Chemistry Assignment-Test Schedule 2007-2008
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 PAPER OR BE PREPARED TO WRITE OUT THE ASSIGNMENT AGAIN.

NOTE: INSTRUCTIONS FOR WRITING A LABORATORY REPORT ARE LOCATED AT THE BOTTOM OF THIS WEB PAGE.

 

Aug 1-12   School Meetings for teachers
Aug 2    
Aug 3  

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

-NOTE: You may find p.841 "How to Write a Laboratory Report" found in the Physical Science textbook helpful to look at as well.
Aug 6    
Aug 7    
Aug 8    
Aug 9    
Aug 10    
Aug 13 Mon

School begins:

-Seating Chart
-1st Day Information from class website
-Ch 1 p.5-18 (Sections 1) powerpoint (branches of chemistry)
-p.7 #1-3 Check off in class
-p.18 #1-4 Check off in class
-Read Ch 1 (sections 1& 2) p.5-18 (know all bold print terms and branches of chemistry on page 6)

-Have your parent(s) sign the lab safety agreement (NOTE: This is a 10 point assignment)


Collegedale Academy Laboratory Safety Agreement

-p.789 Safety Quiz (in class if time available) in groups of two people #1-14 (Cooperative Groups--PAIR SHARE)

Aug 14 Tues Same as Monday
Aug 15 Wed -Collect Lab Safety agreement signed by parent
-Quiz over p.5-18 reading assignment
-Ch 1 Sections 2&3 (properties of matter, elements)
-Read Ch 1 p.20-24 (Section 3)
-study for quiz over TABLE 7-2 (page 210), 1st column of POLYATOMIC IONS
-Pringles Can Hydrogen Demonstration!!!
Aug 16 Thur Same as Wednesday
Aug 17 Fri -Quiz over TABLE 7-2, 1st column of POLYATOMIC IONS
-Ch 1 Vocabulary may be done for 2pts extra credit to replace the 2pts extra credit offered for printing out the Lab Safety Agreement (since the internet has not been available this first week). Turn in the vocabulary at the beginning of the test next Tues/Wed for 2pts ex credit.

Ch 1 Review (Read Ch 1 carefully & study chapter summary p.25) NOTE: Make sure you can apply these ideas.
-the most useful source of information about the elements is the periodic table,
-elements that are close to each other in a period tend to be more similar than those that are far apart,
-know all bold print terms (definition and concepts),
-learn the six branches of chemistry (6), basic and applied (& technological dev) (7),
-be able to recognize chemical & physical changes (12,13),
-be able to recognize chemical, physical, intensive and extensive properties,
-read and carefully study solid, liquid & gas descriptions (spacing, characteristics, volume and shape) (12),
-metal properties and location (22),
-nonmetal properties and location (23),
-noble gases properties and location (24),
-metalloid properties and location (along zigzag line) (24), -homogeneous and heterogeneous solution
-Study hard!!
Aug 20 Mon Picture Day/class meetings
Aug 21 Tues -Test Ch 1 
-Read Chapter 2 p.29-58 
-p.58 Define Vocabulary (all sections)
- NOTE: VOCABULARY MUST BE HAND WRITTEN (NO TYPED VOCABULARY ASSIGNMENTS ACCEPTED).
-Learn 2nd and 3rd column of p.210 Table 7-2 for a Quiz next period.
Aug 22 Wed Same as Tuesday
Aug 23 Thur -Quiz p.210 2nd & 3rd Columns
-Fire Polishing Lab
-Tie back long hair
-Wear safety goggles at all times
-Do NOT touch hot glassware (just because the glass is not red hot doesn't mean it won't still burn you).
-Learn how to use bunsen burners
-Light your burner immediately upon turning on your gas jet -- if it does not lite, turn off the gas jet immediately & get help.
-Cut a 15 cm length of glass tubing for the stirring rod you will make.
-Make one stirring rod (seal both ends completely)
Aug 24 Fri Same as Thursday
Aug 27 Mon -Begin Ch 2 section 1 & 2 PowerPoint/discussion 
-p.31#1-4  (scientific method)
-p.60#27-34 (D = m/v problems -- be able to rearrange the density equation solving for mass or volume)
Aug 28 Tues Same as Monday
Aug 29 Wed -Ch 2 Section 3 PowerPoint p.44-56
-p. 60 #35-46 (significant figures and scientific notation)
Aug 30 Thur Same as Wednesday
Aug 31 Fri Video #1 "The World of Chemistry"
(take notes--numbered, point form--about 15 ideas from the video)
Sept 3 Mon No School -- Labor Day
Sept 4 Tues -Metric Conversions
Lab -- Measure any five objects (test tubes, beakers, doors, etc) in cm and convert each of the measurements into the eleven other metric units (using Table 2-2 p.35).

-p.45 #1,2 Practice only--do in class (percent error)
-p.50 #1-4 Practice only--do in class (significant figures)
-p.57 #1-8 (density, significant figures)
Sept 5 Wed Same as Tuesday
Sept 6 Thur

-p.59 #1-15 
-Review Ch 2 
-use Cooperative Groups (PAIR SHARE) to review Ch 2

 

Review Ch 2:

-Scientific Method (p.29-31)
-system,

-hypothesis,

-model,

-theory is a generalization that explains a body of known facts or phenomena, it is also a believable explanation of a body of observed natural phenomena
-scientific concepts are validated testing hyphotheses

-quantitative (p.29),

-qualitative,
-data is organized, analyzed and classified in order to determine relationships among information

-quantity,

-measurement standards,

-Table 2-1 SI base units

-Table 2-2 SI prefixes

-weight,

-mass is a measure of a quantity of matter

-derived units,

-volume, density, (be familiar with units used to measure various quantities),

-be able to do density calculations,
-when determining density the temperature must be specified (density varies with changes in temperature)

-be able to convert from one unit to another unit using SI prefixes in Table 2-2,

-1L = 1dm3 = 1000 mL = 1000 cm3,

-be able to convert from Celsius to Kelvin (add 273.15 to Celsius to get the Kelvin equivalent),

-precision and accuracy,
-poor precision may result from human error and limitations of the measuring instruments

-be able to determine the # of significant figures in a measurement and do calculations correctly with significant figures,

