St Leonards College

YEAR 11 CHEMISTRY

HANDBOOK

2018

Contents

Errors Significant figuresStates of matter in equationsRevision HintsEquationsVCAA Key Skills Unit 1 VCAA Study DesignUnit 2 VCAA Study DesignAssessment TimetableUnit 1/2 Timetable

ERRORSWhen instruments are manufactured, there is a specified uncertainty within which the instrument is designed to deliver accurate results. You do not need to remember the various uncertainties of instruments exactly, however you are required to know the probable range (to within a power of 10) within which an instrument should operate. Typical uncertainties are:

pipette ± 0.02 mLburette ± 0.02 mLtop loading balances ± 0.005 g10 mL measuring cylinders ± 0.1 mL100 mL measuring cylinders ± 1 mL250 mL standard flasks ± 0.2 mL

Errors in experimental work can be classified in three categories:Gross Errors or MistakesThese are due to careless work or apparatus that is temporarily faulty. By being careful and repeating the experiment several times these errors are easily detected and eliminated.Systematic ErrorsThese result from an error in the equipment. They can be eliminated by careful calibration of the instrument.Random ErrorsThese errors arise from random variations. They cannot be eliminated, but are reduced by repeating the experiment several times and averaging the results.

SIGNIFICANT FIGURESAll of your numeric answers in the examination must be calculated to the correct number of significant figures. Generally you will lose one mark once only on your paper if your answers are incorrect to more one significant figure. Whilst one mark may not seem especially large, it is easy to express answers correctly.

The following rules will allow you to determine the correct number of significant figures. A significant figure is either an integer or a zero that follows an integer. For example:

0.0100 has three significant figures; 100 has three significant figures; 0.001 has one significant figure; 1001.0 has five significant figures; 0.0040 has two significant figures.

When determining the number of significant figures for your answer, use the smaller number of decimal places present in the values you used for the calculations.

Example: Use the Law of Conservation of Mass to calculate the mass of product formed when 1.00 g C6H12 reacts completely with 0.0442 g H2 gas. Solution: 1.00 + 0.0442 = 1.0442 = 1.04 (2 decimal places)

STATES OF MATTER IN EQUATIONSAll reactants and products in equations should have their states correctly included. This means you must use the terms (aq), (g), (s) and (l) properly. You lose one mark once only on your paper for incorrect states in equations.

REVISION HINTS

YOUR REVISION PROGRAMAs part of your revision program, you should: Memorise all the key ideas including definitions, important equations, and details of

instruments, industrial processes and cells. Go over the outcome statements in the Study Design. Go over questions you have done during the term from your text book. You should be

able to do this quite quickly. There is no need to do them all again; just select typical examples of each type. Try working out the main steps in your head to save time. Particularly select the questions with which you previously had difficulty or needed someone to show you.

The Sample Exams can be found via the CEA website, under VCE Chemistry, All papers can be downloaded from the VCAA or CEA websites. The more past examinations you do, the better your marks will be. It is not necessary to

do them as complete exams. As you revise topics, you can complete the appropriate questions, being careful to keep to the time suggested for each question. At other times you may decide that you need practice in doing multiple choice questions - 20 in 20 minutes is a good idea.

Make sure you speak to your teacher about the problems you are constantly finding. When you complete 2 or 3 papers, read your notes completely to remind yourself

regularly of the details of the course. During the weeks before the exams in June and November, this should occur at least twice a week until the exam. You should have one complete set of notes. Amalgamate all revision notes, class notes and summaries.

YOUR REVISION TIMETABLEYou should make up a revision timetable. Work backwards from your examinations. Naturally you will revise for a specific exam the night before. Be careful to allocate equal time during the prior weekend to all subjects in which you have an exam. Work backwards through the weeks before the exams.

