Compounds & Chemical Reactions
Physical Science Unit 2
Physical Science
Compounds & Chemical Reactions
Monday / Tuesday / Wednesday / Thursday / Friday7
Labor Day Holiday / 8
Launch Lab
Stability in Bonding
Lewis Dot Diagrams / 9
Molecular Modeling
Bonds T-Chart / 10
Bond with a classmate
Ionic Bonding / 11
Naming and Writing formulas for Ionic Compounds
14
Naming and Writing formulas for Ionic Compounds / 15
Naming and Writing formulas for Ionic Compounds: Transition Metals / 16
Household Chemical Inventory
Half Day / 17
Naming and Writing formulas for Ionic Compounds: Polyatomic Ions / 18
Quiz: Ionic Compounds
21
Naming and Writing formulas for Covalent Compounds / 22
Naming and Writing formulas for Covalent Compounds / 23
Quiz: Covalent Compounds
Counting Atoms / 24
Types of Chemical Reactions Demos / 25
Conservation of Mass
Conservation of Mass Lab
28
Balancing Equations / 29
Balancing Equations / 30
Review
Balancing Equations Quiz / 1
Review / 2
Test
Compounds & Chemical Reactions
5
Performance Assessment / 6
Performance Assessment / 7
Performance Assessment / 8
Performance Assessment / 9
Teacher Workday
Warm Up Activities – will be on board as you enter the classroom
Tuesday – September 8
Today’s Essential Question:
Warm Up:
Notes:
Wednesday – September 9
Today’s Essential Question:
Warm Up:
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Thursday – September 10
Today’s Essential Question:
Warm Up:
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Friday – September 11
Today’s Essential Question:
Warm Up:
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Monday – September 14
Today’s Essential Question:
Warm Up:
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Tuesday – September 15
Today’s Essential Question:
Warm Up:
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Wednesday – September 16
Today’s Essential Question:
Warm Up:
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Thursday – September 17
Today’s Essential Question:
Warm Up:
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Friday – September 18
Today’s Essential Question:
Warm Up:
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Monday – September 21
Today’s Essential Question:
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Tuesday – September 22
Today’s Essential Question:
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Wednesday – September 23
Today’s Essential Question:
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Thursday – September 24
Today’s Essential Question:
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Friday – September 25
Today’s Essential Question:
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Monday – September 28
Today’s Essential Question:
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Tuesday – September 29
Today’s Essential Question:
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Wednesday – September 30
Today’s Essential Question:
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Thursday – October 1
Today’s Essential Question:
Warm Up:
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Friday – October 2
Today’s Essential Question:
Warm Up:
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Monday – October 5
Today’s Essential Question:
Warm Up:
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Tuesday – October 6
Today’s Essential Question:
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Wednesday – October 7
Today’s Essential Question:
Warm Up:
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Electron Dot Diagrams
Write the electron dot configuration for the following elements.
1. K 2. Br
3. Al 4. P
5. F 6. Si
7. Sn 8. At
9. Xe 10. In
11. Ca 12. Bi
13. H 14. He
Molecular Models Lab
Draw Lewis dot structures for the following molecules. Use the model kit to build each molecule.
§ Predict the shape and bond angle of each.
§ Draw arrow diagrams ( ) to indicate the polarity of bonds.
§ State the polarity of the overall molecule.
§ Draw a 3-D picture of the molecule.
Formula / Lewis dot structure / 3-D picture of molecule (show polarity of bonds)CF4 / N
H
S
B
Shape and bond angle / Is the molecule polar?
Formula / Lewis dot structure / 3-D picture of molecule (show polarity of bonds)
CO32- / N
H
S
B
Shape and bond angle / Is the molecule polar?
Formula / Lewis dot structure / 3-D picture of molecule (show polarity of bonds)
SCl2 / N
H
S
B
Shape and bond angle / Is the molecule polar?
Formula / Lewis dot structure / 3-D picture of molecule (show polarity of bonds)
NH3 / N
H
S
B
Shape and bond angle / Is the molecule polar?
