|
- Exam Topics by Subject and Nine-Week Period
- Allied Health I Semester Exam Study Guide
- Chemistry Review Questions by Nine-Week Period
- Chemistry Third and Fourth Nine-Weeks Semester Exam Topics May 2004
- Physics Fourth Nine-Week Topics
Exam Topics by Subject and Nine-Week Period First Nine-Week Exam Topics
Allied Health I
History of Healthcare
Career Ladder in Healthcare
Tenets of Hippocratic Oath
Current Trends in Healthcare
Future of Healthcare
Patient's Bill of Rights
Client versus Patient
Interpersonal Dynamics
Conflict Resolution Model
Characteristics of the Healthcare Worker
Values/Attitudes/Behavior
Hierarchy of Needs
Communication: Verbal and Nonverbal
Model for Problem Solving and Decision Making
Assertive versus Aggressive Behavior
Guidelines for Good Listening Skills
Legal and Ethical Principles
Code of Ethics
Malpractice and Liability
Confidentiality
Client Rights
Documentation
Allied Health II
Chemistry
Physics
First Nine-Week Exam Topics
1. Safety in the Physics Lab
2. Dimensional Analysis using conversion factors
3. Scientific Notation
4. Significance
5. Accuracy versus Precision
6. Independent Variable versus Dependent Variable
7. Hypothesis – define and apply
8. Vector Quantities versus Scalar Quantities
9. Newton's Three Laws of Motion – define and apply:
1st Law
2nd Law
3rd Law
10.Define, know labels, and use in equations:
Velocity
Acceleration
Displacement
Time
Density
Free Fall
Force
Mass
Gravity
11. Make and interpret Distance-Time, Velocity-Time, and
Acceleration-Time Graphs
12. Discuss Egg Drop Project and results
Second Nine-week Exam Topics
Allied Health I
Allied Health II
Chemistry
Physics
Third Nine-Week Exam Topics
Chemistry
Nine-Week Exam Components:
Cations and Anions
Types of Compounds
Compound Formation using Charges
Naming Compounds
Types of Reactions
Predicting Products
Balancing Chemical Equations
The Mole
Mole Equivalencies
Mole Conversions: single step and multistep
Stoichiometry: mole to mole and mass to mass calculations
Internship
Small Business Terminology
What is a small business?
How is it structured?
What technology (hardware and software) is used to manage the
business and
pay its employees?
What responsibilities and benefits must a small business provide
its employees?
What licenses and fees are needed to open/run a small business?
What laws regulate small businesses?
How can an individual obtain a small business loan from a
bank? ...from the
federal government?
How do the tax laws apply to small businesses?
How can you apply what you have learned to the business at which
you are
interning?
Allied Health II Medical Terminology
Nine-Week Exam Components for Cardiovascular, Lymphatic,
Digestive, and Eye
Systems:
I. Word Parts and Terms
II. New Terms
III. Abbreviations
IV. Review Exercises
Physics
Fourth Nine-Week Exam Topics
Allied Health I
Seeking a Healthcare Career
Laboratory Science Careers
Imaging Careers
Medical Careers
Nursing Careers
Dental Careers
Veterinary Medicine Careers
Rehabilitation Careers
Social Science Careers
Emergency Medicine Careers
Hospital Administration Careers
Chemistry
Thermochemistry
Gas Laws
Solutions
Molarity
Acid-Base Theory and Neutralization
Titration
Gibbs Law
Redox Reactions
Interns
Based on Intern Experience and Nine-Week Report
Allied Health II Medical Terminology
The Nervous System
The Endocrine System
Female Reproductive System
Male Reproductive System
Obstetrics and Neonatology
For each preceding system, the following will be covered:
I. Word Parts and Terms
II. New Terms
III. Abbreviations
IV. Review Exercises
Physics
Static Electricity Coulomb's Law F = kq'q/d-squared
k = proportionality constant 9.0 x 10^9
N.msqd/Csqd
Induction versus Conduction
Electric Fields E = f/q' V = Ed W= = qV P=W/t
= qV/t
F = mg & F = q'E QED mg = q'E
Capacitance C = q/V
Electric Currents Electric current is the rate of flow of
electric charge.
