Each of the following molecules contains at least one...

Each of the following molecules contains at least one multiple (double or triple) covalent bond. Give a plausible Lewis structure for (a) $\mathrm{OCS} ;$ (b) $\mathrm{CH}_{3} \mathrm{CHO}$ (c) $\mathrm{F}_{2} \mathrm{CO} ;$ (d) $\mathrm{Cl}_{2} \mathrm{SO} ;$ (e) $\mathrm{C}_{2} \mathrm{H}_{2}$.

Each of the following molecules contains at least one multiple (double or triple) covalent bond. Give a plausible Lewis structure for (a) $\mathrm{OCS} ;$ (b) $\mathrm{CH}_{3} \mathrm{CHO}$
(c) $\mathrm{F}_{2} \mathrm{CO} ;$ (d) $\mathrm{Cl}_{2} \mathrm{SO} ;$ (e) $\mathrm{C}_{2} \mathrm{H}_{2}$.

Key Concepts

Expanded Octet

The concept of an expanded octet applies to elements in period 3 or below, which can have more than eight electrons in their valence shell due to the availability of d-orbitals. This is important for constructing Lewis structures of molecules that contain such atoms, as they can accommodate additional bonds.

Formal Charge

Formal charge is a theoretical charge assigned to individual atoms within a molecule, calculated by comparing the number of valence electrons in an isolated atom with the electrons it ‘owns’ in a Lewis structure. Minimizing the formal charge across the molecule helps in identifying the most stable and plausible structure.

Multiple Bonds

Multiple bonds involve double or triple bonds, where two or three pairs of electrons are shared between atoms. These types of bonds are used in Lewis structures to satisfy the octet rule when a single bond is insufficient to achieve a stable electron configuration.

Octet Rule

The octet rule is a chemical principle that atoms tend to form bonds in such a way that they each have eight electrons in their valence shell, achieving a noble gas configuration. This rule guides the formation of optimal Lewis structures, though some elements can deviate from it.

Lewis Structures

A Lewis structure is a diagram showing the bonding between atoms of a molecule and the lone pairs of electrons that may exist. It is a key tool in chemistry used to predict the arrangement of electrons in a molecule, determining how atoms are connected through covalent bonds, including single, double, or triple bonds.

Valence Electrons

This concept refers to the electrons in the outermost shell of an atom that are available for bonding. Counting valence electrons is essential in drawing Lewis structures, as it ensures that all electrons are correctly allocated among bonds and lone pairs.

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