nich or || III O IV ○ I and IV ollowing compound(s) have trigonal planar molecular geometry: :F-B-Ë: ..+ H-O-H H-C-H F-N-F H H III

Do not give handwriting solution.

Part B Consider the completed Lewis Structure for caffeine: :O: CH3 HgC CーH // :O: What best describes the geometry for each of the interior carbon atoms (within the ring network)? trigonal planar tetrahedral O tshaped trigonal pyramidal O bent :2-

State the orbital hybridization of each highlighted atom

Why is it less clear to see the electrons on HBrO2 molecular electron geometry than it is on something like H2O? I know there should be 20 electrons on HBrO2, but this leads me to an incorrect drawing. And with the correct drawing, I don't see where all the electrons are. It seems like there's only 10 total. What am I missing here?

Indicate the electron pair geometry and the molecular geometry for each of the six compounds. Compound Electron pair geometry Molecular geometry :ö=s=0: trigonal planar bent :CI-S :ö=c=ö: linear linear 一一 :F-B- -F: :F: :Ci: tetrahedral tetrahedral

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4. What is the difference between a bond dipole and a molecular dipole moment? Explain using H2, HF and CO2. lity Unavailable O HI BUEN Focus I BE

1. How many valence electrons in each of the following: C Br N Cl- DRAWING LEWIS STRUCTURES 2. Complete the Lewis structure for CH,0H: 1. Identify how many total valence électrons are in your How many H. molecule valence e- 2. Arrange the atoms in the expected bonding order A H C O H does each atom bring in? 3. Arrange the electrons to that two electrons are in each bond 3. Draw the Lewis structures for the following: and, as much as possible, all valence shells are filled. Use CH,NH2 F2 lone pairs as needed and FOLLOW the OCTET RULE!!!!

Draw the Lewis structure of AsO³- showing all lone pairs. Select Draw Rings More ||||||||| As G Erase Q2 Q 3- Identify the molecular geometry of AsO³. 4 see-saw O T-shaped tetrahedral octahedral linear square pyramidal trigonal planar trigonal pyramidal bent square planar O trigonal bipyramidal