| A | B |
|---|
| ionic bonding | results from the electrical attraction between cations and anions |
| covalent bonding | sharing of electron pairs between two atoms |
| chemical bond | mutual attraction between the nuclei and valence eectrons of different atoms that binds the atoms together |
| non-polar covalent bond | covalent bond where bonding electrons are shared equally by the bonded atoms, resulting in a balanced electrical charge |
| polar | uneven dstribution of charge |
| polar-covalent | covalent bond in which the boncded atoms have an unequal attraction for shared electrons |
| molecule | neutral group of atoms that are held together by covalent bonds |
| molecular compound | chemical compound whose simplest units are molecules |
| chemical formula | indicats the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts |
| molecular formula | shows shows the types and numbes of atoms combined in a single molcule of a molecular compound |
| bond energy | energy requred to brea a chemical bond and form neutral isolated atoms |
| electron dot-notation | electron configuration notation where only the valence electrons of an atom of a particular elemet are shown, indicated by dots around its symbol |
| Lewis Structures | formulas i which atomic symbols represent nuclei and inner-shell electrons, dot pairs or dashes between tw atomic symbols represent electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent unshared electrons |
| structural formula | indicates the kind, number, arrangement, and bonds but not hte unshared pairs of the atoms in a molecule |
| single bond | covalent bond in which one pair of electrons is shared between two atoms |
| multiple bonds | double and triple bonds |
| resonance | bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
| ionic compound | composed of positive and negative ions that are combinedso that the numbers of positive and negative ions tat are combined so that the numbers of postive and negative charges are equal |
| formula unit | simplest collection of atoms from which an ionic compound's ormula can be established |
| lattice energy | energy released when one mole of an ionic crstalline compound is formed from gaseous ions |
| polyatomic ion | charged group of covalently bonded atoms |
| metallic bonding | chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons |
| malleability | ability of a ubstance to be hammered or beaten into sheets |
| ductility | ability of a substace to be rawn, pulled, or extruded through a small opening to produce a wire |
| VSEPR Theory | repulsio between the sets of valence level surrounding an atom causes these sets t obe oriented as far apart as possible |
| hybridization | mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies |
| hybrid orbitals | orbitals of equal energy producedby the cmbination of two or more orbitals on the same atom |
| dipole | created by equal bt opposite charges that are seperated by a short distance |
| hyrogen bonding | intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule |
| london dispersion forces | intermolecular attrractions resulting from the constant motion of electrons and the creation of instantaneous dipoles |
