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Chemistry 100(02) Fall 2011

Chemistry 100(02) Fall 2011. Instructor: Dr. Upali Siriwardane e-mail : upali@chem.latech.edu Office : CTH 311 Phone 257-4941 Office Hours : M,W, 8:00-9:00 & 11:00-12:00 a.m Tu,Th,F 9:00 - 10:00 a.m.   Test Dates : March 25, April 26, and May 18; Comprehensive Fina

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Chemistry 100(02) Fall 2011

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  1. Chemistry 100(02) Fall 2011 Instructor: Dr. UpaliSiriwardane e-mail: upali@chem.latech.edu Office: CTH 311 Phone 257-4941 Office Hours: M,W, 8:00-9:00 & 11:00-12:00 a.mTu,Th,F 9:00 - 10:00 a.m.   Test Dates: March 25, April 26, and May 18; Comprehensive Fina Exam: 9:30-10:45 am, CTH 328. October 3, 2011 (Test 1): Chapter 1 & 2 October 26, 2011 (Test 3): Chapter 3 & 4 November 16, 2011 (Chapter 5 & 6) November 17, 2011 (Make-up test) comprehensive: Chapters 1-6 9:30-10:45:15 AM, CTH 328

  2. Chapter 3. Chemical Compounds 3.1 Molecular Compounds Page 76 3.2 Naming Binary Inorganic Compounds Page 79 3.3 Hydrocarbons 80 3.4 Alkane and Their Isomers Page 83 3.5 Ions and Ionic Compounds Page 85 3.6 Naming Ions and Ionic Compounds Page 91 3.7 Properties of Ionic Compounds Page 94 3.8 Moles of Compounds Page 98 3.9 Percent Composition Page 103 3.10 Determining Empirical and Molecular Formulas Page 104 3.11 The Biological Periodic Table Page 107

  3. Chapter 3. KEY CONCEPTSChemical Compounds

  4. What is a Compounds? • They are made up of a collection of two or more different atoms and ions. CO2 - carbon dioxide SO2, - sulfur dioxide C3H8 - propane FeCl3, iron (III) chloride SnCl2 tin (II) chliride

  5. Types of Compounds A) Molecular or Covalent Compounds: non-metal + non-metal nonmetal oxide or halides: SO2 Organic compounds: C3H8 B) Ionic compounds: Metal + non-metal: a) Type I ionic compound (fixed charge) NaCl b) Type II ionic compound FeCl2 and FeCl3, SnCl2 and SnCl4

  6. Formula of a Compound • Formula are used to represent elements and compound. • For molecular compounds, formula tell how many of each kind of atom are in a molecule. • For ionic compounds, formula tell the simples ratio of actions and anions. Molecular Weight ? Molecular compounds and Formula Weight? Ionic compounds

  7. Molecular Shows ratio of atoms each element in the compound. E.g ethyl alcohol: C2H6O Condensed Shows groups of atoms bonded together in the formula. E.g ethyl alcohol: CH3CH2OH Structural Shows bonding of important groups in the formula E.g ethyl alcohol: Types of Chemical Formula

  8. Ball and Stick Models of Molecular Compounds

  9. Models of Ethanol

  10. For compounds composed of two non-metallic elements, the more metallic element is listed first. To designate the multiplicity of an element, Greek prefixes are used: mono  1; di  2; tri  3; tetra  4; penta  5; hexa  6; hepta  7; octa  8 Naming Binary Molecular-Covalent Compounds

  11. H2O water (common name) NH3 ammonia (common name) N2O dinitrogen oxide (nitrous oxide) NO nitrogen monoxide (nitric oxide) NO2 nitrogen dioxide N2O4dinitrogentetroxide CO carbon monoxide CS2 carbon disulfide SO3 sulfur trioxide CCl4 carbon tetrachloride PCl5 phosphorus pentachloride SF6 sulfur hexafluoride Simple Binary Molecular Compounds

  12. Hydrocarbons Catenation • The formation of chains of atoms of the same element. • This key feature of carbon permits a vast number of compounds to exist. • Four types of hydrocarbons 1) Alkanes (saturated): single C-C bonds 2) Alkenes (unsaturated): double C=C bond 3) Alkynes (unsaturated): triple bond 4) Aromatic (unsaturated): benzene rings

  13. Classifying Organic Compounds Examples Functional Group Ending Hydrocarbons C and H only -ane Alcohols R-OH -ol Acids R-COOH -oic acid Amines R-NH2 -amine Ketones R(C=O)R’ -one Aldehydes R-CHO -al

  14. alkanes– CnH2n+2 E.g. C5H12 pentane alkenes –CnH2nE.g. C2H4 ethene alkynes –CnH2n-2E.g. C2H2 ethyne alcohols –ROHE.g C2H5OH ethanol where R refers to the hydrocarbon radical backbone created by substituting an -OH functional group for a H atom in the hydrocarbon Hydrocarbons and Alcohols

  15. methane – CH4 ethane – C2H6 propane – C3H8 butane – C4H10 pentane – C5H12 hexane – C6H14 heptane – C7H16 octane – C8H18 nonane – C9H20 decane – C10H22 Alkanes – CnH2n+2

  16. I see much memorization in your future! Base names of hydrocarbons Prefix Carbons • Meth- 1 • Eth- 2 • Prop- 3 • But- 4 • Pent- 5 • Hex- 6 • Hept- 7 • Oct- 8 • Non- 9 • Dec- 10

  17. Butane molecules are present in the liquid and gaseous states in the lighter Butane

  18. As the chain length of Alkane/Alcohols increases so is the boiling point

  19. Straight & Branch-Chain Alkanes

  20. Some Common Alkyl Groups

  21. What is an Isomer? • Compounds with the same number and type of atoms but with different arrangements. • Molecular Formula C5H12 • Condensed formulas. • CH3CH2CH2CH2CH3pentane • CH3CH(CH3)CH2CH3 2-methylbutane • (CH3)4C 2,2-dimethylpropane • All are isomers of C5H12.

  22. AlkaneIsomers is there a formula?

  23. Select the longest chain alkane as the base name Determine the side chains and give them a number corresponding to the carbon number on the base chain Use Greek prefixes of mono-(1), bi-(2), tri(3), etc. for multiplicity of same side chain Naming Branch-Chain Alkanes

  24. Naming Branch-Chain Alkanes

  25. Alcohol example CH3CH2CH2CH2OH C - C - C - C - O - H • Base contains 4 carbon • - Parent alkane name is butane • remove -e and add -ol • alcohol name - butanol • OH is on the first carbon so - • 1-butanol

  26. Characteristics of compounds with ionic bonding: Compound ofmetal and non-metal Composed of ions: cation and anion non-volatile, thus high melting points solids do not conduct electricity, but melts (liquid state) do many, but not all, are water soluble Ionic Compounds

  27. Ions Ions are charged particles formed by the transfer of electrons between elements or combinations of elements. Cation - a positively charged ion. Ca Ca2+ + 2e- Anion - a negatively charged ion. F2 + 2e- 2F-

  28. Formation of Ionic Compound, NaCl

  29. Outermost electrons (valance electrons) in an atom lost or gained metals form positive monatomic ions non-metals form negative monatomic ions Ionic compounds have electrical neutrality Valance Electrons & Charge on Ions

  30. Monatomic Ions (Type I) Group IA  +1 Group A # Group IIA  +2 Group A # Non-metals Group IIB  -1 (8 - Group B #) Monatomic Ions (Type II) Transition metal ionic compounds: have ions with different charges E.g. Iron :Fe2+ and Fe3+ Valence or of Metal Ions

  31. Charges on Some Common Monatomic Cations and Anions

  32. Polyatomic Ions • more than one atom joined together • have negative charge except for NH4+ and its relatives • negative charges range from -1 to -4 Table in the Book

  33. Ammonium NH4+ perchlorate ClO41- cyanide CN1- hydroxide OH1- nitrate NO31- sulfate SO42- carbonate CO32- phosphate PO43- Polyatomic Ions

  34. Names of Ionic Compounds 1. Name the metal first. If the metal has more than one oxidation state, the oxidation state is specified by Roman numerals in parentheses. 2. Then name the non-metal, changing the ending of the non-metal to -ide.

  35. Metals with multiple charges Transition metals. Here it is easier to list the ones that to only have a single common oxidation state. All Group 3B - 3+ Ni, Zn, Cd - 2+ Ag - 1+ Lanthanides and actinides - 3+ (common)

  36. Ionic compounds Some simple ions Cations Al3+ Na+ Mg2+ Cl- Anions O2- N3- Exchange charge as subscripts on the metal and nonmetal Formula for some ionic compounds NaCl MgCl2 AlCl3 Na2O MgO Al2O3 Na3N Mg3N2AlN Give the simple ratio

  37. NaCl Fe2O3 NH4NO3 KClO4 CaCO3 NaOH AgNO3 Mg(C2H3O2)2 Co2(SO4)3 KI Mg3N2 NaCl sodium chloride Fe2O3 iron(III) oxide NH4NO3 ammonium nitrate KClO4 potassium perchlorate CaCO3 calcium carbonate NaOH sodium hydroxide AgNO3 silver nitrate Mg(C2H3O2)2 magnesium acetate Co2(SO4)3 cobalt(III) sulfate KI potassium iodide Mg3N2 magnesium nitride Nomenclature

  38. Ionic Crystal Lattice NaCl “table salt”

  39. Cleaving NaCl

  40. Electrical Conductivity ofIonic Solution Electrolytes Aqueous solutions conducts electricity strong-electrolytes weak-electrolytes Non-electrolytes Aqueous solutions do not conducts electricity

  41. Naming Acids formula starts with H HCl HNO3 H2SO4 HClO3 H3BO3 H3PO4 Hydrochloric acid Nitric acid Sulfuric acid Chloric acid Boric acid Phosphoric acid

  42. Names of acids and ions • HClOhypochlorousClO¯ ”hypochlorite • HClO2chlorous ClO2¯ chlorite • HClO3chloric ClO3¯ chlorate • HClO4perchloric ClO4¯ perchlorate • HNO3 nitric NO3 ¯ nitrate • HNO2 nitrous NO2 ¯ nitrite

  43. Naming bases • formula ends with OH • NaOH sodium hydroxide • Ba(OH)2 barium hydroxide • KOH potassium hydroxide • NH4OH ammonium hydroxide • Ca (OH)2 calcium hydroxide

  44. Percentage Composition description of a compound based on the percent relative amounts of each element in the compound

  45. % Element Composition in Compounds from Formula n x Gram Atomic weight % mass = --------------------------------------- x 100 formula weight (GMW, GFW) n = subscript of the element in the formula

  46. Example: What is the percent composition of carbon in chloroform, CHCl3, a substance once used as an anesthetic? MM = 1(gaw)C + 1(gaw)H + 3(gaw)Cl = (12.011 + 1.00797 + 3  35.453)amu = 119.377amu 1(12.011) %C =  100 = 10.061% C 119.377 1(1.00797) %H =  100 = 0.844359% H 119.377 3(35.453) %Cl =  100 = 89.095% Cl 119.377

  47. Example: What is the percent composition of chloroform, CHCl3, a substance once used as an anesthetic? %C = 10.061% C %H = 0.844% H %Cl = 89.095%Cl 100.00

  48. Mass percent of element in C6H12O6 Molar Mass = 180.16 g/mol 6 x 12 %C = --------- x 100 = 40.00% C 180.16 12 x 1.01 % H = ------------- x 100 = 6.73% H 180.16 6 x 16.00 %O = ------------ x 100 = 53.29% O 180.16 ----------- • 100.02%

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