C1 Atomic Structure and Periodic Name:...

C1 Atomic Structure and PeriodicTable35 Questions

Name: ________________________

Class: ________________________

Date: ________________________

Time:

Marks:

Comments:

of 108Brookvale Groby Learning Trust

The pH scale is a measure of the acidity or alkalinity of a solution.

(a) Draw one line from each solution to the pH value of the solution.

Solution pH value of the solution

5

Acid 7

9

Neutral 11

13

(2)

1

(b) Which ion in aqueous solution causes acidity?

Tick one box.

H+

Na+

O2−

OH−

(1)


(c) When sulfuric acid is added to sodium hydroxide a reaction occurs to produce twoproducts.

The equation is:

H2SO4 + 2NaOH Na2SO4 + 2H2O

How many elements are in the formula H2SO4?

Tick one box.

3

4

6

7

(1)

(d) What is this type of reaction?

Tick one box.

Decomposition

Displacement

Neutralisation

Reduction

(1)

(e) Name the salt produced.

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(1)


(f) Describe how an indicator can be used to show when all the sodium hydroxide has reactedwith sulfuric acid.

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(3)

(Total 9 marks)

John Newlands arranged the known elements into a table in order of atomic weight.

Figure 1 shows part of Newlands’ table.

Figure 1

Group 1 2 3 4 5 6 7

H Li Be B C N O

F Na Mg Al Si P S

Cl K Ca

(a) What are the names of the elements in Group 5 of Newlands’ table?

Tick one box.

Calcium and sulfur

Carbon and silicon

Chlorine and silver

Chromium and tin

(1)

2


(b) In what order is the modern periodic table arranged?

Tick one box.

Atomic mass

Atomic number

Atomic size

Atomic weight

(1)

(c) Give two differences between Group 1 of Newlands’ table and Group 1 of the periodictable.

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(2)


(d) In 1864, atoms were thought to be particles that could not be divided up into smallerparticles.

By 1898, the electron had been discovered and the plum pudding model of an atom wasproposed.

Figure 2 shows the plum pudding model of an atom of carbon and the nuclear model of anatom of carbon.

Figure 2

Compare the position of the subatomic particles in the plum pudding model with the nuclearmodel.

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(4)


(e) Models are used to show the differences between elements, compounds and mixtures.

Which circle shows a model of a mixture?

Tick one box.

(1)

(f) Figure 3 shows a model of carbon dioxide.

Figure 3

What does each line between the atoms in Figure 3 represent?

Tick one box.

Covalent bond

Intermolecular force

Ionic bond

Metallic bond

(1)

(Total 10 marks)


The three states of matter are solid, liquid and gas.

(a) Lithium reacts with water to produce lithium hydroxide solution and hydrogen.

Use the correct state symbols from the box to complete the chemical equation.

aq g l s

2Li(s) + 2H2O(l) 2LiOH(____) + H2(____)

lithium + water lithium hydroxide + hydrogen

(2)

3


(b) Figure 1 shows the melting points and the boiling points of four substances, A, B, C and D.

Figure 1

Which substance is liquid over the greatest temperature range?

Tick one box.

A

B

C

D

(1)


(c) Which two substances are gases at 50 °C?

Tick one box.

A and B

B and C

C and D

A and D

(1)

(d) A different substance, E, has:• a melting point of −50 °C• a boiling point of +120 °C

Plot these two values on Figure 1.

(2)


(e) Figure 2 shows the apparatus a student used to determine the melting point and theboiling point of substance B in Figure 1.

Figure 2

Explain why the student could not use this apparatus to determine the boiling point ofsubstance B.

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(2)

(f) Suggest one reason why the student could not use this apparatus to determine the exactmelting point of substance B.

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(1)

(Total 9 marks)


This question is about calcium.

(a) What type of compound is calcium oxide?

Tick one box.

An acid

A base

A carbonate

A salt

(1)

4

(b) Ionic compounds, such as calcium oxide, have high melting points.

Complete the sentences. Use words from the box.

bonds forces ions layers

Calcium oxide has a giant ionic lattice in which there are strong electrostatic

______________________ of attraction in all directions.

(1)


(c) The figure below shows the electronic structure of an oxygen atom and a calcium atom.

Describe how the calcium atom and the oxygen atom forms calcium oxide.

You should give the charge on each ion formed.

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(4)

(Total 6 marks)


Figure 1 shows a reactor used to produce titanium from titanium(IV) chloride.

Figure 1

The chemical equation for the reaction of titanium(IV) chloride with sodium is:

TiCl4 + 4Na Ti + 4NaCl

titanium(IV) chloride + sodium titanium + sodium chloride

(a) For one reaction:

• 1615 kg titanium(IV) chloride reacted completely with 782 kg sodium• 1989 kg sodium chloride was produced.

Calculate the mass of titanium produced from this reaction.

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Mass of titanium = _________________ kg

(1)

5


(b) The table below shows the solubility of sodium chloride in 100 cm3 of aqueous solution atdifferent temperatures.

Solubility of sodium chloride in g per100cm3

Temperature in °C

35.72 10

35.89 20

36.09 30

37.37 40

36.69 50

37.04 60

On Figure 2:

• plot this data on the grid• draw a line of best fit.

Figure 2

(3)


(c) The product sodium chloride is dissolved in water to separate it from titanium.

At 30 °C the solubility of sodium chloride is 36 kg per 100 dm3.

Calculate the minimum volume of water in dm3, at 30 °C, needed to dissolve 1989 kgsodium chloride.

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Volume of water = ____________________ dm3

(2)

(d) Calculate the percentage by mass of titanium in titanium(IV) chloride (TiCl4).

Give your answer to 3 significant figures.

Relative atomic masses (Ar): Cl = 35.5; Ti = 48

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Percentage of titanium by mass = _______________ %

(3)

(e) Suggest why the reaction is done in an atmosphere of dry argon instead of air containingwater vapour.

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(3)


(f) Explain why titanium conducts electricity.

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(3)

(Total 15 marks)

Elements are made up of atoms.

(a) What is the approximate radius of an atom?

Tick one box.

1 × 10 m

1 × 10−1 m

1 × 10−10 m

1 × 10−100 m

(1)

6

(b) The figure below shows the atoms of five elements.

The letters are not the symbols of these elements.

Complete the sentence.

All of the elements in the figure above are in Group

_____________ of the periodic table.

(1)


(c) Which two atoms in the figure above are isotopes of the same element?

Explain your answer fully.

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(3)

(d) The halogens are in Group 7 of the periodic table.

Explain the trend in reactivity of the halogens.

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(6)

(Total 11 marks)


The apparatus in the figure below is used to separate a mixture of liquids in a fuel.

(a) What is apparatus W on above the figure above?

Tick one box.

Beaker

Boiling Tube

Flask

Jug

(1)

7


(b) What is the name of this method of separation?

Tick one box.

Crystallisation

Electrolysis

Filtration

Distillation

(1)

(c) Name the changes of state taking place at A and B in the figure above.

Use words from the box.

boiling condensing freezing melting

Change of state at A: _________________________________________________

Change of state at B: _________________________________________________

(2)


(d) Table 1 shows the boiling points of the hydrocarbons in the fuel.

