9th Grade

Lab Final / Chemicals List

 

Last updated 08/20/08

 

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Lab Final

Dates to be announced later.

 

We will end the year with our famous practical lab final.  The goal for the students is to use all the laboratory skills, knowledge and strategies they have learned during the year to separate the parts of their mixture and positively identify each part.  We will send home more details nearer the time but wish to stress at this time the IMPORTANCE OF ATTENDANCE during the last five weeks of school.  PLEASE try to avoid making vacation plans and medical and other appointments during science class in the last weeks of the school year.  This lab final assessment will be approximately one third of the final quarter’s grade. 

Chemicals List - Purpose

Students are allowed to bring into the lab a reasonable amount of reference material, and a  key skill for success is the ability to choose, organize and use this reference material. 

 

One of the ways we assist the students is to create an ongoing assignment during the year called “The Chemicals List”.  AN ANNOUNCEMENT WILL BE POSTED ON THIS PAGE WHEN WE START THIS ASSIGNMENT. IT WILL ALSO SHOW UP AS AN ASSIGNMENT ON THE 9TH GRADE ASSIGNMENT LIST AT THAT TIME.

 

The students create and continually update and improve a report tabulating the NAMES of all the chemicals  or substances we use during the school year, their FORMULA ( if possible), the PHASE or state of matter seen, categorize as an element, compound or mixture, METAL OR NONMETAL, state the type of chemical bonding and list the PROPERTIES.

 

By repeatedly referring to and improving the report it reinforces learning about the properties of substances and understanding of how they work and interact. Together with the lab notebook, this is one of the most useful references for success in identifying the mixture components in the Lab Final. There will be  "Chemicals List" lessons to assist students in setting up the tabulated report, with examples to model how to record information about each substance.

 

Properties

 

Definition: The characteristics of a substance.

 

These can be categorized  into physical and chemical properties.

 
PHYSICAL PROPERTIES:

A characteristic that distinguishes one type of matter from another and can be observed WITHOUT CHANGING THE IDENTITY OF THE SUBSTANCE.

A physical description of the substance.

CHEMICAL PROPERTIES:

A property that describes how a substance CHANGES INTO A NEW SUBSTANCE.

This involves CHEMICAL REACTIONS.

Is the substance reactive or inert?

 

NO NEW SUBSTANCES!

NEW SUBSTANCES FORMED!

  • Volume

  • Mass

  • Weight

  • Density

  • Color

  • Streak color

  • Luster

  • Transparent

  • Translucent

  • Volatility

  • Smell

  • Taste

  • Texture

  • Shape / form

  • Crystalline structure

  • Cleavage

  • Fracture

  • Hardness

 

  • Solubility

  • pH

  • Boiling Point

  • Freezing Point

  • Melting point

  • Sublimation

  • Viscosity

  • Magnetism

  • Tensile strength

  • Elasticity

  • Flexibility

  • Malleability

  • Ductility

  • Sectility

  • Heat conductivity

  • Electrical conductivity

 

  

 

  • Corrosion?

  • Reaction with water?

  • Flammability / Reaction with oxygen? (Often a synthesis reaction  - Ex: when magnesium reacts with oxygen as it burns in air))

  • Reaction with acids? (these are single replacement reactions)

  • Reaction with bases?

  • Synthesis reactions (like copper reacting with sulfur)

  • Single-replacement reactions

  • Decomposition reactions (like sodium iodide decomposing)

  • Double -replacement reaction (like salt ion exchange reactions)

 

 

 

Chemicals List Guidelines

  1. Keep an updated list of the substances used in our labs in this table.

  2. At the end of the year there will be about 60 items.

  3. Use LANDSCAPE ORIENTATION so that the properties column can be longer.

  4. Open a word document.

  5. Go to File, Page Setup, and the margins tab. Choose landscape orientation and all narrow 0.5cm margins.

  6. Go to table, insert table, choose 7 columns and 5 rows, and click OK.

  7. Click on each vertical line (do not accidentally select any cells or you will only change the widths on those rows) and drag the lines to approximate the column widths shown in the model chemical list table below, but the last column for the properties should be much wider (possible with your landscape orientation).

  8. Select all the cells in the first row, then go to table, and merge cells.

  9. Write "CHEMICALS LIST" capitalized, 12 font, bold, in this first row, and select the center align icon on the toolbar.

