How would you draw the lewis resonance structure for CH2Br?

Question

Isaac Aronson · Accepted Answer

There are no resonance structures. There is only one valid Lewis structure for the bromomethyl radical.

The Bromomethyl radical has only one possible Lewis structure. This molecule as written in the question has an odd number of electrons

Lucy Alessi · Answer

undefined To draw the Lewis resonance structure for CH2Br, you would represent the carbon atom with two hydrogen atoms attached and a single bond to the bromine atom. The lone pair of electrons on bromine can form a double bond with the carbon atom, leading to resonance. Thus, you would draw another structure where the carbon-bromine bond is a double bond, and the carbon atom has a formal positive charge, while the bromine atom carries a formal negative charge.

Madison Anderson · Answer

undefined To draw the Lewis resonance structure for CH2Br, follow these steps:

1. Determine the total number of valence electrons for the molecule. Carbon contributes 4 electrons, each hydrogen contributes 1 electron, and bromine contributes 7 electrons, totaling 12 electrons.
2. Place the least electronegative atom (carbon) in the center, and surround it with hydrogen and bromine atoms.
3. Connect each atom with a single bond, representing two electrons.
4. Distribute the remaining electrons around the atoms to fulfill the octet rule, starting with the outer atoms first.
5. If necessary, move lone pairs to form multiple bonds to achieve a more stable arrangement and satisfy the octet rule for all atoms.
6. Draw resonance structures by moving electron pairs to form double or triple bonds between different atoms while maintaining the same overall number of valence electrons.

The resonance structure for CH2Br involves moving electron pairs between carbon and bromine to form a double bond and satisfy the octet rule for carbon. This results in a resonance hybrid that represents the actual distribution of electrons in the molecule.

HIX Tutor · Answer

undefined To draw the Lewis structure for CH₂Br (bromomethane), follow these steps:

1. **Count Valence Electrons**:
   - Carbon (C) has 4 electrons.
   - Each Hydrogen (H) has 1 electron. There are 2 H, so that’s 2 electrons.
   - Bromine (Br) has 7 electrons.
   - Total: 4 (C) + 2 (2 H) + 7 (Br) = 13 valence electrons.

2. **Draw the Skeletal Structure**:
   - Place C in the center.
   - Attach 2 H to C and 1 Br to C.
   - It looks like this: H - C - H
                                      |
                                     Br

3. **Distribute Electrons**:
   - Each single bond (C-H and C-Br) takes 2 electrons.
   - Connect C to 2 H and 1 Br: that uses 6 electrons (3 bonds).
   - We have 7 electrons left (13 - 6 = 7).

4. **Place Remaining Electrons**:
   - Place 3 lone pairs (6 electrons) on Br.
   - The remaining 1 electron goes to the lone pair on the carbon.

5. **Check for Octet**:
   - C has 4 electrons in bonds (fulfills part of the octet).
   - Br has 8 electrons (3 lone pairs + 1 bond).
   - H has 2 electrons each (fulfills their requirement).

6. **Final Structure**:
   - H - C - H
                 |
                Br
   - That’s CH₂Br!

And that's it! You have the Lewis structure for CH₂Br!