Name: Period: Date: What Is VSEPR? Now explore the Compare Two Structures link. Try changing the display to explore different combinations.
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1 Name: Period: Date: What Is VSEPR? Exploring The Valence Shell Electron Pair Repulsion (VSEPR) model. Go to the Purdue University website to explore VSEPR theory. Start by clicking on What is VSEPR? Explain in your own words what VSEPR theory is used for? Now explore the Compare Two s link. Try changing the display to explore different combinations. Describe in words what a linear molecule looks like. Describe what a trigonal planar molecule looks like. Describe what a tetrahedral molecule looks like. So why do molecules form in these ways? Based on what you observed, what do you think determines the shape of the molecule? Let s explore further to determine if you are correct. Click on the VSEPR Rules link to learn how molecules get their shape.
2 Rules for VSEPR 1. Draw the Lewis structure for the molecule or ion. 2. Count the total number of regions of high electron density (bonding pairs and unshared electron pairs) around the central atom. Click on the Examples link for more practice. Now try it on your own: Count the regions of high electron density in the molecules given in the Test My Knowledge link, record three of these below. Compound Draw the Lewis Dot # of areas of high e - density
3 3. Identify the most stable arrangement of the regions of high electron density as ONE of the following: a. linear b. trigonal planar c. tetrahedral Note: There are more complicated geometric structures for central atoms with expanded octets. We have not learned these yet, but you are welcome to explore these further on the website. Click on Arranging Regions of High Electron Density to help you fill in the chart below. 4. Now, determine the positions of the atoms based on the types of electron pairs present (i.e., bonding pairs vs. unshared pairs). Fill in the chart below to help you learn the different geometric configurations. 5. Identify the molecular structure based on the positions of the ATOMS (NOT the electron pairs) Click on s Based on VSEPR Theory to help you fill in the chart below. Compound Draw the Lewis Dot # of areas of high e - density Types of regions 2 bonded structure Draw VSEPR Model BeCl 2 0 lone BF 3 trigonal planar NO 2-3 NH bonded 0 lone NH 3 NH 2 - bent
4 Name: Period: Date: DIRECTIONS : Now that you have explored the VSEPR theory, we are going to try some practice. For each practice problem follow the rules for VSEPR theory to determine the molecular shape. RULES FOR VSEPR THEORY 1. Draw the Lewis structure for the molecule or ion. 2. Count the total number of regions of high electron density (bonding and unshared electron pairs) around the central atom. 3. Identify the most stable arrangement of the regions of high electron density. 4. Determine the positions of the atoms based on the types of electron pairs (i.e., bonding pairs vs. unshared pairs). 5. Identify the molecular structure based on the positions of the ATOMS (NOT the electron pairs). Example Problem #1: BeCl2 2 Linear Cl Be Cl Linear Lewis # e - Density Regions Best Arrangement Atom Position Problem #2: SO3 Lewis # e - Density Regions Best Arrangement Atom Position Problem #3: CH4 Lewis # e - Density Regions Best Arrangement Atom Position
5 Problem #4: H2O Lewis # e - Density Regions Best Arrangement Atom Position Problem #5: H3O + Lewis # e - Density Regions Best Arrangement Atom Position Now that you have tried these on your own. Go back to the Purdue University website and check how you did on each practice problem. These are practice problems # 2, 3, 6 and 11 on the site. Now that you have the hang of it, try these. Problem #6: NO3 Lewis # e - Density Regions Best Arrangement Atom Position Problem #7: SiF3 Lewis # e - Density Regions Best Arrangement Atom Position
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