Chemical Bonding I: Drawing Lewis Structures and Determining Molecular Shapes

These flashcards cover key vocabulary terms and definitions related to chemical bonding, Lewis structures, molecular shapes, and properties.

Morphine

A natural product from the opium poppy that relieves pain by binding to opioid receptors.

Bonding Theories

Explanations of how and why atoms attach to form molecules, predict stability, shape, and properties.

Lewis Theory

A bonding theory emphasizing valence electrons to predict molecular properties.

Chemical Bonds

Interactions that lower potential energy between charged particles in atoms.

Covalent Bonds

Bonds formed through the sharing of electrons between atoms.

Bond Polarity

The degree to which electrons are shared unequally in a bond, resulting in dipoles.

Electronegativity

The ability of an atom to attract bonding electrons; increases across a period and decreases down a group.

Polar Covalent Bond

A type of bond where electrons are shared unequally, creating partial charges.

Dipole Moment

A measure of the polarity of a bond; depends on the size of partial charges and their distance.

Percent Ionic Character

The percentage of a bond's dipole moment compared to an entirely ionic bond.

Formal Charge

A bookkeeping method to determine the distribution of electrons in a molecule.

Resonance Structures

Different Lewis structures for the same compound that show delocalization of electrons.

VSEPR Theory

Valence Shell Electron Pair Repulsion theory used to predict molecular shapes.

Molecular Geometry

The three-dimensional arrangement of atoms in a molecule, determined by electron pairs.

Octet Rule

Atoms tend to bond in such a way that they each have eight electrons in their valence shell.

Expanded Octets

Atoms in the third period or below can accommodate more than eight electrons.

Lone Pairs

Nonbonding pairs of electrons that can affect the molecular geometry.

Molecular Polarity

Determined by the presence of polar bonds and the symmetry of the molecule.

Bond Energy

The energy required to break one mole of a bond in a compound.

Bond Length

The distance between the nuclei of bonded atoms; typically shorter for stronger bonds.