INORGANIC Nomenclature - PowerPoint Presentation

INORGANICNomenclature

Nomenclature - Humor“Ferrous Wheel”Fe = iron (Latin = ferrum) Fe 2+ = lower oxidation state = ferr ous Fe3+ = higher oxidation state = ferric BaNa2 “BaNaNa” Fe 2+ Fe 2+ Fe 2+ Fe2+ Fe2+ Fe2+ Fe2+ Fe2+ What weapon can you make from the elements nickel, potassium and iron? A KNiFe

Teacher: What is the formula for water?Student: H, I, J, K, L, M, N, OTeacher: That’s not what I taught you. Student: But you said the formula for water was…H to O. Website: Dihydrogen monoxide Information Campaign mis mis “Little Johnny took a drink, Now he shall drink no more. For what he thought was H 2 O, Was H 2 SO4.” Under aged Pb walks into a bar and the bartender turns to the goldBouncer and says, “Au, get the lead out!” "H-O-H"?! WHAT'S THAT SPELL?! WATER?

Table of Contents‘Nomenclature’Binary Compounds - Metal (fixed oxidation) + NonmetalCriss-Cross Rule Binary Compounds - Metal (variable oxidation) + Nonmetal Binary Compounds - Nonmetal + Nonmetal Ternary Compounds Binary Hydrogen Compounds Meaning of Suffixes Empirical Formulas Subscripts, Superscripts, and Coefficients Centrum Multivitamin Polyatomic Ions

Lecture Outline – Nomenclature Keys Lecture Outline – Nomenclature and Bonding Lecture Outline – Nomenclature and Bonding student notes outline textbook questions http://www.unit5.org/chemistry/Nomenclature.html textbook questions text

Four Types of NamingBinary compoundsTernary compoundsCoordination compoundsOrganic compounds Contain only two types of elements We will cover these in a separate unit These will not be covered Contain more than two types of elements

Binary CompoundsMetals (fixed oxidation) + Nonmetals

ineurine Binary Compounds Binary compounds that contain a metal of fixed oxidation number (group 1, group 2, Al, Zn, Ag, etc.), and a non-metal. To name these compounds, give the name of metal followed by the name of the non-metal, with the ending replaced by the suffix – ide. Examples: NaCl CaS AlI 3 3sodium chlor calcium sulf aluminum iod (Na1+ Cl1-) (Ca2+ S2-) (Al3+ I1-) ide ide ide He 2 C 6 N 7 O 8 F 9 Ne 10 B 5 H 1 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr87 Rf 104 Db105 Sg106 Bh107 Hs108 Mt109 Be 4 Ca20 Sr38 Ba56 Ra88 Mg12 1 2 3 4 5 6 7 * W 1+ 2+ 1+ 2+ 3+

ineurineBinary Compounds Binary compounds that contain a metal of fixed oxidation number (group 1, group 2, Al, Zn, Ag, etc.), and a non-metal. To name these compounds, give the name of metal followed by the name of the non-metal, with the ending replaced by the suffix – ide . Examples: NaCl CaS AlI 3 3sodium chlor calcium sulf aluminum iod (Na1+ Cl1-) (Ca2+ S2-) (Al3+ I1-) ide ide ide

Cations and AnionsCommon Simple Cations and Anions Cation Name Anion Name* H 1+ hydrogen H 1- hydr ide Li 1+ lithium F 1- fluoride Na 1+ sodium Cl 1- chloride K 1+ potassium Br 1- bromide Cs 1+ cesium I 1- iodide Be 2+ beryllium O 2- ox ide Mg 2+ magnesium S 2- sulfide Al 3+ aluminum Ag 1+ silver * The root is given in color. Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86

Ionic Binary Compounds:Single-Charge Cations Keys Ionic Binary Compounds:  Single-Charge Cations Ionic Binary Compounds:  Single-Charge Cations http://www.unit5.org/chemistry/Nomenclature.html

Molecular CompoundSilicon dioxide, SiO2, is a molecular compound. It is also a mineral called quartz (left). Quartz is found in nearly every type of rock. Most sand grains (center) are bits of quartz. Glass is made from sand. A compound containing atoms of two or more elements that are bonded together by sharing electrons.

Criss-Cross Rule

“Perhaps one of you gentlemen would mind telling me just what is outside the window that you find so attractive..?”Image courtesy NearingZero.net

Example: Aluminum ChlorideStep 1: Step 2: Step 3: 1 3 Step 4: AlCl 3 Criss-Cross Rule Al Cl Al Cl 3+ 1- write out name with space write symbols & charge of elements criss-cross charges as subsrcipts combine as formula unit (“1” is never shown) Aluminum Chloride

Example: Aluminum ChlorideStep 1: Aluminum ChlorideStep 2: Al3+ Cl 1- Step 3: Al Cl 1 3 Step 4: AlCl 3 Criss-Cross Rule

Example: Aluminum OxideStep 1: Aluminum OxideStep 2: Al3+ O 2- Step 3: Al O 2 3 Step 4: Al 2 O 3Criss-Cross Rule

Example: Magnesium OxideStep 1: Magnesium OxideStep 2: Mg2+ O 2- Step 3: Mg O 2 2 Step 4: Mg 2 O 2Step 5: MgO Criss-Cross Rule

Naming Binary CompoundsFormula Name BaO ____________________________________ sodium bromide MgI 2 ____________________ KCl ____________________ ________________ strontium fluoride ________________ cesium fluoride barium oxideNaBr magnesium iod ide potassium chloride SrF2 CsF

Rules for ParenthesesParentheses are used only when the following two condition are met: There is a radical (polyatomic ion) present and… There are two or more of that radical in the formula. Examples: NaNO 3 NO31- is a radical, but there is only one of it. Co(NO3)2 NO 31- is a radical and there are two of them (NH4 )2SO4 NH 41+ is a radical and there are two of them; SO42- is a radical but there is only one of it. Co(OH)2 OH1- is a radical and there are two of it. Al2(CO3)3 CO32- is a radical and there are three of them. NaOH OH1- is a radical but there is only one of it.

Ions in Chemical Formulas Keys Ions in Chemical Formulas Ions in Chemical Formulas Ions in Chemical Compounds - Grid http://www.unit5.org/chemistry/Nomenclature.html Ions in Chemical Compounds - Grid

Hungry for Tater Tots?Mr. C at 7 years old.

Ions in Chemical Compounds - GridIons in Chemical Compounds Keys http://www.unit5.org/chemistry/Nomenclature.html Ions in Chemical Compounds - Grid

Chemical Bonding& NomenclatureGeneral Chemistry Notes

Chemical Bonding …atoms share electrons to get a full valence shell Covalent Bonds C 2s 2 2p 2 (4 v.e – ) F 2s 2 2p 5(7 v.e –) both need 8 valence electrons for a full outer shell(octet rule) 1s2 1s2

Covalent bonding F F Fluorine has seven valence electrons A second F atom also has seven By sharing electrons Both end with full orbitals (stable octets) 8 Valence electrons 8 Valence electrons

Chemical BondingIonic Bonds: atoms give up or gain electrons and are attracted to each other by coulombic attraction Na loses an e – Na  Na 1+ + e – Cl gains an e –Cl + e –  Cl 1–ionic compounds = salts Na1+ + Cl 1–  NaCl K1+ + NO31–  KNO 3where NO 3 1– is a polyatomic ion : a charged group of atoms that stay together

Formation of Cation 11 p + sodium atom Na e - loss of one valence electron e - e- e- e- e- e- e- e- e- e - sodium ion Na + 11 p + e - e - e - e - e - e - e - e - e - e - e -

Formation of Anion 17 p + chlorine atom Cl e - e - e - e - e- e- e- e- e- e- e- e - e - e - e - e - e - e - gain of one valence electron chloride ion Cl 1- 17 p + e - e - e - e - e - e - e - e - e - e - e - e - e - e - e - e - e - e -

Formation of Ionic Bondchloride ionCl1-sodium ionNa + 11 p + e - e - e - e - e- e- e- e- e- e- 17 p + e - e - e - e - e - e - e - e - e - e - e - e - e - e - e - e - e - e -

Ionic Bonding - - - - - - - - - - - - - - - - n = 2 Na [Ne]3 s 1 n = 3 n = 3 + - - - - - - - - - - - - - - - - Cl [Ne]3 s 2 3 p 5 Na + [Ne] Cl - [Ne]3 s 2 3 p 6 NaCl Transfer of electrons to achieve a stable octet (8 electrons in valence shell).

Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.Na + Cl 2 NaCl sodium metal and chlorine gas react to form sodium chloride 2 2

Covalent Bonding - - - - n = 1 O [He]2 s 2 2 p4 n = 2 + - - - - - - - O 2 Sharing of electrons to achieve a stable octet (8 electrons in valence shell). - - - - - - - - - - - - - - - - - O [He]2 s 2 2 p 4

Properties of SaltsVERY HARD each ion is bonded to several oppositely- charged ions HIGH MELTING POINTS many bonds must be broken BRITTLE with sufficient force, like atoms are brought next to each other and repel

VocabularyChemical Bondattractive force between atoms or ions that binds them together as a unitbonds form in order to…decrease potential energy (PE)increase stabilityCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

VocabularyCHEMICAL FORMULAmolecular formula formula unit IONIC COVALENT CO 2 NaCl Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

VocabularyCOMPOUNDternary compound binary compound 2 elements more than 2 elements NaNO 3 NaCl Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

VocabularyIONpolyatomic Ion monatomic Ion 1 atom 2 or more atoms NO 3 - Na + Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

IONICCOVALENT Bond Formation Type of Structure Solubility in Water Electrical Conductivity Other Properties e - are transferred from metal to nonmetal high yes (solution or liquid)yes e- are shared between two nonmetals low no usually not MeltingPointcrystal lattice true molecules Types of Bonds Physical State solid liquid or gas odorous Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

“electron sea”METALLIC bond formation type of structure solubility in water conductivity other properties melting point Types of Bonds physical state electrons are delocalized among metal atoms very high yes (any form) no malleable, ductile, lustrous solid Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Ionic Bonding - Crystal LatticeTypes of Bonds Table salt

Ionic Bonding - Crystal LatticeTypes of Bonds Table salt

Covalent Bonding - True MoleculesTypes of Bonds Diatomic Molecule Ammonia Nitrogen Water

Covalent Bonding - True Molecules Types of Bonds Diatomic Molecule Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem Ammonia Chlorine Water

Lewis StructureLewis structure: a model of a covalent molecule that shows all of the valence electrons 1. Two shared electrons make a single covalent bond, four make a double bond, etc. 2. unshared pairs : pairs of un-bonded valence electrons 3. Each atom needs a full outer shell, i.e., 8 electrons. Exception: H needs 2 electrons

Lewis Structurecarbon tetrafluoride (CF4 ) o C o o o x x x x x x F x o C o o o x x x x x x F x x x x x x x F x x x x x x F x x x x x x x F x x C x x x x x x F x x x x x F x x x x x F x x x x x x F x x covalent compounds = molecular compounds (have lower melting points than do ionic compounds)

Lewis Structureo C o o o x H o C o o o H x x H x H x H C H H H H x x x x x x I x o N o o o o o N o o o x x x x x x I x x x x x x x I x x x x x x I x x o o N x x x x x x I x x x x x I x x x x x I x x o o C o o o x x x x x O x x x x x x O x x x x x x O x o C o o o O = C = O x x x x x x x x methane (CH 4 ) carbon dioxide (CO 2 ) nitrogen triiodide (NI 3 )

Properties of Metals conduct heat and electricity; ductile; malleable Other Types of Bonds dipole-dipole forces hydrogen bonds London dispersion forces ion-dipole forces (solutions)

Writing Formulas of Ionic Compoundschemical formula: has neutral charge; shows types of atoms and how many of each To write an ionic compound’s formula, we need: 1. the two types of ions 2. the charge on each ion Na 1+ and F 1– Ba 2+ and O2– Na 1+ and O2– Ba2+ and F1– NaF BaO Na2O BaF2 sodium fluoride barium oxide sodium oxide barium fluoride

Ca3P2Formula Unit Ca 2+ Ca 2+ Ca 2+ P 3- P 3- Ca 2+ P 3- Ca 2+ P 3- Ca 2+ Ca 2+ and P 3– Ca 3 P 2 calcium phosphide

InBr3BaSCriss-Cross Rule criss-cross rule : charge on cation / anion “becomes” subscript of anion / cation ** Warning: Reduce to lowest terms. Al 2 O 3 Al 3+ and O 2– Al 2 O 3 Ba 2+ and S 2– Ba 2 S 2 In 3+ and Br 1– In 1 Br 3 aluminum oxide barium sulfide indium bromide

(NH4)3N Fe 2 (Cr 2 O7) 3 Sn(SO4)2 NH 4 ClO3 Mg(NO2) 2BaSO 4Writing Formulas w/Polyatomic Ions Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion. Ba2+ and SO4 2– Mg 2+ and NO21– NH 4 1+ and ClO 3 1– Sn 4+ and SO 4 2– Fe 3+ and Cr 2 O 7 2– NH 4 1+ and N 3– barium sulfate magnesium nitrite ammonium chlorate tin (IV) sulfate iron (III) dichromate ammonium nitride ?

Multiple Oxidation States“tin fluoride”tin (II) fluoridetin (IV) fluoride Tin is either 2+ or 4+ oxidation state. Sn 2+ F 1- SnF 2 Sn 4+ F 1- SnF 4 tin (II) sulf ide Sn2+ S2- Sn2S2 SnS tin (II) sulf ate Sn 2+ SO 4 2- SnSO 4 tin (II) sulf ite Sn 2+ SO 3 2- SnSO 3 tin (IV) sulfate Sn 4+ SO 4 2- Sn 2 (SO 4 ) 4 Sn(SO 4 ) 2

Compounds Containing Polyatomic IonsInsert name of ion where it should go in the compound’s name. Write formulas: iron (III) nitrate ammonium phosphide ammonium chlorite zinc phosphate lead (II) permanganate Fe(NO 3 ) 3 (NH4)3 PNH 4ClO2 Zn3(PO4 )2 Pb(MnO4)2 Fe 3+NO 3 1– NH 4 1+ P 3– NH 4 1+ ClO 2 1– Zn 2+ PO 4 3– Pb 2+ MnO 4 1– 3 3 3 2 2

Write names:(NH4)2S 2 O 3 AgBrO 3 (NH4 )3N U(CrO4) 3 Cr 2(SO3)3 Writing Formulas of Ionic Compounds ammonium thiosulfate silver bromate ammonium nitride uranium (VI) chromate chromium (III) sulfite CrO 42– SO32– 3 3 2 Cr U ? ? 6+ 3+

Writing Formulas of Covalent Molecules Covalent Molecules contain two types of nonmetals Key: FORGET CHARGES What to do: Use Greek prefixes to indicate how many atoms of each element, but don’t use “mono” on first element. 1 – mono 6 – hexa 2 – di 7 – hepta 3 – tri 8 – octa 4 – tetra 9 – nona 5 – penta 10 – deca

Writing Formulas of Covalent Molecules EXAMPLES: carbon dioxide CO dinitrogen trioxide N 2 O 5 carbon tetrachloride NI3 CO 2carbon monoxide N2 O3 dinitrogen pentoxideCCl 4nitrogen triiodide

Cu 2 Br1–Cu Br 1– 2 Fe 3 O 2– Fe O2– Stock System of nomenclature 4. Write name of anion. FeO Fe 2 O 3 CuBr CuBr2 iron (II) oxide iron (III) oxide copper (I) bromide copper (II) bromide ? ? ? ? A. To name, given the formula: 1. Figure out charge on cation. 2. Write name of cation. 3. Write Roman numerals in ( ) to show cation’s charge. Pb 2+ /Pb 4+ , Sn 2+ /Sn 4+ , transition elements (not Ag or Zn) Multiple-Charge Cations with Elemental Anions 2+ 3+ 1+ 2+

B. To find the formula, given the name: 2. Balance charges to write formula. cobalt (III) chloride Co 3+ Cl 1– CoCl 3 tin (IV) oxide Sn4+ O 2– SnO2 tin (II) oxide Sn2+ O2– SnO 1. Write symbols for the two types of ions.

