Draw one Lewis structure for each of the following...

Draw one Lewis structure for each of the following compounds; show all unshared electron pairs. None of the atoms in the compounds bears a formal charge, and all atoms have octets (hydrogens have duets). (a) $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}$ (b) ketene, $\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{O},$ which has a carbon-carbon double bond (c) acetonitrile, $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{~N},$ which has a carbon-nitrogen triple bond

Draw one Lewis structure for each of the following compounds; show all unshared electron pairs. None of the atoms in the compounds bears a formal charge, and all atoms have octets (hydrogens have duets).
(a) $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}$
(b) ketene, $\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{O},$ which has a carbon-carbon double bond
(c) acetonitrile, $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{~N},$ which has a carbon-nitrogen triple bond

Key Concepts

Multiple Bonding (Double and Triple Bonds)

Multiple bonds, which include double and triple bonds, occur when atoms share more than one pair of electrons. These bonds are essential in satisfying the octet rule for atoms that require more electrons beyond what is provided by single bonds, affecting the geometry and reactivity of the molecule.

Formal Charge

Formal charge is a bookkeeping tool used to assign charges within a molecule to ensure the most likely electron distribution. By calculating formal charges for each atom, chemists check that electrons are assigned in a way that minimizes overall charges, ideally resulting in structures where atoms have no net formal charge.

Lewis Structures

Lewis structures are diagrams that represent the arrangement of valence electrons in atoms within a molecule. They visually show how electrons are distributed among atoms and how atoms are bonded together through shared electron pairs, providing a straightforward way to depict molecular structure.

Valence Electrons and Electron Counting

Understanding valence electrons is crucial because these electrons participate in chemical bonding. In creating Lewis structures, the total number of available valence electrons for a molecule is calculated and then distributed among bonding pairs and lone pairs to accurately represent how atoms achieve stable electron configurations.

Octet and Duet Rules

The octet rule holds that most atoms, especially main group elements, tend to have eight electrons in their valence shell, which imparts stability. Hydrogen and helium are exceptions that require only two electrons (duets) to achieve a stable configuration. These rules guide the placement of electrons in Lewis structures.

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