-be able to round numbers correctly,

-be able to express numbers in scientific notation,

-be able to round numbers correctly in scientific notation as well,

-two variables are inversely proportional when their product has a constant value
-two variables are directly proportional when they are divided they produce a constant
-direct and inverse proportion (be able to recognize their graphs).
-be able to determine the most appropriate unit for measuring something (choose a unit that does not require a very small or very large number).
Sept 7 Fri Mon/Wed classes meet
Sept 10 Mon Fall Picnic
Sept 11 Tues

Test Ch 2 
-p.86 Define Vocabulary (all 3 sections)
-Please number all definitions

Sept 12 Wed Same as Tuesday
Sept 13 Thur -Density Lab
-use standard lab format for lab write up (look at the beginning of this web page).
Sept 14 Fri Mon/Wed classes meet
Sept 17 Mon Begin Ch 3p.65-81 PowerPoint (sections 1,2, & 1st part of 3)
-p.87 #1-16
-Learn Fig 3-11
Sept 18 Tues Same as Monday
Sept 19 Wed -Quiz Section 3-1 Atomic Theory & Structure
Ch 3 p.82-85 Work problems on board and in Cooperative Groups (PAIR SHARE)
-p.83 #1-4 Top of page
-p.83 #1-2 Bottom of page
-p.84 #1-3
-Review & study p.75-85
Sept 20 Thur Same as Wednesday
Sept 21 Fri -Work Problems on the board--Use class period to do assignment while help is available

p.87 #17-28
-use cooperative learning (10:5 Kagan--PAIRS CHECK)
-Study for a quiz over p.81-85 problem solving.

Sept 24 Mon

-Quiz over p.81-85 Problem Solving
Review Ch 3

Ch 3 Review (Read Ch 3 carefully & study chapter summary p.86) NOTE: -Make sure you can apply these ideas.
- Law of Conservation of Mass (p.66),
- law of definite proportions (was explained by Dalton's atomic theory) (66), -law of multiple proportions (66),
- know Dalton's atomic theory (66),
- Dalton's atomic theory has been expanded and modified, in the late 1800's many experiments were performed by passing electric current through gases at low pressures (70),
- know how a cathode ray tube works (know the parts and how the electric current travels from cathode to anode from a high energy power source) 70, -Rutherford's gold foil experiment ,
-several questions about Rutherford--know thoroughly (72),
- nuclear forces (74),
- the electron cloud occupies most of the volume of an atom, atom (70), -isotopes (76),
- atomic number (75),
- know table 3-2 p.76 about the three isotopes of hydrogen,
- know Table 3-3 three isotopes of hydrogen (77),
- atoms of the same element all have the same atomic number,
- atomic mass unit (78),
- average atomic mass (79),
- a single atom of an isotope does not have an average atomic mass,
- be able to determine the number of protons, neutrons and electrons for atoms (p.77 table 3-3, sample problem 3-1, p.78 Practice #1-3,
- Avogadro's # (6.022 x 10 to the 23rd) p.81,
- molar mass (81),
- mole (81),
- know figure 3-11 and be able to convert from atoms, moles, or grams to any other unit--several questions about this topic (82),
- Dalton is credited with being the first to think of the atomic theory,
- the electron was discovered using the cathode ray tube,
- Millikan's experiments measured the charge on the electron,
- Rutherford concluded that the nucleus (dense core) must be positively charged since a few of the positively charged particles (alpha particles) bounced back,
- protons and neutrons have about the same mass,
- the electron is about 1/2000th the mass of a proton or hydrogen atom,
- the nucleus is composed of protons and neutrons,
- atoms are electrically neutral because they have the same number of electrons (-) and protons (+),
- isotopes of the same element have different masses due to the differing numbers of neutrons,
- the radius of an atom is extends to the outer edge of the region occupied by the electrons (called the electron cloud),
- tritium is the radioactive isotope of hydrogen with a mass of 3,
- deuterium is an isotope of hydrogen with a mass of 2 and protium,
- the most common form, has a mass of 1,
- be able to determine the mass number,
- atomic number and the number of protons and neutrons
Sept 25 Tues Same as Monday
Sept 26 Wed Test Chapter 3 
-p.117 Define Vocabulary (all 3 sections)
-Read 4-1 p.91-97
-Polyatomic Ion Quiz next Monday/Tuesday Oct 2-3
Sept 27 Thur Same as Wednesday
Sept 28 Fri -Begin Ch 4 p.91-97 
-p.97 #1-5

-Read p.98-107
Oct 1 Mon -Chemistry Bingo
Ch 4 p.98-107 
-p.104 #1-3
Oct 2 Tues -Same as Monday
Oct 3 Wed -Quiz Polyatomic Ions
-Ch 4 Practice 
-Write electron configurations for elements #13-37
-p.110-116
-p.118 #18-34
Oct 4 Thur Same as Wednesday
Oct 5 Fri -p.119 #35,39,41,42
-Review Ch 4
Oct 8 Mon Friday Schedule on Monday (meet all classes)
-Review Ch 4
-rate of speed of all forms of electromagnetic radiation (3.0 x 10 to the eight m/s) p.91,
-know equation for the speed of light (c = lambda multiplied by v),
-all electromagnetic radiation have the same speed,
-frequency is measured in hertz,
-electromagnetic radiation exhibits wavelike behavior, -wavelength,
-photon,
-quantum,
-photoelectric effect,
-line emission spectrum,
-continuous spectrum,
-when hydrogen is excited and the emitted light is passed through a prism, it is possible to see four different colors of light,
-ground state,
-excited state,
-electron cloud,
-de Broglie believed in the dual wave-particle nature of electromagnetic radiation,
-orbital = the three dimensional region around a nucleus where an electron may be found,
-(quantum numbers n,l,m,s)
-principal quantum number,
-angular momentum quantum number,
-magnetic quantum number,
-spin quantum number,
-p orbitals are dumbbell-shaped and orient about the x,y & z axes,
-s orbitals are spherical, know the number of electrons in level 1 = 2; 2 = 8; 3 = 18; 4 = 32,
-each orbital can hold a maximum of 2 electrons,
-Aufbau principle,
-Pauli exclusion principle, & Hund's rule,
-electron configurations up to element 56 = Barium,
-octet of electrons found in the Noble gases,
-Octet = an element with 8 electrons in its highest main energy level
-use Cooperative Groups (PAIR SHARE) to review Ch 4
Oct 9 Tues -Senior Survival leaves at noon through end of week
NOTE: SCHOOL ENDS AT NOON TUESDAY-FRIDAY
-Begin Ch 5 p.123-126 (Section 5-1 PowerPoint)
-p.127 #1-4 
-p.139 #1,2,4,5
Oct 10 Wed Same as Tuesday
Oct 11 Thur -Postpone Test Ch 4, provide additional time for review
-Review Ch 4 again
Oct 12 Fri Same as Thursday
Oct 15 Mon Friday Schedule Meet all classes
-Test Ch 4
-p.155 Define Vocabulary (all three sections)
-NOTE: Please number all terms
Oct 16 Tues -Video #7 The Periodic Table
-(take notes--numbered, point form--about 15 ideas from the video)
-Individuals taking the PSAT do not have to make up the video.
Oct 17 Wed Same as Tuesday (Mon/Wed classes meet)
-Noon Dismissal -- Fall Break
Oct 18 Thur Staff Development
Oct 19 Fri Fall Break
Oct 22 Mon No School -- Fall Break
Oct 23 Tues -Ch 5 p.128-139 (Section 2 PowerPoint)
-p.155 #1-9,11-15
-Quiz next period p.210 Polyatomic Ions
-use cooperative learning (10:5 Kagan--PAIRS CHECK)
Oct 24 Wed Same as Tuesday
Oct 25 Thur -Ch 5 p.140-154 (Section 5-3 PowerPoint) 
-use cooperative learning (10:5 Kagan--PAIRS CHECK) 
-p.156 #17-22 
-p.157 #39-49
Oct 26 Fri -Mon/Wed classes meet
-Same as Thursday
Oct 29 Mon -Ch 5 Review 
-Chemistry Review Ch 5

