Chemical Bonding Overview
This page provides an overview of different types of chemical bonds and related concepts. It covers ionic, covalent, and metallic bonding, as well as resonance structures and formal charges.
Ionic Bonding
Ionic bonds form between metals and nonmetals. The strength of these bonds is related to the lattice energy, which is the energy required to separate the ions in a solid.
Definition: Bond energy is the energy required to break a bond.
Definition: Bond length is the distance between two bonded atoms where the energy is at its lowest point.
The interaction between ions in an ionic bond can be calculated using Coulomb's Law:
Highlight: Coulomb's Law states that the closer two objects are to each other, the greater the attraction if the charges are opposite, and the greater the repulsion if the charges are the same.
Covalent Bonding
In covalent bonds, electrons are shared between atoms. The strength of covalent bonds can vary based on the type of bond.
Vocabulary: Polar covalent bonds result from unequal sharing of electrons, while nonpolar covalent bonds involve equal sharing.
Electronegativity values are used to determine a bond's polarity. The closer the atoms are, the stronger the force between them.
Example: A carbon-carbon double bond (C=C) is stronger than a single bond (C-C) and adds stability to the molecule.
Resonance Structures
Definition: Resonance structures are multiple valid Lewis structures that represent a single molecule or ion.
Example: The nitrite ion (NO₂⁻) is an example of a molecule with resonance structures.
Formal Charge
Formal charge is a concept used to predict the most stable Lewis structure for a molecule.
Highlight: The most stable molecules typically have a formal charge of zero.
The formal charge can be calculated using the following formula:
Definition: Formal Charge = Valence electrons - (non-bonding electrons + ½ bonding electrons)
This page provides a comprehensive overview of chemical bonding, covering the main types of bonds and related concepts such as resonance structures and formal charges. Understanding these principles is crucial for predicting molecular structure and reactivity in chemistry.
