GEOPHYSICAL SCIENCE
Mid-Term Exam Review Outline
(c:Mid-TermEevSumGEOPHYSICALSCIENCE)
Directions:
 You may bring a 3”x 5” note-card to the exam. The note-card may contain
any notes/information you want to include. You will be provided with a
Periodic Table.
 Format of exam… ~ 125-135 multiple choice questions. Questions are
designed for knowledge of facts and for application of factual knowledge
through analysis of information, problems and scenarios.
USE YOUR TEXTBOOK CHAPTER SUMMARY AND “STANDARDIZED TEST PREP”
AT THE END OF EACH CHAPTER AS A SOURCE OF ASKING YOURSELF
QUESTIONS ABOUT THE THINGS YOU NEED TO KNOW.
Included “labs”- “copter” investigation; Plastics-polymer investigation, Graphing trends
in periodic table’; Web site evaluation
Review Topics: Refer to class textbook ( hint.. refer to “Section summaries”)
and to Handouts from class.
 Chapter 1 Science (Sections 1-1, 1-2, 1-3) …”
o What is Science?
 Branches of science
 Relationship of Science and technology
 Scientific laws
 Scientific theories..DEFINITONS…
 Models
o The Way Science Works
 Scientific Method
 Hypothesis; If, … , then…, because…
 Variables: Independent, dependent, constants, control setup;
 Units of Measurement; S. I. (metric-prefixes e.g. milli- etc.,
base units, mass, distance, volume, conversions.
o Organizing Data.
 Using graphs
 Bar versus line
 Scientific Notation
 Chapter 2 Matter ( Sections 2-1, 2-2, 2-3)
o What is matter?
 Describe the relationship between matte, atoms and elements.
 Describe the structure of Atoms
 What are and how are molecules formed.
 What are compounds? How alike / different from molecules?
 Write chemical formulas for common compounds.
 Distinguish between pure substances and mixtures.
o What are the Properties of Matter
 Physical properties?
 Phase changes? Or change of “state”
 Chemical properties?
 What is density?
o Changes of Matter
 Explain physical change..
 Explain chemical change…
 Mixtures compared to pure substances
 Detecting chemical changes
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Chapter 3 –States of Matter ( Sections 3-1,3- 2, 3-3)
o Matter and energy..
 What is the kinetic theory of matter?
 How does temperature relate to kinetic energy.
 What are the changes of state?
 What are the 4 states of matter?
 What is the behavior of molecules in each state?
 What are the shape and volume characteristics of each state of
matter?
 Temperature change versus change of state.
 What are the names of the processes at each change of state?
 Vaporization, condensation etc.
 Law of conservation of mass and energy.
o Characteristics of Fluids
 Buoyant force
 Pressure exerted by fluids
 Archimedes’s Principle
 Floating as a function of density
 Fluids and pressure
o Relationship of pressure, force and surface area.
P=f/a
o Pascal as a unit of pressure
o What is Pascal’s Principle?
o Behavior of Gases
 Properties of gases
 Pressure of gases on their containers
 Gas Laws… relating pressure volume and temperature.
 Boyles Law… formula?
 Charles Law… formula?
o Formulas of laws to guide thinking.
 …Cartesian Diver investigation… eye dropper/ wire/ water..
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Chapter 4- Atoms and the Periodic Table ( Sec 4-1, 4-2, 4-3 only) (not 4-4)
o Atomic Structure
 Progression of our understanding of knowledge of Atomic
structure..
 Democritus, Dalton, Bohr models of atom
 Nucleus – protons and neutrons.
 Energy levels – orbits electrons
 Charge of particles … electrons, protons and neutrons.
 Organization of the Periodic Table
 Periodic law, periodic function
 Period, Group
o Families –Groups(Columns)
o Period- rows
o Ion formation ..gaining or losing electrons.
o A.P.E
o Symbol of elements, atomic number, mass
number, average mass, isotopes
 Families of Elements
o Characteristics of metals, transition metals,
non-metals, noble gases
Chapter 5- The Structure of Matter (Section 5-1, 5-2, 5-3)
o Compounds and Molecules
 What is a compound? What is a molecule?
 How does the formula of a compound relate to the number of
atoms or ions present in a compound?
o Ionic and Covalent Bonding
 Why do atoms join to form bonds? Stability?
 What is an ionic bond? What is a covalent bond?
 Why do some atoms transfer while others share electrons?
 What is a metallic bond?
 What effect does the type of bond have on the properties of the
compound such as melting point or conductivity?
 What are Polyatomic ions?
 What are anions and cations?
o Compound Formulas and names.
 Write a formula for an ionic compound? Ex NaCl
 Write a formula for an ionic compound using
polyatomic ions. Ex CaCO3
 Write a formula for a covalent compound ex CH4
 Name ionic
Ex Sodium Chloride ( NaCl; Calcium Chloride CaCl2
and covalent compounds
glucose (C6H12O6)
 Differentiate between a molecular formula and a structural
formula.
H
CH4
H-C-H
H
o Organic and Biochemical Compounds
 Organic chemistry… the element carbon
 What are organic compounds?
 How many bonds can carbon form
 What are monomers and polymers?
 What are the polymers essential to life? Examples
 Hydrocarbons? Fuels…
o Propane ( C3H8 ), propene (C3H6) , propyne
(C3H4)..single, double, triple bonds.
 Alcohols. OH group ethanol
 Carbohydrates? Glucose, starch
 Proteins? Amino Acids?
 Nucleic Acids? Nucleotides? DNA polymer

Chapter 6 – The Nature of Chemical Reactions
o Nature of Chemical Reactions
 Signs of chemical reactions occurring..
 Reactants-- Products new substance produced..
 Energy absorbed or released.. endothermic/exothermic
 Matter and energy conserved.
o Reaction Types
 Synthesis
 Decomposition
 Single Replacement (Single exchange)
 Double Replacement (Double exhancge)
 Oxidation/Reduction Reactions
 Combustion reactions
o Balancing Chemical Equations
 Chemical equations
 Conservation of mass
 Balance using coefficients to cause mass balance in reactants
and products.
o Rates of change in Chemical Reactions
 Factors Affecting Reactions Rates
 Nature of substances
 Surface area of substances; greater SA, faster reaction
 Temperature of substances/environment; higher temp
faster reaction.
 Concentration of substances; Higher Concentration,
usually faster reaction; higher pressure, faster reaction
 Presence of catalysts; reduce activation energy
required and speed up reactions. Presence of inhibitors
slow down reactions.
 Chemical equilibrium… reaction occurring at same rate in both
directions… dynamic i.e. continually changes maintaining
“balance”