Suggested readings are listed on the syllabus for each topic.  Note that the test may include any material that was discussed or assigned in class and that all of this material may not be covered by the review questions listyed below.

Topic #1

1. Be able to describe the steps of the scientific method.
2. Be able to define/explain the terms:

    Hypothesis
    Operationally define the hypothesis
    Working hypothesis
    Scientific law
    Theory

3. What is the relationship between a hypothesis, a theory, and a law?
Which is the most certain?  Which is the least certain?

4. What is the real value of a theory in science?

Topic #2

1. What is a physical quantity?
2. Be able to define density?
3. Be able to describe how we determined the density of the rubber stopper in class and to calculate density when given the mass and volume information.
4. What is the difference between mass and weight?
5. Be able to state definitions of mass and weight.
6. What is the difference between a scaler quantity and a vector quantity?  Be familiar with the examples discussed in class.
7. Be able to state Archimedes’ Principle.  Be able to explain why objects float or sink in terms of density differences between the object and the liquid.
8. What is the buoyant force? (see page 110)

Topic #3

1. What is the difference between speed and velocity?
2. Be able to define/explain the following terms.  Which are vector quantities?:
        Velocity
        Acceleration
        Inertia
        Force
        Mass
        Weight

3. Be able to describe each of the following:

        Newton’s First Law of Motion
        Newton’s Second Law of Motion
        Newton’s Third Law of Motion

4. Which of Newton’s Laws of Motion is associated with:

        Inertia?
        Force?
        Action-Reaction pairs?

5. What is the Law of Inertia?

6. What are the 3 essential characteristics of an action-reaction pair.
Be familiar with the action-reaction pairs described in class and in
the textbook (pages 43-45) and be able to explain how each pair satisfies the 3 requirements of an action-reaction pair.

7. For an object to change velocity which of the following must be true?

        Force applied changes
        Acceleration changes

Topic #4

1. What is energy?

2. Be able to define kinetic energy and potential energy.

3. Review figures 3.15, 3.16, 3.17, and 3.18 and the class notes on this topic and be able to analyze these cases in terms of the changes that take place with respect to the potential energy and the kinetic energy.

Topic #5

1. What is temperature?  What is the difference between heat and temperature?

2. If the temperature of a room increases, how does the velocity or rate of motion of the gas molecules and atoms change?  How does the kinetic energy change?

3. If the temperature of a room decreases, how does the velocity or rate
     of motion of the gas molecules and atoms change?  How does the
     kinetic energy change?

4. Be able to describe each of the 3 methods of heat transfer:
                        conduction, convection, and radiation .
     Be familiar with the examples discussed in class for each of these.

5. Be familiar with the 3 temperature scales discussed in class and the
symbols used for each.  What is the chief advantage of the Celsius scale over the Fahrenheit scale?  What is the chief advantage of the Kelvin scale over the other 2 scales?

6. Be able to convert from from the Fahrenheit to the Celsius scale and from the Celsius scale to the Fahrenheit scale.
 

Topic #6

1. Be able to describe, compare, and give an example of each of the following types of waves:  longitudinal waves
     transverse waves .

1a. Understand the relatiojnship between the rarefaction and compression phases of a longitudinal wave and the crest and trough of a transverse wave.

2. Be able to sketch a transverse wave and identify the following parts:
           amplitude
           crest
           trough               (see Fig 10.1)

3. What type of wave is light? sound? an ocean wave?

4. Be familiar with how the speed of transmission (rate of movement) of sound and light waves changes with each of the following?

        Type of material it is moving through
        Density of the material it is moving through
        Temperature

5. Be able to describe each of the following:

        Diffraction of light
        Law of reflection (reflection of light)
        Refraction of light

6. What is responsible for the refraction of light when a ray of light passes from one medium into a second medium?  For example, when light passes from air into a pool of water?

6a. Be able to predict the relationship between the angle of incidence and the angle of refraction when light passes from one medium into another medium.

6b. Be able to predict the relationship between the angle of incidence and the angle of reflection for an incident light ray on a reflective surface.

7. What does a diffraction grating do?

8. Be familiar with the different types of  electromagnetic radiation.

9. Be able to describe some of the general properties of light (see notes).
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Topic 8 – Chapter 15 - Lecture Outline and Questions

I. What is chemistry?

-- see class notes

II. Basic properties of substances:

    A. physical property - property that can be observed without changing the substances present in the sample.

     Examples: color, physical state

    B. chemical property - the tendency to react and to form new substances; the identity of the substance will change when the property is demonstrated.

