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Common Polyatomic Ions

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1 Common Polyatomic Ions
Names of Common Polyatomic Ions Ion Name Ion Name NH ammonium CO carbonate *NO *nitrite HCO bicarbonate NO nitrate *IO *iodate *SO *sulfite *IO *periodate SO sulfate *ClO *hypochlorite HSO hydrogen sulfate *ClO *chlorite OH hydroxide ClO chlorate CN cyanide *ClO *perchlorate C2H3O acetate *BrO *bromate MnO permanganate C2O oxalate PO phosphate Cr2O dichromate *PO *phosphite CrO chromate H2PO dihydrogen phosphate O peroxide Memorize the BOLD ions * = you will be responsible for knowing these Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100

2 *Charges NEVER change between different forms
Polyatomic Ion Trends *Charges NEVER change between different forms +1 oxygen “Per____ate” “Normal” “–ate” form BrO3- bromate ClO3- chlorate IO3- iodate NO3- nitrate CO32- carbonate SO42- sulfate PO43- phosphate -1 oxygen “-ite” form -2 oxygens “hypo___ite” BrO4- ClO4- IO4- BrO2- ClO2- IO2- NO2- CO22- SO32- PO33- BrO- ClO- IO- perbromate bromite hypobromite perchlorate chlorite hypochlorite periodate iodite hypoiodite nitrite carbonite sulfite phosphite

3 Atomic Theory Review

4 Electron Cloud Model Orbital (“electron cloud”) instead of “orbits”
Region in space where there is 90% probability of finding an electron Orbital Shape Orbital 90% probability of finding the electron Electron Probability vs. Distance 40 30 Electron Probability (%) 20 10 50 100 150 200 250 Distance from the Nucleus (pm) Courtesy Christy Johannesson

5 Shapes of s, p, and d-Orbitals
each holds 2 electrons (s2) each of 3 orbitals holds 2 e - = 6 total p electrons (p6) each of 5 orbitals holds 2 e - = 10 total d electrons (d10)

6 s, p, and d-orbitals s orbitals: p orbitals: d 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

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

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

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

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

11 Periodic Patterns for Electron Config
8 1 2 1 2 3 4 5 6 7 3 4 5 6 7 1s 2s 3s 4s 5s 6s 7s 1s 2p 3p 4p 5p 6p 7p d (n-1) 3d 4d 5d 6d 6 7 f (n-2) 4f 5f

12 1s1 Periodic Patterns 1st Period s-block Example - Hydrogen
# of e- in that orbital(s) 1st Period s-block Courtesy Christy Johannesson

13 Electron Configuration Review
S 32.066 16 Electron Configuration Review Longhand Configuration S 16e- 1s2 2s2 2p6 3s2 3p4 Core Electrons Valence Electrons (Highest energy level) Shorthand Configuration S 16e- [Ne] 3s2 3p4 Courtesy Christy Johannesson

14 [Ar] 4s2 3d10 4p2 Periodic Patterns Ge Example - Germanium 32 72.61
Courtesy Christy Johannesson

15 Shorthand Configuration
neon's electron configuration(1s22s22p6) A B 3rd energy level (or 3rd period) [Ne] [Ne] 3s1 1 electron in the s orbital C D orbital shape (s,p,d,f…etc.) [ ] Na = 1s22s22p6 3s1 electron configuration

16 Shorthand Configuration Practice
Element symbol Electron configuration Ca [Ar] 4s2 V [Ar] 4s2 3d3 F [He] 2s2 2p5 Ag [Kr] 5s2 4d9 I [Kr] 5s2 4d10 5p5 Xe [Kr] 5s2 4d10 5p6 Fe [He] 2s22p63s23p64s23d6 [Ar] 4s23d6 Sg [Rn] 7s2 5f14 6d4

17 Periodic Patterns Review
energy level (subtract for d & f) Group # (1-8…excluding d block) total # of valence e- Column within Sublevel block # of e- in sublevel/orbital Courtesy Christy Johannesson

18 Periodic Patterns and Charge Trends
+1 +2 d 1 2 3 4 5 6 7 +3 - 3 - 2 - 1 1s NON-METALS Variable Charge METALS 6 7 f (n-2)

