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ISN V - Chemicals ReactingPositive and Negative Ions List
Diatomic Molecules: H2 O2 I2 N2 Cl2 F2 Br2
Positive 1+
Potassium KLithium LiSilver AgSodium NaCopper (I) CuMercury(I) HgHydrogen HCesium CsAmmonium NH4
Hydronium H3O
Positive 2+
Barium BaBeryllium BeCadmium CdCalcium CaCobalt(II) CoCopper(II) CuIron(II) FeLead(II) PbMagnesium MgMercury(II) HgNickel(II) NiStrontium SrTin(II) SnZinc Zn
Positive 3+
Aluminum AlChromium(III) CrIron(III) FeBoron B
Positive 4+
Tin(IV) SnManganese Mn
Negative 1-
Acetate C2H3O2Bicarbonate HCO3Bisulfate HSO4Bromide BrChloride ClChlorate ClO3Chlorite ClO2Cyanide CNFluoride FHydroxide OHHydride HIodide INitrate NO3Nitrite NO2Permanganate MnO4
Thiocyanate SCN
Negative 2-
Carbonate CO3Chromate CrO4Dichromate Cr2O7Oxide OSulfate SO4Sulfide S
Negative 3-
Nitride NPhosphide P Phosphate PO4
1
ISN V - Chemicals Reacting
2
Page # Item Check in or StickerCheck in or Sticker Points Lost
1 Ions List
-------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------2-3 Table of Contents & ISN Points -------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
4 Things to Know, Updated!
-------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
5 Synthesis Reactions Info 2
Text 158-165 2
6 Reactions and Formulas Info -------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
7-8 12
9 Decomposition Reactions Info 2
Text 166-167 2
10-11 21
12 Catalysts 2
Text 168-169 2
13-14 13
15 Balancing Equations Tutorial -------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
16 Balancing Equations Worksheet 1 2
17 Single-Replacement Info 2
18-19 14
20 Lab Graph (5pts extra credit)
21 Balancing Equations Worksheet 2 2
22 Double-Replacement Info 2
23 Activity Series 2
24 Precipitates & Filtrates 2
TEXT: (170-173) (174-175) (176-177) 6
TEXT 178-179 (2 pts extra credit)
25-26 13
27-28 15
28 Lab Images (CuSO4 + NaOH) 8
29-30 Balancing Equations Worksheet 3 2
31-32 14
32 Lab Images (Zn + CuSO4) 8
33-34 13
35-36 14
36 Explosion Report/Research 10
37 Balancing Equations Worksheet 4 2
TEXT: (180-181) (182-184)(185-187) 6
38 Mind Map 5
39 Outside Reading Article 2
40 Extended Response 8
Parent Signature day before Quiz 5
Total Score 215
3
Page # Item Check in or StickerCheck in or Sticker Points Lost
1 Ions List
-------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------2-3 Table of Contents & ISN Points -------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
4 Things to Know, Updated!
-------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
5 Synthesis Reactions Info 2
6 Reactions and Formulas Info -------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
7-8 12
9 Decomposition Reactions Info 2
10-11 21
12 Catalysts 2
TEXT: (158-165) (166-167) (168-169) 6
13-14 13
15 Balancing Equations Tutorial -------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this ---------------------------------------------------no check for this --------------------------
16 Balancing Equations Worksheet 1 2
17 Single-Replacement Info 2
18-19 14
20 Lab Graph (5pts extra credit)
21 Balancing Equations Worksheet 2 2
22 Double-Replacement Info 2
23 Activity Series 2
24 Precipitates & Filtrates 2
TEXT: (170-173) (174-175) (176-177) 6
TEXT 178-179 (2 pts extra credit)
25-26 13
TEXT: (180-181) (182-184) 4
27-28 15
28 Lab Images (CuSO4 + NaOH) 8
29-30 Balancing Equations Worksheet 3 2
31-32 14
32 Lab Images (Zn + CuSO4) 8
33-34 13
35 Balancing Equations Worksheet 4 2
TEXT: (185-187) 2
36 Outside Reading Article 10
37 Mind Map 2
Parent Signature day before Quiz 5
Total Score 188
Parent signature ____________________________________________date__________
Updated Things 2 Know1. SAFETY FIRST!! (lab walk, fragile things, P.A.S.S., etc)
2. You are required to have a pencil or erasable pen, ISN with cover, calculator.
3. on-line textbook myscienceonline.com
4. Sato’s email address: [email protected]
5. Matter is anything with mass and volume.
6. Matter is made of tiny particles that are always in some motion.
7. Matter can exist in several states(or phases), the most common are solid, liquid, gas and plasma.
8. Temperature is how fast the particles are vibrating and ...
9. An element is the most basic type of matter that is still unique.
10.Atoms are composed of protons, neutrons and electrons.
