1. Naming Ionic Compounds
Physical Science

2. Example: Sugar (Glucose)
TYPES OF FORMULAS
Example: Sugar (Glucose)
Molecular formula - true formula; shows the actual number of atoms in a compound
C6H12O6

3. Example: Sugar (Glucose)
TYPES OF FORMULAS
Example: Sugar (Glucose)
Empirical formula - the simplest whole number ratio (reduce all numbers evenly)
C6H12O6 → CH2O

4. Example: Sugar (Glucose)
TYPES OF FORMULAS
Example: Sugar (Glucose)
Structural formula - shows the arrangement of atoms and bonds in a picture, chain or shape

5. Naming Ions Cations (+ ions) = metal ions Examples: Always named 1st.
Name does not change.
Examples:
Na+1 = sodium
Mg+2 = magnesium
Ga+3 = gallium

6. Naming Ions Anions (- ions) = nonmetal ions Examples:
Always named 2nd.
Change end of name to –ide.
Examples:
F-1 = fluoride (not fluorine)
O-2 = oxide (not oxygen)
P-3 = phosphide (not phosphorus)

7. Polyatomic Ions Polyatomic ion Group of atoms acting as a single ion.
Have a net negative or net positive charge.
Always treat as an unbreakable group!

8. Polyatomic Ions Common polyatomic ions (know these!): ammonium = NH4+1
acetate = C2H3O2-1
nitrate = NO3-1
hydroxide = OH-1
carbonate = CO3-2
sulfate = SO4-2
phosphate = PO4-3
These are listed on the back of your periodic table sheet!

9. Writing names from formulas
Write the name of the cation (metal) first.
Write the name of the anion (nonmetal) by changing the elements’ ending to -ide.
IF you have a polyatomic ion (look at your chart), then write the name as-is.
For ions with variable oxidation #’s (transition elements), write the ox. # in parentheses using Roman numerals.

10. Practice
NaBr
CuF2
Ag2O3

11. Naming Ionic Compounds
Name the following ionic compounds in your notebook:
NaCl = ?
K3N = ?
BaBr2 = ?
MgO = ?
CaS = ?
Al2Se3 = ?
sodium chloride
potassium nitride
barium bromide
magnesium oxide
calcium sulfide
aluminum selenide

12. Writing Formulas from Names
1) Identify ions in formula.
Cation is written first
2) Figure out charges.
They must equal zero!
If the charges cancel out, just write the symbols
3) If charges don’t cancel out, use the Criss-cross method.
Use parentheses when more than one polyatomic ion is needed.
Roman numerals indicate the oxidation #.

13. Ionic Formulas potassium chloride magnesium nitrate K+ Cl-  KCl
copper(II) chloride
K+ Cl-  KCl
Mg2+ NO3-  Mg(NO3)2
Cu2+ Cl-  CuCl2

14. Ionic Formulas calcium oxide aluminum chlorate Ca2+ O2-  CaO
iron(III) oxide
Ca2+ O2-  CaO
Al3+ ClO3-  Al(ClO3)3
Fe3+ O2-  Fe2O3

15. Writing Formulas from Names
Write formulas for the following ionic compounds in your notebook.
potassium iodide
magnesium fluoride
calcium sulfide
rubidium nitride
aluminum bromide
strontium oxide
K+1 and I-1
Mg+2 and F-1
Ca+2 and S-2
Rb+1 and N-3
Al+3 and Br-1
Sr+2 and O-2 KI
MgF2
CaS
Rb3N
AlBr3
SrO

16. Writing Formulas With Polyatomic Ions
If you need to multiply a poly. ion, use parentheses.
Examples:
Na+1 and NO3-1 = NaNO3
Mg+2 and NO3-1 = Mg(NO3)2
Al+3 and NO3-1 = Al(NO3)3
Na+1 and CO3-2 = Na2CO3
Mg+2 and CO3-2 = MgCO3
Al+3 and CO3-2 = Al2(CO3)3

17. Writing Formulas With Polyatomic Ions
Write the following ionic formulas in your notebook. Use parentheses when necessary.
K+1 and OH-1 = ?
NH4+1 and Cl-1 = ?
Mg+2 and C2H3O2-1 = ?
Al+3 and PO4-3 = ?
KOH
NH4Cl
Mg(C2H3O2)2
AlPO4

18. Naming Compounds With Polyatomic Ions
Polyatomic ions do not change their names in compounds.
Example:
Ca(OH)2
calcium hydroxide

19. Naming Compounds With Polyatomic Ions
Name the following compounds in your notebook:
(NH4)2SO4
Ga2(CO3)3
Li3PO4
NaC2H3O2
Be(NO3)2
ammonium sulfate
gallium carbonate
lithium phosphate
sodium acetate
beryllium nitrate

20. Naming Mixed Ionic Compounds
Name the following compounds in your notebook:
InBr3
(NH4)2S
Sr3N2
KNO3
BaTe
ZnCO3
indium bromide
ammonium sulfide
strontium nitride
potassium nitrate
barium telluride
zinc carbonate