19 Electron Configurations for Cations
Metals lose e- to attain a noble gas configuration Metals form positive ions Cations are “paws”itive Metal ions will lose e- from configuration Na: 1s22s22p63s1 Na+: 1s22s22p6 noble gas configuration

20 Formation of a Cation sodium atom sodium ion Na Na+ [Ne] 3s1 [Ne] 11p+
loss of one valence electron 11p+ e- e- e- e- e- e-

21 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 1s22s22p63s23p4 (6 valence electrons) + 2e- S2- 1s22s22p63s23p6 (noble gas configuration)

22 Formation of an Anion chlorine atom chloride ion Cl Cl – [Ne]3s23p5
[Ne]3s23p6 or [Ar] gain of one valence electron e- e- e- 17p+ e- e- e- e- e- e- 17p+ e- e- e- e- e- e- e- e- e- e-

23 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

24 Bonding Review and Writing Ionic Formulas
Table salt Bonding Review and Writing Ionic Formulas

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

26 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

27 K+ e- Br - e- Br K potassium atom bromine atom K+ O2- K+ potassium ion potassium bromide bromide ion potassium oxide KBr K2O Mg2+ Br - Br - magnesium bromide MgBr2

28 ? Bonding Practice NaOH AlN Pb4+ N3- Pb3N4 CaBr2 lead (IV) nitride
Mg2+ OH - Ca2+ ? OH - Pb4+ Pb N3- Pb3N4 N3- CaBr2 Mg(OH)2 lead (IV) nitride Ca(OH)2 or CaO plumbic nitride

29 (NH4)3PO4 Ca3(PO4)2 Al2O3 FeO Ca2+ PO43- NH4+ PO43- Al3+ O2- NH4+ Ca2+

30 Subscripts, Superscripts and Coefficients
Mg2+ PO43- Mg3(PO4 )2 5 coefficient subscripts MAGNESIUM PHOSPHATE

31 Writing Formulas of Ionic Compounds
chemical 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+ and F– Ba and O2– Na+ and O2– Ba and F– NaF BaO Na2O BaF2

32 The Importance of Parentheses
Calcium hydrox ide ide Ca2+ OH- Ca - O H CaOH2 vs. Ca(OH)2 HO - Ca - OH The formulas imply two totally different compounds!

33 Writing Formulas w/Polyatomic Ions
Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion Ba and SO42– BaSO4 Mg and NO2– Mg(NO2)2 NH4+ and ClO3– NH4ClO3 Sn4+ and SO42– Sn(SO4)2 Fe3+ and Cr2O72– Fe2(Cr2O7)3 NH4+ and N3– (NH4)3N

34 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!) Element Latin root ic ous gold, Au aur- Au Au1+ lead, Pb plumb- Pb Pb2+ tin, Sn stann- Sn Sn2+ copper, Cu cupr- Cu Cu1+ iron, Fe ferr- Fe Fe2+

35 Write formulas: Write names: cuprous sulfide Pb3P4 3 Pb? 4 P3– Cu1+ S2– Cu2S plumbic phosphide auric nitride Pb3P2 3 Pb? 2 P3– Au3+ N3– AuN plumbous phosphide ferrous fluoride SnCl4 Sn? 4 Cl1– Fe2+ F1– FeF2 stannic chloride

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

37 Teacher: What is the formula for water?
Student: H, I, J, K, L, M, N, O Teacher: That’s not what I taught you. Student: But you said the formula for water was…H to O. "H-O-H"?! WHAT'S THAT SPELL?! WATER? mis mis Website: Dihydrogen monoxide Information Campaign “Little Johnny took a drink, Now he shall drink no more. For what he thought was H2O, Was H2SO4.” A sign outside the chemistry hotel reads “Great Day Rates, Even Better NO3-1s” What do you do with a dead chemist? Barium Under aged Pb walks into a bar and the bartender turns to the gold Bouncer and says, “Au, get the lead out!”

38 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 a metal with a variable charge and a non-metal (ionic) Contain H+ with various anions (ionic when aqueous) Contain 2 or more nonmetals only

39 Variable charge cations Elemental anions
Fixed charge cations Variable charge cations 1+ H 1 He 2 Elemental anions H 1 1 2+ 3+ 3- 2- 1- Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 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 4 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 5 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 6 * Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 7 W La 57 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 Ac 89 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

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

41 Fixed Charge Compound Nomenclature
Metals (fixed charge) + Nonmetals Objectives: To predict the ionic charge on a cation in a binary ionic compound. To write systematic names and formulas for binary ionic compounds.

