Lewis Structures and Molecular Geometry

These flashcards cover key concepts related to Lewis structures and molecular geometries based on the provided lecture notes.

Lewis Structures

Diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist.

Valence Electrons

Electrons in the outermost shell of an atom that are involved in forming bonds.

Central Atom

The atom in a molecule that is bonded to multiple other atoms; usually the least electronegative.

Octet Rule

Principle stating that atoms tend to bond in such a way that they have eight electrons in their valence shell.

Free Radicals

Molecules that contain an unpaired electron, resulting in high reactivity.

Electron Geometry

The spatial arrangement of all electron groups around a central atom.

Molecular Geometry

The arrangement of atoms in a molecule, not including lone pairs.

Lone Pair

A pair of valence electrons that are not shared with another atom.

Expanded Octets

Allowing central atoms to have more than eight electrons in their valence shell, typically seen in third-period elements and beyond.

Bent Geometry

A molecular shape where the central atom has two bonded atoms and one or two lone pairs, resulting in angle less than 120\degree.

2 electron groups, 2 bonding pairs, no lone pairs on the central atom, resulting in a bond angle of 180°.

Linear

3 electron groups, 3 bonding pairs, no lone pairs on the central atom, resulting in a bond angle of 120°

Trigonal Planar

3 electron groups, 2 bonding pairs, 1 lone pair on the central atom, resulting in a bond angle of <120

Bent

4 electron groups, 4 bonding pairs, no lone pairs on the central atoms, resulting in a bond angle of 109.5

Tetrahedral

4 electron groups, 3 bonding pairs, 1 lone pair on the central atom, resulting in a bond angle of <109.5

Trigonal Pyramidal

4 electron groups, 2 bonding pairs, 2 lone pairs on the central atoms, resulting in a bond angle of <109.5

Bent

5 electron groups, 5 bonding pairs, no lone pairs, resulting in a bond angle of 120 equatorial and 90 axial

Trigonal Bipyramidal

5 electron groups, 4 bonding pairs, 1 lone pair on the central atom, resulting in a bond angle of 120 equatorial and 90 axial

Seesaw

5 electron groups, 3 bonding pairs, 2 lone pairs on the central atom, resulting in a bond angle of <90

T-shaped

5 bonding groups, 2 bonding groups, 3 lone pairs on the central atom, resulting in a bond angle of 180

Linear

6 electron groups, 6 bonding groups, no lone pairs on the central atom resulting in a bond angle of 90

Octahedral

6 electron groups, 5 bonding pairs, 1 lone pair on the central atom, resulting in a bond angle of <90

Square pyramidal

6 electron groups, 4 bonding pairs, 2 lone pairs on the central atom, resulting in a bond angle of <90

Square planar