  10. Copy the column headings (10 font) shown in the model below, into the second row.

  11. Go to view, then header footer, type in your period and name (Period 2    Jane Doe) and click on the toolbar icon to right align. Then click on close on the header footer toolbar.

  12. Click into the remaining three rows and press enter to increase the size of each row equally until the page is full.

  13. Go to edit and "save as", and name your file, including your initials and the date, as shown in this example:  "Chem. List Master_JD_011408."

  14. Navigate to the location in your computer where you like to store your school work. Click on the "new folder" icon and create a new folder called "9th Science 0708." Save this document and any other science work in this folder.

  15. The document you have just created is your MASTER. Print off a copy each time you need a blank new page.

  16. The chemicals list is to be HANDWRITTEN. Why? Too many students are tempted to copy and paste from a friend on this assignment - plagiarized documents.  I need to see your own work.

  17. For each substance, write in the name, formula (if possible), check in the S, L and G columns whether you have seen it in the lab as a solid, liquid and /or gas.

  18. In the last column write first if the substance is one element or a compound or a mixture. Then state if it is a metal , nonmetal or both. Look at the formula to  identify the bonding (N-N is covalent; M-M is metallic; M-N is ionic). Using your general knowledge and our lab work add the physical and chemical properties you currently know. You can subdivide this wide column into two columns and use a list format. Some students divide it into two for physical and chemical properties. Write small and neatly. Leave a gap to add more information you might gain during later labs.

  19. This is an ongoing document you will continually update until the lab final in June.

  20. By listing the properties of each substance you will gain more understanding of the properties of matter, how they help our understanding of its behavior and be able to use properties to identify substances. You will find this easier with time as you gain practice in making the entries.

  21. Keep your writing legible.

  22. To summarize  - the table includes:

·         The NAMES of all the chemicals or substances.

·         Their FORMULA (if possible).

·         The PHASE or state of matter seen (solid, liquid, gas)

·         Whether it is an element, compound or mixture; metal or nonmetal; and the type of chemical bonding.

·         The physical and chemical PROPERTIES.

  1. Model: We will work together in class to brainstorm the properties of the first four or five substances using our properties list sheet to help jog our memories.

  2. Students will complete the entries for all other substances we use in the labs throughout the year. There will be about 60 substances.

  3. You may collaborate with your peers by discussing the properties of these substances with your lab partners. YOU MAY NOT COPY EACH OTHER’S TABLE/WORK.

  4. The information for the properties for each substance on your chemicals list can be collected by taking good notes in class during lessons and labs.

  5. Only add information about properties we have covered in class that you would be able to demonstrate or test in our laboratory.

  6. Chemical List Research: If you would like to do some extra research to prompt your memory and check your notes, try using a chemistry dictionary or the Internet. 

  7. Here are some websites recommended by students:

    If you find a good website or book resource, please let us know so we can add it to this list.

  8. DO NOT add information and numbers from the internet that you do not understand, and/or that we cannot test in our own lab with our own equipment. Points will be deducted for this. 

  9. Be ready to bring your updated chemicals list for grading on any given due date. Keep it in your binder. Keep it up-to-date.

Chemicals List

(approximately 60 items by the end of the year)

 

The chemicals in the cells already in yellow should be entered into your chemicals list.

The chemicals in the cells in white will be added as they are introduced in future labs.

 

Students hand write the details in the last column into their chemicals list. Only the first four are modeled here for reference.

 

#

 NAME FORMULA S L G

  • Compound or element? Or a mixture?

  • Metal or nonmetal?

  • Type of bonding? (N-N is covalent;  M-M is metallic; M-N is ionic)

  • Properties? (Physical/Chemical)
1 Water H20 * * *

COMPOUND

NON-METAL

COVALENT BONDING when pure.

 

Physical properties

  • Liquid at room temperature.

  • Colorless. Odorless. No taste.

  • Low viscosity (runny).

  • Density of 1.0g/cm3.

  • pH of 7 (neutral).

  • Good solvent - called the "Universal Solvent."

  • .

  • .

  • .

  • Boiling point of 100oC.

  • Freezing/Melting point of 0oC.

  • Conducts electricity when any salt impurity is present.

Chemical properties

  • Reacts violently with Sodium (Na) and Potassium (K) - the alkali metals as seen in video demonstration. (However we no longer show these reactions in the classroom lab for safety reasons).

