1. 1-1 CHEM 100, Fall 2011 LA TECH 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 Exam: 9:30-10:45 am, CTH 328. Chemistry 100(02) Fall 2011 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. 1-2 CHEM 100, Fall 2011 LA TECH REQUIRED : Chemistry: The Molecular Science 4th 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. 1-3 CHEM 100, Fall 2011 LA TECH Chapter 1. 1.Why Care about Chemistry 2.Molecular Medicine 3.How Science is Done 4.Identifying Matter: Physical Properties 5.Chemical Changes and Chemical Properties 6.Classifying Matter: Substances and Mixtures 7.Classifying Matter: Elements and Compounds 8.Nanoscale Theories and Models 9.The Atomic Theory 10.The Chemical Elements

4. 1-4 CHEM 100, Fall 2011 LA TECH Chapter 1. KEY CONCEPTS What is chemistry? Scientific Method. Scientific Measurement Physical changes and properties. Temperature Conversions. Factor label method. Conversion factors. Density Calculations. Chemical change and properties. Categories of matter. Separating Mixtures. Elements and Compounds Atomic symbols Macro, micro and nano-scales Prefixes of unit of length Properties of the three states of matter Kinetic-molecular theory Dalton's atomic theory Three chemical Laws Discovery of elements Chemical Elements and properties Chemical Symbolism Interpreting chemical formulas and chemical reaction.

5. 1-5 CHEM 100, Fall 2011 LA TECH 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. 1-6 CHEM 100, Fall 2011 LA TECH Scientific Method

7. 1-7 CHEM 100, Fall 2011 LA TECH Kinetic Molecular Theory Matter consists of particles (atoms or molecules) in continuous, random motion.

8. 1-8 CHEM 100, Fall 2011 LA TECH 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 Properties of Gases

9. 1-9 CHEM 100, Fall 2011 LA TECH Gas Laws (This is not theory) Boyle's Law (V and P)Boyle's Law (V and P) Charles Law (V and T)Charles Law (V and T) Gay-Lussac's combined Gas LawGay-Lussac's combined Gas Law (V, P and T) (V, P and T) Avogadro's Law (V and n)Avogadro's Law (V and n) Ideal Gas Law (V, P, n, R and T)Ideal Gas Law (V, P, n, R and T) Scientific law is a summary or pattern in observation

10. 1-10 CHEM 100, Fall 2011 LA TECH 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. 1-11 CHEM 100, Fall 2011 LA TECH 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. 1-12 CHEM 100, Fall 2011 LA TECH 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. 1-13 CHEM 100, Fall 2011 LA TECH Development of Dalton’s Atomic Theory

14. 1-14 CHEM 100, Fall 2011 LA TECH 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. 1-15 CHEM 100, Fall 2011 LA TECH Law of Conservation of Mass: Law of Constant Proportions: Law of Multiple Proportions: Three Observed Chemical Laws:

16. 1-16 CHEM 100, Fall 2011 LA TECH Law of Conservation of Mass Total mass after a chemical reaction is same as before the reaction. H2 H2 H2 H2 + 1/2 O2 O2 O2 O2 ---> H2OH2OH2OH2O Hydrogen (4g) + oxygen (32g) ----> water 36g after the reaction.

17. 1-17 CHEM 100, Fall 2011 LA TECH A given chemical compound always contains exactly the same proportion of elements by weight. 36g of water contains 4g of hydrogen and 32g of oxygen take any other chemical compound. Law of Constant (Definite) Proportions

18. 1-18 CHEM 100, Fall 2011 LA TECH 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 Law of Multiple Proportions

19. 1-19 CHEM 100, Fall 2011 LA TECH 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. 1-20 CHEM 100, Fall 2011 LA TECH What is an Atom? Very small particle. Smallest particles of elements and molecules There about 110 types of elements or Atoms. There about 110 types of elements or Atoms. Different atoms have different physical properties and chemical reactivity

21. 1-21 CHEM 100, Fall 2011 LA TECH 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. 1-22 CHEM 100, Fall 2011 LA TECH Molecular Medicine

