Final Review - Semester 2
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FINAL EXAM REVIEW (due the day you take your final)
KMT
1.) Define "melting", "freezing", “evaporation" and "condensation."
2.) Describe the movement and the packing of molecules in solids, liquids, and gases.
3.) Describe what happens to the molecules in a solid when they heat up and turn into a liquid.
4.) Convert the following to Kelvin temperatures. Show your calculations: 25oC (room temperature); -180oC (the temperature at which nitrogen boils); 37oC (human body temperature); 100oC (water boiling point)
5.) Convert the following to Celsius temperature. Show your calculations: 1000 K; 50 K; 350 K;
6.) Write out all the units for temperature, pressure, and volume we discussed in class.
7.) Describe what happens to the water molecules when boiling and evaporation occur. What is in the bubbles at the bottom of the boiling water? Do water molecules break apart when evaporation occurs?
8.) Describe how water condenses on the outside of a cold glass. Where does the water come from? Why doesn’t a cold glass form condensation when the weather is very dry (such as in the winter time)?
PVnT
For problems 9-13 below, follow the steps outlined to you in class.
a) Write out the knowns and unknown variables
b) Identify the constants
c) Write out the cause and effect
d) Write out your calculations
9.) A closed syringe has an initial volume of 90 mL and a pressure of 1.5 atm. If you change the pressure to 0.8 atm, what is the final volume?
10.) A rigid steel container is filled with a gas that has an initial temperature of 700 degrees Celsius and a pressure of 1700 mmHg. What would you have to change the temperature to in order to achieve a final pressure of 900 mmHg?
11.) A rigid, stainless steel container initially has 3.5 puffs of air in it, and a pressure of 500 mmHg. If you want to change the pressure to 850 mmHg, how many puffs of air total do you need to have in the container?
12.) A piston held at a constant pressure of 3.5 atm and a volume of 2.4 L is at an initial temperature of 298 K. If the temperature is raised to 1000 K, what is the new volume of the piston?
13.) For each of the following gas law relationships, describe the relationship (for example, "T increases so P ______"), AND sketch a graph of the relationship: Pressure vs. temperature; Pressure vs. number of particles; Pressure vs. Volume; Volume vs. temperature.
Chemical Rxns/Balancing
14.) Balance the following equations
___P + ___H2 --> ___PH3
___CH4O + ___O2 ---> ___CO2 + ___H2O
___K + ___Cl2 ---> ___KCl
15.) Predict what you will see if you did the following reactions, and explain WHY you think you will see this:
Zn(s) + 2HCl(aq) --> H2(g) + ZnCl2(aq)
AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)
NaCl(s) + CaCl2(s) --> NaCl(s) + CaCl2(s)
16.) What is the difference between a reactant and a product? What is the difference between a physical change and a chemical change?
17.) Classify each of the chemical reactions as a combination, decomposition, single exchange, or double exchange reaction:
Moles/Molar Mass
20.) How many total atoms are there in the formula Al(NO3)3? Draw a particle model.
21.) How many oxygen atoms are there in the chemical formula Al2(CrO4)2? Draw a picture
22.) Determine the molar mass of the following compounds:
24.) How many grams are in 0.47 moles of Al2O3 ? Show all of your work and all units.
25.) How many grams are in 1.35 moles of SrCO3? Show all of your work and all units.
26.) How many moles are in 3.70 grams of Fe(OH)3? Show all of your work and all units.
27.) How many moles are in 5.82 grams of Al2(SO4)3 ? Show all of your work and all units.
ONLY DO THESE PROBLEMS IF YOU ARE IN HONORS CHEMISTRY
Stoichiometry
28.) Consider this balanced chemical equation: 1Cu (s) + 2AgNO3 (aq) --> 1Cu(NO3)2 (aq) + 2Ag (s)
A) Write the mole ratio equality of AgNO3 to Cu(NO3)2 Show units and labels.
B) If you start with 6.0 moles of AgNO3 and excess Cu, how many moles of Cu(NO3)2 can you make? Show your calculations.
C) How many GRAMS of Cu(NO3)2 can you make? Show your molar mass equality and all of your calculations including units. (Answer: 562.68 g)
29.) Consider this balanced chemical equation: 2NaCl (aq) + 1Pb(NO3)2 (aq) --> 2NaNO3 (aq) + 1PbCl2 (s)
A) Write the mole ratio equality of NaCl to PbCl2. Show units and labels.
B) Suppose you want to make 30.0 g of PbCl2. How many moles of PbCl2 are there in 30.0 grams?
C) How many moles of NaCl would be needed to complete this reaction? Show all of your calculations including units and labels on everything. (Answer: 0.216 moles NaCl)
D) Suppose you only made 27.6 g of PbCl2 instead of 30.0 g. What would be the percent yield? Show your work. (Answer : 92%)
30.) Consider the balanced chemical equation: 1 Mg + 2 O2 --> 2 MgO
A) Balance the chemical equation.
B) Consider the reaction if you started with 6 atoms of Mg and 4 molecules of O2. Draw a picture showing the reactants before the reaction takes place.
C) How many particles of MgO could you form with 6 atoms of Mg and 4 molecules of O2? Draw a picture showing what is left after the reaction takes place.
D) What is the limiting reactant? What is the excess reactant?
Molarity
31.) A 50.5 g sample of lithium nitrate, LiNO3, is dissolved in enough water to make 920 mL if solution. Determine the molar concentration of the lithium nitrate by following the following steps:
a) Write the molar mass equality for lithium nitrate.
b) Convert 50.5 g of LiNO3 to moles. Show all work and units.
c) Convert 920 mL to liters. Show all work and units.
d) Calculate the molar concentration of lithium nitrate. Show work and all units. (Ans: 0.796 mol/L)
32.) How many grams of potassium chromate, K2CrO4, would you need to make a 1.25 L solution of 0.85 M K2CrO4? Calculate by following the following steps:
a) Calculate the number of moles of K2CrO4 you need. Show all work and units. Start by rearranging the molarity equation and show your equation.
b) Write the molar mass equality for potassium chromate.
c) Convert moles to grams using factor labeling (dimensional analysis). (Ans: 206.3 grams)
33.) What volume is needed to make a 0.72 M solution that contains 25 grams of sodium chloride, NaCl? Solve by following the following steps:
a) Write the molar mass equality of sodium chloride, NaCl.
b) Convert grams of sodium chloride to moles. Show all work and units.
c) Rearrange the molarity equation to find volume. Check your notes to make sure you do this correctly. Calculate the volume in liters. (Ans: 0.594 L)
Acid/Base Chemistry and pH
35.) If an unknown solution reacts (bubbles) with calcium carbonate, is the solution an acid, base or neutral?
36.) Draw the pH scale, indicating where acids, bases and neutral substances are. Give an example of each.
37.) Explain why you cannot turn an acid into a base by diluting with water.
38.) What is a neutralization reaction? What would you use to neutralize an acid? What would you use to neutralize a base?
39.) Describe the relationship that exists between H+ concentration [H+] and pH.
40.) Predict the products for the reactions given below. Be sure to balance each equation, and be sure charges balance. If there is no reaction, briefly explain why:
___HBr + ___HCl -->
___HCl + ___NaOH -->
___HNO3 + ___Ca(OH)2 -->
___NaOH + ___Mg(OH)2 -->
Thermodynamics (Fire Unit)
41.) Draw the heating curve of water graph. Label the axes, and show where solid, liquid and gas phases are, and describe what is happening at each point in the curve)
42.) What is the freezing point of water in Celsius, Fahrenheit, and Kelvin.
43.) What is the boiling point of water in Celsius, Fahrenheit and Kelvin.
44.) Describe how temperature changes in both an endothermic and exothermic reaction.
