Naming Compounds

Name:Unit 3:1Period:Naming CompoundsHow to use this chart—Determine what thecompound is made of andfollow the arrows. Thechart will tell you how toname the compound.Exception—O2 is “peroxide” and canmake polyatomic compounds with only 2 elements! O2 with a non-metalis dioxide. O2 with a metalOR Hydrogen (acting as ametal) is peroxide.What’s it Made of?Metal andnon-metalioniccompoundUSE “- IDE” ENDING(NO PREFIXES!)Name the metal and non-metaland change the ending to “ide”.Li2SMetal and non-metal— ionic2non-metals3 or moreelementscovalentcompoundUSE GREEK PREFIXESPut prefixes in front of element names totell how many atoms are there.Don’t use “mono” for first name,but always for second name.N 2O 42 non-metals—covalentLithium Sulfide(not dilithium sulfide—no prefixes for ionic compounds)Why are ionic compounds so easyto name? Because most ioniccompounds can only form oneway, using the oxidation numbers.In covalent compounds, though,non-metals can sometimes combine in multiple ways (carbonmonoxide; carbon dioxide). So,covalent compounds use prefixes.(di 2 and tetra 4)“Dinitrogen tetroxide”polyatomiccompoundCHECK THE CHART BELOW(NO PREFIXES!)Use the names on the chart.If the polyatomic ion is the cation end thesecond name with “-ide”.NaNO33 elements — polyatomicCheck chart (see below)Na - sodiumNO3 - nitrate (on chart)Sodium nitratePolyatomic IonsGreek PrefixesOxidation #NameFormula1 ammoniumNH4 HCO31-1 NO31-2-peroxideO22-Tricycle – 3 wheels3-phosphatePO43-Pentagon – 5 five sided militarybuilding in Washington, D.C.2-sulfateSO42-2-sulfiteSO32-Mono - 1Di – 2Tri – 3Tetra – 4Penta – 5Hexa – 6Hepta – 7Octa – 8Nona – 9Deca – 10Hints to remember prefixes:Transition Metals Can Have MoreThan One Oxidation NumberIron (II) has an oxidation number of 2 Iron (III) has an oxidation number of 3 .When naming them you must specifyWHICH ONE.FeO—Iron (II) oxideFe2O3— Iron (III) oxideMonorail – one rail trainMonocle – glasses for one eyewith only a single lens.Dilemma – strugglebetween 2 choices.Octopus – 8 legsH3O Decade – 10 yearscstephenmurray.comLegal copying of this worksheet requires written permission.Copyright 2009, C. Stephen Murray

Name:Unit 3:1Period:Metal orNon-metal?NMIron OxideIonic orCovalent?IonicUse the Polyatomic Ion Chart onthe front of the worksheet toname these Polyatomic Ions:Name These Ionic CompoundsMgF2Magnesium Fluor-ideLi2OLithium Ox-HCO31-Hydrogen carbonateNaClSodium Chlor-SO42-O22-SO32-NO31-NH4 CrO42-OH1-PO43-CO32-Barium ChlorideCarbon DioxideK 2OPotassium Ox-Magnesium OxideCaSSulf-BeI2Iod-AlBr3Brom-CaF2MgOLiClAluminum FluorideNitrogen TribromideChromium FluoridePotassium OxideDefine these Greek Prefixes1. CO2A. Carbon monoxideName These Covalent CompoundsPenta Tetra 2. C2O4B. Carbon dioxideSi2O3Disilicon oxideNona Hexa 3. C3O5C. Dicarbon monoxideN3Cl4nitrogen tetrachlorideMono Hepta 4. COD. Tricarbon pentoxideSO2Sulfur oxideOcta Deca 5. C2OE. Dicarbon tetroxidePO5Phosphorous oxTri Di 6. CO8F. Carbon octoxideS2F4sulfur fluorName these Polyatomic Compounds(Remember — no prefixes!)Classify and Name These CompoundsIonic, Covalent, or PolyatomicNameCaSO4Calcium1. BaCl2K2CO3carbonate2. COCuNO3Copper (I)3. Ag2ONH4Clchloride4. K2SO4Mg(NO3)2Magnesium5. MgBr2K3PO4Potassium6. SO3Li2(CrO4)Lithium7. P2O4Mg(OH)2M H8. Be(CrO4)Al(PO4)A P9. LiFK(NO3)11. CO2Ca2SO312. OF2cstephenmurray.comIonicLegal copying of this worksheet requires written permission.Barium chlorideCopyright 2009, C. Stephen Murray

