonia molecule.

Complete Figure 1 to show a dot and cross diagram for an ammonia molecule.

Show the outer shell electrons only.

Figure 1

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(b) Explain why ammonia is a gas at room temperature.

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In industry, ammonia is produced by reacting nitrogen with hydrogen.

The equation for this reaction is:

N2(g) + 3H2(g) ⇌ 2NH3(g)

(c) Calculate the minimum mass of nitrogen required to produce 72.0 grams of ammonia.

Assume all the nitrogen reacts to produce ammonia.

Relative atomic masses (Ar): H = 1 N = 14

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Mass of nitrogen = ____________________ grams(5)

Figure 2 shows information about the percentage yield of ammonia under varying conditions.

Figure 2

The conditions used in the industrial process to produce ammonia are:• 200 atmospheres pressure• 450 °C• iron catalyst.

(d) What is the percentage yield of ammonia under these conditions?

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Percentage of ammonia = ____________________ %(1)

(e) Suggest reasons why these conditions are used in the industrial process.

You should use:• the equation for the reaction• information from Figure 2• your knowledge of reversible reactions.

You should refer to both yield and rate of reaction in your answer.

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(Total 17 marks)

Q2.Sulfur dioxide (SO2) is used to manufacture sulfuric acid.

(a) Explain why sulfur dioxide has a low boiling point.

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(b) The equation shows one stage in the manufacture of sulfuric acid from sulfur dioxide.

2SO2(g) + O2(g) 2SO3 (g)

The reaction is exothermic in the forward direction.

Use Le Chatelier’s Principle to predict the effect of increasing the temperature on the amount of sulfur trioxide (SO3) produced at equilibrium.

Give a reason for your answer.

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(c) Use Le Chatelier’s Principle to predict the effect of increasing the pressure on the amount of sulfur trioxide (SO3) produced at equilibrium.

Give a reason for your answer.(2)

(Total 7 marks)

Q3.The elements in Group 1 of the periodic table are metals.

(a) The elements in Group 1 are called the alkali metals.

Why are they called the alkali metals?

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(b) Explain the increase in reactivity of elements further down the group.

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(c) Lithium oxide is an ionic compound.

Draw a dot and cross diagram to show how lithium and oxygen combine to form lithium oxide.

Only show the electrons in the outer shell of each atom.

Give the charges on the ions formed.(4)

(Total 10 marks)

Q4.This question is about copper.

(a) Copper can be extracted by smelting copper-rich ores in a furnace.

The equation for one of the reactions in the smelting process is:

Cu2S(s) + O2(g) 2 Cu(s) + SO2(g)

Explain why there would be an environmental problem if sulfur dioxide gas escaped into the atmosphere.

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(b) The impure copper produced by smelting is purified by electrolysis, as shown below.

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Copper atoms are oxidised at the positive electrode to Cu2+ ions, as shown in the half equation.

Cu(s) Cu2+(aq) + 2e−

(i) How does the half equation show that copper atoms are oxidised?

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(ii) The Cu2+ ions are attracted to the negative electrode, where they are reduced to produce copper atoms.

Write a balanced half equation for the reaction at the negative electrode.

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(iii) Suggest a suitable electrolyte for the electrolysis.

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(c) Copper metal is used in electrical appliances.

Describe the bonding in a metal, and explain why metals conduct electricity.

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(d) Soil near copper mines is often contaminated with low percentages of copper compounds.

Phytomining is a new way to extract copper compounds from soil.

Describe how copper compounds are extracted by phytomining.

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(e) A compound in a copper ore has the following percentage composition by mass:

55.6% copper, 16.4% iron, 28.0% sulfur.

Calculate the empirical formula of the compound.

Relative atomic masses (Ar): S = 32; Fe = 56; Cu = 63.5

You must show all of your working.

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Empirical formula = ______________________________(4)

(Total 16 marks)

Q5.

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This question is about compounds.

(a) The table gives information about the solubility of some compounds.

Soluble compounds

All potassium and sodium salts

All nitrates

Chlorides, bromides and iodides, except those of silver and lead

Use information from the table to answer these questions.

(i) Name a soluble compound that contains silver ions.

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(ii) Name a soluble compound that contains carbonate ions.

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(b) Metal oxides react with acids to make salts.