45.) When carbon and hydrogen containing compounds undergo combustion, what products are produced?
46.) You dissolve some ammonium chloride, NH4Cl, in water. The initial temperature of the water was 20 degrees Celsius. After dissolving the NH4Cl, the temperature of the water dropped to 15.3 degrees Celsius. What is the change in temperature (ΔT)?
47.) Assume you have 1 gram of each of the substances below. Given their heat capacities (C), rank the following substances in order, going by which heats up the fastest to slowest.
Ethanol, C = 0.58 cal/g*C Aluminum, C = 0.22 cal/g*C water, C = 1.00 cal/g*C
Sodium, C = 0.29 cal/g*C Vegetable Oil, C = 0.40 cal/g*C
48.) Describe how heat is transferred through an object by conduction. Then, describe (using conduction) why it is better to insulate something with Styrofoam (which is mostly air) instead of aluminum foil.
Use the table below to answer questions 50-51
49.) Describe the changes in energy involved in bond breaking and bond making. Which one needs energy? Which one releases energy?
Consider the following reaction. Pictures of each molecule are shown below:
CH4 + 2O2 --> CO2 + 2H2O
50.) Using the table above, calculate the energy required to break all of the reactant bonds.
51.) Calculate the energy required to make all of the product molecules.
52.) Calculate the net energy change. Is the reaction endothermic or exothermic? How do you know?
53.) Draw an energy diagram for the reaction in #49. Label the reactants, products, activation energy, bond breaking energy, bond making energy, and net energy change.
54. Copy the three energy diagrams shown here.
a. Label the net energy change (heat of reaction) on each.
b. Label the activation energy on each.
c. Which diagram represents the most exothermic reaction?
d. Which reaction is endothermic?
55.) What is combustion? What is needed for combustion?
56.) Describe the type of bonding in each substance and determine if it will or will not combust:
a) Fe2O3 b) Cu c) SrCl2 d) C2H4 e) CO2
KMT
1.) Define "melting", "freezing", “evaporation" and "condensation."
2.) Describe the movement and the packing of molecules in solids, liquids, and gases.
3.) Describe what happens to the molecules in a solid when they heat up and turn into a liquid.
4.) Convert the following to Kelvin temperatures. Show your calculations: 25oC (room temperature); -180oC (the temperature at which nitrogen boils); 37oC (human body temperature); 100oC (water boiling point)
5.) Convert the following to Celsius temperature. Show your calculations: 1000 K; 50 K; 350 K;
6.) Write out all the units for temperature, pressure, and volume we discussed in class.
7.) Describe what happens to the water molecules when boiling and evaporation occur. What is in the bubbles at the bottom of the boiling water? Do water molecules break apart when evaporation occurs?
8.) Describe how water condenses on the outside of a cold glass. Where does the water come from? Why doesn’t a cold glass form condensation when the weather is very dry (such as in the winter time)?
PVnT
For problems 9-13 below, follow the steps outlined to you in class.
a) Write out the knowns and unknown variables
b) Identify the constants
c) Write out the cause and effect
d) Write out your calculations
9.) A closed syringe has an initial volume of 90 mL and a pressure of 1.5 atm. If you change the pressure to 0.8 atm, what is the final volume?
10.) A rigid steel container is filled with a gas that has an initial temperature of 700 degrees Celsius and a pressure of 1700 mmHg. What would you have to change the temperature to in order to achieve a final pressure of 900 mmHg?
11.) A rigid, stainless steel container initially has 3.5 puffs of air in it, and a pressure of 500 mmHg. If you want to change the pressure to 850 mmHg, how many puffs of air total do you need to have in the container?
12.) A piston held at a constant pressure of 3.5 atm and a volume of 2.4 L is at an initial temperature of 298 K. If the temperature is raised to 1000 K, what is the new volume of the piston?
13.) For each of the following gas law relationships, describe the relationship (for example, "T increases so P ______"), AND sketch a graph of the relationship: Pressure vs. temperature; Pressure vs. number of particles; Pressure vs. Volume; Volume vs. temperature.
Chemical Rxns/Balancing
14.) Balance the following equations
___P + ___H2 --> ___PH3
___CH4O + ___O2 ---> ___CO2 + ___H2O
___K + ___Cl2 ---> ___KCl
15.) Predict what you will see if you did the following reactions, and explain WHY you think you will see this:
Zn(s) + 2HCl(aq) --> H2(g) + ZnCl2(aq)
AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)
NaCl(s) + CaCl2(s) --> NaCl(s) + CaCl2(s)
16.) What is the difference between a reactant and a product? What is the difference between a physical change and a chemical change?
17.) Classify each of the chemical reactions as a combination, decomposition, single exchange, or double exchange reaction:
- H2 (g) + Cl2 (g) --> 2HCl (g)
- CaCO3 (s) --> CaO (s) + CO2 (g)
- Sn (s) + O2 (g) --> SnO2 (s)
- CaI2 (s) + Cl2 (g) --> CaCl2 (s) + I2 (g)
- AgNO3 (aq) + NaOH (aq) --> AgOH (s) + NaNO3 (aq)
- NaCl (aq) + AgNO3 (aq) --> NaNO3 (aq) + AgCl (s)
- CaCO3 (s) --> CaO (s) + CO2 (g)
Moles/Molar Mass
20.) How many total atoms are there in the formula Al(NO3)3? Draw a particle model.
21.) How many oxygen atoms are there in the chemical formula Al2(CrO4)2? Draw a picture
22.) Determine the molar mass of the following compounds:
- Fe2O3
- CaCO3
- Fe(NO3)3
24.) How many grams are in 0.47 moles of Al2O3 ? Show all of your work and all units.
25.) How many grams are in 1.35 moles of SrCO3? Show all of your work and all units.
26.) How many moles are in 3.70 grams of Fe(OH)3? Show all of your work and all units.
27.) How many moles are in 5.82 grams of Al2(SO4)3 ? Show all of your work and all units.
ONLY DO THESE PROBLEMS IF YOU ARE IN HONORS CHEMISTRY
Stoichiometry
28.) Consider this balanced chemical equation: 1Cu (s) + 2AgNO3 (aq) --> 1Cu(NO3)2 (aq) + 2Ag (s)
A) Write the mole ratio equality of AgNO3 to Cu(NO3)2 Show units and labels.
B) If you start with 6.0 moles of AgNO3 and excess Cu, how many moles of Cu(NO3)2 can you make? Show your calculations.
C) How many GRAMS of Cu(NO3)2 can you make? Show your molar mass equality and all of your calculations including units. (Answer: 562.68 g)
29.) Consider this balanced chemical equation: 2NaCl (aq) + 1Pb(NO3)2 (aq) --> 2NaNO3 (aq) + 1PbCl2 (s)
A) Write the mole ratio equality of NaCl to PbCl2. Show units and labels.
B) Suppose you want to make 30.0 g of PbCl2. How many moles of PbCl2 are there in 30.0 grams?
C) How many moles of NaCl would be needed to complete this reaction? Show all of your calculations including units and labels on everything. (Answer: 0.216 moles NaCl)
D) Suppose you only made 27.6 g of PbCl2 instead of 30.0 g. What would be the percent yield? Show your work. (Answer : 92%)
30.) Consider the balanced chemical equation: 1 Mg + 2 O2 --> 2 MgO
A) Balance the chemical equation.
B) Consider the reaction if you started with 6 atoms of Mg and 4 molecules of O2. Draw a picture showing the reactants before the reaction takes place.
C) How many particles of MgO could you form with 6 atoms of Mg and 4 molecules of O2? Draw a picture showing what is left after the reaction takes place.
D) What is the limiting reactant? What is the excess reactant?
