Students completed their tests for the Hazardous Materials Assignment and worked on review for the test.  Please add p.157 #51 to your review.  The unit test will be on Wednesday, to allow more students the opportunity to ask questions.  The assignment is still due on Wednesday.  There will be extra help at lunch on Wednesday in room 102.

Most students completed the tests on the solids.  Begin to write your lab report.  It is due on Wednesday.  There is extra help on Monday at lunch in room 102.
Your unit test is Tuesday, March 1.  Review questions for the test include:  p.154-157 #6-9, 11, 15-24, 28-30 not looking at values for atomic radius, I.E., E.A - just trends, 39 no design, 40ab, 44, 45, 49, 52; In sentences, explain which would have the higher electron affinity, an atom of chlorine, or an atom of bromine, using terms such as shielding effect, net nuclear charge, core electrons, and/or valence electrons.

Most students completed most of the tests on the solids.  Begin to write your lab report.  It is due on Wednesday.
Your unit test is Tuesday, March 1.  Review questions for the test include:  p.154-157 #6-9, 11, 15-24, 28-30 not looking at values for atomic radius, I.E., E.A - just trends, 39 no design, 40ab, 44, 45, 49, 52; In sentences, explain which would have the higher electron affinity, an atom of chlorine, or an atom of bromine, using terms such as shielding effect, net nuclear charge, core electrons, and/or valence electrons.

A review of naming and writing formulas of compounds from grade 10 was done for ionic compounds.  See p.95-103, 104-105 in your text for help and download the review lesson and some practice questions from the unit 1 page of this site, as the PDF file "ionic nomen lesson".  The articles for your Hazardous Materials Anticipation Guide are in the PDF file "hazmat articles".
Homework:  p.103#20, 21; p.105 #23; p.106 #1-3

There are two main types of compounds:  ionic and molecular.  Molecular compounds can have either polar molecules or non-polar molecules.  The particles in each type of compound have different strengths of attraction, which we can use to explain a number of properties, such as boiling point, solubility in water, odour, and state at room temperature.
Particles can be attracted to each other by forces that cause them to clump together and become a solid.  Ionic attraction is a strong force so ionic compounds are solids at room temperature.  Molecular compounds have strong covalent bonds inside them, but they are attracted to other molecules by weaker intermolecular forces.  Non-polar molecules are attracted by the weakest intermolecular forces, so they are often gases at room temperature.  Polar molecules are attracted by the positive and negative ends of other polar molecules, so these are often liquids and solids at room temperature.  Text reference is p.90-93.  The Power point slide show is on the unit 1 page of this site and is called "interparticle bonding lesson".
Homework:  p. 74 #6; p.84 #6; p.94 #6; and complete the Hazardous Materials Assignment Anticipation Guide, using the links on the unit 1 page of this website.

You should be able to use electronegativities and shape to predict whether a molecule is polar or non-polar.  For help, see p.88-91 in your text. 
Homework:  p.94 #1-4, 7

We learned to use electronegativity values of each element to determine whether the electrons in a covalent bond are equally or unequally shared.  Consult p.71-74, 85-86 in the text for help with this.
We did a molecular model-building activity.  If you were absent today, download the model-building activity from the unit 1 page of the website, in order to complete the Lewis diagrams for the models you will be building.
Homework:  p.84 #3, 4; p.86 #11-13

We had a formative quiz on last week's work.  We learned how to draw Lewis diagrams of compounds with covalent bonds.  Refer to p.75, 81-82 for help with this material. 
Homework:  copy Table 3.1 from p.67 into your notes; answer p.81 #7; p.82 #8-10; p.84 #3, 4

We discussed the reason for the trends in atomic radius, ionization energy, and electron affinity, using the handout "trend explanations" found on the unit 1 page of this site.  Consult p.52, 55, 58 for help with this explanation.
We also discussed how ionic compounds form, using Bohr diagrams, and using Lewis diagrams.  The handouts used, "ionic comp handout" and "Lewis diag handout" are downloadable from the unit 1 page of this site.  Consult the text p.75-78 for help.
Homework:  Complete the questions on the Lewis symbol handout and answer p.46 #6 and p.78 #5.

Refer to p.49-54 in the text for help with this work.
Homework:  p.52 #7; p.55 #8, 9