1. 3-1 CHEM 100, Fall 2013 LA TECH Instructor: Dr. Upali Siriwardane e-mail: upali@coes.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 2013 September 30, 2013 (Test 1): Chapter 1 & 2 October 21, 2013 (Test 2): Chapter 3 & 4 November 13, 2013 (Test 3) Chapter 5 & 6 November 14, 2013 (Make-up test) comprehensive: Chapters 1-6 9:30-10:45:15 AM, CTH 328

2. 3-2 CHEM 100, Fall 2013 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 2013 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 2013 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 2013 LA TECH Elements and Compounds Groupings Atomic elements : Atomic elements : – elements whose particles are single atoms (He) Molecular elements: Molecular elements: – elements whose particles are multi-atom molecules (O 2 ) Molecular compounds: Molecular compounds: – compounds whose particles are molecules made of only nonmetals (H 2 O) Ionic compounds: Ionic compounds: – compounds whose particles are cations and anions (NaCl) Metallic elements Metallic elements – elements whose particles are made up of metal atoms (Cu) Metallic compounds (alloy) Metallic compounds (alloy) – compounds whose particles are mixture of metal atoms (Cu-Zn)

6. 3-6 CHEM 100, Fall 2013 LA TECH The compound propane contains individual C 3 H 8 molecules. The sodium chloride molecule, NaCl, is composed of an array of Na + ions and Cl – ions. Ionic vs. Molecular Compounds The platinum, Pt, metal is composed of an array of Pt atoms.

7. 3-7 CHEM 100, Fall 2013 LA TECH Ionic : Complete transfer of 1 or more electrons from one atom to another, usually between a metal and a nonmetal element Covalent: The sharing of valence 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. Intramolecular Chemical Bonding Types

8. 3-8 CHEM 100, Fall 2013 LA TECH Types of Compounds A) Molecular or Covalent Compounds A) Molecular or Covalent Compounds: non-metal + non-metal nonmetal oxide or halides: SO 2 nonmetal oxide or halides: SO 2 Organic compounds: C 3 H 8 Organic compounds: C 3 H 8 B) Ionic compounds: B) Ionic compounds: Metal + non-metal: Metal + non-metal: Type I a) Type I ionic compound (fixed charge) NaCl Type II b) Type II ionic compound FeCl 2 and FeCl 3, SnCl 2 and SnCl 4

9. 3-9 CHEM 100, Fall 2013 LA TECH 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. 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 Formula Weight? Formula Weight? Ionic compounds

10. 3-10 CHEM 100, Fall 2013 LA TECH

11. 3-11 CHEM 100, Fall 2013 LA TECH

12. 3-12 CHEM 100, Fall 2013 LA TECH Ionic compounds Molecular compounds(Inorganic & organic) Acids and bases Hydrated compounds Nomenclatuere: Naming Compounds

13. 3-13 CHEM 100, Fall 2013 LA TECH Formation of Ionic Compound, NaCl

14. 3-14 CHEM 100, Fall 2013 LA TECH Ionic Compounds Characteristics of compounds with ionic bonding: Compound of metal 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

15. 3-15 CHEM 100, Fall 2013 LA TECH Electrical Conductivity of Ionic Solution Electrolytes Aqueous solutions conducts electricity strong-electrolytes weak-electrolytes Non-electrolytes Aqueous solutions do not conducts electricity

16. 3-16 CHEM 100, Fall 2013 LA TECH Ionic Compounds Type II Type II ionic compound FeCl 2 and FeCl 3, SnCl 2 and SnCl 4 Type I Type I ionic compound (fixed charge) NaCl

17. 3-17 CHEM 100, Fall 2013 LA TECH Type IType II

18. 3-18 CHEM 100, Fall 2013 LA TECH Charges on Some Common Monatomic Cations and Anions

19. 3-19 CHEM 100, Fall 2013 LA TECH Charge on Metal Ions 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 :Fe 2+ and Fe 3+

