Physical Science Assignment-Test Schedule 2008-2009
NOTE:  Labs:  for all lab activities--answer all questions in the lab.  Include all appropriate data collected and conclusions as well.

NOTE:  PLEASE PUT SEPARATE ASSIGNMENTS ON SEPARATE SHEETS OF FULL SIZED NOTEBOOK PAPER.

NOTE: SPIRAL NOTEBOOK PAPER NOT ACCEPTED FOR ANY WORK TURNED IN.

 
Aug 1-8   School Meetings & Registration
   

Writing a Laboratory Report must include the following:
-NOTE: Please always use this pattern for all lab reports.

a) Title,

b) Purpose (indicating why you are doing the lab),

c) Hypothesis (an educated guess as to what will occur during the lab),

d) Materials & Equipment (just the actual items used -- not necessarily the ones listed in the lab itself),

e) Procedure (an accurate, concise description of steps needed to complete the lab work),

f) Data (information collected during a lab, often organized into a data table), and

g) Conclusions (reasoning as to why things happened the way they did during the lab).

     
Aug 11 Mon -School begins
-1st Day information from website
-Laboratory Safety Agreement
-p.839-840 "Lab Skills"
-p.841 "How to Write a Laboratory Report"
-Begin Ch 1 p.4-11 (Sect 1)
-p.11 #1-7 Check off in class

-Take home and have your parent(s) sign lab safety agreement (NOTE: This is a 10 point assignment)

Aug 12 Tues Same as Monday
Aug 13 Wed -Quiz over p.4-11 (10pts)
-Collect Lab Safety agreement signed by parent
-Ch 1 p.12-19 (Section 2)
-p.17 #1-8 (do in class if time permits)
-p.19 #1-5 Check off in class
Aug 14 Thur Same as Wednesday
Aug 15 Fri -Quiz over information given previous period
-p.32-35 Skills Practice Lab
-p.35 #1-6 (Analysis and Conclusions)
Aug 18 Mon

Picture Day/Class Meetings

Aug 19 Tues -Ch 1 p.20-27 (Section 3)
-p.26 #1-7 Check off in class
-p.23 Practice #1,2 Check off in class
-p.24 Practice #1,2 Check off in class
-p.25 Practice #1-4 Check off in class
Aug 20 Wed Same as Tuesday
Aug 21 Thur -Review Ch 1
-p.28 #1-15
-p.29 #22-27

NOTE: THE MOST IMPORTANT THING YOU CAN DO TO PREPARE FOR TESTS IS TO KNOW THE FOLLOWING REVIEW SHEET!!! ALSO 2PTS EXTRA CREDIT WILL BE GIVEN FOR PRINTING OUT THE REVIEW SHEET AND TURNING IT IN AT THE BEGINNING OF THE TEST (NOT ACCEPTED AFTER THE TEST).

-Chapter 1 Review Physical Science Holt Spectrum
-read the chapter carefully
-know objectives for all sections within the chapter
-know all the key terms
-study the summaries located at the end of each section
-study the summaries at the end of each section
-know figure 3 (p.6)
-know the two main branches of science (natural & social)
-the three main branches of natural science are a) life (biological), b) physical & c) earth
-a scientific model is a representation of a real event or object
-the scientific method is a logical series of steps used to solve problems
-making an observation is the usual first step in the scientific method
-scientists test hypotheses by doing experiments
-the SI unit for length is the meter, for mass the kilogram, for time the second, for temperature Kelvin, for electric current the ampere, for amount of substance the mole, for luminous intensity the candela
-deci = 0.1, tenth, centi = 0.01, hundredth, milli = 0.001, thousandth, micro = 0.000 001, millionth, nano = billionth, 0.000 000 001
-be able to convert from centimeters to meters and back
-be able to convert from grams to kilograms and back
-know 10 to the minus 1,2,3,6,9, etc & 10 to the positive (scientific notation)
-be able to determine the number of significant figures in a calculation
-precise measurements and accurate measurements (know the difference)
-pure science continues the search for new knowledge
-in pure science, scientists do experiments to find out about the world
-p.8 know the three tests a scientific theory must pass (explain observations clearly and consistently, experiments that illustrate the theory must be repeatable, you must be able to predict from the theory)
-A scientific theory is an explanation that has been tested by many observations.
-scientific theories must be replaced when new discoveries are made
-scientists use computer models to make predictions
-know figure 12 (p.13) the scientific method is a series of logical steps used to solve a problem
-no experiment is a failure because all experiments are observations of real events.
-know Table 1,2 & 3 on p.16
-weight is a measure of gravitational pull
-be able to interpret pie, line and bar graphs (p.21,22)
-be able to convert to (or from) scientific notation
-know the difference between precision and accuracy p.24,25 (An accurate measurement is close to the true value. A precise measurement is one that is as exact as possible)
Aug 22 Fri Same as Thursday
Aug 25 Mon -Test Ch 1
-Read Chapter 2 (section 1)
-Focus Activity p.37 #1,2
-Define Vocabulary Ch 2 (16 terms total) NOTE: Please # all vocabulary
Aug 26 Tues Same as Monday
Aug 27 Wed -Correct Ch 1 Test for first 25 minutes
-Begin Ch 2 p.38-44
-p.44 #1-8
-read p.45-52 Section 2-2
-Study for a Quiz over today's information for next period
Aug 28 Thur Same as Wednesday
Aug 29 Fri -Quiz over p.38-44 (over the information specified in class last period)
Sept 1 Mon No School -- Labor Day
Sept 2 Tues -Ch 2 (section 2) p.45-52
-p.52 #1-7
-p.49 Quick Lab "Mass & Volume Relationships"
-read p.53-58 section 2-3
Sept 3 Wed Same as Tuesday
Sept 4 Thur -Ch 2 (section 3) p.53-58
-p.58 #1-8
-p.54 Quick Lab "How can physical properties separate a mixture?"
Sept 5 Fri Same as Thursday
Sept 8 Mon -Review Ch 2
-p.60 #1-28