What type of compound is a metal oxide?

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(c) Lead nitrate solution is produced by reacting lead oxide with nitric acid.

(i) State how solid lead nitrate can be obtained from lead nitrate solution.

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(ii) Balance the equation for the reaction.

PbO + HNO3 Pb(NO3)2 + H2O(1)

(iii) Give the total number of atoms in the formula Pb(NO3)2

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(d) An oxide of lead that does not have the formula PbO contains 6.21 g of lead and 0.72 g of oxygen.

Calculate the empirical formula of this lead oxide.

Relative atomic masses (Ar): O = 16; Pb = 207

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You must show your working to gain full marks.

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Empirical formula = ____________________(4)

(Total 10 marks)

Q6.Silicon dioxide is used as a lining for furnaces.

Furnaces can be used to melt iron for recycling.

© Oleksiy Mark/iStock

The diagram shows a small part of the structure of silicon dioxide.

Explain why silicon dioxide is a suitable material for lining furnaces.

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Q7.Spacecraft have been to the planets Venus and Mars. The spacecraft have sent back information about the atmosphere of each planet.

© Tristan3D/Shutterstock

(a) The main gas in the atmosphere of Mars is carbon dioxide.

Explain why, in terms of structure, carbon dioxide is a gas, even at low temperatures.

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(b) The atmosphere on Venus contains droplets of sulfuric acid solution.

(i) Suggest a pH value for sulfuric acid solution.

pH = ______________(1)

(ii) Name the ion which makes sulfuric acid solution acidic.

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(c) The atmosphere of Venus contains the isotopes and

Describe the similarities and the differences in the isotopes and

You should refer to the sub-atomic particles in each isotope.

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(Total 8 marks)

Q8.This question is about gold (Au).

(a) An atom of gold is represented as:

197

Au

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How many neutrons are in this atom of gold? ________________________(1)

(b) Gold ions are used as a catalyst.

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How does a gold atom (Au) become a gold ion (Au3+)?

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(c) A gold catalyst can be used when carbon monoxide reacts with oxygen to make carbon dioxide.

(i) Complete and balance the equation for this reaction.

__ CO + _______ → ___ CO2

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(ii) Carbon dioxide has a very low boiling point.

Explain why.

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(d) Gold is used as a catalyst in industrial processes. Gold is rare and increasingly expensive.

Suggest three reasons why gold is still used in industrial processes.

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(Total 11 marks)

Q9.

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High quality connectors are used to connect a satellite box to a television.The connectors should conduct electricity very well and should not corrode.

By Alphathon (Own work) [CC-BY-SA-3.0 or GFDL], via Wikimedia Commons

The connectors on this scart lead are coated with gold.

(a) Gold is a typical metal.

(i) Describe the structure and bonding of gold.

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(ii) Why is gold a good conductor of electricity?

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(b) The surface of some metals, such as iron, corrode when exposed to the air.

Suggest why this reduces the electrical conductivity of the metal.

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(Total 6 marks)

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Q10.Welding blankets are placed under metals being welded. They protect the area under the welding.

Some welding blankets are made from silicon dioxide which does not melt when hit by sparks or molten metal.

The diagram shows a small part of the structure of silicon dioxide.

Describe the structure and bonding in silicon dioxide and explain why it is a suitable material for making welding blankets.

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(Total 3 marks)

Q11.Electrolysis can be used to remove unwanted hair from the skin.

The hair is first coated with a layer of gel containing ions in solution.

The positive electrode is connected by a patch to the skin.

The negative electrode is connected to the hair. Electricity flows through the gel and causes electrolysis of the body fluid around the hair follicle.

(a) Metal wires conduct electricity to the electrodes.

Explain how metals conduct electricity.

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(b) Explain why the gel containing ions in solution can conduct electricity.

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(c) The body fluid is a solution that contains sodium chloride. The electricity causes the electrolysis of a small amount of this solution.

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This solution contains hydrogen ions that move to the negative electrode.

(i) The half equation represents the reaction at the negative electrode.

2H+ + 2e– → H2

Explain why this reaction is a reduction.

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(ii) As a result of the electrolysis of sodium chloride solution, an alkali forms which kills the hair follicle.

What is the name of this alkali? ____________________________________(1)

(iii) Complete the half equation for the reaction at the positive electrode.

