8/25/2020 HOMEWORK Do all odd exercises in this book on a AP Chemistry separate sheet of paper. DO NOT WRITE IN THE BOOK. The Ultimate Chemical Equations Handbook Chapter 2 and 3 Naming Chapter 1 Binary Compounds First, determine if you have an ionic Symbols and Nomenclature of the compound or a covalent compound. elements A metal and a nonmetal will form an ionic bond. There is interesting info where the Compounds with Polyatomic ions form elements got their name, but nothing ionic bonds. we will cover. Nonmetals bonding together or Nonmetals and a metalloid form covalent bonds. Covalent bonding is very Covalent bonding is very similar to ionic naming different from ionic naming You always name the one that is least Ionic names ignored the subscript electronegative first (furthest from because there was only one possible fluorine) ratio of elements. Most electronegative last, and gets the Covalent gives several possibilities so suffix “-ide”. we have to indicate how many of each atom is present in the name 1 8/25/2020 Prefixes you have to know Examples prefix meaning prefix meaning CO *mono- 1 hex- 6 carbon monoxide di- 2 hept- 7 CO2 tri- 3 oct- 8 carbon dioxide tetr- 4 non- 9 NI3 pent- 5 dec- 10 nitrogen triiodide * the first atom named does not get the prefix P4O6 “mono-”, it just keeps its original name! tetraphosphorus hexoxide Continuing Naming ionic compounds I4O9 For monoatomic anions only tetriodine nonoxide drop the ending and add “-ide” - S2F10 so F disulfur decafluoride fluoride - 2- 4- IF7 Cl , O , C Iodine heptafluoride chloride, oxide and carbide Si2Cl6 disilicon hexachloride Determining the formula of Continuing… ions cations keep the name of the element. Ionic compounds are neutral When naming compounds always name You need to find the lowest number of the positive (cation) first and the each ion to make it neutral negative (anion) last. for example: + 2- so mixing ions of chlorine and sodium Na and O give you 2 sodium for every one oxygen sodium chloride Na2O (positive) (negative) 2 8/25/2020 Several atoms can form a More examples couple of different ions. 3+ 2- Al and O All of these are metals that are not in Al2O3 group 1, 2 or aluminum. + - 2+ 3+ K and Cl for example iron can form Fe or Fe KCl These are said as iron (II) and iron (III) the subscripts don’t effect the name if + 2+ Cu and Cu is Copper (I) and Copper (II) there is only one possibility still (cation)(anion) Aluminum oxide Potassium chloride Figuring out charge on these elements Examples If the ion is named, the charge is in the name. Copper (II) chloride CuCl If you have the formula, use the charges 2 of the other ions present to determine the Cobalt (III) sulfide charge. Co2S3 Remember NiF2 Alkali will always be +1 Nickel (II) fluoride Alkaline Earth +2, Halogens -1, oxygen TiS2 group -2 titanium (IV) sulfide Aluminum will always be +3 Polyatomic ions Common polyatomic ions + - Sulfate 2- Polyatomic Ions- many atoms in one ion Ammonium NH4 Perchlorate ClO4 SO4 Acetate CH CO - Chlorate - 2- 3 2 ClO3 Sulfite SO3 - - 2- Nitrate NO3 Chlorite ClO Carbonate CO You can NOT break these apart in this 2 3 Nitrite NO - Hypochlorite ClO- Dichromate Cr O 2- section. 