- Chapter 2 Review Physical Science Holt Spectrum
-read the chapter carefully
-know objectives for all sections within the chapter
-know all the key terms
-study the summaries located at the end of each section
-study the summaries at the end of each section
-chemistry is the science of what matter is made of and how it changes
-be able to work density problems D = m/v, m = DV, V = m/D
-elements are substances that cannot be broken down into simpler substances
-molecules are the smallest unit of a substance that behaves like the substance
-in order to make water from hydrogen and oxygen 2 hydrogens and one oxygen must combine chemically
-by looking at a chemical formula, be able to determine how many atoms of each element are present (H20)
-pure substances can be represented by a chemical formula
-a carbonated drink is an example of a gas-liquid mixture
-chemical properties indicate how a substance will react with other substances
-matter is anything that has mass and takes up space
-know Fig 3 Iron is the most abundant element in the earth,
-oxygen is the most abundant element in the human body
-salt and water form a homogeneous mixture
-be able to look at a formula and indicate the # and identity of each atom
-pure substances can be represented by chemical formulas
-carbon dioxide can dissolve in water to form a gas-liquid mixture
-a chemical property of matter is reactivity
-physical properties of matter (freezing point, boiling point, density)
-grinding a material is an example of physical change (grilling a burger is a chemical change)
-when water is broken down, oxygen and hydrogen gas form
-know the indications that the chemical change has taken place (release of a gas, change in color, production of a gas, formation of a precipitate)
-the boiling point is when a liquid changes rapidly into a gas
Sept 9 Tues Same as Monday
Sept 10 Wed -Test Ch 2
-Read Chapter 3
-Write out all chapter 3 definitions, please # all terms
-Pre-Reading Questions p.69 #1,2
-Read p.70-79
Sept 11 Thur Same as Wednesday
Sept 12 Fri Video #1 "The World of Chemistry"
(take notes--numbered, point form--about 15 ideas from the video)
Sept 15 Mon p.64-65 Skills Practice Lab "Testing the Conservation of Mass"
-p.65 #1-4 (analysis and conclusion)
-Do a complete lab write-up (using the format on -p.841 "How to Write a Laboratory Report"

-Writing a Laboratory Report must include the following:
-NOTE: Please always use this pattern for all lab reports.

a) Title,

b) Purpose (indicating why you are doing the lab),

c) Hypothesis (an educated guess as to what will occur during the lab),

d) Materials & Equipment (just the actual items used -- not necessarily the ones listed in the lab itself),

e) Procedure (an accurate, concise description of steps needed to complete the lab work),

f) Data (information collected during a lab, often organized into a data table), and

g) Conclusions (reasoning as to why things happened the way they did during the lab).

Sept 16 Tues Same as Monday
Sept 17 Wed -Begin Ch 3 p.70-79 (section 1)
-Vanilla balloon demo
-Read p.80-86
-p.80 Write out answers to all 5 objectives at the top of the page.
-Bring Graph paper for next class.
Sept 18 Thur Same as Wednesday
Sept 19 Fri -Quiz over p.80 Objectives
-Ch 3 p.80-86 (section 2)
-Archimedes "Eye Dropper" Diver demonstration
-p.86 #1-9
-Read p.87-92
-Study p.79 and be able to explain how a refrigerator works
Sept 22 Mon -Ch 3 p.87-92 (section 3)
-p.92 #1-6
-Review Ch 3
-p.94 #1-25
Chapter 3 Review Physical Science Holt Spectrum
-read the chapter carefully
-know objectives for all sections within the chapter
-know all the key terms
-study the summaries located at the end of each section
-study the summaries at the end of each section
-kinetic theory--know three main points p.70
-know four states of matter and be able to describe how particles behave in each state
-energy p.73
-thermal energy p.73
-temperature p.74
-changes of state a) evaporation, b) condensation, c) sublimation p.75
-Law of conservation of mass, law of conservation of energy p.77-78
-fluids p.80
-buoyant force p.80
-pressure, Archimedes' principle p.81
-float vs sink p.82
-pressure p.83 (pascal = SI unit of pressure)
-Pascal's principle p.84
-hydraulic devices p.85
-viscosity p.85
-Bernouli's principle p.86
-Boyle's, Charles's and Gay-Lussac's law p.88-92 (know how each law works)
Sept 23 Tues

