Pav 2013
Chapter 7: Ionic Bonding
Section 7.1 Ions (pg.187-193)
1. Determine the number of valence electrons of the representative elements using a periodic table
2. Describe the formation of a cation as it relates to the Octet Rule.
3. Describe the formation of an anion as it relates to the Octet Rule.
Section 7.2 Ionic Bonds and Ionic Compounds (pg. 194-199)
1. Describe the formation of ionic bonds through electron transfer
2. Interpret the chemical formula of a formula unit.
3. Describe the structure and properties of ionic compounds.
Section 7.3 Bonding in Metals (pg. 201-203)
1.
2.
3.
4.
Describe the nature of a metallic bond.
Describe the crystalline structure of metals
Explain the utility of alloys
Describe the two main types of alloys
Chapter 9: Chemical Names and Formulas
Section 9.1 Naming Ions (pg. 253-258)
1. Name the representative element ions and determine their charges from the periodic table.
2. Determine the name of transition metal ions from the number of electrons lost.
3. Recognize and name several polyatomic anions.
.
Section 9.2 Naming and Writing Formulas for Ionic Compounds (pg. 260-266)
1. Name binary ionic compounds and those containing polyatomic anions given a chemical
formula.
2. Write the chemical formula of binary ionic compounds and those containing polyatomic
anions given its name.
Section 9.3 Naming and Writing Formulas for Molecular Compounds (pg. 268-270)
1. Name binary molecular compounds given chemical formulas
2. Write the chemical formulas for molecular compounds given their names
Section 9.4 Naming and Writing Formulas for Acids and Bases (pg. 271-273)
1. Name binary and oxyacids given chemical formulas
2. Write the chemical formulas for binary and oxyacids given their names
Section 9.5 The Laws Governing Formulas and Names (pg. 274-279)
1. Explain the Law of Definite Proportions as it relates to formula units
2. Explain the Law of Multiple Proportions as it relates to molecules
Written Work
Chapter 7:
p. 207-210 # 41, 43, 44, 45, 47, 48, 57, 73, 91, 93, 102
p. 211 # 2, 4, 11,12,13
Chapter 9:
pg. 281- 284 # 47, 49, 51, 53, 57, 60, 62, 63, 64, 65, 69, 71, 72, 73, 74, 83, 103
Pg. 285 # 12, 14,15
Pav 2013
Chapter 7/9 Supplemental Questions
1. Create a data table to record the physical and chemical properties of sodium chloride and the
elements that it is composed of, sodium and chlorine.
Use may use any resource that is available (except Mrs. Pav )
a.
Write a general statement that compares the compound with the elements it is comprised of.
2. Hard water is water that contains a large quantity of dissolved minerals such as calcium and
magnesium which can precipitate out of solution, form scaling in pipes, and ultimately ruin plumbing
systems.
Many water softeners work by running water through a system that contains a solid substrate (beads)
that is coated with sodium ions. The dissolved minerals having a stronger positive charge than
sodium and therefore have a greater affinity for the substrate than sodium and will replace sodium on
the substrate.
a.
The hardness of water is defined by the unit GPG (grains per gallon). 1 grain is defined
as 64.8mg of calcium carbonate per gallon. The ranges used to classify water as soft or
hard are in units of mg/L. Convert 1grain to mg/L using the following conversion factors.
1 grain = 64.8 mg/gal
1 gal = 4 qt
1.06 qt = 1L
b. The process of water softening adds about 12.5 mg of salt to 8 fluid ounces of drinking
water. If the daily maximum intake of sodium is 2300mg, how many milliliters of
processed water could one drink a day and not exceed the maximum sodium intake.
(8 ounces = 237 ml)
Pav 2013
Writing Ionic Equations
Using Lithium Bromide (LiBr) as an example, write the ionic equations for the following formula units. Keep in
mind that not every combination of cation and anion is 1:1, so you may need multiples of one or each atom to create a
neutral compound.
MgF2
K 3P
Mg3N2
BaS
SnO2
Pav 2013
Molecular Compounds
When naming binary molecular compounds, always name the more __________________________ atom first.
Naming Rules
1. If there is more than one of the 1st atom, precede the atom name by the appropriate prefix (di, tri, tetra, penta,
hexa, hepta, octa, nona, deca)
Example: C6O2
2.
hexacarbon dioxide
If there is only one of the first atom, do not precede the atom name by mono.
CO2 = monocarbon dioxide
3.
