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Common Polyatomic Ions Names of Common Polyatomic Ions Ion Name Ion Name NH 4 + ammoniumCO 3 2- carbonate *NO 2 - *nitriteHCO 3 - bicarbonate NO 3 - nitrate*IO 3 - *iodate *SO 3 2- *sulfite*IO 4 - *periodate SO 4 2- sulfate *ClO - *hypochlorite HSO 4 - hydrogen sulfate*ClO 2 - *chlorite OH - hydroxide ClO 3 - chlorate CN - cyanide *ClO 4 - *perchlorate C 2 H 3 O 2 - acetate *BrO 3 - *bromate MnO 4 - permanganateC 2 O 4 2- oxalate PO 4 3- phosphateCr 2 O 7 2- dichromate *PO 3 3- *phosphiteCrO 4 2- chromate H 2 PO 4 - dihydrogen phosphateO 2 2- peroxide Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100 Memorize the BOLD ions * = you will be responsible for knowing these

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Polyatomic Ion Trends *Charges NEVER change between different forms Normal ate form BrO 3 - bromate ClO 3 - chlorate IO 3 - iodate NO 3 - nitrate CO 3 2- carbonate SO 4 2- sulfate PO 4 3- phosphate BrO 2 - ClO 2 - IO 2 - NO 2 - CO 2 2- SO 3 2- PO 3 3- BrO - ClO - IO - BrO 4 - ClO 4 - IO 4 - -1 oxygen -ite form -2 oxygens hypo___ite +1 oxygen Per____ate bromite chlorite iodite nitrite sulfite phosphite hypobromite hypochlorite hypoiodite perbromate perchlorate periodate carbonite

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Atomic Theory Review

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Electron Cloud Model Orbital (electron cloud) instead of orbits Region in space where there is 90% probability of finding an electron Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem Electron Probability vs. Distance Electron Probability (%) Distance from the Nucleus (pm) 100150200250500 0 10 20 30 40 Orbital 90% probability of finding the electron Orbital Shape

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Shapes of s, p, and d-Orbitals each holds 2 electrons (s 2 ) each of 5 orbitals holds 2 e - = 10 total d electrons (d 10 ) each of 3 orbitals holds 2 e - = 6 total p electrons (p 6 )

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s, p, and d-orbitals s orbitals: Each holds 2 electrons (outer orbitals of Groups 1 and 2) p orbitals: Each of 3 sets holds 2 electrons = 6 electrons (outer orbitals of Groups 3 to 8) d orbitals: Each of 5 sets holds 2 electrons = 10 electrons (found in elements in third period and higher) Orbital Filling Video

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Copyright 2006 Pearson Benjamin Cummings. All rights reserved. Orbitals overlap each other as you get farther from the nucleus

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f-orbitals 7 f orbitals @ 2 e- each = 14 e-

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s, p, d and f orbitals How many g orbitals could exist?

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theoretical g-orbitals 9 g orbitals @ 2 e- each = 18 e-

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s p d f 6767 Periodic Patterns for Electron Config 1s1s1s1s 2s2s2s2s 3s3s3s3s 4s4s4s4s 5s5s5s5s 6s6s6s6s 7s7s7s7s 3d3d3d3d 4d4d4d4d 5d5d5d5d 6d6d6d6d 1s1s1s1s 2p2p2p2p 3p3p3p3p 4p4p4p4p 5p5p5p5p 6p6p6p6p 7p7p7p7p 4f4f4f4f 5f5f5f5f 12345671234567 1 2 (n-1) (n-2) n 3 5 6 7 8 4

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s-block1st Period 1s 1 # of e- in that orbital(s) Periodic Patterns Example - Hydrogen Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

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Shorthand Configuration S 16e - Valence Electrons (Highest energy level) Core Electrons S16e - [Ne] 3s 2 3p 4 1s 2 2s 2 2p 6 3s23s2 3p43p4 Electron Configuration Review Longhand Configuration Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem S 32.066 16

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[Ar]4s 2 3d 10 4p 2 Periodic Patterns GermaniumExample - Germanium Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem Ge 72.61 32

