Chapter 9: Chemical Bonding I, Basic Concepts Flashcards
Bond Enthalpy
The enthalpy change required to break a bond in a mole of gaseous molecules
Bond Length
the distance between the nuclei of two bonded atoms in a molecule
Born-Haber cycle
the cycle that relates lattice energies of ionic compounds to ionization energies, electron affinities, heats of sublimation and formation, and bond enthalpies
Coordinate covalent bond
A bond in which the pair of electrons is supplied by one of the two bonded atoms, also called a dative bond
Coulomb’s Law
the potential energy between two ions is directly proportional to the product of their charges and inversely proportional to the distance between them
Covalent Bond
a bond in which two electrons are shared by two atoms
Covalent Compound
compounds containing only covalent bonds
Double Bond
two atoms are held together by two pairs of electrons
Electronegativity
the ability of an atom to attract electrons toward itself in a chemical bond
Formal charge
the difference between the valence electrons in an isolated atom and the number of electrons assigned to that atom in a lewis structure
Ionic Bond
the electrostatic force that holds ions together in an ionic compound
Lewis dot symbol
the symbol of an element with one or more dots that represent the number of valence electrons in an atom of the element
Lewis structure
a representation of covalent bonding using lewis symbols, shared electron pairs are shown either as lines or as pairs of dots between two atoms, and lone pairs are shown as pairs of dots on individual atoms
Lone pair
Valence electrons that are not involved in covalent bond formation
Multiple Bond
Bonds formed when two atoms share two or more pairs of electrons
