Difference between revisions of "Ch10 Lec 1"
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| − | When we draw the electrons as "dots" we refer to these as '''Lewis Structures'''. If we were to draw the Lewis structure for neon (Ne) it would look like this: [[File:Screen Shot 2020-05-06 at 7.04.22 AM.png| | + | When we draw the electrons as "dots" we refer to these as '''Lewis Structures'''. If we were to draw the Lewis structure for neon (Ne) it would look like this: [[File:Screen Shot 2020-05-06 at 7.04.22 AM.png|50px]] |
Revision as of 12:05, 6 May 2020
(5/6/20, bes)
Welcome to the last Gen Chem lecture for the spring 2020 term. This is been quite an exercise in flexibility. We have covered almost all the topics usually covered, but we have not done them in as much detail as we would have if we met in person. We certainly did a few more WA!
The final exam for this class is scheduled for Weds, May 13th at 8 am. This will be given via WA and similar instruction will apply. I will send an email later with more details.
Covalent Bond (Sec 9.4)
In our previous lecture on ionic bonds, we discussed how elements like to have the "stable" electron configuration of the noble gases. In the case of ionic bonding, elements gain or lose an electron to attain this electron configuration, hence resulting in anions and cations that are electrostatically attracted to each other.
In a covalent bond, elements engage in a "sharing" relationship in order to attain the noble gas electron configuration. For example, we have known for a long time that there are diatomic elements in the periodic table...H2, N2, O2, all halogens like Cl2...why?
- Hydrogen atom has only 1 electron, so if 2 H-atoms share the 2 electrons, then
When we draw the electrons as "dots" we refer to these as Lewis Structures. If we were to draw the Lewis structure for neon (Ne) it would look like this: 