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: Butadiene, C4H6, is a planar molecule that has the following carbon-carbon bond lengths:From left to right, what is the hybridization of each carbon atom in butadiene?

Solution: Butadiene, C4H6, is a planar molecule that has the following carbon-carbon bond lengths:From left to right, what is the hybridization of each carbon atom in butadiene?

Problem

Butadiene, C4H6, is a planar molecule that has the following carbon-carbon bond lengths:

The figure shows a molecule with the following structure: H2CCHCHCH2, with a double bond between the first and the second and also between the third and the fourth carbon atoms. The bond between the second and the third carbon atoms is single and has the length of 1.48 angstroms. Each double bond has the length of 1.34 angstroms.

From left to right, what is the hybridization of each carbon atom in butadiene?

Solution

We are being asked to determine the hybridization of each carbon atom in butadiene.


The figure shows a molecule with the following structure: H2CCHCHCH2, with a double bond between the first and the second and also between the third and the fourth carbon atoms. The bond between the second and the third carbon atoms is single and has the length of 1.48 angstroms. Each double bond has the length of 1.34 angstroms.


Recall: 

Hybridization is a mathematical procedure in which the standard atomic orbitals are combined to form new atomic orbitals called hybrid orbitals that correspond more closely to the actual distribution of electrons in chemically bonded atoms.

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