IN THE EXAMDuring the reading time read the whole paper slowly and carefully. Do not flip back and forward. During the reading time you will slow down your pulse rate and allow your thoughts to begin to work in an ordered way. Take some deep breaths and consciously regain your full composure. By reading with understanding your mind will start to work on the problems. During this time you may also find material in one section of the paper that will assist you with a different question!Decide whether you are doing the multiple-choice or structured questions first.When completing the multiple choice questions do all questions. Do not leave any blank, even if you have to guess. Before you hand in your paper, double check that you have answered all questions. Be careful to write the correct answer in the correct box. In the extended answer section, do the question of which you are most certain first.Check the time at the end of each question.

Reread each question when you finished it and check you have answered all parts, balanced all equations, and included all states and units.If you complete your answer away from the expected section, clearly direct the marker to follow your working.Set out your answers clearly, stating the formulae you intend to use, as this often earns marks.

e.g. n (NaOH) = c x VpH = - log10 [H3O+]

FORMULAEFormulae must be memorised because no information can be taken in to the examination in your calculator memory. Your calculator must not be programmable.

n = m / M n = number of particles NA

n = cV pH = – log10 [H3O+] E = V × I × t [H3O+] = 10-pH

C.F.= (V × I × t) / T [H3O+] × [OH-] = 10-14 at 25oCAr = (relative isotopic mass x relative abundance) / total relative abundance

E = 4.184 × m × T

n amount in moles m mass in gramsM molar mass in grams per moleNA Avogadro’s Number = 6.023 × 1023

c concentration in moles per litre (M)V volume in litresQ charge in CoulombI current in ampst time in sV voltage in volts

VCAA KEY SKILLS for UNITS 1-2

Investigate and inquire scientifically• work independently and collaboratively as required to develop and apply safe and responsible work practices when completing all practical investigations including the appropriate disposal of wastes;• conduct investigations that include collecting, processing, recording and analysing qualitative and quantitative data; draw conclusions consistent with the question under investigation and the information collected; evaluate procedures and reliability of data;• construct questions (and hypotheses); plan and/or design, and conduct investigations; identify and address possible sources of uncertainty;• apply ethics of scientific research when conducting and reporting on investigations.Apply chemical understandings• make connections between concepts; process information; apply understandings to familiar and new contexts;• use first and second-hand data and evidence to demonstrate how chemical concepts and theories have developed and been modified over time;• analyse issues and implications relating to scientific and technological developments;• analyse and evaluate the reliability of chemistry related information and opinions presented in the public domain.Communicate chemical information and understandings• interpret, explain and communicate chemical information and ideas accurately and effectively;• use communication methods suitable for different audiences and purposes;• use scientific language and conventions correctly, including chemical equations and units of measurement.

UNIT 1 - HOW CAN THE DIVERSITY OF MATERIALS BE EXPLAINED

AREA OF STUDY 1 – How can knowledge of elements explain the properties of matter?Outcome 1Key knowledge

Elements and the periodic table• the relative and absolute sizes of particles that are visible and invisible to the unaided eye: small and giantmolecules and lattices; atoms and sub-atomic particles; nanoparticles and nanostructures• the definition of an element with reference to atomic number; mass number; isotopic forms of an element usingappropriate notation• spectral evidence for the Bohr model and for its refinement as the Schrodinger model; electronic configurationsof elements 1 to 36 using the Schrodinger model of the atom, including s, p, d and f notations (with copperand chromium exceptions)• the periodic table as an organisational tool to identify patterns and trends in, and relationships between, thestructures (including electronic configurations and atomic radii) and properties (including electronegativity, firstionisation energy, metallic/non-metallic character and reactivity) of elements.Metals• the common properties of metals (lustre, malleability, ductility, heat and electrical conductivity) with referenceto the nature of metallic bonding and the structure of metallic crystals, including limitations of representations;general differences between properties of main group and transition group metals• experimental determination of the relative reactivity of metals with water, acids and oxygen• the extraction of a selected metal from its ore/s including relevant environmental, economic and social issuesassociated with its extraction and use

