PO
4
3phosphate ion
C
2
H
3
O
2
acetate ion
HC
2
H
3
O
2
Acetic Acid
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Most bonds are somewhere in between ionic and covalent.
• There are 3 forms bonding atoms:
• Ionic —complete transfer of 1 or more electrons from one atom to another (one loses, the other gains)
• Covalent — some valence electrons shared between atoms
• _________ – holds atoms of a metal together

• A lot of chemicals have common names as well as the proper
IUPAC name.
• Chemicals that should always be named by common name and never named by the IUPAC method are:
• H
2
O water, not dihydrogen monoxide
• NH
3 ammonia, not nitrogen trihydride

CATION +
ANION --->
COMPOUND
+
-
A neutral compound requires equal number of + and - charges.

Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2 -3 -2 -1 0
Cd +2

Properties of Ionic Compounds
Forming NaCl from Na and Cl
2
• A metal atom can transfer an electron to a nonmetal.
• The resulting cation and anion are attracted to each other by electrostatic forces
.

NH
4
+
Cl ammonium chloride, NH
4
Cl

Ca 2+ + 2 F ---> CaF
2
Mg 2+ + N -3 ---->
Mg
3
N
2 magnesium nitride
Sn 4+ + O 2---->
SnO
2
Tin (IV) oxide calcium fluoride

Formulas of Ionic Compounds
Formulas of ionic compounds are determined from the charges on the ions
Na
 atoms
+
 ions
   
–
F :

Na + : F :

NaF
    sodium + fluorine sodium fluoride formula
Charge balance: 1+ 1= 0

Writing a Formula
Write the formula for the ionic compound that will form between Ba 2+ and Cl

.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl

Cl 
3. Write the number of ions needed as subscripts BaCl
2

Learning Check
Write the correct formula for the compounds containing the following ions:
1. Na + , S 2a) NaS
2. Al 3+ , Cl b) Na
2
S c) NaS
2 a) AlCl
3
3. Mg 2+ , N 3b) AlCl a) MgN b) Mg
2
N
3 c) Al
3
Cl c) Mg
3
N
2

1. Na + , S 2b) Na
2
S
2. Al 3+ , Cl a) AlCl
3
3. Mg 2+ , N 3c) Mg
3
N
2
Solution

Binary Ionic Compounds:
• 1. Cation first, then anion
• 2. Monatomic cation = name of the element
• Ca 2+ = calcium ion
• 3. Monatomic anion = root + -ide
• Cl

= chlor ide
• CaCl
2
= calcium chlor ide

Naming Binary Ionic Compounds

Examples:
NaCl
CaI
2
Al
2
O
3 sodium chloride calcium iodide aluminum oxide

Learning Check
Complete the names of the following binary compounds:
Na
3
N sodium ________________
KBr potassium ________________
Al
2
O
3
MgS aluminum ________________
_________________________

Transition Metals
Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion.
1+ or 2+ 2+ or 3+
Cu + , Cu 2+ Fe 2+ , Fe 3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

Names of Variable Ions
These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al
(You should already know the charges on these!)
Or another way to say it is: Transition metals and the metals in groups 4A and
5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl
CuCl
SnF
4
PbCl
2
Fe
2
S
3
3
(Fe 3+ )
(Cu + )
(Sn 4+ )
(Pb 2+ )
(Fe 3+ ) iron (III) chloride copper (I) chloride tin (IV) fluoride lead (II) chloride iron (III) sulfide

Examples of Older Names of Cations formed from Transition Metals
(you do not have to memorize these)

Learning Check
Complete the names of the following binary compounds with variable metal ions:
FeBr
CuCl
2 iron (_____) bromide copper (_____) chloride
SnO
2
Fe
2
O
3
Hg
2
S
___(_____ ) ______________
________________________
________________________

3
-
2
-

You can make additional polyatomic ions by adding a H + to the ion!
CO
3
-2
HCO
3
– is carbonate is hydrogen carbonate
H
2
PO
4
–
HSO
4
– is dihydrogen phosphate is hydrogen sulfate

Writing Formulas
• Write each ion, cation first. Don’t show charges in the final formula.
• Overall charge must equal zero .
• If charges cancel, just write symbols.
• If not, use subscripts to balance charges.
• Use parentheses to show more than one of a particular polyatomic ion .
• Use Roman numerals indicate the ion’s charge when needed (stock system)

Sodium Sulfate
Na + and SO
Na
2
SO
4
4
-2
Iron (III) hydroxide
Fe +3 and OH -
Fe(OH)
3
Ammonium carbonate
NH
4
+ and CO
3
–2
(NH
4
)
2
CO
3

Learning Check
1. aluminum nitrate a) AlNO
3 b) Al(NO)
3
2. copper(II) nitrate a) CuNO
3 b) Cu(NO
3. Iron (III) hydroxide
3
)
2 a) FeOH b) Fe
3
OH
4. Tin(IV) hydroxide a) Sn(OH)
4 b) Sn(OH)
2 c) Al(NO
3
)
3 c) Cu
2
(NO
3
) c) Fe(OH)
3 c) Sn
4
(OH)