-Mendeleev arranged elements in the periodic table according to the elements chemical and physical properties.
-Mendeleev left spaces for elements that had not yet been discovered.
-Mosley arranged the periodic table according to increasing atomic number.
-Mendeleev arranged the periodic table according to increasing atomic mass.
-The periodic table is the single most useful source of information about the elements.
-The periodic table allows properties of elements to be determined before they are discovered.
-Know the location of: a) lanthanides, b) actinides, c) alkali metals, d) alkaline earth metals, e) halogens, f) noble gases, g) metals, h) nonmetals, i) metalloids--the elements along the zig-zag line in the periodic table (NOTE: be able to determine to which category an element belongs).
-Know the block (s,p,d,f) to which each of the groups belong.
-Be able to determine the number of elements in a period.
-The discovery of the noble gases changed the periodic table by adding a new group (18).
-The length of a period is determined by the sublevels being filled with electrons.
-Hydrogen is placed separately from the other elements because it has many unique properties.
-The atomic radius is determined by measuring 1/2 the distance between two adjacent nuclei.
-The periodic law = physical and chemical properties of elements are periodic functions of their atomic numbers.
-Elements in a given group have similar properties.
-Know what a period and group are in the periodic table.
-Elements with the s and p orbitals filled are noble gases.
-Outermost electrons are located in the s and p orbitals.
-Be able to determine the noble gas configuration (and notation) of any element.
-The most characteristic property of the noble gasses is that they are mainly unreactive.
-Alkali metals are more reactive than the alkaline earth metals.
-Alkali metals are found in nature in compounds (they are also found in the s block).
-Alkali metals are soft, silvery active metals with one electron in the s orbital.
-Be familiar with s, p, d, and f blocks of the periodic table.
-Know the periodic trends for: a) atomic radii, b) ionization energy, c) electron affinity, d) electronegativity
-Alkaline earth metals are less reactive than the alkali metals.
-When an electron is added to a neutral atom, energy is either released or absorbed.
-Know about exothermic (A + e- => A- + energy) and endothermic (A + energy + e- => A-) processes associated with electron affinity.
-Electron affinity is the energy change that occurs when an electron is acquired by a neutral atom.
-Ionization energy is the energy required to remove and electron from an atom.
-Electronegativity is the ability of an atom in a chemical compound to attract electrons.
-Atomic radius is ½ the distance between nuclei of identical atoms that are bonded together.
-Negative ions are called anions.
-Anions are larger than the neutral atoms from which they are formed.
-Positive ions are called cations.
-Cations are smaller than the neutral atoms from which they are formed.
-Valence electrons are available to be lost, gained, or shared when atoms form molecules.
-use Cooperative Groups, PAIR SHARE, to review Ch 5 
Oct 30 Tues Same as Monday
Oct 31 Wed -Test Chapter 5 
-p.194 Define Vocabulary (40 pts, all sections, please number all terms)
Nov 1 Thur Same as Wednesday
Nov 2 Fri -Video #8 "Chemical Bonds"
-(take notes--numbered, point form--about 15 ideas from the video)
Nov 5 Mon -Begin Ch 6 Sections 6-1 & 6-2 PowerPoint p.161-175
-p.195 #1-9
-p.175 #1-4 (Do in class if time allows)
-Read p.175-185
-Study for a quiz over determining what type of chemical bond is present in a compound.
Nov 6 Tues Plan Test for all sophomores
Nov 7 Wed -Quiz, Determining electronegativity differences & whether a bond is ionic, covalent or polar covalent.
-Ch 6 Complete Section 6-2 & Sections 6-3 & 6.4 PowerPoint p.176-182 (More if time allows)
-p.195 #11-18
Nov 8 Thur Same as Wednesday
Nov 9 Fri Ch 6 Section 6-5 PowerPoint p.183-193
-p.196 #33-49

-2pts/chemical apple pie (up to 14 pts bonus points)
-Make "Apple Pies" and support project 24,000!!!

A CHEMICAL 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.
Nov 12 Mon

Chapter 6 Review

Chemistry Ch 6 Review Sheet
-Chemical bond is the mutual attraction between nuclei and valence electrons.
-Valence electrons are involved in the formation of a chemical bond.
-Atoms by themselves are at relatively high potential energy.
-Atoms become more stable when they are bonded (they have relatively low potential energy).
-Atoms naturally move toward low potential energy.
-Atoms bond and become more stable.
-Know about ionic bonds.
-Ionic bonds are formed by electrostatic attraction between positive (cations) and negative (anions).
-Covalent bonds are formed when atoms share electrons.
-Nonpolar covalent bonds are formed between identical atoms.
-Electronegativity is the electrical attraction of an atom for its shared electrons.
-Polar covalent bonds occur when atoms share electrons unequally.
-Ions attract each other in an ionic bond.
-Most bonds are partially ionic and partially covalent.
-Bonds that are more than 50% ionic (1.7 electronegativity difference) are considered ionic bonds.
-Be able to determine the order of various pairs of elements in terms of their electro negativity differences.
-0.3 Electronegativity difference (5% ionic) and more equals a polar covalent bond.
-Molecular formulas show the types and number of atoms joined in a single molecule.
-Bond length is the separation for which the potential energy is at a minimum.
-Bond energy is the energy required to break a chemical bond.
-Octet rule
-s & p orbitals are filled for the noble gases (except helium).
-Be able to draw Lewis structures (by knowing the number of valence electrons present in the atoms to be joined).
-Formula unit is the simplest ratio of ions that balances total charge (total positive equals total negative).
-Molecular formula are used for covalently bonded compounds.
-Formula units are used for ionic bonded compounds.
-In ionic compounds each cation is surrounded by anions.
-Ions in ionic compounds are organized into crystals.
-Malleability allows one plane of ions to slide past another without breaking bonds.
-Ductility is a characteristic of metallic bonds (along with malleability).
-Know table 6-5 (p.186) to determine the molecular geometry (linear, trigonal planar, tetrahedal, trigonal pyramidal, bent or angular).
-Hydrogen bonding
-Dipole-Dipole forces are strong forces of attraction between positive and negative regions of molecules.
-London dispersion forces are weak intermolecular forces between instantaneous (and induced) dipoles.
-BrINClHOF (Know the 7 diatomic elements)
-use Cooperative Groups, PAIR SHARE
Nov 13 Tues Grades due, pm
Same as Monday
Nov 14 Wed

-NOTE: IF YOU ARE LEAVING EARLY FOR THANKSGIVING, YOU MUST TAKE CH 6 TEST BEFORE YOU LEAVE--NO EXCEPTIONS!!!!!!

-Advance planners: please begin reviewing for the semester exam ch 1-7. The exam review is found on Dec 15 on this web page.

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 15 Thur Same as Wednesday
Nov 16 Fri Continue Review of Ch 6
-If you will miss the test next Mon or Tues--you must take it before you leave today!!! No Exceptions!!!
Nov 19 Mon Test Ch 6 
-p.234 Define Vocabulary -- all three sections (please # terms). 
Nov 20 Tues Same as Monday/Noon Dismissal
Nov 21 Wed Thanksgiving Break
-For those interested doing well on the Semester Exam, the Review Ch 1-7 is online as of Nov 14, 2007. This is a good opportunity to do some advance planning preparing for the semester exam.
Nov 22 Thur Break
Nov 23 Fri Break
Nov 26 Mon -Begin Ch 7 p.203-210 
-Cooperative Learning "Three Minute Pause" 
-p.235 #1-8
Nov 27 Tues Same as Monday
Nov 28 Wed Ch 7 p.211-219
-p.215 #1-3,4(a-e)
-p.235 #9-19
Nov 29 Thur Same as Wednesday
Nov 30 Fri Ch 7 p.221-228
-p.236 #26-30,32-36
Dec 3 Mon Ch 7 p.229-233
-p.237 #36-39
-p.233 #1-5
Dec 4 Tues Same as Monday
-Chambliss Home Christmas Party
Dec 5 Wed Review Ch 7
-Ch 7 Chemistry Review Sheet
-Know all the polyatomic ions (p.210) and be able to use them to write formulas of ionic compounds using the stock system.
-Know the system of naming compounds (nomenclature) for binary compounds as well as acids.
-Know the significance of a chemical formula (p.204)
-Be able to determine the charge of main group elements by their position in the periodic table (p.205)
-Monoatomic and polyatomic ions
-Be able to name binary molecular compounds (p.212)
-Be able to use the rules for assigning oxidation numbers p.216
-Be able to determine the formula mass (molar mass) of any substance.
-Be able to do any calculation indicated in fig 7-4 (eg. mass to moles to formula units or number of atoms)
-Be able to determine a) perecentage composition, b) empirical formulas, c) molecular formulas

Band to Orange Grove Center/AM
Dec 6 Thur Same as Wednesday
Dec 7 Fri Test Ch 7
-p.269 Define Vocabulary -- sections (please # terms). 

-ACT TESTING
Dec 10 Mon Begin Ch 8 p.241-254
-p. 254 #2-5
Dec 11 Tues Same as Monday
Dec 12 Wed Ch 8 p.241-264 
-use cooperative learning (10:5 Kagan--PAIRS CHECK)
-p.270 #18,20-22,25,26,28

-Review Chapter 8

-Chemical reaction
-Know the 5 indications that indicate that a chemical reaction has occurred.
-Coefficient
-Table 8-1 (know all diatomic elements)
-Formula equation
-Table 8-2 Know the table
-Reversible reaction
-Reactants & Products
-Be able to balance equations.
-Know the five types of chemical equations.
-Be able to recognize general reaction types:
a) synthesis: A + B --> AB,
b) decomposition: AB --> A + B,
c) single replacement: A + BX --> AX + B,
d) double replacement: AX + BY --> AY + BX
e) combustion: CH + O2 -> CO2 + H2O
-Electrolysis is the decomposition of a substance by an electric current.


-GCSS Bands Christmas Concert
Dec 13 Thur Same as Wednesday
Dec 14 Fri Mini-Test Ch 8 (Over the last two days information)
-Begin Review for Final Exam
Dec 15 Mon -Continue reviewing for the final examination
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.

Chemistry Final Exam Review

The following is a summary of the concepts over which you will be tested on the exam:
1.  Density (mass, volume) problems
2.  Be able to convert from one metric unit to another (know Table 2-2 p.35)
3.  Be able to convert from Celsius to Kelvin or Kelvin to Celsius
4.  Precision and accuracy
5.  Significant figures (know Table 2-5 and be able to apply to problems)
6.  Be able to determine # of protons, neutrons, and electrons (when provided mass # and atomic #)
7.  Convert from moles to grams and grams to moles (grams to particles and particles to grams).
8.  Determine the number of particles if provided moles or grams of a substance. 
9.  Periodic law (the physical and chemical properties of the elements are functions of their atomic numbers)
10.  Periods and groups (know what they are)
11.  Elements within a group have similar properties 
12.  Metalloids 
13.  Electron configurations 
14.  Ionization energy 
15.  Cations and anions 
16.  Know periodic trend for atomic radius
17.  Chemical bond (ionic, covalent, polar covalent, NOTE: know p.162 Fig 6-2 be able to determine the type of bond based on the % ionic character 0.3 & 1.7)
18.  Valence electrons 
19.  Atoms become more stable (move toward lower potential energy) when they are combined (bonded).
20.  Ionic and covalent bonds 
21.  Nonpolar covalent bonds, polar covalent bonds
22.  Molecule
23.  Bond energy 
24.  Octet (octet rule)  (NOTE:  Noble gases satisfy the noble gas rule without forming compounds) 
25.  Determine the molar mass of compounds
26. Electronegativity
27. Electron affinity
28. Octet rule
29. Quantitative and qualitative observations
30. Scientific notation
31. Halogen, noble gas, alkali metal, alkaline earth metal
32. Know the properties of each group in #31
33. s,p,d,f levels
34. Metals, non-metals, metalloids
35. Ionic character
36. Covalent character
36. Polar covalent

