1. Atoms, Molecules, Ions, and Inorganic Nomenclature Brown, LeMay Ch 2 AP Chemistry Monta Vista High School

2. 2 2.2: Evidence for the Atomic Theory 1.J.J. Thomson’s cathode ray tube: discovery of electrons and the e- charge-to-mass ratio  In a vacuum chamber, flow of high voltage (emitted from cathode to anode) is deflected by magnetic & electrical fields http://highered.mcgraw- hill.com/olcweb/cgi/pluginpop.cgi?it=swf::100%::100%::/sites/dl/free/0072512644/117354/01_Cathode_Ray_Tube.swf::Cathode%20R ay%20Tube http://highered.mcgraw- hill.com/olcweb/cgi/pluginpop.cgi?it=swf::100%::100%::/sites/dl/free/0072512644/117354/01_Cathode_Ray_Tube.swf::Cathode%20R ay%20Tube

3. 2.Robert Millikan’s oil drop: determines charge of e- (and thus the mass)  “Atomized” drops of oil picked up small charges (integral numbers), and balanced oil drops in an electrical & gravitational field http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/004_MILLIKANOIL.MOV http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/004_MILLIKANOIL.MOV

4. 3.Ernest Rutherford’s gold foil: discovery of nucleus as center of positive charge  Alpha particles from radioactive source are deflected from positive gold atom nuclei http://www.mhhe.com/physsci/chemistry/ani mations/chang_2e/rutherfords_experiment.s wf

5. 5 2.3: Structure of the Atom Figure 1: Subatomic particles (Table 2.1; 1 amu = 1.66054 x 10 -24 g). Subatomic particle ChargeLocationMass Proton, p + +1.6 x 10 -19 Cnucleus1.0073 amu Neutron, nNonenucleus1.0087 amu Electron, e - -1.6 x 10 -19 Ce- cloud5.486 x 10 -4 amu

6. 6 Atomic number: number of p + (determines the element) Mass number: sum of p + and n (determines the isotope) Isotopes: atoms of an element that differ in the number of neutrons Isobars: atoms of different elements with same atomic mass but different atomic number. Groups or families: columns on Periodic Table: alkali (1A), alkaline earth (2A), halogens (7A), noble or inert gases (8A); pnictogens (5A) and chalcogens (6A); have same number of valence e - Periods: rows on P.T.; indicates new shell of e - Cations: positively charged ions Anions: negatively charged ions Vocabulary

7. For naming compounds, it is important to identify the type of compound because naming varies with the type of compound. 1. Ionic Compounds - monoatomic ions -polyatomic ions - cations w/variable valency 2. Molecular Compounds 3. Acids- named after anions. Anion ending in –ate; acid named –ic acid, anion ending in – ite; acid ending in –ous acid. 7

8. 8 Two types of acids: a. without oxygen b. oxyacids Hydrates: Coordination Compounds:

9. Figure 2: Inorganic nomenclature; commonly used but not easily predictable cations +4 cations+3 cations Lead (IV) or plumbicPb 4+ Antimony (III) or antimonousSb 3+ Tin (IV) or stannicSn 4+ Arsenic (III) or arsenousAs 3+ Titanium (IV)Ti 4+ Bismuth (III)Bi 3+ Chromium (III) or chromicCr 3+ Cobalt (III) or cobalticCo 3+ Gold (III) or auricAu 3+ Iron (III) or ferricFe 3+ Titanium (III)Ti 3+

10. Figure 2: Inorganic nomenclature; commonly used but not easily predictable cations +2 cations+1 cations CadmiumCd 2+ AmmoniumNH 4 + Cobalt (II) or cobaltousCo 2+ Copper (I) or cuprousCu + Copper (II) or cupricCu 2+ Gold (I) or aurousAu + Iron (II) or ferrousFe 2+ HydroniumH3O+H3O+ Lead (II) or plumbousPb 2+ SilverAg + Mercury (I) or mercurousHg 2 2+ Mercury (II) or mercuricHg 2+ NickelNi 2+ Tin (II) or stannousSn 2+ ZincZn 2+

11. Figure 3: Inorganic nomenclature; commonly used but not easily predictable anions -3 anions-2 anions BorateBO 3 3- CarbonateCO 3 2- PhosphatePO 4 3- ChromateCrO 4 2- DichromateCr 2 O 7 2- OxalateC 2 O 4 2- PeroxideO 2 2- SelenateSeO 4 2- SulfateSO 4 2-

12. Figure 3: Inorganic nomenclature; commonly used but not easily predictable anions -1 anions AcetateC2H3O2-C2H3O2- IsothiocyanateCNS - BromateBrO 3 - HydroxideOH - ChlorateClO 3 - NitrateNO 3 - CyanideCN - PermanganateMnO 4 - HydrideH-H- SuperoxideO2-O2- IodateIO 3 - ThiocyanateSCN -

13. 13 Naming Hydrates Name the compound, then the Greek prefix, and then add -hydrate. Ex:CuSO 4 ۰5 H 2 O copper (II) sulfate pentahydrate

14. 14 Naming Oxyacids & Oxyanions Oxyacid: polyatomic acid that contains a nonmetal bonded to one or more oxygen atoms Figure 4: The “standard” oxyacids (___ic acids) H 3 BO 3 H 2 CO 3 HNO 3 XX X H 3 PO 4 H 2 SO 4 HClO 3 H 3 AsO 4 H 2 SeO 4 HBrO 3 XHIO 3 Also: H 2 CrO 4 = chromic acid

