Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
PT 1: Relative Atomic Mass and Electron Configurations NAME ___________________________________________________________________________________________ 1 18 Hydrogen Helium 184.002602 1.00794 1 H 1 22.989770 2 Lithium Beryllium 6.941 9.012182 3 Li 4 Sodium 22.989770 11 Na Be Electron Configuration Potassium 13 14 Carbon Nitrogen Oxygen Fluorine Neon 10.811 12.0107 14.00674 15.9994 18.9984 20.1797 2-8-1 B 5 6 2-3 C Silicon 3 K 20 Ca 2-8-8-2 4 5 6 Scandium Titanium Vanadium Chromium 44.955910 47.867 50.9415 51.9961 21 Sc 2-8-9-2 V Ti 23 22 2-8-10-2 24 8 Manganese 54.938049 Cr 2-8-13-1 2-8-11-2 7 25 Mn 10 11 Al 13 12 Cobalt Nickel Copper Zinc Gallium Germanium Arsenic 58.6934 63.546 65.39 69.723 72.61 74.92160 Fe 27 Co 28 2-8-15-2 Ni 29 2-8-16-2 Cu 30 2-8-18-1 Zn 31 2-8-18-2 Ga 32 2-8-18-3 Ge Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin 87.62 88.90585 91.224 92.90638 95.94 (98) 101.07 102.90550 106.42 107.8682 112.411 114.818 118.710 Rb Cesium 132.90545 55 Cs **-18-8-1 38 Sr 2-8-18-8-2 Barium 137.327 56 Ba -18-8-2 39 Y 40 Zr 2-8-18-9-2 2-8-18-10-2 Lanthanum 138.9055 57 La 41 Nb 42 2-8-18-13-1 Hafnium Tantalum 178.49 180.9479 72 Hf -18-9-2 -32-10-2 73Ta -32-11-2 Rhenium Osmium Iridium 190.23 192.217 75 Re 76 Os 77 Ir -32-12-2 -32-13-2 -32-14-2 -32-15-2 Rutherfordium Dubnium Seaborgium (267) (268) (271) 89 Ac 104 Rf 105 Db 106 Sg 46 2-8-18-16-1 74W (227) Ra Rh 186.207 Actinium 88 45 183.84 (226) -32-18-8-2 Ru Tungsten Radium Fr 44 2-8-18-15-1 (223) 87 43 2-8-18-14-1 Francium -32-18-8-1 Tc Mo 2-8-18-12-1 Pd 47 2-8-18-18 Ag 48 Cd Platinum Gold Mercury Thallium 195.078 196.96655 200.59 204.3833 78 Pt 79 Au -32-17-1 -32-18-1 -32-18-2 Hassium Meitnerium Darmstadtium Roentgenium Copernicium (270) (276) (281) (280) (285) 108 Hs 109 Mt 110 Ds 111 Rg 112 50 2-8-18-18-3 80 Hg (272) Bh In 2-8-18-18-2 Bhorium 107 49 2-8-18-18-1 33 2-8-18-4 85.4678 37 P 58.933200 Rubidium 2-8-18-8-1 15 Sn Uut 113 S 17 51 Cl 18 2-8-7 Se Krypton 79.904 83.80 Br 36 2-8-18-7 Sb Ar 2-8-8 Bromine 35 2-8-18-6 Kr 2-8-18-8 Tellurium Iodine Xenon 127.60 126.90447 131.29 Te 52 53 I 54 Xe 2-8-18-18-5 2-8-18-18-6 2-8-18-18-7 2-8-18-18-8 Lead Bismuth Polonium Astatine Radon 207.2 208.98038 (209) (210) (222) 83 Bi -32-18-4 84 Po -32-18-5 114 85 At -32-18-6 Flerovium Cn Argon 39.948 34 Antimony 82 Pb -32-18-3 Chlorine 35.4527 2-8-18-6 2-8-18-18-4 81Tl Sulfur Selenium 121.760 Ne 10 2-8 32.066 2-8-6 As F 9 2-7 16 2-8-5 Iron 2-8-14-2 O 8 30.973761 Si 14 17 2-6 Phosphorus 2-8-4 2-8-3 N 7 55.845 26 2-8-13-2 9 16 2-5 28.0855 Mg 15 2-4 Aluminum 12 He Boron Letter Symbol 26.98153 Calcium 40.078 19 Na 24.3050 39.0983 2-8-8-1 2 2 Magnesium 2-8-2 2-8-1 11 Atomic Number 2-2 2-1 Element Name Sodium Atomic Mass 86 -32-18-7 Rn -32-18-8 Livermorium Fl 115 Uup 116 Lv 117 Uus -32-18-9-2 These ** indicate that there are energy levels of 2-8-18 for elements 55 & above Key: italicized symbols = synthetic (human made) an entry in ( ) indicates the longest lived isotope of an element for which the atomic mass is indeterminate Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium 140.116 140.90765 144.24 (145) 150.36 151.964 157.25 158.92534 162.500 164.93032 167.259 168.93421 173.054 174.9668 58 Ce 59 Pr 60 Nd 61 Pm Thorium Protactinium Uranium Neptunium 232.038 231.03588 238.0289 (237) Th 90 91 Pa 92 U 93 Np 62 Sm Plutonium (244) 94 Pu 63 Eu Americium 64 Am Tb Dy Curium Berkelium Californium Einsteinium Fermium (247) (247) (251) (252) (257) Cm 97 Bk 98 Cf 99 Es 68 Er 66 96 67 Ho 65 (243) 95 Gd 100 Fm Tm 69 Mendelevium (258) 101 Md Yb 70 71 Lu Nobelium Lawrencium (259) (262) 102 No 103 Lr PT 2: Categories of Elements and a Few Special "Family" Group 18 = noble gas family Group 1 = alkali metal family Group 2 = alkaline-earth metal 2 family hydrogen H 1 NM 1 1 lithium beryilium Li Be 3 M 2-1 Na 11 M name symbol atomic number Electron Configuration M Metal Metalloid Nonmetal Noble Gas M Me NM NG 2-8-1 K magnesium M M calcium Ca 20 M 2-8-8-1 2-8-8-2 rubidium strontium Rb 37 M 3 16 17 boron carbon nitrogen oxygen fluorine C N O F 6 Me scandium 6 7 8 9 10 11 12 titanium vanadium chromium manganese iron cobalt nickel copper zinc Sc 21 M 22 2-8-9-2 2-8-10-2 2-8-11-2 zirconium niobium yttrium Ti M 2-8-18-8-1 2-8-18-8-2 2-8-18-9-2 2-8-18-10-2 cesium barium lanthanum hafnium M Cs 55 M Ba 56 M 2-8-18-18-8-1 2-8-18-18-8-2 2-8-18-18-9-2 francium radium actinum Ra 88 M La 57 M Ac 89 M Zr 40 M Hf 72 M **18-32-10-2 rutherfordium Rf 104 M 23 V Cr 24 M M molybdenum Nb 41 M Mo 42 M 2-8-18-12-1 tantalum Ta 73 M -18-32-11-2 dubnium NM 2-7 2-8 aluminum silicon sulfur chlorine argon 13 Si 14 Me P S 15 NM 16 NM Cl 17 NM Ar 18 NG 2-8-4 2-8-5 2-8-6 2-8-7 2-8-8 M 2-8-3 gallium germanium phosphorus arsenic Zn 30 M Ga 31 M Ge 32 Me selenium bromine krypton As 33 SM Br 35 NM Kr 36 NG 2-8-13-2 2-8-14-2 2-8-15-2 2-8-16-2 2-8-18-1 2-8-18-2 2-8-18-3 2-8-18-4 2-8-18-5 Se 34 NM 2-8-18-6 2-8-18-7 2-8-18-8 technetium ruthenium rhodium palladium M Ru 44 M Rh 45 M 2-8-18-15-1 2-8-18-161 tungsten rhenium osmium iridium Re 75 M Os 76 M -18-32-13-2 77 2-8-18-18-1 platinum gold Pt M 78 meitnerium Hs 108 M Ag 47 M 2-8-18-18 -18-32-15-2 hassium Bh 107 M silver Pd 46 M Ir -18-32-14-2 bohrium Sg 106 M 9 Cu 29 M 2-8-18-13-2 seaborgium Db 105 M NM 2-6 neon Ne 10 NG Ni 28 M 2-8-18-131 -18-32-12-2 8 NM 2-5 18 Co 27 M Mn Tc 43 M W 74 M 7 Mt 109 M Au 79 M M -18-32-17-1 -18-32-18-1 damstadtium roentgentium Ds 110 M Rg 111 M cadmium indium Cd 48 M tin In 49 M 2-8-18-18-2 2-8-18-18-3 mercury thallium Hg 80 M Sn 50 M 2-8-18-18-4 lead Tl 81 -18-32-18-2 Pb 82 M M -18-32-18-3 copernicium -18-32-18-4 Uut Cn 112 M flerovium Fl 113 114 M antimony tellurium iodine xenon Sb 51 Me Te 52 Me I 53 NM Xe 54 NG 2-8-18-18-8 2-8-18-18-5 2-8-18-18-6 2-8-18-18-7 bismuth polonium astatine radon 85 Me Rn 86 NG Bi 83 M -18-32-18-5 Uup Po 84 M -18-32-18-6 livermorium Lv 115 116 M At -18-32-18-7 -18-32-18-8 Uus 117 NM Lanthanoid Series cerium praeseodymium Ce 58 M Pr 59 M thorium protactinium Th 90 M Pa 91 Actinoid Series M neodymium Nd 60 M uranium U 92 M NG Fe 26 M 25 2-8-13-1 NM 2-4 Al 5 Y 39 M 15 5 4 Sr 38 M Fr 87 14 B Groups 3 -11 = the transition metal family Mg 2-8-2 potassium 13 2-3 12 He 2 2 2-2 sodium 19 4 helium Group 17 = halogen family promethium Pm 61 M neptunium Np 93 M samarium Sm 62 M plutonium Pu 94 M europium gadolinium americium curium Eu 63 M Am 95 M Gd 64 M Cm 96 M terbium dysprosium Dy 66 M Ho 67 M Er 68 M Tm 69 M Yb 70 M Lu 71 M berkelium californium einsteinium fermium mendelevium nobelium lawrencium 98 99 Tb 65 M Bk 97 M Cf M holmium Es M erbium Fm 100 M thulium Md 101 M ytterbium No 102 M lutetium Lr 103 M Uuo 118 Names & Formulas of Some Monatomic Anions Name Formula Bromide Br-1 Chloride Cl-1 Fluoride F-1 Iodide I-1 Hydride H-1 Oxide O-2 Phosphide P-3 Sulfide S-2 Telluride Te-2 Name Densities & Boiling Points of Various Molecular Gases & Gas Mixtures Name Density Normal (kg/m3) @ Boiling Point STP (C) Air 1.29 -194.5 Names & Formulas of Polyatomic Ions Formula Name Formula Acetate Ammonium (not ammonia) C2H3O2-1 NH4+1 Hypochlorite Iodate ClO-1 IO3-1 Arsenate Carbonate Chlorate Chlorite Chromate Cyanide Dichromate Hydrogen Carbonate Hydronium Hydroxide AsO4-3 CO3-2 ClO3-1 ClO2-1 CrO4-2 CN-1 Cr2O7-2 HCO3-1 H3O+1 OH-1 Nitrate Nitrite Perchlorate Peroxide Permanganate Phosphate Sulfate Sulfite Thiocyanate Thiosulfate NO3-1 NO2-1 ClO4-1 O22MnO4-1 PO4-3 SO4-2 SO3-2 SCN-1 S2O3 -2 Names & Formulas of Common Ionic Compounds Ammonia (NH3) 0.771 -33 Carbon Dioxide (CO2) 1.98 -78 Formula Li2CO3 Na2B4O7 NaCl NaI Carbon Monoxide (CO) 1.25 -191 NaHCO3 Sodium hydrogen carbonate (baking soda) Chlorine (Cl2) 3.21 -35 Helium (He) 0.18 -269 Na2CO3 NaClO Sodium carbonate (soda ash) Sodium hypochlorite (chlorine bleach) Hydrogen (H2) 0.089 -253 Hydrogen Chloride (HCl) 1.64 -85 Hydrogen Sulfide (H2S) 1.45 -60.2 KNO3 KCl Potassium nitrate (saltpeter, fertilizer) Potassium chloride (table salt substitute) Methane (CH4) 0.716 -161.6 CaCO3 Calcium carbonate (TUMS, chalk, limestone) Neon (Ne) 0.9002 -246.1 CaO Nitrogen (N2) 1.25 -196 Nitrogen monoxide (NO) 1.34 -152 CaSO4 TiO2 Fe2O3 Oxygen (O2) 1.43 -183 Ag2S Ozone (O3) 2.141 -111.3 Phosgene (CCl2O) 4.248 7.5 Sulfur Dioxide (SO2) 2.92 -10.1 Na2CO3·1.5 H2O2 Al2O3 Name and Synonyms Lithium carbonate Sodium Borate (borax) Sodium chloride (table salt) Sodium iodide (a salt in iodized salt) Sodium percarbonate (oxiclean) Aluminum oxide (corundum, ruby, sapphire) Calcium oxide (lime) Calcium sulfate (gypsum, dry wall) Titanium dioxide or Titanium (IV) oxide (pigment) Iron (III) oxide (one form of iron rust) Silver sulfide (silver tarnish) TABLE OF SELECTED PROPERITES OF SELECTED ELEMENTS Table of Ionic Compounds & Solubility in Water s = soluble (dissolves) i = nearly insoluble ➏ acetate bromide carbonate chloride chromate CH3COO-1 Br-1 CO3-2 Cl-1 s s s s s s s s s s s s s s s s s s s s ss s i s s i s i i i i i i i i i s s s s s s s s ss s i s (possibly a precipitate) ss = slightly soluble (possibly a precipitate) Alkali (Li+1, Na+1, K+1) etc. Aluminum (Al+3) Ammonium (NH4)+1 Barium (Ba+2) Calcium (Ca+2) Copper II (Cu+2) Iron II (Fe+2) Iron III (Fe+3) Lead II (Pb+2) Magnesium (Mg+2) Silver (Ag+1) Zinc (Zn+2) hydroxide iodide nitrate phosphate sulfate CrO4-2 hydrogen carbonate HCO3-1 OH-1 I-1 NO3-1 PO4-3 SO4-2 s i s i s i i i i s ss s s s s s s s s s s s s s s s s s ss i i i i i i i s s s s s i s i ss s i s s s s s s s s s s s s s s i s i i i i i i i i i s s s s ss s s ss ss s ss s Vapor Pressure of Water at Various Temperatures ➐ Temp (C) 0 3 5 8 10 12 14 15 16 18 19 20 21 22 23 24 Pressure (kPa) 0.6 0.8 0.9 1.1 1.2 1.4 1.6 1.7 1.8 2.1 2.2 2.3 2.5 2.6 2.8 3.0 Temp (C) 25 26 27 28 29 30 32 35 37 40 50 60 70 80 90 100 Pressure (kPa) 3.2 3.4 3.6 3.8 4.0 4.2 4.8 5.6 6.3 7.4 12.3 19.9 31.2 47.3 70.1 101.3 ➑ Standard temperature Standard pressure Some Important Constants 0.0 C or 273 Kelvin 1 atmosphere or 101.3 kiloPascals Melting / Freezing point of water Normal Boiling point of water Specific Heat of water Heat of Fusion constant of water Heat of Vaporization constant of water Density of water @ 3.98 C 0.0 C 100 C 4.18 J/g•C 334 J/ 2,226J/g 1.00 g/mL Avogadro’s Number Molar Volume at STP 6.02 x 1023 species 22.4 Liters 8.314 J/molK Universal Gas Constant (R) 0.082057 atmL/molK ➒ st 1 Ionization Energy (kJ/mol) Electronegativity* Table of First Ionization Energies & Electronegativity Values Group 1 Group 2 Group 13 Group 14 Group 15 Group 16 Group 17 H 1312 2.2 Li 520 1.0 Na 496 0.9 K 419 0.8 Rb 403 0.8 Cs 376 0.8 Fr 393 0.7 Group 18 He 2372 - Be 900 1.6 Mg 736 1.3 Ca 590 1.0 Sr 549 1.0 Ba 503 0.9 Ra 509 0.9 B C N O F 801 1086 1402 1314 1681 2.0 2.6 3.0 3.5 4.0 Al Si P S Cl 578 787 1012 1000 1251 1.6 1.9 2.2 2.6 3.2 Ga Ge As Se Br 579 762 944 941 1140 1.8 2.0 2.2 2.6 3.0 In Sn Sb Te I 558 709 831 869 1008 1.8 2.0 2.1 2.1 2.7 Tl Pb Bi Po At 589 716 703 812 926 2.0 2.3 2.0 2.0 2.2 *based upon a scale in which 4.0 is the maximum value Ne 2081 Ar 1521 Kr 1351 Xe 1170 Rn 1037 - Atom Temperature Density Equations Mass # = # of protons + # of neutrons K = C + 273 density = mass volume where K is Kelvin Temperature C is Celsius Temperature in degrees Molar Density(g)STP = 1mol mass 22.4 L Percent Composition % composition by mass = mass of the Part you want x 100 mass of the Whole thing Percent Error % error = | measured value – accepted value | x 100 accepted value Calorimetry q = mc∆T q = mHf q = mHv Hf is the heat of fusion constant in J/g Hv is the heat of vaporization constant in J/g Combined Gas Law P1V1 = P2V2 T1 T2 Ideal Gas Law PV = nRT Molarity (M) Titration (Neutralization) Moles where q is energy in joules m is mass in grams c is specific heat in J/gram•C ∆T is change in temperature in C where P is pressure V is volume T is Kelvin Temperature where P is pressure in atmospheres or kPa V is volume in Liters T is temperature in Kelvin R = 8.314 J/molK when kPa is used 0.082057 atmL/molK when atm is used Molarity = moles of dissolved material Liters of solution (#H1+ ) (Macid)(Vacid) = (Mbase )(Vbase) (#OH1-) moles = grams of substance mole mass of substance where M is molarity and V is volume Acid / Base Indicators & pH Range / Color Color Change In That Range Methyl Orange 3.2-4.4 Red (below 3.2) orange Yellow (above 4.4) Bromothymol 6.0-7.6 Yellow (below 6.0) Blue green Blue (above 7.6) Phenolphthalein 8.2-10 Colorless (below 8.2) (phth) pink Deep Pink (above 10) Litmus 5.5-8.2 Red (below 5.5) purple Blue (above 8.2) Bromcresol Green 3.8-5.4 Yellow (below 3.8) green Blue (above 5.4) Thymol Blue 8.0-9.6 Yellow (below 8.0) green Blue (above 9.6) Indicator pH Scale 9 10 11 12 13 DRANO 8 TUMS 7 Baking soda 6 BASE Egg white 5 Blood 7.3 4 Tap water 3 Black coffee 2 Orange juice 1 Vinegar 0 NEUTRAL Pure water ACID 14 Names & Formulas of Common Arrhenius Acids HBr(aq) Hydrobromic acid HF(aq) Hydrofluoric acid HCl(aq) Hydrochloric acid H2S(aq) Hydrosulfuric acid HNO3(aq) Nitric acid H2SO4(aq) Sulfuric acid H3PO4(aq) Phosphoric acid H2C2O4(aq) Oxalic acid HSO3NH2(aq) Sulfamic acid H2CO3(aq) Carbonic acid HC2H5O2(aq) or Ethanoic acid CH3COOH(aq) (a.k.a. acetic acid) Names & Formulas of Common Arrhenius Bases NH4OH(aq) Ammonium hydroxide (a.k.a. ammonia in water) Ba(OH)2(aq) Barium hydroxide Ca(OH)2(aq) Calcium hydroxide Mg(OH)2(aq) Magnesium hydroxide KOH(aq) Potassium hydroxide NaOH(aq) Sodium hydroxide Other names/types of acids Amino acids (e.g. leucine, valine, serine...) Ascorbic acid Citric acid Other names/types of bases Amines (e.g. CH3NH2) Carbonates (e.g. CaCO3, Na2CO3) Hydrogen Carbonates (NaHCO3) Various Standard & Qualitative Tests A POSITIVE TEST … Test for: Test oxygen gas O2(g) Flaming splint causes the flame to flare up and to burn more brightly than before oxygen gas O2(g) carbon dioxide gas CO2(g) Glowing splint causes the glowing ember to re-light and to burn Bubble gas into Ca(OH)2(aq) produces a white precipitate (solid). Addition of more carbon dioxide reverses the reaction hydrogen gas H2(g) Flaming splint in the presence of atmospheric oxygen, the hydrogen gas ignites, causing a popping sound (like uncorking a champagne bottle) metal (active) React with acid creates bubbles filled with hydrogen gas. Often the un-reacted metal will darken in color. water H2O (l) Blue Cobalt Chloride Paper acid Various indicators causes a color change in selected indicators (see Table 11) base (hydroxide containing) Various indicators causes a color change in selected indicators (see Table 11) carbonate React with an acid creates fizzing due to bubbles of carbon dioxide gas monosaccharides (reducing sugar) Tollen’s test using AgNO3(aq) + KOH(aq) causes the precipitation/deposition of silver metal on glass monosaccharides (reducing sugar) Benedict’s Solution Causes the color of the Benedict’s solution to change from blue to yellow or red polysaccharides (starch) React with a solution of iodine protein Biuret Test turns a chemically treated blue paper a pinkish color causes the color to change from red to blue/black causes a color change from blue to violet or pink for small polypeptides Reaction Type Example Comment(s) Acid Base Neutralization HNO3(aq) + KOH(aq) H2O(l) + KCl(aq) + energy kJ an acid a base water a salt Titration Saponification C51H88O6(s) + 3 NaOH(aq) 3 CH3(CH2)14CO2Na(s) + C3H8O3 a fat a base a soap glycerol (-ine) Making soap Complete Combustion (of an organic compound) CH4(g) + an organic compound Esterification CH3COOH(aq) + CH3CH2OH(l) CH3COOCH2CH3(aq) + H2O(l) an organic acid an alcohol an ester water Nonmetal Oxide in Water O2(g ) oxygen CO2(g) + H2O(l) + energy kJ carbon water dioxide CO2(g) + H2O(l) H2CO3(aq) carbon water carbonic acid dioxide Metal Oxide in Water Na2O(s) + H2O(l) 2 NaOH sodium oxide water sodium hydroxide Active Metal in Acid 2 Li(s) + 2 H2O(l) 2 LiOH(aq) + H2(g) a metal water a base hydrogen gas Carbonate in Acid CaCO3(s) + 2 HCl(aq) CaCl2(aq) + CO2(g) + H2O(l) a carbonate an acid a salt carbon water dioxide Burning associated with flavorings A nonmetal oxide in water produces an acidic solution associated with acid precipitation and soda water A metal oxide in water produces a basic solution A form of neutralization; The old Volcano Reaction; associated with the acidification of lakes Measurement ➊➏ Common units used in Chemistry Unit Abbreviation Length Mass Volume meter gram Liter Pressure Pascal or Atmosphere m g L or 3 dm (cubic decimeter*) Pa or atm *In 1964, the 12th General Conference on Weights and Measures voted on the equivalence and use of 1 L = 1 dm3 http://www.nist.gov/pml/wmd/pubs/upload/appc-13-hb44-final.pdf Prefix Prefixes and interpretations for commonly used units Meaning Example, using meter Alternate Example, using meter milli- one-thousandth 1 millimeter = 1 meter 1,000 1 mL = 0.001 meter cent- one-hundredth 1centimeter = 1 meter 100 1 cm = 0.01 meter deci- one-tenth 1 decimeter = 1 Meter 10 1 dm = 0.1 meter deka- ten 1 dekameter = 10 meters 1 dam = 10 meters hecto- one hundred 1 hectometer = 100 meters 1 hm = 100 meters one thousand 1 kilometer = 1,000 meters 1 kL = 1,000 meters kilo- http://physics.nist.gov/Pubs/SP811/sec06.html and http://www.nist.gov/pml/wmd/pubs/upload/appc-13-hb44-final.pdf ❶➐ Organic Prefixes # of carbons Prefix 1 2 3 4 5 6 7 8 9 10 12 16 ➊➑ The Hydrocarbons Family General Formula Formula Name alkane CnH2n+2 C4H10 butane alkene CnH2n C4H8 1-butene alkyne CnH2n-2 C4H6 1-butyne 18 20 meth eth prop pron: prōp but (pron like beaut-y) pent hex hept oct non dec dodec (laur-yl) Hexadec (cet-yl or myrist-ic) octadec (stear-yl) eicos (arachid-ic) Examples Structure Other Views H H H H | | | | H—C—C—C—C—H | | | | H H H H H H | | H—C—C—C C—H | | | | H H H H H H | | H—C—C—C C—H | | H H CH3CH2CCH arene (aromatic hydrocarbon) CnH2n-6 C6H6 benzene note: the term aromatic refers to a closed ring with C or N with alternating double bonds where "n" equals the number of carbons in the longest (parent) chain ❶➒ Organic Compounds with Functional Groups Class Description a Examples of molecular or condensed formula a Alcohol R-OH (Monohydroxy) 1 (O-H) group bonded to a carbon. Soluble in water (polar molecule) a C3H7OH b C4H9OH Alcohol (Glycol or Dihydroxy) Aldehyde Ester 2 O-H groups (or OH groups) bonded to carbon. Water soluble (polar molecule) a product of an alcohol & carboxylic acid reaction. Ketone C3H6(OH)2 a HCOH b CH3OOCCH3 a CH3OOCCH3 b C2H5OOCC2H5 O || R— C—R' a carbonyl group on an "interior" or nonterminal carbon Carboxylic Acid (the most common form of organic acid) Amine (simple) O || R—C—O-H a carboxyl group (COOH) bonded to a carbon R-Group. RNH | H a derivative of NH3 At least one H is replaced with an organic group. A weak base (B-L) a C3H6O b C6H12O CH3COOH b C2H5COOH a b (also called a halocarbon) R-X a 2-propanone (acetone) Halogen(s) {X} are substituted onto a hydrocarbon, by removing hydrogen(s) b C3H6F2 H H H H | | | | H—C—C—C—C—H | | | | H OH H H 1,2-propanediol (propylene glycol) H H H | | | H—C—C—C—H | | | H O-H O-H b ethanal (acetaldehyde) H O | || H—C—C—H | H b ethyl propanoate H H O H H | | || | | H—C— C—O—C—C—C—H | | | | H H H H b 3-hexanone H H H O H H | | | || | | H—C—C—C—C—C—C—H | | | | | H H H H H H O H | || | H—C—C—C—H | | H H ethanoic acid (acetic acid) b propanoic acid H H O | | || H—C—C—C—O—H | | H H b phenylamine (aniline) H O | || H—C—C—O—H | H a 1-propanamine (1-propylamine) H H H | | | HCCCNH | | | | H H H H C6H5NH2 C3H7Br methanal (formaldehyde) methyl ethanoate H O H | || | H—C—O—C—C—H | | H H C3H7NH2 a b a a Halide 1,2-ethanediol (ethylene glycol) 1-bromopropane Br H H | | | H—C—C—C—H | | | H H H Example Name / Structure 2-butanol O || H—C—H a a b H H | | H—C—C—H | | OH OH a O || R—C—H A carbonyl group on a terminal C with carbon or hydrogen as the "R" group O || R—O—C—R' C2H4(OH)2 b 1-propanol H H H | | | H—C—C—C—O-H | | | H H H a a b Example Name / Structure NH | H b 1,2-difluoropropane H H F | | | H—C—C—C—H | | | H F H