11.The number of protons(atomic number) determines the identity of an element
12.Matter is described by its physical and chemical properties.
13.The periodic table is organized on several levels, including by: atomic number, electron configuration, similar properties.
14.Elements can bond together to form chemicals other than elements.
15.There are three types of bond: ionic, covalent and metallic.
16.The valence electrons determine how an substance bonds.
4
Synthesis Reactions1. What is a synthesis reaction?
2. What types of reactants can be found in a synthesis reaction?
a. elements b.compounds c. a & b
3. In what form is the product of a synthesis reaction always found?
a. element b. compound c. a or b
4. What two reactants produce the compound sodium chloride?
5. What two reactants produce water?
6. What equation represents the formation of magnesium oxide from burning magnesium?
Use this equation/reaction to answer 7-10 ... CO + O2 ⇒ CO2
7. What kind of reaction does the equation represent?
8. What molecular compounds are shown in the equation?
9. What substance is a pure element in the equation?
10. What substance contains the most atoms in the reaction above?
Two reactants A &B, elements or compounds, come together to make a single product, AB. A synthesis reaction pattern
might be symbolized by: A + B ⇒ AB
The hallmark of a synthesis reaction is a single product. Some examples of
synthesis reactions: The reactants, hydrogen gas and oxygen gas burn
(combining with oxygen) to produce water.
H2 + O2 ⇒ H2O
and
The reactants, sulfur trioxide and water react to make sulfuric acid.
H2O + SO3 ⇒ H2SO4
What would you see in a test tube if you were witness to a synthesis reaction? You
would see two different materials combine. A single new material would appear.
5
Pattern to Identify Synthesis Pattern to Identify Single-Replacement
Pattern to Identify Decomposition Pattern to Identify Double-Replacement
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6
LAB: MagnesiumPurpose(s):1. to determine if a metal will burn2. to demonstrate a exothermic synthesis reaction3. to introduce the idea of activation energy
(1pt)Hypothesis(must be names of chemicals): If we heat the Mg in the bunsen burner then the product(s) will be...
________________________________________________________
(1pt) Equation:
Materials: Magnesium, tongs, oxygen, bunsen burner, spark lighter, safety goggles, Petri dishProcedures:
1. Hold Mg in tongs. 2. Ignite one end in the burner. (Don’t stare directly at flame)3. Hold out of burner after lit.4. Record all observations
Observations: Observations:
Reactant(s): (2pt)
use textbook glossary if you don’t know what a reactant is
Reaction:(1pt)
Product(s):(1pt)
7
LAB: Magnesium continued...
Define the terms
1. (1pt) synthesis reaction(from TEXT page 180):
2. (1pt) exothermic (from TEXT page 168)
3. (1pt) activation energy (from TEXT page 183)
4.(1pt) What is the pattern used to identify this type of reaction? (from ISN page 6)
5. (1pt) Attach Image of Product.
Attach Image Here
10 cm wide x 7.5 cm tall
6.(1pt) What is the name of this product? ___________________________ use IONS list in front of ISN
8
Decomposition Reactions1. What is a decomposition reaction?