Same as Monday

Sept 24 Wed -Test Ch 3
-Read Ch 4
-Write out all chapter 4 definitions, please # all terms
-Read Ch 4 p.104-110
-Read p.98-99 Lab "Boiling and Freezing" and be prepared to do the lab in class the next period
Sept 25 Thur Same as Wednesday
Sept 26 Fri SCHOOL PICNIC/ NO SCHOOL
Sept 29 Mon -p.98-99 Skills Practice Lab "Boiling and Freezing"
-use the regular lab write up format
Sept 30 Tues ITBS/GoGATS Testing
Oct 1 Wed ITBS/GoGATS Testing
Oct 2 Thur ITBS/GoGATS Testing
Oct 3 Fri Same as Monday
Oct 6 Mon -Help students complete "Boiling and Freezing" lab, especially graphing data
- Begin Ch 4 p.104-119 (part 1 & part 2)
-p.110 #1-7 (Complete & turn in at the end of class)
-p.119 #1-8
Oct 7 Tues Same as Monday
Oct 8 Wed -Ch 4 p.120-134
-p.128 #1-8
-p.134 #1-9
-Read p.129-134
Oct 9 Thur Same as Wednesday
Oct 10 Fri -Explain section 4-4 "Mole Concept"
-work p.134 #1-9 in class
Oct 13 Mon -Continue working problems p.134 #1-9
-Begin working on p.136 #1-28
-Clear up any questions on any ideas in chapter 4
Oct 14 Tues Same as Monday
Oct 15 Wed -Video #7 "The Periodic Table"
-(take notes--numbered, point form--about 10 ideas from the video 10 pts)
Oct 16 Thur Fall Break
Oct 17 Fri Fall Break
Oct 20 Mon Review Ch 4
-p.136 #1-28
-ExCred p.137 #29-39 (10 pts)
Review Ch 4
-Dalton's atomic theory states that every element is made of atoms that could not be subdivided, atoms of the same element are alike, and atoms can join to form molecules.
-the charge of an electron is negative
-the charge of a proton is positive
-the nucleus is made of protons and neutrons and has a positive charge
-atoms have no electric charge because they have equal numbers of protons and electrons
-according to Bohr's model of the atom, an electron behaves like planets orbiting the sun
-according to Bohr's theory, an electron's path around the nucleus defines its energy level
-atoms of elements in the same group have the same number of valence electrons
-an alkali metal ion, like Li, is much less reactive than a lithium atom because it has a full outermost energy level (valence)
-an atoms atomic number indicates the number of protons in the nucleus of the atom
-know where the alkali metals, alkaline earth metals, halogens and noble gas elements are located
-noble gases exist as single atoms rather than molecules
-semiconductors are elements that can conduct heat and electricity under certain conditions
-most halogens form compounds by gaining an electron to form a negative ion
-group 18, noble gases, are inert (non-reactive) because they have a full outermost energy level
-nonmetals are found on the right side of the periodic table
-metals are found in the center and left side of the periodic table
-a mole is the SI base unit that describes the amount of a substance
-Avogadro's constant is defined as the number of particles found in one mole of a pure substance
-molar mass is defined as the mass in grams of 1 mole of a substance
-be able to convert from moles to grams
-be able to convert from grams to moles
-it is impossible to know the exact location of an electron,
-order of the periodic table is based on the atomic number, -valence electrons determine the chemical properties and an atoms ability to form bonds,
-ionization is the losing or gaining of electrons, an ion is less reactive than an atom in the alkali metals because is has a full outer level,
-atomic numbers indicate an atoms # of protons or positive charges,
-mass # = protons plus neutrons,
-average atomic mass is a weighted average of common isotopes, -atomic mass unit is 1/12 the mass of a carbon-12 atom,
-alkali metals are located on the left side of the periodic table,
-be able to determine if an element is a alkali metal,
-alkali metals are quite reactive because they have one valence electron that is easily removed to form a positive ion,
-noble gases exist as single atoms rather than as molecules, -semiconductors are elements that can conduct heat and electricity under certain conditions,
-halogens form compounds by gaining an electron to form a negative ion,
-Group 18 (noble gases) are inert because their outermost energy level is full,
-nonmetals are found on the right side of the periodic table, -transition metals form compounds by losing electrons to form positive ions,
-a mole is a unit used to describe an amount of substance, -Avogadro's constant is defined as the number of particles in a mole of a substance,
-molar mass is the mass in grams of 1 mole of a substance,
-be able to calculate moles to mass,
-be able to calculate mass to moles (several questions of each type)
Oct 21 Tues SAME AS MONDAY
Oct 22 Wed -Test Ch 4
-Read Ch 5
-Write out all Ch 5 definitions (# all terms)
Oct 23 Thur SAME AS WEDNESDAY
Gas Prices
Oct 24 Fri -Begin Ch 5 Section 1
-p.150 #1-5
Oct 27 Mon -Ch 5 p.151-158 (section 2)
-p.158 #1-8
Oct 28 Tues SAME AS MONDAY
Oct 29 Wed -Complete p.158 #1-8 together (explaining chapter content again while answering questions on the assignment).
-Alkali metal demonstration at creek
Oct 30 Thur SAME AS WEDNESDAY
Oct 31 Fri -p.149 Quick Lab "Which melts more easily, sugar or salt?"
-Each person does their own lab assignment.
-Read p.159-164
Nov 3 Mon -Collect Lab p.149 (make sure to answer the two questions at the end of the lab)
-Ch 5 p.159-164 (section 3)
-p.164 #1-5
-p.152 #1-2 Connection to Social Studies (turn in during class)
Nov 4 Tues SAME AS MONDAY
Nov 5 Wed -Ch 5 p.165-172 Section 4
-p.172 #1-6
-p.146 #1-2 Fine Arts Connection (turn in during class)
Nov 6 Thur SAME AS WEDNESDAY
Nov 7 Fri Review Ch 5
-p.174 #1-26
Ch 5 Review Sheet
-chemical bonds are forces that hold atoms or ions together.
-mixtures are composed of substances that retain their own properties.
-compounds always contain the same elements in the same proportion
-be able to determine the number of atoms of each element in any compound.
-be able to determine whether compounds are ionic or covalent.
-know the comparative strength of bonds in solids, liquids and gases.
-molecules in gases have very little attraction for one another and therefore take up a lot of space.
-atoms form bonds (join) so they can become stable (and they achieve an outermost energy level that is full of electrons).
-bonds that form are not rigid--they are more like flexible springs.
-ionic bonds form between oppositely charged ions.
-covalent bonds form between nonmetal atoms.
-metallic bonds occur where the nucleus of one atom is attracted by a nearby atom's electrons.
-ionic compounds have very high melting points because the ions have very strong attraction for each other.
-metals are good conductors of electricity because their electrons are free to move from atom to atom.
-solid ionic compounds have very high melting points because they contain charged ions that are locked tightly together.
-covalent bonds occur when atoms share electrons.
-oxygen atoms that form negative ions are called oxide ions.
-anions are negative ions.
-cations are positive ions.
-be able to name covalent compounds (using table 7 on page 162).
-know the prefixes p.162 table 7.
-be able to use Roman numerals to name transition metals (groups 3-12).
-a carbon atom can bond to four other atoms because they have four valence electrons.
-know what valence electrons are
-methane is the simplest organic compound.
-alkanes are hydrocarbons that contain single covalent bonds.
-alkenes are hydrocarbons that contain double bonds.
-alcohols are organic compounds that contain carbon, oxygen and hydrogen.
-polymers are large organic molecules that are made of repeating units.
-proteins are polymers of amino acids.
Nov 10 Mon Test Ch 5
-Read Ch 6
-Write out all Ch 6 definitions--please # all terms (15 pts)
Nov 11 Tues SAME AS MONDAY
Nov 12 Wed Begin Ch 6 Sections 1 & 2 p.184-197
-p.189 #1-6
-p.197 #1-8
-Those wishing to do a retest on Ch 5 may do so on Monday at 2:40pm until 3:35 pm (the retake score will be averaged with the original score).
-NOTE: You must sign up so I can make a copies for the correct # of students.
-grades due end of the day
Nov 13 Thur -2pts/Ritz cracker apple pie (up to 14 pts bonus points)
-Make "Ritz Cracker Pies" and support CAD FOR HOPE CAMPAIGN
-Pies must be brought to Mr. Heilman on Monday Nov 24 or Tuesday am before school begins Nov 25 to receive extra credit for chemistry

