Draw the Lewis structure for bromoethane (C2H5Br): Be certain you include any lone pairs.
The Correct Answer and Explanation is:
Lewis Structure for Bromoethane (C₂H₅Br)
Here is the correct Lewis structure for bromoethane:
H H H
| | |
H – C – C – Br
|
H
In this structure:
- Each carbon (C) forms 4 bonds.
- Each hydrogen (H) forms 1 bond.
- Bromine (Br) forms 1 bond and has three lone pairs of electrons.
Now, let’s break this down:
Explanation
Bromoethane (C₂H₅Br) is an organic halide that consists of a two-carbon ethane chain with one hydrogen atom replaced by a bromine atom. To draw the Lewis structure, we follow standard rules for bonding and valence electrons.
Step 1: Count total valence electrons.
- Carbon (C) has 4 valence electrons × 2 = 8
- Hydrogen (H) has 1 valence electron × 5 = 5
- Bromine (Br) has 7 valence electrons = 7
Total = 8 + 5 + 7 = 20 valence electrons
Step 2: Arrange atoms.
The two carbon atoms are connected in a straight chain (C–C). One carbon (CH₃ group) is bonded to three hydrogens. The second carbon (CH₂ group) is bonded to two hydrogens and a bromine atom (Br).
Step 3: Draw single bonds.
- Connect each carbon with a single bond.
- Attach hydrogens to fulfill each carbon’s 4 bonds.
- Attach Br to the CH₂ carbon.
At this point, all atoms are connected, and the carbon atoms follow the octet rule (8 electrons around each). Hydrogen atoms only require 2 electrons (1 bond).
Step 4: Add lone pairs.
Bromine forms only one single bond but needs 8 electrons total. It already has 2 from the bond, so we add three lone pairs (6 electrons) to complete its octet.
Final structure:
- Each H has 1 bond.
- Each C has 4 bonds (satisfying the octet).
- Br has 1 bond and 3 lone pairs.
This structure is stable and reflects the correct electron configuration and bonding of all atoms in bromoethane.