Molarity
31.) A 50.5 g sample of lithium nitrate, LiNO3, is dissolved in enough water to make 920 mL if solution. Determine the molar concentration of the lithium nitrate by following the following steps:
a) Write the molar mass equality for lithium nitrate.
b) Convert 50.5 g of LiNO3 to moles. Show all work and units.
c) Convert 920 mL to liters. Show all work and units.
d) Calculate the molar concentration of lithium nitrate. Show work and all units. (Ans: 0.796 mol/L)
32.) How many grams of potassium chromate, K2CrO4, would you need to make a 1.25 L solution of 0.85 M K2CrO4? Calculate by following the following steps:
a) Calculate the number of moles of K2CrO4 you need. Show all work and units. Start by rearranging the molarity equation and show your equation.
b) Write the molar mass equality for potassium chromate.
c) Convert moles to grams using factor labeling (dimensional analysis). (Ans: 206.3 grams)
33.) What volume is needed to make a 0.72 M solution that contains 25 grams of sodium chloride, NaCl? Solve by following the following steps:
a) Write the molar mass equality of sodium chloride, NaCl.
b) Convert grams of sodium chloride to moles. Show all work and units.
c) Rearrange the molarity equation to find volume. Check your notes to make sure you do this correctly. Calculate the volume in liters. (Ans: 0.594 L)
Acid/Base Chemistry and pH
35.) If an unknown solution reacts (bubbles) with calcium carbonate, is the solution an acid, base or neutral?
36.) Draw the pH scale, indicating where acids, bases and neutral substances are. Give an example of each.
37.) Explain why you cannot turn an acid into a base by diluting with water.
38.) What is a neutralization reaction? What would you use to neutralize an acid? What would you use to neutralize a base?
39.) Describe the relationship that exists between H+ concentration [H+] and pH.
40.) Predict the products for the reactions given below. Be sure to balance each equation, and be sure charges balance. If there is no reaction, briefly explain why:
___HBr + ___HCl -->
___HCl + ___NaOH -->
___HNO3 + ___Ca(OH)2 -->
___NaOH + ___Mg(OH)2 -->
Thermodynamics (Fire Unit)
41.) Draw the heating curve of water graph. Label the axes, and show where solid, liquid and gas phases are, and describe what is happening at each point in the curve)
42.) What is the freezing point of water in Celsius, Fahrenheit, and Kelvin.
43.) What is the boiling point of water in Celsius, Fahrenheit and Kelvin.
44.) Describe how temperature changes in both an endothermic and exothermic reaction.
45.) When carbon and hydrogen containing compounds undergo combustion, what products are produced?
46.) You dissolve some ammonium chloride, NH4Cl, in water. The initial temperature of the water was 20 degrees Celsius. After dissolving the NH4Cl, the temperature of the water dropped to 15.3 degrees Celsius. What is the change in temperature (ΔT)?
47.) Assume you have 1 gram of each of the substances below. Given their heat capacities (C), rank the following substances in order, going by which heats up the fastest to slowest.
Ethanol, C = 0.58 cal/g*C Aluminum, C = 0.22 cal/g*C water, C = 1.00 cal/g*C
Sodium, C = 0.29 cal/g*C Vegetable Oil, C = 0.40 cal/g*C
48.) Describe how heat is transferred through an object by conduction. Then, describe (using conduction) why it is better to insulate something with Styrofoam (which is mostly air) instead of aluminum foil.
Use the table below to answer questions 50-51
49.) Describe the changes in energy involved in bond breaking and bond making. Which one needs energy? Which one releases energy?
Consider the following reaction. Pictures of each molecule are shown below:
CH4 + 2O2 --> CO2 + 2H2O
50.) Using the table above, calculate the energy required to break all of the reactant bonds.
51.) Calculate the energy required to make all of the product molecules.
52.) Calculate the net energy change. Is the reaction endothermic or exothermic? How do you know?
53.) Draw an energy diagram for the reaction in #49. Label the reactants, products, activation energy, bond breaking energy, bond making energy, and net energy change.
54. Copy the three energy diagrams shown here.
a. Label the net energy change (heat of reaction) on each.
b. Label the activation energy on each.
c. Which diagram represents the most exothermic reaction?
d. Which reaction is endothermic?
55.) What is combustion? What is needed for combustion?
56.) Describe the type of bonding in each substance and determine if it will or will not combust:
a) Fe2O3 b) Cu c) SrCl2 d) C2H4 e) CO2
Moles and Molar Mass Review Problems
1. How many particles are in 1 mole of hydrogen gas, H2? How many atoms are there in 1 mole of hydrogen gas?
2. How many particles are in 2 moles of ozone gas, O3? How many atoms are there in 2 moles of ozone?
3. How many total atoms are there represented in the formula Al(NO3)3? Draw a particle model.
4. How many oxygen atoms are there in the chemical formula Al2(CrO4)2? Draw a particle model.
The following problems are worth 2 points each.
5. Determine the molar mass of the following compounds:
- Fe2O3
- CaCO3
- Fe(NO3)3
- Mg3(PO4)2
6. How many grams are in 0.47 moles of Al2O3 ? Show all of your work and all units. Use dimensional analysis (factor label method).
7. How many grams are in 1.35 moles of SrCO3? Show all of your work and all units. Use dimensional analysis (factor label method).
8. How many moles are in 3.70 grams of Fe(OH)3? Show all of your work and all units. Use dimensional analysis (factor label method).
9. How many moles are in 5.82 grams of Al2(SO4)3 ? Show all of your work and all units. Use dimensional analysis (factor label method).
10. How many particles are in 0.72 moles of H2O? How many atoms are in 0.72 moles of H2O? Show all of your work and all units. Use dimensional analysis (factor label method).
Answers to 5-10 (answers mixed up, no units shown): 47.9, 4.33 x 1023, 262.87, 159.7, 0.0346, 241.88, 13.0 x 1023, 0.017, 199.3, 100.09,
Moles and Molar Mass (QUIZ REVIEW)
1. How many particles are in 1 mole of oxygen gas, O2? How many atoms are there in 1 mole of oxygen gas?
2. How many oxygen atoms are there formula Al2(SO3)3? Total atoms? Draw a particle model.
The following problems are worth 2 points each.
3. Determine the molar mass of the following compounds:
TiO2
- Sn(NO3)2
4. How many grams are in 0.58 moles of Fe2O3 ? Show all of your work and all units. Use dimensional analysis (factor label method).
5. How many moles are in 4.92 grams of Pb(OH)2? Show all of your work and all units. Use dimensional analysis (factor label method).
6. How many particles are in 0.82 moles of Au? Show all of your work and all units. Use the relationship
1 mol Au = 6.02 x 1023 particles Au. Use dimensional analysis (factor label method).
Answers to 3-6 (answers mixed up, no units shown): 4.94 x 1023, 92.63, 242.71, 0.204, 79.9
Chemical Reactions Test Review
Reactions homework problems (Test Review)
1. What is the difference between a reactant and a product?
2. Write an word interpretation for the following reaction between a solution of sodium chloride and a solution of silver nitrate:
NaCl (aq) + AgNO3 (aq) --> AgCl (s) + NaNO3 (aq)
3. Write an interpretation for the following reaction between a solution of sodium carbonate and hydrochloric acid:
Na2CO3 (aq) + 2HCl (aq) --> H2O (l) + CO2 (g) + NaCl (aq)
4. In words, describe the difference between sugar melting and sugar dissolving in water. The formula for sugar is C12H22O11. Then, write out the chemical equation for both of these processes. (hint: one of the equations involves "aq" while the other involves "l" for liquid)
5. Describe what you think you would observe in the lab for these chemical equations (hint: in some reactions, you may see bubbles):
8. Describe the following physical changes: melting, freezing, evaporation, condensation, sublimation, deposition.
9. Copy the following equations onto your paper and match the chemical equations with their descriptions:
B. To balance the effect of acid rain, solid calcium oxide has been added to many lakes. It reacts with water to form solid calcium hydroxide, a strong base that is only slightly soluble in water.