RITZ CRACKER APPLE PIE
Source: http://www.alaskajohn.com/geocities/applepie.html
To demonstrate the use of artificial flavors and the limitation of the senses, and to prepare a chemical pie.

MATERIALS

Pastry for two pie crusts
Sugar
Cinnamon
Butter
Cream of tarter (potassium bitartrate)
Crackers (round, snack crackers)
Large Pot
Pie pan

PROCEDURE

Turn on oven at 450 degrees F
Bring 500 ml of water to a boil in a pot (approx. 2 cups)
Mix 1.5 cups of sugar with 1.5 teaspoons of cream of tartar.
Add this mixture to the boiling water.
Add 25 whole crackers, one at a time, to the water.
Boil for 3 min. but do not stir.
Pour this mixture into a pastry-lined pie pan.
Sprinkle with cinnamon.
Dot lightly with butter.
Cover with a pastry top. Pierce the top several times with a knife to allow steam to escape.
Bake at 450 degrees F for 30 minutes, or until done.

SAME AS WEDNESDAY

Nov 14 Fri -Quiz 6-2 Reaction Types (List the five reaction types, provide a general equation and actual examples for each of the five reaction types.) and Exothermic and Endothermic reactions
-Sign up for all the Ice Cream Lab Ingredients
Nov 17 Mon

Rock salt forces the ice surrounding the can of ice cream mix to melt. The "brine solution" or liquid that forms in the wooden bucket absorbs heat from the mix and gradually lowers the temperature of the mix until it begins to freeze. If there were no salt added to the ice, it would melt at 32 degrees Fahrenheit and eventually the ice water and mix would come to equilibrium at 32 degrees. The ice cream mix, however, does not begin to freeze until its temperature falls below 27 degrees. Therefore, in order to freeze the mix, we need a salt concentration, or a ratio of 5 cups of ice to 1 cups of salt. At this concentration, our brine temperature should remain constant at 8 to 12 degrees F. This will give the rapid cooling and freezing that is essential to making smooth creamy ice cream.

More detailed information provided by David Winer, Bethesda, Maryland For ice to melt into liquid water it must absorb a lot of heat energy. In an ice cream maker this heat needed to melt the ice comes from the mix, and so the mix chills. If the ice were not combined with salt, the mix’s cooling would be slow and would stop when the mix reached the temperature of melting freshwater ice-- at 32 degrees. But salt makes ice melt faster, and drops the temperature to that of freezing salt water. The heat used to melt the ice is drawn much faster from the surroundings, which in this case consist of the melted ice AND the ice cream mix. Since the surroundings lose large quantities of heat to the ice, they cool rapidly and continue to cool until they reach the freezing temperature of melting saltwater ice. This temperature is below the cream mixture's freezing point.



Dairy Ice Cream Lab: Things to Bring:
- List the names of all group members. Indicate who is responsible for each item being brought to the ice cream lab. Make a second copy of this sheet to leave with Mr. Heilman.
_______________________Ice cream maker (4 quart size) NOTE: All ingredients must be adjusted when a 2 quart or 6 quart ice cream maker is used.

_______________________Salt, rock (4lbs)

_______________________Can opener

_______________________Plastic spoons & bowls (enough for your lab group)

_______________________Serving spoon, large (for stirring ingredients and serving ice cream)

_______________________One gallon milk (skim, 2% or whole)

_______________________Sweetened condensed milk, 2 cans (14 ounce size) NOTE: Don't bring cans that are several years old--they are usually bad.

_______________________Pudding, Instant (your choice of flavor), 2 packages (5.1 ounce size)

_______________________Toppings (Pecans, Mixed Nuts, M&M’s, Oreo cookie crumbs, etc.)

-Iced is provided by the ice maker in the gymnasium office (no one needs to bring ice).

Vegan Ice Cream Lab: Things to Bring:
- List the names of all group members. Indicate who is responsible for each item being brought to the ice cream lab. Make a second copy of this sheet to leave with Mr. Heilman.
_______________________Ice cream maker (4 quart size) NOTE: All ingredients must be adjusted when a 2 quart or 6 quart ice cream maker is used.

_______________________Salt, rock (4lbs)

_______________________Can opener

_______________________Plastic spoons & bowls (enough for your lab group)

_______________________Serving spoon, large (for stirring ingredients and serving ice cream)

_______________________Silk Soymilk Vanilla, 1/2 gallon

_______________________Silk Creamer (Plain or French Vanilla) 1 quart

_______________________Vanilla (2-4 tsp depending on taste)

_______________________Honey (4-8 ounces depending on how sweet you like your ice cream)

_______________________Pudding, Instant (your choice of flavor), 2 packages of Jell-o Instant 5.1 oz size (yes, its vegan)

_______________________Toppings (Pecans, Mixed Nuts, M&M’s, Oreo cookie crumbs, etc.)

-Iced is provided by the ice maker in the gymnasium office (no one needs to bring ice).


