What is the Lewis Dot Structure, hybridization, and molecular geometry of HBr?
The correct answer and explanation is:
Correct Answer:
- Lewis Dot Structure:
H:Br with six lone electrons around Br.
The hydrogen (H) atom forms a single bond with the bromine (Br) atom.
Br has three lone pairs (6 electrons) and shares one pair with H. - Hybridization:
sp³ for bromine - Molecular Geometry:
Linear
Explanation:
Hydrogen bromide (HBr) is a diatomic molecule made of one hydrogen atom and one bromine atom. To draw the Lewis dot structure, begin with the total number of valence electrons. Hydrogen has one valence electron, and bromine (a Group 17 element) has seven valence electrons. That makes a total of 8 valence electrons.
In the structure, hydrogen and bromine share one pair of electrons to form a single covalent bond. Hydrogen only needs two electrons in its valence shell to be stable, so it is satisfied by this single bond. Bromine, on the other hand, needs eight electrons to complete its octet. It gains two from the bond with hydrogen and has three lone pairs (six electrons) to complete the octet.
The hybridization of bromine in this molecule is sp³. This results from one s orbital and three p orbitals combining to create four hybrid orbitals. One hybrid orbital is used for bonding with hydrogen, and the remaining three contain lone pairs.
The molecular geometry of HBr is linear. This is because the molecule only contains two atoms. The concept of geometry in terms of bond angles does not involve a central atom with multiple bonds, so the molecule takes a straight-line shape. The bond angle is 180 degrees.
Since it is a polar molecule due to the difference in electronegativity between hydrogen and bromine, HBr has a dipole moment directed toward bromine. This contributes to its ability to dissolve in polar solvents like water.