CHM 12600 Study Guide - Final Guide: Paramagnetism, Transition Metal, Diamagnetism
Document Summary
After completing this topic, a student should be able to demonstrate understanding of the concepts by. Bases donate pairs of electrons, acids accept pairs of electrons. A lewis acid is therefore any substance, such as the. H+ ion, that can accept a pair of nonbonding electrons: explaining why transition metals tend to behave as lewis acids. Transition metals: accept electron pair lewis acid. Ligands: donate electron pair lewis base (cid:491). des(cid:268)ri(cid:267)in(cid:307) the nature o(cid:306) a (cid:577)(cid:268)oordinate (cid:268)o(cid:452)alent (cid:267)ond(cid:578). In a complex, the number of ligand atoms bonded to the central metal ion: explaining why water and halide ions, for example, do not behave as bidentate ligands. Shapes without bended structures have coordination sites too far for the electron pair to bind with. Octahedral, and tetrahedral shapes provide convenient angles for bonding: describing the difference(s) between. Linkage isomers: point of attachment of at least one ligand differs (donor atoms differ), different physical and chemical properties.