Year 13 Chemistry (NCEA) Student Information

Transcription

1 Year 13 Chemistry (NCEA) Student Information Science Department Onslow College 2015

2 Introduction Year 13 Chemistry is a full year course, of five topics, that works towards gaining Level Three credits for the National Certificate of Educational Achievement (NCEA). Two standards are assessed internally (6 credits), three of the standards are externally assessed (15 credits). 1. Year 13 Chemistry Topics The chemistry course leading to the NCEA in Chemistry is made up of five topics: Redox Spectroscopy Aqueous solutions acid / base Aqueous solutions solubility Organic Chemistry Chemical Reactivity Topic (a) Relative strengths of oxidants and reductants (b) principles of electrochemical and electrolytic cells (c) reduction potentials and spontaneity of reactions (a) mass spectroscopy (b) infrared (IR) absorption (c) nuclear magnetic resonance (NMR) shifts (d) organic molecular identification (a) proton transfer in aqueous solution (b) equilibrium constants K a, pk a, K w (c) ph calculations (d) acidbase titration curves (e) buffer solutions (f) solubility of sparingly soluble ionic salts (g) K s and solubility (h) Predicting precipitation (a) Isomerism: structural, geometrical and optical (b) functional groups alcohol, aldehyde, ketone, ester, carboxylic acid, acyl chloride, amide, alkene, haloalkane, amine (c) characteristic reactions of organic compounds (d) application of the properties of organic compounds (a) electron configuration, s,p,d, of atoms and ions HKr (b) atomic and ionic radii, ionisation energies, electronegativity (c) Lewis structures, shape and polarity of molecules (d) variation in transition metal compounds (e) enthalpy and entropy changes (f) exothermic and endothermic reactions (g) f H, c H, r H, fus H, sub H and vap H (h) Hess s Law, Bond Energy calculations (i) strength of intermolecular forces temporary dipoles, permanent dipoles, hydrogen bonding; ionic bonding, covalent bonding. Achievement Credits Standard AS 3.7 / AS 3.2 / AS 3.6 / AS 3.5 / AS 3.4 /

3 2. Assessment There will be practice assessment opportunities for the three external standards during the year; one at the end of each topic, the other during the first week of term 4. The external standards require you to describe, explain or interpret, and discuss chemistry ideas. Achieved (describe) requires you to identify, name, draw, give characteristics of, or an account of, carry out simple calculations. Merit (Explain or Interpret) requires you to provide reasons for how and why something occurs and may include related calculations. Excellence (Discuss) requires you to show understanding as to how or why something occurs by linking chemistry ideas/principles. It typically involves justifying, relating, evaluating, comparing and contrasting, analysing, interpreting, and calculating. The chemistry course has two internal achievement standards: AS 3.2 (91388) Demonstrate understanding of spectroscopic data in Chemistry AS 3.7 (91393) Demonstrate understanding of oxidationreduction processes For each internal standard, there will be one assessment opportunity. All work submitted for internal assessment must be your own work. The NCEA booklet gives guidance. Texts/Reference Material This Student Information handbook Continuing Chemistry Student Workbook, and companion CDRom. Web Based Resources 1 The Bestchoice website: Your class teacher will supply you with registration and login details MOODLE: 2

4 Year 13 Chemistry: Year Planner 2015 Term 1 2 February 2 April Redox Internal Standard Organic 2/2 9/2 16/2 23/2 2/3 9/3 16/3 23/3 30/3 Term 2 20 April 3 July Organic cont. Spectroscopy Aqueous solutions Internal Standard 20/4 27/4 4/5 11/5 18/5 25/5 1/6 8/6 15/6 22/6 29/6 Term 3 20 July 25 Sept Aqueous cont Thermochemistry Review 20/7 27/7 3/8 10/8 17/8 24/8 31/8 7/9 14/9 21/9 Term 4 12 October 10 December Revision and Test Papers NCEA Exams 12/10 19/10 26/10 2/11 9/11 16/11 23/11 30/11 7/12 3