Table 1

HydrocarbonBoiling point

in °C

Pentane 36

Hexane 69

Heptane 98

Octane 125

Which hydrocarbon will be the last to collect in the beaker?

Tick one box.

Pentane

Hexane

Heptane

Octane

(1)


(e) The fuel is a mixture of liquids that has been designed as a useful product.

What name is given to this type of mixture?

Tick one box.

Catalyst

Formulation

Polymer

Solvent

(1)

(f) Describe how this fuel is different from crude oil.

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(2)


(g) A student measured the melting point of a solid hydrocarbon four times.

The student’s results are in Table 2.

Table 2

Trial 1 Trial 2 Trial 3 Trial 4

Melting pointin °C

35 48 37 37

Calculate the mean melting point of the hydrocarbon, leaving out any anomalous result.

Give your answer to two significant figures.

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Mean melting point = __________________ °C

(2)

(Total 10 marks)

This question is about drinking water.

(a) Name two methods of treating water from rivers, lakes or the sea to produce drinkingwater.

Tick two boxes.

Anaerobic digestion

Cracking

Desalination

Electrolysis

Sterilising

(2)

8


(b) The table below shows the amounts of dissolved ions in a sample of drinking water.

Dissolved ion Mass in mgper dm3

Cl– 250

Na+ 200

NO3+ 40

What is the name of the ion with the symbol Cl–?

Tick one box.

Calcium ion

Carbonate ion

Chloride ion

Chlorine ion

(1)


(c) Use the information in the table above to complete the bar chart in Figure 1.

Figure 1

(1)

(d) Look at the questions labelled A, B, C, D.

A How many substances are there in drinking water?

B How much fluoride is in drinking water?

C Is fluoride soluble in drinking water?

D Should fluoride be added to drinking water?

Which one of the questions cannot be answered by science alone?

Tick one box.

A B C D

(1)


(e) Give two reasons why the answer you have chosen cannot be answered by science alone.

1. _________________________________________________________________

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2. _________________________________________________________________

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(2)

(f) A sample of drinking water contains 1.5 mg of fluoride per dm3 of water.A person drinks 1 dm3 of this water.

The recommended daily amount of fluoride is 4.0 mg.

Which calculation gives the percentage of the recommended daily amount of fluoride in 1dm3 of this water?

Tick one box.

(1)


(g) Figure 2 shows the effect of fluoride in drinking water on tooth decay in different agegroups.

Figure 2

Describe the pattern of tooth decay in Figure 2 for water without fluoride.

Use data to justify your answer.

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(2)

(h) Describe the effect of adding fluoride to drinking water for the age groups in Figure 2.

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(2)

(Total 12 marks)


The figure below shows an atom of boron.

(a) When the mass of the boron atom is calculated, the mass of the electrons is ignored.

Why is the mass of the electrons ignored?

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(1)

9

(b) How many electrons are there in the boron atom?

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(1)

(c) What is the electrical charge on the nucleus of the boron atom?

Tick one box.

+1

+5

+6

+11

(1)


(d) The mass number of boron is 11.

Use the figure above to calculate the number of neutrons in the nucleus of the boron atom.

Explain how you worked out the answer.

Number of neutrons = _________________________________________________

Explanation _________________________________________________________

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(3)

(e) Phosphorus has a mass number of 31 and has 16 neutrons.

What percentage of the mass number of phosphorus is the number of neutrons?

Give your answer to two significant figures.

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Percentage = ____________________

(2)

(Total 8 marks)

The figure below shows a simple model of the three states of matter.

(a) What is the correct equation to work out the density of a material?

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(1)

10


(b) A student explains density to his teacher using the particle model in the figure above.

His teacher says there are limitations to the model.

Give two limitations of the particle model in the figure above.

1. _________________________________________________________________

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2. _________________________________________________________________

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(2)

(c) When the gas in a container with a fixed volume is heated, the pressure increases as thetemperature increases.

Explain why the pressure increases.

Use the model in the figure above to help you.

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(4)

(Total 7 marks)


A student used paper chromatography to identify the pigments in spinach leaves.

She used propanone as a solvent.

Figure 1 shows the student’s results.

Figure 1

(a) Name the mobile phase and the stationary phase in the student’s experiment.

Mobile phase ________________________________________________________

Stationary phase _____________________________________________________

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(2)

11


(b) What does Figure 1 tell you about the green pigment from spinach?

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(3)

(c) Write the equation that links distance moved by solvent, distance moved by solute and Rf

value.

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(1)

(d) Use Figure 1 to calculate the Rf value for pigment B.

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Rf value = ________________

(3)


(e) Another student set up the apparatus shown in Figure 2.

Figure 2

This student did not set up the apparatus correctly.

Identify the errors the student made.

Explain how the errors she made would affect her results.

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(4)

(Total 13 marks)


Figure 1 shows the plum pudding model of the atom.

This model was used by some scientists after the discovery of electrons in 1897.

Figure 1

Plum-pudding model

In 1911 the scientists Geiger and Marsden investigated the effect of firing alpha particles at verythin sheets of gold foil.

Their experiment is shown in Figure 2. The arrows show the paths taken by alpha particles in theexperiment.

Figure 2

(a) Explain why scientists replaced the plum pudding model of the atom with the nuclear modelof the atom as a result of the experiment.

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(4)

12


(b) According to modern measurements:

• the radius of an atom is about 1 × 10 –10m

• the radius of an atomic nucleus is about 1 × 10 –14m

Show that these values fit with the nuclear model of the atom.

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(2)

(c) In 1931 a scientist discovered that there are hydrogen atoms with mass number 2 as wellas hydrogen atoms with mass number 1.

A year later, another scientist discovered neutrons.

Explain why the discovery of neutrons could explain the presence of hydrogen atoms withdifferent mass numbers.

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(3)

(d) How would the results of the experiment shown in Figure 2 change if neutrons were usedinstead of alpha particles to bombard a thin sheet of gold?

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(2)

(Total 11 marks)


The elements in the periodic table are arranged in groups.

(a) What is similar about the elements in the same group?

Tick one box.

Chemical properties

Atomic numbers

Relative atomic masses

(1)

13

(b) Figure 1 shows the arrangement of electrons in an atom.

Figure 1

What group of the periodic table is this atom in?

Group _________________

(1)


(c) Why are the elements in Group 0 unreactive?

Tick one box.

They are all gases at room temperature

They all have the same atomic number

They are all in the same group of the periodic table

They all have a stable arrangement of electrons

(1)


(d) A teacher demonstrates the reaction of some alkali metals with water.

Look at Figure 2.

Figure 2

The students write what they see.

1. The alkali metals float on water.

2. The alkali metals fizz when they react with water.

3. The universal indicator changes from green to purple.

4. The sodium disappears faster than the lithium.

Give a reason for each of the four things that the students see.

1. The alkali metals float on water.

Reason ___________________________________________________________

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2. The alkali metals fizz when they react with water.

Reason ___________________________________________________________

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3. The universal indicator changes from green to purple.

Reason ___________________________________________________________

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4. The sodium disappears faster than the lithium.

Reason ___________________________________________________________

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(4)

(Total 7 marks)


In 1869 there were 60 known elements.

Mendeleev arranged the elements in order of their atomic mass (atomic weight).

He realised that elements with similar properties occurred at regular intervals.

