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Inorganic Nomenclature
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Metals: Form positive ions.
Non-metals: Form negative ions. (H is the exception).
• Anion: negatively charged ion (Cl-, O2-, NO3-).
•Cation positively charged ion (K+, Al3+, NH4+).
•Monatomic: only one atom (Ne, Na+, I-).
•Diatomic: two atoms (O2, NaCl, I2, LiBr).
•Triatomic: three atoms (K2S, O3, H2O).
•Polyatomic: many atoms. (Poly means more than one). (CH4, C2H6O, NaCl)
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a) Naming Monatomic ions
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monatomic metal ions: Place the word ion after the name of the
metal.
eg. Potassium metal (K) forms the potassium ion (K+).
(monatomic metal ions will have a charge)
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*
*
*
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monatomic metal ions with more than one possible
combining #:
place the roman numeral charge value in brackets between
the metal name and the word ion.
eg. Fe3+ = Iron (III) ion,
Fe2+ = Iron (II) ion,
Cu3+ = Copper (III) ion.
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* Change the ending of the nonmetal to “ide”.
negative charge.)
(means
Element
name
Symbol
Ion name
Ion symbol
Fluorine
F
Fluoride
F-
Chlorine
Cl
Chloride
Cl-
Bromine
Br
Bromide
Br-
Iodine
I
Iodide
I-
Oxygen
O
Oxide
O2-
Sulphur
S
Sulphide
S2-
Selenium
Se
Selenide
Se2-
Nitrogen
N
Nitride
N3-
Phosphorus
P
Phosphide
P3-
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* Polyatomic ions are compounds that carry a charge.
Carbonate =
CO32-
Nitrate = NO3- Phosphate =
PO43-
Hydroxide =
OH-
Sulphate =
SO42-
Permanganate
= MnO4-
Acetate =
CH3COO-
Dichromate =
Cr2O72-
Ammonium =
NH4+
Chromate =
CrO42-
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Polyatomic Ion Names
Symbol
Ammonium
NH41+
Nitrate
NO31-
Nitrite
NO21-
Sulfate
SO42-
Sulfite
SO32-
Bisulfate
Carbonate
Bicarbonate
HSO41CO32HCO31-
Hydroxide
OH1-
Phosphate
PO43-
Chlorate
ClO31-
Chlorite
ClO21-
Permanganate
MnO41-
Chromate
CrO42-
Dichromate
Cr2O72-
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An Ionic Compound is a compound made of ions.
The 3 Formula Rules:
1. Put down the symbols of the ions.
Add brackets around any complex ion.
Write the positive (metallic) ion first.
e.g. Ca Cl
or Ca(OH)
2.
Put combining numbers above each symbol.
e.g. Ca 2+ Cl 1- or
Ca 2+ (OH) 1-
3. cross
out the positive and negative signs
criss-cross the combining numbers and use them as subscripts.
eg. Ca+2 + Cl-1  Ca1Cl2 = CaCl2 or
Ca(OH)2
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*If the subscript is “one”, you don’t need to write it.
(Na1Cl1 = NaCl)
*You must reduce subscripts if possible. Is there a
number that will divide evenly into both subscripts?
(i.e. Mg2O2 = MgO)
*Subscripts inside brackets of complex ions must
NOT be changed
*eg. Ca 2+ + NO3 1-  Ca(NO3)2
*If the subscript outside brackets is one, don’t write
the brackets
*eg. Na(OH)1  NaOH
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Lead (IV) Oxide: Pb+4 O-2  Pb2O4 = PbO2
Lead (II) Oxide: Pb+2O-2  Pb2O2 = PbO
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1. magnesium and oxygen__
Mg2O2  MgO
2. potassium and sulphate___________
K2SO4
3. hydrogen and fluorine___________
HF
4. calcium and hydrogen____________
CaH2
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A. Binary Compounds / Only two elements /a metal and a non-metal
To name: a) Name the metal first without changing its name
b) Name the non-metal second and change its ending to
ide
E.g. BeBr2 = Beryllium bromide
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Sodium and Bromine ________________
__________________
Potassium and Oxygen ______________
 ______________________
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Sodium and Bromine  ____________
NaBr
__Sodium Bromide___________
Potassium and Oxygen __________
K2O
 __Potassium Oxide___
-Some elements can have multiple charges/comb. #s
-Use Roman numerals to specify which ion it is:
Eg
Fe(II) = Fe 2+
Look at the periodic table
Fe(III) = Fe 3+ see more than one comb cap
To name: a) find combining # by reverse criss-cross
b) change combining # to roman numeral, put after metal name
*Only metals can form more than one possible type of ion*
E.g. FeCl2 = Fe 2+ and Cl1- = _Iron (II) Chloride_____________________
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Iron (II) and Oxygen  _________
FeO
 __Iron (II) Oxide___
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Copper (I) and Bromine  ______
CuBr
 _Copper (I) Bromide
To name: Refer to your Periodic Table of Common Ions
Put:
1. positive ion first.
