APChem

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AP Chemistry - Summer Assignment
NOTE:
a. MUST SHOW ALL WORK FOR CREDIT!!
b. Where work is required, do on a separate sheet of paper
c. These are the foundational things you should be able to do when
you walk into class in the fall!
d. We will have a test over this material the first week of class.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Which value has only 4 significant digits?
a. 6.930
b. 0.0450
c. 8450
d. 0.392
____
2. Which is the sum of these values, to the appropriate number of significant digits?
17.358 + 3.502 + 20.14 =
a. 41
c. 41.000
b. 41.00
d. 41.0
____
3. Which is the product of these numbers, to the appropriate number of significant digits?
56.2  9.2057 =
a. 517
c. 517.36
b. 517.4
d. 517.00
____
4. How many significant digits are in the value 530,405,000?
a. 4
c. 6
b. 5
d. 9
____
5. How many significant digits are in the value 0.0050340?
a. 3
c. 7
b. 5
d. 8
Atom
Sodium
Chlorine
Protons
Atoms
Neutrons
12
17
Electrons
17
Mass Number
23
35
____
6. According to the table above, how many neutrons are in an atom of chlorine?
a. 17
c. 34
b. 18
d. 35
____
7. According to the table above, how many electrons are in an neutral atom of sodium?
a. 22
c. 12
b. 11
d. 23
____
8. Which is the number of protons in
a. 26
b. 30
?
c. 56
d. 82
____
9. Which is the number of neutrons in
a. 35
b. 45
?
c. 80
d. 115
____ 10. Which is the correct formula for the compound formed between beryllium and nitrogen?
a. BeN
c. Be3N2
b. Be3N
d. Be2N3
____ 11. What is the correct formula for the compound formed between magnesium and the phosphate ion?
a. MgPO4
c. Mg3(PO4)2
b. Mg3PO2
d. MgP2O8
____ 12. Which is the correct formula for the compound Manganese (III) Fluoride?
a. MnF
c. MnF3
b. Mn3F
d. Mn3F3
____ 13. Which is the correct formula for the compound Chromium (II) Nitrate?
a. (Cr)2NO3
c. CrNO2
b. Cr2NO3
d. Cr(NO3)2
____ 14. Which is the correct name for the compound FeS?
a. Iron Sulfide
c. Iron (II) Sulfide
b. Iron (I) Sulfide
d. Iron (II) Sulfide (II)
____ 15. Which is the correct name for the compound Na3P?
a. Sodium Phosphide
c. Sodium Phosphate
b. Sodium Phosphite
d. Sodium (III) Phosphide
____ 16. Which is the correct name for the compound CoCO3?
a. Carbon Oxygen Carbonate
c. Cobalt Carbonate
b. Cobalt (II) Carbonate
d. Cobalt Carbonoxide
____ 17. Which is the correct name for the compound CaClO2?
a. calcium chloride
c. calcium chlorite
b. calcium perchlorate
d. calcium chlorate
____ 18. Which is the correct name for the compound NH4SO4?
a. Nitrogen Hydrogen Sulfate
c. Ammonium (II) Sulfate
b. Nitrogen Hydrosulfate
d. Ammonium Sulfate
____ 19. Which of the following acids is named incorrectly?
a. HC2H3O2; acetic acid
c. H2SO3; sulfurous acid
b. HBr ; bromic acid
d. HClO3; chloric acid
____ 20. Which of the following elements is a metal?
a. Boron
b. Nitrogen
c. Magnesium
d. Carbon
____ 21. Which type of reaction can be recognized by the general pattern
a. combustion
c. single replacement
b. synthesis
d. Decomposition
?
____ 22. Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a. decomposition
c. synthesis
b. double replacement
d. combustion
____ 23. Which type of reaction is SiO2 + HF  SiF4 + H2O?
a. synthesis
c. single replacement
b. double replacement
d. combustion
____ 24. What are the correct coefficients when this equation is balanced? Sb + O2  Sb4O6
a. 1, 2, 10
c. 4, 3, 1
b. 4, 6, 1
d. 10, 5, 1
____ 25. Which are the product(s) of this reaction? Mg + N2 
a. NMg
c. Mg2N3
b. MgN
d. Mg3N2
____ 26. What are the correct coefficients when this chemical equation is balanced?
P4 + O2  P2O5
a. 4, 2, 7
c. 2, 5, 4
b. 1, 1, 1
d. 1, 5, 2
____ 27. Which is the molar mass of the element Calcium?
a. 20 g/mol
c. 40.078 g/mol
b. 40 g/mol
d. 20.180 g/mol
____ 28. Which is the correct molar mass for the compound FeSO4?
a. 103.85 g/mol
c. 415.4 g/mol
b. 151.85 g/mol
d. 247.85 g/mol
____ 29. Which is the mass of 8 moles of sodium chloride?
a. 7.3 grams
c. 0.137 g/mole
b. 468 grams
d. 468 moles
____ 30. How many grams are in 1.946 moles of NaCl?
a. 113.8 g
c. 0.033 g
b. 30.1 g
d. 44.7 g
____ 31. Calculate the number of molecules in 4.0 mol H2O.
a. 0.60  1023 molecules
c. 2.4  10–23 molecules
24
b. 2.4  10 molecules
d. 2.4  1023 molecules
____ 32. Which is the correct mole ratio for aluminum chloride to chlorine in the chemical reaction
AlCl3 + Br2  AlBr3 + Cl2? (Is the equation balanced?)
a. 1:1
c. 1:3
b. 2:3
d. 3:2
____ 33. Determine the empirical formula of a compound that contains 40.0% carbon, 53.3% oxygen and 6.67%
hydrogen by mass.
a. CH2O
c. C2H2O
b. C3H7O3
d. CHO2
____ 34. What is the percent composition of silicon nitride (Si3N4)?
a. 30.21% Si and 68.79% N
c. 54.03% Si and 45.97% N
b. 42.92% Si and 57.08% N
d. 60.06% Si and 39.94% N
____ 35. The empirical formula for a compound is CH2O, and the molar mass is 180.2g/mol. Which is the molecular
formula for this compound?
a. C6H12O6
c. C8H20O4
b. C7H16O5
d. C3H6O3
____ 36. How many moles of KBr will be produced from 7 moles of BaBr2?
BaBr2 + K2SO4  KBr + BaSO4 ( Is the equation balanced?)
a. 1 mole
b. 7 moles
c. 14 moles
d. 3.5 moles
____ 37. How many moles of Al would be produced from 20 moles of Al2O3?
Al2O3  Al + O2 (Is the equation balanced?)
a. 10 moles
b. 20 moles
c. 40 moles
d. 4 moles
____ 38. If 16.4 g of oxygen gas react with excess hydrogen gas, what mass of water can be produced?
(write and balance the equation first)
a. 9.23g
b. 18.5g
c. 20.4g
d. 23.9g
____ 39. Solid sodium metal and liquid water react to form sodium hydroxide and hydrogen gas. What mass of Na will
be needed to react with excess water to produce 15.0g NaOH?
(write and balance the equation first)
a. 4.3g
b. 5.4g
c. 8.6g
d. 11g
____ 40. What is the number of moles of carbon dioxide produced from the complete combustion of 5.42 moles of
ethanol (C2H6O). Write and balance the equation first. Remember, the combustion of ethanol requires oxygen
gas and produces carbon dioxide gas and water.
a. 5.42 moles
b. 2.71 moles
c. 10.84 moles
d. 16.3 moles
Short Answer
41. Write the formulas for each of the following compounds:
a) silicon dioxide
b) sodium sulfite
c) nitrogen trichloride
d) hydrobromic acid
e) calcium iodide
f) sulfurous acid
g) cesium perchlorate
h) ammonia
i) tin (II) fluoride
j) sulfur hexafluoride
k) potassium chlorate
l) aluminum nitride
m) sodium peroxide
n) nitric acid
o) ammonium sulfite
p) diphosphorous pentoxide
q) cobalt (III) nitrate
42.
How many oxygen atoms are there in 2.54 mg of Ca(OH)2?
SHOW ALL WORK AND SIG FIGS FOR CALCULATIONS!!
_________________________________________________________________________
43.
A sample of methane (CH4) has a mass of 31.1 g. How many molecules of methane are in this
sample? SHOW ALL WORK AND SIG FIGS FOR CALCULATIONS!!
_________________________________________________________________
44.
Which compound has the highest percent by mass of oxygen?
Ba(OH)2, Cu(NO3)2, H2O, H2SO4, H2O2
(show work)
45. Use the following reaction to answer questions a-g
Solid aluminum metal reacts with oxygen gas to produce solid aluminum oxide.
SHOW ALL WORK AND SIG FIGS FOR CALCULATIONS!!
a. Write and balance the equation above, including symbols for the states of matter.
________________________________________________________
b. How many moles of oxygen gas will it take to react completely with 0.400 moles of aluminum?
c. How many grams of oxygen gas is this?
d.How many grams of aluminum are in 0.400 moles?
e. How many grams of aluminum oxide can be produced from 0.400 moles of aluminum?
f. Add the masses of reactants used:___________________
g. Add the masses of products formed:__________________
h. How does the mass from part f compare to the mass from part g? What chemical law does this illustrate?
_____________________________________________________________________
46.
If 11.9g of magnesium chloride reacts with 34.2g of silver nitrate:
a) Write and balance the chemical reaction that occurs
b) Write the net ionic reaction that occurs. (You musts determine which of the products is not
soluble and will precipitate.)
c) Determine the limiting reactant
d) How many grams of the precipitate can theoretically be produced?
e) What is the mass of excess reactant?
_______________________________________________________________
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