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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. REQUIRED: Chemistry: The Molecular Science4th Edition, John W. Moore, Conrad L. Stanitski and Peter C. Jurs. 2010 Brooks and Cole ISBN-10: 1439049300  ISBN-13: 9781439049303  OWL:  Students are required to buy access to OWL program offered by Brooks/Cole's) OPTIONAL: Study Guide: 4th Edition, John W. Moore, Conrad L. Stanitski and Peter C. Jurs. 2010 Brooks and Cole Edited by Michael J. Sanger. Student Solutions Manual:The Molecular Science, 4th by Moore/Stanitski/Jurs, Edited by Jusy L. Ozment Text Book & Resources

  3. Chapter 1. Why Care about Chemistry Molecular Medicine How Science is Done Identifying Matter: Physical Properties Chemical Changes and Chemical Properties Classifying Matter: Substances and Mixtures Classifying Matter: Elements and Compounds Nanoscale Theories and Models The Atomic Theory The Chemical Elements

  4. Chapter 1. KEY CONCEPTS

  5. What is chemistry? • Chemistry deals with non-reversible changes of matter. • Chemistry explains using atoms and molecules. • Chemical Concepts and Models improve your problem solving skills • Chemistry is a Central Science

  6. Scientific Method

  7. Kinetic Molecular Theory Matter consists of particles (atoms or molecules) in continuous, random motion.

  8. Properties of Gases • can be compressed • exert pressure on whatever surrounds them • expand into whatever volume is available • easily diffuse into one another • can be described in terms of their temperatures and pressure, the volume occupied, and the amount (number of molecules or moles) present

  9. Gas Laws (This is not theory) • Boyle's Law (V and P) • Charles Law (V and T) • Gay-Lussac's combined Gas Law • (V, P and T) • Avogadro's Law (V and n) • Ideal Gas Law (V, P, n, R and T) Scientific law is a summary or pattern in observation

  10. Kinetic Molecular Theory: Gases • particles in continuous, random, rapid motion • collisions between particles are elastic • volume occupied by the particles is negligibly small effect on their behavior • attractive forces between particles have a negligible effect on their behavior • gases have no fixed volume or shape, take the volume and shape of the container

  11. Kinetic Molecular Theory: Solid • particles are tightly packed together in regular array • particles vibrate about average positions • seldom squeeze past other atoms • results in a rigid material with a small, fixed volume for a given mass • external shape often reflects internal arrangement of particles

  12. Kinetic Molecular Theory: Liquid • particles are arranged more randomly than in solid • particles less confined so that they can move past one another • particles are a little further apart, thus slightly larger, fixed volume • particles are constantly interacting with one another

  13. Development of Dalton’s Atomic Theory

  14. Alchemist: Discovery of Elements • Early scientist observed chemical changes of matter. They called these changes chemical reactions when there are changes in substances or the physical & chemical properties of the matter. They also observed a pattern or a repeatable observation during chemical reactions.

  15. Three Observed Chemical Laws: • Law of Conservation of Mass: • Law of Constant Proportions: • Law of Multiple Proportions:

  16. Law of Conservation of Mass • Total mass after a chemical reaction is same as before the reaction. • H2 + 1/2 O2 ---> H2O • Hydrogen (4g) + oxygen (32g) ----> water 36g after the reaction.

  17. Law of Constant (Definite) Proportions • A given chemical compound always contains exactly the same proportion of elements by weight. • 36gofwater contains • 4g of hydrogen and 32g of oxygen • take any other chemical compound.

  18. Law of Multiple Proportions When two elements make a series of chemical compounds, the ratio of the masses of the second elements that combine with 1 gram of the first element can always be reduced to simple whole numbers. C O E.g. carbon monoxide 1g 1.33g carbon dioxide 1g 2.66g

  19. Dalton’s atomic theory • All matter is composed of atoms -- the smallest particle of an element that takes part in a chemical reaction. • All atoms of an element are alike. • Compounds are combinations of atoms of one or more elements. The relative number of atoms each element is always the same. • Atoms cannot be created or destroyed by a chemical reaction. They only change how they combine with each other.