Vegan Ice Cream (recipe courtesy of Arlen Byrd, Jan 2003)

List the names of all group members. Indicate who is responsible for each item being brought to the ice cream lab. Make a second copy to leave with Mr. Heilman.
__________________Soy milk—1/2 to 1 gallon, (liquid or powder) of your choice

__________________2 Tablespoons vanilla

__________________2-4 Cups frozen fruit blended (strawberry, peach, etc)

__________________1/2 to 1 cup sugar (white) per quart of ice cream made (depending on how sweet you want your ice cream)

__________________2 cups frozen bananas (or dairy free instant vanilla pudding)

__________________Blender

__________________Ice cream maker

__________________Rock salt (4 pounds)

__________________Toppings (nuts, cookie crumbs, candy, etc)

__________________Plastic spoons & bowls (enough for lab group)

__________________Serving spoon, large (for stirring and serving ice cream, sanitation)

Iced is provided by the ice maker in the gymnasium office (no one needs to bring ice).

The Chemistry of Ice Cream

Finding Science in Ice Cream - An Experiment for Secondary School Classrooms For further information about Finding Science in Ice Cream: Professor Douglas Goff, Ph.D. Department of Food Science University of Guelph Guelph , Ontario N1G 2W1 tel: (519)824-4120 ext. 3878 fax: (519)824-6631 e-mail: dgoff@uoguelph.ca This page was designed as a supplement to a classroom experiment for school teachers on ice cream making. Details of ice cream ingredients, manufacturing, structure, and many other aspects can be found on my main site at: http://foodsci.uoguelph.ca/dairyedu/icecream.html As the hot weather approaches and students minds begin to drift from the rigors of the school classroom or laboratory, a fun afternoon might be spent making ice cream and in so doing, introducing several aspects of the science and technology "behind the scenes".


The concept of melting ice with salt is not new to anyone in this latitude. Indeed, our roads, driveways, and sidewalks are kept bare in the winter by such a process. As salt is applied to ice, a concentrated brine solution forms on the ice, which has a very low freezing point. The freezing point of a 20% solution of salt is -16.6oC. As a result, more ice melts to dilute this solution, until the freezing point of the solution matches the outside temperature (equilibrium is established). The same phenomenon is occuring in the brine solution in the ice cream freezer. As the salt continues to dissolve more ice melts to accommodate this concentrated salt solution with its very low melting point. At the same time, both the heat of solution of the dissolving salt, and the latent heat of fusion of the melting ice are adsorbed from the ice itself, thereby lowering the temperature of the salt, ice and brine mixture. The temperature of this mixture can be controlled by the amount and ratio of salt and ice present. As examples, consider the following data: a 2% NaCl (salt) solution has a freezing point of -1.4oC, 5% salt conc. = -3.5oC, 10% salt = -7.4oC, 15% salt = -11.7oC and 20% salt = -16.6oC. The lowest temperature which can be achieved with a sodium chloride brine is -20oC, at a concentration of 23% salt. Higher concentrations result in salt crystallization. This brine, in turn, is adsorbing heat from the freezing ice cream inside the can, and thus ice and salt need to be continually added to keep the ice temperature low enough to freeze the ice cream. (Bear in mind that the freezing temperature of the ice cream is depressed below 0o due to the presence of dissolved sugars.) This process is a lesson in heat transfer in itself!

Nov 18 Tues SAME AS MONDAY
Nov 19 Wed Ch 6 Sections 3 & 4 p.198-204
-Work on assignment in class
-p.204 #1-5
Nov 20 Thur SAME AS WEDNESDAY
Nov 21 Fri -Quiz "Balancing Equations" (over information from last period)
-Ch 6 Section 4
-p.212 #1-8
Nov 24 Mon -Video #13 "The Driving Forces"
-Take notes (point form) for 15 ideas learned from the video (15pts)
-Pies must be brought to Mr. Heilman on Monday Nov 24 or Tuesday am before school begins Nov 25 to receive extra credit for chemistry
Nov 25 Tues SAME AS MONDAY
NOON DISMISSAL
-PLEASE BEGIN STUDYING FOR THE FINAL EXAM NOW!!!

Review for Semester Exam Ch 1-7

Physical Science Final Exam Review

 