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[ ] neon's electron configuration(1s 2 2s 2 2p 6 ) Shorthand Configuration [Ne] 3s 1 3rd energy level (or 3 rd period) 1 electron in the s orbital orbital shape (s,p,d,fetc.) 1s 2 2s 2 2p 6 3s 1 electron configuration A B C D Na = [Ne]

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Shorthand Configuration Practice [Ar] 4s 2 Electron configurationElement symbol [Ar] 4s 2 3d 3 [Rn] 7s 2 5f 14 6d 4 [He] 2s 2 2p 5 [Kr] 5s 2 4d 9 [Kr] 5s 2 4d 10 5p 5 [Kr] 5s 2 4d 10 5p 6 [He] 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Ca V Sg F Ag I Xe Fe [Ar] 4s 2 3d 6

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Periodic Patterns Review Period # (1-7) energy level (subtract for d & f) Group # (1-8excluding d block) total # of valence e - Column within Sublevel block # of e - in sublevel/orbital Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

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s p d f 6767 Periodic Patterns and Charge Trends 1s1s1s1s 12345671234567 +1 +2 (n-2) n +3 - 3 - 2 - 1 Variable Charge METALS NON- METALS

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Electron Configurations for Cations Metals lose e - to attain a noble gas configuration Metals form positive ions Cations are pawsitive Metal ions will lose e - from configuration Na: 1s 2 2s 2 2p 6 3s 1 Na + : 1s 2 2s 2 2p 6 noble gas configuration

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Formation of a Cation 11p + sodium atom Na [Ne] 3s 1 e-e- loss of one valence electron e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- sodium ion Na + [Ne] 11p + e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e-

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Electron Configurations for Anions Non-metals gain electrons to attain a noble gas configuration They form negative ions Take a look at the e - configuration S 1s 2 2s 2 2p 6 3s 2 3p 4 (6 valence electrons) + 2e - S 2- 1s 2 2s 2 2p 6 3s 2 3p 6 ( noble gas configuration)

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Formation of an Anion 17p + chlorine atom Cl [Ne]3s 2 3p 5 e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- 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 [Ne]3s 2 3p 6 or [Ar] e-e- 17p + e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e-

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Stable Electron Configurations All atoms react to achieve noble gas configuration Noble gases have two s and six p electrons Eight valence electrons Also called the octet rule Ar

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Bonding Review and Writing Ionic Formulas Table salt

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Formation of Ionic Bond sodium ion Na + 11p + e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- chloride ion Cl - 17p + e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- + -

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Ionic Bonding Anions and cations are held together by opposite charges All ionic compounds are called salts Simplest ratio is called the formula unit The bond is formed through the transfer of electrons Electrons are transferred to fill all available orbitals, or achieve a noble gas configuration

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O 2- K+K+ K+K+ Mg 2+ Br - K Br potassium atom bromine atom e-e- e-e- Br - K+K+ potassium ion bromide ion potassium bromide KBr MgBr 2 K2OK2O magnesium bromide potassium oxide

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Bonding Practice Ca 2+ Al 3+ Na + Pb 4+ OH - N 3- Mg 2+ OH - N 3- Pb 4+ N 3- Pb 4+ N 3- Pb 4+ N 3- ? Pb 4+ N 3- Pb 3 N 4 lead (IV) nitride or plumbic nitride NaOH Mg(OH) 2 AlN CaBr 2 Ca(OH) 2 CaO

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Fe 2+ Ca 2+ PO 4 3- NH 4 + O 2- Al 3+ O 2- Ca 3 (PO 4 ) 2 (NH 4 ) 3 PO 4 FeO Al 2 O 3

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Subscripts, Superscripts and Coefficients Mg 3 (PO 4 ) 2 coefficient subscripts superscripts MAGNESIUM PHOSPHATE PO 4 3- Mg 2+ 5

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Writing Formulas of Ionic Compounds chemical formula: has neutral charge; shows types of atoms and how many of each To write an ionic compounds formula, we need: 1. the two types of ions 2. the charge on each ion Na + and F Ba 2+ and O 2 Na + and O 2 Ba 2+ and F NaF BaO Na 2 O BaF 2

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ide Calcium hydrox ide Ca 2+ OH - CaOH 2 Ca(OH) 2 Ca - O H H HO - Ca - OH vs. The Importance of Parentheses The formulas imply two totally different compounds!

