1) Covalent 2) Ionic 3) Organic ◦ Entire unit in Chem 30S

 Generally a bond between 2 non-metal elements  General Rules ◦ First element is named as listed on periodic table ◦ Second element has the suffix –ide ◦ Prefix used for each element to indicate the # of atoms  If only one atom of first element → No prefix used

NumberPrefix 4tetra 1mono 2di 3tri 5penta 6hexa 7hepta 8octa 9nona 10deca

 Name the following ◦ CO 2 ◦ CO ◦ CCl 4 ◦N2O4◦N2O4 ◦ SF 6 ◦ P 2 Cl 5 ◦ PI 3 ◦ P 5 Cl 8 Carbon dioxide Carbon oxide Carbon tetrachloride Dinitrogen tetraoxide Sulfur hexafluoride Diphosphorus pentachloride Phosphorus triodide Pentaphosphorus octachloride

 Write the formulas for the following ◦ Tetranitrogen decaoxide ◦ Disulfur pentafluoride ◦ Hexaselenium tribromide ◦ Nitrogen monoxide ◦ Aluminum Chloride N 4 O 10 S2F5S2F5 Se 6 Br 3 NO IONIC

 3 subcategories ◦ Monatomic Ions ◦ Polyatomic Ions ◦ Transitional Metals  Can use both monatomic and polyatomic  Rules ◦ Formula must be neutral ◦ No # prefixes used as only one possible combination with ions involved ◦ Cation (+ve) listed first, Anion (-ve) listed second

 Monatomic ions are ions that contain only 1 atom  Anion has suffix –ide  Examples ◦ NaCl ◦ AlCl 3 ◦ MgO ◦ Ga 2 P 3 ◦ HF ◦ NaH Sodium Chloride Aluminum Chloride Magnesium Oxide Gallium Phosphide Hydrogen Fluoride Sodium Hydride

 Entire unit MUST be neutral ◦ Add appropriate # of each ion to balance charges  Example  Aluminum Fluoride Al 3+ F-F = +2 Al 3+ 3F = 0 AlF 3

 Example  Gallium Oxide Ga 3+ O = +1 Ga 3+ 2O = -1 Ga 2 O 3 2Ga 3+ 2O = +2 2Ga 3+ 3O = 0

 Examples ◦ Write the formulas for the following  Lithium Sulfide  Magnesium Bromide  Hydrogen Nitride  Aluminum Phosphide  Boron Sulfide Li 2 S MgBr 2 H3NH3N AlP B2S3B2S3

 Ions with more than one atom ◦ Eg)  NO 3 - (Nitrate)  PO 4 3- (Phosphate)  NH 4 + (Ammonium) ◦ The entire item has a charge, not each element in the polyatomic ion  Look at page. 257  The exact ion name is used

 Examples ◦ NaBrO 3 ◦ Na 2 C 2 O 4 ◦ Ca(NO 3 ) 2 ◦ NH 4 Cl ◦ Al 2 (SO 3 ) 3 Sodium Bromate Sodium Oxalate Calcium Nitrate Ammonium Chloride Aluminum Sulfite

 Entire unit MUST be neutral ◦ Add appropriate # of each ion to balance charges  Example  Potassium Permanganate K+K+ MnO = 0 KMnO 4

 Example  Magnesium Nitrite Mg 2+ NO = +1 Mg 2+ 2NO = 0 Mg(NO 2 ) 2

 Transitional Metals can have different charges ◦ Depends on the situation ◦ Example  Fe 2+  Fe 3+  Ti 2+  Ti 4+  When naming, must determine what the charge is ◦ Indicated by using Roman numerals  Must know Roman numerals 1-10

 Example  FeO Fe 2+ O = 0+2 Iron (II) Oxide

 Example  Fe 2 (CO 3 ) 3 2Fe3CO = 0+6 Iron (III) Carbonate 3+

 Write the names for the following ◦ TiS 2 ◦ CuCl ◦ AgNO 3 ◦ CuSO 4 ◦ V(ClO 4 ) 5 Titanium (IV) Sulfide Copper (I) Chloride Silver (I) Nitrate Copper (II) Sulfate Vanadium (V) Perchlorate

 The name indicates the charge ◦ Balance as normal  Example  Zinc (II) Chloride Zn 2+ Cl = +1 Zn 2+ 2Cl = 0 ZnCl 2

 Examples ◦ Nickel (II) Nitride ◦ Chromium (IV) Oxalate ◦ Iron (III) Cyanide ◦ Mercury (I) Acetate (careful) Ni 3 N 2 Cr(C 2 O 4 ) 2 Fe(CN) 3 Hg 2 (CH 3 COO) 2

 Peroxide ◦ A polyatomic ion with 2 oxygen atoms with a 2- charge ◦ Very reactive ion ◦ Explosive in some cases  H 2 0Dihydrogen Monoxide (Covalent)  H 2 O 2 Hydrogen peroxide (Ionic)

 Example  MgO 2  If the oxygen is an oxide ion, then we would have -4  The Mg is +2  This is not balanced  Therefore the O 2 item must have a -2 charge  Peroxide (O 2 2- )

 P.282 #’s ◦ Omit #67 d)& #69 i)& #66 h)