Formula / Lewis dot structure / 3-D picture of molecule (show polarity of bonds)
SiO2 / N
H
S
B
Shape and bond angle / Is the molecule polar?
Formula / Lewis dot structure / 3-D picture of molecule (show polarity of bonds)
N2 / N
H
S
B
Shape and bond angle / Is the molecule polar?
Formula / Lewis dot structure / 3-D picture of molecule (show polarity of bonds)
HCN / N
H
S
B
Shape and bond angle / Is the molecule polar?
Physical Science
Bond T chart
Ionic Bonds Covalent Bonds
Bond with a Classmate
When you find another ion with which you can bond, write in each symbol and charge.
Then write the new compound formed by combining the two. Give the compound’s name.
Remember - Positive ions can only bond with negative ions and vice versa!
+ Ion / Ion / Compound / NameMg 2+ / Cl -1 / MgCl2 / Magnesium Chloride
Write the formula for compound formed by each pair of elements
Charge / -3
Lithium / +1 / Li3N
Beryllium
Boron
Sodium
Aluminum
Magnesium
Calcium
Potassium
Barium
.
Write the name of each compound formed by the pairs of elements below.
Lithium / Lithium Nitride
Beryllium
Boron
Sodium
Aluminum
Magnesium
Calcium
Potassium
Barium
Physical Science
Naming Binary Ionic Compounds
Name the following Binary Compounds
1. KCl ______2. CaBr2 ______
3. BaS ______4. AlN ______
5. Ba3P2 ______6. NaCl ______
7. MgCl2 ______8. CaCl2 ______
9. Na3P ______10. CaO ______
Write the formulas for the following Binary Compounds
1. lithium chloride ______
2. potassium oxide ______
3. magnesium bromide ______
4. rubidium phosphide ______
5. calcium sulfide ______
6. beryllium fluoride ______
7. strontium oxide ______
8. sodium chloride ______
9. sodium phosphide ______
10. calcium nitride ______
Transition Metals Worksheet
Write the formulas for the following compounds.
1. iridium (III) oxide ______
2. lanthanum (III) iodide ______
3. arsenic (V) iodide ______
4. lead (II) chloride ______
5. iron (III) sulfide ______
6. iron (III) oxide ______
7. nickel (II) nitride ______
8. gold (IV) oxide ______
9. copper (II) oxide ______
10. chromium (II) phosphide ______
Write the names for the following compounds.
1. Rb2S ______2. PbO2 ______
3. ZnI2 ______4. PbO2 ______
5. FeO ______6. FeO2 ______
7. MnBr2 ______8. AgCl ______
9. PtO ______10. AuCl4 ______
Name the following compounds.
1. Pb3(PO4)2 ______2. Cu(IO3)2 ______
3. Bi2(SO4)3 ______4. RbNO3 ______
5. CuSO4 ______6. Th(OH)4 ______
7. (NH4)4P4O7 ______8. Ba(MnO4)2 ______
9. Al2(B4O7)2 ______10. Mg(ClO2)2 ______
Write the formulas for the following compounds.
1. ammonium sulfite ______
2. magnesium sulfate ______
3. barium acetate ______
4. rubidium thiocyanate ______
5. potassium permanganate ______
6. calcium peroxide ______
7. silver nitrate ______
8. iron (III) chlorite ______
9. platinum (II) hydroxide ______
10. iron (II) nitrite ______
Complete the following table, being sure that the total charge on the resulting compound is zero.
Ions
/ ChlorideCl1- / Hydroxide
OH1- / Nitrate
NO31- / Sulfate
SO42- /
Sulfide
S2- /Carbonate
CO32- / PhosphatePO43-
Lithium
Li1+Sodium
Na1+
Ammonium
NH41+
Potassium
K1+Calcium
Ca2+Magnesium
Mg2+Aluminum
Al3+Zinc
Zn2+
Iron (II)
Fe2+
Iron (III)
Fe3+
Lead (II)
Pb2+Tin (IV)
Sn4+Copper (I)
Cu1+
Copper (II)
Cu2+CHEMISTRY HOUSEHOLD PRODUCT SURVEY
Directions: Tonight, enlist the support of your parents and siblings to complete the following survey of home products. If you work together the survey can be completed very quickly. You will have fun and you will teach your family a little chemistry! Together, go to the following locations: choose 2 products from each location and make a complete ingredients list of each product. After completing this walk-thru survey, compare and contrast the different ingredients. Explain any similarities between ingredients. For example did you find similar ingredients in more than one product? Ask your parents this question: Why is label reading such a necessity in today’s world?
