Download Chemistry - Onslow College

Year 12 Chemistry
(NCEA)
Student Information
Science Department
Onslow College
2015
Introduction
Year 12 Chemistry is a full year course, of six topics, that works towards gaining Level Two credits
for the National Certificate of Educational Achievement (NCEA). Three of the standards are assessed
internally (10 credits), three of the standards are externally assessed (13 credits)
1. Year 12 Chemistry Topics
The chemistry course leading to the NCEA in Chemistry is made up of six topics:
Topic
Achieveme
nt standard
2.4 (91164)
E
Structure,
Bonding,
Properties and
Energy changes
(a) ionic bonding, covalent bonding,metallic,
polar molecules, electronegativity
(b) Lewis diagrams, shapes of molecules
(c) structures of crystalline solids, intermolecular
bonding, physical properties of compounds
(d) Exo and Endothermic reactions, energy
(enthalpy) changes, bond energy and ∆rH
Inorganic
Chemistry
(a) reactions of ions in solution
(b) solubility rules to determine solubility and
precipitation
(c) tests for anions, cations
(d) balanced equations and ionic equations
2.2 (91162)
Quantitative
Analysis
(a) Acid – base titration
(b) calculations using concentration, moles,
mass, Mr and % composition
2.1 (91161)
Organic Chemistry
(a) hydrocarbons, alcohols, carboxylic acids,
primary amines, haloalkanes
(b) isomerism
(c) addition polymers of alkenes
(a) proton transfer, strong acids and bases,
weak acids and bases
(b) pH, Kw, [H3O+], [OH-]
(c) rates of reaction, collision theory,
temperature, concentration, surface area,
catalyst
(d) equilibrium reactions, temperature,
concentration, surface area, catalyst,
pressure
(e) Kc
2.5 (91165)
(a)
(b)
(c)
(d)
2.7 (91167)
Chemical
Reactivity
Redox
oxidation, reduction, oxidation number
electron transfer in reactions
oxidants and reductants
half ion electron equations, balanced redox
equations
(e) appearance of colour and state of species
1
I
I
E
2.6 (91166)
Credits
5
3
4
4
4
E
I
3
2. Assessment
There will be one assessment opportunity for the three external Achievement Standards. This will
occur in November and will be examined by NZQA by an external exam. There will be practice
assessment opportunities for these external standards during the year; one at the end of the topic,
the other in the school exams.
The external standards require you to demonstrate understanding -
Achievement requires you to identify, name, draw, give characteristics of, or an account of.
Merit requires you to provide reasons for how and why (in-depth understanding).
Excellence requires you to show understanding as to how or why something occurs by linking
chemistry ideas/principles (comprehensive understanding). It may involve you in
justifying, relating, evaluating, comparing and contrasting, analysing.
The chemistry course has three internal achievement standards:
AS 2.1 (91161) Carry out quantitative analysis,
AS 2.2 (91162) Carry out procedures to identify ions present in solution,
AS 2.7 (91167) Demonstrate understanding of oxidation-reduction,
For 2.1, 2.2 and 2.7, there will be one assessment opportunity within the topic. There may also be
an optional, reassessment opportunity, for these internal standards if there is a gear failure, or if a
student has a sick note or similar.
All work submitted for internal assessment must be your own work. The NCEA booklet gives
guidance.
3. Texts/Reference Material
(a) Student Handout (this booklet):
This handout contains course information, assessment information, and learning outcomes. It
also contains a table of ions, solubility rules, periodic table, and a flow chart for cations and
anions.
(b) Workbook and Web based resources:
Students are issued a write on practical text for which you will be invoiced.
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The Bestchoice website: www.bestchoice.net.nz
