CHEMISTRY: Great job practicing multiple bonds with Lewis structures today! Here’s the lecture from yesterday on double and triple covalent bonds, with resonance at the end.
Be careful about getting too happy with double bonding – count electrons and don’t forget CONS. And what else? Oh yes, PRACTICE, PRACTICE, PRACTICE! We’ll put one more twist on Lewis structures tomorrow!
Now go forth and conquer the Lewis Structures Worksheet! Be sure and get the updated worksheet. The last compound should be N2O3.
HON CHEMISTRY 2-13-14 Multiple Bonds & Polyatomic Ions from Tammy Skinner on Vimeo.
It’s so cool how atoms are so detailed and can only work with other certain molecules.
I think I’m starting to get the hang of the lewis structures. They are pretty easy if you think ahead about which atoms will bond together.
I never realized that only certain atoms could form double bonds. That’s pretty interesting.
It really helped when we did those tough Lewis structure problems. I feel like I understand them so much better now.
In our works citied page, do we have to repeat the source every times it’s used in our paper?
Jessica – Not unless the source is being used for something different than what you first used it for.
you taught me something new this week, i knew that bonds existed, i just didnt know about them in depth. I didnt know there were different types.
It would be interesting to know who came up with the idea of CONS and how they determined that only those four atoms could have multiple bonds.
I’m glad we’ve got to practice the Lewis structure so much in class it is helping me understand it better.
Why can only the CONS elements form double bonds?
I found it very helpful and interesting to know that only CONS have double bonds and that polyatomic ions can have resonance structures.
I found it very interesting how a Polyatomic Ion’s Lewis structure is formed. Its just the original structure, but with brackets and its charge.
How do I know where to put the first dots representing the valence electrons of the first element that goes in the middle: (top, bottom, left, right, in twos) ?
Mollie – I base it on what element the first element is going to be bonding to. For example, if it’s bonding to chlorine, I put at least one electron on a side so that chlorine will have something to bond to. If it’s bonding to oxygen, I’ll put two electrons on one side, if I have them, because that’s how many electrons oxygen needs. It doesn’t always work out perfectly, but I try! 🙂
I really have enjoyed all the practice we have done with the lewis structures. I feel like I could ace a test if we had one on Monday!
what is the maximum number of resonance structures a compound or an ion can have?
For my project, if I draw more pictures… Can I get extra credit?
Mary Grace – Not necessarily, it all would depend on what the illustrations were and the amount of detail you put into them. Talk with me about it in class and I’ll explain.
I had no clue that only Carbon, Oxygen, Nitrogen, and Sulfur could form multiple bonds. I find that so interesting.
I’m glad we practiced the Lewis structure so much it really helped me
Lewis structures I find quit easy I wish most of it was like them. Being able to draw them out also seems to bring a substance to something that is there to a level easier to comprehend other than just knowing its smaller than the smallest small.
I get the Lewis structure but it starts to get confusing when the charge is there.
i thought doing the lewis structure would be hard when i first saw it but after we practiced it became extremely easy.
The Polyatomic ion lewis structures are a tad bit more difficult… I don’t enjoy ;-;
Will there be a help session soon on the Lewis structures so I can get some more practice especially with the double and triple bonds?
Bronson – Sure! Let’s talk about it in class and set a date if you guys want to have a help session.
The double and triple bonds confused me at first but now I feel like I have a better grasp of it
Knowing that the CONS elements are the only ones that can form double bonds makes Lewis structures easier
The syllabus says the project is due the 10th instead of the 16th. I hope that is a mistake.
Today I learned that the VSEPR theory explains the shapes of molecules
Today in class was interesting in that we got to use computers and learn about power point and jing.
The representations of the molecules and their bonds in the 3-D molecule lab showed that bonds aren’t just lines between atoms. The atoms are actually sharing pairs of electrons, and the shared pairs of electrons represent the bonds between the atoms in the molecules.
The molecular geometry wasn’t hard at all to learn and pick up on. It seemed like it would be but I actualy enjoyed doing that kind of stuff.
For the project, we don’t have to put how we returned to civilization do we? I read the sheet and it only says to write journal entries for when we do but I was unsure if that had to be a part of our story.
The STEM day was very interesting. I did not know that pharmacists had different jobs other than working at a CVS or Wallgreens.
I found STEM track so interesting! I was informed about so many job options that I never knew existed.
So, we DONT do the book homework this weekend?
Kelly – No book HW this weekend, just your project! 🙂
Thank you for not giving us homework this weekend so we can work on the project and for giving us more time on the 3d molecules.