  • Corrodes Iron (Fe) to rust (iron oxide - Fe2O3).

2 Iron

(Add info from the Single replacement reaction lab after 4/10)

 Fe * . .

ELEMENT.

METAL

METALLIC BONDING.

  • Density of 7.87g/cm3.

  • Grey metal.

  • Shiny luster.

  • MAGNETIC.

  • Malleable. Ductile. Sectile. Flexible.

  • Conducts electricity.

  • Melting point and Boiling point too high for classroom lab testing.

  • Corrodes in the presence of water and oxygen to form rust (iron oxide - Fe2O3).

  • Reacts slowly with acids to form hydrogen gas

3 Sulfur S * . .

ELEMENT.

NON-METAL

COVALENT BONDING.

  • Solid at room temperature.

  • Yellow.

  • Brittle.

  • Pure sulfur has no odor but it seems to have a distinct smell that is really sulfur dioxide, formed when sulfur comes into contact with oxygen and water.

  • Density is 2.07g/cm3.

  • Melting point 113oC. Boiling point 447oC. (Can melt and vaporize in a test tube using an alcohol flame. We use a rubber dam to reduce exposure to vapors).

  • Reacts with copper powder when heated to form black copper sulfide.
4

Sodium Chloride

(table salt)

 

 

NaCl

 		 * . .

COMPOUND of a metal and nonmetal

METAL and NON-METAL

IONIC BONDING

·         Color- transparent white

·         Characteristic salty taste (DO NOT TEST in the lab)

·         Melting point extremely high. (Cannot melt using an alcohol burner)

·         Crystalline structure-cubic. Generally small, giving a gritty texture.

·         Dissolves in water

·         Will conduct electricity when melted or in solution.

·          Flame color test -yellow (for the sodium)

·         Reacts with lead nitrate to form insoluble white lead chloride (white precipitate)

·          Acid resistant
5

Ethyl alcohol (ethanol)

CH3CHOH

.

*

*

 

 

 

 
6

Lauric acid

 

CH3(CH2)10COOH

 

 * * .  

 

 
7

Naphthalene

 

C10H8

 

 * * .  

 

 
8 Para-dichlorobenzene (PDB)

 

 C6H4Cl2 * * .  

 

 
9 Stearic Acid CH3(CH2)16COOH

 

 * * .  

 

 
10

 

Aluminum

 

Al

*

.

.

  
11 Iodine I2 * . *  

 
12

Methyl Alcohol

(Methanol)

CH3OH

.

*

*

 

 

 
13

Glycerin

C3H8O3

.

*

.

 

 

 
14

Sucrose

(table sugar)

 

C12H22O11

 

*

.

.

COMPOUND / nonmetal / COVALENT BONDING

Physical Properties:

Appearance? (lab)

crystalline shape? (lab)

Solubility? (general knowledge and research)

Melting point? (research)

 

Chemical Properties:

Flammable? Reaction with Oxygen? (lab)

 
15

Sodium bicarbonate

(baking soda)

NaHCO3

 

*

.

.

COMPOUND / metal and nonmetal / COVALENT AND IONIC BONDING

Physical Properties:

Appearance? (lab)

Solubility in water?

pH? (research)

Flame test color? (lab)

 

Chemical Properties:

Reaction with acids? (acids reactions lab)
16

Magnesium Sulfate (Epsom Salts)

 

MgSO4

 * . .  
17

Citric acid

 

C6H8O7.H2O

 * . .  

 
18 Copper

(Flame test lab, Synthesis reaction lab  / Single replacement reaction lab)

 Cu * . .

Element / metal / Metallic  bonding

Physical Properties:

Density? Research.

Color?

Luster of the metal and its powder?

Shape / form?

Hardness?

Solubility?

Melting point? Too high to use in our lab.

Magnetism?

Malleability? etc

Heat conductivity?

Electrical conductivity?

Flame test color?

Chemical Properties:

Corrosion? Use your general knowledge.

Reaction with water?

Reaction with Oxygen?

Reaction with sulfur? enter after the synthesis reaction lab

Reaction with acids? Enter after the single replacement lab
19

Sodium Iodide

NaI

 * . .  

 
20 Charcoal C * . .  

 
21

Sodium Carbonate

Na2CO3

 * . .  

