Bonding

MOLCULAR GEOMETRIES

Day 1:  Chemical Bond = a mutual electrical attraction between the nuclei and valence electrons of different atoms that bonds the atoms together.

Day 2  bond energy = the energy required to break a given chemical bond

Day 3:  Lewis Structure = a formula for a structure in which 1) atomic symbols represent nuclei and inner shell electrons, 2) dot-pairs of dashes between two atomic symbols represent electron pairs in covalent bonds, 3) and dots adjacent to only one atomic symbol represent unshared electrons.

Day 4:  VSEPR Theory = repulsion between the sets of valence level electrons surrounding an atom which causes these sets of electrons to be oriented as far apart as possible; yielding a shape.

Day 5:  Lone Pair = a pair of electons that is not involved in the bonding and that belongs exclusively to one atom.

Day 6:  Resonance = the bonding in molecules or ions that cannot be correctly represented by a single Lewis Structure.

Day 7:  Polarity = due to differences in electronegativities and shapes of molecules, some will experience unequal sharing of electrons cause part of the molecule to be more negative than the other (think of two poles of a magnet)

Day 8:  Bond Length = the distance between the nuclei of two bonded atoms.

Day 9: Delocalized electrons = an electron shared by more than two atoms.

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