So the professor allow us to take home this quiz before the exam, but he hasn't post up the answers yet.
I have other classes to tend to so I was hoping to get the answers here. Don't worry, I have attemptted work on them already, but I just need someone to check my work and if I'm doing something wrong please lead me in the right direction.
I posted images as well for clarity.
OK, first molecule is H2NNH2.
-Both N atoms have 3 bonding pairs and 1 lone pair.
-Molecular shape is trigonal pyramidal
-Bond polarity for H-N is polar because ΔEN= 0.9. N-N is nonpolar because ΔEN = 0.
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Molecular Polarity is polar because shape is trigonal pyramidal. THIS IS WHAT I AM NOT SURE OF. HELP. I was thinking nonpolar because the two trigonal pyramidal from each nitrogen cancel each other out. But i look online and everyone say this molecule is polar. So, molecule polarity only dependent on molecular shape then?
Second molecule is IBr3Cl-1
-Iodine has 4 bonding pairs and 2 lone pairs
-Molecular Shape is square planar
-Bond polarity for I-Br is nonpolar because ΔEN = 0.3. I-Cl is polar because ΔEN is 0.5.
Molecular Polarity is nonpolar because of square planar shape. I'm not sure about this. I'm thinking it's polar because at one end, (the I-Cl) end, it is polar. So wouldn't that mean there's a slight polar pull on that end?Help please.
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