HON CHEMISTRY: Can you guess what it is?/ It’s a picture of uranium ore under UV light. Cool, huh! Here’s the discussion from Friday on the average atomic mass homework problems and then the rest of our discussion of the properties of radioactive nuclides.
CHEMISTRY: So, would you like to be Greg on CSI? Great start on empirical formulas today!
The hardest part is that it’s not a set formula for you to plug and play, but if you’ll keep in mind that you’re really just looking for subscripts which are just moles, you’ll be able to think it through. Percent to mass, mass to moles, moles to smallest whole number ratio.
Monday we’ll talk about a little step you get to add at the end. 🙂
HON CHEMISTRY: Welcome to nuclear chemistry! No, really – I think you’ll be surprised how much nuclear chemistry is already a part of your everyday life. And now you know where E=mc2 came from!!
By the way, when you get a chance, read about the life of Marie Cure – fascinating woman of science with an incredible story!
CHEMISTRY: Great job with the different ways to look at percent composition! A little bit different lab procedure, huh?!! If you need to make it up, this lab is answered only on notebook paper – be careful to show correct data and calculations!
BTW – I think you’ll find that percent composition problems are really easy to catch on to. Make sure, though, you can write chemical formulas (I won’t give them to you!) and that you’ve memorized the formulas for acids and those chemical names for common substances so that you’ll have something to find the percent composition of!
PHYSICS: See?! I wasn’t kidding about the balancing rocks movement!
Great job today on making connections between work and energy! I think you’ll like using the work-energy theorem, it’ll save you some time and a couple of steps. Don’t forget about friction!
HON CHEMISTRY: Awwww….aren’t they cute! So what do you think the average atomic mass of puppies is?
Here’s the discussion for Wednesday on isotopes and calculating the average atomic mass of isotopes. Isotopes…. not puppies. 🙂
CHEMISTRY: So the little mole turns out to be a pretty big deal – and a very handy tool!!
Great job today! Here’s discussion on formula mass and molar mass, and then using molar mass and Avogadro’s number as a conversion factor. You’ve got a couple of great tools – so now think through the problems and go forth and conquer!! Be sure and practice them so you don’t forget!
PHYSICS: Funny thing about words, all this work you thought you’d been doing, was it work after all?
Great intro to chapter 5! I think you’ll do great with the work problems, just remember everything from the last chapter and multiply by d!
flickr photo by *hb19
CHEMISTRY: So… how big a bucket do you think we’d need to hold a mole of frogs? 🙂
Nope, not the furry brown creature that burrows underground, it’s a whole different thing! Here’s the lecture from Friday on moles, mass, and Avogadro’s number. I still say he has a cool name… 🙂
HON CHEMISTRY: So how do you feel about being made from earth, air, water, and fire? Here’s the very short intro we did on how we ended up with the atomic theory. Had you ever heard of Lavosier, Proust, and Dalton?
And how did you do with your comparison of Dalton’s Atomic Theory with the Modern Atomic Theory? Could you discuss it in more detail at a later date??