1. 1-1 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. 1-2 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. 1-3 CHEM 100, Fall 2014 LA TECH Chapter 1. 1. Matter, Measurement, and Problem Solving 1. 1 Atoms and Molecules………………………………….. 1 1.2 The Scientific Approach to Knowledge…………….. 3 1.3 The Classification of Matter…………………………… 5 1.4 Physical and Chemical Changes and Physical and Chemical Properties…………………………………….. 9 1.5 Energy: A Fundamental Part of Physical and Chemical Change…………………………………………………….. 12 1.6 The Units of Measurement……………………………... 13 1.7 The Reliability of a Measurement……………………… 20 1.8 Solving Chemical Problems……………………………. 27

4. 1-4 CHEM 100, Fall 2014 LA TECH Chapter 1. KEY CONCEPTS What is chemistry? Scientific Method. Properties of the three states of matter Physical changes and properties. Chemical change and properties. Categories of matter. Elements and Compounds Atomic symbols Chemical Elements and properties Chemical Symbolism Separating Mixtures. Scientific Measurement Prefixes of SI units Macro, micro and nano-scales Conversion factors. Factor label method. Uncertainty and significant figures Temperature Conversions. Density Calculations. Three chemical Laws Dalton's atomic theory Interpreting chemical formulas and chemical reaction. Concept of mole Gram to mole conversion

5. 1-5 CHEM 100, Fall 2014 LA TECH SOLIDS –have rigid shape, fixed volume. External shape can reflect the atomic and molecular arrangement. Reasonably well understood LIQUIDS –have no fixed shape and may not fill a container completely. Not well understood GASES –expand to fill their container. Good theoretical understanding The States of Matter

6. 1-6 CHEM 100, Fall 2014 LA TECH Matter Classifications

7. 1-7 CHEM 100, Fall 2014 LA TECH 1) Describe the classification of matter based on state of matter and composition.

8. 1-8 CHEM 100, Fall 2014 LA TECH 2) What is a pure substance? (Describe it generally and given two examples) 3) What is a chemical element? (Describe it generally and given an example)

9. 1-9 CHEM 100, Fall 2014 LA TECH 4) What is an allotrope of an element? (Describe it generally and given an example)

10. 1-10 CHEM 100, Fall 2014 LA TECH 5) What is a chemical compound? (Describe it generally and given an example)

11. 1-11 CHEM 100, Fall 2014 LA TECH

12. 1-12 CHEM 100, Fall 2014 LA TECH Physical Changes Phase changes Substance does not change into a new substance.Substance does not change into a new substance. Example:Example: –Ice (s) going to water (l) going to steam (g) Physical properties Density Color intensity Particle size Melting/ Freezing point Boiling point Texture Magnetism Physical Changes and Properties of Matter

13. 1-13 CHEM 100, Fall 2014 LA TECH Separating Mixtures to Pure Substances Flotation/buoyancy Depend on the density, of substances. Filtration/sedimentation Depend on the physical state (sloid/liquid) Distillation/evaporation Depend on the boiling points of substances. Chromatographic Separations Dependent of the affinity to substrate (paper). Magnetic Separations Dependent of the magenetic properties.

14. 1-14 CHEM 100, Fall 2014 LA TECH 6) What properties are used to separate mixtures into pure substances?

15. 1-15 CHEM 100, Fall 2014 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).

16. 1-16 CHEM 100, Fall 2014 LA TECH 7) How are the elements given symbols? (Give three examples) 8) How are the compounds given formulas? (Give three examples)

17. 1-17 CHEM 100, Fall 2014 LA TECH Physical Change of Matter

18. 1-18 CHEM 100, Fall 2014 LA TECH Chemical change or chemical reaction:Chemical change or chemical reaction: Making a NEW compoundMaking a NEW compound The transformation of one or more atoms or molecules into one or more different molecules Chemical Changes and Properties of Matter

19. 1-19 CHEM 100, Fall 2014 LA TECH Physical and Chemical Changes and Physical and Chemical Properties 9) What is a physical change? Describe it generally and given an example. 10) What is a chemical change? Describe it generally and given an example.

20. 1-20 CHEM 100, Fall 2014 LA TECH 11) List physical properties: Describe it generally giving an example. a) b) c) d) e)

21. 1-21 CHEM 100, Fall 2014 LA TECH 12) List chemical properties: name them and give an example. a) b) c) d)

22. 1-22 CHEM 100, Fall 2014 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.

23. 1-23 CHEM 100, Fall 2014 LA TECH 13) What is the difference between intensive and extensive properties? Give examples

24. 1-24 CHEM 100, Fall 2014 LA TECH Identify following as physical and chemical change: 14) Identify following as physical and chemical change: Frying an egg Vaporization of dry ice Burning Gasoline Breaking Glass Boiling water Souring MilkCompression of a spring Melting Glass Cutting grass Vine fermentation

25. 1-25 CHEM 100, Fall 2014 LA TECH Introduction to Energy

26. 1-26 CHEM 100, Fall 2014 LA TECH The energy of the universe is CONSERVED. 1st Law of Thermodynamics All matter possesses energy. Energy is classified as either kinetic or potential. Kinetic energy: energy associated with movement KE = I/2 mv2 Potential energy: energy associated with storage PE = mhg Energy can be converted from one form to another. When matter undergoes a chemical or physical change, the amount of energy in the matter changes as well. Energy

27. 1-27 CHEM 100, Fall 2014 LA TECH Changes in matter, both physical and chemical, result in the matter either gaining or releasing energy. Energy Energy is the capacity to do work. Work is the action of a force applied across a distance. A force is a push or a pull on an object. Electrostatic force is the push or pull on objects that have an electrical charge. Energy and Matter: One and the Same

28. 1-28 CHEM 100, Fall 2014 LA TECH 15) What is law of conservation of energy and how it applies to physical and chemical change given below? a) H 2 O(l)  H 2 O (g) b) CH 4 + 2O 2  CO 2 + 2H 2 O Energy: A Fundamental Part of Physical and Chemical Change