Maricopa Community Colleges  BPC135DK   20026-99999 

Official Course Description: MCCCD Approval: 12-13-2011

CHM151AA 2012 Summer I 2012 Summer II

LEC 4.0 Credit(s) 3.0 Period(s) 3.0 Load Acad

LAB 0.0 Credit(s) 3.0 Period(s) 2.4 Load

 

General Chemistry I

 

Detailed study of principles of chemistry for science majors and students in pre-professional curricula.

Prerequisites: [(CHM130 and CHM130LL), or CHM130AA, or one year of high school chemistry with a grade of "C", or better taken within the last five years], and completion of intermediate algebra. Completion of all prerequisites within the last two years is recommended.

 

Course Notes: Student may receive credit for only one of the following: CHM150 and CHM151LL, or CHM151 and CHM151LL, or CHM150AA, or CHM151AA.

 

Course Attribute(s):

General Education Designation: Natural Sciences (Quantitative) - [SQ]

 

 

 

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MCCCD Official Course Competencies:

 

CHM151AA 2012 Summer I 2012 Summer II

General Chemistry I

 

1. Define "chemistry" and describe its main branches. (I)

2. Use the factor-label (dimensional analysis) method in solving chemistry-related problems. (II)

3. Use metric and International System of Units (SI). (II)

4. Define the relationships between matter and energy. (III)

5. Describe the physical states of matter with the aid of the kinetic molecular theory. (III)

6. Classify matter as elements, compounds, or mixtures. (III)

7. Describe the properties of metallic and nonmetallic elements. (III)

8. Write formulas for and give names of simple inorganic compounds. (III)

9. Classify a property or change as physical or chemical. (III)

10. Complete and balance chemical equations. (IV)

11. Write a net ionic equation from a given reaction. (IV)

12. Determine the empirical and molecular formula from percentage composition or mass data. (V)

13. Perform calculations using the mole concept of mass and number. (V)

14. Solve problems involving the ideal gas laws. (VI)

15. Solve problems involving energy changes that result from physical state changes and from chemical reactions. (VII)

16. Apply Hess's law to given set of equations. (VII)

17. Calculate heats of reactions from calorimeter data and/or bond energies. (VII)

18. Solve stoichiometry problems, including problems involving solutions and heats of reactions. (VII)

19. Deduce the electronic structure of atoms and show the relationship between electronic structure and the chemical properties of atoms. (VIII)

20. Use the periodic table to predict the properties of elements and compounds. (VIII)

21. Identify substances as electrolytes or nonelectrolytes. (X)

22. Describe the properties of ionic and covalent compounds. (IX)

23. Write the electron dot structure for an atom, ion, ionic formula, or a covalently bonded specie. (IX)

24. Describe covalent chemical bonding. (IX)

25. Use the concepts of electronegativity and bond polarity in conjunction with Valence Shell Electron Pair Repulsion Theory (VSEPR) theory to predict the shapes and polarities of simple ions and molecules. (IX)

26. Classify intermolecular forces in a given substance. (X)

27. Classify a crystal as molecular, ionic, covalent, or metallic. (X)

28. Describe the properties of solutions. (XI)

29. Identify and evaluate chemical hazards and hazard warning signs (such as the 4-bar Hazardous Material Information System, the 4- diamond National Fire Protection Association System, and Material Safety Data Sheets). (II)

30. Cite the location and operation of common laboratory safety equipment. (II)

31. Given a written experimental procedure, plan and complete a series of steps to safely and successfully complete the experiment within the allotted time. (II)

32. Measure and dispense reagents. (II)

33. Determine the mass of a given substance using a balance, and record it to the correct number of significant figures. (II)

34. Set up and perform routine physical and chemical changes safely and effectively, including heating substances, mixing chemicals, filtering, and diluting solutions. (III)

35. Record and interpret observations of physical and chemical changes, using appropriate chemical terminology. (III)

36. Use measured values to calculate physical properties (e.g., density) to the correct number of significant figures. (II)

37. Given a standardized acid or base, perform a titration, and calculate the unknown concentration of a solution. (XI)

38. Construct and interpret a standard graph. (II)

39. Use scientific measuring devices to obtain chemical data. (II)

40. Apply principles, concepts, and procedures of chemistry to lab experiments. (II)

41. Use the scientific method in interpreting chemical data to arrive at rational conclusions. (I)

42. Use lab equipment properly and safely to perform a variety of chemical procedures and techniques. (I)

43. Prepare written reports, present data in a logical format, analyze data, and report conclusions. (I)

 

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MCCCD Official Course Outline:

 

CHM151AA 2012 Summer I 2012 Summer II

General Chemistry I

 

I. Definition of "chemistry"

A. History

B. Scientific method

II. Measurement

A. Metric system

B. Significant figures

C. Exponential notation

D. Dimensional analysis

III. Matter

A. States of matter

B. Classification of matter

C. Properties of matter

D. Physical and chemical changes

E. Atomic theory

F. Formulas and nomenclature of substances

G. International Union of Pure and Applied Chemistry (IUPAC) nomenclature

IV. Chemical reactions

A. Balancing equations

B. Types of reactions

C. Net ionic equations

V. Mole calculations with formulas and equations

A. Atomic and molecular weights

B. Mass-mole conversions

C. Percentage composition

D. Empirical and molecular formula

E. Stoichoimetry

F. Limiting reagents and percentage yields

G. Solution stoichiometry

VI. Gases

A. Gas laws

B. Stoichiometry with gases

C. Kinetic molecular theory

VII. Thermochemistry

A. Temperature/heat

B. Energy and units

C. Calorimetry

D. Enthalpy and enthalpy changes

E. Hess's law

VIII. Atomic theory and periodic table

A. Fundamental particles

B. Isotopes

C. Quantum theory and electronic structure

D. Periodic table and trends

IX. Chemical bonding

A. Ionic and covalent bonds

B. Electron dot structures

C. Electronegativity

D. Shapes and polarities of molecules

E. Hybrid orbitals

X. Solids and liquids

A. General properties

B. Changes of state

C. Intermolecular attractions

D. Types of solids

E. Phase diagrams

XI. Solutions

A. Definitions

B. Terminology

C. Concentration and stoichiometry

D. Colligative properties

 

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