What is the formal charge on each atom indicated in the following structure. CH3 H3C O ○ O b INN a = +1,b=+1,c=0 a=-1,b=1,c=0 a = 0,b=1,c= +1 a O a = +1,b=0,c=-1 C

How come there are two major resonance structure? Wouldn't the structure with the positive charge on the nitrogen be the only major structure, as it is less electronegative than oxygen?

Examples: Example: H▬N▬H HIN: Examples: :F Н lone pair : -bond pair (2 e-) single bond :F: Non-Polar 8+. H :F: H:Cl: HCl:o is better represented as closer to Cl due to its greater electronegativity. Thus, HCl contains a polar covalent bond. H :0: Polar lone pair 8- :S H -S= :0: 2 bond pairs (4 e-) double bond because the bond electrons are pulled F: Pola

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?

5. Three possible resonance structures for dinitrogen monoxide (N20) are drawn below. :N=N=ö: EN: :NEN- -0: :N-NE0: a. How many total valence electrons are available in N20? b. What is the formal charge on the oxygen atom in the structure farthest to the left? Resonance structures that are considered unimportant when describing the average bonding are those that either have individual atoms bearing a formal charge greater than or equal to two for any individual atom and/or a high total absolute value formal charge for the entire molecule, calculated by adding the absolute values of each of the atoms. Which of these three structures not as important as the other two in determining the accurate structure of N20? Support your conclusion using formal charges. С.

Choose the best Lewis structure for OCN. (It will help to work out the missing formal charges for the atoms in these different structures) [Image description: Lewis structure A has a C atom singly bound to a O atom and a N atom. There are three electron pairs on O and three electron pairs on N. Lewis structure B has a C atom singly bound to a O atom and triply bound to a N atom. There are three electron pairs on O and one electron pair on N. Lewis structure C has a C atom triply bound to a O atom and singly bound to a N atom. There is one electron pair on O and three electron pairs on N. Lewis structure D has a C atom doubly bound to a O atom and a N atom. There are two electron pairs on O and two electron pairs on N.] :0-c-N: :0-c=N: :0=C-N: o=c=N: A B Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b В C C d D

I only need help understanding B. so dont worry about doing the other parts. Thanks!

The structures below are two possible resonance forms for sulfate. 72- 72- :0: :0: :0-S-0: |3| :0: : (a) (b) S. O (single bond) O (double bond), Calculate the formal charge for the atoms in each and write them in the spaces above. Based on formal charge, which is the better (more contributing) structure? Circle the one that has the most preferred formal charges.

3. One curved arrow shows the movement of an electron pair. o a bond (sigma or pi) involves two electrons, so each curved arrow indicates some change in bonding. Step 6: When a curved arrow starts from a o bond and points to a distant atom, the o bond breaks and a new o bond is formed. A -B A-C B* B-C A* or Note that two possible cations can be formed, depending on whether the electrons from the o bond move with atom A or B. Draw curved arrows to form the products shown. Select Draw Rings More Erase Al H. -0: + AIH, H - Al -H étv 0 hulu MacBook Pro GSearch or type URL & 5 7 T Y * 00

Draw the Lewis structure for formaldehyde, CH2O. Include all hydrogens and lone pairs explicitly.