A+ Solution UOP CHM/150 Lewis Structure Model Lab

A+ Solution UOP CHM/150 Lewis Structure Model LabLewis Structure Model
Kathy Carrigan
Version Lewis Structure Model

LAB REPORT ASSISTANT

This document is not meant to be a subsOtute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s quesOons, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ wriOng of lab reports by providing this informaOon in an editable file which can be sent to an instructor.

OBSERVATIONS

Part A: PRACTICE EXAMPLES
Count Valence e-
Formula
Electron Geometry
Molecular Geometry
1 N = 5
3 H = 3
8 / 2 = 4 pair

NH3

Tetrahedral

Trigonal pyramidal

H2O

CBr4

SO3 This is not a
polyatomic ion …
No charge!!!

PI3

CH3Cl Carbon is the central atom

NO 1-
3

CO 2-
3

NH +1
4

CH4

SO2

For the following compounds, there is more than 1 central atom. Count the total number of valence electrons, divide by 2. Draw the Lewis Structures: share the electron pairs around each atom to complete the bonding. Recall that double and triple bonds may be necessary. Determine the structure on each of the central atoms.

Part B: PRACTICE EXAMPLES
Count Valence E
Formula
Structure
Molecular Geometry

1 C = 4
3 H = 3
1 O = 6
1 H = 1
14 e/2 =7 pair

CH3OH

electron
geometry
C – tetrahedral
O – tetrahedral

C = tetrahedral
O = bent
2 bonded
2 non bonded

CH3NH2

CH2CH2
Looks like
H2C – CH2
Hint ; double bond

CH3OCH3
Looks like
H3C – O – CH3

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