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Chemistry 100(02) Fall 2012

Chemistry 100(02) Fall 2012 . Instructor: Dr. Upali Siriwardane e-mail : upali@coes.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 : October 1, 2012 (Test 1): Chapter 1 & 2

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Chemistry 100(02) Fall 2012

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  1. Chemistry 100(02) Fall 2012 Instructor: Dr. Upali Siriwardane e-mail: upali@coes.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: October 1,2012 (Test 1): Chapter 1 & 2 October 22, 2012 (Test 2): Chapter 3 & 4 November 14, 2012 (Test 3) Chapter 5 & 6 November 15, 2012 (Make-up test) comprehensive: Chapters 1-6 9:30-10:45:15 AM, CTH 328 CHEM 100, Fall 2012 LA TECH 2-1

  2. REQUIRED : Textbook: Principles of Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro - Pearson Prentice Hall and also purchase the Mastering Chemistry Group Homework, Slides and Exam review guides and sample exam questions are available online: http://moodle.latech.edu/ and follow the course information links. OPTIONAL : Study Guide: Chemistry: A Molecular Approach, 2nd Edition- Nivaldo J. Tro 2nd Edition Student Solutions Manual: Chemistry: A Molecular Approach, 2nd Edition-Nivaldo J. Tro 2nd Text Book & Resources CHEM 100, Fall 2012 LA TECH 2-2

  3. Chapter 3. Molecules, Compounds, and Chemical Equations 3.1 Hydrogen, Oxygen, and Water 78 3.2 Chemical Bonds 80 3.3 Representing Compounds: Chemical Formulas and Molecular Models.. 82 3.4 An Atomic-Level View of Elements and Compounds 84 3.5 Ionic Compounds: Formulas and Names 87 3.6 Molecular Compounds: Formulas and Names 93 3.7 Formula Mass and the Mole Concept for Compounds 97 3.8 Composition of Compounds 100 3.9 Determining a Chemical Formula from Experimental Data 105 3.10 Writing and Balancing Chemical Equations 110 3.11 Organic Compounds 114 CHEM 100, Fall 2012 LA TECH 2-3

  4. Chapter 3. KEY CONCEPTS • Writing Molecular and Empirical Formulas (3.3) • Classifying Substances as Atomic Elements, Molecular Elements, Molecular Compounds, or Ionic Compounds (3.4) • Writing Formulas for Ionic Compounds (3.5) • Naming Simple Ionic Compounds (3.5) • Naming Ionic Compounds Containing Polyatomic Ions (3.5) • Naming Molecular Compounds (3.6) • Naming Molecular Compounds (3.6) • Naming Acids (3.6) • Calculating Formula Mass (3.7) • Using Formula Mass to Count Molecules by Weighing (3.7) • Calculating Mass Percent Composition (3.8) • Using Mass Percent Composition • as a Conversion Factor (3.8) • Using Chemical Formulas as • Conversion Factors (3.8) • Obtaining an Empirical Formula • from Experimental Data (3.9) • Calculating a Molecular Formula • from an Empirical Formula and • Molar Mass (3.9) • Obtaining an Empirical Formula • from Combustion Analysis (3.9) • Balancing Chemical Equations • (3.10) CHEM 100, Fall 2012 LA TECH 2-4

  5. Intramol ecular Chemical Bonding Types onic:Complete transfer of 1 or more electrons from one atom to another, usually between a metal and a nonmetal element Covalent: The sharing of val ence electrons shared between nonmetal elements Metallic:The communal sharing of electrons between metals *Note: Most molecular bonds are actually somewhere in between covalent and ionic types. CHEM 100, Fall 2012 LA TECH 2-5

  6. -•••■0411414.■•.- prefix name of prefix 1st element lbase name of 2nd element + -ide Example: P20, diphosphorus pentoxide Metal forms more than one type of ion name of cation (metal) base name of anion (nonmetal) + -ide Example: Cali calcium iodide 1- Oxyacids Contain oxygen base name of oxyanion + -ic —,04/ Example: H1PO4phosphoric acid Binary acids Two-element Example: FeCI Example• 1-1C1(aq) Example: H2SW•aq) iron(in) chloride hydrochloric acid sulfurous acid *Acids must be in aqueous solution. CHEM 100, Fall 2012 LA TECH 2-6

  7. Types of Compounds ar or Covalent Compounds: B) Mo lecul non-metal + non-metal nonmetal oxide or halides: SO2 Organic compounds: C3H8 CHEM 100, Fall 2012 LA TECH 2-7