• experimental modification of a selected metal related to the use of coatings or heat treatment or alloy production• properties and uses of metallic nanomaterials and their different nanoforms including comparison with theproperties of their corresponding bulk materials.Ionic compounds• common properties of ionic compounds (brittleness, hardness, high melting point, difference in electricalconductivity in solid and liquid states) with reference to their formation, nature of ionic bonding and crystalstructure including limitations of representations• experimental determination of the factors affecting crystal formation of ionic compounds• the uses of common ionic compounds.Quantifying atoms and compounds• the relative isotopic masses of elements and their representation on the relative mass scale using the carbon-12isotope as the standard; reason for the selection of carbon-12 as the standard• determination of the relative atomic mass of an element using mass spectrometry (details of instrument not required)• the mole concept; Avogadro constant; determination of the number of moles of atoms in a sample of knownmass; calculation of the molar mass of ionic compounds• experimental determination of the empirical formula of an ionic compound.

AREA OF STUDY 2 – HOW CAN THE VERSATILITY OF NON-METALS BE EXPLAINEDOutcome 2Key knowledge

Materials from molecules• representations of molecular substances (electron dot formulas, structural formulas, valence structures, ball and-stick models, space-filling models) including limitations of representations• shapes of molecules and an explanation of their polar or non-polar character with reference to the electronegativities of their atoms and electron-pair repulsion theory• explanation of properties of molecular substances (including low melting point and boiling point, softness, andnon-conduction of electricity) with reference to their structure, intramolecular bonding and intermolecular forces• the relative strengths of bonds (covalent bonding, dispersion forces, dipole-dipole attraction and hydrogenbonding) and evidence and factors that determine bond strength including explanations for the floating of ice and expansion of water at higher temperatures.Carbon lattices and carbon nanomaterials• the structure and bonding of diamond and graphite that explain their properties (including heat and electricalconductivity and hardness) and their suitability for diverse applications• the structures, properties and applications of carbon nanomaterials including graphene and fullerenes.Organic compounds• the origin of crude oil and its use as a source of hydrocarbon raw materials• the grouping of hydrocarbon compounds into families (alkanes, alkenes, alkynes, alcohols, carboxylic acidsand non-branched esters) based upon similarities in their physical and chemical properties including generalformulas, their representations (structural formulas, condensed formulas, Lewis structures), naming accordingto IUPAC systematic nomenclature (limited to non-cyclic compounds up to C10, and structural isomers up toC7) and uses based upon properties• determination of empirical and molecular formulas of organic compounds from percentage composition bymass and molar mass.Polymers• the formation of polymers from monomers including addition polymerisation of alkenes• the distinction between linear (thermoplastic) and cross-linked (thermosetting) polymers with reference to structure, bonding and properties including capacity to be recycled

• the features of linear polymers designed for a particular purpose including the selection of a suitable monomer(structure and properties), chain length, degree of branching, percentage crystalline areas and addition of plasticisers• the advantages and disadvantages of the use of polymer materials.

AREA OF STUDY 3 – RESEARCH INVESTIGATIONOutcome 3Key knowledge

• the characteristics of effective science communication• the chemical concepts specific to the investigation: definitions of key terms; use of appropriate chemicalterminology, conventions, units and representations• the use of data representations, models and theories in organising and explaining observed phenomena andchemical concepts, and their limitations• the nature of evidence and information: distinction between weak and strong evidence, and scientific and non-scientificideas; and validity, reliability and authority of data including sources of possible errors or bias• the influence of social, economic, environmental and ethical factors relevant to the selected chemical

investigation.

