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: Consider the Lewis structure for glycine, the simplest amino acid:What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom?

Solution: Consider the Lewis structure for glycine, the simplest amino acid:What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom?

Problem

Consider the Lewis structure for glycine, the simplest amino acid:

An N with one pair of dots is single bonded left and below to H and right to C.  That C is single bonded above and below to H and right to C.  That C is double bonded above to O (which has two pairs of dots) and right to O (which also has two pairs of dots). That O is single bonded right to H.

What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom?

Solution

We are being asked to identify the hybrid orbitals used by nitrogen (N) and oxygen (O) or the hybridization in NH2CH2COOH. 


We answer this problem, using the given Lewis structure of the compound


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