This behavior can also be seen in the simulation

This behavior can also be seen in the simulation. Click the Real Molecules mode, and select as the molecule. Check the box marked Show Bond Angles , and
switch between the Real and Model radio buttons centered at the top of the simulation. What is being demonstrated is the increased repulsion of lone pairs, and that is
why the model predicts 109.5 , and the actual bond angle is 104.5 . These differences in the bond angles can be seen for the following compounds in the simulation:
, , , , , and . There are no changes to predicted bond angles when all the bonds are in the same plane because the lone pairs are
equally repulsing on each side of the plane, which occurs in the case of and .
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.
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ANSWER:
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T-shaped square planar trigonal planar trigonal bipyramidal
tetrahedral seesaw bent linear
trigonal pyramidal square pyramidal octahedral

11/17/21, 7:39 PM VSEPR and MO Diagrams Workshop Activity - Nov 15th/16th
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Effects of electronegativity in molecular bonds
When atoms participate in a covalent bond, the electrons they share are not always evenly distributed within that bond. Electronegativity describes the tendency for an
atom to draw electrons toward its nucleus. When there is a significant enough difference between the electronegativities of two atoms, the bond is considered polar
covalent since the electrons spend more time near the more electronegative nucleus. In a polar covalent bond, the less electronegative atom will have a partial positive
charge ( ), and the more electronegative atom will have a partial negative charge ( ). If there is no significant difference between the electronegativities of the
atoms, then the bond is considered nonpolar covalent (and the nonpolar aspect can be characterized by the symbol). Finally, when the electronegativity difference is
very large, ionic bonds tend to form instead of covalent bonds. The table below summarizes how to classify bonds based on the numeric difference between the Pauling
electronegativity values of atoms.
Pauling
electronegativity
difference
Type of
bond
<0.4
Nonpolar
covalent
0.4 to 1.7
Polar
covalent
>1.7 Ionic
Part C
The structures of , , and are provided below along with the Pauling electronegativity values of , , and . Use the figure and values to complete
the following statements regarding the polarity of bonds in water, carbon dioxide, and methane.