C. Chloramine gas is added to our water supply in very small amounts to kill bacteria.
D. When octane and oxygen gas are burned in our cars, carbon dioxide and water come out in the exhaust.
E. Saturated fatty acids, like palmitic acid, tend to form long solids and clog people's arteries. These saturated fatty acids can be made from unsaturated fatty acid by adding hydrogen gas.
10. For the equations in #9, label each one as a physical change or a chemical change.
11. Explain the law of conservation of mass.
12. Look at the following chemical reactions. What would you expect to happen to the mass of the reaction if the reaction was carried out in open space on a scale? Explain why you would see this.
14. Why do chemical equations need to be balanced?
15. How are the coefficients in chemical equations different from the subscripts in chemical formulas?
16-17. Balance the following chemical reactions:
20. What is the difference between a single exchange reaction and and double exchange reaction?
Reactions homework (Quiz Review) Due Monday 3/19 for Chen/Hereau; Fritz 3/20.
Predict what you will see if you did the following reactions, and explain WHY you think you will see this:
1. Zn(s) + 2HCl(aq) --> H2(g) + ZnCl2(aq)
2. AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)
3. NaCl(s) + CaCl2(s) --> NaCl(s) + CaCl2(s)
For the reactions in 1-2, complete the following sentences describing the reactions.
4. (describing equation #1) Solid zinc reacts with hydrogen chloride to produce ___________ and ____________ .
5. (describing equation #2) A solution of silver nitrate reacts with a solution of sodium chloride to produce ___________ and _____________ .
6. Why is it necessary to balance chemical equations?
Balance the following chemical equations (don't try this until after we balance equations)
6. ___H2O --> ___H2 + ___O2
7. ___P + ___H2 --> ___PH3
8. ___Na + ___HCl ---> ___H2 + ___NaCl
9. ___CH4O + ___O2 ---> ___CO2 + ___H2O
10. ___K + ___Cl2 ---> ___KCl
Answers to balancing reactions (coefficients problems are mixed up, but they are grouped together): [2, 1, 2, 2]; [3, 2, 2]; [1, 2, 2]; [1, 2, 2]; [2, 2, 3, 4]
1. What is the difference between a reactant and a product?
2. Write an word interpretation for the following reaction between a solution of sodium chloride and a solution of silver nitrate:
NaCl (aq) + AgNO3 (aq) --> AgCl (s) + NaNO3 (aq)
3. Write an interpretation for the following reaction between a solution of sodium carbonate and hydrochloric acid:
Na2CO3 (aq) + 2HCl (aq) --> H2O (l) + CO2 (g) + NaCl (aq)
4. In words, describe the difference between sugar melting and sugar dissolving in water. The formula for sugar is C12H22O11. Then, write out the chemical equation for both of these processes. (hint: one of the equations involves "aq" while the other involves "l" for liquid)
5. Describe what you think you would observe in the lab for these chemical equations (hint: in some reactions, you may see bubbles):
- Mg(s) + 2HCl (aq) --> H2 (g) + MgCl2 (aq)
- 2H2O2 (aq) --> 2H2O (l) + O2 (g)
- 2NaCl (aq) + Pb(NO3)2 (aq) --> 2NaNO3 (aq) + PbCl2 (s)
- Solid sodium chloride dissolves in water.
- Solid titanium reacts with oxygen gas (be careful with oxygen - it is diatomic) to produce titanium dioxide.
8. Describe the following physical changes: melting, freezing, evaporation, condensation, sublimation, deposition.
9. Copy the following equations onto your paper and match the chemical equations with their descriptions:
- CaO (s) + H2O (l) --> Ca(OH)2 (s)
- NH2Cl (g) --> NH2Cl (l)
- C16H30O2 (s) + H2 (g) --> C16H32O2 (s)
- 2C18H14 (l) + 23O2 (g) --> 16CO2 (g) + 14H2O (l)
- H2SO4 (aq) + CaCO3 (s) --> CaSO4 (aq) + CO2 (g) + H2O (l)
B. To balance the effect of acid rain, solid calcium oxide has been added to many lakes. It reacts with water to form solid calcium hydroxide, a strong base that is only slightly soluble in water.
C. Chloramine gas is added to our water supply in very small amounts to kill bacteria.
D. When octane and oxygen gas are burned in our cars, carbon dioxide and water come out in the exhaust.
E. Saturated fatty acids, like palmitic acid, tend to form long solids and clog people's arteries. These saturated fatty acids can be made from unsaturated fatty acid by adding hydrogen gas.
10. For the equations in #9, label each one as a physical change or a chemical change.
11. Explain the law of conservation of mass.
12. Look at the following chemical reactions. What would you expect to happen to the mass of the reaction if the reaction was carried out in open space on a scale? Explain why you would see this.
- NaCl (aq) + AgNO3 (aq) --> NaNO3 (aq) + AgCl (s)
- CaCO3 (s) --> CaO (s) + CO2 (g)
- CaCl2 (aq) + Na2CO3 (aq) --> 2NaCl (aq) + CaCO3 (s)
- Na2CO3 (aq) + C2H4O2 (aq) --> H2O (l) + NaC2H2O2 (aq) + CO2 (g)
14. Why do chemical equations need to be balanced?
15. How are the coefficients in chemical equations different from the subscripts in chemical formulas?
16-17. Balance the following chemical reactions:
- ___N2 (g) + ___H2 (g) --> ___NH3 (g)
- ___K (s) + ___I2 (s) --> ___KI (s)
- ___Mg (s) + ___Br2 (l) --> ___MgBr2 (s)
- ___KClO3 (s) --> ___KCl (s) --> ___O2 (g)
- ___C2H6 (g) + ___O2 (g) --> ___CO2 (g) + ___H2O (l)
- ___Al (s) + ___O2 (g) --> ___Al2O3 (g)
- ___P4 (s) + ___H2 (g) --> ___PH3 (g)
- H2 (g) + Cl2 (g) --> 2HCl (g)
- CaCO3 (s) --> CaO (s) + CO2 (g)
- Sn (s) + O2 (g) --> SnO2 (s)
- CaI2 (s) + Cl2 (g) --> CaCl2 (s) + I2 (g)
- AgNO3 (aq) + NaOH (aq) --> AgOH (s) + NaNO3 (aq)
20. What is the difference between a single exchange reaction and and double exchange reaction?
Reactions homework (Quiz Review) Due Monday 3/19 for Chen/Hereau; Fritz 3/20.
Predict what you will see if you did the following reactions, and explain WHY you think you will see this:
1. Zn(s) + 2HCl(aq) --> H2(g) + ZnCl2(aq)
2. AgNO3(aq) + NaCl(aq) --> AgCl(s) + NaNO3(aq)
3. NaCl(s) + CaCl2(s) --> NaCl(s) + CaCl2(s)
For the reactions in 1-2, complete the following sentences describing the reactions.
4. (describing equation #1) Solid zinc reacts with hydrogen chloride to produce ___________ and ____________ .
5. (describing equation #2) A solution of silver nitrate reacts with a solution of sodium chloride to produce ___________ and _____________ .
6. Why is it necessary to balance chemical equations?
Balance the following chemical equations (don't try this until after we balance equations)
6. ___H2O --> ___H2 + ___O2
7. ___P + ___H2 --> ___PH3
8. ___Na + ___HCl ---> ___H2 + ___NaCl
9. ___CH4O + ___O2 ---> ___CO2 + ___H2O
10. ___K + ___Cl2 ---> ___KCl
Answers to balancing reactions (coefficients problems are mixed up, but they are grouped together): [2, 1, 2, 2]; [3, 2, 2]; [1, 2, 2]; [1, 2, 2]; [2, 2, 3, 4]
Gas Law Test Review
1. Convert the following to Kelvin temperatures. Show your calculations: 25°C (room temperature); -180°C (the temperature at which nitrogen boils); 37°C (human body temperature); 100°C (water boiling point)
2. Convert the following to Celsius temperature. Show your calculations: 1000 K; 50 K; 350 K; 700 K
For all problems, follow the steps outlined to you in class.
a) Write out the knowns and unknown variables
b) Identify the constants
c) Write out the cause and effect
d) Write out your calculations
e) Draw two particle diagrams for "before" and "after"
3. A rigid (constant volume) stainless steel container has an initial pressure of 1.2 atm and a temperature of 25 degrees Celsius. What is the new pressure of the container if the container is put into an oven and heated to 450 degrees Celsius? Remember to change temperature to Kelvins.
4. A closed syringe has an initial volume of 22 mL and a pressure of 1.7 atm. If you want to change the pressure of the syringe to 1.1 atm, what does the new volume have to be?
5. A rigid, stainless steel container initially has 3.5 puffs of air in it, and a pressure of 500 mmHg. If you want to change the pressure to 850 mmHg, how many puffs of air total do you need to have in the container?
6. A piston held at a constant pressure of 3.5 atm and a volume of 2.4 L is at an initial temperature of 298 K. If the temperature is raised to 1000 K, what is the new volume of the piston?
7. A piston has an initial pressure of 550 mmHg, temperature of 20 degrees Celsius, and volume of 4 L. Assuming the amount of air in the piston remains constant, what is the new pressure if the temperature of the piston is increased to 600 degrees Celsius, and the volume of the piston is decreased to 2.7 L?
8. A rigid steel container is filled with a gas that has an initial temperature of 700 degrees Celsius and a pressure of 1700 mmHg. What would you have to change the temperature to in order to achieve a final pressure of 900 mmHg?
9. Convert 250 mmHg to psi. Use the conversion factor 760 mmHg = 14.7 psi to convert.
10. For each of the following gas law relationships, state what the relationship is (for example, "T increases so P ______"), state what kind of relationship this is (direct proportional or inverse), and sketch a graph of the relationship: Pressure vs. temperature; Pressure vs. number of particles; Pressure vs. Volume; Volume vs. temperature.
11. For the graphs in #10, draw particle diagrams at three different points along the graph like we did in class. Make sure you think about what is changing and what is constant (box size, number of particles, whooshie length).
Numerical Answers for 3-9 (no units, order mixed up): 2427.8, 34, 8.05, 2.91, 515, 4.84, 5.95
2. Convert the following to Celsius temperature. Show your calculations: 1000 K; 50 K; 350 K; 700 K
For all problems, follow the steps outlined to you in class.
a) Write out the knowns and unknown variables
b) Identify the constants
c) Write out the cause and effect
d) Write out your calculations
e) Draw two particle diagrams for "before" and "after"
3. A rigid (constant volume) stainless steel container has an initial pressure of 1.2 atm and a temperature of 25 degrees Celsius. What is the new pressure of the container if the container is put into an oven and heated to 450 degrees Celsius? Remember to change temperature to Kelvins.
4. A closed syringe has an initial volume of 22 mL and a pressure of 1.7 atm. If you want to change the pressure of the syringe to 1.1 atm, what does the new volume have to be?
5. A rigid, stainless steel container initially has 3.5 puffs of air in it, and a pressure of 500 mmHg. If you want to change the pressure to 850 mmHg, how many puffs of air total do you need to have in the container?
6. A piston held at a constant pressure of 3.5 atm and a volume of 2.4 L is at an initial temperature of 298 K. If the temperature is raised to 1000 K, what is the new volume of the piston?
7. A piston has an initial pressure of 550 mmHg, temperature of 20 degrees Celsius, and volume of 4 L. Assuming the amount of air in the piston remains constant, what is the new pressure if the temperature of the piston is increased to 600 degrees Celsius, and the volume of the piston is decreased to 2.7 L?
8. A rigid steel container is filled with a gas that has an initial temperature of 700 degrees Celsius and a pressure of 1700 mmHg. What would you have to change the temperature to in order to achieve a final pressure of 900 mmHg?
9. Convert 250 mmHg to psi. Use the conversion factor 760 mmHg = 14.7 psi to convert.
10. For each of the following gas law relationships, state what the relationship is (for example, "T increases so P ______"), state what kind of relationship this is (direct proportional or inverse), and sketch a graph of the relationship: Pressure vs. temperature; Pressure vs. number of particles; Pressure vs. Volume; Volume vs. temperature.
11. For the graphs in #10, draw particle diagrams at three different points along the graph like we did in class. Make sure you think about what is changing and what is constant (box size, number of particles, whooshie length).
Numerical Answers for 3-9 (no units, order mixed up): 2427.8, 34, 8.05, 2.91, 515, 4.84, 5.95
P-V, P-n, & P-T Quiz Review - Due 2/24, Friday
P-n, P-T, and P-V problems (Quiz review)
1. Convert the following to Kelvin temperatures. Show your calculations: -95°C (dry ice temperature); -80°C (the coldest place on earth); 50°C (really hot summer day); 801°C (melting point of table salt)
2. Convert the following to Celsius temperature. Show your calculations: 525 K; 93 K; 840 K; 1.5 K
For all problems, follow the steps outlined to you in class.
a) Write out the knowns and unknown variables
b) Identify the constants
c) Write out the cause and effect
d) Write out your calculations
e) Draw two particle diagrams for "before" and "after"
3. A rigid (constant volume) stainless steel container has an initial pressure of 2.4 atm and a temperature of 340 degrees Celsius. What is the new pressure of the container if the container is put into freezer and cooled to -120 degrees Celsius? Remember to change temperature to Kelvins.
4. A rigid, stainless steel container initially has 4.2 puffs of air in it, and a pressure of 1050 mmHg. If you want to change the pressure to 720 mmHg, how many total puffs of air do you need to have in the container?
5. A rigid steel container is filled with a gas that has an initial temperature of 420 degrees Celsius and a pressure of 800 mmHg. What would you have to change the temperature to in order to achieve a final pressure of 1100 mmHg? (Remember to change temperature to Kelvins, solve the problem, and convert back to Celsius)
6. A piston held at a constant pressure of 3.5 atm and a volume of 2.4 L is at an initial temperature of 298 K. If the temperature is raised to 1000 K, what is the new volume of the piston?
7. A piston has an initial pressure of 550 mmHg, temperature of 20 degrees Celsius, and volume of 4 L. Assuming the amount of air in the piston remains constant, what is the new pressure if the temperature of the piston is increased to 600 degrees Celsius, and the volume of the piston is decreased to 2.7 L? Remember to convert temperature to Kelvins.
8. Convert 960 mmHg to psi. Use the conversion factor 760 mmHg = 14.7 psi to convert.
Numerical Answers for 3-8 (no units, order mixed up): 18.57, 8.05, 2428, 9.62, 680, 2.88
1. Convert the following to Kelvin temperatures. Show your calculations: -95°C (dry ice temperature); -80°C (the coldest place on earth); 50°C (really hot summer day); 801°C (melting point of table salt)
2. Convert the following to Celsius temperature. Show your calculations: 525 K; 93 K; 840 K; 1.5 K
For all problems, follow the steps outlined to you in class.
a) Write out the knowns and unknown variables
b) Identify the constants
c) Write out the cause and effect
d) Write out your calculations
e) Draw two particle diagrams for "before" and "after"
3. A rigid (constant volume) stainless steel container has an initial pressure of 2.4 atm and a temperature of 340 degrees Celsius. What is the new pressure of the container if the container is put into freezer and cooled to -120 degrees Celsius? Remember to change temperature to Kelvins.