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(NH 4 ) 3 N Fe 2 (Cr 2 O 7 ) 3 Sn(SO 4 ) 2 NH 4 ClO 3 Mg(NO 2 ) 2 BaSO 4 Writing Formulas w /Polyatomic Ions Parentheses are required only when you need more than one bunch of a particular polyatomic ion Ba 2+ and SO 4 2 Mg 2+ and NO 2 NH 4 + andClO 3 Sn 4+ andSO 4 2 Fe 3+ andCr 2 O 7 2 NH 4 + andN 3

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Element Latin root -ic -ous gold, Auaur- Au 3+ Au 1+ lead, Pbplumb- Pb 4+ Pb 2+ tin, Snstann- Sn 4+ Sn 2+ copper, Cucupr- Cu 2+ Cu 1+ iron, Feferr- Fe 3+ Fe 2+ 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!) ; (delicious food is not good for you!)

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Cu 2 S AuN FeF 2 plumbic phosphide plumbous phosphide stannic chloride Fe 2+ Write formulas:Write names: cuprous sulfide auric nitride ferrous fluoride Pb 3 P 4 3 Pb ? 4 P 3 Cu 1+ Pb 3 P 2 3 Pb ? 2 P 3 Au 3+ SnCl 4 Sn ? 4 Cl 1 S 2 N 3 F 1

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Nomenclature - Humor Ferrous Wheel Fe = iron (Latin = ferrum) Fe 2+ = lower oxidation state = ferrous Fe 3+ = higher oxidation state = ferric BaNa 2 BaNaNa Fe 2+ What weapon can you make from the elements nickel, potassium and iron? A KNiFe

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Teacher: What is the formula for water? Student: H, I, J, K, L, M, N, O Teacher: Thats not what I taught you. Student: But you said the formula for water wasH to O. Website: Dihydrogen monoxide Information Campaign mis Little Johnny took a drink, Now he shall drink no more. For what he thought was H 2 O, Was H 2 SO 4. Under aged Pb walks into a bar and the bartender turns to the gold Bouncer and says, Au, get the lead out! "H-O-H"?! WHAT'S THAT SPELL?! WATER?

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Four Types of Naming Fixed Charge Ionic Compounds Variable Charge Ionic Compounds Acidic Compounds Covalent Molecules Contain a metal with a fixed charge and a non- metal (ionic) Contain H + with various anions (ionic when aqueous) Contain 2 or more nonmetals only Contain a metal with a variable charge and a non- metal (ionic)

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Li 3 H1H1 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 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 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 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 Fixed charge cations Variable charge cations Elemental anions 1+ 2+ 3+1-2-3-

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Fixed Charge Exceptions Start with Al Go backwards down the stairs Decrease the charge after each stair Al 13 Zn 30 Ag 47 3+ 2+ + 3+

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Fixed Charge Compound Nomenclature Metals (fixed charge) + Nonmetals

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Fixed Charge Compounds Compounds that contain a metal with a fixed charge (group 1, 2, and 3, with Zn 2+, Ag +, etc.), and a non-metal To name these compounds, use the name of metal and the name of the non-metal with the ending replaced by the suffix ide Examples: NaCl (Na + Cl - ) CaS (Ca 2+ S 2- ) AlI 3 (Al 3+ 3I - ) sodium chloride calcium sulfide aluminum iodide

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Cations and Anions Common Simple Cations and Anions CationName AnionName* H + hydrogen H - hydride Li + lithium F - fluoride Na + sodium Cl - chloride K + potassium Br - bromide Cs + cesium I - iodide Be 2+ beryllium O 2- oxide Mg 2+ magnesium S 2- sulfide Al 3+ aluminum N 3- nitride Ag + silver P 3- phosphide Zn 2+ zinc * The root is given in color Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86 EXCEPTIONS

