Compounds & Chemical
Reactions
Physical Science
Unit 2
1
Physical Science
Compounds & Chemical Reactions
Monday
7
14
Naming and Writing
formulas for Ionic
Compounds
21
Naming and Writing
formulas for
Covalent Compounds
28
Balancing Equations
Performance
Assessment
Wednesday
8
9
Stability in Bonding
Lewis Dot Diagrams
Bonds T-Chart
15
16
Launch Lab
Labor Day
Holiday
5
Tuesday
Naming and Writing
formulas for Ionic
Compounds:
Transition Metals
22
Naming and Writing
formulas for
Covalent Compounds
29
Balancing Equations
6
Performance
Assessment
Molecular Modeling
Household Chemical
Inventory
Half Day
23
Quiz: Covalent
Compounds
Thursday
10
Bond with a
classmate
Ionic Bonding
Friday
11
Naming and Writing
formulas for Ionic
Compounds
17
18
24
25
Naming and Writing
formulas for Ionic
Compounds:
Polyatomic Ions
Types of Chemical
Reactions Demos
Conservation of
Mass
Counting Atoms
30
Review
Balancing Equations
Quiz
7
Performance
Assessment
Quiz: Ionic
Compounds
Conservation of
Mass Lab
1
2
Review
8
Performance
Assessment
Test
Compounds &
Chemical Reactions
9
Teacher
Workday
2
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:
Notes:
3
Thursday – September 10
Today’s Essential Question:
Warm Up:
Notes:
Friday – September 11
Today’s Essential Question:
Warm Up:
Notes:
4
Monday – September 14
Today’s Essential Question:
Warm Up:
Notes:
Tuesday – September 15
Today’s Essential Question:
Warm Up:
Notes:
5
Wednesday – September 16
Today’s Essential Question:
Warm Up:
Notes:
Thursday – September 17
Today’s Essential Question:
Warm Up:
Notes:
6
Friday – September 18
Today’s Essential Question:
Warm Up:
Notes:
Monday – September 21
Today’s Essential Question:
Warm Up:
Notes:
7
Tuesday – September 22
Today’s Essential Question:
Warm Up:
Notes:
Wednesday – September 23
Today’s Essential Question:
Warm Up:
Notes:
8
Thursday – September 24
Today’s Essential Question:
Warm Up:
Notes:
Friday – September 25
Today’s Essential Question:
Warm Up:
Notes:
9
Monday – September 28
Today’s Essential Question:
Warm Up:
Notes:
Tuesday – September 29
Today’s Essential Question:
Warm Up:
Notes:
10
Wednesday – September 30
Today’s Essential Question:
Warm Up:
Notes:
Thursday – October 1
Today’s Essential Question:
Warm Up:
Notes:
11
Friday – October 2
Today’s Essential Question:
Warm Up:
Notes:
Monday – October 5
Today’s Essential Question:
Warm Up:
Notes:
12
Tuesday – October 6
Today’s Essential Question:
Warm Up:
Notes:
Wednesday – October 7
Today’s Essential Question:
Warm Up:
Notes:
13
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
14
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
CF4
Formula
Shape and bond angle
Is the molecule polar?
Lewis dot structure
3-D picture of molecule (show polarity of
bonds)
Shape and bond angle
Is the molecule polar?
Lewis dot structure
3-D picture of molecule (show polarity of
bonds)
Shape and bond angle
Is the molecule polar?
Lewis dot structure
3-D picture of molecule (show polarity of
bonds)
N
H
S
B
Formula
SCl2
3-D picture of molecule (show polarity of
bonds)
N
H
S
B
Formula
CO32-
Lewis dot structure
N
H
S
B
15
NH3
N
H
S
B
Formula
SiO2
Lewis dot structure
3-D picture of molecule (show polarity of
bonds)
Shape and bond angle
Is the molecule polar?
Lewis dot structure
3-D picture of molecule (show polarity of
bonds)
Shape and bond angle
Is the molecule polar?
Lewis dot structure
3-D picture of molecule (show polarity of
bonds)
Shape and bond angle
Is the molecule polar?
N
H
S
B
Formula
HCN
Is the molecule polar?
N
H
S
B
Formula
N2
Shape and bond angle
N
H
S
B
16
Physical Science
Bond T chart
Ionic Bonds
Covalent Bonds
17
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
Mg 2+
Ion
Cl -1
Compound
MgCl2
Name
Magnesium Chloride
18
19
20
Write the formula for compound formed by each pair of elements
.
Charge
Charge
Lithium
Nitrogen
Oxygen
Fluorine
Chlorine
Phosphorus
Sulfur
-3
+1
Li3N
Beryllium
Boron
Sodium
Aluminum
Magnesium
Calcium
Potassium
Barium
21
Write the name of each compound formed by the pairs of elements below.
