Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee all chapters
All Chapters
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: Select the correct hybridization for the central atom based on the electron geometry BrF3.

Solution: Select the correct hybridization for the central atom based on the electron geometry BrF3.

Problem

Select the correct hybridization for the central atom based on the electron geometry BrF3.

Solution

When the s and p orbitals combine to form a covalent bond, hybridization occurs. The product of hybridization is a hybrid orbital.


We can determine the hybridization of the central atom of BrF3 through its electron geometry.

First, draw the Lewis structure.


In drawing Lewis structures, there are general guidelines to be followed:


1. The number of valence electrons equals the group number. 

The total number of valence electrons is:


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