Download Learning Intentions Inorganic

ADVANCED HIGHER LEARNING OUTCOMES
ELECTRONIC STRUCTURE
Electromagnetic spectrum and associated calculations
o Know that electromagnetic radiation can be described in terms of
waves
o Define wavelength, frequency, give the symbols and units for
these values
o Give a value for the speed of light with appropriate units
o Know the equation that relates velocity (speed), wavelength and
frequency
o Explain the dual nature of light/radiation
o Know the equations that enable the energy of a photon or of a
mole of photon to be calculated
o Know the name of the constants represented by h and L and
where to find their values.
Electron configuration and the periodic table
o
State the name of the element whose emission spectra provide the evidence for
energy levels
o
Define the terms quanta and quantised
o
Know the which energy transition is associated with the release of a photon
o
Understand how to use an emission spectrum to calculate the energy associated with
the release of a photon.
o
Understand what the energy associated with a photon corresponds to within the atom
o
Know why spectra of elements with more than 1 electron give evidence of sublevels
or orbital’s
o
Understand the terms principle energy level and sublevel
o
Know that electrons have a dual nature
o
Give a definition for ‘orbital’ in terms of probability
o
Name the types of orbital, their characteristic shapes and identify which orbitals and
how many are found in each principle energy level.
o
State the Pauli exclusion principle and state how it governs the maximum number of
electrons in an orbital
o
Define the term degenerate
o
State the Aufbau principle and explain how it relates to the filling of orbitals
o
Be able to draw a diagram to show the relative energies of orbitals in the first 4 shells
o
State Hunds rule and explain how it relates to the way electrons fill degenerate
orbitals
Write electronic configurations using box notation or spectroscopic notation for
elements 1-36
o
o
Identify the 4 blocks of the periodic table and explain how the blocks relate to
electron filling of orbitals
o
Explain how the first ionisation of elements gives evidence of the different stabilities
of different electron configurations
o
Explain how the first, second and third ionisation energies give evidence of the
stabilities of the electron configuration of the species from which the electron is being
removed
Spectroscopy
o
Understand the difference between emission and absorption spectroscopy in terms
of electron transitions and the spectra seen
o
State the approximate wavelength range of visible and u.v. spectra
o
Understand how spectra give evidence of the identity and quantity of a species
BONDING
Covalent Bonding
o
Understand that there is a continuum of bonding and know where ionic, non-polar
covalent and polar covalent bonding lie on the continuum.
o
Explain dative bonding and give a common example
o
Relate the type of bonding likely to be present to the difference in electronegativity of
the elements involved.
o
Use different theories to explain the behaviour of electrons during the formation of
covalent bonds
o
Use Lewis diagrams to show bonding and non-bonding electrons in molecules
o
Explain what is meant by a resonance structure and give 3 examples.
Shapes of molecules and polyatomic ions
o
Predict the shapes of molecules from the number of bonding and non-bonding
electron pairs present.
o
Understand the terms linear, trigonal, tetrahedral, trigonal bipyramidal and octahedral
and relate these to the number of electron pairs present.
o
State the order of repulsion of electron pairs
o
Explain how electron pair repulsion accounts for the differing bond angles seen in
methane, ammonia and water.
Transition Metals
o
Give a definition of a transition metal
o
Explain how the Aufbau principle applies to the atoms of Cu and Cr
o
Know which electrons are lost first when transition metals form ions and explain why.
o
Know how to determine the oxidation state of an element in a compound
o
Explain why transition metals can have ions in different oxidation states with different
stabilities
o
Understand why compounds of the same element can have different colours
o
Explain oxidation and reduction in terms of oxidation number
o
Give a general rule about the oxidation number of oxidising and reducing agents.
Transition Metal Complexes
o
Define
o
Understand the terms monodentate, bidentate and hexadentate as applied to ligands
o
Explain why d orbitals are no longer degenerate in a complex ion
o
Know the IUPAC rules for naming complexes
o
Explain how the position of a ligand in the spectrochemical series affects the size of
the ligand field
o
Explain in terms of d-d transitions why complexes are coloured
o
Define absorption and emission spectroscopy
a) complex ion
b) ligand
c) co-ordination number
o
Relate the wavelengths 200-400nm and 400-700nm to the appropriate type of
spectroscopy
o
Explain how spectrometers use light intensity to determine absorption
o
Explain how transition metals can act as catalysts in terms of their variable oxidation
state, reaction pathways and intermediate complexes