Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

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

Problem

For those given below, which has the smallest bond angle?

A. H2

B. NH3 

C. CH4 

D. XeF4 

E. NH4+

Solution

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:

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