What is the correct Lewis structure
for hypobromous acid, HBrO?
Hint: Consider how many bonds each
atom likes to form.
H-Br-Ö:
H-0-Br::H-0-Br:
The Correct Answer and Explanation is :
To draw the correct Lewis structure for hypobromous acid (HBrO), we first need to consider the number of valence electrons and how many bonds each atom typically forms:
- Valence Electrons:
- Hydrogen (H) has 1 valence electron.
- Bromine (Br) has 7 valence electrons.
- Oxygen (O) has 6 valence electrons. Therefore, the total number of valence electrons in HBrO is:
[
1 \, (\text{H}) + 7 \, (\text{Br}) + 6 \, (\text{O}) = 14 \, \text{valence electrons}
]
- Atoms’ Bonding Preferences:
- Hydrogen forms 1 bond.
- Oxygen typically forms 2 bonds.
- Bromine can form 1 bond but can also expand its octet due to having available d orbitals.
- Constructing the Lewis Structure:
- Start by placing the central atom, which in this case is oxygen (O), between hydrogen (H) and bromine (Br).
- Connect hydrogen and bromine to oxygen with single bonds. This uses 4 of the 14 valence electrons (2 for each bond).
- Place the remaining 10 electrons to satisfy the octet rule for bromine and oxygen.
- Oxygen needs 2 more electrons to complete its octet, which can be achieved by placing 2 lone pairs on oxygen. This accounts for 4 more electrons, leaving 6.
- Bromine can use the remaining 6 electrons as 3 lone pairs to complete its octet.
- Final Lewis Structure:
The Lewis structure can be represented as:
..
H - O - Br
..In this structure:
- The oxygen atom forms a single bond with hydrogen and bromine.
- Oxygen has 2 lone pairs (4 electrons) and is connected to H and Br, fulfilling the octet rule.
- Bromine has 3 lone pairs (6 electrons) and is connected to oxygen with a single bond, also fulfilling its octet requirement.
In conclusion, the correct Lewis structure for hypobromous acid (HBrO) demonstrates that hydrogen and bromine are bonded to oxygen, with oxygen having two lone pairs of electrons. This arrangement satisfies the valence electron count and bonding preferences of the atoms involved.