CH 301 Study Guide - Midterm Guide: Lattice Energy, Atomic Radius, Valence Electron
Document Summary
Formed between a metal and nonmetal (lattice of + and - charged ions) Tightly held set of neutral atoms forming neutral bond. Elements cannot be broken down into simpler substances (physically or chemically) Ionic compounds are collections of many ions (also polyatomic ions) Metals form cations (+) and nonmetals form anions (-) Valence electrons those in the outer shell. Ionic charge +1, +2, transition metals, +3, -3, -2 ,-1, 0. Chemical bonds that have moved from one element in compound to another (forms ions) Sum of ionization energy, electron affinity, and lattice energy. Same trend as atomic radius, but cations and anions have diff. radius. Lattice structure: small size ion = large charge density, greater charge density = greater lattice energy. Minimizing r and energy gives covalent compounds a stable state. Distance at which the p. e. is at a minimum. Difference in energy at minimum compared to separated atoms. Amount of energy required to separate two bonded atoms.
