A. Classify the following molecules as polar or non-polar (write below the chemical formula in the first column. Explain your answer in terms of the (a) Lewis structure (b) molecular geometry and (c) bond polarity. (You can add rows if you need more spaces for your explanation.) Hint: Although I am not asking you to give the no. of bonding and non-bonding pairs, you have to do it to be able to identify the electron pair geometry and molecular geometry. Note: Items #1 to #4 are hypothetical molecules. The number of valence electron/s of the hypothetical atoms are given in parenthesis.) There is no need to give actual molecules to represent them. Polar or Non-polar Explanation 1. nod

A. Classify the following molecules as polar or non-polar (write below the chemical formula in the first column. Explain your answer in terms of the (a) Lewis structure (b) molecular geometry and (c) bond polarity. (You can add rows if you need more spaces for your explanation.) Hint: Although I am not asking you to give the no. of bonding and non-bonding pairs, you have to do it to be able to identify the electron pair geometry and molecular geometry. Note: Items #1 to #4 are hypothetical molecules. The number of valence electron/s of the hypothetical atoms are given in parenthesis.) There is no need to give actual molecules to represent them. Polar or Non-polar Explanation 1. nod

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 70P: Ozone (O3) has a nonzero dipole moment. In the molecule of O3 , one of the oxygen atoms is directly...

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the actual molecule of which this is a Lewis stricture, which of the labeled distances can change?
Ozone (O3) has a nonzero dipole moment. In the molecule of O3 , one of the oxygen atoms is directly bonded to the other two, which are not bonded to each other. (a) Based on this information, state which of the following structures are possible for the ozone molecule: symmetric linear, nonsymmetric linear (for example, different OO bond lengths), and bent. (Note: Even an OO bond can have a bond dipole if the two oxygen atoms are bonded to different atoms or if only one of the oxygen atoms is bonded to a third atom.) (b) Use the VSEPR theory to predict which of the structures of part (a) is observed.
Briefly discribe ?
I already answered the first part which was satisfying the balances filling in the double and triple bonds as well as the unshared electron pairs, as you can see in the second picture I have written those answers and pin. I’m having trouble with converting the Lewis structure into bondline structures if you could please help me out I would appreciate it.
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Im not sure about the electron geometry and molecular for this real molecules. the link is what we have to use Virtual modeling simulation: http://phet.colorado.edu/en/simulation/molecule-shapes
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