UNIT 2: WHAT MAKES WATER SUCH A UNIQUE CHEMICAL

AREA OF STUDY 1 – HOW DO SUBSTANCES INTERACT WITH WATEROutcome 1Key knowledge

Properties of water• trends in the melting and boiling points of Group 16 hydrides, with reference to the nature and relative strengthsof their intermolecular forces and to account for the exceptional values for water• specific heat capacity and latent heat including units and symbols, with reference to hydrogen bonding to accountfor the relatively high specific heat capacity of liquid water, and significance for organisms and water suppliesof the relatively high latent heat of vaporisation of water.Water as a solvent• the comparison of solution processes in water for molecular substances and ionic compounds• precipitation reactions represented by balanced full and ionic equations, including states• the importance of the solvent properties of water in selected biological, domestic or industrial contexts.Acid-base (proton transfer) reactions in water• the Bronsted-Lowry theory of acids and bases including polyprotic acids and amphiprotic species, and writingof balanced ionic equations for their reactions with water including states• the ionic product of water, the pH scale and the use of pH in the measurement and calculations of strengthsof acids and bases and dilutions of solutions (calculations involving acidity constants are not required)• the distinction between strong and weak acids and bases, and between concentrated and dilute acids andbases, including common examples• the reactions of acids with metals, carbonates and hydroxides including balanced full and ionic equations, withstates indicated• the causes and effects of a selected issue related to acid-base chemistry.Redox (electron transfer) reactions in water• oxidising and reducing agents, conjugate redox pairs and redox reactions including writing of balanced half and

overall redox equations with states indicated• the reactivity series of metals and metal displacement reactions including balanced redox equations with statesindicated• the causes and effects of a selected issue related to redox chemistry.

AREA OF STUDY 2 – HOW ARE SUBSTANCES IN WATER MEASURED AND ANALYSED?Outcome 2Key knowledge

Water sample analysis• existence of water in all three states at Earth’s surface including the distribution and proportion of availabledrinking water• sampling protocols including equipment and sterile techniques for the analysis of water quality at variousdepths and locations• the definition of a chemical contaminant and an example relevant to a selected water supply.Measurement of solubility and concentration• the use of solubility tables and experimental measurement of solubility in gram per 100 g of water• the quantitative relationship between temperature and solubility of a given solid, liquid or gas in water• the use of solubility curves as a quantitative and predictive tool in selected biological, domestic or industrial contexts• the concept of solution concentration measured with reference to moles (mol L-1) or with reference to mass orvolume (g L-1, mg L-1, %(m/m), %(m/v), %(v/v), ppm, ppb) in selected domestic, environmental, commercial orindustrial applications, including unit conversions.Analysis for salts in water• sources of salts found in water (may include minerals, heavy metals, organo-metallic substances) and the useof electrical conductivity to determine the salinity of water samples• the application of mass-mass stoichiometry to gravimetric analysis to determine the mass of a salt in a water sample• the application of colorimetry and/or UV-visible spectroscopy, including the use of a calibration curve, todetermine the concentration of coloured species (ions or complexes) in a water sample• the application of atomic absorption spectroscopy (AAS), including the use a calibration curve, to determine theconcentration of metals or metal ions in a water sample (excluding details of instrument).Analysis for organic compounds in water• sources of organic contaminants found in water (may include dioxins, insecticides, pesticides, oil spills)• the application of high performance liquid chromatography (HPLC) including the use of a calibration curve andretention time to determine the concentration of a soluble organic compound in a water sample (excludingdetails of instrument).Analysis for acids and bases in water• sources of acids and bases found in water (may include dissolved carbon dioxide, mining activity and industrialwastes)• volume-volume stoichiometry (solutions only) and application of volumetric analysis including the use ofindicators, calculations related to preparation of standard solutions, dilution of solutions and use of acid-basetitrations to determine the concentration of an acid or a base in a water sample.

AREA OF STUDY 3 – RESEARCH INVESTIGATIONOutcome 3Key knowledge

• the chemical concepts specific to the investigation and their significance, including definitions of key terms,and chemical representations• the characteristics of laboratory techniques of primary qualitative and quantitative data collection relevant

to the investigation: sampling protocols; gravimetric analysis, acid-base titrations and/or pH measurement;precision, accuracy, reliability and validity of data; and minimisation of experimental bias• ethics of and concerns with research including identification and application of relevant health and safety guidelines• methods of organising, analysing and evaluating primary data to identify patterns and relationships includingidentification of sources of error and uncertainty, and of limitations of data and methodologies• observations and experiments that are consistent with, or challenge, current chemical models or theories• the nature of evidence that supports or refutes a hypothesis, model or theory• options, strategies or solutions to issues related to water quality• the key findings of the selected investigation and their relationship to solubility, concentration, acid/base and/or redox concepts• the conventions of scientific report writing including chemical terminology and representations, symbols, chemicalequations, formulas, units of measurement, significant figures and standard abbreviations.