2. What types of reactants can be found in a decomposition reaction?a. elements b. compounds c. a & b
3. How many products are always produced by a decomposition?a. 1 b. 2 c. more than 1
4. What two products are probable outcomes of the decomposition of water, H2O?
5. Can an element be the reactant in a decomposition? circle Y or N?
6. What equation represents the formation of Hydrogen and oxygen from water?
Use the equation/reaction to answer 7-10 C12H22O11 ⇒ C + H2O
7. What kind of reaction does the equation represent?
8. What compounds are shown in the equation?
9. What element is shown in the equation?
10. What substance contains the most atoms in the reaction above?
One compound reactant AB, is broken apart to make more than one product, A + B. The hallmark of a decomposition reaction is a single reactant. A decomposition reaction pattern might be symbolized by:
AB⇒A+ B
An example of a decomposition reactions is: The reactant carbonic acid is decomposed to form water and carbon dioxide
H2CO3 ⇒ H2O + CO2
What would you see in a test tube if you were witness to a decomposition reaction? You would see one material become at least two separate new substances.
9
LAB: Electrolysis of H2OPurpose(s):To find out: “What electrolysis is and how is it related to decomposition”
Hypothesis: (1pt)If electric current is applied to water then
_______________________________ will be produced.
Equation: (1pt)
Materials: Hoffman Apparatus(pictured), water, power source, splint, matches, test tube, 2% Sulfuric acid(H2SO4 )
Procedures: 1. Assemble Hoffman Apparatus 2. Fill with water and small amount of H2SO4 (sulfuric acid) 3. Connect power and turn on 4. Collect gases 5. Test with splints (glowing and burning splints)
Observations:Observations:
Reactant(s): (1pt)
Reaction:(1pt)
Product(s): (2pt)
10
LAB: Electrolysis of H2O page 2Questions:1.(8pt) Research & Explain electrolysis . .
2.(2 pt) Cite your source for #1 in MLA style:
3.(1pt) What is the pattern used to identify this type of reaction?
4.(4pt) What two tests were performed on the products and what did they prove?
11
Catalysts A catalyst is a substance that changes the rate of a chemical reaction. Most catalysts speed up reactions. Catalysts are not changed in a reaction. They are the same at the beginning and at the end of a reaction. They are not reactants or products. Much of the fuel used in cars is made by using catalysts. Catalysts break down large molecules found in crude oil into the simpler molecules that make up gasoline. Catalysts are also used to break down the waste products produced when gasoline burns. A catalytic converter in an automobile changes carbon monoxide(CO) and other pollutants into carbon dioxide(CO2) and water. Catalysts that slow down chemical reactions are called inhibitors. Many inhibitors are used as preservatives in household products. A preservative slows down the rate of decay or spoilage. Without these chemicals, many foods would spoil faster.
1. What does a catalyst do in a chemical reaction?
2. Enzymes in your digestive system are catalysts. Why do you think these substances are needed?
3. Frank and Tony perform an experiment and add a few drops of hydrochloric acid. After the reaction takes place, the hydrochloric acid has been changed into a salt and water. Frank writes in his lab notebook that the hydrochloric acid was a catalyst in the reaction. Is he right? Explain.
4. In what ways are catalysts important in the running of automobiles?
5. How is an inhibitor different from a typical catalyst?
6. Besides preventing food spoilage, can you think of some other practical uses for inhibitors?
12
LAB: DECOMPOSITION OF HYDROGEN PEROXIDE
Purpose(s): To show the effect on the rate of decomposition of hydrogen peroxide (H2O2) by the use of a catalyst, manganese dioxide (MnO2)
(1pt)Hypothesis:
__________________________________________________________________
__________________________________________________________________
(1pt) Equation:
Materials: Goggles, manganese dioxide (MnO2) , hydrogen peroxide (H2O2), test tubes, match, splints, plastic trays, graduated cylinder, test tube holder, beaker of sand, filter, beaker
Procedures: 1. Add 4 grams of MnO2 to 15 ml of H2O2 in a test tube. 2. Observe results and test for O2
3. The test for oxygen involves using a glowing split. If the split re-lights then there is O2 gas present.
4. Put all splints and matches into sand.5. Filter the MnO2 out of the liquid and observe liquid.6. CLEAN UP, USE TEST TUBE BRUSH, THROW AWAY PLASTIC DISH
Observations:Observations:
Reactant(s): (1pt)
Reaction: (1pt)
Product(s): (2pt)
13
LAB: DECOMPOSITION OF HYDROGEN PEROXIDE p2
Questions
1. (3pt) Define a catalyst and give two examples of them.
2. (2pt) What were two major clues that there was a chemical change in this reaction?