  1. -The two main branches of science are natural and social
  2. -Know the branches of biology (ecology, zoology, medicine).
  3. -The three branches of natural science are life, physical, and earth science.
  4. -Technology is applied science which is using science for the benefit of mankind.
  5. -Pure science is continuing the search for new knowledge (which is learning for the sake of knowing).
  6. -Scientists do experiments to find out information about our world.
  7. -Scientific theories allow scientists to make predictions.
  8. -A scientific theory is an explanation that has been tested by many observations.
  9. -A scientific model is a representation of a real event or object.
  10. -Scientific models are used to help us envision real events or objects.
  11. -Scientific theories can be changed or replaced when new discoveries are made.
  12. -Scientific method is a series of logical steps that is followed to solve a problem.
  13. -Experiments are used to validate or test hypotheses.
  14. -An hypothesis is an educated guess that is testable.
  15. -Scientists test a hypothesis by doing experiments.
  16. -The SI unit for temperature is Kelvin.
  17. -Know the SI prefixes used for measurement (e.g. Deci, centi, milli, micro, deca, hecto, kilo, mega).
  18. -Be able to convert from one metric unit to another. e.g. grams to kilograms or centimeters to meters or the opposite direction.
  19. -Be able to read and interpret graphs.
  20. -Be able to express numbers in scientific notation.
  21. -Be able to express scientific numbers in regular notation.
  22. -A precise measurement is one that is as exact as possible.
  23. -A measurement that is accurate is one that is close to the true value.
  24. -Matter is anything that has mass and takes up space.
  25. -Chemistry is the science of what matter is made of and how it changes.
  26. -Oxygen is the most abundant element in the human body.
  27. -Elements are substances that cannot be broken down into simpler substances.
  28. -A molecule is the smallest unit of a substance that behaves like the substance.
  29. -Homogeneous mixture
  30. -Miscible
  31. -Immiscible
  32. -Be able to determine the number of atoms contained in a molecule of a compound.
  33. -Solids will hold its shape without a container.
  34. -Physical changes include breaking, tearing, and grinding.
  35. -Physical properties include freezing point, boiling point and density.
  36. -Digesting food or grilling a burger are examples of chemical changes.
  37. -Evidences of a chemical change taking place are release of a gas, change in color, production of a gas, releasing light or heat, or the formation of a precipitate.
  38. -Evaporation is the process of a liquid becoming a gas.
  39. -Freezing is the process of a liquid becoming a solid.
  40. -The heavier a particle, the slower it moves.
  41. -The speed of atoms and molecules are determined by the size of the atoms and the temperature of the substance.
  42. -Archimedes’ principle states that the buoyant force on an object in a fluid is equal to the weight of the displaced volume of fluid.
  43. -Buoyant force is the upward force exerted on an object immersed or floating on a liquid.
  44. -In order for ice to melt to form water, energy is absorbed.
  45. -Viscosity is the resistance of fluid to flow.
  46. -Kinetic theory states that the higher the temperature, the faster the particles that make up a substance move.
  47. -Evaporation refers to the change of state from a liquid to a gas.  
  48. -Pure substances can be represented by chemical formulas.
  49. -For solids, liquids and gases, know whether they have definite volume or definite shape.
  50. -Boiling point is where a liquid rapidly changes into a gas.
  51. -Know examples of a) Physical properties b) Chemical properties
  52. -Be able to do density problems (D = m/v)
  53. -Be able to determine if a change is chemical or physical.
  54. -Know five evidences that a chemical change has taken place.
  55. -Temperature is a measure of the average kinetic energy of the particles in an object.
  56. -Sublimation, condensation, evaporation, freezing (know what is happening in each process).
  57. -Lighter particles move faster than heavier particles at the same temperature.
  58. -Pascal’s principle states that a fluid in equilibrium in a closed vessel exerts pressure in all directions equally.
  59. -The law of conservation of mass states that mass cannot be created or destroyed.
  60. -Less dense materials float on more dense materials.  Example:  ice floats on liquid water because ice is less dense than water.
  61. -Boyle’s law relates of a gas to its volume.
  62. -Charles’s law is the relationship of volume to temperature.
  63. -Gay-Lussac’s law relates pressure of a gas to its temperature.
  64. -Pressure is determined by dividing force by area.
  65. -Buoyant force is upward force exerted on an object floating on a liquid.
  66. -When the volume of a certain amount of gas is decreased, the pressure will increase.
  67. -Dalton’s atomic theory states that every element is made of atoms that could not be subdivided, atoms of the same element are alike and atoms can join to form molecules.
  68. -Protons have a positive charge and are found in the nucleus of an atom.
  69. -Neutrons have no charge and are found in the nucleus of an atom.
  70. -Electrons carry a single negative charge.
  71. -Atoms have no electric charge because they have equal positive (protons) and negative (electrons) charge.
  72. -Bohr’s model of the atom states that electrons behave like planets orbiting the sun.
  73. -Bohr’s theory states that an electron’s path around the nucleus defines it energy level.
  74. -Modern atomic theory states that it is nearly impossible to determine an electron’s exact position.
  75. -The periodic table is arranged by increasing atomic number.
  76. -Atoms in the same group have similar properties.
  77. -Atoms of elements that are in the same group have the same number of valence electrons.
  78. -Valence electrons determine the chemical properties of atoms.
  79. -Ionization energy is the energy required to remove an electron from an atom.
  80. -Ions are much less reactive than neutral atoms because they have already achieved a noble bas configuration.
  81. -Atomic numbers indicate the number of protons in an atom.
  82. -An atom’s mass or mass number = the number of protons + number of neutrons.
  83. -Average atomic mass is …….
  84. -Alkali metals are located in the left-most column of the periodic table and they are the most reactive of the metals.
  85. -Noble gases exist as atoms rather than as molecules because they are very stable.
  86. -Semiconductors are elements that conduct heat and electricity under certain conditions.
  87. -Halogens are group 17 elements and form compounds by gaining an electron to form a negative ion.
  88. -Group 18 elements called the noble gas elements are inert because their outermost energy level is filled.
  89. -Non-metals are found on the upper right side of the periodic table.
  90. -Metals are found on the left side of the table.
  91. -Metalloids are found along the zigzag line between the metals and nonmetals.
  92. -Molar mass is defined as the mass in grams of 1 mole of a substance.
  93. -Be able to convert from moles to grams.
  94. -Be able to convert from grams to moles.
  95. -Chemical bonds are forces that hold different atoms or ions together.
  96. -Compounds vs. mixtures (compounds always have the same elements in the same proportion).
  97. -Mixtures are different from compounds because each substance in a mixture retains its own properties.
  98. -Gases take up a lot of space because their molecules have very little attraction for one another.
  99. -Atoms often join so that each atom will have an outermost energy level that is full of electrons.
  100. -An ionic bond is a bond that forms between ions with opposite charges.
  101. -Covalent bonds for formed between nonmetals.
  102. -Copper (or any metal) is a good conductor of electricity because its electrons are free to move from atom to atom.
  103. -Covalent bonds are where electron are shared between atoms.
  104. -Polymers are large organic molecules that are made of repeating units.
  105. -Proteins are polymers that are made of amino acids.
  106. -Chemical reactions happen when atoms are rearranged.
  107. -Exothermic reactions occur when energy is transferred from the reactants to the surroundings.
  108. -Endothermic reactions occur when energy is transferred from the surroundings to the reactants.
  109. -The source of energy in photosynthesis is light energy.
  110. -Digestion is an example of a decomposition reaction.
Nov 26 Wed THANKSGIVING VACATION
Nov 27 Thur THANKSGIVING VACATION
Nov 28 Fri THANKSGIVING VACATION
Dec 1 Mon Review Ch 6
-p.214 #1-28

