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Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 90

Amino acids are the building blocks of proteins. The simplest amino acid is glycine (H2NCH2COOH). Draw a Lewis structure for glycine. (Hint: The central atoms in the skeletal structure are nitrogen and the two carbon atoms. Each oxygen atom is bonded directly to the right-most carbon atom.)

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Amino Acids

Amino acids are organic compounds that serve as the building blocks of proteins. Each amino acid contains a central carbon atom, an amino group (–NH2), a carboxyl group (–COOH), a hydrogen atom, and a variable side chain (R group) that determines the specific properties of the amino acid. Glycine, the simplest amino acid, has a hydrogen atom as its side chain.
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Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They are useful for visualizing the arrangement of atoms and the distribution of electrons. In the case of glycine, the Lewis structure will show the connectivity between the nitrogen, carbon, and oxygen atoms, as well as the placement of hydrogen atoms.
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Skeletal Structure

The skeletal structure of a molecule is a simplified representation that focuses on the arrangement of atoms and the bonds between them, often omitting hydrogen atoms for clarity. In glycine, the skeletal structure emphasizes the central nitrogen and carbon atoms, illustrating how they are connected to each other and to the functional groups, which is essential for drawing an accurate Lewis structure.
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Related Practice
Textbook Question

Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. a. BaCO3

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Open Question
Does each compound contain both ionic and covalent bonds? Write ionic Lewis structures for each of them, including the covalent structure for the ion in brackets. Write resonance structures if necessary for the following: b. NH4Cl, d. Sr(CN)2, a. RbIO2, c. KOH.
Textbook Question

Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each carbon ring structure, including any necessary resonance structures. a. C4H8 b. C4H4 c. C6H12 d. C6H6

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Textbook Question

Formic acid is responsible for the sting of ant bites. By mass, formic acid is 26.10% C, 4.38% H, and 69.52% O. The molar mass of formic acid is 46.02 g/mol. Determine the molecular formula of formic acid and draw its Lewis structure.

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Textbook Question

Diazomethane is a highly poisonous, explosive compound because it readily evolves N2. Diazomethane has the following composition by mass: 28.57% C; 4.80% H; and 66.64% N. The molar mass of diazomethane is 42.04 g/mol. Find the molecular formula of diazomethane, draw its Lewis structure, and assign formal charges to each atom. Why is diazomethane not very stable? Explain.

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Textbook Question

The reaction of Fe2O3(s) with Al(s) to form Al2O3(s) and Fe(s) is called the thermite reaction and is highly exothermic. What role does lattice energy play in the exothermicity of the reaction?

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