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Writing & NamingFormulas
of Ionic & Covalent
Compounds
BondingTypes
Ionic, Covalent, or Metallic
• Review
Ionic Compounds
Crystalline Lattice
Ionic Compounds
• Contains a metal and nonmetal
• The valence electrons from the metal are transferred to the nonmetal.
• Metal is listed first, followed by the nonmetal.
• Change the name of the nonmetal to ~ide. – Examples: sulfide, oxide, phosphide.
• Ionic Example: NaClSodium Chloride
Ionic Binary Compound Naming Practice
1.Al2S3
2.Ba3P2
3.BaO
4.CaBr2
5.CsI
1.Aluminum Sulfide
More Ionic Binary Compounds Naming
Practice1.Fr2Cl
2.FrF
3.Sr3N2
4.K2O
5.Mg3P2
1.Francium Chloride
The 5 steps for writing a binary ionic compound
formula1. Write the symbols of the two
elements2. Write the oxidation number of
each as superscripts.3. Drop the positive and negative
signs4. Crisscross the superscripts so
they become subscripts. 5. Reduce when possible
Formula for Aluminum Oxide
1. Write the symbols of the elements
Al O
Formula for Aluminum Oxide
2. Write the oxidation numbers for each element
Al O+3
-2
Formula for Aluminum Oxide
3. Drop the positive & negative sign.
Al O3 2
Formula for Aluminum Oxide
4. Crisscross the superscripts so they become subscripts
Al O3 2
Formula for Aluminum Oxide
5. Reduce subscripts when possible. (not possible here)
Al O32
Examples of Reduction
of SubscriptsSr2O2
Al3P3
Pb2O4
Ba3N2
SrO
Ionic Binary Compound Formula Practice
1.Potassium iodide
2.Lithium bromide
3.Magnesium oxide
4.Sodium nitride
5.Radium phosphide
1. KI
More Ionic Binary Compound Formula
Practice1. Gallium Fluoride
2. Strontium chloride
3. Cesium sulfide
4. Aluminum bromide
5. Barium Phosphide
1. GaF3
Polyatomic Ions
Polyatomic (many atoms) ions are covalent molecules with a charge. They behave as if they were one-atom ion.
Polyatomic Ions
NH4+1
C2H3O2-1
ClO3-1
NO3-1
OH-1
CO3-2
SO4-2
PO4-3
Note: Ammonium is the only polyatomic ion with a + charge.
Treat polyatomic ions as you would an ion – crisscross to determine the formula.
The only difference is that when you have more than one of a Specific polyatomic ion in a formula you must encase
it in parenthesis.
Use your reference sheets to determine the name of the following polyatomics.
Writing Names with Polyatomics
1. Ca3(PO4)2
2. NH4Br
3. NaNO3
4. K2SO4
5. Mg(ClO3)2
1. Calcium Phosphate
As in all ionic compounds you must reduce subscripts, but you cannot change the formula of the polyatomic ion. You can only reduce subscripts outside the parenthesis.
Writing Names with Polyatomics
1. LiOH1. Lithium Hydroxide
2. Potassium
Carbonate
3. Barium Acetate
4. Ammonium Sulfide
5. Strontium Sulfate
Rolling AtomsInstructions:• Obtain a yellow cube and a blue cube • Roll the dice and using the elements that appear
on the tope face, write it’s name, ion, along with the correct formula and name for the compound in the template provided
• Use the dice to write 30 different compound formulas and names. You must have 30 different compounds!! After you reach 15, you will need to come up and get a new set
• When finished, you need to turn in your template and get a molecular naming review half sheet
Metal Nonmetal Metal Ion NM Ion Cmpd. Name Cmpd. Formula
1.
Covalent Compounds
Water Molecule
Hydrogen
Atom
Hydrogen
Atom
Oxygen Atom
Covalent Compounds
• Contains 2 or more nonmetals• The valence electrons are shared
between the nonmetals. • Must use prefixes in the name.• Name tells you the formula. – Example: N2O4 – dinitrogen tetroxide
• You CANNOT reduce the formulas
Covalent Prefixes
Mono -1Di – 2Tri – 3
Tetra – 4Penta – 5
Hexa – 6Hepta – 7Octa – 8Non – 9
Deca -10
A prefix tells you the number of atoms of that element in the
compound.
Naming Covalent Compounds
1. N2O3
2. CH4
3. PO5
4. S2F4
5. P4O10
1. Dinitrogen trioxide
Writing Formulas for Covalent Compounds
1. CO1. Carbon Monoxide
2. Phosphorus
Pentachloride
3. Sulfur hexafluoride
4. Dinitrogen trioxide
5. Sulfur dioxide
Ionic & Covalent Structure
Ionic Compounds
form a
crystalline lattice
– repeating
pattern of ions.
Covalent
compounds form
individual
molecules that
are not connected
to each other.
Na+1 Ions Cl-1 Ions
Sodium Chloride
Water
Name These Compounds
1. PCl3
2. Sr3N2
3. KOH
4. NO2
5. MgCO3
1. Phosphorus
trichloride
Write formulas for these compounds
1. Calcium Chlorate
2. Sodium Bromide
3. Sulfur hexafluoride
4. Carbon tetrachloride
5. Potassium
Phosphate
1. Ca(ClO3)2
Review of Ionic Compounds
Include Metals & NonmetalsYou need oxidation numbersName the metalChange the Nonmetal to –ide….Unless it has a polyatomic and
you give it it’s name…
Summing up: Ionic
• Ionic bonding occurs between a metal and a nonmetal. Metals lose all their valence electrons and become cations. Nonmetals gain enough electrons to fill their valence level and become anions.
• Always crisscross oxidation numbers and reduce to determine the formulas of ionic compounds
• Do not use prefixes in the names.• Ions form a crystalline lattice.
Summing up: Covalent
• Covalent bonding occurs when two nonmetals share electrons to fill their valence energy level.
• Never use oxidation numbers to determine the formula. There aren’t any since the two atoms share electrons, they do not take on a charge.
• Always use prefixes in the names.• Atoms combine to form individual
molecules.
WarmUp
1. What is necessary to write ionic compounds?
2. Which elements are involve d in ionic compounds?
3. When writing names for covalent compounds what must be included?
4. Which elements are involved in covalent compounds?
Chemical Formulas Vocab
Ionic CompoundsValence ElectronsPolyatomic IonsCovalent CompoundsPrefixesCrystalline Lattice StructureMolecules
RememberCovalent Bonds –• Molecules• 2 or more nonmetals• prefixes Phosphorus Pentachloride PCl5• name it with prefixes CO Carbon MonoxideIonic Bonds-• crystalline lattice• metal & nonmetal• criss cross oxidation numbers: Al+3O-2
Al2O3
• name as you see it Aluminum Oxide