Element Latin root -ic -ous gold, Au aur- Au3+ Au1+ lead, Pb plumb- Pb 4+ Pb2+ tin, Sn stann- Sn 4+ Sn2+ copper, Cu cupr- Cu 2+ Cu1+ iron, Fe ferr- Fe 3+ Fe2+ Traditional (OLD) System of Nomenclature …used historically (and still some today) to name compounds w/multiple-charge cations To use: 1. Use Latin root of cation. 2. Use -ic ending for higher charge “ -ous “ “ lower “ 3. Then say name of anion, as usual. ; (“icky” food is good for you!) ; (“delici ous” food is not good for you!)

Cu2SAuN FeF 2 plumbic phosphide plumbous phosphide stannic chloride Fe 2+ Write formulas: Write names: cuprous sulfide auric nitride ferrous fluoride Pb 3 P 43 Pb ? 4 P3– Cu1+ Pb 3 P 2 3 Pb ? 2 P 3– Au 3+ SnCl 4 Sn ? 4 Cl 1– S 2– N 3– F 1– copper (I) sulfide gold (III) nitride iron (II) fluoride lead (IV) phosphide lead (II) phosphide tin (IV) chloride

Bonding Activity

O 2- K 1+ K 1+ Mg 2+ Br 1- Br 1- K Br potassium atom bromine atom e - e - Br 1- K 1+ potassium ion bromide ion potassium bromide K Br potassium atom bromine atom e - Br 1- K 1+ potassium ion bromide ion KBr MgBr 2 K 2 O magnesium bromide potassium oxide

Ca 2+ Al 3+ K 1+ Pb 4+ Br 1- O 2- N 3- K 1+ K 1+ Mg 2+ Br 1- Br 1- PO 4 3- S 2- Cu 2+ OH 1- OH 1- NH 4 1+ NO 3 1- ?

Chemical Bonding Activity Ca 2+ Al 3+ Na 1+ Pb 4+ OH 1- N 2- N 3- M 1+ Mg 2+ OH 1- OH 1- N 3- Pb 4+ N 3- N 3- Pb 4+ N 3- Pb 4+ N 3- ? (nonmetal) M 1+ (metal) Pb 4+ N 3- (metal) (metal) M 2+ (metal) Pb 3 N 4 lead (IV) nitride or plumbic nitride

Chemical Bonding Activity Keys            Chemical Bonding Activity (pink/blue) Chemical Bonding Activity Pieces            Chemical Bonding Activity (pink/blue) Chemical Bonding Activity Pieces http://www.unit5.org/chemistry/Nomenclature.html Power Point

Key Cu 2+ Al 3+ K 1+ Pb 4+ Br 1- O 2- N 3- K 1+ K 1+ Mg 2+ Br 1- Br 1- N 3- N 3- Pb 4+ N 3- Pb 4+ N 3- 1. 2. 3. 4. 5. 6. OH 1- OH 1- NH 4 1+ NO 3 1- 7. KBr K 2 O MgBr 2 AlN Cu(OH) 2 NH 4 NO 3 Pb 3 N 4 http://www.unit5.org/christjs/4bondingact.doc

Key Fe 2+ 8. 9. 10. Ca 2+ Ca 2+ Ca 2+ PO 4 3- PO 4 3- PO 4 3- NH 4 1+ NH 4 1+ NH 4 1+ O 2- Al 3+ Al 3+ O 2- O 2- O 2- 11. Ca 3 (PO 4 ) 2 (NH 4 ) 3 PO 4 FeO Al 2 O 3

Key12. 15. O 2- O 2- Fe 3+ Fe 3+ O 2- O 2- O 2- 13. Pb 4+ S 2- S 2- Pb 4+ S 2- S 2- Pb 2+ S 2- 14. Cu 2+ Cu 1+ Cu 1+ 16. Fe 2 O 3 Pb 2 S 3 PbS CuO Cu 2 O Pb 2 S 4 PbS 2

Binary CompoundsMetals (variable oxidation) + Nonmetals

Binary CompoundsContaining a Metal of Variable Oxidation NumberTo name these compounds, give the name of the metal (Type II cations) followed by Roman numerals in parentheses to indicate the oxidation number of the metal, followed by the name of the nonmetal, with its ending replaced by the suffix –ide. Examples Stock System FeCl 2 (“ic” ending = higher oxidation state; “ous” is lower oxidation state) SnO Tin oxide SnO2 Tin oxide (II) (III) (II) (IV)Traditional (OLD) System Ferrous chloride Ferric chlorideStannous oxide Stannic oxide Iron chlorideIron chloride FeCl3

Type II CationsCommon Type II Cations Ion Stock System Traditional System Fe 3+ iron (III) ferric Fe 2+ iron (II) ferrous Cu 2+ copper (II) cupric Cu 1+ copper (I) cuprous Co 3+ cobalt (III) cobaltic Co 2+ cobalt (II) cobaltous Sn 4+ tin (IV) stannic Sn 2+ tin (II) stannous Pb 4+ lead (IV) plumbic Pb 2+ lead (II) plumbous Hg 2+ mercury (II) mercuric Hg2 2+ mercury (I) mercurous *Mercury (I) ions are always bound together in pairs to form Hg2 2+ Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90

Naming Binary CompoundsFormula Name Hg2O ____________________ HgO ____________________ ________________ copper (II) fluoride ________________ copper (I) sulfide Cr 2 O 3 ____________________________________ lead (IV) oxide mercury (I) oxide PbO2 mercury (II) ox ide CuF2 Cu2S chromium (III) oxide

Li3H1 He 2 C 6 N 7 O 8 F 9 Ne 10 Na11 B 5 Be4 H1 Al13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg 12 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62Eu 63Gd 64Tb 65Dy 66Ho 67 Er68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 La 57 Ac 89 1 2 3 4 5 6 7 * W Single-charge cations Multiple-charge cations Elemental anions 1+ 2+ 1+ 2+ 3+ 1- 2- 3- Periodic Table with charges

Ionic Compounds:Polyatomic Ions with Multiple-Charge Cations Keys           Ionic Compounds:  Polyatomic Ions with Multiple-Charge Cations Polyatomic Ions Grid to Memorize Chart of the Ions and Polyatomic Ions           Ionic Compounds:  Polyatomic Ions with Multiple-Charge Cations http://www.unit5.org/chemistry/Nomenclature.html

Ionic Formulas(Binary, Polyatomic, Transition Metals) Keys Ionic Formula (Binary, Polyatomic, Transition Metals) Ionic Formula (Binary, Polyatomic, Transition Metals) Formulas of Ionic Compounds http://www.unit5.org/chemistry/Nomenclature.html

Ionic Compounds:Traditional System of Nomenclature Keys Ionic Compounds:  Traditional System of Nomenclature Ionic Compounds:  Traditional System of Nomenclature http://www.unit5.org/chemistry/Nomenclature.html

Binary Molecular CompoundsNonmetal + Nonmetal

Binary Compounds Containing Two Nonmetals To name these compounds, give the name of the less electronegative element first with the Greek prefix indicating the number of atoms of that element present, followed by the name of the more electronegative non-metal with the Greek prefix indicating the number of atoms of that element present and with its ending replaced by the suffix –ide . Prefixes you should know: Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca 1 2 3 4 5 6 7 8 9 10

Binary CompoundsContaining Two Nonmetals (Type III Compounds)________________ diarsenic trisulfide________________ sulfur dioxide P 2 O 5 ____________________ ________________ carbon dioxide N2O 5 ____________________ H2 O ____________________As2 S3 SO 2 diphosphorus pentoxideCO 2dinitrogen pentoxide dihydrogen monoxide

