1. 3-1 CHEM 100, Fall 2014 LA TECH Instructor: Dr. Upali Siriwardane e-mail: upali@latech.edu Office: CTH 311 Phone 257-4941 Office Hours: M,W, 8:00-9:30 & 11:30-12:30 a.m Tu,Th,F 8:00 - 10:00 a.m. Or by appointment Test Dates : Chemistry 100(02) Fall 2014 September 29, 2014 (Test 1): Chapter 1 & 2 October 20, 2014 (Test 2): Chapter 3 & 4 November 12, 2014 (Test 3) Chapter 5 & 6 November 13, 2014 (Make-up test) comprehensive: Chapters 1-6 9:30-10:45:15 AM, CTH 328

2. 3-2 CHEM 100, Fall 2014 LA TECH 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. http://moodle.latech.edu/ 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

3. 3-3 CHEM 100, Fall 2014 LA TECH 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 Chapter 3. Molecules, Compounds, and Chemical Equations

4. 3-4 CHEM 100, Fall 2014 LA TECH 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 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)

5. 3-5 CHEM 100, Fall 2014 LA TECH

6. 3-6 CHEM 100, Fall 2014 LA TECH Structural formula Space-filling model Methane, CH 4 CHEMICAL BONDS: THE FORCE BETWEEN ATOMS What Makes a Molecule?

7. 3-7 CHEM 100, Fall 2014 LA TECH 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: – P 2 O 5 : diphosphorous pentaoxide – CO: carbon monoxide 2-10 Molecular Compounds:

8. 3-8 CHEM 100, Fall 2014 LA TECH For compounds composed of two non-metallic elements the more metallic element is listed 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

9. 3-9 CHEM 100, Fall 2014 LA TECH 1) H 2 O, Na 3 PO 4, HCl, C 2 H 6, NH 3, KCl, CH 4, NH 4 Cl, C 6 H 12 O 6, Brass- Cu x Zn y, SO 3, NaCl, CO 2 Identify the types of compounds in the above list: Molecular compound: Ionic compound: Alloy:Organic:Inorganic:

10. 3-10 CHEM 100, Fall 2014 LA TECH H 2 O, Na 3 PO 4, HCl, C 2 H 6, NH 3, KCl, CH 4, NH 4 Cl, C 6 H 12 O 6, Brass- Cu x Zn y, SO 3, NaCl, CO 2 2) Which of the above compounds have Molecular formula: Ionic formula: Distinct empirical formula:

11. 3-11 CHEM 100, Fall 2014 LA TECH 3) Indicating the type and number of atoms in a molecule of the covalent compound: C 6 H 12 O 6. a. C: b. H: c. O: d. Molecular formula: e. Empirical formula: CHEM 100, Fall 2012 LA TECH 2-14

12. 3-12 CHEM 100, Fall 2014 LA TECH H 2 O water (common name) NH 3 ammonia (common name ) N 2 O dinitrogen oxide (nitrous oxide) NO nitrogen monoxide (nitric oxide) NO 2 nitrogen dioxide N 2 O 4 dinitrogen tetroxide CO carbon monoxide CS 2 carbon disulfide SO 3 sulfur trioxide CCl 4 carbon tetrachloride PCl 5 phosphorus pentachloride SF 6 sulfur hexafluoride Simple Binary Molecular Compounds

13. 3-13 CHEM 100, Fall 2014 LA TECH 4) Give systematic names to following binary inorganic molecular compounds a) H 2 O: b) HCl: c) SF 6 : d) BF 3 : e) N 2 O 4 : f) CCl 4 : g) SO 3 : h) PCl 3 :

14. 3-14 CHEM 100, Fall 2014 LA TECH 5) Give the common name of the following molecular compounds a. NH 3 : b. CH 3 COOH: c. C 6 H 12 O 6 : d. C 2 H 5 OH:

15. 3-15 CHEM 100, Fall 2014 LA TECH 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 ACIDS

16. 3-16 CHEM 100, Fall 2014 LA TECH Formula starts with acidic H HCl Hydochloric acid HNO 3 Nitric acid H 2 SO 4 Sulfuric acid HClO 3 Chloric acid H 3 BO 3 Boric acid H 3 PO 4 Phosphoric acid Naming Acids

17. 3-17 CHEM 100, Fall 2014 LA TECH HClO 2 chlorous ClO 2 ¯ “ chlortie ” HClO 3 chloric ClO 3 ¯ chlorate HClO 4 perchloric ClO 4 ¯ perchlorate HNO 3 nitric NO 3 ¯ nitrate HClO hypochlorous ClO ¯ ”hypochlorite” HNO 2 nitrous NO 2 ¯ nitrite Names of acids and ions

18. 3-18 CHEM 100, Fall 2014 LA TECH formula ends with OH Ba(OH) 2 barium hydroxide NaOH sodium hydroxide KOH potassium hydroxide Ca(OH) 2 calcium hydroxide NH 4 OH ammonium hydroxide Naming bases

19. 3-19 CHEM 100, Fall 2014 LA TECH 6) Give the names of the following acids FormulaNameIon (s)FormulaNameIons(s) a) HNO 3 : b) H 3 PO 4 : c) HNO 2 : d) H 3 PO 3 : e) H 2 SO 4 : f) H 2 CO 3 : g) H 2 SO 3 : h) CH 3 COOH:

20. 3-20 CHEM 100, Fall 2014 LA TECH Hydrocarbons alkanes – C n H 2n+2 E.g. C 5 H 12 pentane alkenes – C n H 2n E.g. C 2 H 4 ethene alkynes – C n H 2n-2 E.g. C 2 H 2 ethyne Alcohols ROH E.g C 2 H 5 OH ethanol Hyd rocarbons and Alcohols where R refers to the hydrocarbon radical backbone created by substituting an -OH functional group for a H atom in the hydrocarbon

21. 3-21 CHEM 100, Fall 2014 LA TECH Types of Chemical Formula Molecular Shows ratio of atoms each element in the : C 2 H 6 O Condensed Shows groups of atoms bonded together in the formula. E.g ethyl alcohol: CH 3 CH 2 OH Structural Shows bonding of important groups in the formu E.g ethyl alcohol: a compound. E.g ethyl alcohol

22. 3-22 CHEM 100, Fall 2014 LA TECH 2-25 Models of Ethanol CHEM 100, Fall 2012 LA TECH

23. 3-23 CHEM 100, Fall 2014 LA TECH 7) Given the structural formula of an organic compound, write the for the following: CH 3 CHClCH 2 OH a. molecular formula b. condensed formula c. structural formula d. line formula CHEM 100, Fall 2012 LA TECH 2-26

24. 3-24 CHEM 100, Fall 2014 LA TECH 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 1. Alkanes (saturated): single C-C bonds 2. Alkenes (unsaturated): double C=C bond 3. Alkynes (unsaturated): triple bond 4. Aromatic (unsaturated): benzene rings e lement. Hydrocarbons

25. 3-25 CHEM 100, Fall 2014 LA TECH methane – CH 4 ethane – C 2 H 6 propane – C 3 H 8 butane – C 4 H 10 pentane – C 5 H 12 hexane – C 6 H 14 heptane – C 7 H 16 octane – C 8 H 18 nonane – C 9 H 20 decane – C 10 H 22 Alkanes C n H 2n+2

26. 3-26 CHEM 100, Fall 2014 LA TECH Meth- 1 Eth- 2 Prop- 3 But- 4 Pent- 5 Hex- 6 Hept- 7 Oct- 8 Non- 9 Dec- 10 I see much memorization in your future! Prefix Carbons Base names of hydrocarbons

27. 3-27 CHEM 100, Fall 2014 LA TECH 8) Name, molecular, condensed and line formula of straight chain alkane (saturated hydrocarbons) or n-alkanes. a. 4 carbon n-alkane: b. 7 carbon n-alkane:

28. 3-28 CHEM 100, Fall 2014 LA TECH Compounds with the same number and type of atoms but with different arrangements are called constitutional isomers Condensed formulas Molecular Formula C 5 H 12 CH 3 CH 2 CH 2 CH 2 CH 3 pentane CH 3 CH(CH 3 )CH 2 CH 3 2-methylbutane (CH 3 ) 4 C 2,2-dimethylpropane All are isomers of C 5 H 12. What is an Isomer?

29. 3-29 CHEM 100, Fall 2014 LA TECH Alkane Isomers is there a formula?

30. 3-30 CHEM 100, Fall 2014 LA TECH 9) Draw the structural formula of constitutional isomers of butane with molecular formula C 4 H 10. a. n-butane: CH 3 CH 2 CH 2 CH 3 b. isobutene: (CH 3 ) 3 CH

31. 3-31 CHEM 100, Fall 2014 LA TECH Butane Butane molecules are present in the liquid and gaseous states in the lighter

32. 3-32 CHEM 100, Fall 2014 LA TECH Determine empirical formulas for the following: 1. An ionic compound that has two aluminum ions for every three oxide ions 2. Hexane, C 6 H 14 1. Arabinose, C 5 H 10 O 5 2. Hydrogen peroxide, Al 2 O 3 (C 3 H 7 ) n where n = 2 (CH 2 O) n where n = 2 (HO) n where n = 2

33. 3-33 CHEM 100, Fall 2014 LA TECH Classifying Organic Compounds Examples Functional Group Ending Hydrocarbons C and H only -ane Alcohols OH R-OH -ol Acids COOH R-COOH -oic acid Amines NH 2 R-NH 2 -amine Ketones C=O R(C=O)R’ -one Aldehydes CHO R-CHO -al

34. 3-34 CHEM 100, Fall 2014 LA TECH 10) Classification and the name of the following ClassificationName a.C n H 2n+2 where n is 8: b. CH 3 CH 2 CH 2 CH 2 -OH: c. CH 3 CH 2 CH 2 -COOH: d. CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 -NH 2 : a.CH 3 CH 2 -(C=O)-CH 3 : d) CH 3 CH 2 -CHO:

35. 3-35 CHEM 100, Fall 2014 LA TECH The Many Representations of a Molecule

36. 3-36 CHEM 100, Fall 2014 LA TECH Carbohydrate: Glucose Carbohydrate: Glucose Linear formCyclic form

37. 3-37 CHEM 100, Fall 2014 LA TECH Fats: triglycerides Fats: triglycerides Saturated fats Unsaturated fats

38. 3-38 CHEM 100, Fall 2014 LA TECH 11) Identify the classification or name of the following biologically important molecules a)b)c) d)e)f)