Download Study Guide - seys

DRAFT Study Guide
for the 8th Grade Science Final
Format of the Final:
The Science Final is a comprehensive exam of this year's material. One-third of the content will come from the first half of the
year (Tests 1-4) and two-thirds of the content will come from the second half of the year (Tests 5-9). There will be a multiplechoice section that everyone will complete, and a short answer section where you will choose to complete 4 of the 5 sections.
Example topics from previous years are listed below. A reference sheet and periodic table will be included with the test
booklet on the day of the exam.
A. Multiple-Choice Questions (40% of Exam)
Read each question carefully. Ensure you refer to the tables, graphs or pictures, where appropriate. Select the best
answer for each question. DO NOT WRITE THE ANSWER IN THE MULTIPLE CHOICE BOOKLET. Put the
CAPITAL LETTER of the best answer in the space provided on this sheet BELOW. Make sure the number of the
question and page matches the information on this sheet. Check your answers before you hand in your exam.
B. "Pick 4 of 5" Questions (60% of Exam)
Review the 5 parts, labeled Part 1 through 5, on the top of each page. Pick four (4) of the five (5)
parts to complete. Complete ALL the questions for each of the four parts you pick. Do NOT
leave any questions blank. When you have completed the four parts, put a large "X" through each
page of the part you did NOT pick. EXTRA CREDIT: you may answer questions on this fifth part
that you put an X through. I will award up to 5 points total.
Sample Topics:
1.
Scientific Method & Measurement: hypothesis, evidence, qualitative vs. quantitative, objective vs.
subjective; how to perform calculations
2.
General Chemistry: Atoms and the Periodic Table
3.
Water Chemistry: properties of water; solubility; acids and bases; water contamination
4.
Speed vs. Acceleration: comparing D-T graphs and V-T graphs and calculating speed
Test Content to Review:
List of Tests to Review
Test #
Date
10-2-08
1
10-28-08
2
11-18-08
3
12-16-08
4
1-27-09
5
2-24-09
6
4-7-09
7
5-5-09
8
5-26-09
9
General Topics
Properties of Matter
Volume and Density
Composition of Matter
Periodic Table
Water and Chemical Bonding
Solutions and Chemical Equations
Solubility and Water Quality
pH
Motion and Forces
Sources for MOST (but not all) of the Short Answer and Multiple Choice Questions for the Exam:
 Old Quizzes
 SEPUP Homework
 McDougal-Littel Homework (usually the 6 questions at the end of each lesson)
 McDougal-Littel Chapter Review Questions
[*** Short Answer or MC questions may come VERBATIM from these sources OR be modified into a new order or format!]
Test #1: Properties of Matter
M&E Chapter 2-1: Matter has observable properties.
 Physical and Chemical Properties: definitions, examples, inferences
 Density and buoyancy
 Physical and Chemical Changes: definitions, examples, signs of, inferences
M&E Chapter 2-3: Properties are used to identify substances
 Density, solubility, magnetic properties, heating properties, conductivity
 Mixtures can be separated by using the properties of the substances they contain
SEPUP Chapters
 2: Types of Hazards
 3: A Plan to Separate the Mixture
 5: Separating the Mixture
 6: Identifying Liquids
Sample Questions:
 How should unidentified materials be handled?
 What are the risks associated with chemical hazards?
 How do we distinguish between physical and chemical properties?
 How can you separate the substances in a mixture?
 What’s the difference between a mixture and a compound?
 How can you use the characteristic properties to identify unknown substances?
 How can you tell when a substance is miscible? Corrosive?
 What are the elements of a scientific procedure?
 What are examples of physical properties? Chemical Properties?
 What are signs that a chemical change has taken place?
 What are signs that a physical change has taken place?
 What are the differences between mass and weight?
 How can we calculate density?
 What are some ways we can identify unknown substances?
Test #2: Mass, Volume, and Density
M&E Chapter 1-1: Matter has mass and volume.
 All objects are made of matter
 Mass is a measure of the amount of matter
 Volume is a measure of the space matter occupies
 Matter, Mass, Volume, Density = Definitions, Characteristics, Examples, Non-Examples
 Mass vs. Weight = know the distinction; how does they apply on other
M&E Chapter 1-2: Matter is made of atoms
 Atoms combine to form molecules
 Atoms and molecules are always in motion
Density Lab Skills:
 Memorize and use formulas for Density and Volume of rectangular solid
 Recognize and distinguish units for mass, volume & density
 Reading a meniscus, measuring displaced volume, reading a triple balance scale
SEPUP Chapters




7: Identifying Solids
8: Measuring Volume
9: Measuring Mass; Calculating Density
11: Choosing a Cleaner
Sample Questions:
 What are the differences between matter, mass, weight, and volume?
