(Polar molecules, Non-polar molecules, etc.)
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Hey, I am stuck on the drawing portions of these problems in Sapling. I understand the other parts of the questions and got them right, which makes me think I understand the overall properties and have a general understanding but I can't seem to figure out the structures according to Sapling. Any tips?
Hi! Generally, it's a good idea to first count all the total electrons present in the molecule. Then, find the atom with the lowest electronegativity and put it as your center atom. I like to connect the rest of the atoms to the central one with one bond, then figure out if there needs to be lone pairs or double bonds based on the number of electrons that are left and the formal charge. Hope this helps:)
Hi! For question 17 there are 3 structures for C3H4 you have to draw. One of the structures has a C-C double bond. The other has a C-C triple bond. And the last has a C-C double bond but in a ring shape (the three carbons are formed in a triangle). For question 18, the C-C bonds for all 3 structures has a double bond. Hope that helps!
Hi! Drawing the structures was a little bit harder since sapling was looking for something in particular. As a general rule I would say just play around with the different bond types. First, calculate the number of valence electrons in the molecule. Then, try and form an octet for each atom. After that, calculate the formal charge to match them up. Some are easy to see after a while. For example, O has a formal charge of 0 when it has 2 bonded pairs and 2 lone pairs. C likes to have 4 bonded pairs. Generally, the more electronegative atom goes in the middle and I've noticed H atoms are usually on the outside (since they can only form 1 bond).
Hi! I was stuck on #17 as well. One of the structures will have the C's connected in a ring shape. As for 18, each structure has a similar shape except that the chain of C's gets longer. They each have a double bond as well. Hope this helps!
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