Web Publishing: The Foote School

IPS Assignment Sheet

All work is due the period following its assignment date. Please be sure to bring your text book and lab journal to class every day.

Thursday, May 23: Write the Discussion section of your report, leaving blank spaces for any information you haven't yet gathered or verified. Follow the guidelines given in your sludge packet (and copied below). In addition, be sure that you have updated your abstract and data chart. Remember, ALL written work is to be done independently of your lab partner. You were to have recorded data on the day that it was taken.

Section 4: Discussion. Follow the basic format we have been using. At a minimum, include the following four things: 1). Give background information on important concepts such as characteristic properties and mixtures vs. pure substances. 2). Identify the pure substances in your mixture then support your reasons for those identifications. 3). Include a discussion of possible errors and problems, but make sure this relates directly to your experiments and the reliability of your results. 4). Include any follow up questions and issues, e.g. experiments that could not be performed but which would have strengthened your conclusions. This section should be in narrative form (please use paragraphing, not bullet points). Keep it objective and scientific (avoid the use of pronouns, for example and remember that this is a formal lab -- no slang, etc). A strong discussion section is important.

Your completed sludge report is due on Friday, May 31.

Tuesday, May 20: Intermediate Assignment

Please summarize your current sludge data and observations, categorized by isolated material. Following are examples of summaries that might be given for a solid and a liquid. You are likely to have other qualitative and quantitative information in your summary.

Solid 1 (Tentatively identified as Pretendium)

Solubility: Soluble in water, insoluble in etOH

Melting Point; 46 degrees C

Appearance: white crystalline powder

Other: Magnetic, conducts electricity

Liquid 1 (Not yet identified)

Flammability: flammable

Solubility: Dissolves sugar & Citric acid, Does not dissolve TOP

Boiling Point: 52 degrees C

Appearance: Clear liquid

Also, please review in your sludge packet the requirements for your written abstract. Even though you have not finished identifying your materials, you will be required to have an abstract draft by next Thursday.

Thurs. April 25: Prepare Experiment 6.2: The Decomposition of Water

Purpose: To decompose water into its elements and to distinguish between them.

April 19: Learn the symbols for the following elements

Metals Metals ,Cont.

Lithium Li Cadmium Cd

Sodium Na Mercury Hg

Potassium K Aluminum Al

Beryllium Be Germanium Ge

Strontium Sr Antimony Sb

Barium Ba Bismuth Bi

Titanium Ti Non-metals

Chromium Cr Carbon C

Molybdenum Mo Silicon Si

Tungten W Nitrogen N

Plutonium Pu Phosphorus P

Manganese Mn Arsenic As

Nickel Ni Selenium Se

Platinum Pt Tellurium Te

Copper Cu Polonium Po

Silver Ag Fluorine F

Mon. April 15: Read Section 5.7: A Mixture of Gases, Nitrogen and Oxygen, p. 102 and 5.8: MIxtures and Pure Substances, p. 103. Answer Q. 18 - 24, pp. 103 - 106.

Wed. Feb. 27: Please see notes below from our quick exploration of acid/base chemistry:

Your Unit 4 test will take place over two days. The laboratory practical portion of the test will be Friday,Mar. 1 and the written portion will be Mon., March 5. You can use your lab book and your text on both portions.

Feb. 19: In class we'll investigate the solubility of four solutes in two different solvents.

H.W. Leave space (one full page) for a post-laboratory discussion, then prepare the next lab, Experiment 4.7: The Solubility of Carbon Dioxide. Purpose: To measure the solubility of Carbon Dioxide by dissolving a known mass of the gas into a known volume of water.

Here are notes from today's review:

What have we learned about solutions?

*Some new vocabulary (solute, solvent, solubility, dilute, concentrated, saturated, precipitate, concentration)

*That the process of dissolving falls somewhere between a chemical process and a physical process

*Concentration is a ratio of the amount of solute to the amount of solvent

*The preferred unit for concentration is g/100cm³

*Temperature affects the amount of a substance that dissolve

- Some substances are more soluble in warm solvents

- Some substances actually dissolve better in cold solvents (more about this later)

Feb.1: Prepare Experiment 4.4: The Effect of Temperature on Solubility, p. 73.

Purpose: To compare the solubilities of two solutes in water as they heat and cool.

(write out a materials list and procedure).

Thurs. Jan. 24: In class we'll finish the the unit three test and discuss crystal shape as a characteristic property. Please prepare Experiment 8.6, page 161 using the info below.

8.6: Flame Color of Some Elements

Purpose: What color do some elements produce in a flame?

