1. Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions

2. Monatomic Ions
Ionic compounds consist of a positive metal ion and a negative nonmetal ion combined in a proportion such that their charges add up to a net charge of zero.
NaCl – consists of one Na+ and one Cl-.
Monatomic ions consists of a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons.

3. Monatomic Ions - Cations
Cations tend to lose valence electrons. (1+ charge – lose 1 electron, 2+ charge – lose 2 electrons, etc. )
When the metals in Groups 1A, 2A, and 3A lose electrons, they form cations with positive charges equal to their group number.
The name of the cations of the Group 1A, 2A and 3A are the same as the name of the metal, followed by the word ion or cation.
Na+ is sodium ion, Ca2+ is calcium ion, Al3+ is aluminum ion.

4. Monatomic Ions - Anions
Nonmetals tend to gain electrons to form anions, so the charge of a nonmetallic ion is negative.
The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number.
Group 7A form anions with a 1- charge (7-8 = -1)
Anion names start with the stem of the element name and end in –ide.
Anion of fluorine is fluoride ion (F-), anion of chlorine is chloride ion (Cl-)

5. Ions of Transition Metals
Many of the transition metals (Group 1B – 8B) form more than one cation with different ionic charges.
Two methods are used to name these ions.
Stock System – a roman numeral in parentheses is placed after the name of the element to indicate the numerical value of the charge.
Fe2+ is iron(II) ion Fe3+ is iron(III) ion.
Classical – name of the element is used to form the root name for the element.
Fe2+ is ferrous ion Fe3+ is ferric ion

6. Symbols and Names of common Metal Ions
Cu +
Copper (I) ion
Cuprous ion
Cu 2+
Copper (II) ion
Cupric ion
Hg +
Mercury (I) ion
Mercurous ion
Hg 2+
Mercury (II) ion
Mercuric ion
Fe 2+
Iron (II) ion
Ferrous ion
Fe 3+
Iron (III) ion
Ferric ion
Cr 2+
Chromium (II) ion
Chromous ion
Cr 3+
Chromium (III) ion
Chromic ion
Mn 2+
Manganese (II) ion
Manganous ion
Mn 3+
Manganese (III) ion
Manganic ion
Co 2+
Cobalt (II) ion
Cobaltous ion
Co 3+
Cobalt (III) ion
Cobaltic ion
Pb 2+
Lead (II) ion
Plumbous ion
Pb 4+
Lead (IV) ion
Plumbic ion
Sn 2+
Tin (II) ion
Stannous ion
Sn 4+
Tin (IV) ion
Stannic ion
Cd 2+
Cadmium ion
Zn 2+
Zinc ion
Ag +
Silver ion

7. Polyatomic Ions Polyatomic Ions are composed of more than one atom.
Sulfate ions (SO4 2-) is composed of one sulfur atom and four oxygen atoms.
Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge.
The names of most polyatomic anions end in –ite or –ate.

8. Common Polyatomic Ions
Charge 1 +
NH4 +
Ammonium
Charge 1 ─
ClO ¯
Hypochlorite
OH ¯
Hydroxide
ClO2 ¯
Chlorite
CH3COO ¯
Acetate
ClO3 ¯
Chlorate
CN ¯
Cyanide
ClO4 ¯
Perchlorate
OCN ¯
Cyanate
lO2 ¯
Iodite
HSO3 ¯
Bisulfite
lO3 ¯
Iodate
HSO4 ¯
Bisulfate
lO4 ¯
Periodate
HCO3 ¯
Bicarbonate
NO2 ¯
Nitrite
BrO3 ¯
Bromate
NO3 ¯
Nitrate
MnO4 ¯
Permanganate

9. Common Polyatomic Ions
Charge 2 ─
CO3 2−
Carbonate
CrO4 2−
Chromate
SO3 2−
Sulfite
Cr2O7 2−
Dichromate
SO4 2−
Sulfate
C2O4 2−
Oxalate
S2O3 2−
Thiosulfate
SiO3 2−
Silicate
O2 2−
Peroxide
Charge 3 ─
PO3 3−
Phosphite
AsO3 3−
Arsenite
PO4 3−
Phosphate
AsO4 3−
Arsenate
BO3 3−
Borate
Charge 4 ─
P2O7 4−
Pyrophosphate

10. Section 9.2 Naming Ionic Compounds

11. Naming Binary Ionic Compounds
A binary compound is composed of two elements and can be either ionic or molecular (covalent).
To name any binary ionic compound, place the cation name first, followed by the anion name.
Cs2O is cesium oxide NaBr is sodium bromide
Cu2O is copper(I) oxide CuO is copper(II) oxide

12. Writing Formulas Binary Ionic Compounds
Write the symbol of the cation and then the anion. Add whatever subscripts are needed to balance the charges.
The positive charge of the cation must balance the negative charge of the anion so that the net ionic charge of the formula is zero.
K+ + Cl-  KCl
Ca2+ + Br -  CaBr2
Fe3+ + O2-  Fe2O3
Use the crisscross method – the numerical value of the charge of each ion is crossed over and becomes the subscript for the other ion.

