Transition Elements Quiz

Transition metals are elements that have their highest energy electrons in the d-orbitals, and have variable oxidation states. These states allow for the formation of diverse ions with distinct colours.

The ability of a transition metal to form ions with different charges due to the similar energy levels of its d and s orbitals.

For example, copper can form Cu+ and Cu2+ ions. The oxidation state of the metal must be specified when naming its compounds.

Transition metals have variable oxidation states because the energies of their 3d and 4s orbitals are similar, allowing for the loss of electrons from both.

Transition metals are all metals and tend to lose electrons to form positively charged ions.

The color of transition metal compounds is often due to the changes in electron configuration that occur when they form ions.

The d orbitals can accept electrons, resulting in coloured compounds due to the absorption and emission of light.

The d-orbitals of transition metals are involved in bonding and can be affected by the presence of ligands, leading to distinctive colors.

A type of isomerism in coordination complexes where the arrangement of ligands around the central metal ion differs. This results in molecules with the same formula but different spatial arrangements.

An isomer that has two identical ligands on the same side of the central metal ion.

An isomer that has two identical ligands on opposite sides of the central metal ion.

A type of isomerism in which two molecules are mirror images of each other but cannot be superimposed.

A molecule that rotates the plane of polarized light.

A molecule that does not rotate the plane of polarized light.

A ligand that can bind to a metal ion through two donor atoms.

A complex that contains a metal ion and at least one bidentate ligand.

Transition elements lose electrons from the 4s subshell first, followed by 3d electrons.

The highest possible positive charge an atom can achieve in its ionic form.

Elements with partially filled d subshells in either the neutral atom or its ions.

Scandium forms Sc3+ by losing all 3 of its outer electrons (4s and 3d). Zinc forms Zn2+ by losing its 2 4s electrons. Neither has a partially filled d subshell in their ions, making them not transition elements.

Manganese's maximum oxidation state is +7 because it can lose all 7 of its outer electrons (2 4s and 5 3d electrons).

The charge of a metal atom in a compound, representing the number of electrons lost or gained.

Zirconium has the electronic configuration [Kr] 4d2 5s2, suggesting a maximum oxidation state of +4. It can lose both of its 5s electrons and two 4d electrons.

The oxide of zirconium with a +4 oxidation state is ZrO2.

The stability constant (Kstab) is a measure of the equilibrium position of a reaction where a complex ion is formed. It is defined as the ratio of the product of the concentrations of the complex ion formed to the product of the concentrations of the reactants, all raised to their stoichiometric coefficients in the balanced chemical equation. It is a quantitative measure of the stability of a complex ion.

The units of Kstab can be determined by substituting the units of concentration (mol dm-3) into the equilibrium expression and then canceling out the units. The resulting units will depend on the stoichiometry of the reaction.

A larger value of log10Kstab indicates a larger value of Kstab, which means that the concentration of the products in the equilibrium expression is much greater than the concentration of the reactants. This suggests that the formation of the complex ion is highly favored.

The addition of concentrated ammonia solution to copper(II) chloride results in a color change from greenish-yellow to deep blue due to the formation of a more stable copper(II) ammine complex. The ammonia molecules displace the chloride ions from the copper(II) chloride complex, forming a new complex with a higher stability constant.

The stability constant for a ligand exchange reaction is the ratio of the product of the concentrations of the complex ion formed and the concentration of water to the product of the concentrations of the reactants, all raised to their stoichiometric coefficients.

The value of Kstab for a ligand exchange reaction can be calculated by dividing the equilibrium concentration of the product by the product of the equilibrium concentrations of the reactants, each raised to their respective stoichiometric coefficients.

The units of Kstab for a ligand exchange reaction can be determined by substituting the units of concentration (mol dm-3) into the equilibrium expression and then canceling out the units. The resulting units will depend on the stoichiometry of the reaction.

The energy difference between the split d orbitals in a transition metal ion. It determines the color absorbed by the complex, and thus the color we see.

The arrangement of ligands around a central metal ion in a coordination complex. Different arrangements lead to variations in the energy splitting between d orbitals.

Ligands like ammonia (NH3) cause a larger energy difference (ΔE) between split d orbitals compared to water (H2O) ligands. This results in a deeper blue color.

In tetrahedral complexes, the d orbitals split differently. The t2 orbitals (dxy, dxz, dyz) are lower in energy while the e orbitals (dz2, dx2-y2) are higher in energy.

The color of a coordination complex is a result of the absorption of specific wavelengths of light. The energy absorbed corresponds to the difference between the split d orbitals (ΔE).

The product of the concentrations of the products, each raised to the power of its stoichiometric coefficient, divided by the product of the concentrations of the reactants, each raised to the power of its stoichiometric coefficient.

The larger the stability constant, the more stable the complex ion is. This means that the complex ion is more likely to form and less likely to dissociate.

The reaction will favor the formation of the complex ion with the higher stability constant.

It represents the concentration of a species at equilibrium. For instance, [Cu(H2O)5Cl]+(aq) indicates the concentration of the [Cu(H2O)5Cl]+ complex ion at equilibrium.

The formula of the complex ion with the higher stability constant will be favored.

The reaction will shift towards the formation of the more stable iron(III) fluoride complex.

The central metal ion, Fe3+, is surrounded by six water molecules, each coordinated to the iron ion through an oxygen atom. The structure is octahedral.

The red color arises from the formation of a complex ion where one water molecule in the aqua ion is replaced by a thiocyanate ion, resulting in [Fe(H2O)5(SCN)]2+.