Portland Community College | Portland, Oregon

Course Number:
CH 151
Course Title:
Preparatory Chemistry
Credit Hours:
5
Lecture Hours:
40
Lecture/Lab Hours:
0
Lab Hours:
30
Special Fee:
$12.00

Course Description

Introduces basic chemical principles and computational problems found in General Chemistry with a concentration on developing both analytical and reasoning skills via problem solving. Prepares students wanting to take the CH 221-3 General Chemistry series that have no chemical background or have not taken a college or high school chemistry course in the last 3 years. Prerequisites: WR 115, RD 115 and MTH 95 or equivalent placement test scores. Audit available.

Addendum to Course Description

For CH 151 Competency Exam information  visit the following website:

http://www.pcc.edu/resources/testing/proctored/chemistry.html

Intended Outcomes for the course

Upon completion of the course students should be able to:

  • Demonstrate an emerging ability to use effective written and/or oral communication through the application of preparatory chemical concepts and reasoning using the language of chemistry.
  • Demonstrate an emerging understanding of how preparatory chemistry impacts the natural and technological environments.
  • Demonstrate an emerging ability to use detailed data collection, analysis and collaborative skills in order to explore preparatory chemical principles, critically evaluate models and information, draw conclusions and communicate results.  
  • Demonstrate an emerging understanding of chemical principles and collaborative skills to effectively solve problems encountered in preparatory chemistry using appropriate computational and reasoning skills.

Aspirational Goals

Core Outcome 4: Cultural Awareness

Demonstrate appropriate cultural awareness within the preparatory chemistry field.

Core Outcome 6:  Self Reflection

Demonstrate effective self-reflective skills within the preparatory chemistry field.

Course Activities and Design

At the beginning of the course, the instructor will detail the methods used to evaluate student progress and the criteria for assigning a course grade. The methods may include one or more of the following tools: examinations, quizzes, homework assignments, laboratory write-ups, research papers, small group problem solving of questions arising from application of course concepts and concerns to actual experience, oral presentations, or maintenance of a personal lab manual.


At least two written lecture examinations, including the final examination, are scheduled during theterm. Nonscheduled quizzes may occasionally be given at the discretion of the instructor. Written examinations include typical problems encountered in previous class work and laboratory. These examinations may also include challenge problems that ask students to apply concepts learned in class and lab in a new way in order to evaluate problem-solving ability and development of higher level thinking skills. Since this is a preparatory course, the student's competency in mathematical topics is important to successful completion of the course.

Outcome Assessment Strategies

PCC Core Outcome Mapping Communication - Mapping Level Indicator 1

Demonstrate a limited ability to use effective written and/or oral communication through the application of chemical concepts and reasoning using the language of chemistry

PCC Core Outcome Mapping: Community and Environmental Responsibility - Mapping Level Indicator 1

Demonstrate limited understanding of how chemistry impacts the natural and technological environments.

PCC Core Outcome Mapping: Critical Thinking and Problem Solving - Mapping Level Indicator 1

Demonstrate a limited ability to use detailed data collection, analysis and collaborative skills in order to explore preparatory chemical principles, critically evaluate models and information, draw conclusions and communicate results.

PCC Core Outcome Mapping: Professional Competency - Mapping Level Indicator 1

Demonstrate limited understanding of chemical principles and collaborative skills to effectively solve problems encountered in preparatory chemistry using appropriate computational and reasoning skills.

General

Grades and competency will be determined according to student ability to demonstrate knowledge of specific chemistry topics and complete work by assigned deadlines; participate and complete reports of assigned laboratory experiments; and an evaluation of chemical topics assigned.

Course Content (Themes, Concepts, Issues and Skills)

CH151 Course Specific Objectives

The following objectives will be demonstrated by student on written assignment or assessments in  lab or lecture.

Scientific Method

Define the scientific means of hypothesis, theory and law.

Measurements

List SI units of length, mass, time, and temperature.

List the multipliers, symbols, and numerical meanings for all SI units.

Convert numbers between scientific notation and decimal notation.

Given a quantity, convert from one set of units to another using dimensional analysis showing canceling of units.

This includes:
One factor conversions
Multiple factors conversions
Compound units (eg.: mph to kps)
Numbers and units raised to a power

Given an instrument and an object make a measurement including units with the appropriate level of uncertainty.

Given a physical quantity, identify the correct number of significant figures.

When using measured physical quantities in calculations report the correct number of significant figures in an answer.