Naming Ternary Compounds
 Contains at least 3 elements
 There MUST be at least one polyatomic ion
(it helps to circle the ions)
 Examples:
Na NO
3
Sodium nitrate
K
2
SO
4
Al (HCO
3
)
3
Potassium sulfate
Aluminum bicarbonate or
Aluminum hydrogen carbonate

Learning Check
Match each set with the correct name:
1.
Na
2
CO
3
MgSO
3
MgSO
4 a) magnesium sulfite b) magnesium sulfate c) sodium carbonate
2 .
Ca(HCO
3
)
2
CaCO
3
Ca
3
(PO
4
)
2 a) calcium carbonate b) calcium phosphate c) calcium bicarbonate

Name the following:
1. Na
2
O
2. CaCO
3
3. PbS
2
4. Sn
3
N
2
5. Cu
3
PO
4
6. HgF
2

Write the formula:
1. Copper (II) chlorate
2. Calcium nitride
3. Aluminum carbonate
4. Potassium bromide
5. Barium fluoride
6. Cesium hydroxide

CH
4 methane
CO
2
Carbon dioxide
All are formed from two or more nonmetals.
BCl
3 boron trichloride
Ionic compounds generally involve a metal and nonmetal
(NaCl)

Molecular (Covalent) Nomenclature for two non metals
• Prefix System (binary compounds)
1.
Less electronegative atom comes first.
2. Add prefixes to indicate # of atoms. Omit monoprefix on the FIRST element.
Monois OPTIONAL on the SECOND element (in this class, it’s NOT optional!).
3. Change the ending of the second element to -ide .

PREFIX monoditritetrapentahexaheptaoctanonadeca-
NUMBER
1
2
3
6
7
4
5
8
9
10

• CCl
4
• carbon tetrachloride
• N
2
O
• dinitrogen monoxide
• SF
6
• sulfur hexafluoride

• arsenic trichloride
• AsCl
3
• dinitrogen pentoxide
• N
2
O
5
• tetraphosphorus decoxide
• P
4
O
10

Learning Check
Fill in the blanks to complete the following names of covalent compounds.
CO carbon ______oxide
CO
2
PCl
3
CCl
4
N
2
O carbon _______________ phosphorus _______chloride carbon ________chloride
_____nitrogen _____oxide

1.
P
2
O
5
2.
Cl
2
O
7
3. Cl
2
Learning Check a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide a) chlorine b) dichlorine c) dichloride

Overall strategy for naming chemical compounds.

A flow chart for naming binary compounds.

Mixed Review
Name the following compounds:
1. CaO a) calcium oxide c) calcium (II) oxide b) calcium(I) oxide
2. SnCl
4 a) tin tetrachloride b) tin(II) chloride c) tin(IV) chloride
3. N
2
O
3 a) nitrogen oxide c) nitrogen trioxide b) dinitrogen trioxide

Solution
Name the following compounds:
1. CaO
2. SnCl
4 a) calcium oxide c) tin(IV) chloride
3.
N
2
O
3 b) Dinitrogen trioxide

1. Dinitrogen monoxide
2. Potassium sulfide
3. Copper (II) nitrate
4. Dichlorine heptoxide
5. Chromium (III) sulfate
6. Iron (III) sulfite
7. Calcium oxide
8. Barium carbonate
9. Iodine monochloride

1. BaI
2
2. P
4
S
3
3. Ca(OH)
2
4. FeCO
3
5. Na
2
Cr
2
O
7
6. I
2
O
5
7. Cu(ClO
3
)
2
8. CS
2
9. B
2
Cl
4

• Acids
• Compounds that form H + in water.
• Formulas usually begin with ‘H’.
• In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water)
• Ternary acids are ALL aqueous
• Examples:
• HCl
(aq)
– hydrochloric acid
• HNO
3
– nitric acid
• H
2
SO
4
– sulfuric acid

Acid Nomenclature Review
No Oxygen 
Anion
Ending Acid Name
-ide hydro (stem) ic acid
-ate (stem) ic acid w/Oxygen
-ite (stem) ous acid
An easy way to remember which goes with which…
“In the cafeteria, you ATE something IC ky”

ACIDS start with 'H'
2 elements 3 elements hydro- prefix
-ic ending no hydro prefix
-ate ending becomes
-ic ending
-ite ending becomes
-ous ending

• HBr
(aq)
• 2 elements, ide
• H
2
CO
3
• 3 elements, -ate
• H
2
SO
3
• 3 elements, -ite
 hydro bromic acid
 carbon ic acid
 sulfur ous acid

• hydrofluoric acid
• 2 elements 
H + F-
• sulfuric acid
• 3 elements, -ic
• nitrous acid

H + SO
4
2-
• 3 elements, -ous

H + NO
2
-

HF
(aq)

H
2
SO
4

HNO
2

• HI
(aq)
• HCl
• H
2
SO
4
• HNO
3
• HClO
3

• Hydrobromic acid
• Nitric acid
• Carbonic acid
• Phosphoric acid

Nomenclature Summary Flowchart

Now it’s Study Time
DONE