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Chemistry 100(02) Fall 2013

Chemistry 100(02) Fall 2013. 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 :.

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Chemistry 100(02) Fall 2013

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  1. Chemistry 100(02) Fall 2013 Instructor: Dr. UpaliSiriwardane e-mail: upali@coes.latech.edu Office: CTH 311 Phone257-4941 Office Hours: M,W, 8:00-9:30 & 11:30-12:30 a.m Tu,Th,F8:00 - 10:00 a.m.   Or by appointment Test Dates: 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. 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. Tro2nd Text Book & Resources

  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

  4. Chapter 3. KEY CONCEPTS

  5. Elements and Compounds Groupings • Atomic elements : • elements whose particles are single atoms (He) • Molecular elements: • elements whose particles are multi-atom molecules (O2) • Molecular compounds: • compounds whose particles are molecules made of only nonmetals (H2O) • Ionic compounds: • compounds whose particles are cations and anions (NaCl) • Metallic elements • elements whose particles are made up of metal atoms (Cu) • Metallic compounds (alloy) • compounds whose particles are mixture of metal atoms (Cu-Zn)

  6. Ionic vs. Molecular Compounds The sodium chloride molecule, NaCl, is composed of an array of Na+ ions and Cl– ions. The compound propane contains individual C3H8 molecules. The platinum, Pt, metal is composed of an array of Pt atoms.

  7. Intramolecular Chemical Bonding Types • 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.

  8. 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 Iionic compound (fixed charge) NaCl b) Type IIionic compound FeCl2 and FeCl3, SnCl2 and SnCl4

  9. 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 Formula Weight? Ionic compounds

  10. Nomenclatuere: Naming Compounds • Ionic compounds • Molecular compounds(Inorganic & organic) • Acids and bases • Hydrated compounds

  11. Formation of Ionic Compound, NaCl

  12. 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

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

  14. Ionic Compounds Type IIionic compound FeCl2 and FeCl3, SnCl2and SnCl4 Type Iionic compound (fixed charge) NaCl

  15. Type I Type II

  16. Charges on Some Common Monatomic Cations and Anions

  17. 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+ Charge on Metal Ions

  18. Some Common Polyatomic Ions with Their Charge

  19. 1) Identify the types of ions in the following list: • F-,Fe2+, Fe3+,Ca2+,H3O+,Ba2+,Cl-,Cu+, Cu2+, Sr2+,Ra2+,Ni2+, Ni4+, Br-,CrO42-, Cr2O72-, MnO4-, C2O42-, NH4+, • a) Cations: Type I : • b) Cations: Type II : • c) Monoatomic anions: • d) Polyatomic anions: • e) Polyatomic cations:

  20. 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

  21. 2) Give the names of the following ions:

  22. 3) Give the name of ion and the name and formula of acid it came from

  23. Naming Ionic Compounds: Metal + Nonmetal: Main Group (“p” Block) Metals • Alkali and Alkaline Earth Metals • Metal name first, followed by nonmetal • Nonmetal ending is exchanged with “IDE” Examples: • MgCl2: magnesium chloride • KNO3: potassium nitrate • Alkali (+1) and alkaline earth (+2) metals’ oxidation states are known. • That is why their charge is NOT indicated in the formula name!

  24. Naming Ionic Compounds: Metal + Nonmetal for Transition and Main Group (“p” Block) Metals • Metal name first, followed by nonmetal • Metal’s oxidation state is indicated by a Roman numeral. • Nonmetal ending is exchanged with “IDE.” • Examples: • MnBr4: manganese (IV) bromide • Fe2O3: iron (III) oxide • SnF2: tin (II) fluoride

  25. 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.

  26. 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

  27. 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

  28. 4) Give the formula of following ionic compounds

  29. 5) Write the correct formula for:

  30. Hydrated Compounds vs. Anhydrous Compounds Hydrate CoCl2∙6H2O Anhydrous CoCl2

  31. Hydrates are ionic compounds containing a specific number of waters for each formula unit. Water of hydration is often “driven off” by heating. In formula, attached waters follow CoCl2•6H2O In name, attached waters are indicated by prefix + hydrateafter name of ionic compound. CoCl2•6H2O = cobalt(II) chloride hexahydrate CaSO4•½H2O = calcium sulfate hemihydrate Hydrated Compounds

  32. Problem: 1. What is the formula of magnesium sulfate heptahydrate? 2. What is the name of NiCl2•6H2O?

  33. Answers: 1. What is the formula of magnesium sulfate heptahydrate? 2. What is the name of NiCl2•6H2O? Mg2+ + SO42− MgSO4 MgSO47H2O Ni2+ + 2 Cl− nickel(II) chloride nickel(II) chloride hexahydrate

  34. 6) Give the chemical name or the formulas for the following ionic compounds:

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