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

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Fixed Charge Naming Practice FormulaName 1 BaO____________________ 2________________ sodium bromide 3 MgI 2 ____________________ 4 KCl____________________ 5________________ strontium fluoride 6________________ cesium fluoride barium oxide NaBr magnesium iodide potassium chloride SrF 2 CsF

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(NH 4 ) 3 N Na 2 Cr 2 O 7 Al 2 (SO 4 ) 3 NH 4 ClO 3 Mg(NO 2 ) 2 BaSO 4 Fixed Charge Nomenclature w /Polyatomic Ions Simply insert the name of the polyatomic ion into the final name Ba 2+ and SO 4 2 Mg 2+ and NO 2 NH 4 + andClO 3 Al 3+ andSO 4 2 Na + andCr 2 O 7 2 NH 4 + andN 3 barium sulfate magnesium nitrite ammonium chlorate alumnium sulfate sodium dichromate ammonium nitride

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Polyatomic Ions Quiz phosphate sulfate dichromate permanganate acetate PO 4 3- SO 4 2- Cr 2 O 7 2- .. MnO 4 - .. CH 3 COO - .

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Variable Charge Compound Nomenclature Metals (variable charge) + Nonmetals

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Roman Numeral Review Greek Number Roman Numeral 1I 2II 3III 4IV 5V 6VI 7VII 8VIII 9IX 10X NumberRoman Numeral 1I 5V 10X 50L 100C

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Li 3 H1H1 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 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 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 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 Single charge cations Variable charge cations Elemental anions 1+ 2+3+1-2-3-

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Stock System of nomenclature Variable Charge Ionic Compounds To name, given the formula: 1. Figure out charge on cation 2. Write name of cation 3. Write Roman numerals in ( ) to show cations charge Compounds that contain a metal with variable charge (Pb, Sn, and the transition metalsnot including Ag or Zn), and a non-metal

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Variable charge Naming Practice 4. Write name of anion: FeOFe ? O 2 Fe 2 O 3 2 Fe ? 3 O 2 CuBrCu ? Br CuBr 2 Cu ? 2 Br iron(II) oxide iron(III) oxide copper(I) bromide copper(II) bromide

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Variable Charge Cations Common Type II Cations IonStock 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 Hg 2 2+ mercury (I)mercurous * Mercury (I) ions are always bonded together in pairs to form Hg 2 2+ Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90

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To find the formula, given the name: 2. Balance charges to write formula cobalt (III) chlorideCo 3+ Cl tin (IV) oxideSn 4+ O 2 tin (II) oxideSn 2+ O 2 1. Write symbols for the two types of ions Variable Charge Ionic Compounds SnO SnO 2 CoCl 3

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Naming Variable Charge Ionic Compounds FormulaName 1 Hg 2 O____________________ 2 HgO____________________ 3________________ copper (II) fluoride 4________________ copper (I) sulfide 5 Cr 2 O 3 ____________________ 6________________ lead (IV) oxide mercury (I) oxide PbO 2 mercury (II) oxide CuF 2 Cu 2 S chromium (III) oxide

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Ionic Compounds with Polyatomic Ions 1.________________ iron (II) phosphate 2.________________ ammonium carbonate 3.________________ aluminum sulfate 4. V 2 SO 3 ____________________ 5. AgCN____________________ 6. Ba(ClO 3 ) 2 ____________________ 7.________________ copper (II) hydroxide Fe 3 (PO 4 ) 2 (NH 4 ) 2 CO 3 Al 2 (SO 4 ) 3 vanadium (I) sulfite silver cyanide barium chlorate Cu(OH) 2

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Acidic Compounds Oxysalts + H 2 O Oxyacids

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Acidic Compounds (Nonmetals Dissolved in Water) The prefix hydro- is used to represent hydrogen, followed by the root name of the nonmetal with its ending replaced by the suffix ic acid. Examples: *HCl(aq) HBr(aq) *The name of this gas would be hydrogen monochloride if it was NOT dissolved in water. Acids(aq) without oxygen Hydrochloric acid Hydrobromic acid (aq) = aqueous or dissolved in water