Cl – → Cl2(1)

(Total 6 marks)

Q12.Perfumes contain a mixture of chemicals.

The main ingredients of perfumes are a solvent and a mixture of fragrances.

(a) A sample of the solvent used in one perfume contained 0.60 g of carbon, 0.15 g of hydrogen and 0.40 g of oxygen.

Relative atomic masses: H = l; C = 12; O = 16.

Calculate the empirical (simplest) formula of the solvent.

You must show all of your working to gain full marks for this question.

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(b) Solvent molecules evaporate easily.

Explain why substances made of simple molecules evaporate easily.

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(c) Most companies claim that their perfumes have been tested on skin. A study was made of the tests they used. The study found that each company used different tests.

The perfumes were tested in the companies’ own laboratories and not by independent scientists.

Some companies did not give any information about the tests that they had used.

(i) Suggest why companies test their perfumes on skin.

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(ii) Did the study show that the tests made by the different companies were valid and reliable?

Explain your answer.

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(Total 9 marks)

Q13.The drawing shows a high quality wire used to make electrical connections on a hi-fi system.

Multi-strand "OFC" copperto maitain high signal purity

(a) Copper is used because it is a very good conductor of electricity. Copper is a typical metal.

(i) Describe the structure and bonding in a metal. You may wish to draw a diagram to help you to answer this question.

To gain full marks in this question you should write your ideas in good English. Put them into a sensible order and use the correct scientific words.

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(ii) Explain, by reference to your answer to part (a)(i), why copper conducts electricity.

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(iii) Explain, by reference to your answer to part (a)(i), why copper can be drawn into wires.

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(b) The copper used to make this wire is “OFC” copper. This stands for ‘oxygen free copper’.

(i) It is thought that when molten copper is cooled and solidified it can take in some oxygen from the air. This may slightly decrease the conductivity of the copper.

Suggest why the conductivity might be decreased.

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(ii) To make it oxygen free, the copper is heated in an atmosphere of hydrogen.

Explain how this will remove the oxygen.

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(Total 8 marks)

Q14.The following passage was taken from a chemistry textbook.

Germanium is a white, shiny, brittle element. It is used in the electronics industry because it is able to conduct a small amount of electricity.

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It is made from germanium oxide obtained from flue dusts of zinc and lead smelters.The impure germanium oxide from the flue dusts is changed into germanium by the process outlined below.

STEP 1 The germanium oxide is reacted with hydrochloric acid to makegermanium tetrachloride. This is a volatile liquid in which the germanium and chlorine atoms are joined by covalent bonds.

STEP 2 The germanium tetrachloride is distilled off from the mixture.

STEP 3 The germanium tetrachloride is added to an excess of water toproduce germanium oxide and hydrochloric acid.

STEPS 1 to 3 are repeated several times.

STEP 4 The pure germanium oxide is reduced by hydrogen to form germanium.

(a) Balance the equation below which represents the reaction in step 1.

GeO2 + ______ HCl → GeCl4 + ______ H2O(1)

(b) Write a word equation for the reaction in step 3.

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(c) Suggest why steps 1 to 3 are repeated several times.

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(d) The equation which represents the reaction in step 4 is shown below.

GeO2 + 2H2 → Ge + 2H2O

(i) Explain what is meant by the term ‘reduced’.

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(ii) Calculate the mass of germanium which could be made from 525 g of germanium oxide. (Relative atomic masses: Ge = 73; O = 16).

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Mass _____________________ g

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(e) Germanium is difficult to classify as either a metal or a non-metal.

(i) Give as much evidence as you can from the information in this question to support the view that germanium is a metal. Explain your answer as fully as you can.

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(ii) Give as much evidence as you can from the information in this question to support the view that germanium is a non-metal. Explain your answer as fully as you can.

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(Total 13 marks)

Q15.Iron is used (as steel) to make the body panels for cars.

The iron panels have to be bendable so that they can be pressed into the shape required, but must also be strong. The panels must also be able to conduct electricity because they form part of the electrical circuits of the car.

(a) Iron is a typical metal. Describe the structure and bonding in a metal such as iron. You may use a diagram if you wish.

