Chemical Bonding
Section 1: Types of Chemical Bonds
- bond: the force that holds groups of two or more atoms together and makes them function as a unit
- bond energy: the energy required to break a bond
- ionic bonding: the attraction between oppositely charged ions
- ionic compound: a compound that results when a metal reacts with a nonmetal
- covalent bonding: a type of bonding in which atoms share electrons
- polar covalent bond: a covalent bond in which the electrons are not shared equally because one atom attracts them more strongly than the other
Section 2: Electronegativity
- electronegativity: the relative ability if an atom in a molecule to attract shared electrons to itself
Section 3: Bond Polarity and Dipole Moments
- dipole moment: the magnitudes of separated charges times the distance b/t the charges
Section 4: Stable Electron Configurations and Charges on Ions
Section 5: Ionic Bonding and Structures of Ionic Compounds
Section 6: Lewis Structures
- Lewis structure: a diagram of a molecule showing how the valence electrons are arranged among the atoms in the molecule
- duet rule: the observation that atoms such as hydrogen form stable molecules when they share two electrons
- octet rule: the observation that atoms of nonmetals tend to form the most stable molecules when they are surrounded by eight electrons (to fill their valence orbitals)
- bonding pair: an electron pair found in the space between two atoms
- lone pair: an electron pair that is localized on a given atom; an electron pair not involved in bonding
Section 7: Lewis Structures of Molecules with Multiple Bonds
- single bond: a bond in which two atoms share one pair of electrons
- double bond: a bond in which two atoms share two pairs of electrons
- triple bond: a bond in which two atoms share three pairs of electrons.
- resonance: a condition occurring when more than one valid Lewis structure can be written for a particular molecule. The actual electron structure is represented not by any one of the Lewis structures but by the average of all of them
- resonance structure: various Lewis structures
Section 8: Molecular Structure
- molecular (geometric) structure: the three-dimensional arrangement of atoms in a molecule
- bond angle: the angle formed by 2 bonds; for example, the V-shaped water molecule has a 105 degree bond angle
- linear structure: a molecule with a 180-degree bond angle
- trigonal planar structure: a planar (flat) and triangular molecule with bond angles of 120 degrees
- tetrahedral structure: the structure that achieves the maximum possible separation of 4 electron pairs around a given atom, with bond angles of 109.5 degrees
Section 9: Molecular Structure: The VSEPR Model
- valence shell electron pair repulsion (VSEPR) model: a model the main postulate of which is that the structure around a given atom in a molecule is determined principally by the tendency to minimize electron-pair repulsions
- tetrahedral arrangement: 4 electron pairs arranged in tetrahedron, achieving maximum possible separation
- trigonal pyramid: an arrangement of 4 electron pairs around a given atom where one side is differ from the other 3