NONCREDIT COURSE OUTLINE: HSSCI 11 Last Revised … · NONCREDIT COURSE OUTLINE: HSSCI 11 HSSCI 11 - PHYSICAL SCIENCE 1 - CHEMISTRY ... B. Exothermic reactions C. Endothermic reactions

Last Revised and Approved: 11/06/2009

NONCREDIT COURSE OUTLINE: HSSCI 11

HSSCI 11 - PHYSICAL SCIENCE 1 - CHEMISTRY

Total Hrs Lecture Total Hrs Lab Total Course Hrs

99.50Total Student Hrs

High School Credits 5.00

50.00 0.00 50.00

COURSE DESCRIPTION

This introductory chemistry class introduces students to the study of matter and changes in matter. Topics include states of matter,

chemical and physical changes, the development of the atomic theory, the periodic table and its use, writing chemical formulas,

balancing chemical equations, types of chemical reactions, and an introduction to organic chemistry.

ENROLLMENT RESTRICTIONS

PREREQUISITES COREQUISITES ADVISORIES

OUTLINE OF COURSE CONTENT

The course will address the following topics:

I. The Scientific Method

A. Posing questions

B. Developing a hypothesis

C. Experimental design

D. Data collection and interpretation

E. Conclusions

F. Repeatability and communication.

II. Scientific thought

A. Observing

B. Inferring

C. Predicting.

III. Matter and energy

A. Chemistry

B. Physics.

IV. Scientific development

A. Scientific models

B. Scientific laws

C. Scientific theories.

V. Laboratory safety

A. Lab prep

B. Lab performance

C. Post labs procedures

D. Accidents.

VI. Matter

A. Properties of matter

B. Physical properties

C. Chemical properties.

VII. Elements

A. Atoms

B. Compounds

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HSSCI 11 COURSE OUTLINE



C. Molecules.

VIII. Mixtures

A. Heterogeneous

B. Homogeneous

C. Separating.

IX. Measuring matter

A. Weight

B. Mass

C. Units and Système International

D. Volume and calculation of volume

E. Density and usage of density

F. Floating vs. sinking.

X. Changes in matter

A. Changes of state

B. Changes in shape or form

C. Chemical changes

D. Law of Conservation of Mass.

XI. Matter and thermal energy

A. Temperature and thermal energy

B. Thermal energy and changes in matter.

XII. Energy and matter

A. Kinetic energy

B. Potential energy

C. Chemical energy

D. Electromagnetic energy

E. Electrical energy

F. Energy transformations.

XIII. States of matter

A. Solids

B. Liquids

C. Gases.

XIV. Changes of state

A. Melting

B. Freezing

C. Evaporation

D. Boiling

E. Condensation

F. Sublimation.

XV. Gas behavior

A. Volume

B. Temperature

C. Pressure

D. Boyle’s Law

E. Charles’s Law.

XVI. Development of atomic models

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A. Dalton’s Atomic Theory

B. Thomson and electrons

C. Rutherford and the Gold Foil Experiment

D. Bohr Model

E. Cloud Model.

XVII. Modern atomic model

A. Particle charges

B. Particle masses

C. Scale and size of atoms

D. Atomic number

E. Mass number

F. Isotopes.

XVIII. Mendeleev’s work

A. Periodic table

B. Undiscovered elements

C. Modern periodic table.

XIX. Formation of elements

A. Matter in the sun/ plasma

B. Fusion

C. Supernovas.

XX. Metals

A. Shininess

B. Malleability

C. Ductility

D. Conductivity

E. Reactivity

F. Corrosion.

XXI. Metals and the periodic table

A. Alkali metals and their properties

B. Alkaline Earth metals and their properties

C. Transition metals and their properties

D. Mixed group metals

E. Lanthanides

F. Actinides

G. Particle accelerators.

XXII. Nonmetals

A. Physical properties

B. Chemical properties

C. Carbon family

D. Nitrogen family

E. Oxygen family

F. Halogens

G. Noble gases

H. Hydrogen.

XXIII. Metalloids

A. Conductivity

B. Semiconductors.

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XXIV. Radioactive elements

A. Marie Currie

B. Radioactive decay

C. Polonium and radium

D. Alpha, Beta, Gamma rays

E. Isotopes in science and medicine.

XXV. Atoms and bonding

A. Valence electrons

B. Electron dot diagrams

C. Chemical bonds and stability