5 Redox 3.7 Internal Demonstrate understanding of oxidationreduction processes By the end of this topic students will be able to describe, explain and apply information, and discuss information related to: 1. Appearance, state and behaviour of reactants (oxidants and reductants) and their products. 2. Oxidants are O 2, Cl 2, Fe 3+, dilute acid (with metals), H 2 O 2, I 2, MnO 4, Cu 2+, Cr 2 O 2 7 /H +, OCl, concentrated HNO 3, IO 3, MnO Reductants are Zn, Mg, Fe, Cu, C, H 2, Fe 2+, Br, I, H 2 S, (SO 2, SO 2 3 HSO 3 ), S 2 O 2 3, H 2 O 2, H 2 C 2 O Practical redox reactions 5. Write balanced half electron equations 6. Principles of electrolytic and electrochemical cells related to specific examples 7. Electrode potential as a measure of the relative oxidant and reductant strength 8. Spontaneity of oxidation reduction reactions. 9. Calculations involving redox reactions Text CC Chapters 3 and 4 Assessment Internal Assessment Term 1 AS 3.7 / Credits Demonstrate understanding of oxidationreduction processes Internal Achievement Criteria Achievement Achievement with Merit Achievement with Excellence Demonstrate understanding of oxidationreduction processes. Demonstrate indepth understanding of oxidationreduction processes. Demonstrate comprehensive understanding of oxidationreduction processes. 4

6 Spectroscopy 3.2 Internal Demonstrate understanding of spectroscopic data in chemistry Achieved: only one technique used. Interpretation of spectra of simple organic molecules with a basic knowledge of how the technique works. Merit: linking of data from at least two different spectroscopic techniques to the structural features of organic molecules. Excellence: solving the structures of simple organic molecules by interpreting data from at least two different spectroscopic techniques. Organic molecules are limited to alkanes, alkenes, alcohols, haloalkanes, amines, aldehydes, ketones, carboxylic acids, amides, acid chlorides and esters. Tables of data will be provided including: mass spectrometry (molar mass), characteristic absorptions, infrared IR (functional groups) and 13 C nuclear magnetic resonance NMR (length of carbon chain). Text CC Chapter 11 Assessment Internal Assessment Term 2 AS 3.2 / Credits Demonstrate understanding of spectroscopic data in chemistry Internal Achievement Criteria Achievement Achievement with Merit Achievement with Excellence Demonstrate understanding of spectroscopic data in chemistry. Demonstrate indepth understanding of spectroscopic data in chemistry. Demonstrate comprehensive understanding of spectroscopic data in chemistry. 5

7 Aqueous Solution Chemistry 3.6 External Demonstrate understanding of equilibrium principles in aqueous systems By the end of this topic students will be able to describe, explain and apply, and discuss equilibrium principles in aqueous systems For acids and bases 1. Strong and weak acids and bases in terms of proton transfer 2. Equilibrium constant expressions for K a and K w 3. use of K a (pk a ) and ph as a measure of acid, and base, strength 4. characteristics of acidbase titration curves: shape, initial ph, equivalence point, choice of indicator, pk a and buffer regions as appropriate, including ph at any point in a titration 5. the nature of a buffer solution ie composition, mode of action and importance of buffers 6. relative concentrations of species in solution 7. Calculations involving K a, K w, ph, for monoprotic acids, solutions of bases, buffers. For solubility (sparingly soluble ionic solids) 8. equilibrium constant, K s 9. relative equilibrium concentrations of dissolved species 10. calculations involving interconversion between K s and solubility for sparingly soluble ionic solids of the types AB, A 2 B and AB 2 (no further reaction occurs to change the ph) 11. common ion effect ie solubility in a solution containing one of the ions A or B. Effect of solubility due to the formation of a complex ion, or reaction of a basic anion with added acid 12. use of ionic product, K i and K s to predict precipitation or dissolution Text CC Chapters

8 Aqueous Solution Chemistry 3.6 (continued) Assessment Topic test Term 3 School Chemistry Exam paper Week 1 Term 4 NCEA Exam November AS 3.6 / Credits Demonstrate understanding of equilibrium principles in aqueous systems External Achievement Criteria Achievement Achievement with Merit Achievement with Excellence Demonstrate understanding of equilibrium principles in aqueous systems. Demonstrate indepth understanding of equilibrium principles in aqueous systems. Demonstrate comprehensive understanding of equilibrium principles in aqueous systems. 7