Sodium Hydrogen Carbonate

Background information for 8.6:

Major sub-atomic particles in an atom

* Found in the nucleus

* Positively charged

* Massive (mass of 1 atomic mass unit - amu)

* Determines what the element is (see atomic number)

* Found in the nucleus

* Not consistent in number (isotopes of an element contain different numbers of nneutrons)

*Found in clouds around the nucleus

* Not massive (1/2000 the mass of a proton or neutron)

* Same as the number of protons in an uncharged atom

When electrons lose energy and move "down" a shell, a photon of a specific wavelength (hence color) is given off.

Tues. Jan. 22: We'll have a quick review then take the first part of the unit 3 test. Please have the following problems done in advance: Q. 23 and 24, p. 53; Q. 29, p. 56; Q. 36 and 37, p. 61and Q. 43 and 45, p. 64.

Wed. Jan. 16: Test, Unit 3

Tues. Jan. 15: We'll review all of the Unit 3 experiments and complete a test review.

Fri. Jan 11: Post-lab discussion of Experiment 3.9: Freezing and Melting. Here is data from 8X and 8Y and some of our discussion notes:

During melting or boiling, the heat energy goes into the phase change rather than an increase in temperature, hence the temperature "plateaus".

Tues. Jan. 8: In class we'll perform Experiment 3.9: Freezing and Melting

Mon. Jan 7: In class we'll prepare and perform Experiment 3.11: Boiling Point (this is out of sequence). Purpose: Does a small amount of liquid boil at the same temperature as a large amount? (Is Boiling Point a characteristic property?)

H.W. Read section 3.12: Boiling Point and Air Pressure and prepare Experiment 3.9: Freezing and Melting, p. 53. Purpose: Does a small amount of a material freeze at the same temperature as a large amount?

Here is class data from 8X and 8Z, and background notes from today's Boiling Point lesson:

*Isopropyl Alcohol (Isopropanol) = C₃H₇OH

Boiling point = 82 degrees celsius

Boiling point = 100 degrees celsius

*Boiling point is influenced by air pressure: the higher the air pressure the higher the boiling point. At high altitudes water boils more easily (and consequently at a lower temperature)

Thurs. Jan. 3: In class we'll review density by examining popcord kernels in seltzer and trying to explain the resulting phenomena.

Tues. Nov. 27: In class we'll develop experiments relating to the reaction between calcium chloride and sodium hydrogen carbonate, then begin unit three with a density experience.

H.W. Read Section 3.3: Density, p. 44 & 45 and answer Q. 2 & 3, p. 44 (in the back of your book; label the section UNIT 3 but continue where you left off from UNIT 2).

Wed. Nov. 28: In class we'll discuss significant digits and prepare and perform Experiment 3.5: The Density of Solids.

H.W. Be sure you've done the homework for Tuesday (above). Also, read Section 3.4: Dividing and Multiplying Measured Numbers and answer Q. 7 & 8, p. 46 and 11 & 12, p. 48.

Fri. Oct. 19: In class we'll peform Experiment 2.1: The Mass of Dissolved Salt.

H.W. Answer Q. 1 - 5, p. 29.

Mon. Oct. 22: In class we'll have a post lab discussion of Experiment 2.1 and learn to graphically represent the data.

H.W. Prepare Experiment 2.4: The Mass of Ice and Water. Purpose: Is there a change in mass when ice melts to water in a closed system?

Wed. Oct. 23: In class we'll perform Experiment 2.4 and do the post-lab discussion of the material (it's a short lab).

H.W. Prepare Experiment 2.5: The Mass of Copper and Sulfur. Purpose: Is there a change in mass when copper is reacted with sulfur in a closed system? (Remember, when you prepare a lab you're expected to write a purpose, a materials list and a thorough, numbered procedure)

Thurs. Nov. 1: In class we'll erform Experiment 2.5: The Mass of Copper and Sulfur and record individual and class data.

Wed. Nov. 7: In class we'll have a post-laboratory discussion of Experiment 2.5 and prepare and perform Experiment 2.6: The Mass of a Gas

H.W. Please learn the symbols and corresponding names for the following elements:

C= Carbon, H= Hydrogen, N= Nitrogen, O= Oxygen, P= Phosphorus, S= Sulfur

Na= Sodium, Si= Silicon, Cl= Chlorine, Cu= Copper

Mon. Nov. 12: In class we'll have a post-laboratory discussion of Experiment 2.6: The Mass of a Gas.

H.W. Please read carefully Section 2.7: The Conservation of Mass and 2.8: Laws of Nature, pp. 38 and 39 and answer Q. 12 - 18, pp. 36 - 40.

Thurs. Nov15: Quiz on the elements and symbols you were asked to know. Also, we'll go over the material you read and go over your homework from Monday, then review for the Unit 2 test.

Friday, Nov. 16: Short review then Unit 2 test.