(a) Suggest why one of the groups that is on today’s periodic table was not in Mendeleev’speriodic system.

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(1)

14

(b) Explain the arrangement of the first 20 elements in today’s periodic table.

You should answer in terms of atomic structure.

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(2)


(c) A student put some potassium bromide solution in a test tube.

She added a few drops of chlorine solution and observed the result.

She repeated the process using different potassium halide salts and different halogens.

The table below shows the student’s results.

Solution ofhalogen

Potassiumchloride solution

Potassiumbromide solution

Potassium iodidesolution

Chlorine Orange colour

formsBrown colour

forms

Bromine No reaction Brown colour

forms

Iodine No reaction No reaction

Give the order of reactivity of the halogens from the results in the table above.

Explain how you used the results to show this order of reactivity.

Order ______________________________________________________

Explanation _______________________________________________________

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(2)

(d) Write a balanced ionic equation for the reaction of chlorine with bromide ions in solution.

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(3)


(e) Explain the order of reactivity of Group 7 elements.

Include information about atomic structure.

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(2)

(Total 10 marks)

The table below shows information about some elements.

Element Melting pointin °C

Boiling pointin °C

Fluorine –202 –188

Chlorine –101 –35

Bromine –7 59

Iodine 114 184

Astatine

(a) Look at the table above.

Describe the trend in melting point from fluorine to astatine.

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(1)

15

(b) Estimate the boiling point of astatine.

Use the table above to help you.

Boiling point of astatine = _________________ °C

(1)

(c) Room temperature is 20 °C.

Which element in the table above is a liquid at room temperature?

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(1)


(d) To which group of the periodic table do the elements in the table above belong?

Tick one box.

Group 0

Group 1

Group 5

Group 7

(1)

(e) A chlorine atom has 17 electrons.

On the figure below, use crosses to show the arrangement of electrons in the outer shell ofa chlorine atom.

(1)

(f) Chlorine reacts with sodium bromide solution to produce bromine and sodium chloridesolution.

Complete the symbol equation for the reaction.

___Cl2 + ______ NaBr _________ + ____________

(2)


(g) Which element in the table above will react with sodium chloride solution?

Give a reason for your answer.

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(2)

(Total 9 marks)

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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(2)

16

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

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(4)


(c) Lithium oxide is an ionic compound.

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

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

Give the charges on the ions formed.

(4)

(Total 10 marks)

Five elements, V, W, X, Y and Z, are shown in the periodic table.

The letters are not the chemical symbols of the five elements.

17

Use the correct letter, V, W, X, Y or Z, to answer each question.

(a) Which element is a transition metal?

(1)

(b) Which element is in Group 2?

(1)

(c) Which element is a noble gas?

(1)

(d)Which element has an atomic (proton) number of4?

(1)


(e) Which element forms only 1+ ions?

(1)

(Total 5 marks)

This question is about magnesium.

(a) (i) The electronic structure of a magnesium atom is shown below.

Use the correct answer from the box to complete each sentence.

electrons neutrons protons shells

The nucleus contains protons and _________

The particles with the smallest relative mass that move around the nucleus are called

_________

Atoms of magnesium are neutral because they contain the same number of

electrons and _________

(3)

18


(ii) A magnesium atom reacts to produce a magnesium ion.

Which diagram shows a magnesium ion?

Tick ( ) one box.

(1)

(b) Magnesium and dilute hydrochloric acid react to produce magnesium chloride solution andhydrogen.

Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g)

(i) State two observations that could be made during the reaction.

1. ____________________________________________________________

______________________________________________________________

2. ____________________________________________________________

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(2)


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

Describe a method for making pure crystals of magnesium chloride from magnesiumand dilute hydrochloric acid.

In your method you should name the apparatus you will use.

You do not need to mention safety.

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(6)

(Total 12 marks)

This question is about metals.

(a) Which unreactive metal is found in the Earth as the metal itself?

Tick ( ) one box.

aluminium

gold

magnesium

(1)

19


(b) Complete the sentence.

Aluminium is an element because aluminium is made of

only one type of _________________________ .

(1)

(c) Figure 1 shows the electronic structure of an aluminium atom.

(i) Use the correct words from the box to complete the sentence.

electrons ions protons neutrons shells

The nucleus of an aluminium atom contains _______________ and

_______________ .

(2)

(ii) Complete the sentence.

In the periodic table, aluminium is in Group _______________ .

(1)


(d) Aluminium is used for kitchen foil.

Figure 2 shows a symbol on a box of kitchen foil.

The symbol means that aluminium can be recycled. It does not show the correct chemicalsymbol for aluminium.

(i) What is the correct chemical symbol for aluminium?

___________________________ .

(1)

(ii) Give two reasons why aluminium should be recycled.

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(2)

(e) Aluminium has a low density, conducts electricity and is resistant to corrosion.

Which one of these properties makes aluminium suitable to use as kitchen foil?Give a reason for your answer.

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(2)

(Total 10 marks)


This question is about atomic structure and elements.

(a) Complete the sentences.

(i) The atomic number of an atom is the number of _______________________

(1)

(ii) The mass number of an atom is the number of ________________________

______________________________________________________________

(1)

20

(b) Explain why an atom has no overall charge.

Use the relative electrical charges of sub-atomic particles in your explanation.

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(2)

(c) Explain why fluorine and chlorine are in the same group of the periodic table.

Give the electronic structures of fluorine and chlorine in your explanation.

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(2)


(d) The diagram shows the electronic structure of an atom of a non-metal.

What is the chemical symbol of this non-metal?

Tick ( ) one box.

Ar

O

S

Si

(1)

(e) When elements react, their atoms join with other atoms to form compounds.

Complete the sentences.

(i) Compounds formed when non-metals react with metals consist of

particles called _________________________ .

(1)

(ii) Compounds formed from only non-metals consist of

particles called ____________________ .

(1)

(Total 9 marks)


This question is about carbon and gases in the air.

(a) Carbon atoms have protons, neutrons and electrons.

Complete the table by writing the relative mass of a neutron and an electron.

Name of particle Relative mass

proton 1

neutron

electron

(2)

21

(b) What is the total number of protons and neutrons in an atom called?

Tick ( ) one box.

The atomic number

The mass number

One mole of the atom

(1)

(c) An atom of carbon has six electrons.

Which structure, A, B or C, represents the electronic structure of the carbon atom?

The carbon atom is structure

(1)


(d) Carbon reacts with oxygen to produce carbon dioxide (CO2).

(i) How many different elements are in one molecule of carbon dioxide?

______________________________________________________________

(1)

(ii) What is the total number of atoms in one molecule of carbon dioxide?

______________________________________________________________

(1)

(e) Sometimes carbon reacts with oxygen to produce carbon monoxide (CO).

(i) Calculate the relative formula mass (Mr) of carbon monoxide.

Relative atomic masses (Ar): C = 12; O = 16

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______________________________________________________________

Mr of carbon monoxide = _______________

(1)

(ii) Calculate the percentage by mass of carbon in carbon monoxide.

______________________________________________________________

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Percentage by mass of carbon in carbon monoxide = _____%

(1)


(f) Carbon dioxide is one of the gases in the air.

(i) The graph shows the percentage of argon and the percentage of carbon dioxide inthe air.

What is the percentage of argon in the air?