 How can we calculate density?
 How do we calculate displacement?
 How do we read a graduated cylinder?
 What are some ways we can identify unknown substances?
 How small is an atom?
 How do atoms combine to form molecules?
 How are atoms and molecules always in motion?
 What units of measurement do scientists use to collect data?
 How can we use the measurement-calculation method AND the water displacement method to find the volume of
object?
 What are the formulas for volume and density?
Test #3: Composition of Matter
ME 1.3: Matter combines to form different substances
 Matter can be pure or mixed
 Elements, compounds, mixtures, atoms, and molecules
 Comparing mixtures and compounds
 Parts of mixtures can be the same or different throughout (hetero/homogeneous)
CI Chapter 1-1: Atoms are the smallest form of elements.
 Models of atoms: Dalton, orbits & clouds
 Atomic particle: names, location, charge, mass
 Atomic numbers and atomic mass numbers
 Isotopes and ions: definitions, examples, inferences
SEPUP Chapters
 12: Evaluating Materials = which is the best material for making a drink container?
 13: Product Life Cycle = how can a life-cycle diagram be used to make a decision about a product
Sample Questions:
 What is the difference between a molecule and a compound?
 What is the difference between a heterogeneous and homogeneous mixture?
 What are the three parts of an atom and their charges?
 How is an ion formed?
 How has the atomic model changed over time?
 Draw a diagram of a Lithium ion.
 What is an isotope?
 What is atomic mass and how is it calculated?
 Why is a cloud used to explain how electrons exist in an atom?
Test #4: The Periodic Table
CI Chapter 1-2: Elements make up the periodic table
 The first 36 elements: atomic number, symbol, correct spelling
 Mendeleev’s Periodic Table: how organized?
 Periods and Groups: trends on the table
CI Chapter 1-3: The periodic table is a map of the elements.
 Metals, metalloids and nonmetals: position on table and general properties
 Reactive vs. non-reactive groups
 Specific Groups: Groups 1 (Alkali metals) and 2 (Alkaline metals), Group 17 (Halogens) and Group 18 (Nobel Gases)
 Specific Elements: know name and symbols of first 36 elements in Groups 1, 2, 13 – 18)
SEPUP Chapters:
 15: Families of Elements
 16: Elements and the Periodic Table
 17: Modeling Molecules
Sample Questions:
 What does a chemical formula show?
 How can you use the periodic table to determine the number of subatomic particles in an atom?
 How does density vary as you move across and down the periodic table?
 How does the size of atoms change as you move from left to right across the periodic table?
 How can you use the periodic table to order elements from least reactive to most reactive?
 What are the properties of metals vs. nonmetals?
 What are the properties of the families of elements?
Test #5: Water and Chemical Bonding
CI Chapter 2-1: Elements combine to form compounds.
 Distinction between elements and compounds; properties of each; same elements may form different compounds
 Reading chemical formulas: compound names, element names, number and ratio of atoms
CI Chapter 2-2: Chemical bonds hold compounds together.
 Chemical bonds between atoms involve electrons
 Ionic Bonds: result from electron transfer; reading superscript of ions; examples of ionic bonds; types of elements
forming ionic bonds; properties of ionic compounds (also found in 2-3)
 Covalent Bonds: result from electron sharing; examples of covalent bonds AND polar covalent bonds; types of
elements forming covalent bonds; properties of covalent compounds (also found in 2-3)
CI Chapter 2-3: Substances’ properties depend on their bonds.
 Metallic bonds: properties, examples
 Bonds can make same element look different: 3 forms of carbon
SEPUP Chapters
 30: Define the vocabulary of the three types of water we tasted
 31: Distinguish observations from scientific conclusions concerning Willow Grove’s water quality
 32-33: Identify and explain Dr. Snow’s hypothesis about the spread of cholera; the evidence Dr. Snow discovered; his
conclusions based on the evidence; the limitations of his evidence
 34: Identify and describe categories and sub-categories of water pollution; different ways contaminants enter water
sources and spread to other places
 35: Mystery Liquids
Sample Questions:
 What does the subscript indicate in a chemical formula?
 What are the three forms of carbon? How do they differ?
 How do we name ionic compounds? Give an example.
 How do ionic and covalent bonds differ?
 What is a property of a substance with metallic bonds?
 What parts of atoms are involved in bonding?
 What is the structure of a water molecule?
