1. Review of 1206
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2. - composed of a cation and an anion (usually metal and nonmetal)
Types of Compounds
Ionic Compounds
- composed of a cation and an anion
(usually metal and nonmetal)
eg. NaCl Mg3N2
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3. Cations +
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4. anions e g a t i v r e
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5. - composed of two or more nonmetals eg. CF4 C6H12O6 P4
Types of Compounds
Molecular Compounds
- composed of two or more nonmetals
eg. CF4 C6H12O6 P4
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6. Types of Compounds
NEW STUFF!!
Acids
- acids are hydrogen compounds that are dissolved in water
eg. HF(aq) H2SO4(aq)
aqueous
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7. Naming & Formulas A. Molecular Compounds common formulas PS: HOFBrINCl
prefixes indicate the number of each atom in binary molecular compounds
last element ends in - ide
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8. Naming & Formulas
eg. N3H5
disulfur octahydride
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9. Naming & Formulas B. Ionic Compounds - simple ions
- multivalent metals
- polyatomic ions
- hydrates
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10. BeF2 Naming & Formulas Simple Ions (only one possible charge)
- Cross Over Method
- reduce to lowest terms
eg. calcium chloride
sodium nitride
magnesium sulfide
K2O
BeF2
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11. ‘CrossOver’ Method
magnesium ion
nitride ion 3- 2+ Mg N
Mg3N2
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12. Cancel Charges (LCM) Mg N 2+ 3-
x 2 6-
x 3 6+
Mg3N2
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13. Naming & Formulas Multivalent Ions - Stock system (Roman numerals)
- Classical system
-ic indicates bigger charge
-ous indicates smaller charge
- reduce to lowest terms
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14. Naming & Formulas eg. lead (II) chloride lead (IV) chloride NiCl3
lead (IV) nitride
lead (IV) sulfide
NiCl3
CuO
Cu2O
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15. Naming & Formulas Polyatomic Ions - a group of atoms with a charge
- cross over method / lowest terms
- BRACKETS
eg. calcium hydroxide
ammonium sulfate
PbSO4
Sn3(PO4)4
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16. Naming & Formulas Hydrates - water mixed in with the ions
- heating removes the water to make an anhydrous (dry) compound
- use prefixes to indicate ratio of water to ions
eg. CuSO4• 5 H2O
copper (II) sulfate pentahydrate
lithium chloride dihydrate
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17. Naming & Formulas Acids
- acids form when hydrogen compounds are dissolved in water
- the subscript (aq) is used to indicate aqueous or dissolved in water
- 3 rules for naming acids
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18. Naming & Formulas Ionic name  Acid name
hydrogen ___ide  hydro___ic acid
hydrogen ___ate  ______ic acid
hydrogen ___ite  ______ous acid
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19. Naming & Formulas Writing Acid Names
- write the ionic name for the hydrogen compound
- apply the correct rule for the acid name
eg. HCl(aq)
hydrogen chloride  hydrochloric acid
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20. Naming & Formulas eg. HCl(aq) hydrogen chloride  hydrochloric acid
eg. HClO3(aq)
hydrogen chlorate  chloric acid
eg. HClO2(aq)
hydrogen chlorite  chlorous acid
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21.  hydrogen bromate  H+ BrO3-  HBrO3(aq) Naming & Formulas
Writing Acid Formulas
- use the correct rule to write the ionic name
- use ion charges to write the formula
eg. bromic acid
 hydrogen bromate
 H+ BrO3-
 HBrO3(aq)
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22.  hydrogen bromide  H+ Br -  HBr(aq) Naming & Formulas
hydrobromic acid
 hydrogen bromide
 H+ Br -
 HBr(aq)
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23. Practice: Write the formulas for: Write names for: calcium phosphide
magnesium sulfide
aluminum phosphide
potassium oxide
Write names for:
Li3N
MgO
BeF2
Al2S3
CF4
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24. MultiValent Compounds
FeO
iron (III)oxide
iron oxide
iron (II) oxide
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25. Reaction Types 1. Simple Composition (Synthesis)
Element + Element  Compound
eg.
H O2  H2O
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26. Reaction Types 2. Simple Decomposition Compound  Element + Element
eg.
K2O  K O2
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27. Reaction Types 3. Single Displacement
Compound + Element  Compound + Element
eg.
Cu AgNO3 
Cl NaF 
Cu(NO3) Ag
F NaCl
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28. copper wire is immersed in a silver nitrate solution
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29. Solutions of potassium iodide and lead(II) nitrate are mixed.
Potassium + lead(II) →
iodide nitrate
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30. Reaction Types 4. Double Displacement
Compound + Compound  Compound + Compound
eg.
Pb(NO3) KBr 
KNO PbBr2
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31. Reaction Types 5. Hydrocarbon Combustion
CxHy + O2(g)  CO2(g) + H2O(g)
eg.
C3H8(g)
+ O2(g)  CO2(g) H2O(g)
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32. Predicting Products
Write the name for the products in each of the following.
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33. Predicting Products
Write the formula(s) for the products in each of the following.
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34. Mg + O2 → MgO
AlCl CaI2 → AlI CaCl2
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