MCCCD Official Course Competencies:

CHM151  2007 Fall – 2011 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 SI systems of units. (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 electonegativity and bond polarity in conjunction with 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)

MCCCD Official Course Outline:

CHM151  2007 Fall – 2011 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. 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 VSEPR

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