Prefixes – Binary Molecular CompoundsGreek Prefixes for Two Nonmetals Number Indicated Prefixes 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

Binary Molecular CompoundsN2O dinitrogen monoxideN2O3 di nitrogen tri oxide N2O5 dinitrogen pent oxideICl iodine monochlorideICl3 iodine trichlorideSO2 sulfur dioxide SO3 sulfur tri oxide

Naming Binary CompoundsBinary Compound?Metal Present? Does the metal form more than one cation? Type III Use Greek Prefixes Type IUse the elementname for the cation. Type IIDetermine the charge of the cation; use a Roman numeral after the cationname. Yes Yes Yes No No Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 98

Covalent Binary Compounds:Nonmetal-Nonmetal Combinations Keys Covalent Binary Compounds:  Nonmetal-Nonmetal Combinations Covalent Binary Compounds:  Nonmetal-Nonmetal Combinations http://www.unit5.org/chemistry/Nomenclature.html

Ternary Compounds

Ternary Compounds Ternary compounds are those containing three different elements. (NaNO3, NH4Cl, etc.). The naming of ternary compounds involves the memorization of several positive and negative polyatomic ions, (two or more atoms per ion), and adding these names to the element with which they combine. i.e., Sodium ion, Na 1+ added to the nitrate ion, NO 3 1-, to give the compound, NaNO3, sodium nitrate. Binary rules for indicating the oxidation number of metals and for indicating the numbers of atoms present are followed. The polyatomic ions that shouldbe learned are listed in a separate handout.

(PO4)3-Phosphate PO 4 3- 1 P 4 O @ 2-= 8- @ 3- = 3- 11- ? @ 5+ = 5+ 3-  Fluorine and oxygen are highly electronegative and will attract electrons very strongly. Generally, phosphorus will be 3- oxidation state: however, when combining with oxygen, phosphorus will lose five electrons and take on a 5+ oxidation charge.

phosphatesulfatecarbonatechloratenitrate Polyatomic Ions - Memorize phosph ATE sulf ATE carbonATEchlorATE nitrATEPO4 3- ……………SO4 2- …………… CO32- …………..ClO 31- …………..NO31- ………..…. Eight “-ATE’s” Exceptions: ammoniumhydroxide cyanideNH 41+ ……………OH1- …………… CN1- …………..

Pattern to Memorizing NomenclatureXY“-ide” XYO 3 “ - ate ” XYO 2 “ - ite” XYO “ hypo___ -ite” XYO 4 “per___-ate ” normal 1 less oxygen 2 less oxygen 1 more oxygen

Polyatomic Ion: a group of atoms that stay together and have a single, overall charge. BrO 4 1- Per brom ate ion BrO 3 1- Brom ate ion BrO 2 1- Brom ite ion BrO 1- Hypo brom it e ion CO 4 2- CO 3 2- Carbon ate ion CO 2 2- CO 2- ClO 4 1- ClO 3 1- Chlor ate ion ClO 2 1- ClO 1- IO 4 1- IO 3 1- Iod ate ion IO 2 1- IO 1- NO 4 1- NO 3 1- Nitr ate ion NO 2 1- NO 1- PO 5 3- PO 4 3- Phosph ate ion PO 3 3- PO 2 3- SO 5 2- SO 4 2- Sulf ate ion SO 3 2- SO 2 2- 1 more oxygen “normal” 1 less oxygen 2 less oxygen

Polyatomic Ion: a group of atoms that stay together and have a single, overall charge. BrO 4 1- Per brom ate ion BrO 3 1- Brom ate ion BrO 2 1- Brom ite ion BrO 1- Hypo brom it e ion CO 4 2- CO 3 2- Carbon ate ion CO 2 2- CO 2- ClO 4 1- ClO 3 1- Chlor ate ion ClO 2 1- ClO 1- IO 4 1- IO 3 1- Iod ate ion IO 2 1- IO 1- NO 4 1- NO 3 1- Nitr ate ion NO 2 1- NO 1- PO 5 3- PO 4 3- Phosph ate ion PO 3 3- PO 2 3- SO 5 2- SO 4 2- Sulf ate ion SO 3 2- SO 2 2- 1 more oxygen “normal” 1 less oxygen 2 less oxygen

Ternary CompoundsNaNO2 sodium nitriteKClO3 potassium chlorateCa3 (PO 4 ) 2 calcium phosphateFe(OH)3 iron (III) hydroxideNaHCO3 sodium bicarbonate ‘sodium hydrogen carbonate’

ideCalcium hydrox ide Ca 2+ OH 1- CaOH 2 Ca(OH) 2 Ca - O H H HO - Ca - OH vs.

Common Polyatomic IonsNames of Common Polyatomic Ions Ion Name Ion Name NH 4 1+ ammonium CO 3 2- carbonate NO2 1- nitrite HCO3 1- hydrogen carbonate NO3 1- nitrate (“bicarbonate” is a widely SO3 2- sulfite used common name) SO4 2- sulfate ClO 1- hypochlorite HSO4 1- hydrogen sulfate ClO2 1- chlorite (“bisulfate” is a widely ClO3 1- chlorate used common name) ClO4 1- perchlorate OH 1- hydroxide C2 H3O2 2- acetate CN 1- cyanide MnO4 1- permanganate PO4 3- phosphate Cr2O7 2- dichromate HPO4 2- hydrogen phosphate CrO4 2- chromate H2PO 4 1- dihydrogen phosphate O2 2- peroxide Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100 Print Version

Ternary Compounds________________ calcium phosphate________________ ammonium carbonate________________ aluminum sulfate Na 2 SO 4 ____________________ LiCN ____________________ Ba(ClO 3)2 ____________________________________ copper (II) hydroxide Ca3(PO 4) 2 (NH 4) 2CO3 Al2(SO4)3 sodium sulfate lithium cyanide barium chlorate Cu(OH)2

Magnesium PhosphateStep 1: Magnesium PhosphateStep 2: Mg2+ PO 4 3- Step 3: Mg (PO4 )3 2 Step 4: Mg 3 (PO 4)2

fluoride sulfide sulfide chloride bromide phosphide fluoride iodide chloride oxide phosphide iridium (III) calcium titanium (IV) platinum (II) barium strontium potassium zinc manganese (IV) gold (III) sodium dichromate hydroxide chromate acetate bromate sulfate cyanidenitrite chlorate phosphate nitrate2(Cr2 O7)3 (OH) 2 (CrO4)2 (CH3COO)2 (BrO3)2 SO4CN (NO2)2 (ClO3)4 PO 4 NO 3 Ir Ca Ti Pt Ba Sr K Zn Mn Au Na F 3 S S 2 Cl 2 Br 2 3 P 2 F I 2 Cl 4 2 O 3 3 P Ir 2+,3+,4+,6+ Ca 2+ Ti 3+,4+ Pt 2+,4+ Ba 2+ Sr 2+ K 1+ Zn 2+ Mn 2,3,4,6,7+ Au 1+,3+ Na 1+ variable fixed variable variable fixedfixedfixedfixed variablevariablefixed

fluoride sulfide sulfide chloride bromide phosphide fluoride iodide chloride oxide phosphide iridium (III) calcium titanium (IV) platinum (II) barium strontium potassium zinc manganese (IV) gold (III) sodium Ir CaTiPt BaSrKZn MnAuNa F3 S S 2 Cl2 Br 2 3P2F I2 Cl4 2O3 3P Ir2+,3+,4+,6+Ca2+ Ti3+,4+ Pt2+,4+Ba2+ Sr2+ K 1+ Zn 2+ Mn 2,3,4,6,7+ Au 1+,3+ Na 1+ variable fixed variable variable fixed fixed fixed fixed variable variable fixed

dichromate hydroxide chromate acetate bromate sulfate cyanide nitrite chlorate phosphate nitrate iridium (III) calcium titanium (IV) platinum (II) barium strontium potassium zinc manganese (IV) gold (III) sodium 2 (Cr2O7) 3 (OH)2 (CrO4 )2 (CH3COO)2 (BrO3)2 3SO 4CN (NO2) 2 (ClO3)4 PO4 NO3 IrCaTi PtBaSrKZn MnAu NaIr2+,3+,4+,6+ Ca 2+ Ti 3+,4+ Pt 2+,4+ Ba 2+ Sr 2+ K 1+ Zn 2+ Mn 2,3,4,6,7+ Au 1+,3+ Na 1+ variable fixed variable variable fixed fixed fixed fixed variable variable fixed