1 A = 1 C/s
P = VI p = power V = voltage I = current
V = IR so P = IRI = I^2 R
Q (thermal energy) = I^2Rt (power through
time)
Ohm's Law R = V/I R label ohms (omega sign)
resistance varies directly with voltage
(potential
difference) and indirectly with the current
Series v. Parallel Circuits
Ammeter measures current; goes in series
Voltmeter measures voltage (potential); goes
in parallel
Potentiometer (aka, variable resistor or
rheostat
Series and Parallel Circuitry
V = V.1 + V.2 + V.3 +....+ V.n = IR + IR + IR
+ IR...
Series R = R.1 + R.2 + R.3 + ....
Parallel 1/R1 + 1/R.2 + 1/R.3 + ...
Magnetic Fields
General Properties of Magnets
Left-handed Rules (three)
Domain
Magnetic Induction
Strength of Magnetic Field, B B = F / IL (L=length
of wire)
unit is the tesla, T which if Newton/Ampere times
meter
Force of magnetic field F = BqV
Electromagnetic Induction
Faraday said that if an electric current can induce a
magnetic
field
then a magnetic field should be able to induce a
current.
EMF = BLv (B mag field strength; L length of wire; v
velocity of
wire in the field)
Allied Health I Semester Exam Study Guide What is the healthcare career ladder? How is it structured?
Why is it called a ladder? What is the purpose of a career
ladder?
Know the career ladder for each of the healthcare clusters. For
instance:
What is the career ladder of the nursing healthcare cluster,
starting with
the professional level?
What basic educational levels do each of the following have to
have
regardless
of the healthcare cluster? Professional, Technologist,
Technician,
Assistant, Aide
For instance:
In general, what is the education requirement for technicians
regardless of
the healthcare cluster?
Compare the educational requirements of the laboratory
technologist with
hose
of the laboratory technician.
How do the educational requirements and the duties of the
psychiatrist
differ
from those of the psychologist?
Know the duties of each level of the healthcare career ladder for
each of
the
clusters. For instance:
Compare and contrast the personal characteristics and skills of
the
laboratory healthcare worker with those of the imaging healthcare
worker.
How are the duties of the licensed practical nurse different from
those of
the nurse assistant?
Which medical health care worker performs both clerical and
clinical
functions under the supervision of the physician?
Compare and contrast the responsibilities of the medical doctor
with the
physician assistant.
How are the responsiblilies of the the dental hygienist different
from those
of the dental assistant?
What is credentialing? What are the levels of credentialing?
For instance:
What is the educational path and credentialing of the individual
wishing to
be a medical doctor?
What credentialing is necessary to become a veterinarian?
What areas of specialization are available to:
Medical Doctor
Registered Nurse
Veterinarian
Therapists
What are some advantages and disadvantages of being an animal
heathcare
worker?
What physical characterisitcs and skills must the animal
healthcare worker
possess?
What one characteristic is considered most important to all
healthcare
workers,regardless of the cluster or the level within a health
care ladder?
Why?
What are the essential components of a good resume? What skills
and
experience do think would be especially good to include in a
resume when
applying for a healthcare position?
Review the problem-solving model. Be prepared to analyze
different
healthcare-related scenarios using the problem-solving model.
Be prepared to write a one-page essay on your career choice. Be
able to
describe the career in general terms, state educational
requirements,
duties,
responsibilities, credentialing, advantages/disadvantages, costs
involved,
salary levels, and any other topics specific to your career
choice.
Chemistry Review Questions by Nine-Week Period First Semester Exam (covers first and second nine-week periods)
1. What is the scientific method?
Why do scientists use the scientific method?
2. How is a law different from a theory?
3. What is the difference between a hypothesis and an
experiment?
4. What is matter? What is a substance?
5. How is a chemical property different from a physical
property?
State examples of each.