Assessment Timetable

Each task will be assessed via internal assessment. The dates below are subject to change.

Outcome Task DateUnit 1 AOS 1 Outcome 1 AT-1.1.1 Experimental Report

(Second-hand data analysis)Term 1, Week 3 (1 lesson)

Unit 1 AOS 2 Outcome 2 AT-1.2.2 Test Term 1, Week 9 (1 lesson)Unit 1 AOS 3 Outcome 3 AT-1.3.3 Research Poster Term 2, Week 4 (3 lessons)Unit 2 AOS 1 Outcome 1 AT-2.1.1 Test Term 3, Week 3 (1 lesson) Unit 2 AOS 2 Outcome 2 AT-2.2.2 Practical Report Term 3, Week 6 (3 lessons) Unit 2 AOS 3 Outcome 3 AT-2.3.3 Extended

Experimental Investigation Term 3, Week 9 (3 lessons)

There will also be end of semester exams and Topic tests conducted throughout the year, this are listed in the unit timeline below. If you have a private lesson during a scheduled assessment time you will need to reschedule your lesson with your teacher in advance. If you know you will be absent during a planned assessment time please speak with your teacher to organise this assessment reschedule.

Unit 1-2 Timeline

2017 unit 1 chemistry outline. Term/week

Concepts Text chapter

Minimum set questions from text Edrolo links Practical work/assessment

Homework

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Nanoparticles and the nanoscale.

Elements and the periodic table(Elements, Periodic table, Compounds)

Periodic table trends and electronic configuration

1

2

Ch1.1 -p7 Q2, 4 and 5, p33 Q1,3Ch1.2 - p11 Q2, 3 and 4, p33 Q5Ch1.3 - p14 Q1,2 and 3, p33 Q6,7 Ch1.4 - p17 Q 1-5, p33 Q9, 11,12Ch1.5 - p21 Q1-3, p33 Q13Ch1.6 –p26 Q1,2 and 5, p33 Q14Ch1.7 – p32 Q2, p33 Q17Ch2.1 – p41 Q5,p51 Q3Ch2.2 – p47 q1,2 p51 Q5,6Ch2.3 – p50 Q1,3, p51 Q8,9,12

https://edrolo.com.au/s/70914/https://edrolo.com.au/s/70918/

https://edrolo.com.au/s/70919/

SWB pg 13, ws 2SWB pg 14, ws 3SWB pg 16, ws 5

Holid

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Metals Properties and the metallic

bonding model PRAC Observing trends in

the periodic table properties and uses of

metallic nanomaterials

3 Ch3.1 – p59 Q1,4,5 p80 Q3,4,7Ch3.2 – p62 Q2,3, p80 Q8,9,11Ch3.3 – p65 Q2,3,4 p80 Q14, 15,16,Ch3.4 – p70 Q 1,4 p80 Q21, 23Ch3.5 – p76 Q1-4 p80 Q25, 26Ch3.6 – p79 Q1,3 p80 Q29p82 Q33, 35

https://edrolo.com.au/s/71626/https://edrolo.com.au/s/71627/https://edrolo.com.au/s/71628/

SWB pg 18, ws 7SWB pg 19, ws 8

1/2 Ionic compounds Properties and model Electron transfer

diagrams/Chemical formulas/Uses

4 Ch4.1 – p87 Q1,3,4, p105 Q1,2Ch4.2 –p93 Q1,3, p105 Q4,6Ch4.3 –p98 Q1,4,5, p105Q8,9, 10Ch4.4 – p101 Q,2,3 p105 Q14,16Ch4.5 – p104 Q2,3 p105 Q17,18p105 Q20

https://edrolo.com.au/s/71629/https://edrolo.com.au/s/71630/

TEST Chapter 1/2PRAC- Experimental determination of the relative reactivity of metals with water, acids and oxygen.