Two nonmetals Multiple-charge cation Everything else Roman numeral Polyatomic ions OK Roman numeral for name only Polyatomic ions Greek prefixes Charge Criss- Cross Rule Roman numeral OK Where would you file this? VCrO 4 BaO CBr 4 Nb(ClO 4 ) 5 SCl 2 Rb 2 SO 4 dinitrogen pentoxide platinum (IV) iodate ammonium chlorate potassium iodide nitrogen trichloride manganese (V) sulfide vanadium (II) chromate VCrO 4 N 2 O 5 dinitrogen pentoxide barium oxide BaO Pt(IO 3 ) 4 platinum (IV) iodate carbon tetrabromide CBr 4 NH 4 ClO 3 ammonium chlorate niobium (V) perchlorate Nb(ClO 4 ) 5 KI potassium iodide sulfur dichloride SCl 2 NCl 3 nitrogen trichloride rubidium sulfate Rb 2 SO 4 Mn 2 S 5 manganese (V) sulfide

Two nonmetals Multiple-charge cation Everything else Roman numeral Polyatomic ions Roman numeral for name only Polyatomic ions Greek prefixes Charge Criss- Cross Rule Roman numeral OK Where would you file this? VCrO 4 dinitrogen pentoxide BaO platinum (IV) iodate CBr 4 ammonium chlorate Nb(ClO 4 ) 5 potassium iodide SCl 2 nitrogen trichloride Rb 2 SO 4 manganese (V) sulfide

Write the total number of atoms that make up each compound. Write the compound formed by the following ions: 1) Al 3+ S 2- 2) Mg 2+ PO 4 3- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide 5) Ni2S3 6) triphosphorus heptoxide 7) N2O5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH3C6H2(NO2 )3 10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb 4+ )

Write the total number of atoms that make up each compound. Write the compound formed by the following ions: 1) Al 3+ S 2- 2) Mg 2+ PO 4 3- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide 5) Ni2S3 6) triphosphorus heptoxide 7) N2O5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH3C6H2(NO2 )3 10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb 4+ ) POP QUIZ

Write the total number of atoms that make up each compound. Write the compound formed by the following ions: 1) Al 3+ S 2- 2) Mg 2+ PO 4 3- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide 5) Ni 2S3 6) triphosphorus heptoxide 7) N2O5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH3 C6H2(NO2)3 10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb 4+ ) Answer Key Al 2 S 3 Mg 3 (PO 4 ) 2 barium oxide nickel (III) sulfide LiBr dinitrogen pentoxide MoN 2 8 21 PbI 4 P 3 O 7 aluminum sulfide magnesium phosphate

Polyatomic Ions - Quizoxalatechromatedichromatepermanganateacetate C 2 O 4 2- ……………CrO42- ……………Cr 2O72- …………..MnO 41- …………..CH3COO1- …….

K2OExceptions!Two exceptions to the simple –ide ending are the diatomic oxide ions, O 2 2- and O 2 1-. O22- is called peroxide O21- is called superoxide. Note the differences. barium oxide __________barium peroxide __________ sodium oxide __________ sodium peroxide __________ potassium oxide __________potassium superoxide __________BaO Na2 ODo Not Reduce to lowest terms!KO2 Ba 2+ Na1+K 1+BaO2 Na 2O2

Ionic Compounds:Polyatomic Ions Keys Ionic Compounds:  Polyatomic Ions Chart of the Ions and Polyatomic Ions Polyatomic Ions Grid to Memorize Ionic Compounds:  Polyatomic Ions http://www.unit5.org/chemistry/Nomenclature.html

Ionic Binary Compounds:Multiple-Charge Cations Keys           Ionic Binary Compounds:  Multiple-Charge Cations           Ionic Binary Compounds:  Multiple-Charge Cations http://www.unit5.org/chemistry/Nomenclature.html

Naming Chemical CompoundsBinary Compound?Use the strategysummarized earlier Polyatomic ions present? This is a compound for which naming procedures have not yet been considered. Name the compound using procedures similar to those for naming binary ionic compounds. Yes Yes No No Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 102

Nomenclature Review Flow Chart

Metal + Nonmetal? Formula  Name? Ionic Covalent Two Nonmetals? Multiple Single Use Prefixes!!! *Mono* Hexa Di Hepta Tri Octa Tetra Nona Penta Deca Write name of cation (metal) Determine the charge on the metal by balancing the (-) charge from the anion Write the charge of the metal in Roman Numerals and put in parentheses Write name of anion (Individual anions need –ide ending!) Steps 1 & 4 ONLY d,f-block Pb,Sn Columns 1, 2, 13 Ag + , Zn 2+ (Except: NH 4 + )

Name  Formula? No Prefixes? Prefixes? Determine the ions present and the charge on each (Roman Numeral = cation charge , otherwise use PT) Balance formula (criss-cross) Reduce subscripts (if needed) FORGET CHARGES!!! Use prefixes to determine subscriptsDo NOT reduce subscripts! Ionic Covalent

Oxidation Numbers and Ionic Compounds Keys Oxidation Numbers and Ionic Compounds Oxidation Numbers and Ionic Compounds http://www.unit5.org/chemistry/Nomenclature.html

Names and Formulas of Compounds Keys Names and Formulas of Compounds Names and Formulas of Compounds http://www.unit5.org/chemistry/Nomenclature.html

Binary Hydrogen CompoundsOxysalts + H2O  Oxyacids

Binary Hydrogen Compoundsof Nonmetals When Dissolved in Water(These compounds are commonly called acids.)The prefix hydro - is used to represent hydrogen, followed by the name of the nonmetal with its ending replaced by the suffix – ic and the wordacid added.Examples: *HCl HBr *The name of this compound would be hydrogen chloride if it was NOT dissolved in water. Hydro chlor ic acid Hydrobromic acid

Naming Simple Chemical CompoundsIonic (metal and nonmetal)Covalent (2 nonmetals) Metal Forms only one positive ion Forms more than one positiveion Nonmetal Use the name of element Use elementname followed by a Romannumeral toshow the charge Firstnonmetal Secondnonmetal Beforeelement name use a prefixto matchsubscript Use a prefixbeforeelement name and end with ide SingleNegative Ion Polyatomic Ion Use the name of the element, but end with ide Use the name of polyatomic ion ( ate or Ite )

Naming Ternary Compounds from Oxyacids The following table lists the most common families of oxy acids. one more oxygen atom most “common” one less oxygen two less oxygen HClO 4perchloric acid HClO3chloric acidHClO2chlor ous acidHClOhypo chlorous acid H2SO4sulfuric acidH2SO 3sulfurous acid H3PO 4phosphoric acid H 3 PO 3 phosphor ous acid H 3 PO 2 hypo phosphor ous acid HNO 3 nitr ic acid HNO 2 nitr ous acid (HNO) 2 hypo nitr ous acid

An acid with aname ending inA salt with aname ending in -ic -ous -ate -ite forms forms Hill, Petrucci, General Chemistry An Integrated Approach 1999, page 60

Oxyacids  Oxysalts If you replace hydrogen with a metal, you have formed an oxysalt.A salt is a compound consisting of a metal and a non-metal . If the salt consists of a metal, a nonmetal, and oxygen it is called an oxysalt. NaClO 4 , sodium perchlorate, is an oxysalt.HClO4per chloric acid HClO3chloric acid HClO2 chlorous acidHClO hypochlorous acid NaClO4sodium perchlorate NaClO3sodium chlorate NaClO2 sodium chloriteNaClOsodium hypochloriteOXYACID OXYSALT