D. Chemical bonds and chemical reactions.

XXVI. The Periodic Table

A. Relating periods and groups

B. Noble gases

C. Reactive nonmetals and metals

D. Other metals

E. Other nonmetals

F. Metalloids

G. Hydrogen.

XXVII. Ionic bonds

A. Ionization

B. Polyatomic ions

C. Ionic bonds.

XXVIII. Chemical formulas and naming

A. Formulas of ionic compounds

B. Naming ionic compounds

C. Ionic crystals

D. Properties of ionic compounds.

XXIX. Covalent bonds

A. Electron sharing

B. Number of bonds

C. Double and triple bonds.

XXX. Molecular compounds

A. Melting points and boiling points

B. Conductivity.

XXXI. Bonding

A. Polar bonds

B. Nonpolar bonds

C. Polar bonds in molecules

D. Attractions between molecules.

XXXII. Bonding in metals

A. Metals and alloys

B. Physical properties

C. Chemical properties

D. Metallic bonding.

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XXXIII. Properties and changes of matter

A. Physical properties

B. Chemical properties

C. Changes of matter

D. Bonding and chemical change

E. Evidence for chemical reactions.

XXXIV. Chemical reactions

A. Chemical formulas

B. Stiochiometry

C. Balancing equations

D. Law of Conservation of Mass

E. Open and closed systems

F. Synthesis

G. Decomposition

H. Single replacement

I. Double replacement.

XXXV. Controlling chemical reactions

A. Activation energy

B. Exothermic reactions

C. Endothermic reactions

D. Rates of reactions

E. Surface area

F. Temperature

G. Concentration

H. Catalysts

J. Inhibitors.

XXXVI. Solutions

A. Solutions with water

B. Solutions without water

C. Colloids

D. Suspensions

E. Ionic and molecular solutes

F. Solutes and conductivity

G. Freezing points and boiling points

H. Concentrations

I. Solubility

J. Pressure, temperature, solvent type

K. Saturation.

XXXVII. Acids

A. Properties of acids

B. Reactions with metals

C. Reactions with carbonates

D. Reactions with indicators.

XXXVIII. Bases

A. Properties of bases

B. Reactions with indicators.

XXXIX. Acids and bases

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A. Uses of acids and bases

B. Acids and bases in solution

C. Measuring pH

D. Acid-base reactions

E. Digestion and pH.

XL. Properties of carbon

A. Carbon atoms and bonding

B. Forms of carbon

C. Fullerenes and nanotubes.

XLI. Organic compounds

A. Hydrocarbons

B. Chemical formulas of hydrocarbons

C. Structural formulas

D. Isomers

E. Double and triple bonds/benzene

F. Saturated and unsaturated hydrocarbons

G. Functional groups

H. Polymers.

XLII. Biologically important organic molecules

A. Carbohydrates

B. Proteins

C. Lipids

D. Nucleic Acids

E. Vitamins and minerals

F. Water.

PERFORMANCE OBJECTIVES

Upon successful completion of this course, students will be able to do the following:

1). Explain the goal of science and describe the steps of the scientific method

2). Identify and compare metric units

3). Explore the role of tools in scientific studies

4). Analyze the general properties of matter

5). Compare and contrast physical properties and chemical properties

6). Classify matter as elements, compounds, solutions, or mixtures

7). Analyze the structure of an atom

8). Describe subatomic particles

9). Explore the development and design of the periodic table

10). Compare and contrast the properties of different families of elements and account for these properties

11). Explain chemical bonding and contrast ionic, covalent, and metallic bonding

12). Describe the basis of chemical reactions and interpret and balance equations

13). Compare and contrast exothermic and endothermic reactions and explain the factors that affect reaction rates

14). Analyze the properties of acids, bases and salts

15). Classify different carbon compounds and draw structural formulas for them

16). Identify petrochemical products and explain the process of polymerization

17). Compare and contrast types of nuclear reactions and describe the detection, measurement, and uses of radioactivity