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(b) Explain how the structure and bonding of iron:

(i) allows the body panels to conduct electricity;

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(ii) allows the body panels to be bent into shape;

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(iii) gives the body panels strength.

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(Total 8 marks)

Q16.(i) Complete the drawing to show the electron structure of a hydrogen fluoride

molecule. Draw electrons as dots or crosses.

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(ii) Explain why hydrogen fluoride is a gas at room temperature.

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(Total 3 marks)

Q17.(a) The diagram shows part of the ionic lattice of a sodium chloride crystal.

(i) Complete the spaces in the table to give information about both of the ions in this lattice.

Name of ion Charge

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(ii) When it is solid, sodium chloride will not conduct electricity. However, molten sodium chloride will conduct electricity. Explain this difference.

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(iii) Complete the sentence.

Sodium chloride conducts electricity when it is molten and when it is

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(b) The symbol for a calcium atom can be shown like this:

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(i) What is the mass number of this atom?

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(ii) What information is given by the mass number?

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(c) Calcium burns in oxygen with a brick-red flame. The product is a white solid. It is calcium oxide and its formula is CaO.

(i) Balance the chemical equation for the reaction.

Ca(s) + O2(g) → CaO(s)(1)

(ii) Describe, in terms of electrons, what happens to a calcium atom when it becomes a calcium ion.

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(Total 10 marks)

Q18.(a) By reference to their structure, explain how the particles in a piece of metal are held

together and how the shape of the metal can be changed without it breaking.

(You may use a diagram in your answer.)

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(b) Explain why metals are good conductors of electricity and suggest why this conductivity increases across the periodic table from sodium to magnesium to aluminium.

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(Total 9 marks)

Q19.The diagram shows the elements in Group 4 of the periodic table.

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Carbon is a non-metal and silicon is usually considered to be a non-metal.

Tin and lead have all the usual properties of metals.

Germanium has these properties:

• grey-white shiny solid

• melting point 937°C

• semi-conductor

• reacts with chlorine to form the chloride (GeCl4) which is a liquid molecular compound

• germanium oxide reacts with acids to form a salt solution and water. It also reacts with alkalis.

(a) With reference to their structure, explain why tin and lead are good conductors of electricity.

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(b) Would you classify germanium as a metal or as a non-metal? Give your reasons.

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(Total 6 marks)

Q20.The diagrams show the giant structures of sodium chloride and diamond.

sodium chloride (melting point 801°C) diamond (melting point 4800°C)

(a) The equation shows how sodium choride could be formed.

Balance the equation.

Na + Cl2 → Na Cl(1)

(b) By reference to the detailed structure of sodium chloride explain fully why:

(i) sodium chloride has a quite high melting point,

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(ii) solid sodium chloride melts when it is heated strongly,

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(iii) molten sodium chloride will conduct electricity.

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(c) By reference to the detailed structure of diamond, explain why the melting point of diamond, is higher than that of sodium chloride.

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(Total 7 marks)

Q21.(a) The diagrams represent the atomic structures of two gases, hydrogen and helium.

Hydrogen gas is made up of diatomic molecules (molecules with two atoms).Helium gas exists as single atoms.

(i) How is a molecule of hydrogen formed from two hydrogen atoms? (You may use a diagram as part of your answer)

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(ii) Why does helium exist only as single atoms?

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(b) Hydrogen combines with carbon to form methane.Each molecule contains four hydrogen atoms strongly bonded to a carbon atom.

Explain why methane has a low boiling point.

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(Total 6 marks)

Q22.(a) Copper is a metal.

Explain how it conducts electricity.

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(b) Graphite is a non-metal.

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Use the information to explain why graphite conducts electricity.

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(Total 5 marks)

Q23.Copper is used in plumbing.

© Dave White/iStock

(a) Complete the following sentence.

Elements in the central block of the periodic table, eg copper, iron and zinc, are

called ____________________________ metals.(1)

(b) State three properties that make copper suitable for use in plumbing.

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(c) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate.

Copper can be extracted from copper ores by two methods:

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Method 1 or mining and smelting

Method 2 phytomining.

The main stages in the two methods are shown in the flow diagrams.

Use information from the flow diagrams and your own knowledge to evaluate both methods of copper extraction.

Give the advantages and disadvantages of both methods.

Remember to include a conclusion in your answer.

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(Total 10 marks)

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