www.nobraintoosmall.co.nz
http://www.tristanriley.co.nz/wiki/pmwiki.php?n=Year12Chemistry.Year12Chemistry
http://www.sciencescribe.co.nz/2chem.html
MOODLE: https://moodle2.onslownet.school.nz/
2
Year 12 Chemistry: Year Planner 2015
Term 1
1
2
3
2 February – 2 April
4
5
6
Qualitative
Internal Standard
Identifying Ions in Solution
2/2
9/2
16/2
2
3
23/2
2/3
4
9/3
20/4
27/4
4/5
1
2
11/5
8
1/6
8/6
27/7
3/8
10/8
6
17/8
Term 4
2
3
30/3
9
10
15/6
22/6 29/6
7
8
24/8
31/8
9
10
School Exam
Exams Review
7/9
14/9
21/9
12 October – 10 December
4
5
6
7
8
16/11
23/11
30/11
9
NCEA Exams…
Revision
19/10
26/10
11
20 July – 25 Sept
5
Chemical Reactivity
1
12/10
7
25/5
Term 3
Organic
23/3
Redox
Internal Standard
18/5
4
16/3
6
Structure and Bonding
20/7
9
20 April – 3 July
5
Assessment of
Quantitative
3
8
Quantitative
Internal Standard
Acid-Base ttn, moles, mass and %
Term 2
1
7
2/11
9/11
3
7/12
Inorganic Chemistry
Internal
Carrying out procedures to identify ions present in solution
From their previous studies in science, students should have an understanding of
 Writing formula of ionic substances and simple covalent compounds
 Writing word equations and balanced chemical equations for inorganic reactions
By the end of this topic students will be able to 1. use solubility rules to predict precipitation and identify the precipitate.
2. carry out precipitation reactions and report experimental observations
3. from experimental observations identify unknown anions and cations using the flow chart
4. distinguish between pairs of anions or pairs of cations in solution
5. identify ions, including complex ions in solution
6. write ionic equations
7. complete and write equations for the formation of complex ions
Note:
 Ions are limited to:
Cations
Ag+
Al3+
Ba2+
Cu2+
Mg2+
Pb2+
Na+
Zn2+
CO32-
I-
NO3-
Fe2+
Fe3+
OH-
SO42-
Anions
Cl-
Na+ and NO3- are identified by a process of elimination
 Complex ions are limited to:
[Al(OH)4]-
[Zn(OH)4 ]2-
[Pb(OH)4]2-
[FeSCN]2+
[Ag(NH3)2 ]+
[Cu(NH3)4 ]2+
4
[Zn(NH3)4 ]2+
Text
BC Chapters 1, 3 and 4
Practicals 1.1, 3.1, 3.2, 4.1, 4.2, 4.3 and 4.4
Assessment
Internal assessment – Term 1
Note:
 a table of ions is NOT provided
 solubility rules will NOT be provided
 a flow chart will be provided
AS 91162 v1 Chemistry 2.2
Carry out procedures to identify ions present in
3 Credits
solution
Internal
Achievement Criteria
Achievement
Achievement with Merit
Achievement with
Excellence
 Carry out procedures to
identify ions present in
solution.
 Carry out procedures to
justify the identification of
ions present in solution.
 Carry out procedures to
comprehensively justify
the identifcation ions
present in solution.
5
Quantitative Analysis: Acid – Base
Internal
Carry out an acid – base quantitative analysis
From their previous studies in science, students should have an understanding of
 Names and formula of common lab acids and bases
 Acids, bases and indicators eg litmus, and Universal Indicator
By the end of this topic students will be able to carry out an acid-base titration, and determine the
concentration of an unknown solution and solve quantitative problems
1. carry out a titration to a high degree of accuracy
2. record information systematically
3. use the relationship n = cv, and use a mole ratio from a given chemical equation
4. Use the relationship m = nMr and use a mole ratio from a given equation
5. determine the concentration of an unknown solution
6. use significant figures appropriately.
Text
BC Chapters 6, 7 and 8
Practicals 6.4(D), mole amounts, 7.1, 8.1, 8.2, [+ other ttns]
Assessment
Internal Assessment – Term 1
AS 91161 v1 Chemistry 2.1
Carry out quantitative analysis
4 Credits
Internal
Achievement Criteria
Achievement
Achievement with Merit
 Carry out quantitative
analysis.