Percentage of argon = ____________________ %

(1)

(ii) An instrumental method is used to measure the amount of carbon dioxide in theair.

Give one reason for using an instrumental method.

______________________________________________________________

______________________________________________________________

(1)

(Total 10 marks)


This question is about atoms and isotopes.

(a) Atoms contain protons, neutrons and electrons.

A lithium atom has the symbol

Explain, in terms of sub-atomic particles, why the mass number of this lithium atom is 7.

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(3)

22

(b) Amounts of substances can be described in different ways.

Complete the sentences.

One mole of a substance is the relative formula mass in

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The relative atomic mass of an element compares the mass of an atom of an element withthe mass of an atom of

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(2)

(c) Two isotopes of oxygen are and

Describe the similarities and differences between the isotopes and

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

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(3)

(Total 8 marks)


The diagram shows the chemical symbols of five elements in the periodic table.

(a) Choose the correct chemical symbol to complete each sentence.

(i) The element that is an alkali metal is _____________ .

(1)

(ii) The element that is a transition metal is _____________ .

(1)

(iii) The element in Group 4 is _____________ .

(1)

(iv) The element with a full outer energy level (shell) of electrons is

_____________ .

(1)

(b) Which other element goes in the shaded box?

_______________________

(1)

(Total 5 marks)

23


In 1866 John Newlands produced an early version of the periodic table.

Part of Newlands’ periodic table is shown below.

Column 1 2 3 4 5 6 7

H Li Be B C N O

F Na Mg Al Si P S

Cl K Ca Cr Ti Mn Fe

Newlands’ periodic table arranged all the known elements into columns in order of their atomicweight.

Newlands was trying to show a pattern by putting the elements into columns.

(a) Iron (Fe) does not fit the pattern in column 7.

Give a reason why.

___________________________________________________________________

___________________________________________________________________

(1)

24

(b) In 1869 Dmitri Mendeleev produced his version of the periodic table.

Why did Mendeleev leave gaps for undiscovered elements in his periodic table?

___________________________________________________________________

___________________________________________________________________

(1)

(c) Newlands and Mendeleev placed the elements in order of atomic weight.


The modern periodic table places the elements in order of

______________________ .

(1)


(d) Lithium, sodium and potassium are all in Group 1 of the modern periodic table.

Explain why.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

(2)

(Total 5 marks)

This question is about the halogens (Group 7).

(a) How do the boiling points of the halogens change down the group from fluorine to iodine?

___________________________________________________________________

___________________________________________________________________

(1)

25

(b) Sodium bromide is produced by reacting sodium with bromine.

Sodium bromide is an ionic compound.

(i) Write down the symbols of the two ions in sodium bromide.

______________________________________________________________

(1)

(ii) Chlorine reacts with sodium bromide solution to produce bromine and one otherproduct.

Complete the word equation for the reaction.

chlorine + sodium bromide bromine + ______________

(1)

(iii) Why does chlorine displace bromine from sodium bromide?

______________________________________________________________

______________________________________________________________

(1)

(iv) Use the Chemistry Data Sheet to help you to answer this question.

Suggest which halogen could react with sodium chloride solution to produce chlorine.

______________________________________________________________

(1)

(Total 5 marks)


The positions of eight elements in the modern periodic table are shown below.

26

Choose the correct chemical symbols to complete each sentence.

(a) The two metals that react vigorously with water are ____________ and

____________ .

(1)

(b) The element used as a catalyst in the Haber process is ____________ .

(1)

(c) The two elements with five electrons in their outer shell (highest energy

level) are ____________ and ____________ .

(1)

(d) Iron has ions with different charges.

The other metal that has ions with different charges is ____________ .

(1)

(Total 4 marks)

The diagram shows a carbon atom.

27


(a) (i) A proton is labelled.

Use the correct answer from the box to label each of the other sub-atomic particles.

electron ion molecule neutron

(2)

(ii) The atom of carbon is represented as:

What is the mass number of this carbon atom?

Draw a ring around the correct answer.

6 13 19

(1)

(iii) Complete the sentence.

Atoms of carbon have no overall electrical charge because the number

of protons is the same as the number of _______________________ .

(1)

(b) Butane is represented as:

(i) Use the correct answer from the box to complete each sentence.

bond compound helium hydrogen mixture oxygen

Butane is a ___________________ .

Butane contains atoms of carbon and ___________________ .

Each line between the atoms in butane represents a chemical

_________________ .

(3)


(ii) Which is the correct formula for butane?

Tick (✔) one box.

C4H4

C4H8

C4H10

(1)

(Total 8 marks)

Sulfur is a non-metal.

Sulfur burns in the air to produce sulfur dioxide, SO2

(a) Why is it important that sulfur dioxide is not released into the atmosphere?

Tick (✔) one box.

Sulfur dioxide causes acid rain.

Sulfur dioxide causes global dimming.

Sulfur dioxide causes global warming.

(1)

28

(b) Sulfur dioxide dissolves in water.

What colour is universal indicator in a solution of sulfur dioxide?Give a reason for your answer.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

(2)


(c) Sulfur dioxide is a gas at room temperature.

The bonding in sulfur dioxide is covalent.

Explain, in terms of its structure and bonding, why sulfur dioxide has a low boiling point.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

(3)

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

Sulfur dioxide is produced when fossil fuels are burned.

It is important that sulfur dioxide is not released into the atmosphere.

Three of the methods used to remove sulfur dioxide from gases produced when fossil fuelsare burned are:

• wet gas desulfurisation ( W)

• dry gas desulfurisation ( D)

• seawater gas desulfurisation ( S).

Information about the three methods is given in the bar chart and in Table 1 and Table 2.

Method of removing sulfur dioxide


Table 1

Method Material used How material is obtained

W Calcium carbonate, CaCO3 Quarrying

DCalcium oxide, CaO Thermal decomposition of calcium

carbonate:

CaCO3 CaO + CO2

S Seawater From the sea

Table 2

Method What is done with waste material

WSolid waste is sold for use in buildings.Carbon dioxide is released into the atmosphere.

D Solid waste is sent to landfill.

S Liquid waste is returned to the sea.


Evaluate the three methods of removing sulfur dioxide from waste gases.

Compare the three methods and give a justified conclusion.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

(6)

(Total 12 marks)


(a) Figure 1 shows an atom of element G.

Figure 1

Draw a ring around the correct answer to complete each sentence.

(i) Label A shows

an electron an ion a nucleus

(1)

29

(ii) The particle labelled B is

an isotope a molecule a neutron

(1)

(iii) The mass number of element G is

5 6 11

(1)

(iv) Use the periodic table to identify element G.

Element G is

boron carbon sodium

(1)


(b) Figure 2 shows a compound of G and hydrogen.

Figure 2


(i) The formula of the compound in Figure 2 is

GH3 G3H 3HG

(1)

(ii) The type of bonding shown in Figure 2 is

covalent ionic metallic

(1)

(Total 6 marks)


(a) The symbols for seven different elements are shown in Figure 1.

Figure 1

He

Be

Na S Ar

Ca Fe

Choose the correct symbol from Figure 1 to answer each question.

You may use each symbol once, more than once or not at all.

