Lect 10. Lewis Structures and Molecular Geometry

# Lect 10. Lewis Structures and Molecular Geometry - Lewis...

This preview shows pages 1–7. Sign up to view the full content.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Lewis Structures Molecular Geometry Molecular Polarity Lewis Structures 1 Draw skeleton structure The most electronegative atoms will be the terminal atoms The least electronegative will be the central atom H is always terminal 2. Calculate the number of electrons in the valence shell of the molecule or ion. The number of valence electrons for each atom is the group number (i.e. N = 5, O = 6, H = 1). Adjust for charge of ions (for +ve charge, remove electrons; for -ve charge, add electrons) 3. Distribute the electrons such that each atom has a share of 8 i) Give to the terminal atoms first (most electronegative) ii) Give 8 to the central atom iii) If the central atom has less than 8, use double (or triple) bonds iv) If there are excess electrons at this point, put them on the central atom v) H atoms never from double bonds Drawing Lewis Structures 1 Draw skeleton structure The most electronegative atoms will be the terminal atoms The least electronegative will be the central atom H is always terminal Lewis Structures 1. Calculate the number of electrons in the valence shell of the molecule or ion . The number of valence electrons for each atom is the group number (i.e. N = 5, O = 6, H = 1). Adjust for charge of ions (for positive charge, remove electrons; For negative charge, add electrons) Lewis Structures 3. Distribute the electrons such that each atom has a share of 8 i) Give to the terminal atoms first (most electronegative) ii) Give 8 to the central atom iii) If the central atom has less than 8, use double (or triple) bonds so it gets a share of 8 iv) If there are excess electrons at this point, put them on the central atom v) H or F never from double bonds Lewis electron-dot formulas or Lewis structures....
View Full Document

## This note was uploaded on 04/29/2009 for the course CHEM 211 taught by Professor Papanastasiou during the Spring '07 term at George Mason.

### Page1 / 33

Lect 10. Lewis Structures and Molecular Geometry - Lewis...

This preview shows document pages 1 - 7. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online