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Chemistry Chapter 6.2

Terms in this set (24)

atoms held together by covalent bonds
molecule
molecule examples:
water, CO2, sugar
molecules containing two atoms
diatomic molecules
diatomic molecule examples
N2, O2, F2, Cl2, Br2, I2, H2
chemical compound whose simplest units are molecules
molecular compound
Represents the relative numbers of atoms of each element in a chemical compound by using atomic symbols and numerical subscripts.
chemical formula
When these forces represent molecular compounds, they are called ______
molecular formulas
Anywhere from 2 atoms to millions of atoms can by joined together by ___________________
covalent bonds
If attraction outweighs repulsion
then the atoms bond.
If repulsion outweighs attraction
then the atoms will not bond.
average distance between two bonded atoms
bond length
energy required to break a chemical bond and form nuetral atoms
bond energy
bond energies become__________
larger as lengths become shorter
By sharing electrons
each atom has achieved the stable, noble gas configuration of helium.
In many compounds
atoms of main group elements form bonds so that each atom has an octect of electrons, which makes these atoms stable.
chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octect of electrons.
octet rule
indicates the kind, number, arrangement, and bonds of the atoms in a molecule, but not the lone pairs
structural formula
covalent bond produced by the sharing of one pair of electrons between two atoms
single covalent bond
covalent bond between two atoms produced by the sharing of two pairs of electrons
double covalent bond
covalent bond produced by the sharing of three pairs of electrons
triple covalent bond
double and triple bonds are referred to as ___________
multiple bonds
double bonds have _____________
higher bond energies and are shorter than single bonds.
triple bonds are
even stronger and shorter.
charged group of covalently bonded atoms
polyatomic ion
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