Unit 4
Nomenclature
What’s Coming??
 Nomenclature
 How we name stuff
 Common ions
Nomenclature
 Common Names
 Sugar
 Epsom salts
 Gypsum
 Laughing gas
 TOO MANY CHEMICALS!
 The Naming System
(IUPAC)
 Tells us about the
composition
 Easy to construct the
chemical formula
 Inorganic vs. Organic
Making Ions
 Ion charges are based off of the
valence electrons
 Metals LOSE electrons
 They become +
 Called cations
 Non-metals GAIN electrons
 They become –
 Called anions
 Electrons are lost or gained to obtain
an octet
 Octet = 8 in the valence shell
 Transition metals are goofy
Molecular Formulas
 The formula that
indicates the specific
ratio of the different
atoms
 Tells us how many of
each atom we need to
have a specific
compound
Empirical Formulas
ALL ABOUT THE RATIO: LOWEST common denominator
Law of Definite Proportions
 A given compound ALWAYS displays EXACTLY the same
ratio/proportion of elements
 H2O
 CO2
 C6H12O6
Naming Binary Compounds
 Binary Compounds
 Composed of 2 elements
 Compounds contain either
 Metal and Non-metal – ionic compound
 2 Non-metals
 Three types of binary compounds
 Representative Ionic – The metal forms only 1 type of cation and is a
representative metal
 Transition Ionic– The metal forms more than 1 type of cation and is a
transition metal
 Covalent– Two non-metals are joined together by a sharing of electrons
Rules for Representative Ionic
 The cation is named
first, the anion is
named second
 A cation takes its
name from the name
of the element.
 An anion is named by
taking the root of the
element name and
adding –ide to the end
of the word.
Representative Ionic
 Name the following compounds and indicate which ions
and charges are present. Be sure to label each ion type.
 CsF
 AlCl3
 MgI2
 CaO
 KBr
Rules for Transition Ionic
 Transition metals can have multiple charges…hence
TRANSITION!
 Follow the same rules as Rep. Ionic but….
 You must indicate the charge of the cation
 Use roman numerals and parentheses
 Fe+2 is iron (II)…
 Finding the cation charge can be difficult
 Find the anion charge first and balance using the given ratios
Transition Ionic
 Provide the names for the following compounds. Be sure
to indicate ion charge and to use both naming systems.
 CuCl2
 HgO
 Fe2O3
 MnO2
 PbCl4
Rules for Covalent
 The first element in
the formula is
named first and the
full element name is
used.
 The second element
is named as though
it were an anion.
 Prefixes are used to
denote the number
of atoms present
(see table).
 The prefix “mono” is
never used for the
first element, it is
assumed.
 Latin Pre-fixes
 Mono = 1
 Di = 2
 Tri = 3
 Tetra = 4
 Penta = 5
 Hexa = 6
 Hepta = 7
 Octa = 8
Covalent
 Name the following compounds.
 BF3
 NO
 N2O5
Polyatomic Ions
 Polyatomic ions – ions made of 2 or more atoms
 These ions are assigned special names which must be
looked up or memorized.
 I will provide you with a chart that you may use for your
assessments.
 These ions are named using similar rules to ionic
compounds.
Polyatomic Ions
 Name the following compounds. Indicate the charge on
each of the ions.
 Na2CO3
 CsClO4
 CuSO4
Rules for Naming Acids
 If the anion does not
contain oxygen, the acid is
named with the prefix
“hydro” and the suffix “ic”
is attached to the root
name for the element.
 When the anion contains
oxygen, the name is taken
from polyatomic anion with
a suffix of “ic” or “ous”.
 When the anion ends in
“ate”, the suffix “ic” is
used.
 When the anion ends in
“ite”, the suffix “ous” is
used.
Acids
 Name the following acids. Indicate how many hydronium
(H+) ions can be produced.
 HCl
 H2SO4
 H2SO3
 H3PO4
 HF
Nomenclature Etc. Quiz
1) BF3
2) HClO4
3) MgBr2
4) Co2O3
5) Nickel (III) Sulfide
6) Barium Phosphide
7) Phosphorus tetroxide
8) Manganese (IV)
Phosphate
Provide the #p+, #n0, valence
e-, core e- for the following
elements in the neutral state:
9) Si - 30
10) Se - 74
11) C - 14
12) W - 190