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Acidic Compounds Nonmetals Dissolved in Water Start with the name of the polyatomic ion (with oxygen), and change the ending based on the following rule: If the ion ends in ate, change the suffix to ic acid. If the ion ends in ite, change the suffix to ous acid. Retain any prefixes such as per or hypo in front of the acid name. NEVER use hydro! Examples: HClO 3 (aq) HBrO(aq) Acids(aq) WITH oxygen (oxyacids) Chloric acid Hypobromous acid ClO 3 - = chlorate BrO - = hypobromite

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An acid with a name ending in An ion with a name ending in -ic -ous -ate -ite Hill, Petrucci, General Chemistry An Integrated Approach 1999, page 60 Oxyacid Naming Rules

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Common Oxyacid Names The following table lists the most common families of oxy acids. one more oxygen atom most common one less oxygen two fewer oxygens HClO 4 perchloric acid HClO 3 chloric acid HClO 2 chlorous acid HClO hypochlorous acid H 2 SO 4 sulfuric acid H 2 SO 3 sulfurous acid H 3 PO 4 phosphoric acid H 3 PO 3 phosphorous acid H 3 PO 2 hypophosphorous acid HNO 3 nitric acid HNO 2 nitrous acid

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Acid Nomenclature Practice FormulaName 1 HCl____________________ 2 HClO____________________ 3________________ sulfuric acid 4________________ hydrofluoric acid 5 H 3 N____________________ 6________________ periodic acid hydrochloric acid HIO 4 hypochlorous acid H 2 SO 4 HF hydronitric acid

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Covalent Compounds Nonmetal + Nonmetal

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Writing Formulas of Covalent Compounds Covalent Compounds contain two or more non-metals (NO METALS!) Key: FORGET CHARGES To Name, given the formula: 1. Use Greek prefixes to indicate how many atoms of each element, but dont use mono on first element (least electronegative, excluding H) 2. Add the suffix ide to the second element (most electronegative) 1 mono 6 hexa 2 di7 hepta 3 tri8 octa 4 tetra9 nona 5 penta10 deca Prefixes to memorize!

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Covalent Nomenclature Practice EXAMPLES: 1. carbon dioxide 2. CO 3. dinitrogen trioxide 4. SF 6 5. carbon tetrachloride 6. NI 3 CO 2 carbon monoxide N2O3N2O3 sulfur hexafluoride CCl 4 nitrogen triiodide

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More Practice with covalent compounds 1.________________ diarsenic trisulfide 2.________________sulfur dioxide 3. P 2 O 5 ____________________ 4.________________ nitrogen trihydride 5. N 2 O 5 ____________________ 6. H 2 O____________________ As 2 S 3 SO 2 diphosphorus pentoxide NH 3 dinitrogen pentoxide dihydrogen monoxide

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Naming Simple Chemical Compounds Ionic (metal and nonmetal)Covalent (2 nonmetals) Metal Forms only one positive ion Forms more than one positive ion Nonmetal Use the name of element Use element name followed by a Roman numeral to show the charge First nonmetal Second nonmetal Before element name use a prefix to match subscript Use a prefix before element name and end with ide Single Negative Ion Polyatomic Ion Use the name of the element, but end with ide Use the name of polyatomic ion (ate or Ite)

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fluoride sulfide bromide diphosphide iodide tetrachloride oxide phosphide iridium (III) calcium titanium (IV) hydrochloric acid barium trinitrogen hydrofluoric acid zinc nitrogen gold (III) sodium Ir Ca Ti H Ba N 3 H Zn N Au Na F 3 S S 2 Cl(aq) Br 2 P 2 F(aq) I 2 Cl 4 2 O 3 3 P Ionic/variable Ionic/fixed Ionic/variable Acid Ionic/fixed Covalent Acid Ionic/fixed Covalent Ionic/variable Ionic/fixed Overall Nomenclature Practice

