09+Bonding+and+Naming+Compounds

=Objectives= __Chapter IX: Section I:__ __Chapter IX: Section II:__ __Chapter IX: Section III:__ __Chapter IX: Section IV:__
 * How are the charges of Group A metal and nonmetal ions related to their positions in the periodic table?
 * How are the charges of some transition metal ions determined?
 * What are the two endings of the names of most polyatomic ions?
 * How are the names of binary ionic compounds determined?
 * How do you write the formulas for binary ionic compounds?
 * How do you write the formulas and names of compounds containing polyatomic ions?
 * What does a prefix in the name of a binary molecular compond tell you about the compound's composition?
 * How do you write the formula for a binary molecular compound?
 * What are the three rules for naming acids?
 * How are the formulas of acids determined?
 * How are bases named?

=Outlined Notes= =Objectives= =9.1 Naming Ions= __**Monatomic Ions**__ Monatomic Ions: Ions consisting of a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons, respectively. __Cations__ __Anions__ __Ions of Transition Metals__ Polyatomic Ions: Ions composed of more than one atom.
 * When the metals in Groups 1A, 2A, and 3A lose electrons, they form cations with positive charges equal to their group member.
 * The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number.
 * The charges of the cations of many transition metal ions must be determined from the number of electrons lost.
 * __Polyatomic Ions__**
 * The names of most polyatomic anions end in -//ite// or -//ate//

I. Binary Ionic Compounds 1. Naming Binary Ionic Compounds a. binary compound- composed of two elements and can be either ionic or molecular b. To name any binary ionic compound, place the cation name first, followed be the anion name. 2. Writing Formulas for Binary Ionic Compounds a.Write the symbol of the cation and the anion. Add whatever subscripts are needed to balance the charges. II. Cmopounds with Polyatomic Ions A. Write the symbol for the cation followed be the formula for the polyatomic ion and balance the charges. 1. Naming Compounds with Polyatomic Ions a. To name a compound containing a polyatomic ion, state the cation first and then the anoin just as you did in naming binary ionic compounds.
 * 9.2 Naming and Writing Formulas for Ionic Compounds**

I. Naming Binary Molecular Compounds A. A prefix in the name of a binary molecular copound tells how many atoms of an element are present in each molecule of the compound. II. Writing Formulas for Binary Molecular Compounds A. Use the prefixes in the name to tell you the subscript of each element in the formula. Then write the correct symbols for the two elements with the appropriate subscripts.
 * 9.3 Naming and Writing Fromulas for Molecular Compounds**

I. __Acids__ A. compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water 1. example: hydrochloric acid, sulfuric acid, malic acid, nitric acid //Naming Common Acids // __Anion Ending :__ __Example: __ __Acid Name: __ __Example: __ -ide: chloride: hydro (stem) -ic acid: hydrochloric acid -ite : sulfite: (stem) -ous acid: sulfurous acid -ate: nitrate : <span style="color: rgb(128,0,0);">(stem) -ic acid: <span style="color: rgb(0,128,0);">nitric acid: B. Rules 1. When the name of the anion ends in -ide, the acid name begins with the prefix hydro-. The stem of the anion has the suffix -ic and is followed by the word acid. a. HCl - hydrochloric acid b. H2S - hydrosulfuric acid 2. When the anion name ends in -ite, the acid name is the stem of the anion with the suffix -ous, followed by the word acid. a. H2SO3 - sulfurous acid 3. When the anion name ends in -ate, the acid name is the stem of the anion with the suffix -ic, followed by the word acid. a. HNO3 - nitric acid C. Writing Formulas for Acids 1. Use the rules for writing the name of acids in reverse to write the formulas for acid. //<span style="color: rgb(0,0,128);">Common Acids // <span style="color: rgb(0,128,128);">__Name:__ <span style="color: rgb(128,0,128);">__Formula__ <span style="color: rgb(0,128,128);">Hydrochloric acid: <span style="color: rgb(128,0,128);">HCl <span style="color: rgb(0,128,128);">Sulfuric acid: <span style="color: rgb(128,0,128);">H2SO4 <span style="color: rgb(0,128,128);">Nitric acid : <span style="color: rgb(128,0,128);">HNO3 <span style="color: rgb(0,128,128);">Acetic acid: <span style="color: rgb(128,0,128);">CH3COOH <span style="color: rgb(0,128,128);">Phosphoric acid: <span style="color: rgb(128,0,128);">H3PO4 <span style="color: rgb(0,128,128);">Carbonic acid: <span style="color: rgb(128,0,128);">H2CO3 2. hydrobromic acid: hydro - prefix - ic suffix. Combination of H+ and Br- = HBr D. Names and Formulas for Bases 1. __base__- an ionic compound that produces hydroxide ions when dissolved in water +02. Bases are named in the same way as other ionic compounds. the name of the cation is followed by the name of the anion. 3. To write the formulas for the bases, write the symbol for the metal cation followed by the formula for the hydroxide ion. 4. Balance the ionic charges just as you do for any ionic compound a. example: aluminum hydroxide Al 3+ and OH- = Al(OH)3 IIIII **The Laws Governing Formulas and Names** A. The Laws of Definite and Multiple Proportions 1.
 * 9.4 Acids and Bases-** naming and writing the formula

