The anatomy of the periodic table
 Get out your periodic tables
 Know where the following are on your
periodic table (p.t)
 Group A
 Group B
 Metals
 Nonmetals
 Metalloids (Semimetals)
 Note - aluminum is not considered a metalloid
The anatomy of the periodic table
 Know where the following are on your
periodic table (p.t) continued
 Transition metals
 Inner transition metals
 Alkali metals
 Alkaline metals
 Halogens
 Noble gases
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Naming Compounds
Ionic
Molecular
i.e. covalent
Naming Molecular Compounds
 Molecules are made up of nonmetals
 Prefixes are used to represent numbers of
atoms. See your text for prefixes
 Binary compounds end in -ide
 Examples
 Name? - Cl2O8 and OF2
 Formula for? - dinitrogen tetroxide
 Answers - dichlorine octoxide, oxygen
difluoride, N2O4
Naming Molecular Compounds
 Your turn. Try these.
 Name or write the formula for:
 Boron trichloride
 Dinitrogen tetrahydride
 N 2 O5
PF5
S4N2
CCl4
SO3 H2O
 Answers
 BCl3
N2H4 dinitrogen pentoxide
 Phosphorus pentafluoride
 Tetrasulfur dinitride
 Carbon tetrachloride
Sulfur Trioxide
 Dihydrogen Monoxide
Take ten minutes and work a
few problems on the “Naming
covalent compounds” side of
your worksheet.
Ions
 An atom that carries a charge
 The charge on the ion is called the
Oxidation state or Oxidation Number
 Cation - positively charged atom
Metals form cations
CATions are PAWsitive
 Anion - negatively charged atom
Nonmetals form anions
Naming Cations
Name the metal followed by the word
ion
 Example
Na - sodium - neutral element
Na1+- sodium ion - cation of the element
 Another example:
Mg - magnesium
Mg2+ - Magnesium ion
Naming Anions
 Ending changes are used for Anions
 Elemental anions will end in -ide
 Example
Cl2 - chlorine - neutral element
Cl1- - chloride - anion of the element
 Another example
O2 - oxygen
O2- Oxide
Writing Formulas for Binary Ionic
Compounds
 The periodic table tells you the charge
for group A (aka - the representative
elements)
 Group 1A - 1+ Group 2A - 2+
 Group 3A - 3+ Group 4 - depends
 Group 5A - 3- Group 6A - 2 Group 7A - 1- Group 8A or (0) - does
not form ions
Naming
 Your turn:
Name or write the symbol for the
following:
 Aluminum
 Calcium Ion
 Ga3+
K
Phosphide
Iodine
Nitrogen
Sulfide
Naming Binary Ionic Compounds
Name the metal then the nonmetal with
the ending changing to -ide
The -ide tells the person it is a binary
compound and the anion portion.
 Examples:
MgCl2
K2S
 Magnesium Chloride Potassium Sulfide
Writing Formulas for Binary Ionic
Compounds
 All compounds are electrically neutral
 To write the formula, figure out how many
cations and anions are needed so that the
number of positives and negatives are equal.
Find the least common multiple to figure
out the total number of +’s and -’s. Then
divide by the charge to find out how many
of each atom is needed!
 If X1+ and Y2-, what would be the formula?
 X2Y - Charges total 2 +’s and 2 -’s
Writing Formulas for Binary Ionic
Compounds
 If X3+ and Y2-, what would be the
formula?
 X2Y3 - Charges total 6 +’s and 6 -’s
 Find the formula for the following pairs
of ions:
Na1+ , P3-
 Answers: Na3P
Sr2+ , N3-
Sr3N2
 Now:
Finish side 1 of worksheet
Work sections 1 - 4 on back of worksheet
Work homework problems
Naming Compounds
Is there a metal?
Yes
No
Ionic
Molecular
Does the compound contain a
multivalent ion
aka - transition metal or
group B element
Use prefixes to represent
the number of atoms.
Example: H2O Dihydrogen Monoxide
CO2 Cabon Dioxide
No
Yes
Name the cation first
then name the anion
Example: Lithium Fuoride
Magnesium Carbonate
Name the cation first
Place a roman numeral
Name the anion
Example: Iron (II) Sulfate