Electron and Molecular Geometry Practice

Vocabulary flashcards covering electron geometries, their associated bond angles, and the resulting molecular geometries based on lone pairs.

Linear

An electron geometry with an ideal angle of $180^{\circ}$. It has two electron groups.

Trigonal planar

An electron geometry with an ideal angle of $120^{\circ}$. It has three electron groups.

Tetrahedral

An electron geometry with an ideal angle of $109.5^{\circ}$. It has four electron groups.

Trigonal bipyramidal

An electron geometry with an ideal angle of $120^{\circ}$ and $90^{\circ}$. It has five electron groups.

Octahedral (Electron Geometry)

An electron geometry with an ideal angle of $180^{\circ}$ and $90^{\circ}$. It has six electron groups.

Bent (within a trigonal planar)

Has only 1 lone pair on the central atom.

Trigonal pyramidal (within a tetrahedral)

Has only 1 lone pair on the central atom.

Bent (within Tetrahedral)

Has only 2 lone pairs on the central atom.

Seesaw (within trigonal bipyramidal)

Has only 1 lone pair on the central atom.

T-shaped (within Trigonal bipyramidal)

Has only 2 lone pairs on the central atom.

Linear (from Trigonal bipyramidal)

Has only 3 lone pairs on the central atom.

Square pyramidal (within Octahederal)

Has only 1 lone pair on the central atom.

Square planar (within Octahederal)

Has only 2 lone pairs on the central atom.

T-shaped (within Octahedral)

Has only 3 lone pairs on the central atom.

Linear (within Octahedral)

Has 4 lone pairs on the central atom.

What is the Bond Order formula?

Bond Order = (bonding e^- - anti-bonding e^- ) / 2