42 Fixed Charge Compounds
Compounds that contain a metal with a fixed charge (group 1, 2, and 3, with Zn2+, 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-) sodium chloride CaS (Ca2+ S2-) calcium sulfide AlI3 (Al3+ 3I-) aluminum iodide

43 Common Simple Cations and Anions
Cation Name Anion Name* H+ hydrogen H - hydride Li+ lithium F - fluoride Na+ sodium Cl - chloride K+ potassium Br - bromide Cs+ cesium I - iodide Be2+ beryllium O 2- oxide Mg2+ magnesium S 2- sulfide Al3+ aluminum N 3- nitride Ag+ silver P 3- phosphide Zn2+ zinc *The root is given in color EXCEPTIONS Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86

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

45 Fixed Charge Naming Practice
Formula Name barium oxide BaO ____________________ ________________ sodium bromide MgI2 ____________________ KCl ____________________ ________________ strontium fluoride ________________ cesium fluoride NaBr magnesium iodide potassium chloride SrF2 CsF

46 Fixed Charge Nomenclature w/Polyatomic Ions
Simply insert the name of the polyatomic ion into the final name Ba2+ and SO42– BaSO4 barium sulfate Mg2+ and NO2– Mg(NO2)2 magnesium nitrite NH4+ and ClO3– NH4ClO3 ammonium chlorate Al3+ and SO42– Al2(SO4)3 alumnium sulfate Na+ and Cr2O72– Na2Cr2O7 sodium dichromate NH4+ and N3– (NH4)3N ammonium nitride

47 Polyatomic Ions Quiz PO43- …………… phosphate SO42- …………… sulfate
Cr2O72- ………….. MnO4- ………….. CH3COO- ……. phosphate sulfate dichromate permanganate acetate

48 Variable Charge Compound Nomenclature
Metals (variable charge) + Nonmetals Objectives: To predict the ionic charge on a cation in a binary ionic compound. To write systematic names and formulas for binary ionic compounds.

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

50 Variable charge cations Elemental anions
Single charge cations 1+ Variable charge cations H 1 He 2 Elemental anions H 1 1 2+ 3+ 3- 2- 1- Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 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 4 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 5 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 6 * Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 7 W La 57 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 Ac 89 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

51 Variable Charge Ionic Compounds
Compounds that contain a metal with variable charge (Pb, Sn, and the transition metals—not including Ag or Zn), and a non-metal To name, given the formula: 1. Figure out charge on cation Stock System of nomenclature 2. Write name of cation 3. Write Roman numerals in ( ) to show cation’s charge

52 Variable charge Naming Practice
4. Write name of anion: FeO Fe? O2– Fe2O3 2 Fe? 3 O2– CuBr Cu? Br – CuBr2 Cu? 2 Br – iron(II) oxide iron(III) oxide copper(I) bromide copper(II) bromide

53 Variable Charge Cations
Common 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 bonded together in pairs to form Hg2 2+ Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90

54 Variable Charge Ionic Compounds
To find the formula, given the name: 1. Write symbols for the two types of ions 2. Balance charges to write formula cobalt (III) chloride Co3+ Cl– tin (IV) oxide Sn4+ O2– tin (II) oxide Sn2+ O2– CoCl3 SnO2 SnO

55 Naming Variable Charge Ionic Compounds
Formula Name mercury (I) oxide Hg2O ____________________ HgO ____________________ ________________ copper (II) fluoride ________________ copper (I) sulfide Cr2O3 ____________________ ________________ lead (IV) oxide mercury (II) oxide CuF2 Cu2S chromium (III) oxide PbO2

56 Ionic Compounds with Polyatomic Ions
Fe3(PO4) 2 ________________ iron (II) phosphate ________________ ammonium carbonate ________________ aluminum sulfate V2SO3 ____________________ AgCN ____________________ Ba(ClO3)2 ____________________ ________________ copper (II) hydroxide (NH4)2CO3 Al2(SO4)3 vanadium (I) sulfite silver cyanide barium chlorate Cu(OH)2

57 Acidic Compounds Oxysalts + H2O  Oxyacids

58 Acidic Compounds (Nonmetals Dissolved in Water)
Acids(aq) without oxygen 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. (aq) = aqueous or dissolved in water Examples: *HCl(aq) HBr(aq) Hydrochloric acid Hydrobromic acid *The name of this gas would be hydrogen monochloride if it was NOT dissolved in water.

