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: The compound 2,6-dimethylpyrazine (below) gives chocolate its odor and is used in flavorings. In what type of hybrid orbital do the lone pairs of N reside?

Solution: The compound 2,6-dimethylpyrazine (below) gives chocolate its odor and is used in flavorings. In what type of hybrid orbital do the lone pairs of N reside?

Problem

The compound 2,6-dimethylpyrazine (below) gives chocolate its odor and is used in flavorings. In what type of hybrid orbital do the lone pairs of N reside?

Solution

Recall: Sigma σ bonds are formed from the end-to-end overlap of s-p hybrid orbitals. On the other hand, pi π bonds are formed from the side-to-side overlap of unhybridized p orbitals.

From the Lewis structure, we can see that each nitrogen atom in 2,6-dimethylpyrazine forms two σ bonds, one π bond, and holds a single lone pair.

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