9 Organic Chemistry 3.5 External Demonstrate understanding of structure and reactivity of organic compounds By the end of this topic students will be able to describe, explain and apply principles and discuss the structure, physical properties, and reactions of organic compounds 1. Physical properties of selected functional groups. eg melting point/boiling point, solubility, ph 2. Hydrocarbons as alkanes, alkenes and alkynes substitution reactions of alkanes using Cl 2, Br 2 addition reactions of unsaturated hydrocarbons using H 2 /Pt, H 2 O/H +, Br 2, HCl or HBr(including major and minor products), MnO 4 3. Haloalkanes Substitution reactions with concentrated ammonia substitution reaction with NaOH or KOH in aqueous solution elimination reactions with KOH in alcohol solution 4. Amines Preparation from haloalkanes 5. Alcohols action of oxidising agents, ie MnO 4 and Cr 2 O 7, on primary, secondary and tertiary alcohols substitution reactions with PCl 3, conc. HCl, conc. HBr, SOCl 2 and ZnCl 2 /HCl to form chloroalkanes elimination reaction with concentrated sulfuric acid to form alkenes formation of esters with carboxylic acids, including triglycerides 6. Aldehydes and Ketones the use of Fehling s, Tollens or Benedict s reagents to distinguish between aldehydes and ketones oxidation of aldehydes to carboxylic acids using MnO 4, Cr 2 O 7 /H + reduction with LiAlH 4 7. Esters preparation of esters from alcohols and carboxylic acids, including triglycerides [hydrolysis of esters including in both acid and basic conditions] 8. Carboxylic acids characteristic properties of carboxylic acids acidic properties, reactions with alcohols formation of esters with alcohols, including triglycerides substitution reactions with PCl 5, HCl or SOCl 2 to form acyl chlorides substitution reactions with concentrated ammonia, or amines, to form amides 8

10 9. Acyl chlorides preparation of acyl (acid) chlorides from carboxylic acids by substitution reactions reaction of acyl chlorides with water, ammonia, alcohols and amines 10. Amides Preparation of amides from carboxylic acids by reaction with concentrated ammonia 11. Isomerism Structural (constitutional) isomers, and stereo isomers (geometric and optical isomers) Distinction between compounds using rotation of plane polarized light 12. Polymerisation addition polymers elimination/condensation polymerization to prepare polyamides and polyesters hydrolysis of polymers, using KOH / NaOH or concentrated sulfuric acid polymers include polyesters, polyamides, proteins glycine and alanine as examples of amino acids Note: Assessment of this AS may include work covered in the Level 2 course Chain length up to 8 carbon atoms for all homologous series Larger organic molecules may be used in questions IUPAC convention used to name compounds. Organic structures from this topic are applicable to the internal standard 3.2 Text CC Chapters 8 10 Assessment Topic test Term 2 School Chemistry Exam paper Week 1 Term 4 NCEA Exam November 9

11 AS 3.5 / Credits Demonstrate understanding of structure and reactivity of organic compounds External Achievement Criteria Achievement Achievement with Merit Achievement with Excellence Demonstrate understanding of structure and reactivity of organic compounds Demonstrate indepth understanding of structure and reactivity of organic compounds. Demonstrate comprehensive understanding of structure and reactivity of organic compounds. Level 2 Organic Chemistry Chemistry (AS 2.5) 1. Distinguish between different functional groups using experimental observations. 2. Hydrocarbons as alkanes, alkenes and alkynes naming, structure and structural formula of straight chain and branched hydrocarbons (alkanes, alkenes, alkynes) substitution reactions of alkanes halogenation identification of unsaturated hydrocarbons with bromine and aqueous potassium permanganate addition reactions of unsaturated hydrocarbons using H 2 /Pt, H 2 O/H +, Br 2, HCl (including major and minor products) 3. Haloalkanes name, structure and structural formula for haloalkanes classification of haloalkanes as primary, secondary or tertiary 4. Amines name, structure and structural formula for amines classification of amines as primary, secondary or tertiary 5. Alcohols name, structure and structural formula for alcohols alcohols as primary, secondary, tertiary, characteristic properties of primary alcohols oxidation to carboxylic acids, reactions with carboxylic acids 6. Carboxylic acids name, structure and structural formula for carboxylic acids characteristic properties of carboxylic acids acidic properties, reactions with alcohols 7. Isomerism isomers structural and geometric (cis / trans) 8. Polymerisation formation of addition polymers from monomers 10

12 Chemical Reactivity 3.4 External Demonstrate understanding of properties of particles and thermochemical principles By the end of this topic students will be able to describe, explain and apply and discuss the properties of atoms, molecules and ions, and thermochemical principles 1. Electron configuration using s, p, d of the first 36 elements and their ions 2. Transition metals ie Fe, V, Cr, Mn, Cu, Zn variable oxidation state variation in colour of transition metal ions and their compounds 3. Periodic trends in atomic radius, ionisation energy and electronegativity, 4. Comparison of atomic and ionic radii 5. Lewis structures and shapes of simple covalent molecules and ions with 2 6 electron pairs around the central atom for molecules and polyatomic ions, including multiple bonds 6. Polarity of molecules 7. Constituent particles substances as atoms, ions or molecules 8. Forces between particles as ionic bonds, covalent bonds, temporary dipoles, permanent dipoles, hydrogen bonding 9. Endothermic and exothermic reactions as involving transfer of heat energy between the system and the surroundings 10. Relationship between endothermic and exothermic reactions and bond making and bond breaking processes 11. Define the terms c H, f H, r H, vap H, subh and fus H 12. Relationship of the weak and strong attractive forces between particles and values of melting point, boiling point, fus H, sub H and vap H 13. Enthalpy change by Hess s Law and r H = f H (products) f H (reactants) 14. Enthalpy change using average bond energies 15. Enthalpy changes related to heat and mass, using the specific heat capacity of water 16. ENTROPY changes in chemical reactions and phase changes Text CC Chapters