Write the symbol that represents:

(i) a Group 1 element

______________________________

(1)

30

(ii) a transition metal

______________________________

(1)

(iii) an element with electrons in the same number of energy levels as an atom of argon(Ar)

______________________________

(1)

(iv) an element which forms an oxide that dissolves in water to form an acidic solution

______________________________

(1)

(v) an element that forms a chloride with the formula XCl

______________________________

(1)


(b) A teacher put a cube of sodium metal into water containing universal indicator, as shown inFigure 2.

Figure 2

The equation for the reaction is:

2Na(s) + 2H2O(l) 2NaOH (aq) + H2(g)

sodium + water sodiumhydroxide

+ hydrogen

(i) The sodium floated on the surface of the water. The universal indicator turned purple.

Give three other observations that would be seen during the reaction.

1. ____________________________________________________________

______________________________________________________________

2. ____________________________________________________________

______________________________________________________________

3. ____________________________________________________________

______________________________________________________________

(3)

(ii) Name the ion that made the universal indicator turn purple.

______________________________________________________________

(1)


(c) Figure 3 represents the electronic structure of a sodium atom.

Figure 3

In the space below, draw the electronic structure of a sodium ion. Include the charge on theion.

(2)

(Total 11 marks)

A student investigated the conductivity of different concentrations of sodium chloride solution.The student set the apparatus up as shown in Figure 1.

Figure 1

31


The student measured the conductivity of the pure water with a conductivity meter.

The reading on the conductivity meter was zero.

(a) The student:

• added sodium chloride solution one drop at a time• stirred the solution• recorded the reading on the conductivity meter.

The student’s results are shown in the table below.

Number of drops ofsodium chloride solution

added

Relative conductivityof solution

0 0

1 100

2 120

3 310

4 400

5 510

6 590

7 710

8 800


(i) The student plotted the results on the grid shown in Figure 2.

Plot the four remaining results.

Draw a line of best fit, ignoring the anomalous result.

Figure 2

Number of drops of sodium chloride added

(3)

(ii) One of the points is anomalous.

Suggest one error that the student may have made to cause the anomalous result.

______________________________________________________________

______________________________________________________________

(1)


(iii) The student wanted to compare the conductivity of sodium chloride solution with theconductivity of potassium chloride solution.

State one variable he should keep constant when measuring the conductivity of thetwo solutions.

______________________________________________________________

(1)

(b) (i) Explain, in terms of bonding, why pure water does not conduct electricity.

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

(2)

(ii) Explain why sodium chloride solution conducts electricity.

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

(2)

(iii) After he had added sodium chloride solution, the student noticed bubbles of gas atthe negative electrode.


The gas produced at the negative electrode is __________________

(1)

(Total 10 marks)


Use the periodic table and the information in the table below to help you to answer the questions.

The table shows part of an early version of the periodic table.

Group 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7

H

Li Be B C N O F

Na Mg Al Si P S Cl

(a) Hydrogen was placed at the top of Group 1 in the early version of the periodic table.

The modern periodic table does not show hydrogen in Group 1.

(i) State one similarity between hydrogen and the elements in Group 1.

______________________________________________________________

______________________________________________________________

(1)

32

(ii) State one difference between hydrogen and the elements in Group 1.

______________________________________________________________

______________________________________________________________

(1)

(b) Fluorine, chlorine, bromine and iodine are in Group 7, the halogens.

The reactivity of the halogens decreases down the group.

Bromine reacts with a solution of potassium iodide to produce iodine.

Br2 + 2KI 2KBr + I2

(i) In the reaction between bromine and potassium iodide, there is a reduction ofbromine to bromide ions.

In terms of electrons, what is meant by reduction?

______________________________________________________________

______________________________________________________________

(1)

(ii) Complete the half equation for the oxidation of iodide ions to iodine molecules.

2I−

(2)


(iii) Explain, in terms of electronic structure, why fluorine is the most reactive element inGroup 7.

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

(3)

(Total 8 marks)

A student was trying to produce hydrogen gas.

Figure 1 shows the apparatus she used.

Figure 1

(a) No gas was produced.

The student’s teacher said that this was because the substances in the flask did not react.

(i) Suggest why the substances in the flask did not react.

______________________________________________________________

______________________________________________________________

______________________________________________________________

(1)

33


(ii) Which two substances could the student have put in the flask to produce hydrogensafely?

Tick (✓) one box.

Gold and dilute hydrochloric acid

Potassium and dilute hydrochloric acid

Zinc and dilute hydrochloric acid

(1)

(b) Another student did produce hydrogen from two substances.

Figure 2 shows the apparatus the student used to collect and measure the volume of thehydrogen gas.

Figure 2

Give the name of the apparatus labelled X.

___________________________________________________________________

(1)


(c) The student did the experiment four times. Her results are shown in the table below.

Experiment Volume of hydrogen collected inone minute in cm3

1 49

2 50

3 35

4 48

(i) One of the results is anomalous.

Which result is anomalous? Write your answer in the box.

Give a reason for your choice.

______________________________________________________________

(2)

(ii) Calculate the mean volume of hydrogen collected in one minute.

______________________________________________________________

______________________________________________________________

Mean volume = ____________________ cm3

(2)

(iii) Give a reason why the experiment should be repeated several times.

______________________________________________________________

______________________________________________________________

______________________________________________________________

(1)


(d) A teacher collected two tubes full of hydrogen gas, as shown in Figure 3.

Figure 3

She tested tube A with a lighted splint as soon as she took the bung out.

She tested tube B with a lighted splint a few seconds after taking the bung out.

(i) Suggest why tube B gave a much louder pop than tube A.

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

(1)

(ii) Complete and balance the chemical equation for the reaction that takes place whenthe hydrogen reacts in this test.

H2 + O2

(2)

(Total 11 marks)


Fossil fuels contain carbon.

(a) The figure below represents a carbon atom.


(i) The name of the particle with a positive charge is

an electron.

a neutron.

a proton.

(1)

34

(ii) The centre of the atom is called the

energy level.

molecule.

nucleus.

(1)

(iii) Use the Chemistry Data Sheet to help you to answer this question.

Use the correct number from the box to complete each sentence.

4 6 8 10 12

The mass number of this carbon atom is

In the periodic table, carbon is in Group


(b) Coal is a fossil fuel.

A piece of coal contains:

• 80% carbon

• 9% oxygen

• 1% sulfur

• 5% hydrogen.

The rest of the coal is other elements.

(i) What is the percentage of other elements in this piece of coal?

________________ %

(1)

(ii) Coal burns in air to produce carbon dioxide, sulfur dioxide and water.

Draw one line from each product to the type of pollution caused by each product.

Product Type of pollution

Acid rain

Carbon dioxide

Global dimming

Sulfur dioxide

Global warming

Water

No pollution

(3)

(Total 8 marks)


Glass is made from silicon dioxide.

© Velirina/iStock/Thinkstock

(a) Silicon dioxide has a very high melting point.

Other substances are added to silicon dioxide to make glass. Glass melts at a lowertemperature than silicon dioxide.

Suggest why.

___________________________________________________________________

___________________________________________________________________

(1)

35

(b) Sodium oxide is one of the substances added to silicon dioxide to make glass.

(i) Sodium oxide contains Na+ ions and O2– ions.

Give the formula of sodium oxide.

______________________________________________________________

(1)

(ii) Sodium oxide is made by heating sodium metal in oxygen gas.