Dec 16 Tues -Semester Exam 11:00 am to 12:30 pm

-Semester Exams, 12:30 PM Dismissal
Dec 17 Wed Semester Exams, 12:30 PM Dismissal
Dec 18 Thur Semester Exams, 12:30 PM Dismissal
Dec 19 Fri Exam Make up Day / Semester Grades Due
    Christmas Break
    Christmas Break
    Christmas Break
    Christmas Break
    Christmas Break
    Christmas Break
    Christmas Break
Jan 7 Mon School Resumes
Begin Ch 9 p.275-287
-p.287 #2-5
Jan 8 Tues Same as Monday
Jan 9 Wed -Ch 9 p.288-292
-p.289 #1,2 Practice
-p.291 #1,2 Practice
Jan 10 Thur Same as Wednesday
Jan 11 Fri -Continue Limiting and Excess concepts (work p.289 & 291 for students in class)
-p.297 #22-27
Jan 14 Mon -Quiz Excess & Limiting Reactants (12 pts)
-Grade quiz in class
-Dry Lab Limiting and Excess reactants
-students may retake today's quiz next period (the new quiz score will be allowed to replace today's score)
Jan 15 Tues Same as Monday
Jan 16 Wed -Ch 9 p.293-294
-p.297 #28-29
-p.296 #10-15
-p.294 #4
Jan 17 Thur SNOW DAY!!! NO SCHOOL!!!
Jan 18 Fri Same as Wednesday
-Thursday classes meet
Jan 21 Mon No School
Jan 22 Tues -NOTE: Those attending prayer conference next Wed-Fri need to take Ch 9 Test before they leave for the conference.

Chapter 9 Review Sheet Chemistry

-Stoichiometry
-Reaction stoichiometry
-Composition stoichiometry
-Balanced equations provide mole to mole ratios for any substances in the equation.
-Coefficients provide relative #’s of moles of reactants and products
-By knowing the mole ratios, the mass of the reactants or products can be determined.
-Be able to determine the mole ratios for any reaction (note: the equation must be balanced).  P.S. There will be several of this type of question.
-Be able to convert from moles of one compound to moles of any other compound. (mole to mole conversions).  P.S.  There will be several of this type of question.
-Be able to convert from moles to grams.
-Be able to convert from grams to moles.
-Be able to convert from grams to grams.
-Percent yield questions.
-Know the definition of percent yield.
-It is usual to produce less product than is theoretically possible.
-Assuming 100% efficiency, the maximum product that can be obtained from a chemical equation is called the theoretical yield.
-Actual yield is equal to theoretical yield when yield is 100%
Jan 23 Wed Same as Tuesday
Jan 24 Thur Test Ch 9 
-p.326 Define Vocabulary (all sections) NOTE: Please # all terms.
-NOTE: Those attending prayer conference next Wed-Fri need to take Ch 9 Test before they leave for the conference.
Jan 25 Fri -Mon/Wed classes meet
Same as Thursday
Jan 28 Mon Begin Ch 10 Sections 1 & 2 PowerPoints
-p.327 #1-19
-Study p.303-304 (Know the five assumptions of the Kinetic-Molecular Theory of Gases) for a quiz next period.
Jan 29 Tues Same as Monday
Jan 30 Wed -Quiz over five assumptions of the Kinetic-Molecular Theory of Gases (10pts)
-Gas Law (Charles) Lab
-Do a full lab write-up
Jan 31 Thur Same as Wednesday
Feb 1 Fri Ch 10 Section 3 PowerPoint
-p.328 #20-30
Feb 4 Mon Reinforce Ch 10 concepts
-p.328 #31-38
Feb 5 Tues Grades due/ PM
-Same as Monday
Feb 6 Wed Ch 10 More Practice
-p.329 #39-50
Feb 7 Thur Same as Wednesday
Feb 8 Fri Review Ch 10 

Chemistry Review Ch 10

  1. Kinetic Theory—particles are always in constant motion.
  2. Kinetic Theory—explains the behavior of all types of matter.
  3. Real gases have forces of attraction between them.
  4. Ideal gas – is an imaginary gas that behaves according to all the assumptions of the kinetic theory a) Gases consist of large numbers of tiny particles that are far apart relative to their size.  b) Collisions between gas particles and between particles and container walls are elastic collisions. c) Gas particles are in continuous, rapid, random motion.  They therefore possess kinetic energy, which is energy of motion. d) There are no forces of attraction or repulsion between gas particles. e) The average kinetic energy of gas particles depends on the temperature of the gas.
  5. Totally elastic collision—is one where there is no net loss of kinetic energy.
  6. Expansion (the process by which gases take on the shape of their container), fluidity (the ability to flow), low density, compressibility (particles which are far apart are crowded together), diffusion (spontaneous mixing of the particle of two substances caused by their random motion) and effusion (the process by which gas particles pass through a tiny opening).
  7. Pressure is the force per unit area on a surface.  The SI unit for force is the Newton (N). 
  8. Barometers are used to measure atmospheric pressure.
  9. Know that 1 atm = 760 mm Hg = 760 Torr = 101.325 kPa = 1.01325 x 105 Pa (NOTE:  Be able to convert from any pressure unit to another pressure unit.)
  10. Know STP (standard temperature and pressure), 0oC and 1 atm.
  11. Be able to work pressure/volume, volume/temperature, pressure/temperature and combined gas law questions.
  12. Know Dalton’s law of partial pressures and be able to solve problems using this law.
  13. Be able to use a chart for water vapor pressure and solve problems regarding the collection of gas above a liquid.
    14. Be able to identify Boyle's, Charles's, Gay-Lussac's and Combined gas laws.
Feb 11 Mon Test Ch 10
-p.356 Define Vocabulary (all sections, please # all terms)
Feb 12 Tues Same as Monday
Feb 13 Wed -Begin Ch 11 Section 11.1 & 11.2
-p.357 #11-17
Feb 14 Thur Valentines Day
-Same as Wednesday
Feb 15 Fri -Chapter 11 Section 11.3
-p.358 #18-20
-p.358 #23-26
Feb 18 Mon No School
Feb 19 Tues -Ch 11 Section 11.4
-p.359 #39-42
-p.358 #27-30
Feb 20 Wed Same as Tuesday
Feb 21 Thur -Review Ch 11