23. 1-23 CHEM 100, Fall 2011 LA TECH 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. 1-24 CHEM 100, Fall 2011 LA TECH one that can be observed without changing the substances present in the sample Examples –colordensity –odormelting point –tasteboiling point –feelcompressibility Properties of Matter: Physical Properties

25. 1-25 CHEM 100, Fall 2011 LA TECH 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 reactant products

26. 1-26 CHEM 100, Fall 2011 LA TECH 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. 1-27 CHEM 100, Fall 2011 LA TECH Chemical Change: caramelizing sugar

28. 1-28 CHEM 100, Fall 2011 LA TECH Chemical verses Physical change Sodium reacting Iodine changing with chlorine. from a solid to a gas

29. 1-29 CHEM 100, Fall 2011 LA TECH Pure substances Element Cannot be converted to a simpler form by a chemical reaction. ExampleExamplehydrogen and oxygenCompound Combination of two or more elements in a definite, reproducible way. ExampleExamplewater - H 2 O Both elements and compounds have characteristic properties such as color, boiling point and reactivity

30. 1-30 CHEM 100, Fall 2011 LA TECH Allotropes Graphite Diamond Buckminsterfullerine Forms of element that has different bonding pattern

31. 1-31 CHEM 100, Fall 2011 LA TECH Scheme for the Classification of Matter

32. 1-32 CHEM 100, Fall 2011 LA TECH Mixtures Heterogeneous Homogenous Compounds Atoms Electrons Nucleus Protons Neutrons Pure Substances Elements Hierarchy of Matter

33. 1-33 CHEM 100, Fall 2011 LA TECH Mixtures A combination of two or more pure substances. A combination of two or more pure substances. HomogeneousHomogeneous - Uniform composition (solution) HeterogeneousHeterogeneous - Non-uniform composition Which are homogeneous or heterogeneous? Blood Urine “T-Bone” steak Gasoline Twinkie Salad Dressing

34. 1-34 CHEM 100, Fall 2011 LA TECH Types of Elements metals nonmetals metalloids –semimetals Artificial Elements

35. 1-35 CHEM 100, Fall 2011 LA TECH Atomic Symbols Each element is assigned a unique symbol. arsenicAspotassiumK bariumBanickelNi carbonCnitrogenN chlorineCloxygenO hydrogenHradonRn heliumHetitaniumTi goldAu uraniumU 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). Some elements (about 11) the names were not in English. E.g., Sodium- Na (natrium-latin), potassium-K(kalium-latin).

36. 1-36 CHEM 100, Fall 2011 LA TECH Areas of Chemistry “The study of matter and the changes it undergoes.” Major divisions Inorganic Compounds of elements other than carbon OrganicCompounds of carbon BiochemistryCompounds of living matter PhysicalTheory and concepts AnalyticalMethods of analysis

37. 1-37 CHEM 100, Fall 2011 LA TECH 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. 1-38 CHEM 100, Fall 2011 LA TECH Separation of Mixtures Filtration distillation chromatography

39. 1-39 CHEM 100, Fall 2011 LA TECH Separate a solid (precipitate) form suspension:_________________ separate solids by differences in melting points:_________________ separate materials based on their differences in absorption on a support:______________ Separation of Mixtures (continued.)

40. 1-40 CHEM 100, Fall 2011 LA TECH Chromatography Liquid-column Paper thin-layer (TL Chromatography-TLC) Gas HPLC (high pressure liquid chromatogarphy) Electrophoresis (DNA mapping)

41. 1-41 CHEM 100, Fall 2011 LA TECH Physical States Solid fixed volume and shapeLiquid fixed volume shape of container, horizontal top surfaceGas takes shape and volume of container

42. 1-42 CHEM 100, Fall 2011 LA TECH Nanoscale representations of the three states of matter

43. 1-43 CHEM 100, Fall 2011 LA TECH Macroscale, Microscale, and Nanoscale

44. 1-44 CHEM 100, Fall 2011 LA TECH Sample Sizes macroscale physical properties that can be observed by the unaided human sensesmicroscale samples of matter that have to be viewed with a microscopenanoscale samples that are at the atomic or molecular scale where chemical reactions occur