Sorry for re-posting this question but I feel as if it hasn't been read or something. Otherwise does no one really know the answer? I am really going crazy over it and I have only 1 try left. Please
What is the lowest energy alternative resonance structure for this compound:
CH3-CH-N<triple bond>N
There is a negative charge on CH and a positive charge on the central N
There aren't any organic chemists on right now; that's why an answer to your question has been scant. Dr Russ often checks in and takes care of those questions. He is in the UK (as he notes, he is "on this side of the pond" so his hours are not quite those of the US volunteers. Have patience. Perhaps he will check in later in the day.
Oh i see, thanks a lot =)
No problem, I'm here to help! To determine the lowest energy resonance structure for the compound CH3-CH-N≡N with a negative charge on CH and a positive charge on the central N, we need to analyze the electron distribution and the stability of different resonance structures.
Resonance structures are different representations of a molecule that can be formed by moving electrons around while keeping the arrangement of atoms unchanged. The goal is to create structures with lower energy and greater stability.
To begin, let's consider the Lewis structure of the compound:
CH3-CH-N≡N
In this molecule, carbon (C) forms three sigma (σ) bonds by sharing electrons with three hydrogen atoms (H) and one carbon (C) atom. The central nitrogen (N) forms one sigma (σ) bond with carbon (C) and a triple bond with another nitrogen (N) atom.
The negative charge on the CH group indicates that this region has an extra electron. The positive charge on the central N atom indicates that it is deficient in one electron.
Now, let's explore the possible resonance structures:
1. The first resonance structure involves moving a lone pair of electrons from one of the carbon atoms to form a double bond with the N atom:
CH2=CH-N≡N:
In this structure, carbon (C) has a double bond with nitrogen (N) and a single bond with the other carbon (C) atom.
2. The second resonance structure involves moving a lone pair of electrons from the CH group to form a double bond with the adjacent carbon (C) atom:
C≡CH-N=N:
In this structure, the carbon (C) atom has a triple bond with the adjacent carbon (C) atom and a double bond with the central nitrogen (N) atom.
Now, to determine the lowest energy resonance structure, we need to evaluate the stability of each structure. Generally, structures with more bonds, especially double and triple bonds, are more stable due to the sharing of electrons.
In this case, the second resonance structure (C≡CH-N=N) has two double bonds, whereas the first resonance structure (CH2=CH-N≡N) only has one double bond.
Therefore, the lowest energy alternative resonance structure for the given compound is:
C≡CH-N=N
I hope this helps! If you have any more questions, feel free to ask.