SWB pg 20, ws 9

1/3 Quantifying atoms and compounds Masses of particles

5 Ch 5.1 p117 Q1-6, Ch 5.2 p123 Q1-4

https://edrolo.com.au/s/71632/

PRAC- Mole of ChalkSAC 1 (assessed)

Relative isotopic and atomic masses using mass spectrometry

The mole

https://edrolo.com.au/s/71633/

1/4 Molar mass Empirical and molecular

formulas percentage composition

5 Ch5.3 p128 Q 1-5Ch5.4 p133 Q 1-5Chapter 5 review – all questionsAOS review – all questions

https://edrolo.com.au/s/71634/https://edrolo.com.au/s/71636/https://edrolo.com.au/s/71638/

1/5 Materials from molecules Covalent model Shapes of molecules Polarity of molecules

6 Ch6.1 p145 Q3-5Ch6.2 p153 Q1-6Chapter review

https://edrolo.com.au/s/77364/ https://edrolo.com.au/s/77365/ https://edrolo.com.au/s/77367/

TEST chapter 3/4 SWB pg 58, ws 15

1/6 Properties of molecular substances

Weak bonding between molecules

Carbon lattices and carbon nanomaterials Diamond and graphiteGraphene and fullerenes

7

8

Ch7.1 p160 Q1,3,5 Ch7.2 p166 Q3-5Ch7.3 p174 Q1-6Chapter review

Ch8.1 p183 Q1-4Ch8.2 p188 Q1-4 Chapter review

https://edrolo.com.au/s/77369/

https://edrolo.com.au/s/77378/

PRAC- Comparing the physical properties of different covalent lattices

SWB pg 62, ws 19

1/7 Organic compounds Crude oil Hydrocarbons Homologous series Functional groups Naming of organic

compounds

9 Ch9.1 p200 Q3-6 Ch9.2 p208 Q4-6Ch9.3 p214 Q1-6

https://edrolo.com.au/s/77380/ https://edrolo.com.au/s/77382/ https://edrolo.com.au/s/77385/

TEST chapter 5/6 Exercise: Analysis of the physical properties of the first eight hydrocarbonsExercise: Modelling and naming alkanes

https://edrolo.com.au/s/77390/

SW Worksheet

1/8 Empirical and molecular formula calculations

Chemical and physical properties of hydrocarbons, alcohols, carboxylic acids and simple esters

Ch9.4 p219 Q1,3,4,5 Ch9.5 p224 Q1-5 Ch9.6 p229 Q1-4

Chapter review

https://edrolo.com.au/s/77394/ https://edrolo.com.au/s/77391/ https://edrolo.com.au/s/77392/

Prac: Preparing artificial fragrances and flavours

SWB pg 60, ws 17

1/9 Polymers Formation of addition

polymers Differences between

thermoplastic and thermosetting

Designed polymers Advantages and

disadvantages of the use of polymers

10 Ch10.1 p242 Q1,3,4,5Ch10.2 p254 Q1,2,4,5,6Chapter reviewAOS 2 review p257 - 260

https://edrolo.com.au/s/77395/ https://edrolo.com.au/s/77396/ https://edrolo.com.au/s/77398/

PRAC- Making ghost buster slimeSAC 2 - TEST

SWB pg 67, ws 23

1/10 Properties of water Trends in MP and BP of

Group 16 hydrides Specific heat capacity and

latent heat of water

12 12.1 Q1-412.2 Q3-712.3 Q4-6Review Q1-21

Trends of Grp 16 HydridesLatent HeatSpecific Heat Capacity

Prac: Molar heats of solutions

SWB WS 25SWB WS 26SWB WS 27

2/1 Water as a solvent The solution process Precipitation reactions Ionic equations Importance of solvent

properties in biological, domestic or industrial contexts

13 13.1 Q3-713.2 Q2-513.3 Q1-313.4 Q2-4Review Q1-25

Substances that dissolve in waterPrecipitationIonic Equations

Prac: Effect of polarity on solubility Prac: Stalagmite from a supersaturated solution

