C2 f revision pack by Isaac Newton Academy

Chemistry Unit C2 Discovering Chemistry Study and Revision Pack (Foundation))

Contents C2 Topic 1 ........................................................................................................................................ 2 Specification Statements .............................................................................................................. 2 C2 Topic 1 Exam Questions ......................................................................................................... 3 C2 Topic 2 ........................................................................................................................................ 8 Specification Statements .............................................................................................................. 8 C2 Topic 2 Exam Questions ....................................................................................................... 10 C2 Topic 3 ...................................................................................................................................... 14 Specification Statements ............................................................................................................ 14 C2 Topic 3 Exam Questions ....................................................................................................... 15 C2 Topic 4 ...................................................................................................................................... 21 Specification Statements ............................................................................................................ 21 C2 Topic 4 Exam Questions ....................................................................................................... 23 C2 Topic 5 ...................................................................................................................................... 27 Specification Statements ............................................................................................................ 27 C2 Topic 5 Exam Questions ....................................................................................................... 27 C2 Topic 6 ...................................................................................................................................... 33 Specification Statements ............................................................................................................ 33 C2 Topic 6 Exam Questions ....................................................................................................... 34

C2 Topic 1 Specification Statements Learning objectives I can: 1.1 Explain how Mendeleev: a arranged the elements, known at that time, in a periodic table by using properties of these elements and their compounds b used his table to predict the existence and properties of some elements not then discovered 1.2 Classify elements as metals or non-‐metals according to their position in the periodic table HSW 2 Describe the importance of creative thought in the development of hypotheses and theories 1.3 Describe the structure of an atom as a nucleus containing protons and neutrons, surrounded by electrons in shells (energy levels) 1.4 Demonstrate an understanding that the nucleus of an atom is very small compared to the overall size of the atom 1.5 Describe atoms of a given element as having the same number of protons in the nucleus, where this number is unique to that element 1.6 Recall the relative charge and relative mass of: a a proton b a neutron c an electron 1.7 Demonstrate an understanding that atoms contain equal numbers of protons and electrons HSW 2 Describe how data is used by scientists to provide evidence that increases our scientific understanding 1.8 Explain the meaning of the terms: a atomic number b mass number c relative atomic mass 1.9 Describe the arrangement of elements in the periodic table such that: a elements are arranged in order of increasing atomic number, arranged in rows called periods b elements with similar properties are placed in the same vertical column, called groups HSW 14 Describe how scientists share data and discuss new ideas, and how over time this process helps to reduce uncertainties and revise scientific theories 1.12 Apply rules about the filling of electron shells (energy levels) to predict the electronic configurations of the first 20 elements in the periodic table, given the atomic numbers, as diagrams and in the form 2.8.1 1.13 Describe the connection between the number of outer electrons and the position of an element in the periodic table HSW 11 Present information using scientific conventions and symbols

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C2 Topic 1 Exam Questions 35 marks, 35 minutes Q1. Most atoms contain electrons, protons and neutrons. (a) Describe the positions of these particles in atoms. (3) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (b) A chlorine atom contains 17 electrons. What is the electronic configuration of a chlorine atom? Put a cross ( ) in the box next to your answer. (1) A B C D

10.7 8.8.1 17 2.8.7

(c) Chlorine and bromine are in the same group in the periodic table. (i) Explain, in terms of electrons, why these elements are placed in the same group. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (ii) Describe the appearance of bromine at room temperature and pressure. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. ..............................................................................................................................................

(d) An experiment was carried out to see how large a nucleus is compared to the overall size of an atom. In the experiment a very large number of positively charged particles are fired at a thin sheet of gold. When one of these positively charged particles comes close to the nucleus of a gold atom it is repelled. Explain why only about 1 in every 20 000 positively charged particles are repelled. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (Total for Question is 10 marks) Q2. (a) The diagram shows an atom of lithium. (i) A proton has been labelled. Complete the diagram by labelling the other two particles shown. (2)

(ii) Complete the sentence by putting a cross ( The atomic number of lithium is

) in the box next to your answer. (1)

A B C D

3 6 7 10

(b) (i) Which row of the table shows the charge on a proton and the charge on an electron? Put a cross ( ) in the box next to your answer. (1) %%% A B C D

proton positive negative negative positive

electron positive negative positive negative

(ii) Use a number from the box to complete the sentence.

