Naming Compounds
Hypochlorous Acid
Overview
• Determine names from formulas.
• Determine formulas from names.
How do we know...
• it’s formula is HClO. Why does it have that
name?
• quantities of atoms in hypochlorous acid?
What is a chemical
name?...
•
Common names include - laughing gas (N2O),
quicksilver (Hg), lime (CaO), and saltpeter
(NaNO3).
•
Chemical names are those agreed upon by
IUPAC (International Union of Pure and Applied
Chemistry).
• We can determine many of their
names by using standard
conventions.
Naming Compounds
Ionic
Covalent
Acid
Naming Compounds
Ionic
Covalent
Acid
Disclaimer: What you will learn is useful, but will not apply
to the over 11 million possible compounds.
Naming Compounds
Ionic
Name
the anion
Name
the
cation
Acid
Covalent
Determine
name based on
ending
Put
Elements
in order
add “ide”
use
greek
prefixes
Naming Compounds
Ionic
Name
the anion
Name
the
cation
First we need to
determine the
bond...
Acid
Covalent
Determine
name based on
ending
Put
Elements
in order
add “ide”
use
greek
prefixes
How do we tell ionic,
covalent, and acids apart?
• Ionic has a metal and a non-metal. They can
also be formed with polyatomic ions acting
as cation(s) and anion(s).
• Covalent has two or more metals.
• Acids begin with H and are aqueous
solutions.
Ionic, Covalent, (or
Acid)
• AlBr =
• NaNO =
• CO =
• KHSO =
• H SO =
3
3
2
4
2
4
Ionic, Covalent, (or
Acid)
• AlBr = ionic, metal and non-metal.
• NaNO = ionic, note the nitrate is a
3
3
polyatomic ion.
• CO = covalent, both non-metals.
• KHSO = ionic, metal and non-metal(s).
• H SO = acid, begins with H. Why not
2
4
2
4
covalent?
Molecular Compounds
1. Identify metal(s) and non-metal(s).
2. The name of the element farthest to the left in the
periodic table is written first. If both elements are in
the same group, the lower one is written first.
3. The name of the last element is given with an “-ide”
ending.
4. Place the prefix that applies to the number of atoms.
Prefixes
Number
1
2
3
4
5
6
7
8
9
10
Prefix
None (or mon-)
ditritetrapentahexaheptaoctanonadeca-
Example
chloride
dichloride
trichloride
tetrachloride
pentachloride
hexachloride
heptachloride
octachloride
nonachloride
decachloride
Molecular Compounds
1. Identify metal(s) and non-metal(s). Note: there should be only nonmetals.
2. The name of the element farthest to the left in the
periodic table is written first. If both elements are in
the same group, the lower one is written first. WHY?
•1. There are occasional exceptions to this rule (most commonly oxygen except when
written with fluorine).
3. The name of the last element is given with an “-ide”
ending.
4. Place the prefix that applies to the number of atoms.
Practice
• CF
4
=
1.
Identify metal(s) and non-metal(s).
2.
The name of the element farthest to the left in the periodic table
is written first. If both elements are in the same group, the lower
one is written first.
3.
The name of the last element is given with an “-ide” ending.
4.
Place the prefix that applies to the number of atoms.
Practice
• CF
4
= Carbon Tetrachloride.
Practice
• NF
2 2
=
1.
Identify metal(s) and non-metal(s).
2.
The name of the element farthest to the left in the periodic table
is written first. If both elements are in the same group, the lower
one is written first.
3.
The name of the last element is given with an “-ide” ending.
4.
Place the prefix that applies to the number of atoms.
Practice
• NF
2 2
= dinitrogen difluoride
Practice
• PCl
5
=
Practice
• PCl
5
= Phosphorus Pentachloride.
Practice
• NO
2
5
=
Practice
• N O = dinitrogen pentoxide
• Note: you drop the a in “penta”. You can
2
5
drop the last vowel of the prefix always
before “oxide.”
Examples of Molecular
Compounds
• Cl O = dichlorine monoxide
• NF = nitrogen trifluoride
• N O = dinitrogen tetrafluoride
• P S = tetraphosphorus decasulfide
2
3
2
4
4 10
Practice Molecular
Compounds
• Cl O = dichlorine monoxide
• NF = nitrogen trifluoride
• N O = dinitrogen tetrafluoride
• P S = tetraphosphorus decasulfide
2
3
2
4
4 10
Practice Molecular
Compounds
• Cl O =
• NF =
• NO =
• PS =
2
3
2
4
4 10
Molecular Practice
1. SO2 =
2. PCl5 =
3. N2O3 =
4. SF6 =
5. IF5 =
6. XeO3 =
Molecular Practice
1. SO2 = Sulfur Dioxide
2. PCl5 = Phosphorus Pentachloride
3. N2O3 = Dinitrogen Trioxide
4. SF6 = Sulfur Hexafluoride
5. IF5 = Iodine Pentafluoride
6. XeO3 = Xenon Trioxide
Homework
• Review your notes and the section on
covalent compounds.
• Complete the practice sheet.
• Preview the section on ionic compounds.
Ionic Compounds
1. Name the cation.
2. Name the anion.
3. Name the compound.
Ionic Compounds - Cation
1. Name the cation.
1.1.Cations formed from metals have the
same name as the metal. e.g. Sodium
Chloride.
2. Name the anion.
3. Name the compound.
Ionic Compounds - Cation
1. Name the cation.
1.1.Cations formed from metals have the
same name as the metal. e.g. Sodium
Chloride.
1.2.If a metal can form ions with dif’t
charges, specify the charge with a roman
numeral. e.g. Iron (11) Chloride. Note:
sometimes you’ll see a classical name - ferric chloride.