Complete the diagram to show the outer electrons in an oxygen molecule (O2).

(2)


(c) Glass can be coloured using tiny particles of gold. Gold is a metal.

Describe the structure of a metal.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

(3)

(Total 7 marks)


Mark schemes

(a)

extra lines from solution negate the mark2

(b) H+

1

(c) 31

(d) Neutralisation1

1

(e) sodium sulfate1

(f) Add indicator to sodium hydroxide solution

allow add indicator to sulfuric acid1

Add sulfuric acid (gradually)

allow add sodium hydroxide solution (gradually)1

allow pH probe

until indicator just changes (colour)

or until universal indicator turns green or shows pH71

[9]

(a) Carbon and silicon12

(b) Atomic number1

(c) Hydrogen / fluorine / chlorine are not in Group 1 of the periodic tableorHydrogen and fluorine / chlorine are not in the same group of the periodic table

1


Lithium / sodium / potassium are in Group 1 of the periodic table1

(d) plum pudding model has a single ball of positive charge and nuclear model has positivecharges in the centre / nucleus

1

plum pudding model has electrons in random positions and nuclear model has electronsin fixed positions

1

plum pudding model has no nucleus and the nuclear model has a nucleus1

plum pudding model has no neutrons and the nuclear model has neutrons in the nucleus1

(e)

1

(f) Covalent bond1

[10]

(a) LiOH (aq)

this order1

3

H2 (g)1

(b) C1

(c) A and D1

(d) point x at −10 °C1

point ● at +150 °C1

(e) substance B will not reach its boiling point of 190 °C1

because the boiling point of water is only 100 °C1


(f) there is too much substance B to melt instantly.

allow answers based on thermal conductivity or temperaturegradient from the wall of the test tube to the thermometer

1

[9]

(a) A base14

(b) forces1

(c) calcium loses electrons and oxygen gains electrons

max 3 for incorrect reference to atom / ion or to oxygen / oxide1

two electrons are transferred1

calcium has a 2+ charge1

oxide has a 2– charge1

[6]

(a) 408 kg15

(b) all points correct

± ½ small square2

allow 1 mark if 5 points correct

best fit line1

(c)

1

5525 dm3

1

(d) relative formula mass of TiCl4 is 1901

25.26 %1

Answer given to 3 significant figures = 25.3 %1

25.23% with or without working gains 3 marks

(e) argon is unreactive1


water (vapour) would react with sodium

allow water (vapour) would react with titanium(IV) chloride1

and air contains oxygen that would react with reactants

allow and air contains oxygen that would react with products1

(f) (titanium conducts electricity) because electrons in the outer shell of the metal atoms aredelocalised

1

and so electrons are free to move

allow the delocalised electrons in the metal carry electrical chargethrough the metal

1

through the whole structure1

[15]

(a) 1 × 10−10 m1

6

(b) 1 / one

allow alkali metals1

(c) R and S1

because they have the same number of protons

allow same atomic number, different mass number1

and a different numbers of neutrons1


(d) Level 3 (5–6 marks):A relevant and coherent explanation of the trend in reactivity. The response makeslogical links between the points raised and considers both the number of energy levelsand the distance between the nucleus and the outer energy level.

Level 2 (3–4 marks):Statements that are linked to provide a simple explanation of the trend in reactivity usingeither the number of energy levels or the distance between the nucleus and the outerenergy level.

Level 1 (1–2 marks):Simple statements made about the halogens or the trend in reactivity.

0 marks:No relevant comment

Indicative content

Simple statements / descriptions• have 7 electrons in the outer shell• need to gain an electron• form ions with a -1 charge• halogens further down the group are less reactive (or vice versa)• halogens further down the group have more shells or energy levels (or vice

versa)

Linked statements / explanations• have 7 electrons in the outer shell so need to gain an electron to have the

electronic structure of a noble gas• halogens further down the group are less reactive because they have more

shells or energy levels (or vice versa)• halogens further down the group have more shells or energy levels so less

attractive force on the incoming electron (or vice versa)• halogens further down the group have more shells or energy levels so more

‘shielding’ against the incoming electron (or vice versa)• outer electrons of halogens further down group are further away from the

attractive force of the nucleus (or vice versa)• an electron is less easily gained because there are more shells or energy

levels (or vice versa)• an electron is less easily gained because the outer electrons are further from

the attractive force of the nucleus (or vice versa)6

[11]

(a) Flask17

(b) Fractional distillation1

(c) A – boiling

in this order1


B – condensing1

(d) Pentane1

(e) Formulation1

(f) the fuel is a pure compound1

and crude oil is a mixture

or

the fuel is made up of four hydrocarbons

allow crude oil contains a large number of compounds and the fuelcontains four

and crude oil could have many more1

(g) (35 + 37 + 37 / 3) = 36.331

361

allow (35 + 48 + 37 + 37 / 4 =) 39(.25) for 1 mark

[10]

(a) Desalination18

Sterilising1

(b) Chloride ion1

(c) correct bar for NO3-

1

(d) D1

(e) any two from:• people have the right to choose (opinion)• ethical / moral question• cannot be tested by experiment

2

(f)

1


(g) the percentage tooth decay increases with age1

by 4 % for each increasing age group1

(h) reduces tooth decay (for all age groups)1

greater reduction in older people1

[12]

(a) because the mass of an electron is very small

do not accept has no mass1

9

(b) 5 / five1

(c) +51

(d) 61

(because) mass number = no. protons + no. electrons

allow atomic number = 51

(so the number of) neutrons = 11 – 5

allow mass number – number of protons1

(e) (16 / 31) × 100 = 51.61

= 52

incorrect sig. figs max 1 mark1

[8]

(a) density = mass / volume110

(b) any two from:

• no forces shown between spheres• atoms / molecules / ions are not solid spheres• not all the same size.

2

(c) at higher temperatures particles have more kinetic energy1

(so) the (average) speed of the particles increases1


(so there are) more frequent collisions with the wall of the container1

which apply a greater force on wall of container (so pressure rises)1

[7]

(a) mobile phase propanone111

stationary phase paper1

(b) any three from:

• contains chlorophyll a, b and carotene• contains Pigment B• does not contain pheophytin• contains (at least) one unknown substance• contains five substances• contains a substance that does not dissolve in the solvent

3

(c)

1

(d) both measurements correct

solvent front = 9.0 cm and pigment B distance = 5.0 cm1

Rf = 5.0 / 9.01

= 0.56

allow ecf from incorrect measurements1

(e) origin line drawn in ink1

so it will run or dissolve in the solvent or split up1

spots under solvent or solvent above spots / origin line1

so they will mix with solvent or wash off paper or colour the solvent or dissolve in thesolvent

1

[13]

(a) most alpha particles went straight through, suggesting lots of empty space112

a few alpha particles bounced back, suggesting small central nucleus1


with all the positive charge1

the plum pudding model does not explain the results because it shows the whole atom as aball of positive charge with no empty space

1

(b) the figures show that the radius of an atom is 10 000 times bigger than the nucleus1

consistent with the nuclear model, which says that the atom has a tiny nucleus at thecentre of the atom

1

(c) all hydrogen atoms have just one proton (in the nucleus)1

some hydrogen atoms also have one neutron1

protons and neutrons have the same relative mass so mass number of these atoms is 21