15. Oxyanions: polyatomic anions that contain a nonmetal bonded to one or more oxygen atoms. Figure 5: Naming oxyacids and oxyanions Oxyacids Example Format Oxyanions Example Format Oxida -tion # Perchloric acid, HClO 4 Per_____ic acidPerchlorate, ClO 4 - per___ate +7 Chloric acid, HClO 3 _____ic acidChlorate, ClO 3 - ___ate +5 Chlorous acid, HClO 2 _____ous acidChlorite, ClO 2 - ___ite +3 Hypochlorous acid. HClO Hypo_____ous acid Hypochlorite, ClO - hypo___ite +1

16. Figure 6: Complete for sulfur oxyacids & oxyanions. OxyacidOxyanion Oxidation # (Persulfuric acid)(H 2 S 2 O 8 )(Persulfate)(S 2 O 8 2- )(+7) Sulfuric acidH 2 SO 4 SulfateSO 4 2- +6 Sulfurous acidH 2 SO 3 SulfiteSO 3 2- +4 Hyposulfurous acidH 2 SO 2 HyposulfiteSO 2 2- +2

17. 17 Other Oxyacids Patterns H 3 PO 4 phosphoric acid H 2 PO 4 1- dihydrogen phosphate HPO 4 2- hydrogen (or monohydrogen) phosphate PO 4 3- phosphate H 2 CO 3 carbonic acid HCO 3 1- hydrogen carbonate or bicarbonate CO 3 2- carbonate

18. Chemistry of Coordination Compounds Brown, LeMay Ch 24 AP Chemistry Monta Vista High School To properly view this presentation on the web, use the navigation arrows below and left-click on each page to view any animations.

19. 24.1: Structure of Complexes Complex: species in which a central metal ion (usually a transition metal) is bonded to a group of surrounding molecules or ions Coordination compound: compound that contains a complex ion or ions.

20. A coordination compound, or complex, consists of: Metal ion Ligand or complexing agent: molecule or ion with a lone pair of e - that bonds to a metal ion

21. Lewis Structures of common ligands NH 3 CN - S 2 O 3 2- SCN - H 2 O (not always included in formula, however)

22. Notation Write complexes in square brackets, with charge on outside Ex: Cu 2+ (aq) + 4 NH 3 (aq) → [Cu(NH 3 ) 4 ] 2+ (aq) H | Cu 2+ (aq) + 4 :N ─ H (aq) → Cu | H :NH 3 H 3 N: :NH 3 2+

23. 24.3: Nomenclature 1.Name cation before anion; one or both may be a complex. (Follow standard nomenclature for non- complexes.) 2.Within each complex (neutral or ion), name all ligands before the metal. Name ligands in alphabetical order If more than one of the same ligand is present, use a numerical prefix: di, tri, tetra, penta, hexa, … Ignore numerical prefixes when alphabetizing.

24. Neutral ligands: use the name of the molecule (with some exceptions) NH 3 ammine-H 2 Oaqua- Anionic ligand: use suffix –o Br - bromo-CN - cyano- Cl - chloro- OH - hydroxo- 3.If the complex is an anion, use –ate suffix Record the oxidation number of the metal in parentheses (if appropriate). Ex: [Co(NH 3 ) 5 Cl]Cl 2 pentamminechlorocobalt (III) chloride

25. Nomenclature practice 1. K 4 [Fe(CN) 6 ] 2. [Cr(NH 3 ) 4 (H 2 O)CN]Cl 2 3. Na[Al(OH) 4 ] potassium hexacyanoferrate tetrammineaquacyanochromium (III) chloride sodium tetrahydroxoaluminate

26. Practice Websites for Naming 26 http://quizlet.com/526633/polyatomic-ions-flash-cards/ http://quizlet.com/206265/polyatomic-ion-quiz-flash-cards/ http://www.sciencegeek.net/Concentration/Anions/anions.html http://www.sciencegeek.net/Concentration/Monatomics/monatomi c.html http://www.sciencegeek.net/APchemistry/APtaters/directory.shtml http://www.syvum.com/cgi/online/serve.cgi/contrib/chem/Polyatom s.tdf?0

27. Naming Compounds Flow Chart Does the formula start with H? NO YES Does it begin with a metal that has more than one oxidation number? (e.g. Fe, Ni, Cu, Sn, Hg) NOYES Does the formula contain a polyatomic ion? NOYES Are both elements nonmetals? NO YES Name the first element, Then the second element with an –ide ending. Name the first element using the proper prefix (never mono–). Name the second element with the proper prefix (including mono–) and –ide ending. 1 = mono– 4 = tetra– 7 = hepta– 10 = deca– 2 = di–5 = penta– 8 = octa– 3 = tri–6 = hexa–9 = nona– (not nano–) Name the first element, then the polyatomic ion. If two elements are present, name both, then the polyatomic ion (e.g. NaHCO 3 is sodium hydrogen carbonate). It is an acid (must be aqueous). Does the acid contain a polyatomic ion? NOYES Does the acid end with a polyatomic ion? –ite–ate Name the polyatomic ion, replacing the –ate ending with –ic. Add the word acid. Name the polyatomic ion, replacing the –ite ending with –ous. Add the word acid. Write the prefix hydro–, then the name of the second element with –ic ending. Add the word acid. Name the first element followed by its oxidation number (Roman Numeral) or “old school” –ic or –ous endings.