CO2 = carbon dioxide
Precede the second atom name by the appropriate prefix, including mono if there is only one of that atom. Drop
the last syllable (or 2) and add –ide to the element name
C2O Dicarbon monoxide
Element
C
N
O
F
P
Name
Carbide
Nitride
Oxide
Fluoride
Phosphide
Element
S
Cl
Se
Br
I
Name
Sulfide
Chloride
Selenide
Bromide
Iodide
Provide the name of the following molecular compounds
Compound
Compound Name
P 6O 3
Hexaphosphorus trioxide
NS4
Se8O
C7Br5
S2F2
Provide the Chemical Formulas given the following names
Compound Name
Dinitrogen monofluoride
Nonaphosphorus decachloride
Sulfur hexabromide
Tetracarbon pentasulfide
Octanitrogen trifluoride
Compound
Pav 2013
Ionic Compounds
Ionic compounds form from the combination of _____________________ and ______________________.
Atoms that lose electrons are called ____________________ and have a ___________________ charge.
Atoms that gain electrons are called ___________________ and have a ___________________ charge.
Naming ionic compounds with metals that only form one ion
1. State the name of the first atom
2. Drop the last syllable (or 2) from the second atom name and add –ide
Element
C
N
O
F
P
Name
Carbide
Nitride
Oxide
Fluoride
Phosphide
Element
S
Cl
Se
Br
I
Name
Sulfide
Chloride
Selenide
Bromide
Iodide
Name the following ionic compounds
Compound
CaBr2
Compound Name
Calcium Bromide
Na2O
Ag2S
K3P
Al2N3
Given the compound name, identify the ions involved and provide the chemical formula
Compound Name
Cation
Anion
Compound
Beryllium Chloride
Be2+
Cl-
BeCl2
Sodium Sulfide
Lithium Phosphide
Magnesium Nitride
Calcium Oxide
Pav 2013
Naming Ionic Compounds Using the Stock System (for atoms that have more than one possible charge)
Element
Copper (Cu)
Chromium (Cr)
Iron (Fe)
Lead (Pb)
Tin (Sn)
1+
X
2+
X
X
X
X
X
3+
4+
X
X
X
X
Follow the 1st atom name by the Roman numeral that represents its charge in parenthesis
Example
Copper (I) Chloride = CuCl
or
Copper (II) Chloride = CuCl2
Name the following ionic compounds using the stock system
Compound
Cation
Anion
Name
FeCl2
Fe2+
Cl-
Iron (II) Chloride
PbF4
Sn3P2
CoO
CrP
Provide the chemical formula give the names of the following ionic compounds
Name
Cation
Anion
Copper (II) Nitride
Cu2+
N3-
Tin (IV) Oxide
Lead (II) Iodide
Chromium (III) Phosphide
Iron (III) Bromide
Compound
Cu3N2
Pav 2013
Ionic compounds that contain polyatomic cations or anions
There is only one polyatomic cation, NH4+ (ammonium ion)
When naming polyatomic anions, the charge for each member of a pair is the same. The ions differ by the number of
atoms each member contains.
Example:
SO32- and SO42The name of the member of the pair with the fewer number of atoms ends in –ite, the other ends in –ate.
SO32- (sulfite) and SO42- (Sulfate)
When forming compounds with polyatomic ions, place parenthesis around the entire ion before attempting to add
subscripts (balance the charges)
Provide the names of the following compounds which contain polyatomic ions
Compound
Cation
Anion
Name
Ba(NO3)2
Ba2+
NO3-
Barium Nitrate
MgSO3
(NH4)3P
NaCN
Pb(HPO4)2
Form the compound containing polyatomic ions given the names
Name
Magnesium Phosphate
Ammonium Sulfite
Calcium Oxalate
Lithium Bicarbonate
Aluminum Permanganate
Cation
Anion
Compound
Mg2+
PO43-
Mg3(PO4)2
Pav 2013
Acids


An acid is a substance that produces H+ ions in solution.
There are two common types of acids – Binary (hydrogen plus a monatomic anion or a polyatomic anion that does
not contain oxygen, ex. HCl or HCN) and oxyacids (hydrogen plus a polyatomic anion containing oxygen, ex. HNO 3)
Naming Binary Acids
1. Hydro- is the prefix of all binary acids
2. Change the ending of the nonmetal to –ic.
Naming Oxyacids
1. There is no prefix for oxyacids
2. –ate anions are –ic acids (ex. H2SO4 = sulfuric acid)
3. –ite anions are –ous acids (ex. H2SO3 = sulfurous acid)
Name
Phosphoric Acid
Cation
Anion
Compound
H+
PO43-
H3PO4
H+
Hydroiodic Acid
HBr
H+
H+
H2SO3