The relative mass of a proton is . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . (1) (c) The electronic configuration of lithium is 2.1. The electronic configuration of sodium is 2.8.1. (i) Explain, in terms of their electronic configurations, why lithium and sodium are both in group 1 of the periodic table. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (ii) Explain, in terms of their electronic configurations, why lithium is placed in period 2 and sodium is placed in period 3 of the periodic table. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (Total for Question is 9 marks)

Q3. Elements Mendeleev produced the first periodic table. In a version of his periodic table, he put these elements in group 1. hydrogen lithium sodium potassium copper rubidium silver caesium gold (a) Some of the elements in this list are also in group 1 of the modern periodic table. Which element is in the list above and also in group 1 of the modern periodic table? Put a cross ( ) in the box next to your answer. (1) A B C D

gold silver copper sodium

(b) The element francium is now included in group 1 of the modern periodic table but did not appear anywhere in Mendeleevâ&#x20AC;&#x2122;s periodic table. Suggest why francium was not in Mendeleevâ&#x20AC;&#x2122;s periodic table. (1) .............................................................................................................................................. .............................................................................................................................................. (c) Explain why hydrogen is not included in group 1 in most versions of the modern periodic table. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (d) The atomic number and electronic configurations of three elements are shown in the table below. element lithium sodium potassium

atomic number

electronic configuration

3 11 19

2.1 2.8.1 2.8.8.1

Describe how the electronic configuration of sodium shows the group and period of sodium in the periodic table. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. 6

*(e) An atom of beryllium has an atomic number of 4 and a mass number of 9. Describe the numbers and arrangements of the protons, neutrons and electrons in this atom. (6) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. Q4. Explain why hydrogen is not included in group 1 in most versions of the modern periodic table. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. Q5. The atomic number of oxygen is 8. The mass number of an atom of oxygen is 17. Describe the number and type of particles in the nucleus of this atom. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. ..............................................................................................................................................

C2 Topic 2 Specification Statements Learning objectives

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2.1 Demonstrate an understanding that atoms of different elements can combine to form compounds by the formation of new chemical bonds

2.2 Describe how ionic bonds are formed by the transfer of electrons to produce cations and anions

2.3 Describe an ion as an atom or group of atoms with a positive or negative charge

2.4 Describe the formation of sodium ions, Na+, and chloride ions, Cl–, and hence the formation of ions in other ionic compounds from their atoms, limited to compounds of elements in groups 1, 2, 6 and 7

HSW 11 Present information using scientific conventions and symbols

2.5 Demonstrate an understanding of the use of the endings ‘–ide’ and ‘– ate’ in the names of compounds

2.6 Deduce the formulae of ionic compounds (including oxides, hydroxides, halides, nitrates, carbonates and sulfates) given the formulae of the constituent ions

2.8 Describe the properties of ionic substances including sodium chloride and magnesium oxide, limited to:

b their ability to conduct electricity as solids, when molten and in aqueous solution

HSW 12 Describe the benefits, drawbacks and risks of using new scientific and technological developments

2.9 Recall the general rules which describe the solubility of common types of substances in water:

b all nitrates are soluble

c common chlorides are soluble except those of silver and lead

d common sulfates are soluble except those of lead, barium and calcium

e common carbonates and hydroxides are insoluble except those of sodium, potassium and ammonium

2.10 Demonstrate an understanding that insoluble salts can be formed as precipitates by the reaction of suitable reagents insolution

HSW 10 Use qualitative and quantitative approaches when presenting scientific ideas and arguments, and recording observations

2.11 Demonstrate an understanding of the method needed to prepare a pure, dry sample of an insoluble salt

2.12 Prepare an insoluble salt by precipitation

2.13 Use solubility rules to predict whether a precipitate is formed when named solutions are mixed together and to name the precipitate

I can:

a melting points and boiling points

a all common sodium, potassium and ammonium salts are soluble

2.14 Recall that the insoluble salt, barium sulfate, is given as a

b it is safe to use as, although barium salts are toxic, its insolubility prevents it entering the blood

HSW 5 Plan to test a scientific idea, answer a scientific question or solve a scientific problem