20. 3-20 CHEM 100, Fall 2013 LA TECH NameFormula acetateC2H3O2–C2H3O2– carbonateCO 3 2– hydrogen carbonate (aka bicarbonate) HCO 3 – hydroxideOH – nitrateNO 3 – nitriteNO 2 – chromateCrO 4 2– dichromateCr 2 O 7 2– ammoniumNH 4 + NameFormula hypochloriteClO – chloriteClO 2 – chlorateClO 3 – perchlorateClO 4 – sulfateSO 4 2– sulfiteSO 3 2– hydrogen sulfate (aka bisulfate) HSO 4 – hydrogen sulfite (aka bisulfite) HSO 3 – Some Common Polyatomic Ions with Their Charge

21. 3-21 CHEM 100, Fall 2013 LA TECH 1) Identify the types of ions in the following list: F -,Fe 2+, Fe 3+,Ca 2+,H 3 O +,Ba 2+,Cl -,Cu +, Cu 2+, Sr 2+,Ra 2+,Ni 2+, Ni 4+, Br -,CrO 4 2-, Cr 2 O 7 2-, MnO 4 -, C 2 O 4 2-, NH 4 +, a) Cations: Type I : b) Cations: Type II : c) Monoatomic anions: d) Polyatomic anions: e) Polyatomic cations:

22. 3-22 CHEM 100, Fall 2013 LA TECH Polyatomic Ions More than one atom joined together have negative charge except for NH 4 + and its relatives negative charges range from -1 to -4 -1 to -4 Table in the Book

23. 3-23 CHEM 100, Fall 2013 LA TECH a) Cl - b) SO 4 2- c) SO 3 2- d) Fe 3+ e) Sr 2+ f) CO 3 -2 g) NO 3 - h) PO 4 3- i) Hg 2+ j) Hg 2 2+ k) Cr 2 O 7 2- l) MnO 4 - m) C 2 O 4 2- n) NH 4 +, o) U 4+ p) HCO 3 - q ) C 2 H 3 O 2 - or CH 3 COO - r) HSO 3 - s) HPO 4 - t) H 2 PO 4 - 2) Give the names of the following ions:

24. 3-24 CHEM 100, Fall 2013 LA TECH Ion Ion name Acid formula Acid name Ion Ion name a) ClO - i) IO - b) ClO 2 - j) IO 2 - c) ClO 3 - k) IO 3 - e) ClO 4 - l) IO 4 - f) SO 4 -2 m) SeO 4 -2 g) C 2 H 3 O 2 - n)BrO 3 - 3) Give the name of ion and the name and formula of acid it came from

25. 3-25 CHEM 100, Fall 2013 LA TECH Alkali and Alkaline Earth Metals Alkali and Alkaline Earth Metals – Metal name first, followed by nonmetal “IDE” – Nonmetal ending is exchanged with “IDE” Examples: – MgCl 2 : magnesium chloride – KNO 3 : potassium nitrate Alkali (+1) and alkaline earth (+2) metals’ oxidation states are known. Alkali (+1) and alkaline earth (+2) metals’ oxidation states are known. – That is why their charge is NOT indicated in the formula name! Naming Ionic Compounds: Metal + Nonmetal: Main Group (“p” Block) Metals

26. 3-26 CHEM 100, Fall 2013 LA TECH Metal name first, followed by nonmetal Metal’s oxidation state is indicated by a Roman numeral. Nonmetal ending is exchanged with “IDE.” Examples:Examples: » MnBr 4 :manganese (IV) bromide » Fe 2 O 3 :iron (III) oxide » SnF 2 :tin (II) fluoride Naming Ionic Compounds: Metal + Nonmetal for Transition and Main Group (“p” Block) Metals

27. 3-27 CHEM 100, Fall 2013 LA TECH 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. 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. changing the ending of the non-metal to -ide.

