Download Ionic Compounds 1. What is the formula for aluminum phosphate

Spring Final
Ionic Compounds
1. What is the formula for aluminum phosphate?
2. Will fluorine form an anion, or a cation? Why?
3. What do the exponents in the ions Fe2+ and Fe3+ mean?
4. Write the correct chemical formula for the compound cobalt(III) oxide.
5. Write the correct chemical formula for the compound tin(II) phosphate.
Bonding – Trends, ions, naming ionic & covalent compound, Lewis Structures, VSEPR
1. For the elements Cs, F, and Cl, the order of increasing electronegativity is:
2. For the elements Rb, F, and O, the order of increasing atomic radius is:
3. Which of the following Lewis structures best describes BF3?
4. What are the VSEPR shapes of the following compounds: OF2 , NCl3
For the following COVALENT compounds:
- Draw Lewis Structrure
- Name VSEPR shape
- Name compound
5. NH3
6. H2O
7. CH4
8. Name/write the formula for the following compounds:
-
Sb2S3.
P2Se5.
PdO.
samarium trichloride.
molybdenum hexafluoride.
dinitrogen pentoxide.
dipotassium pentasulfide.
Stoichiometry – Balancing reactions, limiting reactants, percentage yield
1. What is the molar mass of ethanol (C2H5OH)?
2. What is the molar mass of cryolite (Na3AlF6)?
3. How many grams are in a 5.292-mol sample of sodium hydroxide?
4. Balance the reaction the following reactions:
-
As(OH)3(s) + H2SO4(aq) As2(SO4)3(aq) + H2O(1)
NH3(g) + O2(g) NO2(g) + H2O(g)
C4H10(g) + O2(g) CO2(g) + H2O(g)
PCl5 + H2O POCl3 + HCl
H2SnCl6 + H2S SnS2 + HCl
5. A 5.18-g sample of potassium chlorate was decomposed according to the following equation:
2KClO3  2KCl + 3O2
How many moles of oxygen are formed?
6. Consider the following reaction: CH 4 ( g )  4Cl2 ( g )  CCl4 ( g )  4 HCl ( g )
What mass of CCl4 is formed by the reaction of 1.71 g of methane with an excess of chlorine?
7. What is a limiting reactant?
Use the following information for answer questions 8-9:
Phosphoric acid, H3PO4 , can be prepared by reaction of sulfuric acid with “phosphate rock” according to the
equation:
Ca3(PO4)2(s) + 3H2SO4(aq)  3CaSO4(s) + 2H3PO4(aq)
8. What is the molar mass of Ca3(PO4)2?
9. How many moles of phosphoric acid is produced from 103 g of Ca3(PO4)2 and 18.1 g of H2SO4?
10. A 5.95-g sample of AgNO3 is reacted with BaCl2 according to the equation:
2AgNO3(aq) + BaCl2(aq)  2AgCl(s) + Ba(NO3)2(aq)
to actually produce 4.19 g of AgCl.
What is the percent yield of AgCl?
11. The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.6 g of CCl4, carbon tetrachloride:
2CHCl3(g) + Cl2(g)  2CCl4(g) +H2(g)
What is the percent yield?
12. Why must a chemical equation be balanced to solve stoichiometry problems? How is this related to a law of
chemistry (your answer should not just name the law, but explain it)?
13. Consider the equation O2(g) + CS2(l) CO2(g) + SO2(g). How does the equation violate the law of conservation of
mass? How can the equation be rewritten to conform to the law of conservation of mass?
Gases – Gas Laws, Ideal Gas Law, Gas Stoichiometry, KMT
Use the following to answer questions 1-2: Consider three 1-L flasks at STP. Flask A contains NH3 gas, flask B
contains NO2 gas, and flask C contains N2 gas.
1. Which contains the largest number of molecules?
2. In which flask do the molecules have the highest average velocity, speed?
3. A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is
21.6oC. Determine the temperature at which the volume of the gas is 3.46 L.
4. A balloon has a volume of 2.46 liters at 24.0oC. The balloon is heated to 48.0oC. Calculate the new
volume of the balloon.
5. Body temperature is about 308 K. On a cold day, what volume of air at 271 K must a person with a lung
capacity of 2.00 L breathe in to fill the lungs?
6. What volume is occupied by 19.6 g of methane (CH4) at 27oC and 1.23 atm?
7. Use the kinetic molecular theory of gases to predict what would happen to a closed sample of a gas
whose temperature increased while its volume decreased.
8. The following gases are at the SAME temperature. They are in a l.0 L scuba-diving tank. They are all at 1
atm. Order the gases from slowest to fastest: F2, Cl2, NO, NO2, CH4
9. What causes air pressure?
10. What is Boyle’s law?
11. What is Charles’s law?
12. What is Gay-Lussac’s law?
13. What is Avogadro’s law?
14. In the picture, the two balloons are at 0 degrees C, and 1 atm.
a. Which balloon contains more moles of gas?
b. Which balloon would weigh more?
c. Which law do these balloons demonstrate?
15. Explain why a soda with CO2 will lose its bubbles slower than soda with a N2
16. Explain why a cold soda loses its bubbles slower than a cold soda
Solutions – Like Dissolves Like, Molarity, Reaction Types, Solubility
1. An unknown substance dissolves in water but not in benzene (a nonpolar solvent). Molecules of what
type are present in the substance?
2. A 87.2-g sample of SrCl2 is dissolved in 112.5 mL of solution. Calculate the molarity of this solution.
3. How many grams of NaCl are contained in 350. mL of a 0.171 M solution of sodium chloride?
4. What mass of calcium chloride, CaCl2, is in 3.576 L of a 1.56 M solution?
5. Which of the following ion will produce an INSOLUBLE precipitate with a sulfate ion?
6. Which of the following compounds is SOLUBLE in water?
7. What does concentration measure? What is meant by a high/low concentration: a large amount of solvent or
solute?
8. How is a solute different from a solvent?
9. What property is necessary for two materials to dissolve in each other?
Reaction Types
1. Which of the following equations correctly describes the combustion of CH4 and O2 to produce water
(H2O) and carbon dioxide (CO2)?
a. Can you recognize a combustion equation?
2. Tell what type of chemical reaction is represented by the following chemical equation. Then balance the
equation: C3H8(g) + O2(g)
CO2(g) + H2O(l)
3. Tell what type of chemical reaction is represented by the following chemical equation. Then balance the
equation: Ga(s) + S(s)
Ga2S3(s)
4. Write a balanced equation, the complete ionic equation, and net ionic equation (if necessary) for the following
reactions. Label any precipitates with an (s)
a. Cu(s) + 2AgNO3(aq) 2Ag(s) + Cu(NO3)2(aq)
b. BaCl2(aq) + CuSO4(aq)  BaSO4(s) + CuCl2(aq)
c. Ni(NO3)2(aq) + CaCl2(aq)  NiCl2(aq) + CaNO(3)2(aq)
d. K2CO3(aq) + MgI2(aq)  2KI(aq) + MgCO3(s)
e. 3Na2CrO4(aq) + 2AlBr3(aq)  6NaBr(aq) + Al2(CrO4)3(s)
f. 2Au(NO3)3(aq) + 3Zn(s)  2Au(s) + 3Zn(NO3)2(aq)
g. barium nitrate + sodium sulfate 
h. sodium hydroxide + potassium bromide 
i. silver nitrate + potassium chloride 
Oxidation-Reduction Reactions – Oxidation, reduction, agents, balancing redox reactions
1. In which of the following does nitrogen have an oxidation state of +4?
A) HNO3
B) NO2
C) N2O
D) NH4Cl
E) NaNO2
For questions 2-5 use the following options:
A) Reduced
B) oxidized
C) the reducing agent
D) the oxidizing agent
E) both A and B
F) both A and C
G) both A and D
H) both B and C
I) both B and D
J) both C and D
2.
3.
4.
5.
In the reaction 2Cs(s) + Cl2(g) 2CsCl(s), Cl2 is
In the reaction P4(s) + 10Cl2(g) 4PCl5(s), the reducing agent is
In the reaction N2(g) + 3H2(g) 2NH3(g), N2 is
In the reaction C(s) + O2(g) CO2(g) carbon is
6. In the reaction 2Ca(s) + O2(g) 2CaO(s), which species is oxidized?
7. Balance the following oxidation-reduction reaction using the half-reaction method:
Fe3+ + I– Fe2+ + I2