2.15 Describe tests to show the following ions are present in solids or solutions:

b CO3 2− using dilute acid and identifying the carbon dioxide evolved

c SO4 2−using dilute hydrochloric acid and barium chloride solution

d Cl− using dilute nitric acid and silver nitrate solution

2.16 Recall that chemists use spectroscopy to detect the presence of very small amounts of elements and that this led to the discovery of new elements, including rubidium and caesium

HSW 2 Describe how data is used by scientists to provide evidence that increases our scientific understanding

a it is opaque to X-‐rays

a Na+, K+, Ca2+, Cu2+ using flame tests

C2 Topic 2 Exam Questions 33 marks 33 minutes

Q1. (a) Barium sulfate contains

barium ions, Ba2+ sulfate ions, SO42â&#x20AC;&#x201C;

(i) Give the formula of barium sulfate. (1) .............................................................................................................................................. (ii) Give the meaning of the term ion. (1) .............................................................................................................................................. .............................................................................................................................................. (b) This is an X-ray photograph of part of a patient's body. Before the photograph was taken a suspension of barium sulfate was introduced into his body to show the required part.

Many barium salts are toxic. Barium sulfate is insoluble in water. Explain why it is safe for the patient to have barium sulfate in his body. (2) .............................................................................................................................................. .............................................................................................................................................. ..............................................................................................................................................

*(c) Barium sulfate is prepared by reacting barium chloride with sodium sulfate. The barium sulfate is formed as a precipitate. Describe an experiment to prepare a pure, dry sample of barium sulfate, starting with barium chloride crystals and sodium sulfate crystals. (6) .............................................................................. .............................................................................. .............................................................................. .............................................................................. .............................................................................. .............................................................................. .............................................................................. .............................................................................. .............................................................................. .............................................................................. .............................................................................. (d) Barium reacts with chlorine to produce barium chloride, BaCl2. Write the balanced equation for this reaction. (2) .............................................................................. ..................... (Total for Question = 12 marks) Q2. Calcium chloride solution reacts with silver nitrate solution. Solid silver chloride and calcium nitrate solution are formed. (i) Complete the sentence by putting a cross ( The formula of a salt is Ca(NO3)2. The name of this salt is

) in the box next to your answer. (1)

A B C D

calcium nitride calcium nitrate calcium chloride silver nitrate

(ii) The mixture produced in the reaction is filtered to obtain the silver chloride. The solid silver chloride is washed with water and left to dry. The yield of dry silver chloride was 3.0 g. The theoretical yield of dry silver chloride in this experiment was 4.0 g. 1. Suggest why the yield was less than 4.0 g. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. 2. Calculate the percentage yield of this experiment. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. 11

Q3. Lead iodide is an insoluble salt. Use words from the box to complete the sentences. Each word may be used once, more than once, or not at all. (4) dried

filtered

gas

metal

precipitate

solution

(i) Lead iodide can be prepared by mixing potassium iodide solution and lead nitrate . . . . . . . . . . . (ii) The lead iodide forms as a solid . . . . . . . . . . . . . . . . . . . . (iii) To separate the solid lead iodide, the mixture is . . . . . . . . . . . . . . . . . . . . (iv) To obtain a pure sample of solid lead iodide, the solid is washed and then . . . . . . . . . . . . . . . . Q4. Magnesium flares provide a bright light in an emergency. When the magnesium burns it reacts with oxygen to form magnesium oxide. (a) Explain why magnesium oxide is a compound. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (b) When magnesium reacts with oxygen, one magnesium atom and one oxygen atom form one magnesium ion and one oxide ion. These diagrams show the arrangement of electrons in a magnesium atom and in a magnesium ion.

