chemistry worksheet.docx - Molecular Shapes VSEPR Theory ...

Molecular Shapes, VSEPR Theory, and Hybridization of Atomic Orbitals
Introduction and Procedure
In this lab you will draw the Lewis structure for a variety of covalent/molecular compounds. You will
determine the number of total electron groups (pairs), bonding groups (pairs) and lone groups (pairs)
around each interior atom using the VSEPR Theory . Then you will use Table 10.1 of your textbook to
determine the bond angle, and molecular and electronic shape of each interior atom. This will also allow
you to determine the hybridization of each interior/center atom as proposed by the Valence Bond
Theory . These topics are covered in more detail in Sections 10.2, 10.4 and 10.7 in your textbook.
When analyzing a central atom to determine molecular geometry using VSEPR Theory, remember to
count double and triple bonds as a single bonding electron group . Also remember that uncharged
carbon atoms have no lone pairs, uncharged nitrogen atoms have one lone pair and uncharged oxygen
atoms have two lone pairs.
Once you have completed the paper analysis of each molecule, you should draw its structural formula
including lone pairs and build its molecular model.
The key to the molecular model kits:
Black Carbon
White Hydrogen
Red Oxygen
Blue Nitrogen – note there are two forms of nitrogen, with 3 or 4 holes
Green Halogens (also purple and orange if present)
Yellow Sulfur
Tan Trigonal bipyramidal (sp 3 d)
Silver Octahedral (sp 3 d 2 )
Short grey sticks for single (sigma) bonds
Long grey sticks for multiple (sima plus one or more pi bonds)
NOTE: Table 11.1 for VSEPR Analysis
A laminated photocopy of Table 10.1 from your textbook should be available for lab use.
Do not remove this from the lab. See your textbook for in lecture and at home use.

Results
1. Water
Lewis structure using dots to represent bonding electrons:
Lewis structure using lines to represent pairs of bonding electrons: