We can calculate the formal charge by following expression , FC = Valence electron - Nonbonding electron - bonding electron/2. FCO = 6 - 4 - 4/2 = 6 - 6 = 0. FCN = 5 - 4 - 4/2 =5 - 6 = -1 ,therefore option D is correct .
4. Calculate the formal charge on both the nitrogen and the oxygen in the molecule below....
1. A molecule which has C, N, O and H has no formal charge on any of the atoms. which statement best describes the valence (bonds and lone pairs) of carbon, nitrogen, and oxygen? A) Carbon: two bonds, zero lone pairs; nitrogen: three bonds, two lone pairs B) Oxygen: two bonds, two lone pairs; nitrogen: three bonds, one lone pair C) Carbon: three bonds, one lone pair; oxygen: two bonds, two lone pairs D) Carbon: four bonds, zero lone pairs;...
Hi, I'm trying to understand how oxygen and nitrogen, when in a molecule with 4 bonds to them, for example, NH4+ and H3O+ bear a POSITIVE charge when they gain that additional proton? I think I understand that nitrogen's FC would be calculated 5-0-4= +1, but now, I'm having the same problem with nitrogen because wouldn't the formal charge be calculated 6-3-3=0?? Do I have the formula wrong? What is GOING ON!!?
Consider Lewis formulas A & B. Calculate the formal charges on carbon and nitrogen in both species. All lone pairs are shown.
Organic Chemistry question: (4 pts) Please calculate the formal charge on each carbon atom in the species below. For full credit, please show your work. All lone pairs have been drawn in. No overall charges are shown. I- H - C- CH2= C CH O- HH
What is the formal charge on the oxygen to the left in the molecule below?
When the molecule shown below is acting as a base, is the oxygen or nitrogen more likely to receive the hydrogen? Justify your answer with resonance structures. (Note: Lone-pairs are not shown, but should be included in your resonance structures.) ZI
When the molecule shown below is acting as a base, is the oxygen or nitrogen more likely to receive the hydrogen? Justify your answer with resonance structures. (Note: Lone-pairs are not shown, but should be included in your resonance structures.) ZI
4. Shown below is the formal structure of the amino acid threonine (on the left) and its structure as it exists at physiological pH ( 7.3). In each case, the molecule itself is neutral; however al pH 7.3 th is an atom with a formal + charge and an atom with a formal - charge. For both structures add any necessary lone pairs of electrons and where appropriate put formal charges. (8 points)
Hope someone could help me to solve these problems Will rate! 2. Calculate the formal charge of each atom in the following Lewis structure for Po43- O P- O: (show your calculations of formal charges on the space provided below) a) Formal charge of P b) Formal charge of oth1 c) Formal charge of o#2 d) Formal charge of oth3 e) Formal charge of oth4 3. Complete the following diagram to draw one of the Lewis structures for PO43- with...
16. Draw the Lewis Structure for the carbon monoxide molecule. Calculate the carbon-oxygen bond order- this is a simple consideration Calculate the formal charge on each atoni in the molecule. Discuss the stability of CO and the meaning of the formal charges you calculated. 17. Draw the Lewis Structure for methane. Calculate the formal charge on each atom in the molecule. 18 Draw the Lewis Structure for the ammonium ion (NH). Calculate the formal charge on each atom in the...