 | Term | Definition |
| |
Chemical Bond |
a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
| |
Ionic Bonding |
chemical bonding that results from the electrical attraction between large numbers of cations and anions |
| |
Covalent Bonding |
the sharing of electron pairs between two atoms |
| |
Non-polar covalent bond |
a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution |
| |
Polar |
having uneven distribution of charge |
| |
Polar-covalent Bond |
a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons |
| |
Molecule |
a neutral group of atoms that are held together by covalent bonds |
| |
Molecular compound |
a chemical compound whose simplest units are molecules |
| |
Chemical formula |
indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscrpts |
| |
Molecular Formula |
types and numbers of atoms combined in a single molecule of a molecular compound |
| |
Diatomic Molecule |
a molecule with only two atoms |
| |
Bond Length |
the distance between two bonded atoms at their minimum potential energy |
| |
Bond Energy |
then energy required to break a chemical bond and form neutral isolated atoms |
| |
Octed Rule |
Chemical compounds tend to form so that each atom by gaining losing sharing electrons has an octet of electrons in its highest occupied energy level |
| |
Electron dot nNotation |
an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by the dots placed around the elements |
| |
Unshared Pair |
a pair of electrons that is not involved in bonding and that belongs exclusively to one atom; une pair |
| |
Lewis Structures |
formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent unshared electron |
| |
Structural Formula |
indicates the kind number arrangement bonds but not the unshared pairs of the atoms in a molecul |
| |
Single Bond |
a covalent bond produced by the sharing of one pair of electrons between two atoms |
| |
Ionic Compound |
composed of postivite and negative ions that are combined so that the numbers of positive or negative charges are equal |
| |
Formula Unit |
the simplest collection of atoms from which an ionic compound's formula can be established |
| |
Lattice Energy |
the energy relased when one mole of an ionic crystalline compound is formed from gaseous ions |
| |
Molecular Polarity |
the uneven distribution of molecular charge |
| |
VSEPR theory |
repulsion between the sets of valence level electrons surrounding an atom causes thses sets to be oriented as far apart as possible |
| |
Hybridization |
the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies |
| |
Dipole |
created by equal but opposite charges that are seperated by a shore distance |
| |
Dipole-Dipole |
the forces of attraction between polar molecules |
| |
Hydrogen Bonding |
the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons and electronegative atom in a nearby molecule |
| |
London Dispersion Forces |
the intermolecular attractions resulting fromt he constant motion of electrons and the creation of instantaneous dipoles |
Share on Facebook
Share on MySpace