3. (1pt) Was this reaction exothermic?
4. (1pt) What is the pattern used to identify this type of reaction?
14
Balancing Equations TutorialSTEP I . Start with the word equation for the reaction. Magnesium plus oxygen yields magnesium oxide
STEP 2. Rewrite the equation-using symbols and formulas (use list on ISN #1).
STEP 3. Make sure the same number of each kind of atom appears on each side of the equation.
€
Mg+O2 → MgO
STEP 4. If unequal, Use coefficients to balance the equation.
STEP 5. Recheck the number and kind of each atom
RULES To Live By!!1. ONCE YOU’VE DETERMINED A SUBSCRIPT IN STEP 2,
NEVER CHANGE IT AGAIN
2. ONLY CHANGE COEFFICIENTS FOR BALANCING
HEY!Watch out for
diatomic elements like O2
€
Mg+O2 → MgO
€
2Mg +O2 → 2MgO
15
2 1 Mg 1 2
2 O 1 2
1 Mg 1
2 O 1
Balancing chemical equations #1Complete the table by listing the number of each different atom in the formulas shown.
example H2O 2 Hydrogens 1 Oxygen
#1 H2SO4
#2 2Pb(NO3)2
#3 3Fe2(SO4)3
Fill in the missing chemical symbols to balance the equations.
4.
€
2__+ Cl2 ⇒ 2NaCl
5.
€
___2+ F2 ⇒ 2HF
6.
€
4 ___+O2 ⇒ 2Ag2O
7.
€
Zn + H2O⇒ ZnO+ ____28.
€
SnO2 + 2C⇒ 2CO+ ____
9.
€
2NO+ ___2 ⇒ 2NO2
BALANCE each equation with COEFFICIENTS
10. Mg + O2 ⇒ MgO
11. H2 + O2 ⇒ H2O
12. Na + ZnO ⇒ Na2O + Zn
16
Single-Replacement Reactions
1. What is a single-replacement reaction?
2. What types of reactants are found in a single-replacement reaction? a. elements b. compounds c. a & b
3. How many products are always produced by a single replacement? a. 1 b. 2 c. more than 1
4. The pattern for single replacements is A+BC⇒ B + AC. Use the letters XYZ and rewrite the pattern.
5. Can an element be a reactant in a single replacement?
6.What would the equation be for calcium plus magnesium oxide yields magnesium plus calcium oxide?
One compound reactant, BC, trades out one element B for another A . The identifier of a single-replacement reaction is a compound plus an element. This reaction can also be called single-displacement and single-substitution. A single-replacement reaction pattern might be symbolized by:
A + BC ⇒ AC + B
An example of a single-replacement reaction is:
Zinc plus hydrochloric acid yields zinc chloride plus hydrogen.
Zn + HCl ⇒ ZnCl2 + H2
What would you see in a test tube if you were witness to a single-replacement reaction? You would see one element and one compound become a different element and different compound.
17
LAB: Zinc (Zn) and Hydrochloric Acid (HCl)Purpose(s): To determine what kind of reaction is shown; is it exothermic or endothermic; what are the products of the reaction?
(1pt) Hypothesis:
(1pt) Equation:
Zn + ____HCl ⇒ _________ + _________
Materials: latex gloves, “mossy” zinc, HCl, 4 test tubes, 2 thermometers, wood matches, graduated cylinder, test tube rack, stop watch, goggles
Procedures:1. Measure and add 12 milliliters of HCl to each small test tube.2. Record your observations on the next page.3. Place thermometers in each and
record in the table below for time 0 minutes.4. Add zinc to one of the test tubes, call it tube #2.5. Cover both tubes with the large test tubes.6. Observe the temperatures of both tubes every minute for 8 minutes. (1pt)7. After 8 minutes, test both tubes for hydrogen gas with a burning match.8. Pour all liquids and solids into the funnel in the fume hood.9. Extra Credit.- Make an line graph of both tubes on one graph, time on x-axis,
temperature on y axis and attach it to ISN 20
Time in min Temperature ˚CTube #1
Temperature ˚CTube #2 (Zinc)
0
1
2
3
4
5
6
7
8
WARNING! Acid is corrosive, use
goggles and gloves at all times
18
LAB: Zinc (Zn) and Hydrochloric Acid (HCl)Observations:Observations:
Reactant(s): (2pt)
Reaction: (1pt)
Product(s): (2pt)
1.(1pt) What kind of reaction was shown in this lab?
