Instructions 1.Show all notes below to your chemistry instructor (they must be in your Chemistry folder—you may have taken these notes in a previous class period) 2.Write both the name and the formula for each of 1-23 below (problems are on colored slides)

Use the diagram and instructions to make a foldable. REMEMBER:THIS FOLDABLE CAN BE USED ON QUIZZES! Fold, staple and cut paper as shown at right (Cuts are shown with dashed lines) Title foldable “Rules for Compound Names and Formulas” and “Ionic Compounds”, “Acids” and Covalent Compounds” in spaces shown at right. Label flaps “Naming Rules”, “Formula Rules” and “Examples” on flaps as shown (1 pt. placement, 1 pt. color, 1 pt. neatness—use light pencil lines for straight labels) On “Naming” flaps, write rules for naming ionic, acid, and covalent compounds given in notes. Include both binary and ternary rules. (3 pts.) On “Formulas” flaps, write rules for writing formulas for ionic, acid, and covalent compounds given in notes. Include both binary and ternary formulas (3 pts.) On “Example” flaps, write as many specific compound name and its formula for ionic, acid, and covalent compounds as you want. Include both binary and ternary examples (3 pts.) Rules for Compound Names and Formulas Ionic (has a Metal) Acids (Hydrogen and nonmetal and (aq) written) Covalent (two nonmetals) Naming Rules Formula Rules Examples of names and formulas Cut here Your name here

Airbags Unit Goals 1.Learn How balanced equations are used to design AIRBAGS. 2.Learn why some reactions go fast (as with AIRBAG inflation) and some go slow (making hydrogen gas) 3.Use a balanced equation to calculate the AMOUNT of GAS needed to fill an AIRBAG. SHORT-TERM GOAL Learn to name and write formulas for compounds used in AIRBAGS and in other chemical reactions 1.Notes on rules for naming/writing formulas for compounds (10 pts.) 2.Summarize Compound Naming/Formulas notes on a foldable. (10 pts.) 3.Use Compound Naming/Formulas FOLDABLE to take a quiz (20 pts.)

Naming Ionic Compounds Ionic compounds are made up of what two types of compounds? Metal (always written first) and nonmetal. For Ionic names write the metal name FIRST then the nonmetal name with and “–ide” ending. For example NaCl is named— Sodium chloride Not sodium chlorine

Write Formulas with Names 1.AlCl 3 2.K 3 N 3.Mg 3 P 2 4.For transition metals indicate the charge with a roman numeral 5.FeCl 3 6.CuF 2

Writing Ionic Formulas For example sodium azide (sodium nitride)—the compound used to create nitrogen gas for airbags. Write the symbol for the metal first and then the symbol for the nonmetal Write charges of these ion taken from the periodic table or your “IONS” sheet Criss-cross! Na N

Writing and Naming Ionic Compounds with Polyions What is a polyion? An ion made up covalently bonded elements (usually oxygen) that ionically gains electrons to have a complete octet and be more stable (less reactive) For example sulfate,SO 4 -2 (not sulfide, S 2- ) Show stability using Lewis structure— 30 valence electrons total (5 elements x 6 valence each for these group 6 atoms) Sulfur is in the middle of the skeletal structure Place bonding electron pairs then fill in rest Two electrons short of an octet for all Two more electrons come from a metal (an ionic bond) to make it a 2- ion O O S O O Iron II Fe

Write Names and Formulas of compounds below 7.Calcium phosphide 8.Aluminum sulfide 9.Magnesium oxide (charges the same? Don’t bring down) 10.Tin II chloride (use roman numeral to determine charge of transition element) 11.Iron III nitride

Writing and Naming Ionic Formulas with Polyions Same rules as BINARY (compounds with two atoms) ionic compounds. See “Ions” sheet for full list of polyion names and formulas. For example calcium phosphate Write the symbol for the metal first and then the symbol for the nonmetal Write charges of these ion taken from the periodic table or your “IONS” sheet Criss-cross! BUT use parenthesis around polyions ALWAYS. Ca PO ( ) 2

Writing Ionic Formulas with Polyions--Examples 12.Sodium carbonate 13.Aluminum sulfate 14.Iron III phosphate 15.Copper I bicarbonate 16.Calcium phosphide 17.Chromium IV borate 18.Magnesium chlorate Learn the strategies by practicing them to get the correct answer. You wont practice the strategies by copying the correct answer from this slide.

