Draw a Lewis Structure for each species. e. CH3CHO f. CH3S(O)CH3 g. H2SO4 h. CH3NCO

Ch.1 - Structure and Bonding

Wade9th EditionOrganic ChemistryISBN: 9780135213728Not the one you use?Change textbook

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Wade 9th Edition

Ch.1 - Structure and Bonding

Problem 31e-h

Chapter 1, Problem 31e-h

Draw a Lewis Structure for each species.
e. CH₃CHO
f. CH₃S(O)CH₃
g. H₂SO₄
h. CH₃NCO

Verified step by step guidance

To draw the Lewis structure for CH3CHO (acetaldehyde), start by identifying the central atoms. Carbon is typically a central atom. Arrange the atoms as CH3-C-H=O, where the carbonyl group (C=O) is a key feature.

For CH3S(O)CH3 (dimethyl sulfoxide), recognize that sulfur is the central atom bonded to two methyl groups (CH3) and an oxygen atom. The sulfur atom will have a double bond with the oxygen atom, and single bonds with each methyl group.

In the case of H2SO4 (sulfuric acid), sulfur is the central atom. It is bonded to four oxygen atoms, with two of these oxygen atoms forming double bonds with sulfur, and the other two oxygen atoms each bonded to a hydrogen atom, forming hydroxyl groups.

For CH3NCO (methyl isocyanate), start by arranging the atoms with carbon as the central atom. The structure is CH3-N=C=O, where the nitrogen is bonded to the methyl group and the carbon is double-bonded to both nitrogen and oxygen.

Ensure that all atoms in each structure satisfy the octet rule (or duet for hydrogen), and adjust the placement of lone pairs and multiple bonds as necessary to achieve this. Count the total number of valence electrons to verify that the structure is correct.

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Key Concepts

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

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist. They are essential for visualizing the arrangement of atoms, the distribution of electrons, and predicting the shape and reactivity of the molecule. Each line represents a pair of shared electrons, while dots represent lone pairs.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in forming chemical bonds. In drawing Lewis structures, knowing the number of valence electrons helps determine how atoms bond and how many bonds an atom can form. For example, carbon has four valence electrons, allowing it to form four covalent bonds.

Formal Charge

Formal charge is a concept used to determine the most stable Lewis structure for a molecule. It is calculated by subtracting the number of electrons assigned to an atom in the structure from the number of valence electrons in the free atom. Structures with formal charges closest to zero are generally more stable, guiding the correct placement of electrons in the structure.

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