2.(1pt) Was it exothermic or endothermic?
3.(2pt) What test was performed and what did it prove?
4.1pt) What is the pattern for these types of reactions?
19
PLACE GRAPH HERE 5 points
20
BALANCING EQUATIONS #2
Use IONS LIST on ISN 1 to balance these equations. 1. calcium + oxygen⇒ calcium oxide
2. calcium oxide ⇒ calcium + oxygen
3. potassium + sodium fluoride⇒ potassium fluoride + sodium
4. potassium nitride + calcium carbonate⇒ potassium carbonate + calcium nitride
21
Double-Replacement Reactions
1. What is a double-replacement reaction?
2. What types of reactants are found in a double-replacement reaction? a. elements b. compounds c. a & b
3. How many products are always produced by a double replacement? a. 1 b. 2
4. The pattern for double replacements is AB+CD⇒AD + CB. Use the letters WXYZ and rewrite the pattern.
5. Can an element be a product in a double replacement?
6. What would the formula be for magnesium hydroxide + calcium chloride yields magnesium chloride + calcium hydroxide?
One compound reactant, AB, trades partners with another compound CD. The identifier of a double-replacement reaction is a compound plus a compound. This reaction can also be called double-displacement and double-substitution. A double-replacement reaction pattern might be symbolized by:
AB + CD ⇒ AD + CB An example of a Double-replacement reaction is:
potassium phosphate + calcium sulfate yields potassium sulfate + calcium phosphate
K2PO4 + CaSO4 ⇒K2SO4 + CaPO4
What would you see in a test tube if you were witness to a double-replacement reaction? You would see two compounds become two different compounds.
22
Activity SeriesIn a single-replacement reaction, one element replaces another element in a compound, forming a new compound. This kind of reaction can be shown by the following general equation:
A + BC ⇒ AC + B
In order for element A to replace element B, element A must be more active than element B. Scientists have done experiments to determine which elements are more active than others. They have organized their results into a table called an Activity Series. The element at the top of the table is the most active; the element at the bottom of the table is the least active.
Study the activity series below. Then answer the questions.
1. What is the most active element listed in this table? _________________
2. What is the least active element listed? ____________________
3. Explain why the following reaction occurs: Zn + 2HCl ⇒ ZnCl2 + H2
4. Would the reaction above take place if the metal were copper instead of zinc? Why or why not?
5. Predict what will happen when the following substances are mixed: K + AlCl3 ⇒ ?
6. Predict what will happen when these substances mix: Zn+AgNO3 ⇒ ?
7. Predict what will happen when these substances mix: Cu + AlCl3 ⇒?
Activity SeriesActivity Series
Symbol Element
K Potassium
Ca Calcium
Na Sodium
Mg Magnesium
Al Aluminum
Zn Zinc
Cr Chromium
Fe Iron
Ni Nickel
Sn Tin
Pb Lead
H Hydrogen
Cu Copper
Hg Mercury
Ag Silver
Au Gold
23
Precipitates & Filtrates Chemical reactions produce new substances, products, with properties that are different from the initial substances, reactants. Often the new products can be separated into two categories. A precipitate is a solid material that is formed in a solution by chemical reactions and settles to the bottom of the container in which the reaction takes place. A precipitate may also be a substance removed from another by a filter. The substance, especially liquid, that has passed through a filter is called a filtrate. The easy separation of the precipitate and the filtrate points to the fact that the products are a mixture. The table below shows some compounds and whether they will form a precipitate in water. I indicates that the compound is insoluble and will form a precipitate. S indicates soluble in water and no precipitate forms. P indicates that the compound is partially soluble and a precipitate might form
Questions:
1. Will Copper nitrate produce a precipitate? Y/N
2. Will Silver chloride produce a precipitate? Y/N
3. Name three other compounds that will form precipitates in water.
24
LAB Mini-Volcano Purpose(s): 1. to demonstrate activation energy & a wick 2. to show a decomposition reaction 3. to show a cool demo!
