Chapter 8: Basic Concepts of Chemical Bonding Lecture Notes

These flashcards cover the key concepts of chemical bonding discussed in the lecture, including types of bonds, important rules, and properties related to chemical structures.

Ionic Bonding

Electrostatic attraction between oppositely charged ions.

Covalent Bonding

The sharing of electrons between atoms.

Metallic Bonding

Bonding in which metal atoms have electrons that are relatively free to move around the metal.

Lewis Symbols

Chemical symbols surrounded by dots to symbolize valence electrons.

Octet Rule

Atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons.

Electronegativity

The ability of atoms in a molecule to attract electrons to themselves.

Bond Polarity

The degree to which electrons are shared equally or unequally in a covalent bond.

Formal Charge

A test to determine the efficiency of electron distribution in a molecule.

Resonance

The use of multiple Lewis structures to describe a molecule that cannot be accurately depicted by a single structure.

Multiple Bonds

Bonds in which two or more pairs of electrons are shared between atoms, such as single, double, or triple bonds.

Ionic Bonding

Electrostatic attraction between oppositely charged ions.

Covalent Bonding

The sharing of electrons between atoms.

Metallic Bonding

Bonding in which metal atoms have electrons that are relatively free to move around the metal.

Lewis Symbols

Chemical symbols surrounded by dots to symbolize valence electrons.

Octet Rule

Atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons.

Electronegativity

The ability of atoms in a molecule to attract electrons to themselves.

Bond Polarity

The degree to which electrons are shared equally or unequally in a covalent bond.

Formal Charge

A test to determine the efficiency of electron distribution in a molecule.

Resonance

The use of multiple Lewis structures to describe a molecule that cannot be accurately depicted by a single structure.

Multiple Bonds

Bonds in which two or more pairs of electrons are shared between atoms, such as single, double, or triple bonds.

Exceptions to the Octet Rule

Situations where atoms in molecules may have fewer or more than eight valence electrons around them, often seen in central atoms of period 3 and below.

Valence-Shell Electron-Pair Repulsion (VSEPR) Theory

A model that predicts the geometry of individual molecules from the number of electron pairs surrounding their central atoms.

Molecular Geometry

The three-dimensional arrangement of atoms in a molecule, which is determined by the positions of the atomic nuclei and the nonbonding electron pairs.

Dipole Moment

A measure of the polarity of a molecule, resulting from the unequal distribution of electron density among its atoms.