Nitrogen
Lithium
Oxygen
Fluorine
Chlorine
Phosphorus
Sulfur
Lithium
Nitride
Beryllium
Boron
Sodium
Aluminum
Magnesium
Calcium
Potassium
Barium
22
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 ______________________________
23
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 __________________________
24
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 __________________________
25
Complete the following table, being sure that the total charge on the resulting
compound is zero.
Ions
Chloride
Cl1-
Hydroxide
OH1-
Nitrate
NO31-
Sulfate
SO42-
Sulfide
S2-
Carbonate
CO32-
Phosphate
PO43-
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+
26
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:
27
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 ___________________________
28
*Note: Oxidation Number is
another word for “charge.”
1-
29
30
Identify the following reactions as either:
SYNTHESIS (S), DECOMPOSTION (D), SINGLE
DISPLACEMENT (SD), DOUBLE DISPLACEMENT (DD)
_____ 1. 2H2 + O2  2H2O
_____ 2. N2 + 3H2  2NH3
_____ 3. 2HgO  2Hg + O2
_____ 4. Xe + 3F2  XeF6
_____ 5. P4 + 5O2  2P2O5
_____ 6. Zn + 2HCl  ZnCl2 + H2
_____ 7. Fe2(SO4)3 + 6KOH  3K2SO4 + 2Fe(OH)3
_____ 8. 2Al + 3FeO  Al2O3 + 3Fe
_____ 9. Al2(SO4)3 + 3Ca(OH)2  2Al(OH)3 + 3CaSO4
_____ 10. FeCl3 + 3NH4OH  Fe(OH)3 + 3NH4Cl
_____ 11. Ca(ClO3)2  CaCl2 + 3O2
_____ 12. 2Au2O3  4Au + 3O2
_____ 13. SiC + 2Cl2  SiCl4 + C
_____ 14. 3Fe + 4H2O  Fe3O4 + 4H2
_____ 15. 2H2O2  2H2O + O2
31
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
32
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?
33
Balancing Chemical Equations
Balance the equations below:
1)
____ N2 + ____ H2  ____ NH3
2)
____ KClO3  ____ KCl + ____ O2
3)
____ NaCl + ____ F2  ____ NaF + ____ Cl2
4)
____ H2 + ____ O2  ____ H2O
5)
____ Pb(OH)2 + ____ HCl  ____ H2O + ____ PbCl2
6)
____ AlBr3 + ____ K2SO4  ____ KBr + ____ Al2(SO4)3
7)
____ CH4 + ____ O2  ____ CO2 + ____ H2O
8)
____ C3H8 + ____ O2  ____ CO2 + ____ H2O
9)
____ C8H18 + ____ O2  ____ CO2 + ____ H2O
10)
____ FeCl3 + ____ NaOH  ____ Fe(OH)3 + ____NaCl
11)
____ P + ____O2  ____P2O5
12)
____ Na + ____ H2O  ____ NaOH + ____H2
13)
____ Ag2O  ____ Ag + ____O2
14)
____ S8 + ____O2  ____ SO3
15)
____ CO2 + ____ H2O  ____ C6H12O6 + ____O2
16)
____ K + ____ MgBr  ____ KBr + ____ Mg
17)
____ HCl + ____ CaCO3  ____ CaCl2 + ____H2O + ____ CO2
18)
____ HNO3 + ____ NaHCO3  ____ NaNO3 + ____ H2O + ____ CO2
19)
____ H2O + ____ O2  ____ H2O2
20)
____ NaBr + ____ CaF2  ____ NaF + ____ CaBr2
21)
____ H2SO4 + ____ NaNO2  ____ HNO2 + ____ Na2SO4
34
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
15. _____ Fe + _____ O2 →_____ Fe2O3
16. _____ Fe2(SO4)3 + _____ KOH →_____ K2SO4 + _____ Fe(OH)3
17. _____ C7H6O2 + _____ O2 →_____ CO2 + _____ H2O
18. _____ H2SO4 + _____ HI →_____ H2S + _____ I2 + _____ H2O
19. _____ FeS2 + _____ O2 →_____ Fe2O3 + _____ SO2
20. _____ Al + _____ FeO →_____ Al2O3 + _____ Fe
21. _____ Fe2O3 + _____ H2 →_____ Fe + _____ H2O
22. _____ Na2CO3 + _____ HCl →_____ NaCl + _____ H2O + _____ CO2
23. _____ K + _____ Br2 →_____ KBr
24. _____ C7H16 + _____ O2 →_____ CO2 + _____ H2O
25. _____ P4 + _____ O2 →_____ P2O5
35