Chemistry of First-Row Transition Elements

Study Notes

Students should be able to list the first-row transition elements.
Students should be able to describe the properties of transition elements.
Students should be able to explain fundamental concepts in coordination chemistry.
Students should be able to name metal complexes using IUPAC conventions.
Students should be able to explain crystal field theory (CFT).
Students should be able to illustrate CFT with examples of coordination compounds diagrammatically.
Students should be able to articulate the advantages of CFT over other bonding theories.
Students should be able to discuss the comparative chemistry of specific elements (e.g., Ga, In, Tl; Ge, Sn, Pb; As, Sb, Bi; Se, Te, Po).

Chemistry of first-row transition metals
Properties of transition elements
Basic concepts of coordination chemistry
IUPAC nomenclature for coordination compounds
Introduction to coordination chemistry with a focus on crystal field theory (CFT)
Comparative chemistry of selected elements:
- Gallium (Ga), Indium (In), Thallium (Tl)
- Germanium (Ge), Tin (Sn), Lead (Pb)
- Arsenic (As), Antimony (Sb), Bismuth (Bi)
- Selenium (Se), Tellurium (Te), Polonium (Po)

Transition elements are elements with an incomplete d-subshell in their atoms or cations.
Found in the d-block of the periodic table, positioned between Groups 2 and 3.
The first transition series spans from scandium to zinc.
Transition elements, in period 4, are sandwiched between the highly electropositive s-block metals and electronegative elements of the p-block.

Generally, transition metals are hard, have high melting and boiling points, and strong metallic bonding.
They are good conductors of heat and electricity.
Transition metals exhibit variable oxidation states. This is because of the availability of electrons in their 3d and 4s orbitals for bonding.

The following sections are examples of the comparative study components of the course.

Chemical Reactivity: Transition metals demonstrate less variation in chemical properties due to progressive filling of inner d orbitals, in contrast to the trends in s- and p-block elements.
Variable Oxidation States: The availability of 3d and 4s electrons for bonding results in a range of oxidation states in transition metals, which is characteristic of transition elements. This contrasts with the more fixed oxidation state in non-transition elements from other groups.