Problem: For those given below, which has the smallest bond angle?A. H2O B. NH3 C. CH4 D. XeF4 E. NH4+

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: