1. Matter and Nomenclature Test Etiquette

2. The Discovery of Atomic Structure Cathode Rays and Electrons

3. The Discovery of Atomic Structure Radioactivity

4. The Modern View of Atomic Structure CyberChem-Atom/Universe

5. Atomic/Subatomic Structure Particle NucleusSurrounding ProtonNeutronElectron Abbreviation p+ne-e- Relative Mass 1~ 1.001~ 0.0005 Composition 2 u + 1 d1 u + 2 delementary Charge +10 Discovery Mass SpectrometryMass Differences Cathode Ray Tube & Oil Drop Expt. CyberChem-Big Bang

6. Quarks

7. The Modern View of Atomic Structure Isotopes, Atomic Numbers, and Mass Numbers Atomic number (Z) = number of protons in nucleus. Mass number (A) = total number of nucleons in nucleus (i.e., protons and neutrons). Isotopes: same Z but different A.

8. Examples Speciesp+p+ ne-e- charge 31 P 60 Co ? 25 5376

9. Atomic Weights The Atomic Mass Scale 1 H weighs 1.6735 x 10 -24 g and 16 O 2.6560 x 10 -23 g. We define: mass of 12 C = exactly 12 amu. Using atomic mass units: 1 amu = 1.66054 x 10 -24 g 1 g = 6.02214 x 10 23 amu

10. The Periodic Table Alkali metals Alkaline Earth metals Halogens Noble Gases Chalcogens Transition Metals Inner Transition Metals

11. Ions and Ionic Compounds Predicting Ionic Charge

12. Naming Inorganic Compounds

14. Examples: Type I - Metals combining with Nonmetals

16. Common (Type II) Cations IonSystemic NameOlder Name Fe 3+ Iron(III)Ferric Fe 2+ Iron(II)Ferrous Cu 2+ Copper(II)Cupric Cu + 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

17. Examples: Type II – Transition Metals combining with Nonmetals

19. Examples: Type III – Nonmetals combining with Nonmetals

20. Common Acids AcidName HClHydrochloric acid H2SH2SHydrosulfuric acid (liquid) Hydrogen sulfide (gas) HNO 3 Nitric acid H 2 SO 4 Sulfuric acid HC 2 H 3 O 2 Acetic acid Practice Samples Practice Samples and Key

21. FormulaNameType 1 KMnO 4 2 NBr 3 3 MgSO 4 4 LiNO 3 5 NH 3 6 Cu(NO 3 ) 2 7 AgCl 8 BaO 9 CoI 2 10 HC 2 H 3 O 2 11 aluminum hydroxide 12 sodium carbonate 13 ferric oxide 14 silicon tetrafluoride 15 ammonium phosphate 16 lead(II) sulfide 17 hydrogen peroxide 18 nitric acid 19 sulfuric acid 20 bromine trifluoride Chemistry 212(01/02/03) – Nomenclature Practice Samples

22. Some Simple Organic Compounds Alkanes Organic chemistry: the study of the chemistry of carbon compounds. Alkanes contain only C and H and are called hydrocarbons. The names of alkanes all end in the suffix –ane. Alkanes are named according to the number of C atoms in their backbone chain: Methane has one C atom (CH 4 ) Ethane has two C atoms (CH 3 CH 3 ) Propane has three C atoms (CH 3 CH 2 CH 3 ), etc. HyperC-75

24. Some Simple Organic Compounds Some Derivatives of Alkanes When H atoms in alkanes are replaced by heteroatoms (atoms other than C or H), then we have introduced a functional group into the alkane. When an H is replaced by –OH, then we form an alcohol. Alcohols are also named by the number of C atoms. Consider propanol: there are two places for the OH: on an end C or the middle C. When the OH is located on the end C, we call the substance 1-propanol. When the OH is on the middle C, we have 2-propanol. HyperC-75

25. Some Simple Organic Compounds Some Derivatives of Alkanes When the single bonds in an alkane are replaced by one or more double bonds, then we form alkenes. When a double bond is formed between C and O, we form carboxylic acids, ketones, aldehydes, and esters. Any organic molecule with double or triple bonds is called unsaturated. HyperC-75

26. Matter and Nomenclature Law of Conservation of Mass/Energy M + NM (Ionic) TM + NM (ic vs. ous) NM + NM (Covalent)