(i) In the diagram below the arrangement of electrons in an oxygen atom is given. Draw the arrangement of electrons in the oxide ion. (1)

(ii) Explain, in terms of their electrons, how a magnesium atom, Mg, and an oxygen atom, O, react together to form a magnesium ion, Mg2+, and an oxide ion, O2â&#x20AC;&#x201C;. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (iii) Magnesium oxide is an ionic compound. Which of these is a property of solid magnesium oxide? Put a cross ( ) in the box next to your answer. (1) A B C D

it has a high melting point it has a low boiling point it conducts electricity it is malleable

*(c) You are given two solid sodium salts, which are unlabelled. One of the solids is sodium chloride. The other solid is sodium carbonate. Describe how you could carry out a flame test to show that they are both sodium salts and describe another test to identify one of the salts completely. (6) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (Total for Question is 12 marks)

C2 Topic 3 Specification Statements Learning objectives I can:

I can do this very well

I can do this quite well

I need to do m ore work on this

3.1 Describe a covalent bond as a pair of electrons shared between two atoms

3.2 Recall that covalent bonding results in the formation of molecules

3.3 Explain the formation of simple molecular, covalent substances using dot and cross diagrams, including:

b hydrogen chloride

c water

d methane

f carbon dioxide

HSW 1 Present information using scientific conventions and symbols

3.5 Describe the properties of typical simple molecular, covalent compounds, limited to:

b poor conduction of electricity

3.6 Demonstrate an understanding of the differences between the properties of simple molecular, covalent substances and those of giant molecular, covalent substances, including diamond and graphite

HSW 3 Describe how phenomena are explained using scientific models

3.4 Classify different types of elements and compounds by investigating their melting points and boiling points, solubility

3.8 Describe the separation of two immiscible liquids using a separating funnel

3.9 Describe the separation of mixtures of miscible liquids by fractional distillation, by referring to the fractional distillation of liquid air to produce nitrogen and oxygen

HSW 5 Plan to test a scientific idea, answer a scientific question or solve a scientific problem

3.10 Describe how paper chromatography can be used to separate and identify components of mixtures, including colouring agents in foodstuffs

3.11 Evaluate the information provided by paper chromatograms, including the calculation of Rf values, in a variety of contexts, such as the food industry and forensic science

HSW 4 Identify questions that science cannot address and explain why these questions cannot be addressed.

a hydrogen

a low melting points and boiling points, in terms of weak forces between molecules

in water and electrical conductivity (as solids and in solution) including sodium chloride, magnesium sulfate, hexane, liquid paraffin, silicon(IV) oxide, copper sulfate, and sucrose (sugar)

C2 Topic 3 Exam Questions 35 marks 35 minutes (a) A separating funnel is shown.

The separating funnel can be used to separate two immiscible liquids, such as oil and water. Describe how you would use a separating funnel to separate two immiscible liquids. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (b) Paper chromatography can be used to separate coloured substances. A student carried out a chromatography experiment on four food colourings. The four food colourings were brown, green, yellow and red. The diagram shows the results.

Use the results of the chromatography experiment to describe the colours present in the brown food colouring. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (c) An experiment is carried out on two solutions to see if they conduct electricity. The apparatus used is shown.

The two solutions used are sodium chloride solution and sucrose solution. Sodium chloride is an ionic compound. Sucrose is a simple molecular, covalent compound. Explain what happens when each solution is tested in the circuit shown. (3) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (d) Calculate the relative formula mass of water, H2O. (Relative atomic masses: H = 1.0, O = 16) (1) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (Total for Question = 8 marks)

Q2. (a) Some food colourings are a mixture of coloured substances. Paper chromatography can be used to separate the coloured substances in food colourings. Charles carried out a chromatography experiment to test which food colouring was present in a coloured drink. He used samples of three food colourings, X, Y and Z. He also tested a sample of the colouring in the drink. Charles obtained this chromatogram.

(i) Charles looked at the chromatogram to find out which food colourings contained more than one coloured substance. State all the food colourings that contain more than one coloured substance. (1) .............................................................................................................................................. (ii) Food colouring Y is banned. Explain how Charles can tell that the drink that he tested did not contain the banned food colouring. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (iii) Calculate the Rf value for the coloured substance in food colouring X.

(2)

*(b) Describe in detail how the experiment should be carried out to produce the chromatogram shown in (a). (6) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (c) The drink contained water. Complete the dot and cross diagram for water by adding the electrons of the hydrogen atoms. (1)

(Total for Question is 12 marks)

Q3. (a) Hydrogen chloride is a gas at room temperature. The diagram shows the outer shell electrons in a molecule of hydrogen chloride.