Test #6: Solutions and Chemical Reactions
CI Chapter 3-1: Chemical reactions alter arrangements of atoms.
 Atoms interact in chemical reactions; different from physical changes; evidence of chem. reactions
 Definitions of reactants and products
 Three types of chemical reactions
 Factors that affect the rate of chemical reaction: concentration, surface area, temperature, catalysts
CI Chapter 3-2: Balancing Chemical Reactions
 Types of chemical reactions
 Factors that affect the rate of a chemical reaction
 Function of a catalyst
 What happens during a chemical reaction/signs that a chemical reaction has occurred
CI Chapter 4-1: Solutions as a Type of Mixture
 Types of Solutions: 3 states of matter can be either the solvent OR solute
 Difference between ionic and covalent solutions
 How solutes affect the freezing and boiling points of solvents
SEPUP Chapters
 35: Comparison of Water & Ethanol in terms of shape of drop, density, melting point and boiling point; phase change
diagram
 36: Chemical formulas and structural diagrams of the 6 molecules we modeled in class; Comparison of Water &
Alcohols in terms of their molecules
 37: Identify solvents vs. solutes; How to separate solvents from solutes; color vs. clarity in solutions
Sample Questions:
 What are the signs that a chemical reaction has occurred?
 How do you know a reaction is balanced?
 How does polarity affect solubility?
 What are coefficients and subscripts?
 How does the addition of a solute affect boiling points and freezing points of solvents?
 What is a catalyst?
 Why is water called the “universal solvent?”
 What is the difference between a synthesis and a decomposition reaction?
Test #7: Solubility

CI Chapter 4.2: Degrees of concentration; solubility is affected by temperature and pressure; solubility is affected by
molecular structure
SEPUP Chapters
 38: Dissolving Duel: solubility of different solutes in water vs. ethanol
 39: Contaminants and Water Cycle: water cycle parts and processes; how contaminants may be picked up or left
behind
 40: Parts Per Million: converting ppm to %, fractions and ratios
 41: Testing Water Quality: potential health problems from readings that exceed Federal Water Quality Standards for
iron, copper, nitrate and pH
 43: Municipal Water Treatment: steps in water treatment
 44: Willow Grove Water Quality Report: interpreting data from water quality reports
Sample Questions:
 How can a solution be made more or less concentrated?
 What two factors affect solubility of a gas?
 Why doesn’t oil dissolve in water?

What does it mean if a solution is saturated?
Test #8: Acids and Bases
CI Chapter 4.3:
 Properties, structures and examples of acids and bases, acid and base strength, pH scale, neutralization
SEPUP Chapters:
 41: Testing Water Quality: potential health problems from readings that exceed Federal Water Quality Standards for
iron, copper, nitrate and pH
 44: Willow Grove Water Quality Report: interpreting data from water quality reports
 45: Precipitating Specific Contaminants
 47: Acids, Bases and the pH Scale: pH scale a measure of H+ ions; role of pH in environment and drinking water
 50: The Chemistry of Acids and Bases: the process of neutralization and chemical equations
Sample Questions:
 What are the properties of acids and bases?
 What is a neutral pH?
 What does pH actually measure?
 How can a solution be neutralized?
 What are various methods of removing contaminants from water?
 Write the basic reaction for acid-base neutralization
 What is the difference between a strong acid and a weak acid?
Test #9: Motion and Forces
M&F Chapters 1.1 and 1.2
 1.1: an object in motion changes position; motion is relative and depends on a reference point
 1.2: speed measures how fast position changes; calculating speed; average speed; distance-time graphs; velocity
includes speed and direction
SEPUP Chapters
 73: Choosing a Safe Vehicle: What features of vehicles affect safety? (e.g. maximum speed, breaking speed, length,
width, height)
 74: Measuring Speed: Designing an experiment to calculate speed; calculating speed using the distance time formula;
advantages to the number of occurrences, trials and averaging; graphing; limitations of the lab
 75: Interpreting Motion Graphs: how to use a graph to describe motion; distance-time graphs; acceleration
Sample Questions:
 What is the purpose of a reference point?
 How can we calculate speed?
 What is the difference between speed and velocity?
 Describe a situation where an object has changing velocity but constant speed.
 What is the difference between average speed and instantaneous speed?
 Why is velocity a vector quantity?
 How do you know that an object is in motion?
 What is relative motion?
 How does apparent motion depend on the observer’s motion?
 How can a distance vs. time graph be used to determine the speed of an object?
 What are the differences between distance-time graphs and velocity-time graphs?