4. A rigid, stainless steel container initially has 4.2 puffs of air in it, and a pressure of 1050 mmHg. If you want to change the pressure to 720 mmHg, how many total puffs of air do you need to have in the container?
5. A rigid steel container is filled with a gas that has an initial temperature of 420 degrees Celsius and a pressure of 800 mmHg. What would you have to change the temperature to in order to achieve a final pressure of 1100 mmHg? (Remember to change temperature to Kelvins, solve the problem, and convert back to Celsius)
6. A piston held at a constant pressure of 3.5 atm and a volume of 2.4 L is at an initial temperature of 298 K. If the temperature is raised to 1000 K, what is the new volume of the piston?
7. A piston has an initial pressure of 550 mmHg, temperature of 20 degrees Celsius, and volume of 4 L. Assuming the amount of air in the piston remains constant, what is the new pressure if the temperature of the piston is increased to 600 degrees Celsius, and the volume of the piston is decreased to 2.7 L? Remember to convert temperature to Kelvins.
8. Convert 960 mmHg to psi. Use the conversion factor 760 mmHg = 14.7 psi to convert.
Numerical Answers for 3-8 (no units, order mixed up): 18.57, 8.05, 2428, 9.62, 680, 2.88
Pressure-Volume problems for Quiz (Due 2/14, Tuesday)
You MUST SHOW ALL WORK to receive credit!!!
1. Convert 470 mmHg to kPa. Use the conversion factor 760 mmHg = 101.3 kPa.
2. Convert 35 psi to atm. Use the conversion factor 1 atm = 14.7 psi.
3. Sketch a graph of pressure vs. volume where pressure is the dependent variable and volume is the independent variable. What type of relationship is this?
4. Explain why the curve in the graph of P vs. V does not cross the x-axis or y-axis at all. Think about what happens when the syringe plunger is pulled out all the way - what happens to the pressure? What happens to the pressure if the syringe plunger is pushed all the way in?
5-8 For all problems, follow the steps outlined to you in class.
a) Write out the knowns and unknown variables
b) Identify the constants
c) Write out the cause and effect
d) Write out your calculations
e) Draw two particle diagrams for "before" and "after"
5. A closed syringe has an initial volume of 35 mL and a pressure of 760 mmHg. If the volume of the syringe is adjusted to 42 mL, what is the new pressure in the syringe?
6. A closed syringe has an initial pressure of 13 psi and a volume of 25 cm3. The pressure inside the syringe is adjusted to 18 psi. What is the new volume of the syringe?
7. A closed syringe has an initial volume of 15 mL and a pressure of 2.4 atm. You pull the syringe back to a volume of 24 mL. What is the new pressure in the syringe?
8. A closed syringe has an initial volume of 90 mL and a pressure of 1.5 atm. If you change the pressure to 0.8 atm, what is the final volume?
Numerical Answers to questions 1-2, and 5-8 (mixed up, no units shown): 2.38, 18.06, 1.5, 62.6, 633.3, 168.75
Kinetic Molecular Theory HW - Due Friday, 1/20 (Honors Chemistry)
1. Define "kinetic molecular theory"
2. What does it mean for matter to "flow"? to "keep its shape?" to be "compressible?"
3. Describe solids, liquids, and gases in terms of flow, keeping shape, and compressibility.
4. Define "melting" and "freezing."
5. Define "evaporation" and "condensation."
6. Describe the movement and the packing of molecules in solids, liquids, and gases.
7. Describe what happens to the molecules in a solid when they heat up and turn into a liquid.
8. Describe what happens to the molecules in a liquid when they heat up and cool down. Why is there a space left at the top of bottles containing liquids?
SEMESTER 1 FINAL REVIEW - Due Tuesday 1/24 (1st Hr), Wednesday 1/25 (3 & 4th Hr), Thursday 1/26 (6th Hr)
Metric Units and Factor Label Method Quiz, Due Wednesday 1/18/12
Complete the assignment by showing all calculations or answering completely.
1. Complete the following conversion factors. Be sure to memorize these:
a) 1 m = ______ cm; b) 1 m = ______ mm; c) 1 km = ______ m;
d) 1 cm = ______ mm; e) 1 L = ______ mL;
f) 1 in = ______ cm; g) 1 ft = _______ in; h) 1 yard = _______ ft
2. Convert the following to scientific notation:
a) 385,100,000 b) 357 c) 0.000000518 d) 0.3551
3. Do the following calculations. Show your work.
a) (3.91 x 10^5) x (4.14 x 10^-3)
b) (4.98 x 10^-6) x (3.14 x 10^-4)
c) (6.97 x 10^8)
-----------------
(7.35 x 10^4)
d) (8.44 x 10^3)
----------------
(3.98 x 10^-7)
4. Use the factor label method to do the following conversions. You must show your work and all units to receive credit.
a) 893 km = ? inches (convert km to m, m to cm, cm to in, put answer in scientific notation)
b) 0.59 miles = ? cm (convert miles to ft, ft to in, in to cm, put answer in scientific notation)
c) 15.8 lbs = ? kg (use 1 kg = 2.20 lbs)
d) 3.51 ft = ? mm (convert ft to in, in to cm, cm to mm)
e) 56 calories = ? Joules
Smells 3 Quiz Review - Due 12/14/11, Wednesday (Honors Chem)
1. Explain in your own words what a polar molecule is.
2. Methanol, CH3OH, is attracted to a charged wand. The hydrogen atoms have a partial positive charge and the oxygen atom has a partial negative charge.
a. Draw a picture showing how you predict the methanol molecules are oriented when they are attracted to a wand with negative charges.
b. Do you expect methanol to bead up or spread out on waxed paper? Explain your thinking.
c. Do you expect methanol to dissolve in water? Explain your thinking.
3. Benzene, C6H6, is not attracted to a charged wand, and it spreads out on waxed paper. Do you expect benzene to dissolve in water? Explain your thinking.
4. How can you determine which atom in a covalent bond is partially positive?
5. Consider the following pairs of atoms. Place each set in order of increasing bond polarity. Describe the trend.
Li-F Na-F K-F Rb-F Cs-F
6. Place a partial positive or partial negative charge on each atom in the following pairs of atoms. Describe the trend.
H-B H-C H-N H-O H-F
7. Is hydrogen always partially positive when bonded to another atom? Explain.
8. Describe or draw what happens to the electrons in a polar covalent bond, a nonpolar bond, and an ionic bond.
9. Name three pairs of atoms with ionic bonds. For each pair show the difference in electronegativity between the two atoms.
10. Name three pairs of atoms with polar covalent bonds. For each pair show the difference in electronegativity between the two atoms.
11. Describe one theory of why small nonpolar molecules do not have a smell.
12. For each of the molecules listed, draw a Lewis dot structure and indicate the shape of the molecule. Decide whether these substances smell. Explain your reasoning for each.
a. H2Se b. H2 c. Ar d. HOF e. CHClF2
13. Methane, CH4, gas leaks can be very dangerous and explosive. Why do you think dimethyl sulfide, C2H6S, is added to natural gas that is used in homes and buildings?
2. Methanol, CH3OH, is attracted to a charged wand. The hydrogen atoms have a partial positive charge and the oxygen atom has a partial negative charge.
a. Draw a picture showing how you predict the methanol molecules are oriented when they are attracted to a wand with negative charges.
b. Do you expect methanol to bead up or spread out on waxed paper? Explain your thinking.
c. Do you expect methanol to dissolve in water? Explain your thinking.