(i) Give the name of the type of bond between the hydrogen and chlorine atoms in the molecule. (1) .............................................................................................................................................. (ii) Give the formula of a molecule of hydrogen chloride. (1) ..............................................................................................................................................

(iii) Complete the sentence by putting a cross ( A property of hydrogen chloride is that it

) in the box next to your answer. (1)

A B C D

conducts electricity has a high melting point has a low boiling point exists as a giant structure

(b) Hydrogen, H2, reacts with fluorine, F2, to form hydrogen fluoride, HF. Write the balanced equation for the reaction. (2) .............................................................................................................................................. *(c) Methane is a gas at room temperature. It exists as molecules, CH4. Methane has a low boiling point. It does not conduct electricity. Explain, in terms of the nature of its molecules and the forces between its molecules, why methane has a low boiling point and does not conduct electricity. (6) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (Total for Question is 11 marks)

Q4. The diagram shows part of the structure of diamond.

Complete the sentences by putting a cross ( ) in the box next to your answer. (i) The bonds between carbon atoms in diamond contain (1) A protons B neutrons C electrons D ions (ii) The structure of diamond is (1) A B C D

simple molecular, covalent giant molecular, covalent ionic metallic

Q5. The apparatus shown can be used to test the electrical conductivity of liquids.

Describe how you would use this apparatus to show that the electrical conductivity of hexane is that of a typical simple molecular, covalent compound. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. ..............................................................................................................................................

C2 Topic 4 Specification Statements Learning objectives

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b simple molecular covalent

c giant molecular covalent

d metallic; and that each type of substance has different physical properties, including relative melting point and boiling point, relative solubility in water and ability to conduct electricity (as solids and in solution)

HSW 3 Describe how phenomena are explained using scientific models

4.1 Classify elements as … transition metals based on their position in the periodic table

4.2 Describe the structure of metals as a regular arrangement of positive ions surrounded by a sea of delocalised electrons

4.3 Describe and explain the properties of metals, limited to malleability and the ability to conduct electricity

4.4 Recall that most metals are transition metals and that their typical properties include:

b the formation of coloured compounds

HSW 13 Explain how and why decisions about uses of science and technology are made

4.1 Classify elements as alkali metals (group 1) ... based on their position in the periodic table

4.6 Describe alkalia metal as:

b metals with comparatively low melting points

4.7 Describe the reactions of lithium, sodium and potassium with water to form hydroxides which are alkaline, and hydrogen gas

4.8 Describe the pattern in reactivity of the alkali metals lithium, sodium, and potassium with water and use this pattern to predict

HSW 2 Describe how data is used by scientists to provide evidence that increases our scientific understanding

4.1 Classify elements as … halogens (group 7)… based on their position in the periodic table

4.9 Recall the colours and physical states of the halogens at room temperature

4.10 Describe the reactions of halogens with metals to form metal halides

I can: 4.5 Demonstrate an understanding that elements and compounds can be classified as: a ionic

a high melting point

a soft metals

the reactivity of other alkali metals

HSW 13 Explain how and why decisions that raise ethical issues about uses of science and technology are made

4.12 Investigate displacement reactions of halogens reacting with halide ions in solution

4.11 Recall that halogens react with hydrogen to produce hydrogen halides, which dissolve in water to form acidic solutions

4.13 Describe the relative reactivity of the halogens as shown by their displacement reactions with halide ions in aqueous solution

HSW 7 Work safely, individually and with others, when collecting first-‐ hand data

4.1 Classify elements as … noble gases (group 0) … based on their position in the periodic table

4.14 Describe the noble gases as chemically inert, compared with the other elements and demonstrate an understanding that this lack of reactivity can be explained by the electronic arrangements in their atoms

4.15 Demonstrate an understanding that the discovery of the noble gases was due to chemists:

c performing experiments to test this hypothesis and show the presence of the noble gases

