Metal Coordination Complexes

Lewis bases form coordination complexes with transition metals and ions

Ligands that form a single coordination covalent bond

Multidentate ligands that form more than one bond

Ligands that bond in coplanar fashion

Ligands that bind in a co facial fashion

Nomenclature used to describe the geometry/symmetry of coordination complexes

Model explaining how the presence of ligands can affect the electron configuration of the metal atom

A way of gauging the relative stability of a complex

All molecules have identity, i.e., they can rotate about 360 degrees and yield the same , indistinguishable configuration

A line that divides a molecule into two identical parts, such that every atom through i meets equivalent atoms at a distance equidistant from i

Rotation about 360degrees/n yields the same configuration;

Reflection through s mirror plane yields the same configuration; can have sigma v (vertical) or sigma h (horizontal) mirror planes

Some molecules exist such that rotation about an acid followed by a reflection through a plane perpendicular to the axis, yields the same configuration

When the reflections are applied to a molecule and results in a representation that’s indistinguishable from the starting configuration

The group of all possible symmetry operations that can be performed on molecules of a given configuration

Field created by charged ligands where the energy cause the d orbitals to be split by the electric field into two or more groups that will have different designation depending on the symmetry

Oh (octahedral), Td (tetrahedral), C4v (square planar)

High spin (HS) and low spin (LS)

A complex caused when the strength of the crystal field interaction energy is less than the energy required to pair up the electrons

A complex caused when the crystal field interaction energy is greater than the pairing energy

They interact strongly with the d orbitals and will follow the Aufbau principle; low spin usually

Interact weakly with the d orbitals and will follow Hund’s rule; high spin usually

Electrons will completely fill the lower energy levels first

Spread the electrons first before pairing the mm up; all orbital take one e- before any of them accepts a second