2 2 7 Cyanide CN- - 2- Iodate IO3 Chromate CrO4 the “ide” suffix only applies to - - 2- Thiocyanate SCN Bromate BrO3 Oxalate C2O4 monoatomic anions Hydrogen 2- HCO - OH- Silicate SiO3 carbonate 3 Hydroxide - - Phosphate PO 3- Hydrogen sulfate HSO4 Permanganate MnO4 4 Hydrogen HSO - Thiosulfate S O 2- Arsenate AsO 3- sulfite 3 2 3 4 3 8/25/2020 YOU WILL HAVE TO Determining the formula of MEMORIZE THESE! ions This is one of the big differences from last Ionic compounds are neutral year. Remember– don’t break a polyatomic We will have a quiz just like the elements ion apart quiz last year over these! for example: Ammonium carbonate For the summer assignment test you must + 2- NH4 and CO3 have the following memorized (NH4)2CO3 Sulfate, carbonate, chlorate, chlorite, nitrate, hydroxide and ammonium. Chapter 4 acids and salts Oxyanions Oxyanions- negative ions containing Oxyanions may contain the prefix oxygen. “hypo-”, less than, or “per-”, more than. These have the suffix “-ate” or “-ite” For example - “-ate” means it has more oxygen atoms ClO4 Perchlorate bonded, “-ite” has less - ClO3 Chlorate For example - ClO2 Chlorite 2- - SO4 sulfate ClO Hypochlorite 2- SO3 sulfite Acids Naming acids Does it contain oxygen? + Certain compounds produce H ions in If it does not, it gets the prefix “hydro-” water, these are called acids. and the suffix “-ic acid” You can recognize them because the HCl neutral compound starts with “H”. Hydrochloric acid For example HCl, H2SO4, and HNO3. HF Don’t confuse a polyatomic ion with a Hydroflouric acid neutral compound. HCN - HCO3 is hydrogen carbonate (or Hydrocyanic acid bicarbonate), not an acid. 4 8/25/2020 Naming Acids Examples If it does contain an oxyanion, then HNO3 replace the ending. Nitric acid If the ending was “–ate”, add “-ic acid” HI If the ending was “–ite”, add “-ous Hydroiodic acid acid” H3AsO3 H SO Sulfuric Acid 2 4 Arsenous acid H2SO3 Sulfurous Acid Chapter 5 Complex ions Ch 6 Organic Complex ion- transition metal ion with Alkanes- straight chain hydrocarbons attached ligands with all single bonds 3- Fe(CN)6 Alkenes- hydrocarbons with a double 2- bond Ni(SCN)4 Glance over this chapter. Skip the problems, Alkynes- hydrocarbons with a triple most this material is out of the test. bond Cyclic hydrocarbons- rings Name this molecule Root words And give its molecular formula # of C # of C 4 ethyl octane atoms atoms C H Meth 1 Hex 6 10 22 Eth 2 Hept 7 4 propyl decane Prop 3 Oct 8 But 4 Non 9 C13H28 Pent 5 Dec 10 5 8/25/2020 Name and give the formula Functional groups halogenated *R means any carbon chain Alcohols Carboxylic Acids R-OH R-C=O -OH -ol -oic acid Aldehydes Ketones NOT at the edge Methyl cyclohexane at the edge R-C-R R=O =O C7H14 -one -al 2,4 dichloro 3 methyl 3 bromo 2, 2 diethyl 1 hexanal 1 cyclobutanone C10H19BrO C5H6Cl2O 2, 3 dimethyl 2, 2 dibromo 1 cyclohexanol hexanoic acid C6H9Br2OH C7H15COOH Predicting organic reactions example Addition reactions occur by adding 1- butene is reacted with fluorine halogens or hydrogen to alkene or alkynes. In the reaction, the new molecule takes the place of the double or triple bond. C4 H8 + F2 C4H8F2 Cl2 + CH3-CH=CH2 CH3-CClH- CClH2 6 8/25/2020 Predicting organic reactions Predicting organic reactions Substitution reactions occur by Combustion reactions occur when an adding halogens to an alkane. organic compound is burned in oxygen. In the reaction, the new molecule takes The products of a complete combustion the place of a hydrogen. are water vapor and carbon dioxide. Cl2 + CH3-CH3 CH3-CClH2 + HCl C6H12O6 + 6 O2 6 H2O+ 6 CO2 Cl2 + C2H6 C2ClH5 + HCl Predicting organic reactions Examples Esterification reactions Fluorine is added to 2 propene Made by reacting carboxylic acids with alcohols. Ethanol is burned in oxygen Chlorine is added to propane R-C-O-H H-O-R O= + R-C-O-R + H-O-H alcohol Ethanoic acid is reacted with 1-butanol Carboxylic acid O= Ester 7.