ACID SALT per stem ic changes to per stem ate stem ic changes to stem ate stem ous changes to stem ite hyper stem ous changes to hypo stem ite HClO 3 + Na 1+ NaClO3 + H1+ acid cation salt

Meaning of Suffixes

Suffixes have meaning“-ide” binary compound sodium chloride (NaCl) “- ite ” or “- ate ” polyatomic compound sulfite (SO 32-) sulf ate (SO42-) “-ate” means one more oxygen than “-ite ”“-ol ” alcohol methyl alcohol (methanol) “-ose” sugar sucr ose“-ase” enzyme sucrase

Oxidation States in Formulas and Namesdinitrogen monoxide N2O nitrogen (I) oxidedinitrogen trioxide N2O3 nitrogen ( III ) oxide dinitrogen pentoxide N 2O5 nitrogen (V) oxide sulfur dioxide SO2 sulfur (IV) oxide sulfur trioxide SO3 sulfur (VI) oxide Traditional System Stock System +1 -2 +3 -2 +5 -2+4 -2 +6 -2 (Two non-metals) stock system is NOT preferred for two non-metals

Empirical Formula %  g g  mol mol / mol

% Mg = x 10024 g95 g Percentage Composition Mg magnesium 24.305 12 Cl chlorine 35.453 17 Mg 2+ Cl 1- MgCl 2 1 Mg @ 24.305 amu = 24.305 amu2 Cl @ 35.453 amu = 70.906 amu95.211 amu 25.52% Mg 74.48% Cl (by mass...not atoms) It is not 33% Mg and 66% Cl % = x 100 part whole

Empirical and Molecular FormulasA pure compound always consists of the same elements combined in the same proportions by weight.Therefore, we can express molecular composition as PERCENT BY WEIGHT. Ethanol, C 2 H 6 O 52.13% C 13.15% H 34.72% O

Empirical Formula Quantitative analysis shows that a compound contains 32.38% sodium, 22.65% sulfur, and 44.99% oxygen. Find the empirical formula of this compound. = 1.408 mol Na = 0.708 mol S = 2.812 mol O / 0.708 mol / 0.708 mol / 0.708 mol = 2 Na = 1 S = 4 O Na 2SO4 32.38% Na22.65% S44.99% O 32.38 g Na 22.65 g S 44.99 g O sodium sulfate Step 1) %  g Step 2) g  mol Step 3) mol mol Na 2 SO 4

Empirical FormulaA sample weighing 250.0 g is analyzed and found to contain the following:27.38% sodium 1.19% hydrogen14.29% carbon57.14% oxygen Determine the empirical formula of this compound. Step 1) convert %  gram Step 2) gram  moles Step 3) mol / mol Assume sample is 100 g. 27.38 g Na 1.19 g H 14.29 g C 57.14 g O / 1.19 mol = 1 Na / 1.19 mol = 1 H / 1.19 mol = 1 C / 1.19 mol = 3 O NaHCO 3

Empirical & Molecular FormulaA 175 g hydrocarbon sample is analyzed and found to contain ~83% carbon.The molar mass of the sample is determined to be 58 g/mol. Determine the empirical and molecular formula for this sample.Determine the empirical formula of this compound. Step 1) convert %  gram Step 2) gram  moles Step 3) mol / mol Assume sample is 100 g. / 6.917 mol = 1 C / 6.917 mol = 2.5 H (2.4577 H) CH 2.5 Then, 83 g carbon and 17 g hydrogen. C 2 H5 MM molecular = 58 g/mol58/29 = 2 Therefore 2(C2H5) = C4H10 MMempirical = 29 g/mol 2 C @ 12 g = 24 g 5 H @ 1 g = 5 g 29 g butane (~17% hydrogen) (contains only hydrogen + carbon )

1 mol S1 mol ZnCommon Mistakes when Calculating Empirical FormulaGiven: Compound consists of 36.3 g Zn and 17.8 g S. Find: empirical formula 36.3 g Zn 65.4 g Zn = 2 Zn 17.8 g S 17.8 17.8 = 1 S Zn 2 S 36.3 g Zn 17.8 g S 32.1 g S = 0.555 mol Zn = 0.555 mol S Chemical formula indicates MOLE ratio , not GRAM ratio 0.555 mol 0.555 mol 1 1 Zn S ZnS zinc sulfide

Empirical Formula of a HydrocarbonCxHyg H2O g CO 2 mol H 2 O mol CO 2mol C mol H burn in O 2 1 mol CO 2 44.01 g x1 mol H2O 18.02 gx 2 mol H 1 mol H2O x 2 mol C 1 mol CO2 x Empirical formula Kotz & Treichel, Chemistry & Chemical Reactivity , 3 rd Edition , 1996, page 224

Empirical and Molecular Formulas Keys Empirical and Molecular Formulas Empirical and Molecular Formulas             Empirical & Molecular Formula Empirical and Molecular Formulas  http://www.unit5.org/chemistry/Nomenclature.html

Errors in Chemical Formulas and Nomenclature Keys           Errors in Chemical Formulas and Nomenclature           Errors in Chemical Formulas and Nomenclature http://www.unit5.org/chemistry/Nomenclature.html Airs n Knomenclayture

Find the molar mass and percentage composition of zinc acetateacetate = CH3COO1-Zn 2+ CH 3 COO 1- Zn(CH3COO)2 1 Zn @ 65.4 g/mol = 65.4 g4 C @ 12 g/mol = 48 g 6 H @ 1 g/mol = 6 g 4 O @ 16 g/mol = 64 g Zn(CH 3COO)2 183.4 g / 183.4 g x 100% = 35.6 % Zn / 183.4 g x 100% = 26.2 % C/ 183.4 g x 100% = 3.3 % H / 183.4 g x 100% = 34.9 % O

1 mol Cl 35.5 g Cl 1 mol Y 88.9 g Y A compound is found to be 45.5% Y and 54.5% Cl. Its molar mass (molecular mass) is 590 g. a) Find its empirical formula b) Find its molecular formula Assume a 100 g sample size 45.5 g Y 54.5 g Cl = 0.5118 mol Y = 1.535 mol Cl / 0.5118 mol / 0.5118 mol = 1 Y = 3 Cl YCl 3 1 Y @ 88.9 g/mol = 88.9g 3 Cl @ 35.5 g/mol = 106.5 g YCl 3 195.4 g 590 / 195.4 = 3 3 (YCl 3 ) Y 3 Cl 9

Molar Mass vs. Atomic Mass 6.02x10 23 H 2 = _______ H2 = _____H2O = ________ H 2O = _____ MgSO4 = ________MgSO4 = _____ (NH4)3 PO4 = _____(NH 4)3PO4 = ________ Percentage CompositionEmpirical vs. Molecular Formula %  g g  mol mol molEmpirical Formula 2 amu 18 amu 120 amu 149 amu 2 g 18 g 120 g 149 g % = x 100 % part whole (lowest ratio) (by mass)

Subscripts, Superscripts and Coefficients

Subscripts, Superscripts and Coefficients Al 3 (SO 4 ) 2 coefficient subscripts superscripts ALUMINUM SULFATE SO 4 3- Al 2+ 5

Subscripts, Superscripts and Coefficients MgSO 4 MAGNESIUM SULFATE SO 4 2- Mg 2+ 3

Subscripts, Superscripts and Coefficients subscript MAGNESIUM NITRATE NO 3 1- Mg 2+ 4 2 MgNO 3 Mg(NO 3 ) 2

Interpretation of a Chemical FormulaSulfuric AcidH2SO4 Two atoms of hydrogen One atom of sulfur Four atoms of oxygen S O O O O H H

Chemical FormulasC8H18 Subscript indicates that there are 8 carbon atoms in a molecule of octane. Subscript indicates that there are 18 hydrogen atoms in a molecule of octane. Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 203