4.16 Relate the uses of the noble gases to their properties, including:

b low density

c non-‐flammability

4.17 Use the pattern in a physical property of the noble gases, such as boiling point or density, to estimate an unknown value for another member of the group

a noticing that the density of nitrogen made in a reaction differed from that of nitrogen obtained from air b developing a hypothesis about the composition of the air

a inertness

C2 Topic 4 Exam Questions 25 Marks 25 Minutes

Q1. Complete the balanced equation for the reaction of iron with chlorine to form iron chloride. (2) ..................... Fe +..................... Cl2 2FeCl3 Q2. The table shows the states and colours of three of these elements at room temperature. The information for chlorine is missing. colour at room state at room temperature element temperature fluorine gas pale yellow chlorine bromine liquid dark red iodine solid grey Use the information in the table to describe the appearance of chlorine at room temperature. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. Q3. Group 7 (a) The elements fluorine, chlorine, bromine and iodine are all in group 7 of the periodic table. (i) State the name given to the elements in group 7. (1) .............................................................................................................................................. (ii) Give the symbol for an atom of bromine. (1) .............................................................................................................................................. (b) The table shows the states and colours of three of these elements at room temperature. The information for chlorine is missing. colour at room state at room temperature element temperature fluorine gas pale yellow chlorine bromine liquid dark red iodine solid grey Use the information in the table to describe the appearance of chlorine at room temperature. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. ..............................................................................................................................................

*(c) When chlorine is added to a solution of potassium bromide, a colour change is seen. When chlorine is added to a solution of potassium fluoride, no colour change is seen. Explain how these observations provide evidence for the order of reactivity of bromine, chlorine and fluorine. (6) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. Q4. The elements lithium, sodium and potassium are all in the same group of the periodic table. (a) Complete the sentence by putting a cross ( ) in the box next to your answer. These elements are in (1) A B C D

group 0 group 1 group 2 group 7

(b) Give the symbol of an atom of another element that is in the same group of the periodic table as lithium, sodium and potassium. (1) .............................................................................................................................................. (c) The table shows the relative hardness and melting points of the three alkali metals, lithium, sodium and potassium, and the three transition metals, iron, copper and nickel. metal lithium sodium potassium iron copper nickel

relative hardness 0.6 0.4 0.5 5.0 3.0 4.0

melting point / 째C 181 98 63 1535 1083 1455

Alkali metals and transition metals have different typical properties. Draw one straight line from alkali metals and one from transition metals to their typical properties. (2)

(d) Potassium reacts with water. In a class demonstration, a teacher drops a piece of potassium on to water.

(i) The teacher ties back her hair and wears a laboratory coat and goggles. Suggest another safety precaution that the teacher should take. (1) .............................................................................................................................................. .............................................................................................................................................. (ii) The word equation for this reaction is given below. Two of the state symbols have been given. Write the other two state symbols in the spaces provided. (2) potassium(s) + water (l) â&#x2020;&#x2019; potassium hydroxide(. . . . . . . . .) + hydrogen(. . . . . . . . .)

(iii) Describe what you see when potassium is added to water. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (iv) Balance the equation for the reaction between potassium and water by putting numbers in the spaces provided. (2) . . . . . . . . . K + 2H2O â&#x2020;&#x2019; . . . . . . . . . KOH + H2 (Total for Question is 11 marks)

C2 Topic 5 Specification Statements Learning objectives I can:

I can do this very well

I can do this quite well

I need to do m ore work on this

5.1 Measure temperature changes accompanying some of the following types of change:

b neutralisation reactions

c displacement reactions

d precipitation reactions

5.2 Define an exothermic change or reaction as one in which heat energy is given out

5.3 Define an endothermic change or reaction as one in which heat energy is taken in

5.4 Describe the breaking of bonds as endothermic and the making of bonds as exothermic

5.5 Demonstrate an understanding that the overall heat energy change for a reaction is:

HSW 3 Describe how phenomena are explained using scientific models

5.7 Investigate the effect of temperature, concentration and surface area of a solid on the rate of a reaction such as hydrochloric acid and marble chips

5.8 Recall that the rates of chemical reactions vary from very fast, explosive reactions to very slow reactions

5.9 Describe the effect of changes in temperature, concentration and surface area of a solid on the rate of reaction

HSW 11 Present information using scientific conventions and symbols

5.10 Describe how reactions can occur when particles collide H and explain how rates of reaction are increased by

H 5.11 Demonstrate an understanding that not all collisions lead to a reaction, especially if particles collide with low energy