  8. MOLECULAR ACIDS* NonmetalH and one or 414_ only more nonmetals base name of oxyanion + -k Example, II 3 PO4 phospliovi( acid (xiimplc:1);,05 diphosphorus pentoxide CHEM 100, Fall 2012 LA TECH Example'. HiS03(aq) sulfurous acid *Acids mug be in aqueous base Dame of nonmetal -ic Example; HCI(ao) hydrochloric acid 2-8

  9. CHEMICAL BONDS: THE FORCE BETWEEN ATOMS What Makes a Molecule? Methane, CH4 2613 Pearson Educalwrt Inc CHEM 100, Fall 2012 LA TECH 2-9

  10. Molecular Compounds: Nonmetal Name the most “metallic” of the nonmetals first. + Nonmetal Change the ending of the nonmetal to “IDE.” • Indicate the number of atoms of the nonmetal by Latin prefixes. • Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca • Examples: • – P2O5: diphosphorous pentaoxide • – CO: carbon monoxide CHEM 100, Fall 2012 LA TECH 2-10

  11. For compounds composed of two non-metallic e ements, the more metallic element is listed first. To designate the multiplicity of an el ement, Greek prefixes are used: mono  1; di  2; tri  3; tetra  4; penta  5; hexa  6; hepta  7; octa  8 Naming Binary Molecu lar-Coval ent Compounds CHEM 100, Fall 2012 LA TECH 2-11

  12. 1) H2O, Na3PO4, HCl, C2H6, NH3, KCl, CH4, NH4Cl, C6H12O6, Brass- CuxZny, SO3, NaCl, CO2 Identify the types of compounds in the above list: Molecular compound: Ionic compound: Alloy: Organic: Inorganic: CHEM 100, Fall 2012 LA TECH 2-12

  13. H2O, Na3PO4, HCl, C2H6, NH3, KCl, CH4, NH4Cl, C6H12O6, Brass- CuxZny, SO3, NaCl, CO2 2) Which of the above compounds have Molecular formula: Ionic formula: Distinct empirical formula: CHEM 100, Fall 2012 LA TECH 2-13

  14. 3) Indicating the type and number of atoms in a molecule of the covalent compound: C6H12O6. C: H: O: Molecular formula: Empirical formula: CHEM 100, Fall 2012 LA TECH 2-14

  15. Simple Binary M olecul ar Compounds H2O water (common name) NH3ammonia (common name) N2O dinitrogen oxide (nitrous oxide) NO nitrogen monoxide (nitric oxide) NO2 nitrogen dioxide N2O4 dinitrogen tetroxide CO carbon monoxide CS2 carbon disulfide SO3 sulfur trioxide CCl4 carbon tetrachloride PCl5 phosphorus pentachlorid e 2-15 SF6 sulfur hexafluoride CHEM 100, Fall 2012 LA TECH

  16. 4) Give systematic names to following binary inorganic molecular compounds a) H2O: b) HCl: c) SF6: d) BF3: e) N2O4: f) CCl4: g) SO3: h) PCl3: CHEM 100, Fall 2012 LA TECH 2-16

  17. alkanes – CnH2n+2E.g. C5H12 pentane alkenes – CnH2nE.g. C2H4 ethene alkynes – CnH2n-2E.g. C2H2 ethyne alco hols – ROH E.g C2H5OH ethanol Hyd rocarbons and Alco hols where R refers to the hydrocarbon radical backbone created by substituting an -OH functional group for a H atom in the hydrocarbon 2-17 CHEM 100, Fall 2012 LA TECH

  18. 5) Give the common name of the following molecular compounds NH3: CH3COOH: C6H12O6: C2H5OH: CHEM 100, Fall 2012 LA TECH 2-18

  19. Acids • Types of acids • Binary acids • H+ and nonmetal anion In aqueous solutions, acids contain the H+ cation and • Oxyacids • H+ cation and polyatomic anion anion. 2-19 CHEM 100, Fall 2012 LA TECH

  20. Naming Acid s Formula starts with H HClHyd rochl oric acid HNO3Nitric acid H2SO4Sulfuric acid HClO3Chloric acid 2-20 H3BO3Boric acid H3PO4Phosphoric acid CHEM 100, Fall 2012 LA TECH

  21. Names of acid s and ions HClO2 chlorous ClO2¯ chl HClO3 chloric ClO3¯ chl HClO4 perchloric ClO4¯ perchl HNO3 nitric NO3 ¯ nitrate CHEM 100, Fall 2012 LA TECH HClO hypochlorous HNO2 nitrous NO2 ¯ nitrite ClO ¯ ”hypochlorite orate orite orate 2-21