Hypothesis: (1pt)If we supply enough activation energy then the ammonium dichromate will decompose into...
Equation: (1pt)(use word equation to write the symbol equation) Ammonium dichromate yields nitrogen and water and chromium(III) oxide
Materials: ammonium dichromate, magnesium, watch glass, bunsen burner, striker, fume hood
Procedures: 1. Make a 3 cm high mound of (NH4)2Cr2O7 on the wire mesh 2. Insert the Mg wick into the center 3. Ignite the Mg with the bunsen burner
Observations:Observations:
Reactant(s): (1pt)
Reaction: (1pt)
Product(s): (3pt)
25
LAB Mini-Volcano Questions:1. (1pt) Describe decomposition reactions
2. (2pt) What is the pattern used to identify them.
3. (1pt) What does the prefix “di” mean?
4. (1pt) Re-Write and balance the equation for this experiment.
5. (1pt) There were really two reactions in this experiment, what supplied the activation energy for the second reaction?
26
LAB: Copper(II) sulfate & Sodium hydroxidePurpose(s): 1. To demonstrate a double replacement 2. To produce and predict a precipitate using a solubility list (2pt) Hypothesis: If we combine CuSO4 and NaOH then the products
will be ___________________________________________________________
(1pt) Prediction for purpose #2
_________________________________________________________
(1pt) Equation (hint: use ISN #1):
_________________________________________________________
Materials: 1 large test tube test tube rack 2 graduated cylinders goggles1 filter 1 beaker gloves 1 funnel CuSO4 NaOH
Procedures:1. Measure 5 ml of CuSO4 solution in the 10mL graduate and pour into test tube2. Measure 15 ml of NaOH solution in a separate 50 mL graduate and pour little by
little into test tube,observing the reaction as you go3. After all solution has reacted, filter tubes into 100 ml beaker using funnels & filters4. Observe both products, the filtrate and the precipitate.5. Take photos of both.6. Place your just filter off to the side to dry overnight.7. CLEAN UP, put all glassware on drying rack
Observations:Observations:
Reactant(s): (2pt)
Reaction: (1pt)
Product(s): (2pt)
27
LAB: Copper(II) sulfate & Sodium hydroxide⬇Reactants ⬇Products
⬇name: ⬇name:
Image here7 cm Wide x 5.25 cm Tall
name 1 ptimage 1 pt
Image here7 cm Wide x 5.25 cm Tall
name 1 ptimage 1 pt
⬇name: ⬇name:
Image here7 cm Wide x 5.25 cm Tall
name 1 ptimage 1 pt
Image here7 cm Wide x 5.25 cm Tall
name 1 ptimage 1 pt
Questions1. (1pt) What are DOUBLE REPLACEMENT REACTIONS?
2. (1pt) What is the pattern used to identify DOUBLE REPLACEMENT REACTIONS.
3. (2pt) Explain Precipitates & Filtrates
4. (1pt) What is the name of the precipitate? ___________________________________
5. (1pt) What was the name of the filtrate? ___________________________________
28
Balancing Equations #3 Instructions: Use “positive & negative ions list” to balance these equations.
1. potassium + iron(II) chloride ⇒ potassium chloride + iron (II)
2. magnesium + iron(II) hydroxide ⇒ magnesium hydroxide + iron (II)
3. potassium hydroxide + aluminum chloride ⇒ potassium chloride + aluminum hydroxide
4. magnesium hydroxide + calcium chloride ⇒ magnesium chloride + calcium hydroxide
5. iron(II) chloride + magnesium sulfate ⇒ iron(II) sulfate + magnesium chloride
29
6. potassium phosphate + calcium sulfate ⇒ potassium sulfate + calcium phosphate
7. aluminum hydroxide + sulfuric acid ⇒ aluminum sulfate + water
8. H3PO4 ⇒ H4P2O7 + H2O
9. C + SO2 ⇒ CS2 + CO
10.Ca3(PO4)2 + SiO2 + C ⇒ CaSiO3 + CO + P
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LAB: Shake It!Purpose(s): 1. to identify characteristics and clues to chemical change 2. to practice balancing an equation
(2pt) Hypothesis:If we add Zinc to Copper(II) sulfate then the products will be...__________ ____________________________________________________________________________
(2pt) Equation:
Materials: CuSO4 solution, zinc, large test tube, stopper (cork), safety goggles, filter paper, 100 ml beaker, funnel, graduated cylinder, stirring rod.
