Syllabus: https://www.luther.edu/mertzecl/courses/chem372/
Chemistry 372 is a course including molecular and solid-state bonding and structure, molecular symmetry, and coordination and organometallic chemistry.
Introductory topics in inorganic chemistry including descriptive inorganic chemistry, solid-state chemistry, and coordination chemistry with the latter area consisting of nomenclature, stereochemistry, bonding, and reaction mechanisms.
This course focuses on the concepts of inorganic chemistry with emphasis on atomic structure, periodicity, group and bonding theories, symmetry, solid-state structures of metals, ionic compounds and semiconductors, as well as transition metal coordination chemistry.
Descriptive chemistry of the main group elements with some emphasis on the non-metals. Transition metal compounds: aspects of bonding, spectra, and reactivity; complexes of n-acceptor ligands; organometallic compounds and their role in catalysis; metals in biological systems; preparative, analytical, and instrumental techniques.
In searching for a way to review topics before exams, I was informed about this powerpoint template which is macro'd to be operated as a realistic Jeopardy game. The site for the original author of the macro is:
https://sites.google.com/site/dufmedical/jeopardy
(Jeopardy for PowerPoint by Kevin R. Dufendach is licensed under a Creative Commons Attribution 3.0 United States License.)
A systematic study of both the fundamental principles and the descriptive chemistry needed to understand the properties of the main group elements and their compounds. (Three lecture, one recitation, and three laboratory hours per week) Prerequisites: CHEM 1200.
This article describes the synthesis and characterization of ternary rare-earth gallium bismuthide, LaGaBi
Inorganic chemistry is a branch of synthetic chemistry typified by its focus on compounds composed of elements other than carbon and hydrogen. But don’t let that fool you!
This activity is a guided approach to answering the following: "Give an example of a silver (Ag+) salt that is expected to be soluble in water." It requires students to consider both HSAB and Bronsted acid/base concepts when evaluating solubility.
I use the activity at the end of the unit on reactivity of ions in aqueous solutions, after we have gone over all of the relevant concepts, and the question (without scaffolding) is similar to what I might ask on an exam.