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Glossary of Chem Honors Chapter 6

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molecule
neutral group of atoms that hare held together my covalent bonds
molecular compound
chemical compound whose simplest units are molecules
chemical formula
indicates the relative numbers of atoms in each kind of chemical compound by using atomic symbols and numerical subscripts
molecular formula
shows the types and numbers of atoms combined in a single molecule of a molecular compound
diatomic molecule
a molecule carrying 2 atoms
bond length
the distance between 2 bonded atoms at their minimum potential nergy/ the average distance btween 2 bonded atoms
bond energy
energy required to break a bond
octet rule
chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level
chemical bond
the forces that hold groups of atoms together and make them function as a unit
form to make molecule more stable
intramolecular
within a molecule
ionic
covalent- polar, non, coordinate
covalent network
metallic
intermolecular bonds
between 2 more more molecules already bonded by intramolecular bonds
h bonds
dipole-diople interactions
london dispersion forces
ion-molecule interactions
ionic bonding
electrostatic attaction between cation and an anion. metal and nonmetal
crystal lattices
high mps
brittle
dissolve in water good conductor of electro
not in solid
monatomic ions
one atom ions (ca-)
polyatomic ions
ions consisting of more than 1 (SO42-)
covalent
2 nonmetals
shared pair of electrons between 2 atoms
united- molecule
lower mps
dipole moments0 2 poles, positive and negative pole
Dipole-dipole
2 polar molecules w/ permanent diple + and = attract
Hydrogen bonds
H with F, N, O
London Dispersion Forces
LDF- constant movement of electrons in electron cloud- instantaneous dipole,increase w/ size of the atom
Ion-dipole
Ions interact w. charged ends of polar molecules
Van Der Waals forces
LDFs and Dipole-dipole

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