REFRIGERATOR
Product Name #1 ______
Ingredients:
Product Name #2 ______
Ingredients:
KITCHEN PANTRY
Product Name #1 ______
Ingredients:
Product Name #2 ______
Ingredients:
LAUNDRY ROOM
Product Name #1 ______
Ingredients:
Product Name #2 ______
Ingredients:
BATHROOM
Product Name #1 ______
Ingredients:
Product Name #2 ______
Ingredients:
GARAGE
Product Name #1 ______
Ingredients:
Product Name #2 ______
Ingredients:
Covalent Compounds
Write the formulas for the following covalent compounds.
1. phosphorous trichloride ______
2. nitrogen monoxide ______
3. dinitrogen pentoxide ______
4. carbon dioxide ______
5. nitrogen trihydride ______
6. xenon tetrafluoride ______
7. diarsenic pentoxide ______
8. carbon disulfide ______
9. chlorine monofluoride ______
10. sulfur trioxide ______
Name the following covalent compounds.
1. CCl4 ______2. SO2 ______
3. SO3 ______4. ClF3 ______
5. PCl3 ______6. AsF5 ______
7. SiO2 ______8. H2O ______
9. P2O3 ______10. N2O3 ______
Identify the following reactions as either:
SYNTHESIS (S), DECOMPOSTION (D), SINGLE DISPLACEMENT (SD), DOUBLE DISPLACEMENT (DD)
_____ 1. 2H2 + O2 à 2H2O
_____ 2. N2 + 3H2 à 2NH3
_____ 3. 2HgO à 2Hg + O2
_____ 4. Xe + 3F2 à XeF6
_____ 5. P4 + 5O2 à 2P2O5
_____ 6. Zn + 2HCl à ZnCl2 + H2
_____ 7. Fe2(SO4)3 + 6KOH à 3K2SO4 + 2Fe(OH)3
_____ 8. 2Al + 3FeO à Al2O3 + 3Fe
_____ 9. Al2(SO4)3 + 3Ca(OH)2 à 2Al(OH)3 + 3CaSO4
_____ 10. FeCl3 + 3NH4OH à Fe(OH)3 + 3NH4Cl
_____ 11. Ca(ClO3)2 à CaCl2 + 3O2
_____ 12. 2Au2O3 à 4Au + 3O2
_____ 13. SiC + 2Cl2 à SiCl4 + C
_____ 14. 3Fe + 4H2O à Fe3O4 + 4H2
_____ 15. 2H2O2 à 2H2O + O2
Conservation of Mass
In a chemical reaction, the total mass of the substances formed by the reaction is equal to the total mass of the substances that reacted. This principle is called the law of conservation of mass, which states that matter is not created or destroyed during a chemical reaction. In this experiment, sodium hydrogen carbonate, NaHCO3 (baking soda), will react with hydrochloric acid, HCl. The substances formed by this reaction are sodium chloride, NaCl; water, H2O; and carbon dioxide gas, CO2.
Strategy
You will show that new substances are formed in a chemical reaction. You will show the conservation of mass during a chemical reaction.
Materials
sealable plastic sandwich bag containing sodium hydrogen carbonate, NaHCO3 hydrochloric acid, HCl plastic pipette paper towel metric balance
Procedure
Obtain the plastic sandwich bag containing a small amount of sodium hydrogen carbonate.
Fill the pipette with the hydrochloric acid solution. Use a paper towel to wipe away any acid that might be on the outside of the pipette. Discard the paper towel. WARNING: Hydrochloric acid is corrosive. Handle with care.