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dichromate hydroxide acid acetate acid sulfate cyanide nitrite chlorate phosphate acid iridium (III) calcium nitric platinum (II) bromous strontium potassium zinc manganese (IV) gold (III) sulfurous (Cr 2 O 7 ) 3 (OH) 2 NO 3 (aq) (CH 3 COO) 2 BrO 2 (aq) SO 4 CN (NO 2 ) 2 (ClO 3 ) 4 PO 4 SO 3 (aq) Ir 2 Ca H Pt H Sr K Zn Mn Au H2H2 Ionic/variable Ionic/fixed Acid Ionic/variable Acid Ionic/fixed Ionic/variable Acid Ionic Nomenclature Practice

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Covalent Ionic (M + NM) Two or more NMsVariable charge cation Fixed charge cation 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 these? 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 N2O5N2O5 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

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Suffixes have meaning -idebinary compound sodium chloride (NaCl) -ite or -atepolyatomic compound sulfite(SO 3 2- ) sulfate (SO 4 2- )-ate means one more oxygen than -ite -olalcohol methyl alcohol (methanol) -osesugar sucrose -aseenzyme sucrase

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Extra Slides H H O S O O O

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Compounds Containing Polyatomic Ions Insert name of ion where it should go in the compounds name. Write formulas: iron (III) nitrate ammonium phosphide ammonium chlorite zinc phosphate lead (II) permanganate Fe(NO 3 ) 3 (NH 4 ) 3 P NH 4 ClO 2 Zn 3 (PO 4 ) 2 Pb(MnO 4 ) 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 32 2

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Write names: (NH 4 ) 2 S 2 O 3 AgBrO 3 (NH 4 ) 3 N U(CrO 4 ) 3 Cr 2 (SO 3 ) 3 Writing Formulas of Ionic Compounds ammonium thiosulfate silver bromate ammonium nitride uranium (VI) chromate chromium (III) sulfite CrO 4 2 SO 3 2 3 32 Cr U ? ? 6+ 3+

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Element Latin root -ic -ous gold, Auaur- Au 3+ Au 1+ lead, Pbplumb- Pb 4+ Pb 2+ tin, Snstann- Sn 4+ Sn 2+ copper, Cucupr- Cu 2+ Cu 1+ iron, Feferr- Fe 3+ Fe 2+ 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!) ; (delicious food is not good for you!)

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Cu 2 S AuN FeF 2 plumbic phosphide plumbous phosphide stannic chloride Fe 2+ Write formulas:Write names: cuprous sulfide auric nitride ferrous fluoride Pb 3 P 4 3 Pb ? 4 P 3 Cu 1+ Pb 3 P 2 3 Pb ? 2 P 3 Au 3+ SnCl 4 Sn ? 4 Cl 1 S 2 N 3 F 1

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Polyatomic Ion: a group of atoms that stay together and have a single, overall charge. BrO 4 1- Perbromate ion BrO 3 1- Bromate ion BrO 2 1- Bromite ion BrO 1- Hypobromite ion CO 4 2- CO 3 2- Carbonate ion CO 2 2- CO 2- ClO 4 1- ClO 3 1- Chlorate ion ClO 2 1- ClO 1- IO 4 1- IO 3 1- Iodate ion IO 2 1- IO 1- NO 4 1- NO 3 1- Nitrate ion NO 2 1- NO 1- PO 5 3- PO 4 3- Phosphate ion PO 3 3- PO 2 3- SO 5 2- SO 4 2- Sulfate ion SO 3 2- SO 2 2- 1 more oxygennormal1 less oxygen2 less oxygen

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Two nonmetalsMultiple-charge cationEverything 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 N2O5N2O5 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

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Two nonmetalsMultiple-charge cationEverything 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

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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 givenwrite the proper name. When a name is givenwrite the proper formula. 3) BaO 4) lithium bromide 5) Ni 2 S 3 6) triphosphorus heptoxide 7) N 2 O 5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT) CH 3 C 6 H 2 (NO 2 ) 3 10) phosphoric acid H 3 PO 4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb 2+ or Pb 4+ )

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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 givenwrite the proper name. When a name is givenwrite the proper formula. 3) BaO 4) lithium bromide 5) Ni 2 S 3 6) triphosphorus heptoxide 7) N 2 O 5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT) CH 3 C 6 H 2 (NO 2 ) 3 10) phosphoric acid H 3 PO 4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb 2+ or Pb 4+ ) POP QUIZ