  20. What is an Atom? • Very small particle. • Smallest particles of elements and molecules • There about 110 types of elements or Atoms. • Different atoms have different physical properties and chemical reactivity

  21. Models of matter Models are commonly used to help visualize atoms and molecules. • Atom- The smallest unit of an element that has all of the properties of an element. • Molecule -The smallest unit of a pure substance that has the properties of that substance. It may contain more that one atom and more than one element. • Ions- Charged particles formed by the transfer of electrons between atoms or molecules

  22. Molecular Medicine

  23. Properties of Substances • Physical properties: • Physical properties are descriptions of matter such as color, density, viscosity, boiling point, and melting point. • Chemical properties: • Chemical properties relates to the changes of substances making up the matter. For example, corrosiveness, Flammability

  24. Properties of Matter:Physical Properties one that can be observed without changing the substances present in the sample • Examples • color density • odor melting point • taste boiling point • feel compressibility

  25. Properties of Matter Chemical Property • the tendency to react and form new substances • reactants undergo chemical change to produce products: Chemical Reaction sucrose => carbon + water reactant products

  26. Extensive and Intensive Properties • Extensive properties • Depend on the quantity of sample measured. • Example - mass and volume of a sample. • Intensive properties • Independent of the sample size. • Properties that are often characteristic of the substance being measured. • Examples - density, melting and boiling points.

  27. Chemical Change: caramelizing sugar

  28. Chemical verses Physical change Sodium reacting Iodine changing with chlorine. from a solid to a gas

  29. Pure substances • Element • Cannot be converted to a simpler form by a chemical reaction. • Example hydrogen and oxygen • Compound • Combination of two or more elements in a definite, reproducible way. • Example water - H2O • Both elements and compounds have characteristic properties such as color, boiling point and reactivity

  30. Graphite Diamond Buckminsterfullerine Allotropes Forms of element that has different bonding pattern

  31. Scheme for the Classification of Matter

  32. Hierarchy of Matter Mixtures Heterogeneous Homogenous Pure Substances Compounds Elements Atoms Nucleus Electrons Neutrons Protons

  33. Mixtures • A combination of two or more pure substances. • Homogeneous - Uniform composition (solution) • Heterogeneous - Non-uniform composition • Which are homogeneous or heterogeneous? • Blood Urine “T-Bone” steak • Gasoline Twinkie Salad Dressing

  34. Types of Elements • metals • nonmetals • metalloids – semimetals • Artificial Elements

  35. Atomic Symbols • Each element is assigned a unique symbol. arsenic As potassium K barium Ba nickel Ni carbon C nitrogen N chlorine Cl oxygen O hydrogen H radon Rn helium He titanium Ti gold Au uranium U • Each symbol consists of 1 or 2 letters. The first is capitalized and the second is lower case. • Symbol may not match the name - often had a different name to start with. • Some elements (about 11) the names were not in English. E.g., Sodium-Na (natrium-latin), potassium-K(kalium-latin).

  36. Areas of Chemistry “The study of matter and the changes it undergoes.” Major divisions • InorganicCompounds of elements other than carbon • OrganicCompounds of carbon • Biochemistry Compounds of living matter • Physical Theory and concepts • Analytical Methods of analysis

  37. How do you Separate Mixtures? • Flotation: based on density • Filtration: Solid- liquid • Distillation- Liquid-liquid • Magnetic Separation- Magnetic • Chromatography: • 1) Paper 2) Column 3) Gas

  38. Separation of Mixtures • Filtration • distillation • chromatography

  39. Separation of Mixtures (continued.) • Separate a solid (precipitate) form suspension:_________________ • separate solids by differences in melting points:_________________ • separate materials based on their differences in absorption on a support:______________

  40. Chromatography • Liquid-column • Paper • thin-layer (TL Chromatography-TLC) • Gas • HPLC (high pressure liquid chromatogarphy) • Electrophoresis(DNA mapping)

  41. Physical States • Solid • fixed volume and shape • Liquid • fixed volume • shape of container, horizontal top surface • Gas • takes shape and volume of container

  42. Nanoscale representations of the three states of matter

  43. Macroscale, Microscale, and Nanoscale

  44. Sample Sizes • macroscale • physical properties that can be observed by the unaided human senses • microscale • samples of matter that have to be viewed with a microscope • nanoscale • samples that are at the atomic or molecular scale where chemical reactions occur

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