This has been an awesome eleven-weeks (or so) – you have been fantastic! Thanks so much for all your hard work. I have the best chemistry and physics student in the world!! Have a wonderful Lord’s day today, and let’s ask the God for a wonderful campus revival next week!
CHEMISTRY: Finally! We finished average atomic mass! 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 Thursday on moles, mass, and Avogadro’s number. I still say he has a cool name…
CHEMISTRY: Can you believe atoms are that small – and the nucleus even waaaaaay smaller! Here’s another picture of atomsfrom the IBM Almaden Research Center. These are iron atoms on top of copper. Being able to move atoms around like this was a giant leap in the field of nanotechnology! (Sorry about that, bad pun! ) Here’s the short lecture from Wednesday. What did you think about Lise Meitner’s story? Well, now you’ve finally got the formula for average atomic mass. Use it to do the problems tonight. You can do it!
HON CHEMISTRY: Chocolate atoms? Good luck studying for the chapter 3 test! Here’s the review from Wednesday. Don’t forget to practice the problems and practice applying what you are learning. I’ll be praying for you!
PHYSICS: So an object at rest can be at equilibrium, but what about an object that is moving? And how does equilibrium relate to Newton’s first law? Or Newton’s second law? And what if you don’t have balanced forces. Here’s the lecture from Tuesday on just that! Now remind me, net forces produce what?
HON CHEMISTRY: Hey guys, here’s the lecture from Tuesday on moles, molar mass, and Avogadro’s number. Remember, it’s all in terms of one mole. The mass of one mole, the molar mass, is the average atomic mass of the element in grams (periodic table). And the number of atoms in one mole is …. well you know that. Speaking of moles, isn’t he cute? Well, beauty being in the eye of the beholder and all. Hmmmm………
CHEMISTRY: Thank you, Lord, for keeping us safe today! And thank you, guys, for being patient while we waited for the bad weather to pass over. Hasn’t this just been the strangest chapter – schedule wise, I mean? It seems every day we don’t get where I wanted us to because of some interruption or other. But I’ll tell you, I’m trusting God with that! Here’s the lecture from Tuesday on atomic number and isotopes. How are you doing on writing nuclear symbols? Also make sure you can use them to determine the number of protons, neutrons, electrons, etc. Tomorrow let’s finish average atomic mass!
HON CHEMISTRY: Hey guys, a couple of your fellow students have requested a help session tomorrow, Wednesday, morning at 7:15. That’s great for me. As a matter of fact, I think it’s a good idea to have it before the day of the test. I’ll be there, hope to see you too – and hopefully no flat tires this time! BTW – have you checked out the Ch3 Study Suggestions & Stuff to Know sheet on Edline? Click here for a copy: Ch3 Study Suggestions & Stuff to Know
Oh, and FYI – homework for Tuesday night is Pg. 88 – 91: 14 – 18, 21 – 24, 28 (Only do b, c, and e on the ones with parts!)
HON CHEMISTRY: Awwww….aren’t they cute! So what do you think the average atomic mass of puppies is? Here’s the lecture from Monday on calculating the average atomic mass of isotopes. Isotopes…. not puppies.
CHEMISTRY: Great job on using experimental results to form a conclusion! Here’s the lecture from Monday on the discovery of electrons, the nucleus, and neutrons. Lots of stuff to learn, but make sure you just don’t learn facts. Check out the videos in the VodPod collection below. You can find the cathode ray tube experiment, Rutherford’s gold foil experiment, and others. Be able to explain not only what they did in their experiments, but how Thompson and Rutherford used the experimental results to discover the electron, nucleus and protons. And we’ll finish your “atoms” tomorrow!