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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

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Prefixes you have to know Examples prefix meaning prefix meaning  CO *mono- 1 hex- 6  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

 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)

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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 CO  You can NOT break these apart in this 2 3 Nitrite NO - Hypochlorite ClO- Dichromate Cr O 2- section. 2 2 7 CN- - 2- Iodate IO3 Chromate CrO4

 the “ide” suffix only applies to - - 2- 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

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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 ), not an acid.

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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

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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

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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

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