What is the name of the structure and the formal charges? All unshared valence electrons are shown.
:O::
|
H3C-N-CH3
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CH3
The :O:: and CH3 bonds with the N.
I need help ASAP!
trimethylamine N-oxide
http://en.wikipedia.org/wiki/Trimethylamine_N-oxide
The structure you have provided can be recognized as a molecule of methylamine. To determine the formal charges, we need to compare the number of valence electrons each atom has to the number of electrons assigned to it in the Lewis structure.
Starting with the nitrogen (N) atom, we can see that it is bonded to three hydrogen (H) atoms and one carbon (C) atom. Nitrogen has 5 valence electrons, and in the structure, it has 4 unshared electrons around it. Therefore, it has a formal charge of zero (5 - 4 = 1).
Moving on to the carbon (C) atom, it is also bonded to the nitrogen (N) atom and three hydrogen (H) atoms. Carbon has 4 valence electrons, and in the structure, it has 4 unshared electrons around it. So, carbon also has a formal charge of zero (4 - 4 = 0).
Finally, for the hydrogen (H) atoms, they each have 1 valence electron and are not involved in any additional bonds or lone pairs. Hence, they also have a formal charge of zero (1 - 0 = 1).
To summarize, the formal charges in the structure of methylamine are:
- Nitrogen (N) atom: 0
- Carbon (C) atom: 0
- Hydrogen (H) atoms: 0
It's important to note that formal charges are a way of representing the distribution of electrons in a molecule, and they do not necessarily reflect the actual charge of the atom in the molecule.