jump to first page section 6.3 ionic bonding and ionic compounds
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Section 6.3 Ionic Bonding and Ionic Compounds
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Warm-Up
How is a chemical formula for a covalent compound different from the chemical formula for an ionic compound?
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Ionic Compounds
Made up of positive ions (cations) and negative ions (anions) that are combined so that the numbers of positive and negative charges are equal.
The chemical formula of an ionic compound represents the simplest ratio of the compound’s combined ions.
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CrystalsCrystals
Most ionic compounds Most ionic compounds are are crystalline solids - crystalline solids - a three-dimensional a three-dimensional network of positive and network of positive and negative ions mutually negative ions mutually attracted to one another.attracted to one another.
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Formula Units Unlike molecular compounds, ionic compounds are
not made up of independent units that can be isolated and examined
Ionic solids exist as repeating units of positively and negatively charged ions in a 3-dimensional structure.
Formula units are the simplest collection of atoms from which an ionic compound’s formula can be established and that gives electrical neutrality
Calcium fluoride, CaF2 (fluorite)
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Monatomic Ions
By gaining or losing electrons many main group elements form ions with noble gas configurations.
Ions formed from a single atom are called monatomic ions.
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There is a PATTERN for which charge will form on an atom for the main groups.
+1 }SKIP+2 +3+4-4 -3 -2 -1 0
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Formulas for Ionic CompoundsFormulas for Ionic Compounds
The charges must balance to 0, and the formula must reflect this.
Ionic compounds do not form by the combination of isolated ions, but we can use electron dot notation to see the changes that take place in ionic bonding.
Li and F LiF Mg and F MgF2
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Formulas for Ionic CompoundsFormulas for Ionic Compounds
In your table groups come up with rule(s) for writing chemical formulas for ionic compounds.
Li and F LiF Al and O Al2O3
Li and O Li2O Al and F AlF3
Mg and F MgF2
Mg and O MgO
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Rule???Rule???
Crisscross the charges!Crisscross the charges! Write the symbol for each ion, metals Write the symbol for each ion, metals
first.first. Write the charge above each.Write the charge above each. If the charges add up to zero, you’re If the charges add up to zero, you’re
done.done. If they don’t, play the criss-cross game.If they don’t, play the criss-cross game. Example:Example:
LiLi++ OO2- 2- = Li = Li22OO
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Your TurnYour Turn
Write the formula for the following:
a.a. Li and S Li and S
b.b.Al and OAl and O
c.c. I and KI and K
d.d.Mg and FMg and F
e.e. N and AlN and Al
f.f. Ca and BrCa and Br
Li2S
Al2O3
KI
MgF2
AlN
CaBr2
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What’s in a name?Activity Directions:
1.In your table groups, examine the table on page 2 and come up with at least three rules for naming ionic compounds based on the examples given.
2.Answer the making sense question and practice problems #1-6 and 1-8.
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3 Rules?
• Positive ion (metal) always comes first
• Change ending of nonmetal to –ide
• Add Roman numerals to show the charge on transition metals
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Name the following ionic compounds:
1. NaCl
2. K2S
3. Ca3N2
4. FeS
5. CoF2
6. ZnCl2
Sodium Chloride
Potassium Sulfide
Calcium Nitride
Iron (II) Sulfide
Cobalt (II) Fluoride
Zinc (II) Chloride
Actually just Zinc Chloride b/c Zinc only has 1 possible charge
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Write the following ionic compounds:
1. Magnesium iodide
2. Lithium bromide
3. Calcium Phosphide
4. Aluminum Nitride
4. Aluminum Chloride
5. Potassium Oxide
6. Iron (III) Sulfide
7. Copper (II) Chloride
MgI2
LiBr
Ca3P2
AlN
AlCl3
K2O
Fe2S3
CuCl2
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Check-in:
• Write the symbols for the cation and anion in the ionic compound PbCl4 and name the compound.