Carefully place the pipette in the bag. Press the bag gently to eliminate as much air as possible. Be careful not to press the bulb of the pipette. Seal the bag.
Measure the mass of the sealed plastic bag using the metric balance. Record this value in the Data and Observations section.
Remove the plastic bag from the balance. Without opening the bag, direct the stem of the pipette into the sodium hydrogen carbonate. Press the bulb of the pipette and allow the hydrochloric acid to react with the sodium hydrogen carbonate. Make sure that all the acid mixes with the sodium hydrogen carbonate.
Observe the contents of the bag for several minutes. Record your observations in the Data and Observations section.
After several minutes, measure the mass of the sealed plastic bag and its contents.
Record this value in the Data and
Data and Observations
Table 1
Mass of plastic bag before reaction (in grams)Observations from step 6
Mass of plastic bag after reaction (in grams)
Questions and Conclusions
Why was it important for the plastic bag to be sealed?
What did you observe that indicated that a chemical reaction took place?
Compare the mass of the plastic bag and its contents before and after the chemical reaction.
Does your comparison in question 3 confirm the conservation of mass during this chemical reaction? Explain.
Strategy Check
_____ Can you demonstrate that new substances are formed in a chemical reaction?
_____ Can you show the conservation of mass during a chemical reaction?
Balancing Chemical Equations
Balance the equations below:
1) ____ N2 + ____ H2 à ____ NH3
2) ____ KClO3 à ____ KCl + ____ O2
3) ____ NaCl + ____ F2 à ____ NaF + ____ Cl2
4) ____ H2 + ____ O2 à ____ H2O
5) ____ Pb(OH)2 + ____ HCl à ____ H2O + ____ PbCl2
6) ____ AlBr3 + ____ K2SO4 à ____ KBr + ____ Al2(SO4)3
7) ____ CH4 + ____ O2 à ____ CO2 + ____ H2O
8) ____ C3H8 + ____ O2 à ____ CO2 + ____ H2O
9) ____ C8H18 + ____ O2 à ____ CO2 + ____ H2O
10) ____ FeCl3 + ____ NaOH à ____ Fe(OH)3 + ____NaCl
11) ____ P + ____O2 à ____P2O5
12) ____ Na + ____ H2O à ____ NaOH + ____H2
13) ____ Ag2O à ____ Ag + ____O2
14) ____ S8 + ____O2 à ____ SO3
15) ____ CO2 + ____ H2O à ____ C6H12O6 + ____O2
16) ____ K + ____ MgBr à ____ KBr + ____ Mg
17) ____ HCl + ____ CaCO3 à ____ CaCl2 + ____H2O + ____ CO2
18) ____ HNO3 + ____ NaHCO3 à ____ NaNO3 + ____ H2O + ____ CO2
19) ____ H2O + ____ O2 à ____ H2O2
20) ____ NaBr + ____ CaF2 à ____ NaF + ____ CaBr2
21) ____ H2SO4 + ____ NaNO2 à ____ HNO2 + ____ Na2SO4
Balancing Chemical Equations Worksheet
1. _____ H2 + _____ O2 → _____ H2O
2. _____ N2 +_____ H2 →_____ NH3
3. _____ S8 + _____ O2 →_____ SO3
4. _____ N2 + _____ O2 →_____ N2O
5. _____ HgO →_____ Hg + _____ O2
6. _____ CO2 + _____ H2O →_____ C6H12O6 + _____ O2
7. _____ Zn + _____ HCl →_____ ZnCl2 + _____ H2
8. _____ SiCl4 + _____ H2O →_____ H4SiO4 + _____ HCl
9. _____ Na + _____ H2O →_____ NaOH + _____ H2
10. _____ H3PO4 →_____ H4P2O7 + _____ H2O
11. _____ C10H16 + _____ Cl2 →_____ C + _____ HCl
12. _____ CO2 + _____ NH3 →_____ OC(NH2)2 + _____ H2O
13. _____ Si2H3 + _____ O2 →_____ SiO2 + _____ H2O3
14. _____ Al(OH)3 + _____ H2SO4 →_____ Al2(SO4)3 + _____ H2O