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Naming Compounds
Unit D.5
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IONIC COMPOUNDSPart 1:
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Ionic Formulas
• An ionic compound formula is a ratio of the number of cations to anions
• E.g.: CaCl2 will have 1 Calcium atom per 2 chlorine atoms
• The ratios are determined by the charge of each atom
• Calcium has a +2 charge, so there needs to be two chlorine atoms per atom of calcium
+2 -1
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For the visual learners out there…
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Here’s Calcium Chloride
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Balancing Ionic Formulas: Crisscross Method
Ca + Cl
1. Write the charges of each atom based upon its location in the periodic table
2+ -1
2. Bring the numbers down diagonally, ignoring the sign3. Reduce to smallest possible ratio, if necessary. Remove redundant numbers.
21
= CaCl2
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Practice
1. Mg + O .
2. Na + S______________ .
3. Sr + Cl .
4. Be + O_______________
5. Li + F .
MgONa2S
SrCl2
BeOLiF
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Naming Ionic Compounds
• Number of atoms does not affect naming• The regular name of the metal cation always
comes first• The suffix of the anion changes to –ide• NaCl = Sodium Chloride• NaF = Sodium Fluoride• CaBr2 = Calcium Bromide
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Common AnionsElement Name as Anion Example
Sulfur Sulfide Sodium SulfideFluorine Fluoride Calcium FluorideIodine Iodide Potassium Iodide
Bromine Bromide Strontium BromideChlorine Chloride Sodium ChlorideOxygen Oxide Iron Oxide
Nitrogen Nitride Barium NitrideCarbon Carbide Tungsten Carbide
Phosphorous Phosphide Nickel Phosphide
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Try these.
1. Na2S2. Li3N3. Ag2O4. CaBr2
5. K2O6. SrCl2
________________
________________
________________
________________
________________
________________
Sodium SulfideLithium Nitride
Silver Oxide
Calcium BromidePotassium Oxide
Strontium Chloride
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Ions with multiple charges
• Transition metals can have different ionic states
• Iron, for example, can sometimes have a +2 charge, while other times it will have a +3
• To avoid confusion, we notate Iron with a +2 charge as Iron(II), while Iron with a +3 charge would be Iron(III)
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Demo
• Iron(III) Oxide = Fe3+ + O2- = Fe2O3
Iron(II) Oxide = Fe2+ + O2- = FeO
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Now try these
1. FeO______________
2. Fe2O3
_____________________
3. NiBr3
_____________________
4. CrO______________
5. Cr2O3
_____________________
Iron(II) Oxide
Iron(III) Oxide
Nickel(III) Bromide
Chromium(II) Oxide
Chromium(III) Oxide
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Writing Formulas from Names
• Use periodic trends to predict ionic charges of atoms (Group I = +1, Group II = +2, etc)
• Overall charge of compound should equal 0• Use the “crisscross method” to assign number
of atoms & reduce to lowest # ratio• “Sodium Fluoride” = Na+ + F- =• “Calcium Chloride” = Ca2+ + Cl- = CaCl2
NaF
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Practice
1. Calcium Bromide2. Potassium Sulfide3. Nickel(II) Iodide4. Copper(II) Oxide5. Strontium Fluoride
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Polyatomic ions
• Some molecules have an overall charge, like ions
• These are called polyatomic ions
• They are treated as a single unit and can NOT be separated!
• Naming system is otherwise the same
Barium Sulfate
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Balancing polyatomic ions
Al+3 + SO42-
Al2(SO4)3
Treat the entire polyatomic ion as 1 unit
For balancing, place the polyatomic anion in parenthesis
( )32
Naming Conventions are the same as regular ions
Aluminum Sulfate
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Balance and name the following using
1. Na + SO42-
_______________________2. Ca + OH-
_______________________3. Mg + NO3
-
_______________________4. Sr + CO3
2-
______________________5. NH4
+ + NO3-______________________
Na2SO4 Sodium SulfateCa(OH)2 Calcium Hydroxide
Mg(NO3)2 Magnesium Nitrate
SrCO3 Strontium CarbonateNH4NO3 Ammonium Nitrate
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Naming Covalent Compounds
• Number of atoms is represented by prefix• All atoms in a molecule have their own
separate prefixes and are listed in order of appearance
• First element only has a prefix if it is greater than 1
• Last element ends in -ide
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Prefix # of atoms Example Formula
mon 1 Carbon Monoxide CO
di 2 Carbon Dioxide CO2
tri 3 Sulfur Trioxide SO3
tetra 4 Carbon tetrachloride CCl4
penta 5 dinitrogen pentoxide N2O5
hexa 6 Sulfur hexafluoride SF6
hepta 7 Iodine heptafluoride IF7
octa 8 heptaphosphorous Oxtafluoride P7F8
nona 9 tetraiodine nonafluoride I4F9
deca 10 Disulfur decafluoride S2F10
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Practice
1. CO____________
2. NO2
__________________
3. SF2
__________________
4. CCl4
__________________
5. NI3
__________________
Carbon Monoxide
Nitrogen dioxide
Sulfur difluoride
Carbon tetrachloride
Nitrogen triiodide
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Naming Acids
• All* Acids begin with Hydrogen
• HCl, H2SO4, HNO3, etc• Although there is a
naming system, most scientists just memorize them
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