HON CHEMISTRY: Here’s our exam help session from this afternoon. Don’t just read and memorize your notes. Practice, practice, practice!!!

HON CHEMISTRY: So what do you think would cause these beautiful colors? Great intro to the properties of acids and bases, indicators and pH! Don’t forget The Physics Classroom assignment. If you need help on the last two levels, click on the Help Me button. It will give you the pH chart that matches certain indicator colors. Here’s a hint – Phenolphthalein indicator is always hot pink/magenta in a base.

And last hint – the more negative the H3O+ concentration (that means the higher the negative exponent) the more of a base that it is. The lower the number of the exponent (which actually makes it a higher number) the more of an acid it is.

How’s the exam review packet coming along?

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HON CHEMISTRY – Are you practicing for tomorrow’s test? And how are you doing with your own “Stuff to Know” sheet?

For chapter 6, you don’t have to use orbital notation to show covalent bonds. Also, hybridization won’t be on this test. Practice Lewis structures, molecular geometry, dipoles, drawing ionic bonding, and the discussion questions! There will be two on this test – one from chapter 5 and one from chapter 6. God bless you as you study and practice!

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HON CHEMISTRY: Molten iron, wow! Here’s our review of drawing ionic bonds and our discussion of ionic vs. covalent bonding, followed by metallic bonding.

Aren’t you glad there are no structures to draw for metallic bonds?! Make sure you can use the electron sea model to explain the properties of metals. Also be able to compare and contrast all three types of bonds.

HON CHEMISTRY: So how ’bout Johannes van der Waals and those intermolecular forces? Tons of application, from bugs walking on water to little fishes breathing dissolved oxygen. And what about the condensation that forms on the outside of an iced tea glass? Hmmm….

And then on to a different way that atoms come together – ionic bonding. Keep in mind that when you write ionic bonding, you’re not trying to arrange a single structure like you do with Lewis structures. Instead, you’re writing an equation that shows electrons being lost by one atom and gained by another atom. And make sure you put the dots in the right order!

Under today’s vodcast – the help session from this afternoon and our practice with Lewis structures.

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Help Session from Tuesday afternoon (Lewis structures)

HON CHEMISTRY: So we’ve put it all together – Lewis structures, molecular geometry, dipoles, and bond type. Here’s our look at the homework worksheet. How’d you do?

After that, a beginning look at the importance of molecular geometry with solubility, and a beginning look at intermolecular forces. Lots of applications, from using peanut butter to get gum out of your hair to little fishes breathing dissolved oxygen. Let’s do more tomorrow!

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