SWB WS 28 SWB WS 29SWB WS 30

2/2 Measurement of solubility and concentration Solubility and solubility

tables Solubility curves

14 14.1 Q3-614.2 Q3-614.3 Q2-414.4 Q1-614.5 Q3-4

Solubility CurvesApplications of Solubility CurvesUnits of Concentration

Prac: Deriving a solubility curveSWB pg 120

TEST- CHPT 12/13

SWB WS 34

Units of concentration Review Q1-22 Unit Conversions2/3 Research investigation SAC 3 – POSTER 2/4 Research investigation SAC 3 – POSTER2/52/62/7 EXAMS2/8 EXAMS2/9 UNIT 2 START2/10 Lowry-Bronsted theory

Reactions involving acids and bases and equation writing

Ionic product of water, pH

15 15.1 Q1-615.2 Q1-4

Acid/Base TheorySpectator IonspH

Prac: Reactions of hydrochloric acid

SWB WS 33SWB WS 35

2/11 Strengths of acids and base (No Ka )

Dilutions of solutions Strong and weak acids and

bases and dilute and concentration solutions

Selected acid-base issue – Ocean acidity

15 15.3 Q1,3,5,715.4 Q2,4,615.5 Q1ac, 2, 3ace, 4aceg15.6 Q1-3 Review

Acid Base ConcentrationsAcid Base reactionsAcid and Metal reactionsAcid and carbonate reactions

SWB WS 36

3/1 Redox reactions in water Oxidation and reduction Writing equations Reactivity series Selected redox issue -

Corrosion

16 16.1 Q2-516.2 Q1-316.3 Q1,2,4Review Q1-28

Redox NumbersIdentifying Oxidation and ReductionOxidising AgentsRedox Conjugate PairsWriting Half equationsWriting REDOX equations

Demo: Oxidation-reduction reactionsPrac: The electrochemical series of metals

SWB WS 38 SWB WS 39

3/2 Water sample analysis Water distribution and

availability Sampling protocols

17 17.2 Q2,3Review Q1,4,6,8,11

Water sample analysisWater Contaminants

TEST- CHPT 15/16

Selected water sample and contaminant

3/3 Analysis of salt in water Sources of salts Mass-mass stoichiometry

18 18.1 Q1,2,4,5,7,818.2 Q1-318.3 Q2,3,4

Salt AnalysisMass Stoich

Prac: Products of a decomposition reactionSAC 1

3/4 Gravimetric analysis Colorimetry and UV-Vis

spectroscopy AAS and Calibration

18 18.4 Q1-4,6,818.5 Q2,4,5 Review Q1-29

UV-Vis ColorimetryApplications of UV-VisAAS

Experiment: Colorimetric determination of phosphorus content in lawn fertiliserExercise: AAS - Determination of concentration of iron in a breakfast cereal SW Worksheets

3/5 Analysis for organic compounds Organic contaminants in

water Chromatography and HPLC

19 19.1 Q1,3,5,719.2 Q1-419.3 Q1-5Review Q1-25

Sources of OrganicsHPLC

Prac: Chromatography of inks and smartiesTest – Analysing compounds in Water

3/6 Analysis for acids and bases Sources of acids and bases

in waterways Volume-volume

stoichiometry Volumetric analysis

including standard solutions and dilutions

20 20.1 Q3,420.2 Q1-320.3 Q2,3,420.4 Q1-320.5 Q1-3Review Q1-18

Acid Base AnalysisStandard SolutionsAcid Base Titrations

Prac: Preparation of a standard solutionPrac: Analysis of brick cleanerSAC 2

3/73/8 Practical Investigation SAC 3 – POSTER 3/9 Practical Investigation SAC 3 – POSTER 4/14/24/3 EXAMS4/4 EXAMS4/5 EXAMS