-p.359 #43,45-51
Chemistry Review Ch 11

  1. Gay-Lussac's law of combining volumes says that at constant temperature and pressure, the volumes of gaseous reactants and products can be expressed in small whole number ratios.
  2. The law of combining volumes applies only to samples of gases at under the same conditions.
  3. Be able to write and balance equations to be used for determining volumes of reactants and products.
  4. Avogadro states that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules.
  5. Under constant conditions, gas volume is directly proportional to the number of moles of a gas.
  6. Standard molar volume is 22.4 L, it is the volume occupied by 1 mole of a gas at STP, it is the same for all gases at STP.
  7. Be able to use the ideal gas law, PV = nRT (be able to rearrange it to isolate any of the variables) to solve problems.
  8. Be able to calculate the Molar Mass of any gas using: M = mRT/PV
  9. The ideal gas law is equivalent to Charles’s law when the numbers of moles and the pressure are constant.
  10. Know the value for R (0.0821 L*atm/mol*K)).
  11. The coefficients in a chemical equation (for reactants and products that are gases) indicate the volumes of the gases.
  12. Avogadro’s law indicates that equal volumes of gases contain equal numbers of molecules (this is another way of stating #4).
  13. Be able to do gas stoichiometry questions.
  14. Be able to solve questions using Graham’s law of effusion (rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses).
Feb 22 Fri Same as Thursday
Feb 25 Mon -Test Ch 11
-p.387 Ch 12 Define Vocabulary (all sections, please # all terms) 
Feb 26 Tues Same as Monday
Feb 27 Wed -Begin Ch 12 Section 12-1
-p.388 #1-10
Feb 28 Thurs Same as Wednesday
Feb 29 Fri Leap Year
-Ch 12 Section 12-2
-p.388 #11-17
Mar 3 Mon Spring Break
Mar 4 Tues Spring Break
Mar 5 Wed Spring Break
Mar 6 Thur Spring Break
Mar 7 Fri Spring Break
Mar 10 Mon -Review 12-1 & 12-2 using PowerPoint
-Work sample problems to illustrate today's assignment
-p.389 #18-23
Mar 11 Tues Same as Monday
Mar 12 Wed -Quiz over p.389 #18-23
-Sections 12-3 & 12-4 PowerPoint
-Practice Ch 12 problems in class
-p.389 #27-31
Mar 13 Thur Same as Wednesday
Mar 14 Fri Review Ch 12
-A fluid is a substance that can flow and therefore take the shape of its container.
-Know the five properties of liquids: a) relatively high density, b) relative incompressibility, c) ability to diffuse, d) surface tension, e) evaporation and boiling, f) formation of a solid (solidification/freezing).
-Gases have more energy than liquids
-Liquids have more energy than solids
-Intermolecular forces in liquids include London dispersion forces, hydrogen bonding, and dipole-dipole attractions
-Solids have strong enough attractive forces to hold particles in fixed positions (liquids and gases do not)
-Particles in gases are far apart, liquids closer together and the closest together in solids
-When liquid particles have enough kinetic energy--they may escape to the gas state
-If the average kinetic energy of a liquid decreases enough--it will solidify/freeze
-Particles in a solid can vibrate weakly around fixed positions
-Solids have the strongest forces of attraction when compared with liquids or gases
-Gases then liquids then solids (in order of the greatest to least amount of energy present in their particles)
-Gases then liquids then solids (in order farthest apart to closest together)
-Gases then liquids then solids (in order of least attractive forces to strongest attractive forces)
-Solids have a definite volume because their particles are held in fixed positions
-Gases then liquids then solids (in order of most compressible to least compressible)
-Gases have no definite shape or volume
-Liquids have no definite shape but have a definite volume
-Solids have a definite shape and volume
-Crystalline solids have a definite melting point
-Crystalline solids can exist of single crystals & their particles are held in relatively fixed positions
-Amorphous solids have particles that occur in random patterns
-Examples of amorphous solids include glass and plastic
-Know the four types of crystals a) Ionic Crystals -- positive and negative ions arranged in regular patterns, they are hard and brittle, and have high melting points and are good insulators, b) Covalent Network crystals -- each atom is covalently bonded to its nearest neighboring atoms. This bonding occurs throughout a large number of atoms. They are hard and brittle with high melting points and are usually nonconductors or semiconductors, c) Metallic Crystals -- are metals atoms surrounded by a sea of electrons, they are excellent conductors of electricity due to the freedom of the outer electrons to move through the crystal, d) Covalent Molecular Crystals -- are covalently bonded molecules held together by intermolecular forces, they tend to be easily vaporized, are relatively soft, and are good insulators
-Equilibrium is when two opposing processes occur at equal rates
-Molecules can escape the surface of a liquid when their energy is sufficient to break free from the attractive forces of the liquid
-Equilibrium vapor pressure of a liquid is the pressure exerted by a vapor in equilibrium with its liquid at a given temperature
-Volatile liquids tend to have weak attractive forces and evaporate easily
-Equilibrium vapor pressures for water correlate directly to the temperature of the water
-The higher the altitude, the less the atmospheric pressure
-Water boils at lower temperatures at higher altitudes due to the decreased atmospheric pressure
-When water boils -- the temperature of the water remains constant
-During the process of freezing, a liquid loses potential energy
-Be able to work problems using molar heat of vaporization and molar heat of fusion
Mar 17 Mon -Test Ch 12
-p.419 Ch 13 Define Vocabulary (all sections, please # all terms)
Mar 18 Tues Same as Monday
Mar 19 Wed -Lab "Charles Law" use syringes to demonstrate how temperature changes bring about changes in volume
-Do a full lab write up

