Chemistry 100(02) Fall 2013

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 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. Chapter 1. KEY CONCEPTS

5. What is chemistry? • 1. Chemistry deals with non-reversible changes of • matter • 2. Chemistry explains using atoms, molecules and • ions. • 3. Chemical Concepts and Models improve your • problem solving skills • 4. Chemistry is a Central Science

6. What is an Atom? • Very small particle. • 2. Chemistry explains using atoms, molecules and • ions. • 3. Chemical Concepts and Models improve your • problem solving skills • 4. Chemistry is a Central Science

7. The States of Matter • 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

8. Matter Classifications

9. 1) Describe the classification of matter based on state of matter and composition.

10. 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)

11. 4) What is an allotrope of an element? (Describe it generally and given an example)

12. 5) What is a chemical compound? (Describe it generally and given an example)

14. Physical Changes and Properties of Matter • Physical Changes • Phase changes • Substance does not change into a new substance. • 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

15. 6) What properties are used to separate mixtures into pure substances?

16. 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).

17. 7) How are the elements given symbols? (Give three examples) •  8) How are the compounds given formulas? (Give three examples)

18. Physical Change of Matter

19. Chemical Changes and Properties of Matter • Chemical change or chemical reaction: • Making a NEW compound • The transformation of one or more atoms or molecules into one or more different molecules

20. 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.

21. 11) List physical properties: Describe it generally giving an example. • a) • b) • c) • d) • e)

22. 12) List chemical properties: name them and give an example. • a) • b) • c) • d)

23. 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.

24. 13) What is the difference between intensive and extensive properties? Give examples

25. 14) Identify following as physical and chemical change:

26. Introduction to Energy

27. Energy • 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.

28. Energy and Matter: One and the Same • Changes in matter, both physical and chemical, result in the matter either gaining or releasing 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.

29. Energy: A Fundamental Part of Physical and Chemical Change • 15) What is law of conservation of energy and how it applies to physical and chemical change given below? • a) H2O(l)  H2O (g) • b) CH4 + 2O2 CO2 + 2H2O