6. What is the difference between an element and a compound?
7. Distinguish between a gas, a liquid, and a solid. Which
of these
states of matter has more energy?
8. What is energy? What are the forms of energy?
How are they different from each other?
9. How is potential energy different from kinetic energy?
10. Explain the Law of the Conservation of Energy and the Law
of the
Conservation of Mass.
11. Describe distillation. What is its function?
12. Describe a chemical reaction.
13. During a chemical reaction, how is the mass affected?
14. Distinguish between a heterogeneous and a homogeneous
mixture.
Give examples of each.
15. Distinguish between accuracy and precision.
16. State the rules for determining how many significant
digits are in a
measurement.
17. Practice the problems in the text dealing with significant
digit
determination.
18. Practice the problems in the text dealing with adding,
subtracting,
multiplying, and dividing significant digits.
19. What are the SI units? State each and the labels
associated with
each.
20. How is mass different from weight?
21. Practice problems converting between units, such as:
kg > g > mg, mg > g > kg, L > mL, mL > L
22. What is the difference between temperature and heat?
23. What are the units for temperature? What are the units
for heat?
24. How do you convert between Celsius and Kelvins?
25. How do you convert between calories and Joules?
26. Define density and state its formula.
27. How is density affected when mass is increased and volume
remains the
same?
28. How is density affected when volume is increased and mass
remains the
same?
29. Practice problems in the text dealing with density where
you find
(a) density given mass and volume,
(b) mass given density and volume, and
(c) volume given mass and density.
30. What is a conversion factor? Why is it used?
31. What is dimensional analysis? To what does the term
dimensional
refer?
32. Practice dimensional analysis problems from the text.
33. State the principles of Daltons Law.
34. Which of these are now considered incorrect and state why.
35. What is atomic number?
36. What is mass number?
37. How can mass number be used to calculate the number of
protons or the
number of neutrons?
38. What is an isotope of an element?
39. What is atomic mass? Why is it not a whole number?
40. Explain the difference between a family and a period on a
periodic
table.
41. What does the number at the top of a column on a periodic
table
represent?
42. What does a period on a periodic table represent?
43. What is the difference between a representative element, a
transition
element, and an inner transition element?
44. Where are the metals on the periodic table? Where are the
nonmetals?
How do the physical properties of metals different from
nonmetals?
45. Where are the alkali metals? Where are the alkaline earth
metals?
Where are the halogens? Where are the inert or noble
gases?
46. What is an ion? What is the difference between a cation
and an anion?
47. How does a neutral atom become a cation? How does a
neutral atom
become an anion?
48. Where are cations located on the periodic table? Where
are anions
located on the periodic table?
49. What is a polyatomic ion?
50. Write the symbols with the charge for each of the
following
polyatomic
ions:
ammonium ion
hydroxide ion
nitrate ion
carbonate ion
sulfate ion
phosphate ion
51. How is an ionic compound different from a molecular
compound? How
are
electrons bonded in each type of compound?
52. Why do you use prefixes in molecular compounds but not in
ionic
compounds? What are the names of the prefixes from 1
through 10?
(See p. 105 in text if you cannot name these.)
53. Why can you not use charges to form molecular compounds?
54. How do you name ionic compounds? Name NaCl, Al(OH)3
55. How do you name molecular compounds? Name P2O5.
56. How do you name the two types of acids (binary and
polyatomic)?
Name HCl. Name H2SO4.
57. What does a subscript represent in a compound?
58. What is the mole?
59. What is the purpose of the mole?
60. What is molar mass?
61. State the three quantities the mole can be equivalent to.
62. Practice problems converting between the mole and
representative
particles, between the mole and mass, and between the mole
and volume.
63. Practice problems converting between particles and mass,
particles
and
volume, and mass and volume.
64. What does percent composition mean?
65. What is the percent composition of sodium in sodium
chloride?
66. What are the five types of reactions? State the
definition of each
and give three examples of each type.
67. What does it mean to balance a reaction? What law demands
that a
reaction be balanced?