Stock System of NomenclatureCuCl2 Name of Roman cation numeral indicating charge Name of anion + copper (II) chloride

Chemical FormulasAl2(SO4)3 Subscript 2 refers to 2 aluminum atoms. Subscript 4 refers to4 oxygenatoms insulfate ion. Subscript 3 refers toeverything inside parentheses.Here there are 3 sulfate ions, with a total of 3 sulfur atomsand 12 oxygen atoms. Davis, Metcalfe, Williams, Castka, Modern Chemistry , 1999, page 204

Naming Binary Ionic CompoundsAl2O3Name of cation Name of anion aluminum oxide Davis, Metcalfe, Williams, Castka, Modern Chemistry , 1999, page 207

The OLD System of NomenclatureCuCl2Name of Name of anion cation Cupric chloride -ic higher oxidation # -ous lower oxidation # + Davis, Metcalfe, Williams, Castka, Modern Chemistry , 1999, page 208

Multi-vitamins

Centrum Multi-VitaminIngredients: ascorbic acid, beta carotene, biotin, calcium pantothenate, calciumphosphate, carnauba wax, chromium chloride, crospovidone, cupr ic sulfate , cyanocobalamin, dl-alpha tocopheryl acetate, FD & C blue no. 2 aluminum lake,hydroxypropyl cellulose, ferrous fumarate, hydroxypropyl methylcellulose, lactose, Magnesium oxide, magnesium stearate, manganese sulfate, microcrystalline cellu-lose,niacinamide, nickel sulfate, phytonandione, polyethylene glycol, potassium chloride, potassium citrate, potassium iodide, povidone, pyridoxine hydrochloride, riboflavin, silica gel, sodium borate, sodium metavanadate, sodium molybdate,sodium selenate, stannous chloride , stearic acid, thiamin mononitrate, titaniumdioxide, triacetin, vitamin A acetate, vitamin D 3, zinc oxide. PC7563-46-00 Warning: Accidental overdose of iron-containing products is a leading cause of fatal poisoning in children under 6. Keep this product out of reach of children.In case of accidental overdose, call a doctor or poison control immediately.

Chromium (III) ChlorideStep 1: Chromium (III) ChlorideStep 2: Cr3+ Cl 1- Step 3: Cr Cl 1 3 Step 4: CrCl 3 RECALL: Chromium forms oxides in which metal exhibits oxidation states of +3 and +2. STOCK system indicates oxidation state of compound. Assume Cr3+ (chromium (III) chloride). Return to Centrum Bottle

Cupric SulfateStep 1: Cupric SulfateStep 2: Cu2+ SO 4 2- Step 3: Cu (SO 4)2 2 Step 4: Cu 2 (SO 4)2 Step 5: CuSO4 RECALL: “ic” higher oxidation & “ous” lower oxidation Cu2+ (higher) Cu1+ (lower) Return to Centrum Bottle

Manganese (III) SulfateStep 1: Manganese (III) SulfateStep 2: Mn3+ SO 4 2- Step 3: Mn (SO 4)2 3 Step 4: Mn 2 (SO 4)3 RECALL: Manganese forms oxides in which metal exhibits oxidation states of +2, +3, +4, and +7. STOCK system indicates oxidation state of compound. Assume Mn3+ (manganese (III) sulfate). Return to Centrum Bottle

Stannous ChlorideStep 1: Stannous (tin) ChlorideStep 2: Sn2+ Cl 1- Step 3: Sn Cl 1 2 Step 4: SnCl 2 RECALL: “ic” higher oxidation & “ous” lower oxidation Sn4+ (higher) Sn2+ (lower) Return to Centrum Bottle

Stannic ChlorideStep 1: Stannic (tin) ChlorideStep 2: Sn 4+ Cl 1- Step 3: Sn Cl 1 4 Step 4: SnCl 4 RECALL: “ic” higher oxidation & “ous” lower oxidation Sn4+ (higher) Sn 2+ (lower) Return to Centrum Bottle

Chromium ChlorideStep 1: Chromium (II) ChlorideStep 2: Cr2+ Cl 1- Step 3: Cr Cl 1 2 Step 4: Cr 1 Cl2 Step 5: CrCl 2RECALL: Chromium has multiple oxidation states. Name with STOCK system. Assume Chromiun (II). Return to Centrum Bottle

Calcium PhosphateStep 1: Calcium PhosphateStep 2: Ca2+ PO 4 3- Step 3: Ca (PO4 )3 2 Step 4: Ca 3 (PO 4)2 Return to Centrum Bottle

Zinc OxideStep 1: Zinc OxideStep 2: Zn2+ O 2- Step 3: Zn O 2 2 Step 4: Zn 2 O2 Step 5: ZnO Return to Centrum Bottle

Polyatomic Ions

Common Polyatomic IonsIon Name Ion Name NH 4 + ammonium nitrite nitrate phosphate hydrogen phosphate dihydrogen phosphate carbonatehydrogen carbonate (bicarbonate is a widelyused common name)sulfite sulfate hydrogen sulfate(bisulfate is a widelyused common name) hydroxidecyanide hypochloritechlorite chlorate perchlorate acetate permanganate dichromate chromate peroxide NO 2 - NO 3 - SO 3 2- HSO 4 - OH - CN - PO 4 3- CO 3 2- SO 4 2- MnO 4 - O 2 2- Cr 2 O 7 2- HPO 4 2- H 2 PO 4 - ClO 2 - ClO 3 - ClO - HCO 3 - ClO 4 - C 2 H 3 O 2 - CrO 4 2- Names of Common Polyatomic Ions

Vocabulary - Chemical Bonds Keys http://www.unit5.org/chemistry/Nomenclature.html Vocabulary – Chemical Bonds Vocabulary – Chemical Bonds

1 2 3 4 5 6 1 2 3 4 5 6 Electronegativities 7 Be 1.5 Al 1.5 Si 1.8 Ti 1.5 V 1.6 Cr 1.6 Mn 1.5 Fe 1.8 Co 1.8 Ni 1.8 Cu 1.9 Zn 1.7 Ga 1.6 Ge 1.8 Nb 1.6 Mo 1.8 Tc 1.9 Ag 1.9 Cd 1.7 In 1.7 Sn 1.8 Sb 1.9 Ta 1.5 W 1.7 Re 1.9 Hg 1.9 Tl 1.8 Pb 1.8 Bi 1.9 1.5 - 1.9 N 3.0 O 3.5 F 4.0 Cl 3.0 3.0 - 4.0 C 2.5 S 2.5 Br 2.8 I 2.5 2.5 - 2.9 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Ba 0.9 Fr 0.7 Ra 0.9 Below 1.0 H 2.1 B 2.0 P 2.1 As 2.0 Se 2.4 Ru 2.2 Rh 2.2 Pd 2.2 Te 2.1 Os 2.2 Ir 2.2 Pt 2.2 Au 2.4 Po 2.0 At 2.2 2.0 - 2.4 Period Actinides: 1.3 - 1.5 Li 1.0 Ca 1.0 Sc 1.3 Sr 1.0 Y 1.2 Zr 1.4 Hf 1.3 Mg 1.2 La 1.1 Ac 1.1 1.0 - 1.4 Lanthanides: 1.1 - 1.3 * * y y 1A 2A 3B 4B 5B 6B 7B 1B 2B 3A 4A 5A 6A 7A 8A Hill, Petrucci, General Chemistry An Integrated Approach 2 nd Edition, page 373 8B

Metal (fixed) + Non-metalbinary -ideNaCl sodium chloride Metal (variable) + Non-metal STOCK system (Roman Numeral) CrCl 2 chromium (II) chloride OLD system [-ic (higher) & - ous (lower)] CuCl 2 cupric chloride Sn stannumPb plumbumCu cuprumAu aurumFe ferrum Polyatomic Ions [-ate (one more O) & -ite (one less O)] LiNO3 lithium nitr ateLiNO2 lithium nitr iteLi3N lithium nitrideTWO Elements Three or more Elements Review Cu 1+ or Cu2+ Group 1, Group 2, Ag, Zn, Al Transition Elements Cr 2+ Cl 1- Ternary Compounds (binary compound)