Given a mass and volume calculate the density of a substance.

Convert temperatures between Celsius, Kelvin, and Fahrenheit scales.

Matter and Atomic Structure

Given a particle level picture, macroscopic description, or chemical symbol classify the type of matter.  (Benchmark: 85%)

Given a property of matter, classify as physical or chemical. (Benchmark: 85%)

Classify changes in matter as physical or chemical on the particle level. (Benchmark: 85%)

Name the three subatomic particles and provide their relative mass, charge, and location in the atom. (Benchmark: 85%)

Convert between a chemical species and the number of protons, neutrons, and electrons.  (Benchmark: 85%)

Given two or more chemical species determine if they are isotopes.  (Benchmark: 85%)

Given the isotopic abundance and atomic weight of each isotope they should be able to determine the average atomic weight.  (Benchmark: 85%)

Graphing

Given a set of data containing two related quantities, construct an appropriately labeled and scaled hand-drawn graph.  (Benchmark: 85%)

Given a set of data containing two related quantities, construct an appropriately labeled computer-generated graph. (Benchmark: 85%)

Given a graph with a linear correlation between variables, write a linear equation using physical variables and units instead of x and y. (Benchmark: 85%)

Determine slope and y-intercept of  linear set of data with appropriate units. (Benchmark: 85%)

Periodic table: groups, periods, regions (metals, nonmetal, metalloids)

Given the name or symbol of an element and a periodic table, identify if the element is a metal, nonmetal, or metalloid. (Benchmark: 85%)

Given the name or symbol of an element and a periodic table, identify if the element is a main-group element or a transition metal. (Benchmark: 85%)

Given the name or symbol of an element and a periodic table, identify the period and group number of the element on an exam. (Benchmark: 85%)

Given the name or symbol of an element and a periodic table, identify if that element is an alkali metal, alkaline earth metal, halogen, noble gas, or none of these on an exam. (Benchmark: 85%)

Name and write the symbols of the diatomic seven. (Benchmark: 85%)

Compounds and Nomenclature

Given the symbol for a monatomic (of a fixed-charge or variable-charged element) or polyatomic ion correctly write the systematic name. (Benchmark: 85%)

Given the systematic name for a monatomic (of a fixed-charge or variable-charged element) or polyatomic ion correctly write the symbol: phosphate, sulfate, nitrate, carbonate, hydroxide, ammonium and chlorate (Benchmark: 85%)

Given the name of an ionic compound (which may contain a fixed-charge or variable charge metal and may contain a polyatomic ion), write the formula. (Benchmark: 85%)

Given the formula of an ionic compound (which may contain a fixed-charge or variable charge metal and may contain a polyatomic ion), write the name. (Benchmark: 85%)

Given the name of a binary covalent inorganic compound, write the formula. (Benchmark: 85%)

Given the formula of a binary covalent inorganic compound, write the name. (Benchmark: 85%)

Predict the charge of monatomic main group ions.  (Benchmark: 85%)

Describe ionic compounds as an extended three dimensional array, lattice structure, versus discrete molecules in covalent compounds.   (Benchmark: 85%)

Explain that the formula of an ionic compound specifies the ratio of cations to anions, while the molecular formula specifies the number of atoms in the molecule. (Benchmark: 85%)

Differentiate between aqueous solutions of ionic and covalent compounds. (Benchmark: 85%)
 

Moles

Define the mole and explain the need for this chemical counting unit. (Benchmark: 85%)

Convert between mass of the substance the number of moles. (Benchmark: 85%)

Convert between the mass of the substance and the number of particles. (Benchmark: 85%)

Given a compound formula and the mass of the substance calculate the mass of constituent elements and number of component particles (elements or ions).    (Benchmark: 85%)

Given a chemical formula calculate the percent composition of each component element. (Benchmark: 85%)

Chemical Equations

Recognize physical evidence that chemical reaction has occurred. (Benchmark: 85%)   

Given a chemical equation classify the equation as a combination, decomposition, single replacement, or double displacement reaction. (Benchmark: 90%)

Given a sentence that describes a chemical reaction write a chemical equation. (Benchmark: 85%)

Given the reactants in an aqueous chemical reaction predict products in a double displacement reaction.  (Benchmark: 75%)

Given an unbalanced chemical equation balance the equation (Benchmark: 85%)

Student will use the ratio from the balanced equation to solve mole to mole and mass to mass calculations involving reactions. (Benchmark: 70%)