5.12 Recall the effect of a catalyst on the rate of reaction

5.13 Demonstrate an understanding that catalytic converters in cars:

b work best at high temperatures

HSW 13 Explain how and why decisions about uses of science and technology are made

a salts dissolving in water

a exothermic if more heat energy is released making bonds in the products than is required to break bonds in the reactants b endothermic if less heat energy is released making bonds in the products than is required to break bonds in the reactants

increasing the frequency and/or energy of collisions

a have a high surface area to increase the rate of reaction of carbon monoxide and unburnt fuel from exhaust gases with oxygen from the air to produce carbon dioxide and water

C2 Topic 5 Exam Questions 34 Marks 34 Minutes 27

Q1. Catalysts are added to some reactions. (i) Explain what a catalyst is. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (ii) Explain the benefits of using catalytic converters in car exhaust systems. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. Q2. Zinc is a metal. Zinc reacts with dilute hydrochloric acid to produce zinc chloride and hydrogen. (a) Write the word equation for the reaction of zinc with dilute hydrochloric acid. (1) .............................................................................................................................................. (b) A student wanted to investigate the speed of the reaction between zinc and dilute hydrochloric acid. Describe how the student could use this apparatus to obtain the results in the table.

time after start of experiment / minutes 0 1 2 3

volume of hydrogen produced / cm3 0 30 42 50 (3)

.............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (c) Complete each sentence by putting a cross (

) in the box next to your answer.

(i) For a reaction to take place the reacting particles must 28

(1) A B C D

dissolve boil collide evaporate

(ii) The reaction can be slowed down by (1) A B C D

using a bigger volume of the same acid cooling the hydrochloric acid increasing the concentration of the hydrochloric acid adding a catalyst

(d) When zinc powder is used, instead of larger pieces of zinc, the reaction is faster. Explain, using ideas about particles, why the reaction is faster when zinc powder is used. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (e) The reaction is exothermic. Describe how you could prove that this reaction is exothermic. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (Total for Question is 10 marks) Q3. Some people use a hand warmer to warm their hands in winter.

(a) A chemical reaction takes place in the hand warmer. This reaction gives out heat energy. Give the name for reactions that give out heat energy. (1) ..............................................................................................................................................

(b) In the hand warmer, iron reacts with oxygen. Complete the word equation for this reaction. (2) iron + . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . â&#x2020;&#x2019; . . . . . . . . . . . . . . . . . . . . . . . . . . . . . (c) Some hand warmers contain sodium chloride mixed with the reactants. If sodium chloride is present, it is not used up but the chemical reaction is faster. Complete the sentence by putting a cross ( ) in the box next to your answer. In this reaction the sodium chloride is acting as (1) A B C D

a precipitate a catalyst an element an alkali metal

(d) When ammonium nitrate crystals are dissolved in water, heat energy is taken in. A student puts some water in a beaker. He puts a thermometer in the water. He adds some ammonium nitrate crystals and stirs the mixture. Describe what the student would see. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (e) In an experiment, the time taken for some potassium chloride crystals to dissolve in water has been measured. A student is given the same mass of potassium chloride to dissolve in the same volume of water. State one change that could be made to the potassium chloride crystals and one change that could be made to the water to make the dissolving faster. (2) change made to the potassium chloride crystals .............................................................................................................................................. .............................................................................................................................................. change made to the water .............................................................................................................................................. .............................................................................................................................................. (Total for Question is 8 marks)

Q4. (a) A technician made some dilute sodium hydroxide solution by carefully adding some solid sodium hydroxide to pure water. This is the hazard symbol on a bottle of solid sodium hydroxide.

(i) State what this symbol shows about sodium hydroxide. (1) .............................................................................................................................................. (ii) Sodium hydroxide solution reacts with dilute hydrochloric acid. During the reaction heat is released. What type of reaction is this? Put a cross (

) in the box next to your answer. (1)

A B C D

displacement endothermic neutralisation precipitation

(b) A catalyst is added to some reactions. Explain the meaning of catalyst. (2) .............................................................................................................................................. .............................................................................................................................................. ..............................................................................................................................................