2. Name the anion.
3. Name the compound.
Ionic Compounds - Cation
1. Name the cation.
1.1.Cations formed from metals have the same name
as the metal. e.g. Sodium Chloride.
1.2.If a metal can form ions with dif’t charges,
specify the charge with a roman numeral. e.g. Iron
(11) Chloride. Note: sometimes you’ll see a classical name - ferric chloride.
1.3.Cations formed from nonmetals have names
ending in “-ium”. These are uncommon.
Common(nest) examples are Hydronium ion
(H30+) and Ammonium ion (NH4+).
2. Name the anion.
3. Name the compound.
Ionic Compounds - Anion
1. Name the cation.
2. Name the anion.
2.1.Monatomic ions have names formed by
replacing the end of the element with an
“-ide”. e.g. Lithium Bromide (LiBr).
Note: some simple polyatomic ions also
end in “-ide” e.g. hydroxide (OH-).
3. Name the compound.
Ionic Compounds - Anion
1. Name the cation.
2. Name the anion.
2.1.Monatomic ions have names formed by replacing
the end of the element with an “-ide”. e.g. Lithium
Bromide (LiBr). Note: some simple polyatomic
ions also end in “-ide” e.g. hydroxide (OH-).
2.2.Most polyatomic ions contain oxygen and end in
“-ate” to denote the most common form. The
ending “-ite” is used for ions that have the same
charge but one less oxygen. e.g. Sulfate (SO42-) and
sulfite (SO32-). These are referred to as oxyanions.
3. Name the compound.
Ionic Compounds - Anion
1. Name the cation.
2. Name the anion.
2.1.Monatomic ions have names formed by replacing the end of
the element with an “-ide”. e.g. Lithium Bromide (LiBr). Note:
some simple polyatomic ions also end in “-ide” e.g. hydroxide
(OH-).
2.2.Most polyatomic ions contain oxygen and end in “-ate” to
denote the most common form. The ending “-ite” is used for
ions that have the same charge but one less oxygen. e.g.
Sulfate (SO42-) and sulfite (SO32-). These are referred to as
oxyanions.
2.3.When H+ is added on the front of an oxyanion, write hydrogen
before the name. e.g. hydrogen carbonate ion (HCO3-) as
opposed to carbonate (CO32-). Note: prefixes apply to the H.
3. Name the compound.
Ionic Compounds - Putting
it together...
1. Name the cation.
2. Name the anion.
3. Name the compound. Simply put the
names of the ions together with the
cation first. e.g. Calcium Chloride (CaCl2)
Ionic Practice
• LiI =
Ionic Practice
• LiI = Lithium Iodide
Ionic Practice
• CaBr
2
=
Ionic Practice
• CaBr
2
= Calcium Bromide
Ionic Practice
• Ag O=
2
Ionic Practice
• Ag O= Silver Oxide
2
Ionic Practice
• CuCl =
Ionic Practice
• CuCl = Copper (I) Chloride
Ionic Practice
• FeCl
2
= Iron (II) Chloride
Ionic Practice
• FeCl
2
=
Ionic Practice
• FeCl
2
= Iron (II) Chloride
More Ionic Practice
• Ba(OH) =
• K2 O =
• Cr O =
• KHSO =
2
S
4
2
3
4
More Ionic Practice
• Ba(OH) = Barium Hydroxide
• K2 O = Potassium Sulfate
• Cr O = Chromium (III) Oxide
• KHSO = Potassium Hydrogen Sulfate
2
S
4
2
3
4
Acids
1. Acids based on anions whose name ends in “-ide”
a. “-ide” =
“hydro-” + ______ + “-ic” + “acid”
Acid Practice
• HCl =
• H and Cl
• Note: contains the chloride ion.
• “hydro”+________+”ic”+”acid”
+
-
Acid Practice
• HCl = Hydrochloric Acid
Acid Practice
• HS=
• H and S
• Note: contains the sulfide ion.
2
+
2-
Acid Practice
• H S = Hydrosulfuric acid
2
Acids
1. Acids based on anions whose name ends in “-ide”
a. “-ide”
“hydro-” + “-ic” + “acid”
2. Acids based on anions whose name ends in “-ate” or
“-ite”
a. “-ate”
“-ic” + “acid”
b. “-ite”
“-ous” + “acid”
c. If there is a “per-” or “hypo-”, these prefixes are
retained.
Acid Practice
• H PO =
• H and PO
• Note: contains the phosphate ion
• _____ + “ic” + “acid”
3
4
+
4
3-
Acid Practice
• H PO
3
4
= Phosphoric Acid
Acid Practice
• H PO =
• H and PO
• Note: contains the phosphite ion
• _____ + “ous” + “acid”
3
3
+
3
3-
Acid Practice
• H PO
3
3
= Phosphorous Acid
Acid Practice
• HClO =
• H and ClO
• Note: contains the hypochlorite ion
• _____ + “ous” + “acid”
+
-
Acid Practice
• HClO = Hypochlorous Acid
Assorted Acid Practice
• HI =
• HBr =
• HNO =
• HNO =
• H CO =
3
2
2
3
Assorted Acid Practice
• HI = Iodic Acid
• HBr = Bromic Acid
• HNO = Nitric Acid
• HNO = Nitrous Acid
• H CO = Carbonic Acid
3
2
2
3
Note about Acids
• The previous compounds are H O
2
solutions.
• When the compounds are not in water,
they are named “hydrogen” + stem name of
the nonmetal + “-ide”.
• e.g. Hydrogen Sulfide, H S
2
Homework
• Complete the practice sheet.
• Be sure to have read pages 108-120.