Physical Science Ch 6 Test Review
- NOTE: Make sure that you can apply these ideas to situations that will be presented within the test.
-Know five signs that indicate that a chemical reaction has (or is) taking place. (heat, light, precipitate, change in color, production of a gas)
-A reactant is a substance that undergoes a change in a chemical reaction.
-In a chemical reaction atoms are rearranged.
-Exothermic reactions are those in which energy is transferred from reactants to the surroundings.
-Endothermic reactions are those where energy is transferred from the surroundings to the reactants.
-Chemical energy is energy that is derived from the atoms and molecules.
-Photosynthesis is a good example of the energy of the sun (light energy) being transferred to chemical (stored) energy in plants.
-Know the five general types of chemical reactions (what is happening in each type).
a) synthesis: A + B --> AB
b) decomposition: AB --> A + B
c) single displacement: A + BC --> AC + B
d) double displacement: AB + CD --> AD + CB
e) combustion: C xH y + O 2 --> CO 2 + H 2O
-The product of the synthesis reaction between sodium and chlorine gas is sodium chloride.
-Know the equation Na + Cl2 --> NaCl
-When methane reacts with oxygen it produces carbon dioxide and water.
-When water decomposes (electrolysis), it produces hydrogen gas and oxygen gas.
-Digestion is an example of decomposition.
-Radicals are fragments of molecules that have one or more electrons available for bonding.
-Redox reactions are those where one substance accepts electrons (is reduced) and another gives electrons (is oxidized).
-Balancing a chemical reaction (often) requires changing or adding coefficients.
-Be able to determine the number of moles used/produced in a reaction by looking at a balanced chemical equation.
-Know the law of definite proportions and how it works.
-In any balanced chemical equation, the total mass of the reactants equals the total mass of the products.
-Any balanced chemical equation indicates the number of particles of reactants and products as well as the number of moles of reactants and products.
-Know factors that speed up the rate of a chemical reaction (increasing the surface area, increasing the pressure, increasing the temperature, adding a catalyst).
-Enzymes are biological catalysts which speed up the rate of a chemical reaction.
-Enzymes are proteins that act as catalysts in chemical reactions.
-Inhibitors are catalysts that slow down a reaction.
-Chemical equilibrium is where the forward rate (production of products) is equal to the reverse rate (production of reactants).
-Whenever the concentration of one substance in an equilibrium is increased, then the reaction proceeds so that less of that particular substance is produced.
-Electrolysis is when water is broken down into hydrogen and oxygen.
-LeChatelier's principle states: If a change is made to a system in chemical equilibrium, the equilibrium shifts to oppose the change until a new equilibrium is reached.
Dec 2 Tues Same as Monday
Dec 3 Wed Test Ch 6
-Write out all Ch 7 definitions (please # all terms), do during class if possible to avoid an assignment over Thanksgiving break.

Begin Ch 7 p.224-231
-p.231 #1-7
Dec 4 Thur Same as Wednesday
Dec 5 Fri Ch 7 p.232-244
-p.238 #1-6
-Read & study p.232-244
Dec 8 Mon -Quiz p.232-244
-Review 7.3 as necessary (do problems calculating molarity)
-p.244 #1-7
-p.245 #1-6 Graphing Skills-
Dec 9 Tues Same as Monday
Dec 10 Wed p.246 #1-23, extra credit #24-27
Review Ch 7
Chapter 7 Review Physical Science Holt Spectrum
-read the chapter carefully
-know objectives for all sections within the chapter
-know all the key terms
-study the summaries located at the end of each section
-study the summaries at the end of each section
-homogeneous
-heterogeneous
-suspension
-colloid
-emulsion
-solution
-solute
-solvent
-alloy
-know three ways to increase the rate at which a solute dissolves
-olive oil is an example of a non-polar compound
-egg whites, paint, blood and whipped cream are all examples of colloids
-distillation
-polar compound
-hydrogen bonding
-nonpolar compound
-be able to determine the ability of a substance to dissolve as it relates to the relative strength of forces between the solvent molecules.
-explain how a solute affects the freezing point and boiling point of a solution
-like dissolves like (eg. polar will dissolve polar and nonpolar will dissolve nonpolar)
-solubility (grams of solute per 100 grams of solvent)
-concentration
-unsaturated solution
-saturated solution
-supersaturated solution
-be able to determine the molarity (moles of solute / liter of solution)of a solution
-be comfortable with reading graphs (eg. p.245)
Dec 11 Thur Same as Wednesday
Dec 12 Fri Test Ch 7 (to be included on the final exam)
-Review for Exam

The greatest want in the world is the want of men

Men who will not be bought or sold,

Men who in their inmost souls are true and honest,

Men who do not fear to call sin by its right name,

Men whose conscience is as true to duty as the needle to the pole

Men who will stand for the right though the heavens fall.
Dec 15-18 Mon-Th


Review for Semester Exam Ch 1-7

Physical Science Final Exam Review

 

