1. Elfi Susanti VH SBI CLASS Chemistry Department FKIP UNS

8. Electron Configurations in the Periodic Table

9. H 1 1s 1 [CORE] VALENCE SHELL He 2 1s 2 Li 3 1s 2 2s 1 [1s 2 ]2s 1 Be 4 1s 2 2s 2 [1s 2 ]2s 2 B 5 1s 2 2s 2 2p 1 [1s 2 ]2s 2 2p x 1 C 6 1s 2 2s 2 2p 2 [1s 2 ]2s 2 2p x 1 2p y 1 N 7 1s 2 2s 2 2p 3 O 8 1s 2 2s 2 2p 4 F 9 1s 2 2s 2 2p 5 Ne 10 1s 2 2s 2 2p 6 Na 11 1s 2 2s 2 2p 6 3s 1 [1s 2 2s 2 2p 6 ]3s 1

10. E N E R G Y 1s 2s 2p 3s 3p 4s 3d

12. Be [1s 2 ] 2s 2 Be . . nuclues Valence Electron

13. Table 1-2 in text The A groups are regular.

17. Structure formula

19. Structural Formulas for C 4 H 10 O Isomers Kekulé Formula Condensed Formula Shorthand Formula

24. Covalen bonding

25. Polar Covalen bonding

26. To determine stability of compound as ion or neutral . . NH 2 - ( Formal Charge = 5 - 4 - 2 = -1 ) 5e - N : . .. N : . . . . H H

27. azide anion has two negative-charged nitrogens and one positive-charged nitrogen, the total charge being minus one. Ozone, the central oxygen atom has three bonds and a full positive charge while the right hand oxygen has a single bond and is negatively charged. The overall charge of the ozone molecule is therefore zero. nitromethane has a positive-charged nitrogen and a negative-charged oxygen, the total molecular charge again being zero.

28. _ +2 2 - Determine formal charges !!! S O O O O .. .. : .. : : .. .. : .. : : _ _ _ net ionic charge

29. Group Formula Class Name Specific Example IUPAC Name Common Name Alkene H 2 C=CH 2 Eth ene Ethylene Alkyne HC ≡ CH Eth yne Acetylene Arene C 6 H 6 Benzene Benzene

30. Group Formula Class Name Specific Example IUPAC Name Common Name Halide H 3 C-I Iodomethane Methyl iodide Alcohol CH 3 CH 2 OH Ethan ol Ethyl alcohol Ether CH 3 CH 2 OCH 2 CH 3 Diethyl ether Ether Amine H 3 C-NH 2 Aminomethane Methylamine Nitro Compound H 3 C-NO 2 Nitromethane Thiol H 3 C-SH Methane thiol Methyl mercaptan Sulfide H 3 C-S-CH 3 Dimethyl sulfide

31. Group Formula Class Name Specific Example IUPAC Name Common Name Nitrile H 3 C-CN Ethanenitrile Acetonitrile Aldehyde H 3 CCHO Ethan al Acetaldehyde Ketone H 3 CCOCH 3 Propan one Acetone Carboxylic Acid H 3 CCO 2 H Ethan oic Acid Acetic acid Ester H 3 CCO 2 CH 2 CH 3 Ethyl ethan oate Ethyl acetate Acid Halide H 3 CCOCl Ethan oyl chloride Acetyl chloride Amide H 3 CCON(CH 3 ) 2 N,N-Dimethylethanamide N,N-Dimethylacetamide Acid Anhydride (H 3 CCO) 2 O Ethan oic anhydride Acetic anhydride

32. The Shape of Molecules

34. Distinguishing Carbon Atoms

35. Resonance This averaging of electron distribution over two or more hypothetical contributing structures ( canonical forms ) to produce a hybrid electronic structure

38. Atomic and Molecular Orbitals

39. structure of methane (CH 4 ), the 2s and three 2p orbitals must be converted to four equivalent hybrid atomic orbitals , each having 25% s and 75% p character, and designated sp 3 . These hybrid orbitals have a specific orientation, and the four are naturally oriented in a tetrahedral fashion.

40. Molecular Orbitals In general, this mixing of n atomic orbitals always generates n molecular orbitals.

45. This attractive force has its origin in the electrostatic attraction of the electrons of one molecule or atom for the nuclei of another. If there were no van der Waals forces, all matter would exist in a gaseous state , and life as we know it would not be possible. It should be noted that there are also smaller repulsive forces between molecules that increase rapidly at very small intermolecular distances.

47. Boiling Points (ºC) of Selected Elements and Compounds Increasing Size Atomic Ar (40) -186 Kr (83) -153 Xe (131) -109 Molecular CH 4 (16) -161 (CH 3 ) 4 C (72) 9.5 (CH 3 ) 4 Si (88) 27 CCl 4 (154) 77 Molecular Shape Spherical: (CH 3 ) 4 C (72) 9.5 (CH 3 ) 2 CCl 2 (113) 69 (CH 3 ) 3 CC(CH 3 ) 3 (114) 106 Linear: CH 3 (CH 2 ) 3 CH 3 (72) 36 Cl(CH 2 ) 3 Cl (113) 121 CH 3 (CH 2 ) 6 CH 3 (114) 126 Molecular Polarity Non-polar: H 2 C=CH 2 (28) -104 F 2 (38) -188 CH 3 C≡CCH 3 (54) -32 CF 4 (88) -130 Polar: H 2 C=O (30) -21 CH 3 CH=O (44) 20 (CH 3 ) 3 N (59) 3.5 (CH 3 ) 2 C=O (58) 56 HC≡N (27) 26 CH 3 C≡N (41) 82 (CH 2 ) 3 O (58) 50 CH 3 NO 2 (61) 101

51. Compound Formula Mol. Wt. Boiling Point Melting Point dimethyl ether CH 3 OCH 3 46 – 24ºC – 138ºC ethanol CH 3 CH 2 OH 46 78ºC – 130ºC propanol CH 3 (CH 2 ) 2 OH 60 98ºC – 127ºC diethyl ether (CH 3 CH 2 ) 2 O 74 34ºC – 116ºC propyl amine CH 3 (CH 2 ) 2 NH 2 59 48ºC – 83ºC methylaminoethane CH 3 CH 2 NHCH 3 59 37ºC trimethylamine (CH 3 ) 3 N 59 3ºC – 117ºC ethylene glycol HOCH 2 CH 2 OH 62 197ºC – 13ºC acetic acid CH 3 CO 2 H 60 118ºC 17ºC ethylene diamine H 2 NCH 2 CH 2 NH 2 60 118ºC 8.5ºC

53. All atoms and molecules have a weak attraction for one another, known as van der Waals attraction . This attractive force has its origin in the electrostatic attraction of the electrons of one molecule or atom for the nuclei of another, and has been called London dispersion force . In general, larger molecules have higher boiling points than smaller molecules of the same kind, indicating that dispersion forces increase with mass, number of electrons, number of atoms or some combination thereof. The following table lists the boiling points of an assortment of elements and covalent compounds composed of molecules lacking a permanent dipole. The number of electrons in each species is noted in the first column, and the mass of each is given as a superscript number preceding the formula.