IONIC COMPOUNDS

12/9 Today you need… The paper from the side table Your polyatomic/d-block chart Quick review  Name the following on a clean sheet of paper (you have 10 minutes): Li2O -C2S4 Be(NO3)2 -AlPO4 Co(OH)2

12/1 Pre-AP Turn in your molecular geometry HW Have a seat and clear your desk Today you will take TWO quizzes. The first one will be another memorization quiz. If you already made an A on this quiz, you are exempted. The second quiz will be a simple one over covalent compounds. You will review on your own and then take the quiz. Today we will continue with naming IONIC compounds. They are different then covalent, so you will need to pay attention when we are learning this.

On a clean piece of paper: 1. NAME : SO2, N2O5, SF6, CBr3 2. FORMULA: As2O5, XeF5, CCl4 3. What are the shapes of SO2, CCl4, CBr3, Br2, BF3 4. List the seven diatomic elements 5. What is another name for a covalent compound? 6. How are electrons BONDED in a covalent compound? 7. How do you think you will be able to tell the difference between covalent and ionic compounds?

12/2 Pre-AP Pick up the paper from the side table and have a seat Take out the periodic table you colored and took notes on yesterday. I will quickly teach you to name and write formulas for binary ionic compounds and ionic compounds that have a d-block metal. HW: Naming Ionic Compounds Part 1 and Part 2

Ionic COMPOUNDS: Compounds made up of a METAL (cation) and a nonmetal (anion). Electrons are TRANSFERRED between the metal and the nonmetal to obtain a noble gas configuration. There are THREE different types of ionic compounds you will learn to name and write formulas for: 1. Binary ionic 2. Ionic compounds containing polyatomics 3. Ionic compounds with the metal located in the d-Block

Monatomic Ions: need to know their trend on the periodic table Ions formed from a single atom Gain or lose electrons to attain a noble gas configuration

Monatomic Ions: Common Charges 1+ Chart with charges of ions on page 205 2+ 3+ NA 3- 2- 1-

NAMING TYPE 1: Binary Ionic Compounds Compounds composed of 2 different elements that are ionically bonded Charges of ions must “cancel out” so the overall charge on the compound is 0. Use the “crisscross method” to write the formula.

Binary Ionic Compunds: Crisscross method Find the formula for a compound formed by the ions of aluminum and oxygen. Write the symbols for the ions side by side, CATION FIRST. Al3+ O2- Cross over the charges by using the number only from each ions’ charge. Make this the subscript for the other ion. Al2O3 Check the subscripts to make sure that they cannot be simplified.

Binary Ionic Compounds: Crisscross Method (swap and drop) Write the formulas for the binary ionic compounds formed between the following elements: Sodium and phosphorus Gallium and nitrogen Na3P GaN

Naming Binary Ionics Combine the names of the cation and anion, cation first. Example: Al2O3 Cation: aluminum Anion: oxide Compound: Aluminum oxide Most elements form only one ion, so you usually don’t have to indicate the charge in the name.

NAMING TYPE 2: ionic compounds with d-Block metals Some elements can form more than one ion. Example: Iron can form a +2 and +3 ion When you name these compounds, you have to indicate which ion is present. If I asked you to write the formula for iron oxide without telling you if it was Fe+2 or Fe+3, then you could write 2 different formulas FeO Fe2O3 Use Roman numerals in parentheses in the name to indicate the charge on the ion. FeO is Iron (II) oxide Fe2O3 is Iron (III) oxide

Pre-AP 12-1 Today you need the papers from the side table AND your answer document We will quiz the last 10 minutes of class over bonding We will review naming binary IONIC compounds and learn to name compounds with the metal in the d-block and compounds containing polyatomic ions

QUICK CHECK: Write the formula: NAME: Lithium flouride Beryllium nitride Strontium bromide NAME: CaCl2 MgO2 K2S N5O10

D-Block ionic compounds Use ROMAN NUMERALS to indicate the charge of the CATION when formula writing. The roman numeral will be written between the cation and anion when naming a compound.

Naming Practice Write the formula Chromium (III) fluoride Iron (III) oxide Tin (II) sulfide Lead (II) chloride

Naming Practice Name the following compounds Cr3N2 CuO CoF3 Ag2S

NAMING TYPE 3: Compounds Containing Polyatomics Chart of polyatomics on page 210. Compounds containing polyatomics are named the same way at binary ionics. Name the cation Name the anion Example: Name the compound AgNO3 Cation: silver Anion: nitrate Compound: silver nitrate

Polyatomic Examples Write the formula for tin (IV) sulfate Cation: Sn+4 Anion: SO42- Formula using crisscross method: Sn2(SO4)4 If you need more than one polyatomic ion, put it in parentheses to avoid confusion! Wrong: Sn2SO44 Right: Sn2(SO4)4

Polyatomic Examples Write formulas for the following ionic compounds: Sodium iodide NaI Calcium nitrite Ca(NO3)2 Copper (II) sulfate CuSO4

Polyatomic Examples Give the names for the following compounds Ag2O Silver oxide KClO3 Potassium chlorate FeCrO4 Iron (II) chromate