(c) Dilute hydrochloric acid reacts with calcium carbonate to produce carbon dioxide gas. Three different experiments were carried out using large pieces of calcium carbonate, small pieces of calcium carbonate and powdered calcium carbonate. The size of the calcium carbonate pieces was the only factor that was changed. In each experiment the volume of carbon dioxide released in five minutes was measured. The results are

Describe what this shows about the effect of the surface area of calcium carbonate on the rate of this reaction. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. *(d) Hydrochloric acid reacts with magnesium metal to produce hydrogen gas. magnesium + hydrochloric acid â&#x2020;&#x2019; magnesium chloride + hydrogen Describe how you could use magnesium ribbon and a solution of hydrochloric acid to show that decreasing the concentration of the hydrochloric acid changes the rate of this reaction. (6) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (Total for Question = 12 marks)

C2 Topic 6 Specification Statements Learning objectives I can: 6.1 Calculate relative formula mass given relative atomic masses 6.2 Calculate the formulae of simple compounds from reacting masses and understand that these are empirical formulae HSW 11 Present information using scientific conventions and symbols 6.3 Determine the empirical formula of a simple compound, such as magnesium oxide. 6.4 Calculate the percentage composition by mass of a compound from its formula and the relative atomic masses of its constituent elements HSW 10 Use qualitative and quantitative approaches when presenting scientific ideas and arguments, and recording observations 6.6 Recall that the yield of a reaction is the mass of product obtained in the reaction 6.7 Demonstrate an understanding that the actual yield of a reaction is usually less than the yield calculated using the chemical equation (theoretical yield) 6.8 Calculate the percentage yield of a reaction from the actual yield and the theoretical yield 6.9 Demonstrate an understanding of the reasons why reactions do not give the theoretical yield due to factors, including: a incomplete reactions b practical losses due to the preparation c competing, unwanted reactions HSW 12 Describe the benefits, drawbacks and risks of using new scientific and technological developments 6.10 Demonstrate an understanding that many reactions produce waste products which: a are not commercially useful b can present economic, environmental and social problems for disposal HSW 13 Describe the social, economic and environmental effects of decisions about the uses of science and technology

I can do this very well

I can do this quite well

I need to do m ore work on this

C2 Topic 6 Exam Questions 20 Marks 20 Minutes

Q1. Calcium chloride solution reacts with silver nitrate solution. Solid silver chloride and calcium nitrate solution are formed. (i) Complete the sentence by putting a cross ( ) in the box next to your answer. The formula of a salt is Ca(NO3)2. The name of this salt is (1) A B C D

calcium nitride calcium nitrate calcium chloride silver nitrate

(a) Which of these hazard symbols should be on a cylinder of chlorine to show that it is toxic? Put a cross ( ) in the box next to your answer. (1)

(b) Safety precautions must be taken when carrying out this experiment. (i) State a precaution that must be taken because chlorine is toxic. (1) .............................................................................................................................................. .............................................................................................................................................. (ii) State any other precaution that should be taken. (1) .............................................................................................................................................. .............................................................................................................................................. (c) (i) This periodic table shows the position of four elements, A, B, C and D.

Iron is a transition metal. Which letter shows the position of iron in the periodic table? ........................................... (1) (ii) State two properties of iron or its compounds which show that it is a typical transition metal. (2) Property 1: ............................................................................................................................................................ ............................................................................................................................................................ Property 2: ............................................................................................................................................................ ............................................................................................................................................................

(d) Calculate the relative formula mass of iron chloride, FeCl3. (Relative formula masses: Cl = 35.5, Fe = 56) (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. answer........................................... (e) Complete the balanced equation for the reaction of iron with chlorine to form iron chloride. (2) ..................... Fe +..................... Cl2 Ă ď&#x192; 2FeCl3 (f) In an experiment iron reacts with chlorine to produce 13.00 g of iron chloride. The theoretical yield of this reaction is calculated to be 16.25g. Calculate the percentage yield of the reaction. (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. answer........................................... Q3. (i) Calculate the relative formula mass of silver chloride, AgCl. (relative atomic masses: Cl = 35.5, Ag = 108) (1) .............................................................................................................................................. relative formula mass = . . . . . . . . . . . . . . . . . . . . (ii) Calculate the percentage by mass of silver, Ag, in silver chloride, AgCl. (relative atomic masses: Cl = 35.5, Ag = 108) (2) .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. percentage of silver = . . . . . . . . . . . . . . . . . . . . %