Transcript Chemical Names and Formulas

Naming Chemical
Compounds
Beating The System
 The system of naming that is used worldwide today is called the IUPAC system.
 IUPAC is an acronym for International
Union of Pure and Applied Chemistry.
 The names and formulas used by IUPAC
are universal throughout the world – much
like the scientific names used in biology –
you Homo sapiens!
 This system helps to eliminate language
barriers and problems of communication.
Names for
Binary Ionic Compounds
 A binary ionic compound is an ionic compound that is made of
just two elements.
 The elements involved with binary ionic compounds have formed
ions – one positive and one negative.
 These compounds have a first and last name just like you. The
positive ion is always placed first in the formula and is written as
the first name. The negative ion is second in both instances.
 The general form of the name of a binary ionic compound is…
Metal nonmetide
 Notice that the first name stays the same as on the periodic table
while the second name gets shortened and ends in “ide”.
 Examples:
 K2S
NaCl
Mg2N3
 Potassium sulfide Sodium chloride
Magnesium nitride
Ionic Compounds with
Transition Metals
 There are several metals on the periodic table that are
“shifty”. They are capable of having more than one ionic
charge. Of course, being metals, this charge is positive.
 These metals are:




Copper – Cu – I & II
Iron – Fe – II & III
Lead – Pb – II & IV
Tin – Sn – II & IV
 When naming a compound, these metals must be
identified not only with their name but with their charge.
 The formulas of compounds that include these “shifty”
metals do not have any Roman numerals in them.
Naming Ionic Compounds
with Transition Metals
 These, too, have a first and last name.
 The first name is the name of the metal. This
name is followed by a Roman numeral in
brackets – just to show what form of the “shifty”
metal it is.
 The second name is the name of the nonmetal –
shortened with the “IDE” ending.
 Example:
 Cu3N
SnO2
 Copper (I) nitride
Tin (IV) oxide
Polyatomic Ionic Compounds
 A polyatomic ion is a
cluster of atoms that travel
together as a single unit
that carries an overall
charge.
 Many of the polyatomic ions
are negatively charged so
when they are in an ionic
compound they replace the
nonmetal.
 The polyatomic ions you
need to know are:
 Name (formula) charge








Hydroxide (OH)1Nitrate (NO3)1Chlorate (ClO3)1Bicarbonate (HCO3)1Carbonate (CO3)2Sulfate (SO4)2Phosphate (PO4)3Ammonium (NH4)1+
Naming Polyatomic
Ionic Compounds
 Polyatomic compounds also get two names just like we do.
 The first name will be the name of the positive ion –
usually a metal – no changes are made to this first name.
 The second name will be the name of the polyatomic
ion as it is – there are no changes made to the name of
polyatomic ions when they are used in a compound.
 The second name – if the second part of the compound is
just a nonmetal (not a polyatomic) – will be the shortened
name of the nonmetal with the “IDE” ending.
 Examples:
 CaSO4
 Calcium sulfate
K3PO4
NH4Cl
Potassium phosphate
Ammonium chloride
Hydrated Salts
 A hydrated salt is an ionic compound that contains
molecules of water within its structure.
 These compounds are named by using the name of the ionic
compound (the salt) followed by the term “hydrate” – which
means water.
 To indicate the amount of water being held within the
structure, we use a prefix in front of the “hydrate” part of the
name.
 These prefixes are:
Mono – 1
Di – 2
Tri – 3
Tetra – 4
Penta – 5
Hexa – 6
Hepta – 7
Octa – 8
Nona – 9
Deca – 10
 Examples:
 CuSO4·5H2O
MgSO4·7H2O
 Copper (II) sulfate pentahydrate
Magnesium sulfate heptahydrate
Binary Covalent Compounds
 Binary covalent compounds are those
which are made of two nonmetals bonded
together because they are sharing
electrons. (Two bullies are sharing the
toys!)
 Covalent compounds do not form ions so
you can’t go “positive ion first & negative
ion second”. This means you have to name
them differently than the ionic compounds.
Naming Binary
Covalent Compounds
 The covalent compounds use only nonmetals. They still have
two names just like us.
 Prefixes are used to show how much of each nonmetal is used to
make the compound.
 The prefixes used are:
Mono – 1
Di – 2
Tri – 3
Tetra – 4
Penta – 5
Hexa – 6
Hepta – 7
Octa – 8
Nona - 9
Deca – 10
 The first name is the name of the first nonmetal used. It will
have a prefix only if there is more than one of it used. No prefix
needed if there is only one of the first nonmetal.
 The second name is the name of the second nonmetal used – it
will be shortened with an “IDE” ending and will have a prefix
(even if there is only one of it). The second nonmetal always gets
a prefix.
 Examples:


N2O
Dinitrogen monoxide
CCl4
Carbon tetrachloride
Binary Acids
 A binary acid is an acid that contains
hydrogen and one other element.
 The general formula for any binary acid is:
Hydro-nonmetal-ic acid
 Examples:
 HCl (aq)
 Hydrochloric acid
HBr (aq)
Hydrobromic acid
Ternary Acids
 A ternary acid is an acid that contains hydrogen
and a polyatomic ion.
 The name of the polyatomic ion used in the acid
will help us form the name of the acid.
 If the polyatomic ion ends in “ate”, the ending of the
acid’s name will become “ic”. (I think of the saying “I
ate something icky”, to help me keep these straight.)
 If the polyatomic ends in “ite”, the ending of the acid’s
name will become “ous”.
 Examples:
 HNO3 (aq)
 Nitric acid
HNO2 (aq)
Nitrous acid
H2SO4 (aq)
Sulfuric acid
Try Naming These Examples












Li2O
FeCl3
Al2(CO3)3
N2O3
FeCl2·4H2O
HF (aq)
PbS2
NaHCO3
H3PO4 (aq)
MgCl2·10H2O
H2SO3 (aq)
S2Br4












Lithium oxide
Iron (III) chloride
Aluminum carbonate
Dinitrogen trioxide
Iron (II) chloride tetrahydrate
Hydrofluoric acid
Lead (IV) sulfide
Sodium bicarbonate
Phosphoric acid
Magnesium chloride decahydrate
Sulfurous acid
Disulfur tetrabromide
THE END!