3. Benzene, C6H6, is not attracted to a charged wand, and it spreads out on waxed paper. Do you expect benzene to dissolve in water? Explain your thinking.
4. How can you determine which atom in a covalent bond is partially positive?
5. Consider the following pairs of atoms. Place each set in order of increasing bond polarity. Describe the trend.
Li-F Na-F K-F Rb-F Cs-F
6. Place a partial positive or partial negative charge on each atom in the following pairs of atoms. Describe the trend.
H-B H-C H-N H-O H-F
7. Is hydrogen always partially positive when bonded to another atom? Explain.
8. Describe or draw what happens to the electrons in a polar covalent bond, a nonpolar bond, and an ionic bond.
9. Name three pairs of atoms with ionic bonds. For each pair show the difference in electronegativity between the two atoms.
10. Name three pairs of atoms with polar covalent bonds. For each pair show the difference in electronegativity between the two atoms.
11. Describe one theory of why small nonpolar molecules do not have a smell.
12. For each of the molecules listed, draw a Lewis dot structure and indicate the shape of the molecule. Decide whether these substances smell. Explain your reasoning for each.
a. H2Se b. H2 c. Ar d. HOF e. CHClF2
13. Methane, CH4, gas leaks can be very dangerous and explosive. Why do you think dimethyl sulfide, C2H6S, is added to natural gas that is used in homes and buildings?
Smells 1 & 2 Test Review - Due 12/14/11, Wednesday
Follow the link to the test review - http://sites.google.com/site/drvjchen/chemistry
Scroll down to where it says "Smells 1 & 2 Test Review"
Scroll down to where it says "Smells 1 & 2 Test Review"
Smells 1 Quiz Review - Due 12/01/11, Thursday
Quiz Homework:
1-2. What is a molecule, what kind of atoms are involved in molecules, and what kind of bonding holds them together?
3. What is the difference between a molecule and an atom?
4. Describe the patterns in the formulas and names for things that smell minty, sweet, fishy, and putrid.
5-6. Draw structural formulas of the following molecules using HONC 1234: one structure of C4H10, two unique structures of C4H10O, and two unique structures of C3H9N.
7. Draw Lewis dot symbols of C, N, O, F, and Ne.
8-10. Draw Lewis dot structures of the following compounds: H2, O2, F2, Br2, I2, N2, Cl2, CH2Cl2, H2S, HCl, NH3, PF3
More Practice (not going to be on the quiz)
Part B: These things have multiple bonds. Always start with carbon in the middle and branch outwards:
CO2, CH2O, C2H4, C2H
1-2. What is a molecule, what kind of atoms are involved in molecules, and what kind of bonding holds them together?
3. What is the difference between a molecule and an atom?
4. Describe the patterns in the formulas and names for things that smell minty, sweet, fishy, and putrid.
5-6. Draw structural formulas of the following molecules using HONC 1234: one structure of C4H10, two unique structures of C4H10O, and two unique structures of C3H9N.
7. Draw Lewis dot symbols of C, N, O, F, and Ne.
8-10. Draw Lewis dot structures of the following compounds: H2, O2, F2, Br2, I2, N2, Cl2, CH2Cl2, H2S, HCl, NH3, PF3
More Practice (not going to be on the quiz)
Part B: These things have multiple bonds. Always start with carbon in the middle and branch outwards:
CO2, CH2O, C2H4, C2H
Alchemy 4-5 Test Review - Due 11/16/11, Wednesday
Complete the assignment by answering in complete sentences.
1. Predict the flame colors of the following compounds: NaCl, Sr(NO3)2, CuSO4, KCl
2. Does nitrate produce a colored flame? Explain your thinking.
3. What do beryllium, Be, magnesium, Mg, and calcium, Ca, all have in common?
4. Summarize the key patterns of the shell model from the periodic table. Make sure you discuss how you can determine the number of shells in an atom, and the number of valence electrons.
5. How many valence electrons do the following elements have: Ca, S, Br, Al, P
6. Draw shell models for the elements B, F, and Ar. How many valence electrons does each atom have?
7. Define "ion."
8. Explain the difference between an anion and a cation.
9. What noble gas is closest to magnesium, Mg, on the periodic table? What must happen to Mg for it to have an electron arrangement similar to that of a noble gas? What is the charge of the Mg ion when it forms?
10. What noble gas is closest to sulfur, S, on the periodic table? What must happen to S for it to have an electron arrangement similar to that of a noble gas? What is the charge of the S ion when it forms?
11. When chlorine gains an electron to become a chloride ion with a -1 charge, it ends up with the electron arrangement of argon. Why doesn't it become an argon atom?
12. Write the cation, anion, compound formula, and compound name for combinations of the following elements:
13. Write the cation, anion, and compound name for the following combinations of ions:
14. Write the cation and anion in each compound, then determine the correct chemical formula:
15. Determine the charge on the transition metal cation in each of the compounds listed, then name the compound:
18. Determine the type of bonding in each substance:
1. Predict the flame colors of the following compounds: NaCl, Sr(NO3)2, CuSO4, KCl
2. Does nitrate produce a colored flame? Explain your thinking.
3. What do beryllium, Be, magnesium, Mg, and calcium, Ca, all have in common?
4. Summarize the key patterns of the shell model from the periodic table. Make sure you discuss how you can determine the number of shells in an atom, and the number of valence electrons.
5. How many valence electrons do the following elements have: Ca, S, Br, Al, P
6. Draw shell models for the elements B, F, and Ar. How many valence electrons does each atom have?
7. Define "ion."
8. Explain the difference between an anion and a cation.
9. What noble gas is closest to magnesium, Mg, on the periodic table? What must happen to Mg for it to have an electron arrangement similar to that of a noble gas? What is the charge of the Mg ion when it forms?
10. What noble gas is closest to sulfur, S, on the periodic table? What must happen to S for it to have an electron arrangement similar to that of a noble gas? What is the charge of the S ion when it forms?
11. When chlorine gains an electron to become a chloride ion with a -1 charge, it ends up with the electron arrangement of argon. Why doesn't it become an argon atom?
12. Write the cation, anion, compound formula, and compound name for combinations of the following elements:
- potassium and bromine
- calcium and oxygen
- lithium and oxygen
- calcium and chlorine
- aluminum and chlorine
- aluminum and oxygen
- magnesium and nitrogen
13. Write the cation, anion, and compound name for the following combinations of ions:
- sodium and carbonate
- magnesium and nitrate
- calcium and hydroxide
- aluminum and sulfate
- potassium and phosphate
14. Write the cation and anion in each compound, then determine the correct chemical formula:
- copper(II) sulfide
- nickel(II) nitrate
- iron(II) carbonate
- cobalt(II) sulfate
- iron(III) carbonate
- chromium(VI) oxide
15. Determine the charge on the transition metal cation in each of the compounds listed, then name the compound:
- HgS
- CuCO3
- NiCl2
- C3H6O(l), acetone (nail polish remover)
- Ti (s), titanium
- LiNO3 (s), lithium nitrate
- CuZn (s), bronze
18. Determine the type of bonding in each substance:
- zinc, Zn(s); propane, C3H8(l); calcium carbonate, CaCO3(s)
Alchemy 4 Quiz #2 Review - Due 11/4/11
Write the cation and anion (with charges), formula, and name for the following combinations of elements or groups:
1. Na and O
2. Ca and Cl
3. K and N
4. Rb and S
5. Mg and F
6. Al and Br
7. Al and O
8. Li and Br
9. Be and Cl
10. Ca and N
11. Sr and S
Write the cation and anion (with charges), formula, and name for the following combinations of elements or groups. Use your notes to write the anions.
