CHE 106 Lecture Notes - Lecture 29: Covalent Bond, Lattice Energy, Electron Configuration
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Document Summary
Lattice energy: heat of formation from 1 mol of its ionic constituents in the gas phase. Heat of formation: of a crystal, , can be measured relative to the elements, in standard states. Born-haber cycle and hess law: if a reaction is carried out in a series of steps, h for the overall reaction equals sum of enthalpy changes for individual steps; state function. Metals lose electrons to form cations to form noble gas configuration; electrons leave valence shell first. Properties of ionic compounds: well defined 3d structure, crystalline, high melting point, brittle. Covalent bonds: share valence electrons; creates electron configuration of different element. Lone pairs: electron located on only one electron in a lewis structure. Single bond: covalent bond in which single pair of electrons is shared (only 2 are shared) Double bond: involves the sharing of two pairs between atoms (4 shared) Triple bond: sharing of three pairs of electrons between atoms (6 shared)
