A stepbystep explanation of how to draw the H2SO4 Lewis Dot Structure (Sulfuric acid).

For the H2SO4 structure use the periodic table to find the total number of valence electrons for the H2SO4 molecule. Once we know how many valence electrons there are in H2SO4 we can distribute them around the central atom with the goal of filling the outer shells of each atom.

In the Lewis structure of H2SO4 structure there are a total of 32 valence electrons. H2SO4 is also called Sulfuric acid.

Note that H2SO4 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:    • Formal Charges: Calculating Formal Ch...  

Steps to Write Lewis Structure for compounds like H2SO4
1. Find the total valence electrons for the H2SO4 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:    • How to Draw Lewis Structures: Five Ea...  
• More practice:    • Lewis Dot Structure Practice Problems...  
• Counting Valence Electrons:    • Finding the Number of Valence Electro...  
• Calculating Formal Charge:    • Formal Charges: Calculating Formal Ch...  
• Exceptions to the Octet Rule:    • Exceptions to the Octet Rule  

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 Sulfuric 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

Chapters
0:00 Counting Valence Electrons
0:33 Place Least Electronegative Element in Center
0:42 Forming chemical bond & Complete Octets
1:40 Formal Changes