Grade 12 U Chemistry Page

Date: May 2002

First off, if it has been a while since you have done chemistry then you should go to the grade 11 material. Go to my main home page at http://www.oocities.org/rjwarren_stm (yellow page) and visit the links listed there.
Look at the topics that are not in this course. This is the material that you should already know. Review it if necessary

Main Topics = Course Outline

  1. Atomic Structure and Molecular Architecture
  2. Organic Chemistry; Nomenclature, Homologous Groups or Families and Reactions
  3. Energy, Enthalpy and Reactions Rates
  4. Equilibrium; An Introduction
  5. Equilibrium; Applications, Acid Base Equilibrium
  6. Redox reactions and Electrochemisrty
  7. Independent Investigation on Nuclear Chemistry

Skip to Units on Enthalpy, Equilibrium and Electrochemistry

Continue on to page two click here and away you go!

Units in Review

Unit I

A review of grade 11 Topics covered are: Atomic models: Dalton's Atomic Theory, Thompson model, Bohr model, Sommerfeld's mathematical improvementsP> Black body radiation data was one on the reasons that caused the development of Quantum Theory of the Atom. Here's a graph of the data with classical and Planc's theoretical explination.

The above picture is that of light being broken into its rainbow of colours; only a small fragment of the Electromagnetic Spectrum Here's the rest of the story

Hydrogen spectrum is the easiest to study. Three series to know are i) Lyman, ii) Balmer, iii) Paschen. Balmer series is shown below.

Be able to explain this spectrum in terms of energy level photon emmissions

Lab on gas discharge tube spectrum; noble gas
To review these spectrum lines visit Spectrum
Zeeman Effect and what it leads to. Below is an actual line spectrum showing the effect. The multiple lines are caused by a strong magnetic field.

de Brolie's wave model. Quantum numbers; n, l, ml & ms . s, p, d diagrams with appropriate m values. All of these orbital probability functions are derived from the Schrodinger wave equation

Which when solved for the assigned values of l result in these shapes

These are orbital shape designations based on the value on l

Electron configurations. Energy level diagrams
Orbital degeneracy, Hund's Rule, Aufbau principle, Pauli Exclusion principle, Heinsburger Uncertainty Principle
How do s, p, d, f fit into the periodic table?

Stability of half and full orbitals, electron configuration exceptions (Cr & Cu). Ionic bonding, electronegativity, ionization energy, electron affinity, polar bond, polar molecules.An example of a polar BOND is shown below

When the water molecule forms the two polar bonds do not cancel each other out but act in the same direction resulting in a dipole moment in the water molecule
Be also observant of the shapes of these molecules

More diagrams of polarity in molecules

Some general overall trends in the periodic table are listed in this diagram

Lewis dot diagrams, is an example of nitrogen as an atom
Here's nitrogen in the nitric acid complex

Covalent bonding ==> shapes of molecules

VSEPR theory and predicting molecular shapes. See example sheet or student generated note. Similar to what is below but much more complete.

You must be able to identify the shape of molecules, give the number of lone pairs and bonding pairs surrounding the central atom.

Molecular aggragates

In this chapter or sub-unit we are concerned with NOT what holds atoms together forming molecules, but what forces hold these molecules together with other molecules. If molecules did not stick together all materials would be gaseous. Hence, forces exist that hold molecules together resulting in liquids and when very strong, solids. These different forces will be investigated.

Molecular Architecture & Bonding
Hand-outs on; Language of Chemistry Molecular Architecture, Types of Solids, The Forces: strong & weak, Characteristics of Crystaline solids
Forces holding atoms/molecules together with each other. Key word is INTERMOLECULAR
Bonding Forces: Strong and Weak
Strong => Ionic, Covalent, & Metallic
Weak => Hydrogen bonding, Dipole-dipole, & London or Induced dipole
Molecular forces
London Forces, van der Waals forces, dipole interactions
Metallic, Ionic, Covalent, Network aggragates. Network lattice structures in two and three dimensions.
Properties of these materials

A short summative note can be found at Intermolecular Forces

Unit Two

Organic: A very good set of notes may be found at Organic Notes Start of organic; hybridazation of the carbon atom single double and triple bond formation. Use of model
Sigma, pi bonds with sp3, sp2, sp, hybridization.

Start out with basic nomenclature, Alkanes, Alkenes Alkynes IUPAC naming system. Cis, trans isomers, naming chloro-alkanes
The alkane, alkene, alkyne family of homologous compounds; some examples are shown below

Bond rotations resulting in isomers.

Preparation and reactions of the following listed series or families. Make sure you can recognize the functional group that defines the family or series .

Functional groups and how to name these compounds.
Simple reactions, tests for unsaturate bonds, formation of esters,

Addition to an Alkene

Make sure you know the name of this type of reaction.

Here's a summary of various reactions for the alkenes

Use of oxidizing reagents such as KMNO4 and K2Cr2O7.
Reactions of primary, secondary and tertiary alcohols and products produced.
Experiments that should be done: an outline and results.
Group lab on this, while you use your text book for summaries.

Polymers: Condensation & Addition , names of the six or seven most common, uses and monomers that produce them. Making Nylon 6, 10. Quiz on nomenclature and reactions.

Continue on to page two click here and away you go!