  1. -The two main branches of science are natural and social
  2. -Know the branches of biology (ecology, zoology, medicine).
  3. -The three branches of natural science are life, physical, and earth science.
  4. -Technology is applied science which is using science for the benefit of mankind.
  5. -Pure science is continuing the search for new knowledge (which is learning for the sake of knowing).
  6. -Scientists do experiments to find out information about our world.
  7. -Scientific theories allow scientists to make predictions.
  8. -A scientific theory is an explanation that has been tested by many observations.
  9. -A scientific model is a representation of a real event or object.
  10. -Scientific models are used to help us envision real events or objects.
  11. -Scientific theories can be changed or replaced when new discoveries are made.
  12. -Scientific method is a series of logical steps that is followed to solve a problem.
  13. -Experiments are used to validate or test hypotheses.
  14. -An hypothesis is an educated guess that is testable.
  15. -Scientists test a hypothesis by doing experiments.
  16. -The SI unit for temperature is Kelvin.
  17. -Know the SI prefixes used for measurement (e.g. Deci, centi, milli, micro, deca, hecto, kilo, mega).
  18. -Be able to convert from one metric unit to another. e.g. grams to kilograms or centimeters to meters or the opposite direction.
  19. -Be able to read and interpret graphs.
  20. -Be able to express numbers in scientific notation.
  21. -Be able to express scientific numbers in regular notation.
  22. -A precise measurement is one that is as exact as possible.
  23. -A measurement that is accurate is one that is close to the true value.
  24. -Matter is anything that has mass and takes up space.
  25. -Chemistry is the science of what matter is made of and how it changes.
  26. -Oxygen is the most abundant element in the human body.
  27. -Elements are substances that cannot be broken down into simpler substances.
  28. -A molecule is the smallest unit of a substance that behaves like the substance.
  29. -Homogeneous mixture
  30. -Miscible
  31. -Immiscible
  32. -Be able to determine the number of atoms contained in a molecule of a compound.
  33. -Solids will hold its shape without a container.
  34. -Physical changes include breaking, tearing, and grinding.
  35. -Physical properties include freezing point, boiling point and density.
  36. -Digesting food or grilling a burger are examples of chemical changes.
  37. -Evidences of a chemical change taking place are release of a gas, change in color, production of a gas, releasing light or heat, or the formation of a precipitate.
  38. -Evaporation is the process of a liquid becoming a gas.
  39. -Freezing is the process of a liquid becoming a solid.
  40. -The heavier a particle, the slower it moves.
  41. -The speed of atoms and molecules are determined by the size of the atoms and the temperature of the substance.
  42. -Archimedes’ principle states that the buoyant force on an object in a fluid is equal to the weight of the displaced volume of fluid.
  43. -Buoyant force is the upward force exerted on an object immersed or floating on a liquid.
  44. -In order for ice to melt to form water, energy is absorbed.
  45. -Viscosity is the resistance of fluid to flow.
  46. -Kinetic theory states that the higher the temperature, the faster the particles that make up a substance move.
  47. -Evaporation refers to the change of state from a liquid to a gas.  
  48. -Pure substances can be represented by chemical formulas.
  49. -For solids, liquids and gases, know whether they have definite volume or definite shape.
  50. -Boiling point is where a liquid rapidly changes into a gas.
  51. -Know examples of a) Physical properties b) Chemical properties
  52. -Be able to do density problems (D = m/v)
  53. -Be able to determine if a change is chemical or physical.
  54. -Know five evidences that a chemical change has taken place.
  55. -Temperature is a measure of the average kinetic energy of the particles in an object.
  56. -Sublimation, condensation, evaporation, freezing (know what is happening in each process).
  57. -Lighter particles move faster than heavier particles at the same temperature.
  58. -Pascal’s principle states that a fluid in equilibrium in a closed vessel exerts pressure in all directions equally.
  59. -The law of conservation of mass states that mass cannot be created or destroyed.
  60. -Less dense materials float on more dense materials.  Example:  ice floats on liquid water because ice is less dense than water.
  61. -Boyle’s law relates of a gas to its volume.
  62. -Charles’s law is the relationship of volume to temperature.
  63. -Gay-Lussac’s law relates pressure of a gas to its temperature.
  64. -Pressure is determined by dividing force by area.
  65. -Buoyant force is upward force exerted on an object floating on a liquid.
  66. -When the volume of a certain amount of gas is decreased, the pressure will increase.
  67. -Dalton’s atomic theory states that every element is made of atoms that could not be subdivided, atoms of the same element are alike and atoms can join to form molecules.
  68. -Protons have a positive charge and are found in the nucleus of an atom.
  69. -Neutrons have no charge and are found in the nucleus of an atom.
  70. -Electrons carry a single negative charge.
  71. -Atoms have no electric charge because they have equal positive (protons) and negative (electrons) charge.
  72. -Bohr’s model of the atom states that electrons behave like planets orbiting the sun.
  73. -Bohr’s theory states that an electron’s path around the nucleus defines it energy level.
  74. -Modern atomic theory states that it is nearly impossible to determine an electron’s exact position.
  75. -The periodic table is arranged by increasing atomic number.
  76. -Atoms in the same group have similar properties.
  77. -Atoms of elements that are in the same group have the same number of valence electrons.
  78. -Valence electrons determine the chemical properties of atoms.
  79. -Ionization energy is the energy required to remove an electron from an atom.
  80. -Ions are much less reactive than neutral atoms because they have already achieved a noble bas configuration.
  81. -Atomic numbers indicate the number of protons in an atom.
  82. -An atom’s mass or mass number = the number of protons + number of neutrons.
  83. -Average atomic mass is …….
  84. -Alkali metals are located in the left-most column of the periodic table and they are the most reactive of the metals.
  85. -Noble gases exist as atoms rather than as molecules because they are very stable.
  86. -Semiconductors are elements that conduct heat and electricity under certain conditions.
  87. -Halogens are group 17 elements and form compounds by gaining an electron to form a negative ion.
  88. -Group 18 elements called the noble gas elements are inert because their outermost energy level is filled.
  89. -Non-metals are found on the upper right side of the periodic table.
  90. -Metals are found on the left side of the table.
  91. -Metalloids are found along the zigzag line between the metals and nonmetals.
  92. -Molar mass is defined as the mass in grams of 1 mole of a substance.
  93. -Be able to convert from moles to grams.
  94. -Be able to convert from grams to moles.
  95. -Chemical bonds are forces that hold different atoms or ions together.
  96. -Compounds vs. mixtures (compounds always have the same elements in the same proportion).
  97. -Mixtures are different from compounds because each substance in a mixture retains its own properties.
  98. -Gases take up a lot of space because their molecules have very little attraction for one another.
  99. -Atoms often join so that each atom will have an outermost energy level that is full of electrons.
  100. -An ionic bond is a bond that forms between ions with opposite charges.
  101. -Covalent bonds for formed between nonmetals.
  102. -Copper (or any metal) is a good conductor of electricity because its electrons are free to move from atom to atom.
  103. -Covalent bonds are where electron are shared between atoms.
  104. -Polymers are large organic molecules that are made of repeating units.
  105. -Proteins are polymers that are made of amino acids.
  106. -Chemical reactions happen when atoms are rearranged.
  107. -Exothermic reactions occur when energy is transferred from the reactants to the surroundings.
  108. -Endothermic reactions occur when energy is transferred from the surroundings to the reactants.
  109. -The source of energy in photosynthesis is light energy.
  110. -Digestion is an example of a decomposition reaction.

Final Exams