![]() ![]() Here is another very in-depth discussion on color. Physics classroom has a good explanation. When we combined colors in Kindergarten we used the subtractive method. With the additive method, the primary colors are red, blue, and green. I did a bit of googling and the primary colors are different depending on which method of combining colors you use. WARNING: In this module, he tells the kids that the primary colors are red, blue, and green. The math isn’t difficult and shouldn’t be too difficult to teach. Wile includes light in this module so that the student will understand Rutherford’s experiment and how it let to the Bohr model. His experiment led to the planetary model of the atom which later led to Bohr’s model of the atom. This was later disproved by Ernest Rutherford. He believed the electrons were suspended in the atom like plums in plum pudding. Thompson discovered electrons using the Cathode Ray Tube. He spent a lot of time on this and made it much more wordy than it needed to be, in my opinion. Basically teach the kids how to write the isotopes and determine how many protons and neutrons an element has based on its symbol. I don’t think he does a very good job of explaining the isotopes. Carbon-13 just has one more neutron than Carbon-12. ![]() Carbon-12 and Carbon-13 are still Carbon atoms. It is important to understand that isotopes are atoms that have the same number of protons, but different numbers of neutrons. They should know what the mass number tells and be able to tell how many protons, electrons, and neutrons any atom has. Now, if you are like me, you have already discussed this in-depth with the kids. It is likely that you won’t even need to explain this topic any further. The experiment is unnecessary, and we had little success with it when we did it. This is one of those things that the kids should already know if they have played with magnets at any time in their lives. Like charges repel and opposite charges attract. I think it is because we have been focusing so much on the periodic table that this was an easy module to move into. I decided that I wanted to move into Module 7. It is sad but colorful!Īfter telling you that I was going to move into Module 4 after Module 3, I changed my mind. To avoid any kind of issue, I made my own. I get nervous about grabbing pictures from other places. I wanted to have a picture sitting at the top of my post. This is my first attempt at drawing in paint. This is the foundation of drawing Lewis structures. There is just a little more that you will have to learn in the next module about bond shapes. Remove the rest of your paired electrons.Īnd there you go. So, instead two more Chlorine atoms join the party.ĭoes that just look like a bunch of red dots? It does. Remember, it wants to have a full 8 as well. One chlorine atom can’t give a Phosphorus atom three of its electrons. This is how we draw the Lewis structure in order to get the correct bonds.Ĭhlorine has one unpaired electron. If I were to pair up two electrons, there would be an empty spot. There must be an electron at each of the spots on the compass before you start pairing them up. No, you can’t pair up two of the singles. Here are the Lewis structures of Phosphorus and Chlorine. We know all the other electrons are happily paired together. You don’t need to draw all the electrons after you know how they are bonded. Yes, this may look like your face while you study Chemistry, but it is really just a Lewis structure showing how an O 2 is bonded. So, if I want to draw the Lewis structure for the oxygen bond, I just match up the lonely electrons. Now, I know that oxygen is a diatomic atom, meaning that they never go it alone. I just drew six, happy little dots around an oxygen atom. This tells me that Oxygen has 6 valence electrons. You only need to know the number of valence electrons which you get from the group number of the element. That is all you have to know. Here is a quiz to check your knowledge.ĭrawing Lewis structures is not difficult. If you are still have trouble check out this page to compare the two. It is easiest for me to remember that two non-metals form covalent bonds, and a metal and a non-metal form an ionic bond. ![]() Some are happy to share as in a covalent bond. Remember that all the atoms want 8 valence electrons in their outer shells. You can find some links there to help you write the chemical formulas. I wrote about nomenclature in my post about on Module 3. If you have explained the periodic table in detail, your student shouldn’t have any difficulty with this module. I touched on it a little in my discussion of Module 7. Understanding this module is important for all Chemistry. It is important to understand how atoms bond. Module 8 discusses molecular structure which should have been covered in the very first week of class. ![]()
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