28. 3-28 CHEM 100, Fall 2013 LA TECH Ionic compounds Na + Mg 2+ Al 3+ Cl - O 2- N 3- Some simple ions Formula for some ionic compounds NaClMgCl 2 AlCl 3 Na 2 O MgO Al 2 O 3 Na 3 N Mg 3 N 2 AlN Cations Anions Exchange charge as subscripts on the metal and nonmetal Give the simple ratio

29. 3-29 CHEM 100, Fall 2013 LA TECH Nomenclature NaCl Fe 2 O 3 NH 4 NO 3 KClO 4 CaCO 3 NaOH AgNO 3 Mg(C 2 H 3 O 2 ) 2 Co 2 (SO 4 ) 3 KI Mg 3 N 2 NaClsodium chloride Fe 2 O 3 iron(III) oxide NH 4 NO 3 ammonium nitrate KClO 4 potassium perchlorate CaCO 3 calcium carbonate NaOH sodium hydroxide AgNO 3 silver nitrate Mg(C 2 H 3 O 2 ) 2 magnesium acetate Co 2 (SO 4 ) 3 cobalt(III) sulfate KI potassium iodide Mg 3 N 2 magnesium nitride

30. 3-30 CHEM 100, Fall 2013 LA TECH silver carbonate potassium hydrogen phosphate aluminum hydroxide sodium bicarbonate calcium acetate potassium permanaganate calcium perchlorate magnesium hydrogen sulfite sodium hypochlorite iron(II) carbonateIron(II)chloride nonahydrate barium oxide 4) Give the formula of following ionic compounds

31. 3-31 CHEM 100, Fall 2013 LA TECH tin(IV) chloritemercury(II) phosphate tin(II) carbonate mercurous acetate lead(II) chromate copper(I) sulfitestannous dichromate iron(III) nitrateferric sulfateferrous hydroxide potassium perchlorate lead(IV) hydrogen phosphate aluminum sulfate iron(II) bicarbonate barium iodatetin(II) hydrogen sulfide magnesium dihydrogen phosphate plumbous cyanide silver phosphate 5) Write the correct formula for:

32. 3-32 CHEM 100, Fall 2013 LA TECH Hydrate CoCl 2 ∙ 6H 2 O Anhydrous CoCl 2 Hydrated Compounds vs. Anhydrous Compounds

33. 3-33 CHEM 100, Fall 2013 LA TECH Hydrates are ionic compounds containing a specific number of waters for each formula unit. Hydrates are ionic compounds containing a specific number of waters for each formula unit. Water of hydration is often “driven off” by heating. Water of hydration is often “driven off” by heating. In formula, attached waters follow In formula, attached waters follow – CoCl 26H 2 O In name, attached waters are indicated by In name, attached waters are indicated by prefix + hydrate after name of ionic compound. – CoCl 26H 2 O = cobalt(II) chloride hexahydrate – CaSO 4½H 2 O = calcium sulfate hemihydrate PrefixNo. of Waters hemi½ mono1 di2 tri3 tetra4 penta5 hexa6 hepta7 octa8 Hydrated Compounds

34. 3-34 CHEM 100, Fall 2013 LA TECH Problem: 1. What is the formula of magnesium sulfate heptahydrate? 2. What is the name of NiCl 2 6H 2 O?

35. 3-35 CHEM 100, Fall 2013 LA TECH Answers: 1. What is the formula of magnesium sulfate heptahydrate? 2. What is the name of NiCl 2 6H 2 O? Mg 2+ + SO4 2− MgSO4 MgSO4  7H2O Ni 2+ + 2 Cl − nickel(II) chloride nickel(II) chloride hexahydrate

36. 3-36 CHEM 100, Fall 2013 LA TECH

37. 3-37 CHEM 100, Fall 2013 LA TECH UO 2 Co 3 (PO 4 ) 2 cobaltic nitrate magnesium dihydrogen phosphate CaCl 2  2H 2 O ammonium ferrous sulfate hexahydrate 6) Give the chemical name or the formulas for the following ionic compounds: