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
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Part A: PRACTICE EXAMPLES |
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Count Valence e- |
Formula |
Electron Geometry |
Molecular Geometry |
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1 N = 5 3 H = 3 8 / 2 = 4 pair |
NH3 |
Tetrahedral |
Trigonal pyramidal |
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H2O |
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CBr4 |
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SO3 This is not a polyatomic ion … No charge!!! |
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PI3 |
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CH3Cl Carbon is the central atom |
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NO 1- 3 |
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CO 2- 3 |
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NH +1 4 |
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CH4 |
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SO2 |
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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.
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Part B: PRACTICE EXAMPLES |
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Count Valence E |
Formula |
Structure |
Molecular Geometry |
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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 |
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CH3NH2 |
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CH2CH2 Looks like H2C – CH2 Hint ; double bond |
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CH3OCH3 Looks like H3C – O – CH3 |
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