(Polar molecules, Non-polar molecules, etc.)
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Is it safe to assume that any covalently bonded molecule with a lone pair on the central atom will be polar? How can polarity be determined with larger molecules in class Lavelle usually draws arrows to demonstrate what direction the positive and negative poles are at how is this determined.
yes going off of the previous post, molecules that are symmetric are non-polar, for example, a square planar molecule is non-polar despite having two lone pairs due to it being symmetric, usually larger molecules with different elements that isn't symmetrical are non-polar. To help determine if it is polar or not find the central atom and see if the dipoles are the same on both sides .
With that logic, it would make sense that due to the presence of a lone pair then the shape would not be symmetrical, therefore electrons would not be evenly shared. However I would say drawing out the structure just to demonstrate and prove its polarity. I'm not sure that your reasoning would suffice during a test.
405211415 wrote: To help determine if it is polar or not find the central atom and see if the dipoles are the same on both sides .
Going off of this, to determine if the dipoles are the same or not, you can look at the electronegativity of the (different) atoms surrounding the central atom.
amogha_koka3I wrote:So just to confirm, does polarity have anything to do with if there are single, double, or triple bonds?
Just as VSEPR structures daren't drawn according to whether they have single, double, or triple bonds, polarity is also not determined in this way. Polarity doesn't have to do with single, double, or triple bonds.
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