Ionic Compounds Level 2

Metal Cations Type I * metals whose ions can only have one possible charge Groups IA & IIA Al, Ga, In, Zn, Cd, & Ag * determine charge by position on the Periodic Table IA = 1+; IIA = 2+ Al, Ga, and In = 3+; Zn & Cd = 2+; Ag = 1+

Type II * metals whose ions can have more than one possible charge * Mostly transition and post transition metals

Polyatomic Ions * made of more than one atom. * groups of atoms that travel together—NEVER apart. * The given charge is on the entire polyatomic ion—not on individual atoms within the polyatomic ion.

Naming & Writing Formulas

Type I Metals Naming * ALWAYS name the cation first and the anion second * Cation – metal name * Anion – 1. if nonmetal change end of name to -ide 2. if polyatomic ion use the name

Name the following Potassium Chloride KCl NaCl MgO Sodium Chloride Li3PO4 NH4Cl Potassium Chloride Sodium Chloride Magnesium Oxide Lithium Phosphate Ammonium Chloride

MgF2 Writing the Formula Magnesium Fluoride Mg+2 F-1 F-1 1. Write the ions that make up the compound Mg+2 F-1 2. Do the charges add to equal zero? No – go to 3; Yes – go to 4. F-1 3. Add ions as needed so the compound has a charge of zero MgF2 4. Write the number of each ion as a subscript and you have the formula (DO NOT include charges & DO NOT write 1s)

Zn(NO3)2 Zinc Nitrate Zn+2 NO3-1 NO3-1 1. Write the ions that make up the compound Zinc Nitrate 2. Do the charges add to equal zero? No – go to 3; Yes – go to 4. Zn+2 NO3-1 3. Add ions as needed so the compound has a charge of zero NO3-1 4. Write the number of each ion as a subscript and you have the formula (DO NOT include charges & DO NOT write 1s) *If you have more than 1 of a polyatomic ion, you must put the ion in parenthesis* Zn(NO3)2

Write the formula for the following Calcium Oxide Aluminum Chloride Ammonium Nitrate Ca2+ O2- CaO Al3+ Cl- AlCl3 NH4+ NO3- NH4NO3

Type II Metals PbI4 Lead (IV) Iodide Writing the Formula Pb+4 I-1 I-1 1. Write the ions that make up the compound I-1 I-1 2. Do the charges add to equal zero? No – go to 3; Yes – go to 4. I-1 3. Add ions as needed so the compound has a charge of zero PbI4 4. Write the number of each ion as a subscript and you have the formula (DO NOT include charges & DO NOT write 1s)

CuCO3 Copper (II) Carbonate Cu+2 CO3-2 1. Write the ions that make up the compound Copper (II) Carbonate 2. Do the charges add to equal zero? No – go to 3; Yes – go to 4. Cu+2 CO3-2 3. Add ions as needed so the compound has a charge of zero CuCO3 4. Write the number of each ion as a subscript and you have the formula (DO NOT include charges & DO NOT write 1s) *If you have more than 1 of a polyatomic ion, you must put the ion in parenthesis*

Co2O3 Cobalt (III) oxide Co+3 O-2 Co+3 O-2 O-2 1. Write the ions that make up the compound 2. Do the charges add to equal zero? No – go to 3; Yes – go to 4. Co+3 O-2 Co+3 O-2 3. Add ions as needed so the compound has a charge of zero O-2 4. Write the number of each ion as a subscript and you have the formula (DO NOT include charges & DO NOT write 1s) Co2O3

Write the formula for the following: Tin (II) Nitrate Iron (III) Phosphate Copper (I) Oxide Sn2+ NO3- Sn(NO3)2 Fe3+ PO4-3 FePO4 Cu+ O-2 Cu2O

Naming * ALWAYS name the cation first and the anion second * Cation – metal name (charge of metal) *** you must determine the charge of the metal and use that after the name*** * Anion – 1. if nonmetal change end of name to -ide 2. if polyatomic ion use the name

FeCl3 Iron (III) chloride Cl- Fe+? Cl- Cl- Name the following: 1. Name the metal 2. Use a Roman Numeral to show the charge of the metal (because Type II) Use the anion and the number of atoms in the formula to determine the charge Cl- Fe+? Cl- The anion side has a total charge of -3 Cl- There is only one cation so it must have a charge of +3 to cancel the charge of the anion side -3 3. Name the anion

Fe3P2 Iron (II) phosphide Fe+? P-3 Name the following: 1. Name the metal 2. Use a Roman Numeral to show the charge of the metal (because Type II) USE the anion and the number of atoms in the formula to determine the charge Fe+? P-3 The anion side has a total charge of -6 -6 There are three cations so each must have a charge of +2 to cancel the charge of the anion side 3. Name the anion

Name the following CuSO4 VCl5 Fe2O3 Cu?+ SO42- Copper (II) Sulfate If there is one SO4 with a (-2) charge, the one Cu must have a (+2) to balance it CuSO4 VCl5 Fe2O3 Cu?+ SO42- Copper (II) Sulfate If there are five Cl’s with a (-1) charge each, the one V must have a (+5) to balance the (-5) from Chlorine V?+ Cl- Vanadium (V) Chloride Three O’s with a (-2) charge add up to -6. There are two Fe’s to cancel it out. Each Fe must have a (+3) to balance it. Fe?+ O2- Iron (III) Oxide