# Electron Pairs
# Lone Pairs
Electronic Geometry
Molecular Geometry
Lewis Structure
Sketch of Shape
I need to do the above things for SBr6 and BrCl5. If anybody can help that would be great!
http://teachers.yourhomework.com/lipetz/bondingandpolarity.pdf
BrCl5 on page 3 of the following (I think it's BrF5 but you can substitute.)
http://course1.winona.edu/mengen/Chemistry%20212/212%20Laptop%20Labs/Experiment%208%20Molecular%20Shapes%20and%20Structure%202009.pdf
Sure! I can break it down for you. Let's first start by understanding the basic concepts involved in determining the electron pairs, lone pairs, electronic geometry, molecular geometry, Lewis structure, and sketch of shape.
1. Electron Pairs: In chemistry, electron pairs refer to the electron groups that surround the central atom in a molecule or ion. They can be either bonding pairs (shared between atoms) or lone pairs (non-bonding pairs of electrons).
2. Lone Pairs: Lone pairs are electron pairs that are not involved in bonding and are located on the central atom. They can affect the shape of a molecule and its reactivity.
3. Electronic Geometry: Electronic geometry describes the spatial arrangement of electron pairs around the central atom, including both bonding and lone pairs. It is determined by the number of electron pairs and their arrangement according to the valence shell electron pair repulsion theory (VSEPR theory).
4. Molecular Geometry: Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, considering only the bonded atoms. It is influenced by both electron pairs and lone pairs on the central atom.
5. Lewis Structure: A Lewis structure represents the bonding between atoms in a molecule using electron dot diagrams. It shows the arrangement of both bonding and lone pairs of electrons around the central atom.
6. Sketch of Shape: The sketch of shape provides a visual representation of the molecule's geometry, focusing on the arrangement of bonded atoms while ignoring the lone pairs.
Now, let's apply these concepts to the molecules SBr6 and BrCl5.
1. SBr6:
To determine the electron pairs and lone pairs, we first need to know the Lewis structure:
- Start by assigning all the valence electrons of each atom.
- Determine the central atom (in this case, sulfur) based on its lower electronegativity compared to bromine.
- Connect the surrounding atoms (bromine) to the central atom using single bonds.
- Distribute the remaining electrons as lone pairs on the central atom and surrounding atoms until they have a full octet (except for hydrogen).
The Lewis structure of SBr6 will have six single bonds between the sulfur atom (central atom) and bromine atoms surrounding it. There will be no lone pairs of electrons on sulfur since it is in group 6 of the periodic table and has six valence electrons.
2. BrCl5:
Again, we need to determine the Lewis structure first:
- Assign the valence electrons of each atom.
- Identify the central atom based on electronegativity (In this case, bromine).
- Connect the surrounding atoms (chlorine) to the central atom using single bonds.
- Distribute the remaining electrons as lone pairs on the central atom and surrounding atoms until they have a full octet (except for hydrogen).
The Lewis structure of BrCl5 will have five single bonds between the bromine atom (central atom) and chlorine atoms surrounding it. There will be no lone pairs of electrons on bromine since it is in group 7 of the periodic table and has seven valence electrons.
Now, let's determine the electronic and molecular geometries, as well as sketch the shapes:
1. SBr6:
- Electronic Geometry: Since there are no lone pairs on the central sulfur atom and six bonding pairs, the electronic geometry will be octahedral.
- Molecular Geometry: The molecular geometry will also be octahedral since there are no lone pairs on the central atom.
- Sketch of Shape: The sketch of shape for SBr6 will show a central sulfur atom bonded to six surrounding bromine atoms, arranged in an octahedral shape.
2. BrCl5:
- Electronic Geometry: In the case of BrCl5, since there are no lone pairs on the central bromine atom and five bonding pairs, the electronic geometry will be trigonal bipyramidal.
- Molecular Geometry: The molecular geometry will also be trigonal bipyramidal since there are no lone pairs on the central atom.
- Sketch of Shape: The sketch of shape for BrCl5 will show a central bromine atom bonded to five surrounding chlorine atoms, arranged in a trigonal bipyramidal shape.
I hope this helps you understand the concepts and how to determine electron pairs, lone pairs, electronic and molecular geometry, Lewis structure, and sketch of shape for SBr6 and BrCl5.