Carry out in-depth
quantitative analysis.
6
Achievement with
Excellence

Carry out comprehensive
quantitative analysis.
Achievement Criteria
Achievement
Achievement with Merit
Achievement with
Excellence
3 titre values within 0.4 mL
3 titre values within 0.4 mL
3 titre values within 0.2 mL
Average titre is within 0.8 mL of
the expected outcome
Average titre is within 0.5 mL of
expected outcome
Average titre is within 0.2 mL of
the expected
All titre values may be used
Only concordant titre values
used
Only concordant titre values
used
Solve quantitative problems that
use n = cv and m = nMr in at
least two steps
stoichiometry is not 1:1
Minor error
Solve quantitative problems that
use n = cv and m = nMr to
calculate one variable
7
units and sf
Solve quantitative problems that
use n = cv and m = nMr in
more than two steps
Structure, Bonding and Energy Changes
External
Demonstrate understanding of bonding, structure and energy changes
From their previous studies in science, students should have an understanding of
 Structure of atom
 Charges on ions
 The differences between atoms, elements, molecules and compounds
 Formula of ionic and simple covalent compounds
 Properties of metals
By the end of this topic students will be able to describe, link and discuss
1.
Bonding within molecules as
 Ionic
 Covalent
 Metallic
2.
Constituent of particles in solids as
 Atoms
 Molecules
 Ions
3.
Draw Lewis structures of molecules with
 2, 3 or 4 electron pairs around the central atom
 4 electron pairs around any atom
 double or triple bonds
4.
Shapes of simple molecules as
 Linear
 Trigonal planar
 Tetrahedral
 Trigonal pyramid
 bent
5.
Polarity of molecules linked to polar bonds (electronegativity), and shape of molecule.
6.
Types of solids as
 Molecular
 Ionic
 Metallic
 Covalent network
8
7.
Forces between particles in solid as
 Ionic
 Covalent
 Metallic
 Weak intermolecular forces
8.
Exothermic and Endothermic reactions including energy (enthalpy) changes
associated with differing amounts of substances, changes of state,
and enthalpy changes associated with bond making and breaking
9.
Properties of solids as
 Electrical conductivity ie movement of charged particles - electrons or ions
 Malleable/ ductile / hardness ie in terms of structure
 Melting point and Boiling point ie in terms of strength of bond / force between
particles.

Solubility ie solubility in terms of particles and the attractive forces in solute,
solvent and solution.
Text
BC – Chapters 2, 9, 10 and 11
Practicals 2.1, 2.2, 9.1, 9.2(D), 9.3, 10.1, 10.2(D), 10.3 and 11.2 (tbc)
Assessment
Topic test – Term 2
School Exam – Term 3
NCEA Exam – November
AS 91164 v1 Chemistry 2.4
Demonstrate understanding of bonding, structure, properties
5 Credits
and energy changes
External
Achievement Criteria
Achievement
Achievement with Merit
Achievement with
Excellence
 Demonstrate
understanding of bonding,
structure and energy
changes.
 Demonstrate in-depth
understanding of bonding,
structure and energy
changes.
 Demonstrate
comprehensive
understanding of bonding,
structure and energy
changes.
9
Organic Chemistry
External
Demonstrate understanding of the properties of selected organic
compounds.
By the end of this topic students will be able to describe, link and discuss
1. Use conventions
 Chain length up to 8 carbon atoms for all homologous series
 IUPAC convention used to name compounds
 Equations using names or structural formulae
 Structural formulae as either condensed or expanded
2. Distinguish between different functional groups using experimental observations.
3. 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 H2/Pt, H2O/H+, Cl2 , Br2 ,
HCl (including major and minor products)
4. Haloalkanes
 name, structure and structural formula for haloalkanes
 classification of haloalkanes as primary, secondary or tertiary
 substitution reaction of haloalkanes with ammonia
 elimination of hydrogen halide from haloalkane
5. Amines
 Primary amines
 Basic reaction of amines (including water and carboxylic acids)
6. Alcohols
 name, structure and structural formula for alcohols
 alcohols as primary, secondary, tertiary,
10
 characteristic properties of primary alcohols – oxidation to carboxylic acids, reactions with
carboxylic acids
 elimination reactions of alcohols
 substitution reactions with hydrogen halides (and PCl5)
7. Carboxylic acids
 name, structure and structural formula for carboxylic acids
 characteristic properties of carboxylic acids – acidic properties, reactions with alcohols and
amines
8. Isomerism
 isomers – structural and geometric (cis / trans)
9. Polymerisation
 formation of addition polymers from monomers
Text
BC Chapters 12 – 14
Practicals 12.1, 13.1, 13.3, 14.1, 14.2, 14.3, 14.4(D),14.5 and 14.6
Assessment
Topic test – Term 3
School Exam – Term 3
NCEA Exam – November
AS 91165 v1 Chemistry 2.5
4 Credits
Demonstrate understanding of the properties of selected
organic compounds
External
Achievement Criteria
Achievement
Achievement with Merit
Achievement with
Excellence
 Demonstrate
understanding of the
properties of selected
organic compounds
 Demonstrate in-depth
understanding of the
properties of selected
organic compounds
Demonstrate comprehensive
understanding of the
properties of selected organic
compounds
11
Chemical Reactivity
External
Demonstrate understanding of chemical reactivity
From their previous studies in science, students should have an understanding of
 Factors affecting the rate of reaction
 Names and formula of common lab acids and bases
 Reactions of acids with metals, bases and metal carbonates
 Acids, bases and indicators eg litmus, methyl orange and phenol phthalein; UI
 pH scale
 salts formed from reaction of acid with metal, base or carbonate
By the end of this topic students will be able to describe, interpret and discuss
1. Acids and bases
 acids and bases in terms of proton transfer
 calculations involving Kw, pH, [H3O+], [OH-]
 properties of aqueous solutions of strong and weak acids and bases including ionic species –
properties will be: conductivity, rates of reaction and pH
2. Rates of reaction
Factors that affect the rates of reaction as
 Concentration
 Temperature
 Surface area
 Catalyst
12
3. Equilibrium reactions
 Dynamic nature of equilibrium
 equilibrium constant expressions from equations, calculating value of Kc
 reactions as reactant favoured (K <1) or product favoured (K >1)
 factors that affect the position of equilibrium as