 
22

Cuprous (copper II) Chloride

CuCl

 * . .  

 
23

CopperII Sulfate

 

CuSO4

 * . .  

 
24

Cobaltous Sulfate

CoSO4

 * . .  

 
25

Ferric (iron III) Oxide (rust)

Fe2O3

 * . .  

 
26

Calcium Chloride

CaCl2

 * . .  

 
27

Ferrous (iron II) Sulfate

FeSO4

 * . .  

 
28

Lithium Carbonate

Li2CO3

 * . .  

 
29

Strontium Chloride

SrCl2

 * . .  
30

Magnesium Carbonate

MgCO3

 * . .  

 
31

Lithium Chloride

LiCl

 * . .  

 
32 Ammonium Chloride NH4Cl * . .  

 
33

Paraffin Wax

 

Hydrocarbon with a high molecular weight.

*

*

.

 
34

Calcium Carbonate  (chalk, shell, marble)

 

CaCO3

 

 * . .  
35

 

Magnesium

(synthesis reaction lab and single replacement reaction lab)

 

 Mg * . .  
36

Starch (or starch in water solution)

Decomposition reaction lab.

Very long polymer (chain) of glucose molecules (C6H12O6)

 *      
37

Lead Nitrate

(Double replacement reaction lab)

 

 Pb(NO3)2 * . .  
38

Zinc

(single replacement reaction lab )

 

 Zn * . .  
39

Hydrochloric acid in solution (single replacement reaction lab)

 HCl

 

   *    
40

Sodium Hydroxide

(we used the solution in the acid-base neutralization lab)

NaOH

 

 

 *      
41

Calcium Hydroxide solution

(limewater)

Demo - test for carbon dioxide

Ca(OH)2

 

 

 *    

Compound / metal and non-metal / covalent and ionic bonding

White solid calcium hydroxide

Soluble in water to form a colorless solution

Strong base

Solution goes "chalky" when carbon dioxide gas is bubbled through the solution. A white precipitate of calcium carbonate is formed.

 

 

 
42

Ammonia Solution

Demo - solubility of ammonia gas

NH4OH

 

 

   *  

Compound / non-metal / covalent and ionic bonding

Colorless solution

Produces a strong odor of ammonia gas

Basic - pH of about 11

If wet red litmus paper is placed over the solution it will quickly turn blue.

 
43

Sulfuric Acid in solution

(acid reactions lab)

H2SO4

 

   *    
44

Nitric Acid in solution

(acid reactions lab)

HNO3

 

   *    
45

Wood

(acid reactions lab)

Complex

 *      
46

Sand

Silicon dioxide

(acid reactions lab)

SiO2

 *      
47

Potassium nitrate

(Effect of Temp. on Solubility)

KNO3

 

 *      
48

Isopropyl alcohol (isopropanol or rubbing alcohol)

(Solvents lab)

(CH3)2CHOH

 

 

   * *  
49

Cork

 

Complex

 *      
50

Rubber

 

Hydrocarbon

 *      
51

Plastic

 

 Hydrocarbon *      
52

Obsidian

 

SiO2

 *      
53

Coal

 

 C *      
54

Graphite

 

 C *      
55 Paper (once living - mostly cellulose)

Complex

 

 

 *      
56 Popcorn kernel Complex

 

        
             
             

 

DEFINITION BREAKDOWNS AND EXTRA NOTES ON PHYSICAL PROPERTIES

Word or Phrase

Definition Breakdown

Students add Examples / Extra notes

Volume

 

·    A physical property

·    Describes the amount of SPACE an object takes up

·    Measured using a ruler to measure dimensions and making calculations, or by displacement of water

·    Units: cubic centimeters (cm3) or milliliters (ml)

 

Mass

 

·    A physical property

·    Describes the amount of MATTER in an object

·    Measured using a BALANCE

·    Units are grams

 

Weight

 

·    A physical property

·    A FORCE due to gravity

·    The measure of attraction between objects

·    Measured using a SPRING SCALE

·    Units are Newtons

 

Density

 

·    A physical property

·    Describes how much mass is contained in a given volume of an object

·    Found by dividing the mass of the object by its volume.

                          D = M

                                V

·    The unit of density is g/cm3

 

 

      

Phase

 

·    A physical property

·    Describes the state in which matter can exist

·