2. negative ion second.
E.g. Ba 2+ + SO42- = BaSO4 = Barium sulphate
E.g. Ba 2+ + PO43- = Ba3(PO4)2 = Barium phosphate
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Potassium and Bicarbonate  _________
KHCO3__
 Potassium Bicarbonate _
Magnesium and Nitrate  _______
Mg(NO3)2__
 __Magnesium Nitrate
* Class work: p. 71 – 72
* #4. a – o
* #5. a – o
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Crystals of ionic compounds often have water “stuck” to them.
eg. when Copper (II) Sulphate is crystallized from a water solution,
the resulting crystals have the formula:
CuSO4 · 5H2O
5 water molecules are attached to every CuSO4
the waters attached are called “Hydrates”
prefixes are used to tell the number of Hydrates attached
Prefix Used
# of water molecules
mono
1
di
2
tri
3
tetra
4
penta
5
hexa
6
hepta
7
octa
8
nona
9
deca
10
compound name + prefix + “hydrate”
Hydrate name =
eg. name of CuSO4 · 5H2O
Ca(NO3)2 · 4H2O
= “copper (II) sulfate pentahydrate”
=
“calcium nitrate tetrahydrate”
Homework: p. 73
#6. a,c,e,g,i
#7. a,c,e,
*
* usually are covalently bonded molecules
* composed of two different types of atoms
* it is assumed one particle is cation-like and the other is anionlike
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1.
Use prefix system (mono, di, tri, …)
2. Cation-like element written 1st, anion-like
element written 2nd
3. Ending of name changed to “ide”
eg. CO = Carbon monoxide.
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4. Place prefix, according to the number of that atom within the
molecule, in front of the elements’ name
So P2S3 is written: “Diphosphorus trisulphide”
****exception: if only one atom in cationic spot, then do not place
the prefix mono in front of the elemental name.
eg. NO2 = Nitrogen dioxide, not mononitrogen dioxide.
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*
NCl3 =
Nitrogen trichloride.
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P4O6 =
Tetraphosphorus hexaoxide.
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S2F2 =
Disulphur difluoride.
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NI3 =
Nitrogen triiodide.
*
ICl =
Iodine monochloride.
* Homework p. 74 #8 a,c,e,g
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#9 a,c,e,g,i
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An acid is a compound starting with an H (hydrogen), and has a pH < 7.
Most acids contain: oxygen, hydrogen a non-metal.
When dissolved in water, an acid breaks apart:
acid
“anion”
eg:
HNO2
acid
+
water
→
NO2anion
+
+ H+
H+
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ACID
ANION
HF
Hydrofluoric acid
HCl
Hydrochloric acid
HBr
Hydrobromic acid
HI
Hydroiodic acid
HNO2 Nitrous acid
NO2- Nitrite ion
HNO3 Nitric acid
NO3- Nitrate ion
H3PO4 Phosphoric acid
PO43- Phosphate ion
H2SO3 Sulphrous acid
SO32- Sulphite ion
H2SO4 Sulphuric acid
SO42- Sulphate ion
HClO Hypochlorous acid
ClO- Hypochlorite ion
HClO2 Chlorous acid
ClO2- Chlorite ion
HClO3 Chloric acid
ClO3- Chlorate ion
HClO4 Perchloric acid
ClO4- Perchlorate ion