changes in temperature (  rH given),

concentration,

pressure or

addition of a catalyst
Text
BC Chapters 15 – 17
Practicals 15.1, 15.2, 15.3, 16.1, 16.2, 17.1 and 17.2
Assessment
School Exam – Term 3
NCEA Exam – November
AS 91166 v1 Chemistry 2.6
Demonstrate understanding of chemical reactivity
4 Credits
External
Achievement Criteria
Achievement
Achievement with Merit
Achievement with
Excellence
Demonstrate understanding
Demonstrate in-depth
Demonstrate comprehensive
of chemical reactivity
understanding of chemical
understanding of chemical
reactivity
reactivity
13
Redox
Internal
Demonstrate understanding of oxidation – reduction
From their previous studies in science, students should have an understanding of
 Reactivity series
By the end of this topic students will be able to describe, apply and discuss
1. Oxidation Number
 Determine the oxidation number for binary compounds and monatomic ions
 Oxidation and reduction in terms of change in oxidation number
2. Electron transfer in reactions
3. Oxidants
 as O2, I2, Cl2, Br2, H+, Fe3+, H2O2, MnO4-(aq)/H+, Cr2O72-(aq)/H+, OCl-, Cu2+, IO3-, conc.HNO3
4. Reductants
 as metals, C, CO, H2, Fe2+, Br-, I-, SO2, HSO3-, H2S, SO32-, H2O2
5. Carry out redox reactions
 use the properties of oxidants and reductants to identify the product of redox reactions
 Properties are limited to appearance ie colour and state
 identify the oxidant and/or reductant from reactions
6. Equations
 writing balanced oxidation–reduction equations
 classifying balanced half-equations as oxidation or reduction
7. Halogens as Oxidants
14
Text
BC Chapter 5
Practicals 5.1, 5.2 and 5.3
Assessment
Internal assessment – Term 2
AS 91167 v1 Chemistry 2.7
Demonstrate understanding of oxidation-reduction
3 Credits
Internal
Achievement Criteria
Achievement
Achievement with Merit
Achievement with
Excellence
Demonstrate understanding
of oxidation-reduction.


Demonstrate in-depth
understanding of
oxidation-reduction.
15
Demonstrate
comprehensive
understanding of
oxidation-reduction.
Table of Ions
Cations
+1
H+
Li+
Na+
K+
Ag+
NH4+
H3O+
+2
Mg2+
Ca2+
Ba2+
Zn2+
Pb2+
Mn2+
Cu2+
Fe2+
Hydrogen
Lithium
sodium
potassium
silver
ammonium
hydronium
+3
magnesium
calcium
barium
zinc
lead
manganese
copper(II)
iron (II)
Al3+
Fe3+
Cr3+
aluminium
iron (III)
chromium
Anions
-2
-1
FClBrIOHNO3CH3COOHCO3HSO3MnO4-
fluoride
chloride
bromide
iodide
hydroxide
nitrate
ethanoate
bicarbonate
bisulfite
permanganate
O2S2CO32SO42SO32Cr2O72CrO42-
-3
oxide
sulfide
carbonate
sulphate
sulfite
dichromate
chromate
PO43-
phosphate
Solubility Rules for Ionic Solids
1
Soluble
Group 1 metal ion compounds, Nitrate and
Ammonium compounds
2
Soluble
All metal Halides Except Pb2+ and Ag+ (PbAg)
3
Soluble
All metal Sulphates Except Ba2+, Ca2+ and Pb2+
(ABCP)
4
INsoluble
All Oxides, Hydroxides and Carbonates Except for
rule no. 1
16