Chemical Bonding I: Drawing Lewis Structures and Determining Molecular Shapes

These flashcards cover the key concepts and terms from the lecture on chemical bonding, focusing on molecular shapes, Lewis structures, and polarity.

Morphine

A natural product from opium poppy with pain-relieving attributes, mimicking endorphins due to similar molecular shape.

Lewis Theory

A simple bonding theory that emphasizes valence electrons to explain bonding and predict properties of molecules.

Electronegativity

The ability of an atom to attract bonding electrons to itself; influences bond polarity.

Dipole Moment (μ)

A measure of bond polarity, proportional to the size of the partial charges and the distance between them.

Formal Charge

An electron bookkeeping system to distinguish between competing Lewis structures, calculated using the formula: (# of valence electrons) - (# of nonbonding electrons) - (1/2 × # of bonding electrons).

Expanded Octet

Occurs when a central atom can accommodate more than eight electrons, possible only for p-block atoms in period 3 or later.

VSEPR Theory

Theory that predicts molecular shapes based on the premise that electron groups around a central atom are arranged as far apart as possible.

Polar Covalent Bond

A type of bond formed between two atoms with differing electronegativities resulting in unequal sharing of electrons.

Octahedral Geometry

Electron geometry that occurs when there are six electron groups around a central atom, resulting in bond angles of 90°.

Resonance Structures

Multiple valid Lewis structures for the same compound that differ only in the position of electrons.