(d) neutrons are not attracted or repelled by a positive nucleus1

so the neutrons would all pass through the foil1

[11]

(a) Chemical properties113

(b) three / 31

(c) They all have a stable arrangement of electrons1

(d) less dense than water

allow lighter than water1

gas / hydrogen produced1

an alkali / hydroxide is produced1

sodium is more reactive than lithium1

[7]

(a) did not appear because they had not been discovered or they are unreactive or they didnot form compounds

1

14


(b) arranged in order of atomic / proton number1

elements in the same group have the same number of electrons in the outer shell1

(c) chlorine>bromine>iodine

table shows that chlorine displaces bromine and iodine1

and bromine displaces iodine1

(d) Cl2(aq) + 2 Br–(aq) Br2(aq) + 2 Cl–(aq)

correct formulae1

correct balancing1

correct state symbol1

(e) the further down the group, the halogen becomes less reactive because outer electrons arefurther from the nucleus

1

so less attractive force on an incoming electron1

[10]

(a) the melting point increases115

(b) 337 °C

allow an answer in the range 278 °C to 337 °C1

(c) bromine1

(d) Group 71


(e)

7 electrons in outer shell1

(f) Cl2 + 2NaBr Br2 + 2NaCl

correct formulae for products1

correct balancing1

(g) fluorine1

(because it is) more reactive than chlorine

allow because it is the most reactive element1

[9]

(a) because they form hydroxides116

that give alkaline solutions (in water)1

(b) the atoms have more electron shells (as move down the group)1

so the electron in the outer shell is further away from the nucleus1

which reduces the attraction to the nucleus1

so the electron is lost more easily from the atom1

(c)

electronic structure of lithium drawn correctly1


electronic structure of oxygen drawn correctly1

correct charge on ions (Li+ and O2–)1

correct number of each ion (2 lithium, 1 oxygen)1

[10]

(a) Y1

(b) W1

(c) V1

(d) W1

(e) X1

[5]

17

(a) (i) neutrons

this order only1

electrons1

protons1

(ii) box on the left ticked1

18

(b) (i) effervescence / bubbling / fizzing / bubbles of gas

do not accept just gas alone1

magnesium gets smaller / disappears

allow magnesium dissolves

allow gets hotter or steam produced

ignore references to magnesium moving and floating / sinking andincorrectly named gases.

1


(ii) Marks awarded for this answer will be determined by the Quality ofCommunication (QC) as well as the standard of the scientific response.Examiners should also refer to the information in the Marking Guidance andapply a ‘best–fit’ approach to the marking.

0 marksNo relevant content

Level 1 (1−2 marks)There are simple statements of some of the steps in a procedure for obtainingmagnesium chloride.

Level 2 (3−4 marks)There is a description of a laboratory procedure for obtaining magnesiumchloride from dilute hydrochloric acid and magnesium.

The answer must include a way of ensuring the hydrochloric acid is fullyreacted or a method of obtaining magnesium chloride crystals.

Level 3 (5−6 marks)There is a well organised description of a laboratory procedure for obtainingmagnesium chloride that can be followed by another person.

The answer must include a way of ensuring the hydrochloric acid is fullyreacted and a method of obtaining magnesium chloride crystals.

examples of the points made in the response:• hydrochloric acid in beaker (or similar)• add small pieces of magnesium ribbon• until magnesium is in excess or until no more effervescence occurs *• filter using filter paper and funnel• filter excess magnesium• pour solution into evaporating basin / dish• heat using Bunsen burner• leave to crystallise / leave for water to evaporate / boil off water• decant solution• pat dry (using filter paper).

*Student may choose to use a named indicator until it turns a neutral colour,record the number of pieces of magnesium added then repeat without theindicator.

6

[12]

(a) gold119

(b) atom (s)1


(c) (i) protons

any order

allow proton1

neutrons

allow neutron1

(ii) 3 / three1

(d) (i) Al

ignore any numbers / charges1

(ii) any two from:• limited resource• expensive in terms of energy / mining• effects on the environment, such as, landfill, atmospheric pollution,

quarrying

allow uses a lot of energy to extract.2

(e) resistant to corrosion1

does not react (with water or food)

allow one mark for low density with a suitable reason given1

[10]

(a) (i) protons

allow “protons or electrons”, but do not allow “protons andelectrons”

1

(ii) protons plus / and neutrons1

20

(b) (because the relative electrical charges are) −(1) for an electron and +(1) for a protonallow electrons are negative and protons are positive

1

and the number of electrons is equal to the number of protons

if no other mark awarded, allow 1 mark for the charges cancel out1


(c) (the electronic structure of) fluorine is 2,7 and chlorine is 2,8,7

allow diagrams for the first marking point1

(so fluorine and chlorine are in the same group) because they have the same numberof or 7 electrons in their highest energy level or outer shell

if no other mark awarded, allow 1 mark for have the same / similarproperties

1

(d) S1

(e) (i) ions1

(ii) molecules1

[9]

(a) 1

must be in this order1

very small

accept negligible, 1 / 2000

allow zero1

(b) The mass number1

(c) C1

21

(d) (i) 21

(ii) 31

(e) (i) 281

(ii) 42.9

accept ecf from (e)(i)

accept 42 - 431


(f) (i) 0.91

(ii) any one from:• accurate• sensitive• rapid• small sample.

1

[10]

(a) because this lithium atom has

3 protons1

and 4 neutrons1

mass number is total of neutrons and protons

accept protons and neutrons have a mass of 1

accept number of neutrons = 7 - 3(protons)

ignore mass of electron is negligible1

22

(b) grams

accept g1

12C

allow carbon-12 or C-12

ignore hydrogen or H1

(c) any three from:

max 2 if no numbers given

numbers if given must be correct

• both have 8 protons

accept same number of protons• 18O has 10 neutrons• 16O has 8 neutrons

accept different number of neutrons or 18O has two more neutronsfor 1 mark

• both have 8 electrons.

accept same number of electrons3

[8]


(a) (i) Na

allow sodium1

(ii) Cu

allow copper1

(iii) C

allow carbon1

(iv) He

allow helium1

23

(b) H

allow hydrogen

do not allow H21

[5]

(a) (iron) is a metal

accept transition element

allow (iron) had different properties (to oxygen and sulfur)

ignore electrons1

24

(b) so that elements with similar properties could be placed together

allow to make the pattern fit

ignore undiscovered elements1

(c) atomic number(s)

allow proton number(s)1

(d) all have one electron in the outer shell (highest energy level)

allow same number of electrons in the outer shell (highest energylevel)

1

(so they) have similar propertiesorreact in the same way

allow specific reactions e.g. with water1

[5]

(a) increase125


(b) (i) Na+ and Br−

both required1

(ii) sodium chloride

allow NaCl

do not allow sodium chlorine1

(iii) chlorine is more reactive than bromine

allow converse argument

allow symbols Cl, Cl2, Br and Br2

allow chlorine / it is more reactive

do not allow chloride or bromide1

(iv) fluorine

allow F / F2.

do not allow fluoride.1

[5]

(a) Li and K

either order

allow lithium and potassium1

26

(b) Fe

allow iron1

(c) N and As

either order

allow nitrogen and arsenic1

(d) Cu

allow copper1

[4]

(a) (i) Neutron (top label)127

Electron (bottom label)1

(ii) 131

(iii) electrons1


(b) (i) compound1

hydrogen1

bond1

(ii) C4H101

[8]

(a) Sulfur dioxide causes acid rain.128

(b) red / orange / yellow

do not accept any other colours1

because sulfur dioxide (when in solution) is an acid1

(c) (there are) weak forces (of attraction)

do not accept any reference to covalent bonds breaking1

between the molecules

do not accept any other particles1

(these) take little energy to overcome

award third mark only if first mark given1


(d) Marks awarded for this answer will be determined by the Quality of Communication(QC) as well as the standard of the scientific response. Examiners should also referto the information on page 5 and apply a ‘best-fit’ approach to the marking.