Name:Period:cstephenmurray.comLegal copying of this worksheet requires written permission.Copyright 2009, C. Stephen Murray

Name:Unit 3:2Period:Oxidation Numbers, Notation, Lewis Dot DiagramsThe oxidation numbers tell you how many electrons an element will gain or lose.This tells you how it will combine with other elements.Oxidation NumbersOxidation Numbers1Atoms gain or loseelectrons when nearcertain otherelements to fulfillthe octet rule:“If I 8 I full”.Full electron levelsare more stable. Ifan atom has 1 or 2valence electrons itwill lose them tohave a full innerlevel. If an atom has6 or 7 valenceelectrons, it willgain electrons to fillan electron level.1A1H232A3Li4Be11Na12Mg19K20Ca12Dividesmetals andnon-metalsTransition Metals(Oxidation #s vary)(Positive Ions)NotationCharge(Oxidation #)1 Na 24Positive becausethey LOSEelectrons.-2-12 33As34Se35Br36Kr34-3-2-10The elements incolumn 18A (theNoble Gases) havean oxidation # of 0.This means theydon’t gain or loseelectrons, so theydon’t react orform compounds.They are INERT.Negative becausethey GAINelectrons.Non-metals(Negative Ions)Losers of electrons become positive(a positive ion).Electrons are negative, so losingnegatives makes it more positive.MgNumberof atomsSubscripts tell youthe number of atomsin a molecule.O2Lost 2 electrons2 Oxygen atomsNo number means 1 atomGainers of electrons become negative(a negative ion).Electrons are negative, so gainingnegatives makes it more negative.The above notation tells you that each ofthe Sodium atoms lost 1 electron.Since there are 2 Sodium atoms, therewere 2 electrons lost (1 each).The charge is the oxidation number.O2–H2OSO4Gained 2 electrons2 Hydrogen atoms1 Oxygen atoms1 Sulfur atom4 Oxygen atomsDot Diagrams (sometimes known as Lewis dot diagrams) are a depiction of an atom’svalence electrons. They are a powerful tool in helping you understand, see, and evenpredict molecular bonding.Lewis Dot DiagramsOpenings show whereelectrons can be gained orshared from other atoms.The dots representvalence electronsNeOOpenNeon has 8 valence electronsand no openings. Neon hasfulfilled the octet rule and willnot react with other atoms.Oxygen has 6 valenceelectrons, so it wants2 more to be full.X’s can be used tokeep track of electronsfrom other atoms.Electrons can movearound for bonding.Mg MgRightcstephenmurray.com-313A 14A 15A 16A 17AMetalsChemicalsymbol0Also rightMagnesium has 2 valenceelectrons. It will lose them toa non-metal and become apositive ion.Legal copying of this worksheet requires written permission.Li ClThe x shows that Lithiumgives its one valence electronto Chlorine. Chlorine nowhas 8 and is full.Copyright 2009, C. Stephen Murray

Name:Unit 3:2Period:1. Oxidation #sA. Show the number of atoms in amolecule.1. MetalsA. Elements in column 18A that don’tcombine into molecules.2. Negative ionB. An atom that lost electrons.2. Nonmetals3. Positive ionC. Shows the number of electronscommonly gained or lost.3. Octet RuleB. The oxidation numbers of theseelements can vary.D. Way to show an atom’s valenceelectrons to visualize bonding.4. Noble GasesD. Elements that gain electrons.5. TransitionMetalsE. Atoms tend to be more stable with8 valence electrons.4. Subscript5. Lewis DotDiagramsE. An atom that gains electrons.C. Elements that lose electrons.Give abbreviations and oxidation numbersGive these elements with oxidation # in ion notationCalcium (Ca) 2O2–.Carbon ( )Oxygen (O).Fluorine ( )Potassium ( )Nitrogen ( )Nitrogen ( )Lithium ( )Chlorine ( )Hydrogen ( )Beryllium ( )Hydrogen ( )Helium ( )Magnesium ( )Silicon ( )Calcium ( )Aluminum ( )Krypton ( )Boron ( )Bromine ( )MgCl2 How many Chlorines?MgCl2 How many total atoms?Li2O How many Oxygen?Al2O3 How many Aluminums?Li2O How many total atoms?Al2O3 How many total atoms?C12H22O11 How many Hydrogens?CO2 How many Carbons?C6H12O6 How many total atoms?CO2 How many total atoms?H2O How many Hydrogens?H2O How many total atoms?How many electrons are gained or lost?Na1 Lost 1Cu2 3 AlCl1-2ON3-0HeSi4 Draw the Lewis Dot Diagrams for the LithiumFluorineGive abbreviations and valence electronsOxygen (O ).6Silicon ( )Lithium ( )Nitrogen ( )Bromine ( )Hydrogen ( )Helium ( )Magnesium ( )Aluminum ( )Neon ( )Draw 3 different Lewis Dot Diagrams for Nitrogen.Which of these is incorrect?A.BeD.C.B.BeBeBePut boxes around any electrons openingsOcstephenmurray.comFCDraw Lewis Dot Diagrams for Lithium and Oxygen, then putthem together to find how they combine.LithiumOxygenCombinedKLegal copying of this worksheet requires written permission.Copyright 2009, C. Stephen Murray

