Write Lewis structures for (a) N2^+ (b) XeF7^- (c) tetracyanoethene, C6 N4

Name: Problem 20, Chapter 6: Chemistry The Molecular Science
Uploaded: 2021-05-20T15:59:52-08:00
Duration: 2 min
Channel: Lottie Adams
Description: Write Lewis structures for (a) N2^+ (b) XeF7^- (c) tetracyanoethene, C6 N4

step 1 Chemical bond that involves the sharing of electron pairs between atoms and these electron pairs

Write Lewis structures for (a) N2^+ (b) XeF7^- (c)...

Key Concepts

Resonance Structures

Resonance structures are multiple valid Lewis diagrams for a single molecule or ion differing only in the distribution of electrons. They are used to represent electron delocalization when no single Lewis structure adequately describes the bonding, thereby providing a more accurate picture of the electron distribution in the molecule.

Octet Rule

The octet rule is the principle that atoms tend to form bonds to achieve eight electrons in their valence shell, mimicking the electron configuration of noble gases. This rule is a guiding factor when drawing Lewis structures, although some atoms are exceptions due to factors like their position in the periodic table.

Expanded Octet (Hypervalency)

Expanded octet, or hypervalency, refers to the ability of certain atoms, typically those from the third period onward, to accommodate more than eight electrons in their valence shells. This concept is important when drawing Lewis structures for molecules involving such atoms, as it allows for additional bonding beyond the typical octet configuration.

Valence Electron Counting

Valence electron counting involves determining the total number of electrons available for bonding by summing the valence electrons of all atoms present, adjusted for any overall charge on the molecule or ion. This count is essential for distributing electrons correctly in a Lewis structure and for ensuring that each atom has an appropriate share of electrons.

Lewis Structures

Lewis structures are diagrams that illustrate the bonding between atoms of a molecule and the lone pairs of electrons that may exist. They serve as a basic model for understanding molecular bonding and geometry, showing how valence electrons are arranged to satisfy bonding requirements and the octet rule where applicable.

Formal Charge

Formal charge is a concept used to assess the distribution of electrons in a molecule or ion by comparing the number of electrons an atom ‘owns’ in the Lewis structure to its number of valence electrons in the uncombined state. Calculating formal charges helps in determining the stability of a given structure and directs the placement of electrons in a way that minimizes energy.

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