CURRICULUM SUMMARY –Autumn Term (September-December) 2014
SUBJECT: Chemistry
Week
1
2
3
4
5
6
YEAR GROUP: IB1 SL HL
Learning objectives
Stoichiometric relationship
To be able to deduce chemical equations when reactants and products
are specified.
To understand the concept of ‘atom economy’.
To be able to calculate the molar masses of atoms, molecules and
formula units.
To be able to determine the molecular formula of a compound from its
empirical formula.
To be able to solve problems relating to reacting quantities, limiting and
excess reactants, theoretical, experimental and percentage yields.
To calculate reacting volume of gases and manipulate the ideal gas
equation.
To use the experimental method of titration to calculate the concentration
of a solution.
To solve problems relating to molar concentration, amount of solute and
volume of solution.
Atomic Structure
To be able to deduce the number of protons, neutrons and electrons in
atoms and ions using the nuclear symbol notation.
To be able to calculate the abundance of isotopes from given data,
including mass spectra.
To be able to describe the relationship between colour, wavelength,
frequency and energy across the electromagnetic spectrum.
TEACHER: Dr Kumi Osanai
Activities (in brief)
power point presentations
worksheet and past paper exercises
videos/tutorial video
practicals/demonstrations
mini test
Standardisation of a solution
Acid-base titration to determine the concentration
Determination of the molar mass of volatile liquids
Back titration – determination of MCO3
power point presentations
orbital modeling
Flame colour and emission spectra of s-block
metals
worksheet and past paper exercises
videos/tutorial video
practicals/demonstrations
7
8
9
10
To describe the emission spectrum of hydrogen.
To be able to recognize the shape of atomic orbitals of s and p.
To be able to apply for the Aufbau principle, Hund’s rule and the Pauli
exclusion principle to write electron configurations.
(HL Additional)
To be able to solve problems using E = hv.
To be able to deduce the group of an element from its successive
ionization energy data.
To be able to explain the trends and discontinuities in first ionization
energy across a period.
To be able to calculate the value of the first ionization energy.
Periodicity
To able to deduce the electron configuration of an atom from the
element’s position on the periodic table.
To be able to predict the metallic and non-metallic behavior of an
element.
To be able to explain and describe the pH change for the reactions of
Na2O, MgO, P4O10, and the oxides of nitrogen and sulfur with water.
To be able to discuss the similarities and differences in the properties of
elements in the same group.
mini test
power point presentation
Properties of the alkali metals
Halogen physical properties and generating
chlorine
Aqueous halogens/potassium halide
displacement reaction
Physical and chemical properties of the period 3
elements
Periodic properties of the elements in the third
period
Shape of molecules
worksheet, videos, practicals, mini test
(HL Additional)
To be able to explain the ability of transition metals to form variable
oxidation states from successive ionization energies.
To be able to explain the nature of the coordination bond within a complex (HL Additional)
ion.
Determining the formula of a complex ion
To be able to deduce the total charge given the formula of the ion and
ligands present.
To be able to explain the magnetic properties in transition metals in terms
of unpaired electrons.
To be able to explain the effect of different ligands on the splitting of the
11
12
13
14
15
d-orbitals in transition metal complexes and colour observed using the
spectrochemical series.
To be able to explain the effect of the identity of the metal ion, the
oxidation number of the metal and the ligand on the colour of transition
metal ion complexes.
Chemical bonding and structure
To be able to deduce the formula and name of an ionic compound from its
component ions, including polyatomic ions.
To be able to explain the physical properties of ionic compounds in terms
of their structure.
To be able to deduce the polar nature of a covalent bond from
electronegativity values.
To be able to deduce the Lewis structure of molecules and ions showing
all valence electron.
To be able to use the VSEPR theory to predict the electron domain
geometry and the molecular geometry.
To be able o predict the bond angles.
To be able to predict the molecular polarity from bond polarity and
molecular geometry.
To be able to deduce the resonance structures.
To deduce the type of intermolecular force present in substances.
To be able to explain the physical properties (volatility, electrical
conductivity and solubility) in term of their structure and intermolecular
forces.
To be able to explain the electrical conductivity, malleability trend in
melting points of metals.
To be able to understand the properties of alloys in terms of nondirectional bonding.
(HL Additional)
To be able to predict whether sigma or pi bonds are formed from the
linear combination of atomic orbitals.
Power point presentation
Shape of molecules and ions and VSEPR theory
– modeling
Bond polarity and intermolecular forces
Intermolecular forces and ideal gas behavior
Bond enthalpy and energy profile - simulation
worksheet, videos, practicals, mini test
16
17
To be able to deduce the Lewis structures of molecules and ions showing
all valence electrons.
To be able to deduce using VSEPR theory of the electron domain
geometry and molecular geometry with five and six electron domains
associated with bond angles.
To be able to explain the wavelength of light required to dissociate
oxygen and ozone.
To be able to apply FC to ascertain which Lewis structure is preferred
from different Lewis structure.
To be able to describe the formation of sp3, sp2 and sp hybrid orbitals in
methane.
To be able to identify the relationship between Lewis structure, electron
domains, molecular geometries and types of hybridization.
Energetics/thermochemistry
To be able to calculate the heat change when the temperature of a pure
substance is changes using the equation.
To be able to conduct a calorimetry experiment for an enthalpy of
reaction.
To be able to apply the Hess’s law to calculate enthalpy changes.
To be able to calculate the enthalpy.
To be able to determine the enthalpy change of a reaction that is the sum
of multiple reactions with known enthalpy changes.
To be able to calculate the enthalpy changes from known bond enthalpy
values and compare these to experimentally measured values.
To be able to evaluate the potential energy profiles in exo- and
endothermic reactions.
To be able to understand the bond strength in ozone relative to oxygen in
its importance to the atmosphere.
(HL Additional)
To be able to construct Born-Haber cycles to group 1 and 2 oxides and
chlorides.
Power point presentation
Enthalpy change of displacement reaction
Enthalpy change of neutralization reactions
Measuring enthalpy change of a hypothetical
reaction by Hess’s law
worksheet, videos, practicals, mini test
(HL Additional)
To be able to construct the energy cycles from hydration, lattice and
solution enthalpy.
To be able to calculate the enthalpy changes from Born-Haber or
dissolution energy cycles.
To be able to relate size and charge of ions to lattice and hydration
enthalpies.
To be able to perform lab experiment which could include single
displacement reactions in aqueous solutions.