12. Na and hydroxide
13. Ca and nitrate
14. Al and sulfate
15. Mg and phosphate
16. Sr and hydroxide
17. Al and nitrate
18. K and carbonate
19. Na and sulfate
20. Ca and phosphate
21. Ca and carbonate
22. Mg and nitrate
1. Na and O
2. Ca and Cl
3. K and N
4. Rb and S
5. Mg and F
6. Al and Br
7. Al and O
8. Li and Br
9. Be and Cl
10. Ca and N
11. Sr and S
Write the cation and anion (with charges), formula, and name for the following combinations of elements or groups. Use your notes to write the anions.
12. Na and hydroxide
13. Ca and nitrate
14. Al and sulfate
15. Mg and phosphate
16. Sr and hydroxide
17. Al and nitrate
18. K and carbonate
19. Na and sulfate
20. Ca and phosphate
21. Ca and carbonate
22. Mg and nitrate
Alchemy 3 Test Review - Due 10/21/11
Alchemy Investigation 3 Test (All Classes, 10/21/11)
Complete the assignment by answering in complete sentences.
1. What evidence caused Thomson to change Dalton's solid sphere model into the plum pudding model?
2. What evidence caused Rutherford to change Thomson's plum pudding model into the nuclear model?
3. What evidence caused Bohr to change Rutherford's nuclear model into the solar system model?
4. List the three parts of the atom and describe where each is located, the charge on each particle, and the mass of each particle.
5. Draw a solar system model showing one electron, one proton, and one neutron.
6. What does the atomic number of an element tell you? What does the atomic mass tell you?
7. Make a table like the one below. Use a periodic table to fill in the missing information
Element Chemical Symbol Atomic Number Number of protons Number of electrons Number of neutrons Mass of an atom Average atomic mass
Nickel 59
Ne 20
24 24.31
15 31
30 65
8. Draw a simple atomic model for an atom of neon, Ne.
9. Place the following elements in order from lowest number of protons to highest number of protons: S, Mg, N, Na, Se, Sr. Then give the following information about a neutral atom of each: name, atomic number, number of protons, number of electrons, group number.
10. Explain the difference between the average atomic mass given on the periodic table and the mass of an atom.
11. How are potassium-39, potassium-40, and potassium-41 different from each other? Write the isotope symbols for the three isotopes of potassium.
12. How many protons, neutrons, and electrons are in each: fluorine-23, cobalt-59, molybdenum-96
13. An isotope of iron, Fe, has 26 protons and 32 neutrons. What is the approximate mass for this isotope? Write the isotope symbol for this isotope.
14. Find the element phosphorus, P, on the periodic table. What is the average atomic mass of phosphorus? What is its atomic number? Predict which isotope you would find in greatest abundance for phosphorus.
15. Where are most of the radioactive isotopes found on the periodic table?
16. What is the difference between a nuclear reaction and a chemical reaction?
17. What is the difference between alpha decay and beta decay?
18. Explain why the mass of an atom changes when an alpha particle is emitted. Write an equation of an example reaction.
19. Explain why the mass number of an atom does not change when a beta particle is emitted. Write an equation of a example reaction.
20. Write equations for the following particles undergoing beta decay: potassium-42, iodine-131
21. Write equations for the following particle undergoing alpha decay: platinum-175, thorium-232
22. What is the difference between fission and fusion?
23. Write a nuclear equation for the formation of iron-54 through fusion.
Complete the assignment by answering in complete sentences.
1. What evidence caused Thomson to change Dalton's solid sphere model into the plum pudding model?
2. What evidence caused Rutherford to change Thomson's plum pudding model into the nuclear model?
3. What evidence caused Bohr to change Rutherford's nuclear model into the solar system model?
4. List the three parts of the atom and describe where each is located, the charge on each particle, and the mass of each particle.
5. Draw a solar system model showing one electron, one proton, and one neutron.
6. What does the atomic number of an element tell you? What does the atomic mass tell you?
7. Make a table like the one below. Use a periodic table to fill in the missing information
Element Chemical Symbol Atomic Number Number of protons Number of electrons Number of neutrons Mass of an atom Average atomic mass
Nickel 59
Ne 20
24 24.31
15 31
30 65
8. Draw a simple atomic model for an atom of neon, Ne.
9. Place the following elements in order from lowest number of protons to highest number of protons: S, Mg, N, Na, Se, Sr. Then give the following information about a neutral atom of each: name, atomic number, number of protons, number of electrons, group number.
10. Explain the difference between the average atomic mass given on the periodic table and the mass of an atom.
11. How are potassium-39, potassium-40, and potassium-41 different from each other? Write the isotope symbols for the three isotopes of potassium.
12. How many protons, neutrons, and electrons are in each: fluorine-23, cobalt-59, molybdenum-96
13. An isotope of iron, Fe, has 26 protons and 32 neutrons. What is the approximate mass for this isotope? Write the isotope symbol for this isotope.
14. Find the element phosphorus, P, on the periodic table. What is the average atomic mass of phosphorus? What is its atomic number? Predict which isotope you would find in greatest abundance for phosphorus.
15. Where are most of the radioactive isotopes found on the periodic table?
16. What is the difference between a nuclear reaction and a chemical reaction?
17. What is the difference between alpha decay and beta decay?
18. Explain why the mass of an atom changes when an alpha particle is emitted. Write an equation of an example reaction.
19. Explain why the mass number of an atom does not change when a beta particle is emitted. Write an equation of a example reaction.
20. Write equations for the following particles undergoing beta decay: potassium-42, iodine-131
21. Write equations for the following particle undergoing alpha decay: platinum-175, thorium-232
22. What is the difference between fission and fusion?
23. Write a nuclear equation for the formation of iron-54 through fusion.
Alchemy Investigation 3 Quiz Review - Due 10/17/11
Complete the assignment by answering in complete sentences.
1. Describe the key features of the solid sphere model of the atom and who developed this model.
2. Describe the key features of the plum pudding model of the atom and who developed this model.
3. Describe the key features of the nuclear model of the atom and who developed this model.
4. Describe the key features of the solar system model of the atom and who developed this model.
5. Describe the location and charge of all three parts of the atom (proton, neutron, and electron).
6. Describe how you determine the number of protons of an element.
7. Describe how you determine the number of electrons of an element and WHY you can do this for a neutral atom.
8. Describe how you determine the number of neutrons of an atom.
9. List the following pieces of information for the element sodium, Na
a) atomic number, number of protons,, number of electrons.
b) if an atom of sodium a mass of 23 amu, how many neutrons would this atom have? Show how you calculated this.
10. List the following pieces of information for the element fluorine, F
a) atomic number, number of protons,, number of electrons.
b) if an atom of fluorine has 10 neutrons, what would be the mass of this atom? Show how you calculated this.?
1. Describe the key features of the solid sphere model of the atom and who developed this model.
2. Describe the key features of the plum pudding model of the atom and who developed this model.
3. Describe the key features of the nuclear model of the atom and who developed this model.
4. Describe the key features of the solar system model of the atom and who developed this model.
5. Describe the location and charge of all three parts of the atom (proton, neutron, and electron).
6. Describe how you determine the number of protons of an element.
7. Describe how you determine the number of electrons of an element and WHY you can do this for a neutral atom.
8. Describe how you determine the number of neutrons of an atom.
9. List the following pieces of information for the element sodium, Na
a) atomic number, number of protons,, number of electrons.
b) if an atom of sodium a mass of 23 amu, how many neutrons would this atom have? Show how you calculated this.
10. List the following pieces of information for the element fluorine, F
a) atomic number, number of protons,, number of electrons.
b) if an atom of fluorine has 10 neutrons, what would be the mass of this atom? Show how you calculated this.?