Chapter 7 Chemical Bonding and Molecular Geometry
Chapter 7 Key Terms
location in a trigonal bipyramidal geometry in which there is another atom at a 180° angle and the equatorial positions are at a 90° angle
angle between any two covalent bonds that share a common atom
separation of charge in a bond that depends on the difference in electronegativity and the bond distance represented by partial charges or a vector
(also, bond length) distance between the nuclei of two bonded atoms
(also, bond dissociation energy) energy required to break a covalent bond in a gaseous substance
distance between the nuclei of two bonded atoms at which the lowest potential energy is achieved
thermochemical cycle relating the various energetic steps involved in the formation of an ionic solid from the relevant elements
bond formed when electrons are shared between atoms
property of a molecule that describes the separation of charge determined by the sum of the individual bond moments based on the molecular structure
covalent bond in which two pairs of electrons are shared between two atoms
arrangement around a central atom of all regions of electron density (bonds, lone pairs, or unpaired electrons)
tendency of an atom to attract electrons in a bond to itself
one of the three positions in a trigonal bipyramidal geometry with 120° angles between them; the axial positions are located at a 90° angle
charge that would result on an atom by taking the number of valence electrons on the neutral atom and subtracting the nonbonding electrons and the number of bonds (one-half of the bonding electrons)
molecule that contains an odd number of electrons
molecule containing at least one main group element that has more than eight electrons in its valence shell
tendency of heavy atoms to form ions in which their valence s electrons are not lost
strong electrostatic force of attraction between cations and anions in an ionic compound
energy required to separate one mole of an ionic solid into its component gaseous ions
diagram showing lone pairs and bonding pairs of electrons in a molecule or an ion
symbol for an element or monatomic ion that uses a dot to represent each valence electron in the element or ion
shape in which two outside groups are placed on opposite sides of a central atom
two (a pair of) valence electrons that are not used to form a covalent bond
arrangement of atoms in a molecule or ion
structure that includes only the placement of the atoms in the molecule
shape in which six outside groups are placed around a central atom such that a three-dimensional shape is generated with four groups forming a square and the other two forming the apex of two pyramids, one above and one below the square plane
guideline that states main group atoms will form structures in which eight valence electrons interact with each nucleus, counting bonding electrons as interacting with both atoms connected by the bond
covalent bond between atoms of different electro negativities; a covalent bond with a positive end and a negative end
(also, dipole) molecule with an overall dipole moment
(also, nonpolar covalent bond) covalent bond between atoms of identical electronegativities
situation in which one Lewis structure is insufficient to describe the bonding in a molecule and the average of multiple structures is observed
two or more Lewis structures that have the same arrangement of atoms but different arrangements of electrons
average of the resonance forms shown by the individual Lewis structures
bond in which a single pair of electrons is shared between two atoms
shape in which four outside groups are placed around a central atom such that a three-dimensional shape is generated with four corners and 109.5° angles between each pair and the central atom
shape in which five outside groups are placed around a central atom such that three form a flat triangle with 120° angles between each pair and the central atom, and the other two form the apex of two pyramids, one above and one below the triangular plane
shape in which three outside groups are placed in a flat triangle around a central atom with 120° angles between each pair and the central atom
bond in which three pairs of electrons are shared between two atoms
valence shell electron-pair repulsion theory (VSEPR)
theory used to predict the bond angles in a molecule based on positioning regions of high electron density as far apart as possible to minimize electrostatic repulsion
quantity having magnitude and direction