Polyatomic Ions [-ate (one more O) & -ite (one less O)]per____ate NORMAL _____ ite hypo_____ite chloratenitratecarbonatesulfatephosphate ammonium, cyanide, hydroxide Nonmetal & Nonmetal (Greek prefixes)……DO NOT REDUCE! Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca 1 2 3 4 5 6 7 8 9 10 ClO 3 1-NO 31-CO32-SO42- PO43- NH41+CN 1-OH1- chloritenitritecarbonitesulfitephosphite ClO 21-NO21-CO2 2- SO 3 2- PO 3 3- perchlorate pernitrate percarbonate persulfate perphosphate ClO 4 1- NO 4 1- CO 4 2- SO 5 2- PO 5 3- 2 less oxygen 1 less oxygen 1 more oxygen ClO 1- NO 1- CO 2- SO 2 2- PO 2 3- hypochlorite hyponitrite hypocarbonite hyposulfite hypophosphite Memorize How many atoms are in a formula unit of ammonium hypophosphite? NH 4 1+ PO 2 3- (NH 4 ) 3 PO 2 3 18 _____ ate

Molecular Models Activity Keys Molecular Model's Activity Molecular Model's Activity http://www.unit5.org/chemistry/Nomenclature.html

Molecular Models Activityammoniahydrogen monochloridetrichloromethaneurea propane butane nitrogen triiodide ( video) carbon tetrachloride methanewaterethane ethyne dihydrogen monosulfide carbon dioxide supplies

Bonding and Shape of MoleculesNumber of BondsNumber of Unshared Pairs Shape Examples 2 3 4 3 2 0 0 0 12 LinearTrigonal planarTetrahedral PyramidalBent BeCl2BF3 CH4, SiCl4NH 3, PCl3H2O, H2 S, SCl2-Be- B C N : O : : Covalent Structure

Lewis Structures1) Count up total number of valence electrons2) Connect all atoms with single bonds - “multiple” atoms usually on outside - “single” atoms usually in center; C always in center, H always on outside. 3) Complete octets on exterior atoms (not H, though) 4) Check - valence electrons match with Step 1 - all atoms (except H) have an octet; if not, try multiple bonds - any extra electrons? Put on central atom - no unpaired electrons (free radicals) Gilbert Lewis

Carbon tetrachlorideC Cl Cl Cl Cl CCl 4 C 109.5 o Cl Cl Cl Cl Carbon tetrachloride – “carbon tet” had been used as dry cleaning solvent because of its extreme non-polarity. Tetrahedral geometry

MethaneC H H H H C 109.5 o H H H H Methane –The first member of the paraffin (alkane) hydrocarbons series. a.k.a. (marsh gas, CH 4 ). Tetrahedral geometry

Water .. .. H H O Bent geometry SO 2 d (-) d (+) Polar molecule

EthaneC H C H H H H H space-filling molecule ball-and-stick Lewis dot notation C 2 H 6 molecular formula C = 1 s 2 2 s 2 2 p 2

EtheneC H C H H H H H space-filling molecule ball-and-stick Lewis dot notation C 2 H 4 molecular formula

EthyneC C H H C C H H No octet Stable octet 6 electrons = triple bond C C H H C 2 H 2 C C H H each C “feels” 6 electrons each C “feels” 7 carbons Ethyne – a.k.a. “acetylene”

Dihydrogen monosulfide .. .. H H S Bent SO 2

Carbon dioxideO O C Linear geometry C O O CO 2 C O O

AmmoniaN H H H N 107 o H H H .. NH 3 .. H H H N Trigonal Pyramidal geometry N H H H

HAmino Acids – Functional Groups Amine Carboxylic Acid Base Pair NH 2 1- R- COOH NH 3 NH 21-NH 41+amine ammonia ammonium ionN H HH : N H H H H : 1+ N H H : 1- : H + lose H + H + +

Hydrogen monochlorideH Cl HCl H Cl d (-) d (+) H Cl Polar molecule HCl( g ) + H 2 O( l )  HCl( aq ) hydrogen chloride water hydrochloric acid

TrichloromethaneC Cl Cl Cl H CHCl 3 C 109.5 o H Cl Cl Cl C Cl Cl Cl H d (-) d (+) Polar molecule Tetrahedral geometry

UreaC O N H H N H H C O N H H N H H CO(NH 2 ) 2 NOT “di-urea” Urea – The first organic compound to be synthesized (Wohler, 1828).

Propane C H C H H C H H H H H C C C H H H H H H H H C 3 H 8

ButaneC H C H H C H C H H H H H H H - C - C - C - C - H H H H H H H H H C 4 H 10 C C C H H H H H H H H C H H

Nitrogen triiodideN I I I N 107 o I I I .. NI 3 Trigonal Pyramidal geometry Video clip: (slow motion) detonation of N I 3

Supplies 15 black (carbon) 8 green (chlorine and iodine) 1 yellow (sulfur) 4 blue (oxygen) 4 red (nitrogen) 42 hydrogen (hydrogen) 67 bonds (bonds)

C Cl I S O N H C Cl Cl Cl Cl C H H H H C O O S H H C C H H C Cl Cl Cl H H Cl CCl 4 CH 4 CO 2 C 2 H 2 HCl CHCl 3 SH 2

C H C H H C H C H H H H H H C H C H H C H H H H H N H H H N I I I

Decomposition of Nitrogen Triiodide

Decomposition of Nitrogen Triiodide 2 NI 3 ( s ) N 2 ( g ) + 3 I 2 ( g ) NI 3 I 2 N 2

C 109.5 o H H H H N 107 o H H H .. O 104.5 o H H .. .. CH 4 , methane NH 3 , ammonia H 2 O, water .. O O O lone pair electrons O O O O 3 , ozone

.. .. .. The VSEPR Model O O C Linear The Shapes of Some Simple AB n Molecules O O S Bent O O S O Trigonal planar F F F N Trigonal pyramidal T-shaped Square planar F F Cl F F F Xe F F F F F P F F Trigonal bipyramidal Octahedral F F F S F F F AB 6 SO 2 Brown, LeMay, Bursten, Chemistry The Central Science , 2000, page 305

KEYS - NomenclatureObjectives Worksheet - binary cmpds: single charge cation Worksheet - ions in chemical formulas Worksheet - ionic cmpds: polyatomic ions w multiple-charge cation Worksheet - ionic formulas (binary, polyatomic, transition) Worksheet – ionic cmpds: traditional system of nomenclature Worksheet - covalent binary cmpds: non-metal - non-metal Worksheet - ionic cmpds: polyatomic ions Worksheet - ionic binary cmpds: multiple charge cation Outline (general) Worksheet - oxidation numbers and ionic cmpds Worksheet - names and formulas of cmpds Worksheet - empirical and molecular Worksheet - vocab (bonding) Activity – bonding PP Activity - molecular models activity - mole pattern Worksheet - errors in chemical formulas and nomenclature Worksheet - binary compounds Worksheet - ions in chemical compounds Textbook - questions

Resources - NomenclatureObjectives Worksheet - binary cmpds: single charge cation Worksheet - ions in chemical formulas Worksheet - ionic cmpds: polyatomic ions w multiple-charge cation Worksheet - ionic formulas (binary, polyatomic, transition) Worksheet - traditional system of nomenclature Worksheet - covalent binary cmpds: non-metal - non-metal Worksheet - ionic cmpds: polyatomic ions Outline (general) Worksheet - empirical and molecular Worksheet - vocab (bonding) Activity - bonding pieces Activity - molecular models Activity - mole pattern Worksheet - binary compounds Worksheet - ions in chemical compounds Textbook - questions Workshee t - ionic binary cmpds: multiple charge cation Worksheet - oxidation numbers and ionic cmpds Worksheet - names and formulas of cmpds Worksheet - errors in chemical formulas and nomenclature General Chemistry PP