  22. formula ends with OH Naming bases NaOH Ba(OH)2 barium hydroxid KOH sodium hydroxid potassium hydroxid e e e 2-22 Ca(OH)2 calcium hyd NH4OH roxide ammonium hydroxid e CHEM 100, Fall 2012 LA TECH

  23. 6) Give the names of the following acids CHEM 100, Fall 2012 LA TECH 2-23

  24. Types of Chemical Formula Molecular Shows ratio of atoms each element in the : C2H6O Condensed Shows groups of atoms bonded together in the formula. E.g ethyl alcohol: CH 3CH2OH Structural Shows bonding of important groups in the formu E.g ethyl a cohol : a 2-24 compound. E.g ethyl alcohol CHEM 100, Fall 2012 LA TECH

  25. 2-25 Models of Ethanol CHEM 100, Fall 2012 LA TECH

  26. 7) Given the structural formula of an organic compound, write the for the following: CH3CHClCH2OH molecular formula condensed formula structural formula line formula CHEM 100, Fall 2012 LA TECH 2-26

  27. 2-27 Catenation The formation of chains of atoms of the same This key feature of carbon permits a vast number of compounds to exist. Four types of hydrocarbons Alkanes (saturated): single C-C bonds Alkenes (unsaturated): double C=C bond Alkynes (unsaturated): triple bond Aromatic (unsaturated): benzene rings Hyd e ement. rocarbons CHEM 100, Fall 2012 LA TECH

  28. Alkanes CnH2n+2 methane – CH4 ethane – C2H6 propane – C3H8 butane – C4H10 pentane – C5H12 hexane – C6H14 heptane – C7H16 octane – C8H18 nonane – C9H20 decane – C10H22 CHEM 100, Fall 2012 LA TECH 2-28

  29. Base names of hydrocarbons Prefix Carbons Meth- 1 Eth- 2 Prop- 3 But- 4 Pent- 5 Hex- 6 Hept- 7 Oct- 8 - 9 Dec- 10 2-29 I see much memorization in your future! Non CHEM 100, Fall 2012 LA TECH

  30. 8) Name, molecular, condensed and line formula of straight chain alkane (saturated hydrocarbons) or n-alkanes. 4 carbon n-alkane: 7 carbon n-alkane: CHEM 100, Fall 2012 LA TECH 2-30

  31. What is an Isomer? Compounds with the same number and type of atoms but with different arrangements are called constitutional isomers Condensed formul Mol ecul ar FormulaC5H12 as. CH3CH2CH2CH2CH3 pentane CH3CH(CH3)CH2CH3 2-methylbutane (CH3)4C 2,2-dimethylpropane All are isomers of C5H12. CHEM 100, Fall 2012 LA TECH 2-31

  32. Alkane Isomers is there a formula? Molecular Number of Molecular Number of Formula Isomers Formula Isomers CH4 1 C2H6 C3H81 C4Hio 2 C51-112 3 C61-114 5 C71-116 9 C81-11 18 C9H20 C101122 Cl2H26 C 151132 C 201142 C 30H62 C40H82 35 75 355 4,347 366,319 4,111,846,763 62,491,178,805,831 CHEM 100, Fall 2012 LA TECH 2-32

  33. 9) Draw the structural formula of constitutional isomers of butane with molecular formula C4H10. n-butane: CH3CH2CH2CH3 isobutene: (CH3) 3CH CHEM 100, Fall 2012 LA TECH 2-33

  34. 2-34 Butane Butane molecules are present in the liquid and gaseous states in the lighter CHEM 100, Fall 2012 LA TECH

  35. Determine empirical formulas for the following: 1. An ionic compound that has two aluminum ions for every three oxide ions Hexane, C6H14 Arabinose, C5H10O5 Hydrogen peroxide, Al2O3 (C3H7)n where n = 2 (CH2O)n where n = 2 (HO)n where n = 2 CHEM 100, Fall 2012 LA TECH 2-35

  36. Classifying Organic Compound s Examples Functional Group Ending Hydrocarbons C and H only -ane Alcohols R-OH -ol Acids R-COOH Amines R-NH2-amine KetonesR(C=O)R’-one Aldehydes R-CHO-al -oic acid CHEM 100, Fall 2012 LA TECH 2-36

  37. 10) Classification and the name of the following

  38. The Many Representations of a Molecule TABLE 3.1 Benzene, Acetylene, Glucose, and Ammonia Name of Empirical Molecular Structural Compound Formula Formula Formula Ball-and-Stick Model Space-Filling Model

  39. 11) Identify the classification or name of the following biologically important molecules CHEM 100, Fall 2012 LA TECH 2-39

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