6.3 Naming Compound and Writing Formulas Key Concepts: 1. What information do the name and formula of an ionic compound provide? 2. What information do the name and formula of a molecular compound provide?

I. Naming Binary Ionic Compounds A. Compound made from only two elements B. Name of the cation first, then the name of the anion. C. Name of the anion ends in the suffix “ide.” See Table 16 on p. 171

I. Naming Binary Ionic Compounds D. Examples- Name the following MgBr 2 ________________________________ Al 2 S 3 ______________________________ CaCl 2 ______________________________ AlCl 3 ______________________________

II. Naming Binary Compounds with Metals with Multiple Ions A. Many transition metals that form more than one type of ion. B. Show the charge of the cation when naming the compound. C. Use Roman numerals in parenthesis to show the charge of the cation. D. See Table 17 on p. 172 or periodic table in your planner

II. Naming Binary Compounds with Metals with Multiple Ions E. Examples- Name the following: Cu 2 O________________________________ FeF 3 ________________________________ Mn 2 O 7 ________________________________ NiBr 3 ________________________________

III. Naming Binary Compounds with Polyatomic Ions A. Covalently bonded group of ions that has a positive or negative charge and acts like a unit. B. Most polyatomic ions are anions. C. May need to use parenthesis to show how many of each polyatomic unit is in the compound. D. See the Table 19 on page 173- Tape the hand out into your planner.

III. Naming Binary Compounds with Polyatomic Ions E. Examples- Name the following: Na 2 CO 3 ________________________________ Be (OH) 2 ________________________________ KClO 3 ________________________________ NH 4 OH ________________________________

IV. Writing Formulas for Ionic Compounds A. Overall charge must equal zero. B. To write the chemical formula for an ionic compound: 1. Write the element symbol of the cation first, then anion. 2. Write the charge with the number first then the sign. *Write the formula for lithium oxide Li 1+ O 2-

IV. Writing Formulas for Ionic Compounds 3. Use subscripts to indicate the number of ions needed to balance the charges. 4. Use the crisscross method to determine correct subscripts.

IV. Writing Formulas for Ionic Compounds 5. Examples: a. Write the formula for aluminum nitride. Step 1: Need the symbol & charge for each element in the compound. Step 2: Write each ion beside each other.

IV. Writing Formulas for Ionic Compounds Step 3: Crisscross the value (not the sign) of the subscripts. *Check – does the overall charge = 0? Step 4: Rewrite the formula without superscripts. If both subscripts are the same, simplify to 1:1 ratio)

IV. Writing Formulas for Ionic Compounds b. Write the chemical formula for rubidium iodide.

IV. Writing Formulas for Ionic Compounds c. Write the chemical formula for barium fluoride.

IV. Writing Formulas for Ionic Compounds d. Write the chemical formula for tin (IV) oxide.

IV. Writing Formulas for Ionic Compounds e. Write the chemical formula for cobalt (II) bromide.

IV. Writing Formulas for Ionic Compounds f. Write the chemical formula for calcium phosphate.

IV. Writing Formulas for Ionic Compounds g. Write the chemical formula for ammonium sulfate.

V. Molecular Compounds A. Most metallic element appears first in the name. 1. Farther to left on the periodic table 2. Closer to the bottom, if both are in the same group. B. Rules for naming: 1. Use prefixes that tell how many of each atom are in the compound. See Table 20 p. 175 (must know!!) 2. Use suffix “-ide” for the name of the second element.

V. Molecular Compounds C. Name the following: CCl 4 ________________________________ SO 2 ________________________________ P 4 S 5 ________________________________ AsF 5 ________________________________ N 4 O ________________________________

V. Molecular Compounds D. Write the formula for the following: Chlorine trifluoride ______________________ Beryllium dichloride ______________________ Iodine pentafluoride ______________________ Diphosphorus pentoxide ______________________