Problem: Part B. Consider the following pairs of molecules that have the same electron geometries. Based on your observations between the Model and Real bond angles in the PhET simulation, complete the sentences to accurately compare the bond angles in each molecule.Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.The types of electron groups not only affect the electron and molecular geometries but have differing effects on bond angles. Lone pairs of electrons repulse other electron groups more strongly than single bonds. For instance, four single bonds in a tetrahedral formation will yield 109.5 bond angles because all bonds equally repulse each other. In the case of three single bonds and one lone pair (e.g., in NH3, the electron geometry is tetrahedral, and the molecular geometry is trigonal pyramidal), the bond angle between the three single bonds will actually be more acutethan the predicted 109.5 (instead, they are 107.8 ) because the repulsion from the lone pair forces the bonds closer together.

FREE Expert Solution
79% (257 ratings)
Problem Details

Part B. Consider the following pairs of molecules that have the same electron geometries. Based on your observations between the Model and Real bond angles in the PhET simulation, complete the sentences to accurately compare the bond angles in each molecule.

Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.

The types of electron groups not only affect the electron and molecular geometries but have differing effects on bond angles. Lone pairs of electrons repulse other electron groups more strongly than single bonds. For instance, four single bonds in a tetrahedral formation will yield 109.5 bond angles because all bonds equally repulse each other. In the case of three single bonds and one lone pair (e.g., in NH3, the electron geometry is tetrahedral, and the molecular geometry is trigonal pyramidal), the bond angle between the three single bonds will actually be more acute

than the predicted 109.5 (instead, they are 107.8 ) because the repulsion from the lone pair forces the bonds closer together.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Molecular vs Electron Geometry concept. You can view video lessons to learn Molecular vs Electron Geometry. Or if you need more Molecular vs Electron Geometry practice, you can also practice Molecular vs Electron Geometry practice problems.