1. Atoms, Molecules, Ions, and Inorganic Nomenclature Brown, LeMay Ch 2 AP Chemistry

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

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

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

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 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. 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+

8. 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+

9. 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-

10. 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 -

11. 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.

12. 12 Naming Hydrates Name the compound, then the Greek prefix, and then add -hydrate. Ex:CuSO 4 ۰5 H 2 O copper (II) sulfate pentahydrate

13. 13 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

14. 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

15. 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

16. 16 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