    Examples: explosiveness, flammability, rust

III. Reactions – see Handout on Types of Reactions

III. Kinds of Matter
     A. substances - either elements or compounds
    - cannot be separated into simpler substances by physical
      methods

    B. element - a (pure) substance which cannot be decomposed into simpler substances by chemical methods or physical methods
        1. atom - the smallest formula unit of an element; smallest unit of an element that enters into chemical combination

        (What is a formula unit?   the smallest unit of a substance that contains both the number and type of every atom indicated in the formula for that substance)
 

        2. symbols - one or two letters
          - first letter is always capitalized
          - see class notes for examples

    C. compound - a (pure) substance composed of 2 or more different elements which has a constant composition and which may not be broken down into
    simpler substances by physical methods; it may be broken down into elements by chemical methods

        1. molecule – particle containing 2 or more atoms that are strongly
                                        bonded together
                          - smallest formula unit of a compound
        2.  chemical formula - shorthand representation of a compound where:
            a. element symbols are used to represent types of atoms present
            b. subscripts written to the right of each element symbol are used to show the relative numbers of each atom
            c. examples:
                                  -- see class notes

    D. mixture - material composed of 2 or more substances which are present in variable composition; may be separated into simpler substances by physical
    methods; mixtures are not substances

IV. Types of Mixtures: homogeneous and heterogeneous mixtures (pages 11-12)

     A. heterogeneous mixture
        - composition is not uniform throughout the sample, changing from
           part of the sample to another part

        - often more than one state or phase of matter present

        - visible boundaries between the substances that make it up

        - Examples: see class notes

     B. homogeneous mixture
       - composition is uniform throughout sample

      - usually one state or phase of matter present

      - described as a solution, which may be gaseous, liquid, or solid

          1. solution has 2 components: solvent and solute

               a. solvent  - component into which the solute is dissolved

                - water is the solvent for aqueous systems

                b. solute  - solution component that is dissolved by the
                                  solvent

                - Example: NaCl dissolved in water

                          NaCl(aq)

          2. gaseous solution : air is an example

          3. liquid solution : aqueous NaCl is an example
             solute:
             solvent:

          4. solid solution : alloy is an example

                a. alloy - homogeneous solid mixture composed of 2 or more
                     metals or a metal combined with another substance

                 Examples:   steel

V. Basic overview of the periodic table (Sections 16.1 – 16.3)

     A.  atomic number - the number of protons in the nucleus of an atom
           - given the symbol  Z
           - determines element identity

     B.  atomic symbol - element symbol

    C. atomic mass - (basic definition) - the weighted average mass in atomic
                                                      mass units (abbr. amu) of one
                                                     atom of an element

    D. There are 3 basic types of elements: metals, nonmetals, and
                                                          metalloids

        1. metals - good conductors of heat and electricity
            - malleable
            - ductile

        2. nonmetals - not good conductors of heat and electricity
                            - brittle

        3. metalloids - semiconductors
                            - weak conductors of electricity

    E.  Location of elements on the periodic table:
              metals - left-hand side of table
        nonmetals - right-hand side of table
        metalloids - elements with atomic number 5, 14, 32, 33, 51, 52
        (found on either side of heavy line)

    F. The horizontal rows are called periods.

    G. The vertical columns are called groups or families.

    H. Elements are arranged in sequence across the rows in increasing atomic number and are grouped into families having similar chemical properties.

VI. Basic Properties of the Elements

    A. Properties of metals:

        1. good conductors of heat and electricity
        2. malleability (adj. malleable)
        3. ductility (adj. ductile)
        4.metallic luster (adj. lustrous) - shiny appearance
        5. usually solids at room temperature (except for mercury)

     B. Properties of nonmetals:
       1. Poor conductors of heat and electricity
           a. An important exception is graphite (a form of carbon)
                (1) allotropes - different forms of the same element
                              Examples for carbon:
                                        diamond - insulator
                                         graphite - good conductor of electricity

       2. Do not have lustrous appearance.
       3. Brittle (not malleable or ductile)
       4. May be gases, liquids, or solids at room temperature

    C. Metalloids - (or semimetals) - show some properties of metals and some properties of nonmetals

       1. Semiconductors - weak conductors of electricity - see notes

VII. Overview of Atomic Structure (see class notes; Text, 128-132)
    A. Bohr Model of the atom – advantages and disadvantages
     B. Quantum-mechanical model of the atom – advantages