Wayne Breslyn | H2SO3 Lewis Structure: How to Draw the Lewis Structure for Sulfurous acid @wbreslyn | Uploaded 11 years ago | Updated 3 hours ago
A step-by-step explanation of how to draw the H2SO3 Lewis Structure (Sulfurous acid).
When we have an H (or H2) in front of a polyatomic molecule (like CO3, SO4, NO2, etc.) we know that it's an acid. This means that the Hydrogen atoms will be attached to the outside of the oxygen molecules. Knowing this information makes it much easier to draw the Lewis structure for H2SO3.
A step-by-step explanation of how to draw the H2SO3 Lewis Dot Structure (Sulfurous acid).
For the H2SO3 structure use the periodic table to find the total number of valence electrons for the H2SO3 molecule. Once we know how many valence electrons there are in H2SO3 we can distribute them around the central atom with the goal of filling the outer shells of each atom.
In the Lewis structure of H2SO3 structure there are a total of 26 valence electrons. H2SO3 is also called Sulfurous acid.
Note that H2SO3 can have an Expanded Octet and have more than eight valence electrons. Because of this there may be several possible Lewis Structures. To arrive at the most favorable Lewis Structure we need to consider formal charges. See how to calculate formal charges: https://www.youtube.com/watch?v=vOFAPlq4y_k
----- Steps to Write Lewis Structure for compounds like H2SO3 ------
1. Find the total valence electrons for the H2SO3 molecule.
2. Put the least electronegative atom in the center. Note: Hydrogen (H) always goes outside.
3. Put two electrons between atoms to form a chemical bond.
4. Complete octets on outside atoms.
5. If central atom does not have an octet, move electrons from outer atoms to form double or triple bonds.
----- Lewis Resources -----
Lewis Structures Made Simple: https://youtu.be/1ZlnzyHahvo
More practice: https://youtu.be/DQclmBeIKTc
Counting Valence Electrons: https://youtu.be/VBp7mKdcrDk
Calculating Formal Charge: https://youtu.be/vOFAPlq4y_k
Exceptions to the Octet Rule: https://youtu.be/Dkj-SMBLQzM
Lewis Structures, also called Electron Dot Structures, are important to learn because they help us understand how atoms and electrons are arranged in a molecule, such as Sulfurous acid. This can help us determine the molecular geometry, how the molecule might react with other molecules, and some of the physical properties of the molecule (like boiling point and surface tension).
Chemistry help at https://www.Breslyn.org
A step-by-step explanation of how to draw the H2SO3 Lewis Structure (Sulfurous acid).
When we have an H (or H2) in front of a polyatomic molecule (like CO3, SO4, NO2, etc.) we know that it's an acid. This means that the Hydrogen atoms will be attached to the outside of the oxygen molecules. Knowing this information makes it much easier to draw the Lewis structure for H2SO3.
A step-by-step explanation of how to draw the H2SO3 Lewis Dot Structure (Sulfurous acid).
For the H2SO3 structure use the periodic table to find the total number of valence electrons for the H2SO3 molecule. Once we know how many valence electrons there are in H2SO3 we can distribute them around the central atom with the goal of filling the outer shells of each atom.
In the Lewis structure of H2SO3 structure there are a total of 26 valence electrons. H2SO3 is also called Sulfurous acid.
Note that H2SO3 can have an Expanded Octet and have more than eight valence electrons. Because of this there may be several possible Lewis Structures. To arrive at the most favorable Lewis Structure we need to consider formal charges. See how to calculate formal charges: https://www.youtube.com/watch?v=vOFAPlq4y_k
----- Steps to Write Lewis Structure for compounds like H2SO3 ------
1. Find the total valence electrons for the H2SO3 molecule.
2. Put the least electronegative atom in the center. Note: Hydrogen (H) always goes outside.
3. Put two electrons between atoms to form a chemical bond.
4. Complete octets on outside atoms.
5. If central atom does not have an octet, move electrons from outer atoms to form double or triple bonds.
----- Lewis Resources -----
Lewis Structures Made Simple: https://youtu.be/1ZlnzyHahvo
More practice: https://youtu.be/DQclmBeIKTc
Counting Valence Electrons: https://youtu.be/VBp7mKdcrDk
Calculating Formal Charge: https://youtu.be/vOFAPlq4y_k
Exceptions to the Octet Rule: https://youtu.be/Dkj-SMBLQzM
Lewis Structures, also called Electron Dot Structures, are important to learn because they help us understand how atoms and electrons are arranged in a molecule, such as Sulfurous acid. This can help us determine the molecular geometry, how the molecule might react with other molecules, and some of the physical properties of the molecule (like boiling point and surface tension).
Chemistry help at https://www.Breslyn.org