-NOTE: Please always use this pattern for all lab reports. See Aug 3

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

-NOTE: You may find p.841 "How to Write a Laboratory Report" found in the Physical Science textbook helpful to look at as well.
Mar 20 Thur Same as Wednesday
Mar 21 Fri No School, Staff Development
Mar 24 Mon -Begin Ch 13 PowerPoint Section 1  
-p.420 #1-12
-NOTE: Spring Week of Prayer Mar 24-28
Mar 25 Tues Same as Monday
Mar 26 Wed -p.816 Experiment 9-1 "Mass and Mole Relationships in a Chemical Reaction" 
-p.818 Analysis and Interpretation #1-6
-p.818 Conclusions #1-2
-Do a complete Lab write up (NOTE: See march 19 web page)
Mar 27 Thur Same as Wednesday
Mar 28 Fri -Chapter 13
-Introduce molarity concept and problem solving using molarity.
-p.420 #13-22
Mar 31 Mon -Chapter 13
-Use entire class for completing p.420 #13-22
-Introduce molality concept and problem solving using molality.
-p.421 #23-28, 30-32
Apr 1 Tues Same as Monday
Apr 2 Wed -Continue working on p.421 #23-28, 30-32 (turn in by the end of the class period)
-Begin to review (after completing & turning in the assignment)
Apr 3 Thur Same as Wednesday
Apr 4 Fri Review Ch 13

Chemistry Review Ch 13

  1. Homogeneous --
  2. Heterogeneous
  3. Soluble
  4. Solution
  5. Solute
  6. Solvent
  7. Table 13-1 (be familiar with various solute-solvent combinations for solutions)
  8. Know three types of mixtures and their characteristics (table 13-3)
  9. Table 13-2 (only liquid aerosol, where liquid is dispersed in a gas)
  10. Tyndall effect – when light is scattered by colloidal particles dispersed in a transparent medium.
  11. Metal solutions are alloys.
  12. Electrolytes (solutions that conduct electricity—they contain ions) example sodium chloride or any other ionic compound.
  13. Electrolytes ionize in water.
  14. Nonelectrolytes (solutions that do not conduct electricity—they do not contain ions). An example is sugar.
  15. Know three factors which increase the rate of dissolving: a) increasing the surface area of the solute, b) agitating the solution, c) heating a solvent. P.401-402
  16. Temperature is a measure of the average kinetic energy of the particles.
  17. Stirring increases the rate of dissolution because it brings fresh solvent into contact with the solute.
  18. Solution equilibrium – is the physical state in which the opposing processes of dissolution (the process by which a solid, gas, or liquid is dispersed in a gas, solid, or, a liquid to form a solultion)and crystallization of a solute occur at equal rates.
  19. Saturated – is a solution that contains the maximum amount of dissolved solute.
  20. Unsaturated – A solution that contains less solute than a saturated solution under the existing conditions.
  21. Supersaturated – is a solution that contains more dissolved solute than a saturated solution contains under the same conditions (can be obtained by heating and dissolving the maximum amount of solute and then cooling the filtered solution).
  22. Solubility of a solute depends upon the temperature of the solvent.
  23. Like dissolves like refers to the similarity in molecular polarity.
  24. Carbon tetrachloride is a nonpolar solvent.
  25. Know the energy changes according to fig 13-16 p.409 during the formation of a solution (a) solute particles becoming separated from a solid = energy absorbed, b) solvent particles being moved apart to allow solute particles to enter a liquid = energy absorbed, c) solvent particles being attracted to and solvating solute particles = energy released).
  26. Know the effect of temperature on solubility of solids in liquids and on gases in liquids.
  27. Hydration – the solution process with water as the solvent is hydration.
  28. Hydrates -- when crystallized from aqueous solutions, some ionic substances form crystals that incorporate water molecules.
  29. Solvated – a particle that is surrounded by solvent molecules.
  30. Immiscible – Liquid solutes and solvents that are not soluble in each other.
  31. Miscible – Liquids that dissolve freely in one another in any proportion are miscible.
  32. Henry’s law – The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas on the surface of the liquid.
  33. Effervescence is the escape of gas from a gas-liquid solution.
  34. Heat of solution is the net amount of heat absorbed or released when a specific amount of solute dissolves in a solvent. It is expressed in kilojoules per mole of solute at a specified temperature.
  35. Pressure has its greatest effect on solubility of gases in liquids.
  36. Concentration – is a measure of the amount of solute in a given amount of solvent or solution.
  37. Molarity (M) = moles of solute / L of solution
  38. Molality (m) = moles of solute / kg of solvent
  39. Be able to work problems with molarity and molality.
Apr 7 Mon -Test Ch 13
-p.447 Define vocabulary (all sections) 
Apr 8 Tues Same as Monday
Apr 9 Wed -Begin Ch 14 PowerPoint Section 14-1 (up to slide #15)
-Provide examples to illustrate freezing point depression and boiling point elevation problems (include electrolytes). Do the following questions for fp & bp.
-p.441 #1-4 (do in class together)
-p.445 #1-3 (do in class together)
-p.447 #1-8
Apr 10 Thur Same as Wednesday
Apr 11 Fri -Video #25 Chemistry and the Environment
-(take notes--numbered, point form--about 15 ideas from the video)
-ACT TEST
-Noon Dismissal Alumni Weekend
Apr 14 Mon -SIGN UP FOR ICE CREAM LAB WED/THUR
-p.440 #1-4
-p.441 #1-4
-Art/Cooperative Learning (20pts)
-Using a poster paper provided you are to make a group (or individual drawing of any of the following figures or single figure if it is complicated)
-1) Figures 14-1 & 14-3
-2) Figure 14-5
-3) Figures 14-6 & 14-7
-4) Figures 14-8 & 14-9
-NOTE: Each group/individual drawing will be graded for both neatness and accuracy. You must include a brief explanation for each of the figures (the descriptive heading included in the text with each drawing is acceptable).
-NOTE: It would be best if you would choose a concept that you find difficult and it shoud help you to visualize the idea by doing a drawing about it.
-NOTE: Each person must remain active during the class period until the project is completed. If the project is not completed during class, you may take it home but it is due the next class period.
-NOTE: Colored pencils and paper are provided.
Apr 15 Tues Same as Monday
Grades Due, PM
Apr 16 Wed

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 0 Celsius due to the presence of dissolved sugars.) This process is a lesson in heat transfer in itself!