13. Writing Formulas Polyatomic Ionic Compounds
An –ate or –ite ending on the name of a compound indicates that the compound contains a polyatomic anion that includes oxygen.
Write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges.
Ca2+ + NO3-  Ca(NO3)2
Sr2+ + SO32-  SrSO3
Li+ + CO32-  Li2CO3
Use the crisscross method – the numerical value of the charge of each ion is crossed over and becomes the subscript for the other ion.

14. Naming Polyatomic Ionic Compounds
First recognize that the compound contains a polyatomic ion.
State the cation first and then the anion
NaClO
sodium hypochlorite
(NH4)2C2O4
ammonium oxalate
Li2CO3
lithium carbonate

15. Naming and Writing Formulas for
Section 9.3
Naming and Writing Formulas for
Molecular Compounds

16. Naming Molecular Compounds
Binary ionic compounds are composed of the ions of two elements, a metal and a nonmetal.
Binary molecular compounds are composed of two elements, two nonmetals and they are not ions.
Binary molecular compounds are composed of molecules, not ions, so ionic charges cannot be used to write formulas or to name them.
In addition, when two nonmetallic elements combine, they often do so in more than one way. (CO, CO2)
Prefixes in the names of binary molecular compounds help distinguish compounds containing different amounts of the same two elements.

17. Naming Molecular Compounds
The prefix in the name of a binary molecular compound tells how many atoms of each element are present in each molecule of the compound.
Prefix
Number
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10

18. Naming Molecular Compounds
The names of all binary molecular compounds end in –ide.
CO is carbon monoxide
CO2 is carbon dioxide
If just one atom of the first element is in the formula, omit the prefix mono-
Name the elements in order listed in the formula
Use prefixed to indicate the number of each kind of atom
The suffix of the name of the second element is –ide.
N2O is dinitrogen monoxide
SF6 is sulfur hexafluoride.

19. Writing Formulas Molecular Compounds
Use the prefixes in the name to tell you the subscript of each element in the formula.
Then write the correct symbols for the two elements with the appropriate subscripts.
Dinitrogen tetraoxide
N2O4
Diphosphorus trioxide
P2O3

20. Naming and Writing Formulas for
Section 9.4
Naming and Writing Formulas for
Acids and Bases

21. Naming Acids
Acid is a compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water.
When naming acids, the acid consists of an anion combined with as many hydrogen ions as needed to make the molecule electrically neutral.
The general chemical formulas of acids is HnX.
X is a monatomic or polyatomic anion
n is a subscript indication the number of hydrogen ions combined with the anion.

22. Naming Acids
Three rules are used to name acids. The name depends on the name of the anion and its suffix (-ide, -ite, -ate)
a. When the name of the anion ends in –ide, the acid name begins with the prefix hydro-.
b. The stem of the anion has the suffix –ic and is followed by the word acid.
H Cl  HCl
Hydrogen ion chloride ion hydrochloric acid
H S  H2S
Hydrogen ion sulfide ion hydrosulfuric acid

23. Naming Acids
Three rules are used to name acids. The name depends on the name of the anion and its suffix (-ide, -ite, -ate)
a. When the anion name ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by the word acid
H SO  H2SO3
Hydrogen ion sulfite ion sulfurous acid
H CIO  HCIO2
Hydrogen ion chlorite ion chlorous acid

24. Naming Acids
Three rules are used to name acids. The name depends on the name of the anion and its suffix (-ide, -ite, -ate)
a. When the anion name end in –ate, the acid name is the stem of the anion with the suffix –ic followed by the word acid.
H NO  HNO3
Hydrogen ion nitrate ion nitric acid
H SO  H2SO4
Hydrogen ion sulfate ion sulfuric acid

25. Writing Formulas for Acids
Use the rules for writing the names of acids in reverse to write the formula for acids.
Hydrobromic acid
Hydro indicates the bromide ion
HBr
Phosphorous acid
-ous indicates the phosphite ion
H3PO3
phosphoric acid
-ic and beginning with the anion name indicates the phosphate ion
H3PO4

26. Bases
A base is an ionic compound that produced hydroxide ions (OH-) when dissolved in water.
Bases are named the same way as other ionic compounds – the name of the cation is followed by the name of the anion.
NaOH is sodium hydroxide
To write the formulas for bases, write the symbol for the cation followed by the formula for the hydroxide ion. (then use the crisscross method to write the formula as you do as you do for any ionic compound)
Aluminum hydroxide – Al3+ + OH-  Al(OH)3
Ammonium hydroxide – NH4+ + OH-  NH4OH