0 marksNo relevant content

Level 1 (1 – 2 marks)A relevant comment is made about the data.

Level 2 (3 – 4 marks)Relevant comparisons have been made, and an attempt made at a conclusion.

Level 3 (5 – 6 marks)Relevant, detailed comparisons made and a justified conclusion given.

examples of the points made in the response

effectiveness

• W removes the most sulfur dioxide• D removes the least sulfur dioxide

material used

• Both W and D use calcium carbonate• Calcium carbonate is obtained by quarrying which will create scars on

landscape / destroy habitats• D requires thermal decomposition, this requires energy• D produces carbon dioxide which may cause global warming / climate change• S uses sea water, this is readily available / cheap

waste materials

• W product can be sold / is useful• W makes carbon dioxide which may cause global warming / climate change• D waste fill landfill sites• S returned to sea / may pollute sea / easy to dispose of

6

[12]

(a) (i) an electron129

(ii) a neutron1

(iii) 111

(iv) boron1

(b) (i) GH31


(ii) covalent1

[6]

(a) (i) Na

allow sodium / phonetic spelling

if more than one answer is given apply list principle1

30

(ii) Fe

allow iron / phonetic spelling


(iii) Na or S

allow sodium or sulfur / sulphur / phonetic spelling


(iv) S

allow sulfur / sulphur / phonetic spelling


(v) Na

allow sodium / phonetic spelling


(b) (i) any three from:

• effervescence / fizzing or bubbles or gas produced

do not allow incorrectly named gas• sodium melts or turns into a ball• sodium moves (on the surface)• steam / mist / vapour is produced

ignore heat / temperature / flame / spark• sodium gets smaller / disappears

allow dissolves• colour of indicator is darker / more intense near the sodium

Must be linked to near the sodium.3

(ii) hydroxide or OH–

allow OH without a charge

do not allow OH+

1


(c)

diagram showing electron configuration of ion is 2,81

charge on ion is +

Bracket not necessary

[2,8]+ is worth 1 mark as there is no diagram1

[11]

(a) (i) points correctly plotted ( ± ½ small square)

four points = 2 marks

three points = 1 markMax 2

31

straight line of best fit using full range of points from 0,01

(ii) any one from:

must explain why the point is below the line

• the solution may not have been properly stirred• the electrodes may have been a larger distance apart• the drop of sodium chloride may have been a smaller volume / smaller

allow not enough sodium chloride added

allow smaller amount of sodium chloride

do not allow too few drops added

ignore the student may have misread the conductivity meter1

(iii) any one from:

• the volume of pure water

allow amount• the concentration (of the solutions added)• the volume (of the drops) of solution added

ignore number of drops• the distance between the electrodes• the same electrodes or electrodes made of the same material• same depth or surface area of electrodes in the water• constant power supply

ignore current• stirred

1


(b) (i) because (pure) water is covalent / molecular (simple) or contains molecules1

therefore (pure) water has no free / mobile electrons or ions

molecules do not have a charge or molecules do not contain ionsgains 2 marks

1

(ii) because there are ions in sodium chloride

allow Na+ and / or Cl–(ions) or ionic bonding.

Ignore particles other than ions for MP1.1

which can move or carry the current / charge

MP2 must be linked to ions only.1

(iii) Hydrogen

allow H2 / H1

[10]

(a) (i) any one from:

• one electron in the outer shell / energy level• form ions with a 1+ charge

1

32

(ii) any one from:

• hydrogen is a non-metal• (at RTP) hydrogen is a gas• hydrogen does not react with water• hydrogen has only one electron shell / energy level• hydrogen can gain an electron or hydrogen can form a negative / hydride

/ H–ion• hydrogen forms covalent bonds or shares electrons

accept answers in terms of the Group 1 elements1

(b) (i) (bromine) gains electrons

it = bromine

do not accept bromide ion gains electrons

ignore loss of oxygen1

(ii) I2must both be on the right hand side of the equation

1


+ 2e–

2I– – 2e– ➔ I2 for 2 marks1

(iii) fluorine is the smallest atom in Group 7 or has the fewest energy levels inGroup 7 or has the smallest distance between outer shell and nucleus

the outer shell must be mentioned to score 3 marks1

fluorine has the least shielding or the greatest attraction between the nucleusand the outer shell

1

therefore fluorine can gain an electron (into the outer shell) more easily1

[8]

(a) (i) copper is less reactive than hydrogen or copper is unreactive133

(ii) Zinc and dilute hydrochloric acid1

(b) (gas) syringe1

(c) (i) 35

allow 31

because not close to others

accept it is much lower than the others

ignore references to trends or patterns

dependent on the first mark1

(ii) (49 + 50 + 48) / 3

= 49

correct answer with or without working gains 2 marks1

allow ecf from anomaly identified in (i) for 2 marks:

• Exp 1 anomalous gives 43.3

• Exp. 2 anomalous gives 44

• Exp. 4 anomalous gives 44.7

answer of 45.5 or 46 (anomaly not excluded) gains 1 mark

correct working excluding anomaly but with wrong answer gains 1mark

1


(iii) so that a mean can be calculated

accept improves accuracy of the mean or so anomalies can beidentified / discarded or to reduce effect of random errors

ignore makes it a fair test

ignore reliability, validity, repeatability, reproducibility1

(d) (i) idea of mixing with oxygen / air, letting air / oxygen in

accept converse1

(ii) H2O

do not accept incorrect additional products1

balancing 2 … (1) … 2

allow fractions or multiples

dependent on first mark1

[11]

(a) (i) a proton134

(ii) nucleus1

(iii) 12

order must be correct1

41

(b) (i) 5 / five (%)1

(ii) Carbon dioxide > global warming1

Sulfur dioxide > acid rain1


Water > no pollution

1

[8]

(a) weaker bonds

allow (other substances) react with the silicon dioxide

or

fewer bonds

ignore weaker / fewer forces

or

disruption to lattice

do not accept reference to intermolecular forces / bonds1

35

(b) (i) Na2O

do not accept brackets or charges in the formula1

(ii)

electrons can be shown as dots, crosses, e or any combination

2 bonding pairs

accept 4 electrons within the overlap1

2 lone pairs on each oxygen

accept 4 non-bonding electrons on each oxygen1


(c) lattice / regular pattern / layers / giant structure / close-packed arrangement1

(of) positive ions or (of) atoms1

(with) delocalised / free electrons

reference to incorrect particles or incorrect bonding or incorrectstructure = max 2

1

[7]


C1 Atomic Structure and Periodic Name:...

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