A+ Solution UOP CHM/150 Lewis Structure Model Lab

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Lewis Structure Model

Kathy Carrigan

Version Lewis Structure Model

 

LAB REPORT ASSISTANT                                                                                 

 

This document is not meant to be a subsƟtute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s quesƟons, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ wriƟng of lab reports by providing this informaƟon 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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