68. What is a coefficient used for?
69. Practice identifying reactions by type using the reactions
in the
text.
70. Practice balancing reactions using the reactions in the
text.
Chemistry Exam Review Third Nine-Week Topics
Forming and Naming Compounds
To use ions to form compounds and name those compounds according
to type.
Reactions
To use the five reaction types to predict products and balance
each reaction
to satisfy the law of the conservation of matter.
The Mole
To use the mole concept to convert between the units of
particles, mass,
and volume.
Stoichiometry
To apply stoichiometric calculations to reactions to obtain
quantitative
data to support scientific conclusions.
Note: Use the Worksheets in this section to practice mole
conversions and
stoichiometric calculations
Chemistry Exam Review Fourth Nine-Week Topics
Content: 25% third nine-week topics; 75% fourth nine-week
topics.
Heat in Chemical Reactions
What is an exothermic reaction?
Why do almost all chemical reactions involve changes in energy?
On which side of a chemical equation does the energy term appear
in an
exothermic reaction? Endothermic reaction?
Is cloud formation an exothermic or endothermic process?
What information is provided by the enthalpy change, DH, of a
reaction?
Explain the significance of the sign of the enthalpy change for a
reaction.
Why is the DH for a reaction proportional to the quantity of
reactants?
How is Hess law used to find DH for a reaction?
Identify the following as exothermic or endothermic: Br2 (s) -->
Br2 (l) &
Br2 (g) --> Br2 (l)
Behavior of Gases
State the postulates of the kinetic-molecular theory of gases.
List five properties of gases.
How does the kinetic-molecular theory account for gas pressure?
What are the four gas variables?
Define STP for gases.
State and describe the following laws: Boyles, Charles, Gay-
Lussacs.
Show how the following three gas laws are all represented in the
combined
gas
law.
State and describe Daltons Law of Partial Pressures.
How does the kinetic-molecular theory account for Boyles Law,
Charles Law,
and Gay-Lussacs Law?
State and describe the units in the Ideal Gas Law.
Why must Kelvins be used in gas law problems instead of degrees
Celsius?
Which assumptions of the kinetic-molecular theory are not valid
with real
gases?
How is the density of a gas related to its temperature?
How can a balloon get life in air?
Solutions
What is a solution?
Describe its properties.
What are the two components of a solution? How can you
differentiate
between
them?
Describe molarity and state its formula.
What is a saturated solution? An unsaturated solution? A
supersaturated
solution?
What is solubility?
How does a solution form? What role does energy play in this
process?
List and describe three factors that affect the solubility of a
substance.
Explain how the rate at which a solute dissolves can be increased.
In terms of the kinetic-molecular theory, explain why the
solubility of a
gas
in a liquid generally decreases with an increase in temperature.
Acids, Bases, and Salts
State the Arrhenius definitions of an acid and a base.
What is a neutralization reaction? In addition, give two
examples.
What are the Bronsted-Lowry definitions of an acid and a base?
What are conjugate acids and conjugate bases according to
Bronsted-Lowry?
How is Arrhenius theory different from Bronsted-Lowrys theory?
What are Lewis definitions of an acid & base?* *See Ch 18 of
the Addison-
Wesley textbook.
What does the acid dissociation constant indicate about an acid?
What does
the base dissociation constant indicate about a base?
What is an acidic hydrogen?
What structural similarity do Bronsted-Lowry bases have in common?
Reactions of Acids and Bases
What is the pH scale?
What does this scale measure?
What is the pH of a solution that has an [H+] = 1.0 x 10-8 ?
What is the [OH-] of a solution if its [H+] = 1.0 x 10-8 ?
What is the pOH of a solution if it has a pH of 2.0?
How can titration be used to determine the concentration of a
base?
How can the normality of an acid or a base be determined using
the
solutions
molarity?
Redox
Define oxidation and reduction.
What happens during oxidation and reduction?
Where in the periodic table do you think strong oxidizing agents
are found?
Reducing agents?
Which reaction types undergo redox?
