Metals
Transition Metals
Metals

 Binary Ionic Compounds
 Consist of two elements: metal cation and a non-metal anion
 Metal is named first and says its own name
 Non-metal is named second and changes its suffix to “ide”
 For transition metals with more than one ionic charge
 Use the anions to determine their charge
 Indicate their charge with roman numerals
 Only Ag + , Zn 2+ , and Cd 2+ have 1 charge. You do not need
Roman numerals for these

Ions Compound Name
Sodium & chlorine Sodium chloride
Aluminum & chlorine Aluminum chloride
Aluminum & oxygen Aluminum oxide
Sodium & sulphur
Iron (2 +) & Oxygen
Sodium sulphide iron (II) oxide
Iron (3+) & Oxygen iron (III) oxide

 Binary Ionic Compounds
 Write down the symbols for each individual ion side by side – cation first, anion second
 Balance the charges by crossing them
(Swap & Drop)
 *Charges become subscripts*
 Write the formula
 Note:
 You do not need to write the subscript 1 in the formula
 You should reduce the subscripts if possible

Compound
Name
Sodium chloride
Aluminum oxide
Na
Al
+
3+
Ions
& Cl
& O
-
2iron (III) oxide Fe 3+ & O 2iron (II) oxide Fe 2+ & O 2-
Formula
NaCl
Al
2
O
3
Fe
2
O
3
Fe
2
O
2
 FeO

 Ternary Ionic Compounds
 Ionic compounds that contain polyatomic ions
 Polyatomic ions act as a single unit (subscripts included)
 Monatomic cations say their own name; monatomic anions end in the suffix “ide”
 Polyatomic ions always say their own name
 When more than one polyatomic ion is used in a formula, it will be placed in brackets

Ions Compound Name
Ammonium & chlorine Ammonium chloride
Potassium & sulfate Potassium sulfate
Lead (2+) & phosphate Lead (II) phosphate
Ammonium & oxalate Ammonium oxalate

 Ternary Ionic Compounds
 Same as binary ionic compounds
 Make sure that when you balance the charges that the subscript for a polyatomic ion is OUTSIDE of the brackets
 This is because polyatomic ions act as a single unit and the subscript applies to the entire unit
 Remember, numbers WITHIN the brackets of a polyatomic ion CANNOT be reduced

Compound
Name
Ions
Ammonium sulphide
NH 4+ & S 2-
Potassium carbonate
K + & CO
3
2-
Iron (II) nitrate Fe 2+ & NO
3
-
Sodium sulfate Na + & SO
4
2-
Formula
(NH
4
)
2
S
K
2
CO
3
Fe(NO
3
)
2
Na
2
(SO
4
)

Have a characteristic formula structure: “HX”
 Where “H” is a hydrogen cation
 Where “X” is an anion
 So generally, if you see a formula for an ionic compound that starts with an “H” it is likely an acid

 Scenario 1 – The anion ends in the suffix “ide”
 Add the prefix “hydro” to the anion
 Change the suffix to “ic”
 Add the word “acid” to the end
 i.e. HF  hydrogen & fluoride
  hydrofluoric acid
 i.e. HCN  hydrogen & cyanide
  hydrocyanic acid

 Scenario 2 – The anion ends with the suffix “ate”
 Change the suffix of the anion to “ic”
 Add the word “acid” to the end
 Note: no need for the “hydro” prefix
 Hint to remember – “If you ATE it, its Icky”
 i.e. HNO
3
 hydrogen & nitrate
  nitric acid
 i.e. H
2
SO
4
 hydrogen & sulfate
  Sulfuric acid

 Scenario 3 – The anion ends with the suffix
“ite”
 Change the suffix on the anion to “ous”
 Add the word “acid” to the end
 Note: no need for the “hydro” prefix
 i.e. HNO
2
 hydrogen & nitrite
  nitrous acid
 i.e. H
2
SO
3
 hydrogen & sulfite
  sulfurous acid

 Use the prefix/suffix combinations to figure out the anion
 Balance the charges with a H+ cation (s)
 Write the formula
 i.e. – permanganic acid
  permanganate anion  MnO
4
-
  HMnO
4

 Prefixes are used to indicate the number of atoms
 The prefix “mono” is only used for the second atom; no mono prefix needed for the first atom
 The second atom named ends with the suffix, “ide”
 Prefixes:
 1 – “mono”
 2 – “di”
 3 – “tri”
 4 – “tetra”
 5 – “penta”
 6 – “hexa”
 7 – “hept”
 8 – “oct”
 9 – “non”
 10 - “deca”

 N
2
H
4
:
 Dinitrogen tetrahydride
 SO
3
:
 Sulfur trioxide
 CO
2
:
 Carbon dioxide
 P
2
O
5
:
 Diphosphorus pentoxide
 PCl
3:
 Phosphorus trichloride

 Read the prefixes to determine the amount of each atom
 Examples:
 carbon tetrachloride:
 CCl
4
 dinitrogen trioxide:
 N
2
O
3
 carbon disulfide:
 CS
2
 dihydrogen monosulfide:
 H
2
S
 sulfur hexafluoride:
 SF
6

 The number of atoms in a formula is determined by the subscripts
 If there is no subscript, this means that there is only one of a particular atom
 i.e.: NaCl
○ 1 Na atom and 1 Cl atom
○ 2 atoms total
 When you are dealing with polyatomic ions, remember that the subscript found outside of the brackets is applied to every atom inside the brackets by using the distributive property of multiplication
 i.e.: Mg(NO
3
)
2
○ 1 Mg atom, 2 N atoms, 6 O atoms
○ 9 atoms total

 To find the mass of a molecule/compound, simply add up all of the masses of the individual atoms in the compound
 Value is known as the “Molar Mass” of a molecule/compound
 i.e.: NaCl
 i.e.: Mg(NO
3
)
2