59 Acidic Compounds Nonmetals Dissolved in Water
Acids(aq) WITH oxygen (oxyacids) 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: HClO3(aq) HBrO(aq) ClO3- = chlorate Chloric acid BrO- = hypobromite Hypobromous acid

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

61 Common Oxyacid Names The following table lists the most common families of oxy acids. one more oxygen atom HClO4 perchloric acid most “common” HClO3 chloric acid H2SO4 sulfuric acid H3PO4 phosphoric acid HNO3 nitric acid one less oxygen HClO2 chlorous acid H2SO3 sulfurous acid H3PO3 phosphorous acid HNO2 nitrous acid two fewer oxygens HClO hypochlorous acid H3PO2 hypophosphorous acid

62 Acid Nomenclature Practice
Formula Name hydrochloric acid HCl ____________________ HClO ____________________ ________________ sulfuric acid ________________ hydrofluoric acid H3N ____________________ ________________ periodic acid hypochlorous acid H2SO4 HF hydronitric acid HIO4

63 Covalent Compounds Nonmetal + Nonmetal Objectives:
To write systematic names and formulas for binary molecular compounds.

64 Writing Formulas of 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 don’t 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 di 7 hepta 3 tri 8 octa 4 tetra 9 nona 5 penta 10 deca Prefixes to memorize!

65 Covalent Nomenclature Practice
EXAMPLES: carbon dioxide CO dinitrogen trioxide SF6 carbon tetrachloride NI3 CO2 carbon monoxide N2O3 sulfur hexafluoride CCl4 nitrogen triiodide

66 More Practice with covalent compounds…
As2S3 ________________ diarsenic trisulfide ________________ sulfur dioxide P2O5 ____________________ ________________ nitrogen trihydride N2O5 ____________________ H2O ____________________ SO2 diphosphorus pentoxide NH3 dinitrogen pentoxide dihydrogen monoxide

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

68 Overall Nomenclature Practice
Ir Ca Ti H Ba N3 Zn N Au Na F3 S S2 Cl(aq) Br2 P2 F(aq) I2 Cl4 2O3 3P iridium (III) calcium titanium (IV) hydrochloric acid barium trinitrogen hydrofluoric acid zinc nitrogen gold (III) sodium fluoride sulfide bromide diphosphide iodide tetrachloride oxide phosphide Ionic/variable Ionic/fixed Acid Covalent

69 Ionic Nomenclature Practice
Ir2 Ca H Pt Sr K Zn Mn Au H2 (Cr2O7)3 (OH)2 NO3 (aq) (CH3COO)2 BrO2(aq) SO4 CN (NO2)2 (ClO3)4 PO4 SO3 (aq) iridium (III) calcium nitric platinum (II) bromous strontium potassium zinc manganese (IV) gold (III) sulfurous dichromate hydroxide acid acetate sulfate cyanide nitrite chlorate phosphate Ionic/variable Ionic/fixed Acid

70 Covalent Ionic (M + NM) Ionic (M + NM) Two or more NM’s
Variable charge cation Fixed charge cation carbon tetrabromide sulfur dichloride N2O5 NCl3 vanadium (II) chromate niobium (V) perchlorate Mn2S5 Pt(IO3)4 rubidium sulfate barium oxide NH4ClO3 KI Greek prefixes Roman numeral Roman numeral for name only Charge Polyatomic ions OK Polyatomic ions OK Where would you file these? Criss-Cross Rule VCrO4 VCrO4 dinitrogen pentoxide dinitrogen pentoxide BaO BaO platinum (IV) iodate platinum (IV) iodate CBr4 CBr4 ammonium chlorate ammonium chlorate Roman numeral Nb(ClO4)5 Nb(ClO4)5 potassium iodide potassium iodide SCl2 SCl2 nitrogen trichloride nitrogen trichloride Rb2SO4 Rb2SO4 manganese (V) sulfide manganese (V) sulfide

71 Suffixes have meaning “-ide” binary compound
sodium chloride (NaCl) “-ite” or “-ate” polyatomic compound sulfite (SO32-) sulfate (SO42-) “-ate” means one more oxygen than “-ite” “-ol” alcohol methyl alcohol (methanol) “-ose” sugar sucrose “-ase” enzyme sucrase

72 Extra Slides H O S

73 Compounds Containing Polyatomic Ions
Insert 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 Fe3+ 3 NO31– Fe(NO3)3 3 NH41+ P3– (NH4)3P NH41+ ClO21– NH4ClO2 3 Zn2+ 2 PO43– Zn3(PO4)2 Pb2+ 2 MnO41– Pb(MnO4)2

74 Writing Formulas of Ionic Compounds
Write names: (NH4)2S2O3 AgBrO3 (NH4)3N U(CrO4)3 Cr2(SO3)3 ammonium thiosulfate silver bromate ammonium nitride U ? 6+ 3 CrO42– uranium (VI) chromate 2 Cr ? 3+ 3 SO32– chromium (III) sulfite

75 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!) Element Latin root ic ous gold, Au aur- Au Au1+ lead, Pb plumb- Pb Pb2+ tin, Sn stann- Sn Sn2+ copper, Cu cupr- Cu Cu1+ iron, Fe ferr- Fe Fe2+

76 Write formulas: Write names: cuprous sulfide Pb3P4 3 Pb? 4 P3– Cu1+ S2– Cu2S plumbic phosphide auric nitride Pb3P2 3 Pb? 2 P3– Au3+ N3– AuN plumbous phosphide ferrous fluoride SnCl4 Sn? 4 Cl1– Fe2+ F1– FeF2 stannic chloride

77 BrO41- BrO31- BrO21- BrO1- CO42- CO32- CO22- CO2- ClO41- ClO31- ClO21-
Polyatomic Ion: a group of atoms that stay together and have a single, overall charge. BrO41- Perbromate ion BrO31- Bromate ion BrO21- Bromite ion BrO1- Hypobromite ion CO42- CO32- Carbonate ion CO22- CO2- ClO41- ClO31- Chlorate ion ClO21- ClO1- IO41- IO31- Iodate ion IO21- IO1- NO41- NO31- Nitrate ion NO21- NO1- PO53- PO43- Phosphate ion PO33- PO23- SO52- SO42- Sulfate ion SO32- SO22- 1 more oxygen “normal” 1 less oxygen 2 less oxygen

78 Multiple-charge cation Everything else
Two nonmetals Multiple-charge cation Everything else carbon tetrabromide sulfur dichloride N2O5 NCl3 vanadium (II) chromate niobium (V) perchlorate Mn2S5 Pt(IO3)4 rubidium sulfate barium oxide NH4ClO3 KI Greek prefixes Roman numeral for name only Roman numeral Charge Polyatomic ions OK Polyatomic ions OK Where would you file this? Criss- Cross Rule VCrO4 VCrO4 dinitrogen pentoxide dinitrogen pentoxide BaO BaO platinum (IV) iodate platinum (IV) iodate CBr4 CBr4 ammonium chlorate ammonium chlorate Roman numeral Nb(ClO4)5 Nb(ClO4)5 potassium iodide potassium iodide SCl2 SCl2 nitrogen trichloride nitrogen trichloride Rb2SO4 Rb2SO4 manganese (V) sulfide manganese (V) sulfide

79 Multiple-charge cation Everything else
Two nonmetals Multiple-charge cation Everything else Greek prefixes Roman numeral for name only Roman numeral Charge Polyatomic ions OK Polyatomic ions Where would you file this? Criss- Cross Rule VCrO4 dinitrogen pentoxide BaO platinum (IV) iodate CBr4 ammonium chlorate Roman numeral Nb(ClO4)5 potassium iodide SCl2 nitrogen trichloride Rb2SO4 manganese (V) sulfide

80 Write the compound formed by the following ions:
1) Al3+ S2- 2) Mg2+ PO43- 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 Write the total number of atoms that make up each compound. Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)

81 POP QUIZ Write the compound formed by the following ions: 1) Al3+ S2-
2) Mg2+ PO43- 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 Write the total number of atoms that make up each compound. Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)


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