loss of valence electrons gain of negatively charged electrons name of the anion typically ends in...
TRANSCRIPT
Anion = (-) charge ion
gain of negatively charged electrons name of the anion typically ends in -ide
Ionic Compounds
compounds composed of cations and anions
electrically neutral
Held together by IONIC BOND› electrostatic forces
Chemical Formula and Formula Unit
Chemical Formula › indicates the number of atoms of each
element found in each molecule of that compound
Formula Unit = lowest whole-number ratio of ions in an ionic compound› Ionic compounds do not exist as individual
molecules
Ionic Bonding
All the electrons must be accounted for, and each atom will have a noble gas configuration (which is stable).
Ca P
Lets do an example by combining calcium and phosphorus:
ionic compounds
crystalline solids at room temperature arranged in repeating three-
dimensional patterns very stable structure high melting points
“Molecule”
a neutral group of atoms joined together by covalent bonds
there is no such thing as a molecule of sodium chloride or magnesium chloride
ionic compounds exist as collections of positively and negatively charged ions
Melting and Boiling points
Molecular compounds have relatively lower melting and boiling points than ionic compounds › gases or liquids at room temperature
Molecular Formula shows how many atoms of each element
a molecule contains› water molecule = two hydrogen atoms and
one oxygen atom molecular formula = H2O.
› carbon dioxide molecule = two oxygen atoms and one carbon atom molecular formula = CO2
Note:› If there is only one atom, the subscript 1 is
omitted
Molecular Formula
The molecular formula for ethane is C2H6
› one molecule of ethane contains two carbon atoms and six hydrogen atoms
reflects the actual number of atoms in each molecule› not necessarily lowest whole-number ratios
Octet Rule applies to molecules
electron sharing occurs so that atoms attain the electron configurations of noble gases
likely to form covalent bonds:› atoms of the nonmetals and metalloids › Groups 4A, 5A, 6A, and 7A
Halogens form single covalent bonds
pair of valence electrons not shared between atoms is called an unshared pair
Double bonds and Triple bonds
two shared pairs of electrons = double covalent bond
sharing three pairs of electrons = triple covalent bond.
polyatomic ion
tightly bound group of atoms that has a positive or negative charge and behaves as a unit