CHEM 1210 Study Guide - Midterm Guide: Lattice Energy, Molecular Geometry, Electron Affinity

• School: Ohio State University
• Department: Chemistry
• Course: CHEM 1210
• Professor: Matthew Stoltzfus

Document Summary

Metal from left side of periodic table bonded to nonmetal. Typically, a metal with low ionization energy bonded to nonmetal with high electron affinity: covalent: shared electrons. Dipole: 2 electrical charges of equal magnitude separated by a distance. Dipole moment=magnitude x distance: metallic: electrons flow through metal. Lewis structures: formal charge: charge an atom would have if each bonding pair was shared equally. Formal charge=valence electrons-1/2 of bonding electrons-lone pairs. Multiple bonds: sigma bond: overlap of 2s, s/p, p/p,p/sp orbitals, pi bond: overlap of 2p orbitals perpendicular to nuclear axis. Triple bond-sigma and 2 pi: molecular orbitals: hold only 2 electrons (entire molecule, bond order=1/2 (bonding electrons-antibonding electrons) 1=single bond: paramagnetic: unpaired electrons, diamagnetic: no unpaired electrons. Cations are smaller than atoms (more positive, protons pull electrons closer) Anions are bigger than atoms (more negative, electrons pull away) When sorting by lattice energy: group by charge first, then by radius.