Apr 17 Thur Same as Wednesday
Apr 18 Fri -p.445 Practice #1-3
-Complete the art/chemistry cooperative learning poster
-Introduce the effect of electrolytes on colligative properties & work p.444 Sample problem 14-6
Apr 21 Mon

Chemistry Review Sheet Chapter 14

  1. Dissociation
  2. Ionization
  3. Be able to determine the number of ions produced from dissolving one mole of a solid that dissociates.
  4. Remember that the right side of a dissolving equation shows the charge and the symbol (aq).
  5. Double-replacement reactions may result in a precipitation reaction.
  6. Be able to use the general solubility guidelines to determine whether pairs of solutions will produce any precipitate.
  7. Net ionic equation (be able to recognize and determine the reaction)
  8. Spectator ions
  9. Molecular compounds may contain non-polar covalent or polar covalent bonds.
  10. The attraction of water molecules overcomes the strength of covalent bonds in molecular compounds that are electrolytes.
  11. Hydronium ion (H3O+) is a hydrated proton.
  12. Strong electrolyte
  13. Weak electrolyte
  14. Colligative properties depend upon the concentration of the solute particles.
  15. Vapor pressure lowering, freezing point depression, boiling point elevation and osmotic pressure are all colligative properties since they all depend upon the concentration of solute particles in a solution
  16. Be able to work problems with boiling point elevation and freezing point depression with non-electrolytes and electrolytes.  NOTE:  Be able to solve for any variable in the equations. 
  17. Be able to compare the effect of a non-electrolyte with an electrolyte.
  18. Electrolytes produce more than one mole of particles per mole of solute as compared with non-electrolytes.  
Apr 22 Tues Same as Monday
Apr 23 Wed -Test Ch 14 
-p.476 Define Vocabulary (all sections) NOTE: Please # all term
Apr 24 Thur No School, Staff Development
Apr 25 Fri No School, Staff Development
Apr 28 Mon -Begin Ch 15 Section 1 & 2 PowerPoint up to slide #16
-p.477 #1-9
Apr 29 Tues Same as Monday
Apr 30 Wed Ch 15 Section 3 PowerPoint up to slide # 22
-p.477 #10-16
May 1 Thur Same as Wednesday
May 2 Fri Video #15The Busy Electron (electrochemical cells)
-Use point form to record any 15 ideas you learned from the video. (15pts)
-NOTE: In order to promote increased performance on the final exam, there is no assignment for today or Mon/Tues May 5-6. PLEASE BEGIN TO STUDY NOW FOR THE FINAL EXAM!!!!!!
May 5 Mon Video #16 The Proton in Chemistry (pH, acids and bases)
-Use point form to record any 15 ideas you learned from the video. (15pts)
May 6 Tues Same as Monday
Spring Choir Concerts
May 7 Wed -p.477 #17-23,26-28
-Continue Ch 15 (Reviewing sections 1,2, & 3)
-clarify any questions for problem solving
May 8 Thur Same as Wednesday
May 9 Fri Chapter 15 Review 
p.454 Know the five properties of acids:  a)  sour taste, b) turn pH paper red, c) produce hydrogen when reacting with active metals, d) react with bases to produce salt and water, e) some acids are electrolytes 
p. 454 Binary acid – is an acid that contains only two different elements: hydrogen and one of the more electronegative elements. 
p. 454 Be able to recognize a binary acid. 
p.455 Know the rules for naming a binary acid.
-a) The name of a binary acid begins with the prefix hydro-, b) The root of the name of the second element follows this prefix, c) The name then ends with the suffix –ic. 
p.455 Oxyacid – is an acid that is  a compound of hydrogen, oxygen, and a third element, usually a nonmetal. 
p.456 Know the five common industrial acids and their uses and properties: 
-Sulfuric – is manufactured in largest quantity of any acid.  It is the most commonly produced industrial chemical in the world.  It is used in automobile batteries. 
-Nitric – is used in making explosives, rubber, plastics, dyes, and pharmaceuticals (drugs). 
Phosphoric Acid – is used for manufacturing fertilizers, flavoring beverages and in making detergents. 
-Hydrochloric acid – is produced in the stomach to aid in digestion. 
-Acetic acid – white vinegar is 4-8 % acetic acid.
p.457 Know the five properties of bases:  a) bitter taste, b) turn pH paper blue, c) are slippery in dilute solutions, d) react with acids to produce salt and water, e) are electrolytes (conduct electricity). 
p.459 Arrhenius acid – is a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution. 
p.459 Arrhenius base – is a substance that increases the concentration of hydroxide ions, OH-, in aqueous solution. 
p.460 Strong acid – is one that ionizes almost completely in aqueous solution to produce H3O+ (it is an electrolyte). 
p.461 Strong base – is one that dissociates almost completely in aqueous solution (it is an electrolyte).
p.464 Bronsted-Lowry acid – is a molecule or ion that is a proton donor. 
 Know example:  HCl + H2O à H3O + Cl-  (be able to identify BL acid or base) 
p.465 Bronsted-Lowry base – is a molecule or ion that is a proton acceptor. 
p.465-466 Be able to recognize a mono, di or triprotic acid. 
p.465 Monoprotic acid – an acid that can donate only one proton (hydrogen ion) per molecule. 
p.465 Polyprotic acid – is an acid that can donate more than one proton per molecule. 
p.466 Diprotic acid – is an acid that can donate two protons per molecule.
p.466 Triprotic acid – is an acid that is able to donate three protons per molecule. 
p.467 Lewis acid – is an atom, ion, or molecule that accepts an electron pair to form a covalent bond.    The Lewis definition is the broadest of the three definitions for acids and bases. 
p.468 Lewis base – is an atom, ion, or molecule that donates an electron pair to form a covalent bond. 
p.469 Conjugate acid – The species that is formed when a Bronsted-Lowry base gains a proton is the conjugate acid of that base. 
p.469 Conjugate base – The species that remains after a Bronsted-Lowry acid has given up a proton is the conjugate base of that acid. 
p.471 Amphoteric – is any species that can react as either an acid or a base. 
p.475 Neutralization – is the reaction of hydronium ions and hydroxide ions to form water molecules.
p.475 Salt – is an ionic compound composed of a cation (metal) from a base and the anion from an acid. 
May 12 Mon Test Ch 15 
-p.546 Define Vocabulary (all sections), please number all terms
May 13 Tues Same as Monday
May 14 Wed -Begin Ch 16 Section 1 PowerPoint up to slide #10
-p.505 #15-19
May 15 Thur Same as Wednesday
May 16 Fri Review for Final Exam

Chemistry Final Exam Review Chapters 8-11,13,14

Ch 8
-p.241 Know the four indications that a chemical reaction has taken place
-precipitate
-know the diatomic molecules
-subscript & superscript and coefficients