=Reference Pages= PH Scale






 * ~ Element ||~ Cation ||~ Preferred Name ||~ Other Name ||
 * copper || Cu+ || copper (I) || cuprous ||
 * ^  || Cu2+ || copper (II) || cupric ||
 * iron || Fe2+ || iron (II) || ferrous ||
 * ^  || Fe3+ || iron (III) || ferric ||
 * lead || Pb2+ || lead (II) || plumbous ||
 * ^  || Pb4+ || lead (IV) || plumbic ||
 * mercury || Hg22+ || mercury (I) || mercurous ||
 * ^  || Hg2+ || mercury (II) || mercuric ||
 * tin || Sn2+ || tin (II) || stannous ||
 * ^  || Sn4+ || tin (IV) || stannic ||
 * **Acid** || **Name** || **Anion** || **Name** ||  || **Acid** || **Name** || **Anion** || **Name** ||
 * H2SO4 || sulfuric || SO42- || sulfate ||  || HCl || hydrochloric || Cl- || chloride ||
 * HNO3 || nitric || NO3- || nitrate ||  || HBr || hydrobromic || Br- || bromide ||
 * H3PO4 || phosphoric || PO43- || phosphate ||  || HClO3 || chloric || ClO3- || chlorate ||
 * HC2H3O2 || acetic || C2H3O2- || acetate ||  || HClO2 || chlorous || ClO2- || chlorite ||
 * H2SO3 || sulfurous || SO32- || sulfite ||  || HBrO3 || bromic || BrO3- || bromate ||
 * HNO2 || nitrous || NO2- || nitrite ||  || HBrO || hypobromous || BrO- ||
 * hypobromite =Practice Problems=
 * HC2H3O2 || acetic || C2H3O2- || acetate ||  || HClO2 || chlorous || ClO2- || chlorite ||
 * H2SO3 || sulfurous || SO32- || sulfite ||  || HBrO3 || bromic || BrO3- || bromate ||
 * HNO2 || nitrous || NO2- || nitrite ||  || HBrO || hypobromous || BrO- ||
 * hypobromite =Practice Problems=

=Assignments=

=Practice Problems= **1.** Name the following ionic compounds:

Cr2(SeO4)3 Sr(ClO)2 MnO2 Na2O2


 * 2.** Give the chemical formulas for the following ionic compounds:

cobaltic nitrate vanadium(V) oxide magnesium dihydrogen phosphate ammonium ferrous sulfate hexahydrate

. Name the following covalent compounds:

NO2 NO N2O P4O10


 * 4.** Give the chemical formulas for the following covalent compounds:

hydrogen sulfide dinitrogen tetroxide


 * 5**. Name the following compounds/ions:

Na3N CaCr2O7 HI(aq) H2S(aq) SeO3 SO32-


 * 6.** Give the chemical formulas for the following compounds/ions:

periodic acid potassium superoxide gallium arsenite copper(I) sulfate radium ion ammonium hydrogen phosphate


 * __PRACTICE PROBLEM ANSWERS 1-6__

1.** Name the following ionic compounds:

Cr2(SeO4)3 //**chromium(III) selenate** (Se and S are elements of the same group. Since SO42- is called sulfate, an educated guess is to name the SeO42- selenate.)// Sr(ClO)2 //**strontium hypochlorite**// MnO2 //**manganese(IV) oxide** ( 'manganese dioxide' is not a systematic// //name. The systematic naming method does not use prefixes in naming ionic compounds.)// Na2O2 //**sodium peroxide** (sodium dioxide is incorrect because the anion is a peroxide anion, not an oxide anion.)//
 * 2.** Give the chemical formulas for the following ionic compounds:

cobaltic nitrate //**Co(NO3)3**// vanadium(V) oxide //**V2O5**// magnesium dihydrogen phosphate //**Mg(H2PO4)2** dihydrogen phosphate is H2PO4-// ammonium ferrous sulfate hexahydrate ** (//N// //H4)2Fe(SO4)2�6H2O// **


 * 3.** Name the following covalent compounds:

NO2 //**nitrogen dioxide**// NO //**nitrogen monoxide;** it is commonly called nitric oxide.// N2O //**dinitrogen monoxide;** it is also called nitrous oxide or laughing gas.// P4O10 //**tetraphosphorus decaoxide**//
 * 4.** Give the chemical formulas for the following covalent compounds:

hydrogen sulfide //**H2S** (It is not called dihydrogen sulfide because it takes two H+ to combine with one S2- to make a electrically neutral molecule. No other combination is possible.)// dinitrogen tetroxide //**N2O4**//
 * 5.** Name the following compounds/ions:

Na3N //**sodium nitride**// CaCr2O7 //**calcium dichromate**// HI(aq) //**hydroiodic acid**// H2S(aq) //**hydrosulfuric acid**// SeO3 //**selenium trioxide**// SO32- //**sulfite ion** (it is not sulfur trioxide because it is an anion.)// periodic acid //**HIO4** (Read the name as per-io-dic acid)// potassium superoxide //**KO2** (the cation is K+ and the anion is O2- )// gallium arsenite //**GaAsO3**// copper(I) sulfate //**Cu2SO4** (It takes two Cu+ to go with one SO42- )// radium ion //**Ra2+**// ammonium hydrogen phosphate //**(NH4)2HPO4** (the cation is ammonium = NH4+, the anion is hydrogen phosphate = HPO42-//
 * 6.** Give the chemical formulas for the following compounds/ions:

=Labs= [] Acids and Bases Lab
 * [] Naming Ionic Compounds Lab**

=Sample Test= [] []
 * []**

= = =**Links**= [] [] [] [] [] [] and Sulfur: [] (video) [] [] ||