Determine the Lewis structure of each compound (H2O, NH3, CH4, XeF4 and NH4+) and figure out the bond angles.
For the Lewis structure, follow the steps below:
Step 1: Determine the central atom in this molecule.
Step 2: Calculate the total number of valence electrons present.
Step 3: Draw the Lewis structure for the molecule.
Step 4: Determine the number of electron groups around the indicated atom.
Step 5: Determine the electron geometry and bond angle using this table:
Electron Regions Geometry Bond Angles
2 linear 180˚
3 trigonal planar 120˚
4 tetrahedral 109.5˚
4 trigonal pyramidal <109˚
5 trigonal bipyramidal 90˚, 120˚, and 180˚
6 octahedral 90˚ and 180˚
6 square pyramid 90˚
The possible electron pair and molecular geometries are:
For those given below, which has the smallest bond angle?
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