Determine oxidation numbers;which substance(s) are reduced;which
are
oxidized;write half-reactions; balance using electrons;state
which substance
is the oxidizing agent and which is the reducing agent.
Can an element undergo oxidation as well as reduction in the same
reaction?
Use a reaction to demonstrate your point.
Thermodynamics
How is a spontaneous reaction different from a nonspontaneous
reaction?
What two concerns are addressed by thermodynamics?
Can enthalpy alone be an indicator of spontaneity of a reaction?
How do you determine enthalpy of a reaction?
What happens to the sign of DH when a chemical equation of a
reaction is
reversed?
Give two examples of exothermic reactions that are not
spontaneous.
What is entropy?
Explain how the entropy change of the surroundings is related to
the
enthalpy
change of a reaction?
What is Gibbs free energy equation?
State and describe the signs of delta G for a spontaneous
reaction and for a
nonspontaneous reaction.
What is happening when delta G equals zero?
Is a reaction spontaneous or nonspontaneous if it is endothermic
and
experiencing a decrease in entropy? Explain your choice.
Law of Conservation of Energy: Energy can be neither created nor
destroyed. If so, why do conservationists want us to conserve
energy.
Note: Use the Categories marked with a star on this webpage to go
to review material for each of the topics for this nine
weeks.
Chemistry Third and Fourth Nine-Weeks Semester Exam Topics May 2004 Chemistry Topics
Spring Semester Exam 2004
Semester Exam questions include material from:
25% of third nine-weeks topics and
75% of fourth nine-weeks topics
Third Nine-Week Topics
Reactions 5 types, predicting, balancing
Stoichiometry
Moles, Mass, Volume, Particles
Percent Yield
Limiting Reagent
Exothermic & Endothermic Reactions
Heat of Reaction
Fourth Nine-Week Topics
Solutions and Concentration
Molarity
Dilutions
Colligative Properties
molality
Reversible Reactions & Chemical Equilibrium
LeChateliers Principle
Acid-Base Chemistry
Properties
pH
Acid-Base Theories Arrhenius, Bronsted-Lowry, and Lewis
Strong versus Weak Acids and Bases
Titration
Normality
Reduction-Oxidation Reactions (Redox)
Gas Laws Combined & Ideal
Phase Change
Nuclear Reactions alpha rx, beta rx
Physics Fourth Nine-Week Topics Physics
Static Electricity Coulomb's Law F = kq'q/d-squared
k = proportionality constant 9.0 x 10^9
N.msqd/Csqd
Induction versus Conduction
Electric Fields E = f/q' V = Ed W= = qV P=W/t
= qV/t
F = mg & F = q'E QED mg = q'E
Capacitance C = q/V
Electric Currents Electric current is the rate of flow of
electric charge.
1 A = 1 C/s
P = VI p = power V = voltage I = current
V = IR so P = IRI = I^2 R
Q (thermal energy) = I^2Rt (power through
time)
Ohm's Law R = V/I R label ohms (omega sign)
resistance varies directly with voltage
(potential
difference) and indirectly with the current
Series v. Parallel Circuits
Ammeter measures current; goes in series
Voltmeter measures voltage (potential); goes
in parallel
Potentiometer (aka, variable resistor or
rheostat
Series and Parallel Circuitry
V = V.1 + V.2 + V.3 +....+ V.n = IR + IR + IR
+ IR...
Series R = R.1 + R.2 + R.3 + ....
Parallel 1/R1 + 1/R.2 + 1/R.3 + ...
Magnetic Fields
General Properties of Magnets
Left-handed Rules (three)
Domain
Magnetic Induction
Strength of Magnetic Field, B B = F / IL (L=length
of wire)
unit is the tesla, T which if Newton/Ampere times
meter
Force of magnetic field F = BqV
Electromagnetic Induction
Faraday said that if an electric current can induce a
magnetic
field
then a magnetic field should be able to induce a
current.
EMF = BLv (B mag field strength; L length of wire; v
velocity of
wire in the field)
| |
