Chapter 6 Vocabulary Flashcards
a mutual electrical attraction between the nuclei and the valence electrons of different atoms that binds the atoms together
chemical bond
repulsion be†ween the sets of valence level electrons surrounding an a†om causes these sets to be oriented as far apart as possible
VSEPR theory
results in the sharing of electron pairs between two atoms
covalent bond
a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge
non polar covalent bond
an uneven distribution of charge
polar
bonded atoms have an unequal attraction for the shared electrons
polar covalent bond
neutral group of atoms that are held together by covalent bonds
molecule
a chemical bond with the simplest units of molecules
molecular compound
relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
chemical formula
shows the types and numbers of atoms combined in a single molecule of a molecular compound
molecular formula
the energy required to break a chemical bond
bond energy
uses valence electrons in the form of dots around the element symbol
electron dot notation
formulas in which atomic symbols represent nuclei and innershell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds and dots adjacent to only one atomic symbol represents unshared electrons
Lewis structure
a covalent bond in which one pair of electrons is shared between the two atoms
single bond
indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule
indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule
triple and double bonds
multiple bond
bonding in molecules or Ions that cannot be correctly represented by a single Lewis structure
resonance structures
a combo of positive and negative ions that when combined the number of + and - charges are equal
ionic bonding
the simplest collection of atoms from which an ionic compounds formula can be written
formula unit
the energy released when one mole of an ionic crystalline compound is formed from the gaseous ion
lattice energy
the bonding that results from the attraction between metals and their sea of electrons
metallic bonding
