Molecular Geometry and Lewis Structures

Flashcards based on Molecular Geometry and Lewis Structures lecture notes.

ABnem

A = central atom, B = directly bonded atoms to A, and e = nonbonding (unshared) pairs of electrons in molecular geometry formula.

Linear Molecular Geometry

Molecular geometry with 2 electron regions, 2 bonding regions, and 0 nonbonding regions, such as HgCl2 and CO2.

Trigonal Planar Molecular Geometry

Molecular geometry with 3 electron regions, 3 bonding regions, and 0 nonbonding regions, such as BF3 and SO3.

Bent Molecular Geometry

Molecular geometry with 3 electron regions, 2 bonding regions, and 1 nonbonding region, such as SO2 and NO2-.

Tetrahedral Molecular Geometry

Molecular geometry with 4 electron regions, 4 bonding regions, and 0 nonbonding regions, such as CH4 and SiCl4.

Trigonal Pyramidal Molecular Geometry

Molecular geometry with 4 electron regions, 3 bonding regions, and 1 nonbonding region, such as NH3 and PF3.

Octet Rule

The principle that atoms are most stable with eight electrons in their valence shell (except for hydrogen, which is stable with two).

Formal Charge

The charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms.

Resonance

When multiple valid Lewis structures can be drawn for a molecule, representing different possible arrangements of electrons.

Valence Electrons

The electrons in the outermost shell of an atom that participate in chemical bonding.