Name:Period:cstephenmurray.comLegal copying of this worksheet requires written permission.Copyright 2009, C. Stephen Murray

Name:Unit 3:3Period:Ionic CompoundsOpposite Ions AttractIon Charges AddAn ion is an atom with a positive or negativecharge because it has gained or lost electrons.With multiple ions, their charges add together.Just as with protons and electrons: oppositelycharged atoms attract. Positive ions (metals) attractnegative ions (nonmetals), forming ionic compounds.Oxidation NumbersPositive ions attract Negative ionsNa1 Na1 2 chargeSo Na1 2 2 chargePositiveion of 2 Ions makeioniccompounds.Each Sodium atom gives up 1 electron,so 2 Sodium atoms (Na2) will give up2 electrons and have a charge of 2 .Electron arrows are an easyway to visualize electronsbeing given or accepted byatoms.Losing 1 electronHow do elements combine to formcompounds? Elements rarely occurnaturally as individual atoms. Instead,each sample of an element contains ahuge number of atoms! When placedtogether most elements will begin tolose electrons (becoming a positive ion)or gain electrons (becoming a negativeion). The positive ions are attracted tonegative ions and combine into ioniccompounds.K1 As atoms combine into compounds, eventually one element will run out first. Thisis the limiting reactant, the reactant that islimited in amount. When one element isgone, the reaction will stop.When the wood is allburned, the fire willstop. Wood is the limiting reactant becausethere is still oxygen.F1-K1 KSulfur’s oxidation number is 1,so it will gain 1 electron.O2 When elementscombine there area lot of atoms of eachelement. Each atomwill gain or lose electrons according to itsoxidation number.1 O2 O2 O2 O2 O2 Each oxygen gains2 electrons.K1 K1 K1 O2 Oxygen is not full, so itwill attract another K.O2 Oxygen is now full and thecompound is balanced.Each oxygen will attract two potassiums, sopotassium and oxygen will always combine as K2O.F1 Mg1 Limiting ReactantTwo F1– for every Mg2 Each potassiumloses 1 electron.Ionic compounds always combine in aparticular ratio (same number of eachatom) so that they are balanced.The net charge must equal zero!cstephenmurray.comK1 K1 K1 Magnesium FluorideMgF2Magnesium’s oxidation numberis 2, so it will lose 2 electrons.An ionic bondK1 Negativeion of 1-Mg2 Gaining 1 electronIonic CompoundsF1-The number of electron arrows comes from the oxidationnumbers. Positives give electrons; negatives receive.The SymbolsElectron ArrowsattractsMg2 Mg1 Mg1 F1 F1 F1 FBalanced Ionic Compound:MgF2: Magnesium Fluoride1 F1 F1 F1 Magnesium and fluorine combine in a 1 to 2 ratio: MgF2. In this simplifiedexample, the 8 fluorine atoms could combine with 4 magnesium atoms.Since there are only 3 magnesium atoms, the magnesium will run out first,making magnesium the limiting reactant. In the real world there are billionsof atoms when they form compounds. Chemists are able to know how manyatoms there are by the weight of the samples.Legal copying of this worksheet requires written permission.Copyright 2009, C. Stephen Murray