18). Demonstrate safety and sanitary lab practices in the use of lab equipment

19). Demonstrate the ability to do independent laboratory work

20). Select and use appropriate tools and technology (such as computer-linked probes, spreadsheets, and graphing calculators) to

perform tests, collect data, analyze relationships, and display data

21). Identify and communicate sources of unavoidable experimental error

22). Identify possible reasons for inconsistent results, such as sources of error or uncontrolled conditions

23). Formulate explanations by using logic and evidence

24). Solve scientific problems using metric units

25). Distinguish between hypothesis and theory as scientific terms

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26). Recognize the usefulness and limitations of models and theories as scientific representations of reality

27). Recognize the issue of statistical variability and the need for controlled tests

28). Recognize the cumulative nature of scientific evidence

29). Analyze situations and solve problems that require combining and applying concepts from more than one area of science

30). Investigate and debate a science-based societal issue.

ASSIGNMENTS

Assignments will be consistent with, but not limited by, the following types and examples:

1). Analyze and interpret data obtained during in class laboratory experiments

2). Generate, read, and interpret graphs and data tables

3). Compare and contrast key concepts such as “endothermic and exothermic reaction”

4). Read and interpret current research studies related to the course material.

Outside-of-class assignments are required and may include, but will not be limited to, the following types and examples:

1). Make flash cards and learn the pertinent vocabulary related to the course material such as “the four states of matter and the

characteristics of each state”

2). Read chapter text and outline the key concepts using supplemental chapter outline packets, for example “how are the elements

organized on the periodic table”

3). Write essays related to the course content and documentation of lab procedures and observations

4). Maintain an organized notebook including all labs, lecture notes, homework, and vocabulary lists.

STUDENT LEARNING OUTCOMES

Learning Outcome Mode of Assessment

1. Chemistry is the study of the properties of matter and how

matter undergoes changes. Students will be able to define

matter, discuss the various types of matter, and show an

understanding of the Law of Conservation of Mass.

1. Exam multiple choice, true ans false, completion, short

answer, and essay questions.

2. Students will be able to read, interpret, analyze and evaluate

a chart, graph, or data table and answer questions based

upon their understanding of chemistry and the information

provided in the table, graph, and/or chart.

2. Exam multiple choice, true ans false, completion, short

answer, and essay questions.

3. Students will be able to solve basic chemistry problems using

metric measurements.

3. Examination problems

4. Physical Science I students will be able to identify and

compare metric units and solve mathematical problems in

chemistry using these metric units.

4. Examination math questions

Laboratory data collection and analysis

METHODS OF INSTRUCTION

Instructional methodologies will be consistent with, but not limited by, the following types or examples:

1). Instructor lectures

2). Laboratory experiments

3). Class demonstrations.

METHODS OF EVALUATION

Evaluation methodologies will be consistent with, but not limited by, the following types or examples:

1). Written exams including essay questions to test for content, terminology, and knowledge of subject matter

2). Post-laboratory lab reports to assess knowledge and understanding of major scientific concepts

3). Daily “brainteasers” to assess smaller individual concepts and terminology

4). Laboratory write-up and exam questions to assess student's ability to read, interpret, or construct a data table or graph based on

course-related data

5). Participation in class discussions related to course material and lecture topics.

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REQUIRED TEXTBOOKS

Examples of typical textbooks for this course include the following:

1). Prentice Hall Science Explorer, Physical Science. Pearson-Prentice Hall, 2005. ISBN: 0-13-190123-0

OTHER REQUIRED INSTRUCTIONAL MATERIALS

1). Calculator

2). Instructor-provided supplemental chapter outline packets.

COURSE REPEATABILITY

Total Completions Allowed: In Combination With:

1

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NONCREDIT COURSE OUTLINE: HSSCI 11 Last Revised … · NONCREDIT COURSE OUTLINE: HSSCI 11 HSSCI 11 - PHYSICAL SCIENCE 1 - CHEMISTRY ... B. Exothermic reactions C. Endothermic reactions