Pb4+ and Cl1- Lead (IV) Chloride
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1. Name the following binary ionic compounds.
a. K3Nb. CoF2
c. PbI2
d. SnS2
e. NiOf. ZnCl2g. Ag3P
Homework #1-2
Potassium nitrideCobalt (II) Fluoride
Lead (II) IodideTin (IV) SulfideNickel (II) OxideZinc (II) Chloride
Silver (I) Phosphide
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2. Write the formulas for the following names:
a. Magnesium iodideb. Lithium bromidec. Aluminum chlorided. Calcium phosphidee. Potassium oxidef. Iron (III) sulfideg. Copper (I) Chlorideh. Gold (III) iodidei. Zinc (II) oxide
MgI2
LiBrAlCl3Ca3P2
K2OFe2S3
CuClAuI3
ZnO
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Monotomic IonsMonotomic Ions
Ions formed from a Ions formed from a single atom. single atom. Main Main group ions form to group ions form to a noble gas a noble gas configuration:configuration:
AlAl3+3+, O, O2-2-, etc., etc.Transition metals can Transition metals can
show many different show many different charges: Pbcharges: Pb2+2+, Pb, Pb4+4+, , etc.etc.
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Ratios To balance the charge, the ratio of the ions in a
formula unit depends on the charges of the combined ions.
Example: Names – cation first, anion last. Calcium fluoride (the -ine of the anion is dropped and replaced by -ide as a suffix because the fluorine is now in an ionic compound).
Ca2+ + 2F- → CaF2
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Naming Binary Ionic Compounds
Nomenclature: naming system.
We will go over the Stock System of Nomenclature (Chapter 7, Section 1, pp. 206-210).
You MUST use Table 7-1 p. 205 and Table 7-2 p. 210 to
help you in naming ionic compounds.
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Polyatomic IonsPolyatomic Ions
Consist of more than Consist of more than one atom and the one atom and the group is charged:group is charged:
NHNH44++, SO, SO44
2-2-, etc., etc.
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Formation of Ionic CompoundsFormation of Ionic Compounds• Ionic compounts do not form by the
combination of isolated ions, but electron dot notation can be used to demonstrate the changes that take place.
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Mama Nature Strikes Again
Since nature favors situations of lowered potential energy, ions do this by arranging into an orderly 3-D arrangement known as a crystal lattice.
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Structure:Structure:
3-D crystals 3-D crystals balancebalance + and -charges + and -charges ex. Naex. Na1+1+ClCl1- 1- = NaCl, = NaCl,
CaCa2+2+ 2F 2F1-1- = CaF = CaF22
The ions in the crystal are surrounded The ions in the crystal are surrounded by ions of opposite charge.by ions of opposite charge.
Energy is released Energy is released
when ions form bonds.when ions form bonds.
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Lattice EnergyLattice Energy This is the This is the
energy released energy released when one mole when one mole of an ionic of an ionic crystalline crystalline compound is compound is formed from formed from gaseous ions gaseous ions (see table 6-3 on (see table 6-3 on p. 179).p. 179).
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Ionic vs. Molecularbonding:
Very strong, hard and brittle.
Solids at room T Higher bp/mp Conduct heat & electricity
in molten state. Many soluble in water.
Strong within molecule; weak between molecules.
Mostly gases and liquids @ room T (vaporize readily)
Lower bp/mp. Don’t conduct.
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Polyatomic Ions
Groups of covalently bonded atoms can have charges.
Ex. PO43−
The phosphate anion is a covalently bonded molecule that has gained 3 electrons and has become an ion. It is able to bond with another ion such as Fe2+ to give Fe3(PO4)2 [iron (II) phosphate].
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Assignment:Worksheets:
6-3 Review
Chapter 6 Review, pp. 195-198, 11, 19, 35-39, 41, 42, 54, 56, 57, 63-65.
Do all assignments from the book separately.