Procedures: 1. Observe reactants, take photos FIRST!! 2. Fill test tube with 25 ml of CuSO4. 3. Add zinc. 4. Put in cork and shake vigorously for 60 sec. while holding cork in. 5. Filter the products, use stirring rod to scoop out solids. 6. Clean up- Liquids to sink, solids to the trash, clean all lab-ware, plastic trays to fume hood.
Observations:Observations:
Reactant(s): (2pt)
Reaction: (1pt)
Product(s): (2pt)
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LAB: Shake It!Questions:
1.(2pt) What are two clues of chemical change in this lab? (see page 166-168 in textbook)
2.(1pt) Explain why Zn replaced copper, according to the Activity Series worksheet.
3.(1pt) What type of chemical reaction is this? (Remember the Dance!) ___________________
4.(1pt) What is the pattern used to identify this reaction? (not the equation!!! the PATTERN)
⬇Reactants ⬇Products
⬇name: ⬇name:
Image here7 cm Wide x 5.25 cm Tall
Image here7 cm Wide x 5.25 cm Tall
⬇name: ⬇name:
Image here7 cm Wide x 5.25 cm Tall
Image here7 cm Wide x 5.25 cm Tall
Extra credit: Go to the CuSO4 Survey in Quia for the question(s)
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LAB: Deep FreezePurpose(s): to demonstrate an endothermic reaction
(1pt) Hypothesis:
If barium hydroxide & ammonium thiocyanate are mixed then the temperature will...____________________________________ (increase/decrease/stay the same)
Equation: Ba(OH)2 *8H2O + NH4SCN Ba(SCN)2 + NH3 + H2O
Materials:barium hydroxide, ammonium thiocyanate, beaker, wood block, water dropper, fume hood, gloves
Procedures:1. Mix 20 g of barium hydroxide & 10 g of ammonium thiocyanate in the beaker2. Place a drop of water on the wood block3. Set the beaker on the drop, lift when frozen
Observations:Observations:
Reactant(s): (2pt)
Barium hydroxide
ammonium thiocyanate
Reaction: (1pt)
Product(s): (3pt)
Ba(SCN)2 -
NH3-
H2O-
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LAB: Deep FreezeQuestions1. (2pt) Think of two uses for a reaction that is endothermic.
use #1-
use #2-
2. (2pt) What were two clues that a chemical reaction occurred?(see page 166-168)
clue #1-
clue #2-
3. (2pt) When you balance the equation for this lab, you will notice a * in the equation. The Ba(OH)2 in the reaction actually has water in it already. Balance this with coefficients in front just like any other. Write below.
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Balancing Equations #4 (LAST PRACTICE!)1. Potassium plus aluminum oxide yields potassium oxide plus aluminum
2. Sodium plus sodium nitrate yields sodium oxide plus nitrogen
3. Hydrogen phosphate plus magnesium hydroxide ⇒ magnesium phosphate plus water
4. aluminum plus sulfur (S8) yields aluminum sulfide
5. barium chlorate yields barium chloride plus oxygen
6. What types of reactions are shown in 1-5 above?1- 4-2- 5-3-
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Outside Reading Article And Extended Response
Find a current article (2004-present)that relates to our current ISN.To find articles you can use these two great research resources:
1. Go to the NBJH homepage then Click on Library Resource Center and then use the data ---or---Use “Sato’s Science Search Engine” linked on Mr. Sato’s site
3. Write a Response should be one/two paragraphs that includes:•Summary of the Key Ideas from the article.•CONNECTIONS from the article to...
•the TEXT from the current ISN (include page number and quote)•something from this unit we did during class time•your own life
•Your own EXTENSION OF IDEAS presented in the article•Conclusion
4. Put into Quia
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Mind MapUse my links page or make your own document to create a concept map for these terms: chemical reaction, chemical equation, chemical formulas, reactants, products, coefficients, subscripts.
attach map here
15 cm wide x 17 cm tall
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