MCCCD Official Course Competencies:

CHM130  2008 Fall – 2010 Summer II

Fundamental Chemistry

1.

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

2.

Describe the relationships between matter and energy. (II)

3.

Distinguish between physical and chemical properties and changes. (II)

4.

Interpret symbols and formulas in terms of numbers and kinds of atoms. (II)

5.

Describe the physical states of matter with the aid of the Kinetic Molecular theory. (II, IX)

6.

Classify matter as elements, compounds, or mixtures. (II)

7.

Describe the properties of metallic and non-metallic elements. (II)

8.

Use the Unit-Factor Method in solving chemistry-related problems. (III)

9.

Name and write formulas for simple inorganic compounds. (IV, VII)

10.

Describe the relationship between the outer electronic structure of atoms and their chemical properties. (V)

11.

Use the Periodic Table to estimate the properties of elements and compounds. (V)

12.

Characterize the fundamental particles comprising the atom with respect to charge and mass. (V)

13.

State the number of protons, electrons, and neutrons in any given isotope, neutral or charged. (V)

14.

Use the Periodic Table in predicting the number of electrons, formula for a compound, and metallic or nonmetallic characteristics. (V)

15.

Draw a Lewis structure (electron dot) for a given ion or compound. (VI)

16.

State the type of intermolecular force that exists for a given substance. (VI)

17.

Describe the properties of ionic and covalent compounds. (VI)

18.

Describe the shape and polarity of simple molecules. (VI)

19.

Complete and balance simple chemical equations. (VIII)

20.

Solve elementary stoichoimetry problems. (VIII)

21.

Classify a reaction as endothermic or exothermic. (VIII)

22.

List the factors affecting the rate of a reaction. (VIII)

23.

Describe the chemical and physical properties of water. (IX)

24.

Describe the properties of solutions. (X)

25.

Identify substances as electrolytes or nonelectrolytes. (X)

26.

Classify substances as acids, bases, or salts. (XI)

27.

Explain the behavior of buffer systems. (XI)

28.

Define the pH scale of measuring the relative acidity of solutions. (XI)

29.

Define and identify redox reaction as exemplified by single replacement and combustion reactions. (XII)

MCCCD Official Course Outline:

CHM130  2008 Fall – 2010 Summer II

Fundamental Chemistry

I. Definition of chemistry

II. Properties of matter

A. State of matter

B. Classification of matter

C. Physical vs chemical changes

D. Energy

III. Measurement

A. Metric system

B. Unit-factor method of solving problems

C. Density

D. Temperature scales

IV. Mole concept

A. Atomic and molecular weights

B. Mass-mole conversions

C. Percentage composition

V. Atomic theory and periodic table

A. Fundamental particles

B. Isotopes

C. Quantum theory

1. Energy levels

2. Orbitals

3. Electron configuration

4. Valence electrons

D. Periodic Table and trends

E. Electronegativity

VI. Chemical bonding

A. Ionic and covalent bonds

B. Electron dot structures

C. Shape and polarity of molecules

VII. Nomenclature

A. Binary and ternary

B. Ionic-Stock

C. Covalent-classical

VIII. Chemical equations

A. Balancing equations

B. Types of chemical reactions

C. Stoichiometry

D. Heats of reaction

E. Rates of reactions

F. Driving forces

G. Equilibrium

IX. Properties of solids, liquids, and gases

A. Kinetic molecular theory

B. Changes of state (terminology involved)

C. Properties of states

D. Inter-molecular forces and changes of state

E. Water, hydrogen, and oxygen

X. Solutions

A. Definition

B. Properties

C. Weight percent concentration

D. Molarity

E. Terminology

XI. Acids-bases

A. Arrhenius definitions

B. Bronsted/Lowry definition

C. pH scale

D. Buffers

XII. Electrochemistry

A. Oxidation/reduction

B. Redox reactions