Polyions Have Great Structure! Don’t Change the Subscripts! O O P O O Iron III Fe Because: 1.All atoms, the nonmetals that share electrons and the metal that loses electrons, ALL HAVE AN OCTET! 2.Tetrahedron shape is also stable

Writing and Naming Acids—Binary and Ternary Acids can be recognized by the “H-” on the front of the formula and (aq) beside it and by the word “acid” in the name. Binary Acid Formulas—have a “H”, ONE other nonmetal, and (aq)— aqueous—since almost all acids are water solutions. Name BINARY ACIDS by adding “hydro-” to the other nonmetal name and adding “-ic” to the end. –H 2 S (aq) –is hydro-sulfur-ic –HCl (aq) –is hydro-chlor-ic Write BINARY ACID formulas by simply adding as many “H’s” in front of the other nonmetal as the charge indicates –Hydrobromic acid –Is HBr (aq) since Br is a -1 ion –Hydrophosphoric acid –Is H 3 P (aq) since P is a -3 ion

Writing and Naming Acids—Binary and Ternary Ternary Acids—have “H-” and MORE THAN ONE other nonmetal (one of the polyions on your “Ion” sheet). –Name by changing the ending of the other nonmetal name. –Change polyions names ending with “-ate” to “-ic” –Change polyion names ending with “-ite” to “-ous” – DO NOT ADD “hydro-” TO THE FRONT OF THE NAME! –H 2 SO 4 (aq) –is sulfur-ic no “hydro-” in front! –HClO 2 (aq) –is chlor-ous Write formulas as you would a binary acid—with as many “H’s” on front as the charge of the polyion –Phosphorous acid –H 3 PO 3 (aq) because the name has no “hydro-” in front and because “- ous” acids are made from “-ite” polyions. The PO 3 is a -3 ion so there are 3 H+ bonded to this ion. Always put (aq) next to an acid formula.

Writing and Naming Covalent Compounds We’ll learn binary (compounds with 2 types of elements) ONLY To name these –Use prefixes before element names to indicate number of atoms –Slap an “-ide” on the end of the name –For example SO 2  sulfur dioxide 19.CO 2 –Hint (“mono-” prefix is not used with first element) 20.CO –Hint (“mono-” prefix is used with first element) 21.P 4 O 8 21.To write formulas use prefixes in the name to determine subscripts –For example Pentanitrogen heptaphosphide –N5P7–N5P7 22. Dinitrogen heptafluoride 23, triphosphorous hexachloride Covalent Compound Prefixes (pg. 95 of text) Mono- 1 atom Di- 2 atom tri- 3 atom tetra- 4 atom penta- 5 atom hexa- 6 atom hepta- 7 atom octa- 8 atom nona- 9 atom deca- 10 atom

Foldable Activity—12 pts. (This foldable can be used on the quiz!) Fold, staple and cut paper as shown at right (Cuts are shown with dashed lines) Title foldable “Rules for Compound Names and Formulas” and “Ionic Compounds”, “Acids” and Covalent Compounds” in spaces shown at right. Label flaps “Naming Rules”, “Formula Rules” and “Examples” on flaps as shown (1 pt. placement, 1 pt. color, 1 pt. neatness—use light pencil lines for straight labels) On “Naming” flaps, write rules for naming ionic, acid, and covalent compounds given in notes. Include both binary and ternary rules. (3 pts.) On “Formulas” flaps, write rules for writing formulas for ionic, acid, and covalent compounds given in notes. Include both binary and ternary formulas (3 pts.) On “Example” flaps, write as many specific compound name and its formula for ionic, acid, and covalent compounds as you want. Include both binary and ternary examples (3 pts.) Rules for Compound Names and Formulas Ionic (has a Metal) Acids (Hydrogen and nonmetal and (aq) written) Covalent (two nonmetals) Naming Rules Formula Rules Examples of names and formulas Cut here Your name here