13 Assessment 3.4 Topic test Term 3 School Chemistry Exam paper Week 1 Term 4 NCEA Exam November AS 3.4 / Credits Demonstrate understanding of properties of particles and thermochemical principles External Achievement Criteria Achievement Achievement with Merit Achievement with Excellence Demonstrate understanding of properties of particles and thermochemical principles. Demonstrate indepth understanding of properties of particles and thermochemical principles. Demonstrate comprehensive understanding of properties of particles and thermochemical principles. 12

14 Table of Ions Cations H + Na + K + Ag + NH 4 + H 3 O + hydrogen sodium potassium silver ammonium hydronium Mg 2+ Ca 2+ Ba 2+ Zn 2+ Pb 2+ Mn 2+ Cu 2+ Fe 2+ magnesium calcium barium zinc lead manganese copper(ii) iron (II) Al 3+ Fe 3+ Cr 3+ aluminium iron (III) chromium Anions F Cl Br I OH NO 3 CH 3 COO HCO 3 HSO 3 MnO 4 OCl IO 3 fluoride chloride bromide iodide hydroxide nitrate ethanoate bicarbonate bisulfite permanganate hypochlorite iodate O S CO 3 SO 4 SO 3 Cr 2 O 7 CrO 4 S 2 O 3 S 4 O 6 C 2 O 4 oxide sulfide carbonate sulphate sulfite dichromate chromate thiosulphate tetrathionate ethandioate / oxalate PO 4 3 phosphate Solubility Rules for Ionic Solids 1 Soluble Group 1 metal ion compounds, Nitrate and Ammonium compounds 2 Soluble All metal Halides Except Pb 2+ and Ag + (Pbag) 3 Soluble All metal Sulphates Except Ba 2+, Ca 2+ and Pb 2+ (ABCP) 4 INSoluble All Oxides, Hydroxides and Carbonates Except for rule no. 1 13

15 Standard Electrode Potential at 298K / V K + (aq) + e K (s) 2.92 Ca 2+ (aq) + 2e Ca (s) 2.87 Na + (aq) + e Na (s) 2.71 Mg 2+ (aq) + 2e Mg (s) 2.36 Al 3+ (aq) + 3e Al (s) 1.66 Zn 2+ (aq) + 2e Zn (s) 0.76 Fe 2+ (aq) + 2e Fe (s) 0.44 Cr 3+ (aq) + 3e Cr (s) 0.41 Ni 2+ (aq) + 2e Ni (s) 0.25 Pb 2+ (aq) + 2e Pb (s) H 3 O + (aq) + 2e H 2(g) + 2H 2 O (l) 0 SO 4 (aq) + 4H + (aq) + 2e SO 3 (aq) + 2H 2 O (l) 0.17 Cu 2+ (aq) + e Cu + (aq) 0.17 Cu 2+ (aq) + 2e Cu (s) 0.34 I 2(s) + 2e 2I (aq) 0.54 O 2(g) + 2H + (aq) + 2e H 2 O 2(l) 0.68 Fe 3+ (aq ) + e Fe 2+ (aq) 0.77 NO 3 (aq) + 2H + (aq) + e NO 2(g) + H 2 O (l) 0.78 Ag + (aq) + e Ag (s) 0.80 S 4 O 6 (aq) + 2e 2S 2 O 3 (aq) 0.80 Br 2(l) + 2e 2Br (aq) IO 3 (aq) + 12H + (aq) + 10e I 2(aq) + 6H 2 O (l) 1.20 MnO 2(s) + 4H + (aq) + 2e Mn 2+ (aq) +2H 2 O (l) 1.23 Cr 2 O 7 (aq) + 14H + (aq) + 6e 2Cr 3+ (aq)+ 7H 2 O (l) 1.33 Cl 2(g) + 2e 2Cl (aq) 1.36 PbO 2(s) + 4H + (aq) + 2e Pb 2+ (aq) + 2H 2 O (l) 1.46 MnO 4 (aq) + 8H + (aq) + 5e Mn 2+ (aq) + 4H 2 O (l) 1.51 H 2 O 2(l) + 2H + (aq) + 2e 2H 2 O (l) 1.78 F 2(g) + 2e 2F (aq)