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
Sections
Molecular vs Electron Geometry
Bond Angles
Hybridization
Molecular Orbital Theory
Heteronuclear Diatomic Molecules
Additional Practice
Electronegativity
Benzene
Orbital Overlap
Bond Order
Delocalized Electrons
Homonuclear Diatomic Molecules
Additional Guides
Molecular Geometry
VSEPR Theory
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Next SectionMolecular Orbital Theory

Solution: What is the hybridization of the central atom of each of the following molecules? Match the atoms below with their number---sp, sp2, sp3, sp3d, sp3d2COH2H2SPBr5

Solution: What is the hybridization of the central atom of each of the following molecules? Match the atoms below with their number---sp, sp2, sp3, sp3d, sp3d2COH2H2SPBr5

Problem

What is the hybridization of the central atom of each of the following molecules? Match the atoms below with their number---sp, sp2, sp3, sp3d, sp3d2

COH2

H2S

PBr5

Solution

$COH_2$: Carbon, being the central atom, has 3 groups around it, so it is $sp^2$ hybridized because it needs 3 orbitals, 1 s and 2 p.

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