Transition Metals and Coordination Compounds

The ability of a solution to conduct electricity. It depends on factors like temperature, concentration of ions, and the nature of the electrolyte.

The force responsible for maintaining a constant flow of electricity in a circuit. It can be thought of as the 'push' that keeps electrons moving.

Describes a material where electrons move freely, allowing for good electrical conductivity.

The process of using an electric current to break down a chemical compound. It involves the formation of ions in a solution.

A law stating that the amount of chemical reaction during electrolysis is directly proportional to the amount of electricity passed.

A law stating that the amount of substances liberated by the same amount of electricity is proportional to their chemical equivalent weights.

A primary battery can only be used once, after which it becomes unusable. It cannot be recharged.

Kohlausch's law states that at infinite dilution, each ion contributes independently to the total molar conductivity of an electrolyte, regardless of the other ions present.

The rate at which a reaction proceeds, measured as the change in concentration of a reactant or product over time.

The sum of the exponents of the concentration terms in the rate law for a reaction, indicating how the rate changes with reactant concentration.

The minimum amount of energy that reactant molecules need to have to react and form the activated complex, often lowered with catalysts.

A reaction that occurs in one step, involving a single molecular collision.

A reaction that appears to be first order, but actually involves multiple steps, with one step being much slower than others.

The time it takes for half of the reactants to be consumed in a reaction, often used to characterize reaction rates.

A reaction where the rate is independent of the concentration of the reactants.

The proportionality constant in the rate law, representing the rate of the reaction at unit concentration of reactants.

The oxidation states of transition elements differ by unity (e.g., +2 and +3 for Fe). Non-transition elements have oxidation states that differ by two units (e.g., +2 and +4 for Sn).

Heavier transition elements often favor higher oxidation states (e.g., W(VI) is more stable than Cr(VI)). In contrast, heavier p-block elements tend to have lower oxidation states due to the inert pair effect (e.g., Pb(II) is more stable than Sn(II)).

Lanthanoids react with dilute acids to produce hydrogen gas. When reacting with water, they form lanthanoid hydroxides and release hydrogen gas.

The spin-only magnetic moment of an ion can be calculated using the formula √n(n+2) BM, where n is the number of unpaired electrons. For example, M2+ with 3 unpaired electrons has a magnetic moment of 3.87 BM.

Cr and Cu have unusually high second ionization enthalpies because removing a second electron disrupts their stable d5 and d10 configurations, respectively, leading to a loss of exchange energy.

Cr has a lower first ionization enthalpy than Zn because removing an electron from Cr doesn't change its d electron configuration. Zn, on the other hand, requires more energy to remove an electron from its 4s orbital.

Transition metal alloys are typically hard and have high melting points. This is attributed to their strong metallic bonding and the formation of complex crystal structures.

Coordination compounds have a central metal atom (or cation) surrounded by ligands (anions or neutral molecules). They retain their identity in solutions and solids.

The isomer of a coordination complex where identical ligands occupy adjacent positions around the central metal ion.

A compound containing a complex ion and counter ions that are not part of the coordination sphere. In aqueous solutions, they dissociate fully into their constituent ions.

The arrangement of ligands around the central metal ion.

A complex ion where the ligands are coordinated to the central metal ion through sigma bonds, resulting in a weak field splitting energy.

A complex ion where the ligands are coordinated to the central metal ion through both sigma and pi bonds, resulting in a strong field splitting energy.

The energy difference between the d orbitals in a complex ion, caused by the interaction between the metal ion and the ligands.

A complex ion with no unpaired electrons.

A complex ion with one or more unpaired electrons.

The number of ligands directly attached to the central metal atom in a coordination complex. For example, in [Co(NH3)6]3+, cobalt has a coordination number of 6.

The spatial arrangement of ligands around the central metal atom. Examples include linear, tetrahedral, square planar, and octahedral.

The charge on the central metal atom in a coordination complex. It can be determined by considering the charges of the ligands and the overall charge of the complex.

A coordination compound is paramagnetic if it has unpaired electrons, meaning it is attracted to a magnetic field. A coordination compound is diamagnetic if all electrons are paired, meaning it is not attracted to a magnetic field.

The specific order in which ions are named in a coordination compound. The cation is named first, followed by the anion.

Negative ligands often have the suffix '-o' added to their names. For example, cyanide (CN-) becomes cyano.

Neutral ligands are named without any special suffix. Some common examples include ammonia (NH3) as ammine, water as aqua, and carbon monoxide as carbonyl.

Positive ligands are named with the suffix '-ium' added to their original names. For example, nitronium (NO2+) is a positive ligand.

The number of donor atoms in a ligand that are directly bound to the central metal ion. For instance, a bidentate ligand has two donor atoms and can form two bonds to the metal ion.

A ligand that can bond to the central metal ion through two different donor atoms. For example, NO2- ion can coordinate through either nitrogen or oxygen.

A compound where a metal ion is surrounded by ligands, forming a complex ion. The complex ion is usually enclosed in square brackets to distinguish it from other ions present.

The ability of a ligand to donate electron pairs to the metal ion, forming coordinate covalent bonds.

The specific arrangement of ligands around the central metal ion in a coordination complex.

The tendency of a ligand to remove electron density from the central metal ion, weakening the metal-ligand bond. Strong ligands cause a large splitting of the d orbitals in the metal ion.

When a molecule or ion can coordinate to a metal ion through more than one atom, for example, ethylenediamine can bind through both its nitrogen atoms.