Write Lewis structures for these molecules or ions. (a) CN^- (b) tetrafluoroethylene, C2 F4, th

step 1 In this question, we are asked to write loose structures for these molecules or ions. The first

Write Lewis structures for these molecules or ions. (a) CN^-...

Write Lewis structures for these molecules or ions.
(a) $\mathrm{CN}^{-}$
(b) tetrafluoroethylene, $\mathrm{C}_{2} \mathrm{~F}_{4},$ the molecule from which Teflon is made
(c) acrylonitrile, $\mathrm{CH}_{2} \mathrm{CHCN},$ the molecule from which Orlon is made

Key Concepts

Lewis Structures

A method for depicting the arrangement of valence electrons among the atoms in a molecule or ion. They are drawn using dots for nonbonding electrons and lines for bonds, allowing a visual understanding of bonding patterns, electron pairs, and how atoms achieve stable configurations.

Valence Electrons

These are the outermost electrons of an atom involved in chemical bonding. Understanding the count and arrangement of valence electrons is essential when constructing Lewis structures, as it determines how atoms bond and form molecules or ions.

Octet Rule

This is the principle that atoms tend to form bonds until they are surrounded by eight electrons in their valence shell, similar to the electron configuration of noble gases. The rule guides the distribution of electrons in Lewis structures, although exceptions may occur.

Formal Charge

A calculated charge that helps determine which Lewis structure is most likely to represent a molecule or ion. It is obtained by comparing the number of electrons an atom owns in the structure to its number of valence electrons in the free atom, ensuring overall charge balance.

Multiple Bonds

These occur when atoms share more than one pair of electrons, such as in double or triple bonds. Multiple bonds are used in Lewis structures to satisfy the octet rule for atoms that cannot achieve a full octet through single bonds alone.

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