Name: ______________________________________________ Previous Chemistry I Teacher: _______________
AP Chemistry II – Summer Review Packet 2014
Remember to round all numbers significantly and to include units for all numerical answers. You may use the
Modern Chemistry online textbook for help: www.my.hrw.com. Username: rcschemh. Password: rutherford.
Circle all your answers and show all your work. This will count as your first test grade in AP Chemistry II.
1. You are given 2.700 moles of sodium chloride, NaCl. How many grams of salt would you have?
2. Name the compound and determine the percentage composition of Ca3(PO4)2. Round to two decimal places.
3. How many atoms of gold are in a pure gold ring with a mass of 10.60 grams?
4. You are given 63.50 % Ag, 8.25 % N, 28.25 % O. Calculate the empirical formula.
5. The coefficients in a chemical equation represent the number of ____________ and the subscripts in a chemical formula
represent the number of _________________.
6. In the reaction Zn + 2HCl  ZnCl2 + H2, what is the molar ratio of hydrochloric acid to hydrogen gas? ________
7. The substance that restricts the participation of other reactants in a chemical reaction is known as the _____________ reactant.
8. The substance not completely used up in a chemical reaction is known as the ____________________ reactant.
9. What is the SI unit for mass? _____________ Temperature? ____________ Length? _____________
10. What volume would be occupied by 7.75 g of a substance with a density of 1.71 g/cm3?
11. For the reaction SO3 + H2O  H2SO4, calculate the percentage yield if 500.0 g of sulfur trioxide react with excess water to
produce 575.0 g of sulfuric acid. Round to two decimal places.
1|Page of 5
Name: ______________________________________________ Previous Chemistry I Teacher: _______________
12. How many silver atoms can be produced if 0.00350 g of Cu are reacted with excess AgNO3 according to the equation?
Cu + 2AgNO3  2Ag + Cu(NO3)2
13. If 100. g of CuS and 56.0 g of O2 are available using the equation 2CuS + 3O2  2CuO + 2SO2, which reactant is limiting?
Show your work.
14. Write these numbers in standard notation:
4.5 x 10 3
_____________________________
b) 8.997 x 10—2
_____________________________
a)
15. Convert the following measurements:
a)
10.5 g = ________________________ kg
b) 1.57 km = _______________________ m
c)
3.5 mol = ______________________ mmol (millimoles)
d) 1.25 L = ____________________ mL
e)
548.6 mL = ___________________ cm3
16. What is the molarity of a solution that contains 0.202 mol KCl in 7.980 L of solution?
17. Calculate the percentage error if a student experimentally measures the density of an object to be 4.224 g/mL and the
accepted value is 4.450 g/mL. Round to two decimal places.
18. What is the molarity of a solution that contains 125.0 g NaCl in a 4.00 L solution?
19. How many moles of HCl are present in 0.700 L of a 0.330 M HCl solution?
2|Page of 5
Name: ______________________________________________ Previous Chemistry I Teacher: _______________
20. Write these numbers in scientific notation:
a) 1,253,000
__________________________
b) 0.00755
__________________________
c) 102.400
__________________________
21. What is an electrolyte? What is the difference between a strong and weak electrolyte?
22. Homogeneous mixtures which appear uniform are called ______________________________.
23. Liquids that have particles that will settle out are called _______________________________.
24. The substance which is being dissolved in a solution is called the __________________________.
25. The substance doing the dissolving in a solution is called the _____________________________.
26. Calculate the molality of a solution that was prepared by dissolving 25.4 moles of sugar in 2.50 kg of water.
27. Draw the Lewis Dot Diagram of the following:
a)
Br2
b) H2O
c) NH3
d) CF4
28. How many protons, neutrons, and electrons are in the following elements?
Na
p+: _________
n0: __________ e-: ___________
b) S -2
p+: _________
n0: __________ e-: ___________
p+: _________
n0: __________ e-: ___________
a)
c)
K +1
29. As the concentration of the solute increases, the boiling point of the solution increases/decreases. (Circle)
30. Acids taste _____________________. Bases feel _______________________.
31. Strong acids are strong/weak electrolytes. (Circle)
32. A strong base will create a strong/weak conjugate acid. (Circle)
33. An amphoteric species is one that acts like _____________________________________________.
3|Page of 5
Name: ______________________________________________ Previous Chemistry I Teacher: _______________
34. Calculate the pH of an HCl solution with a [H3O+] concentration of 0.1250M.
35. What is the concentration of [OH¯ ] in pure water? _______________________________________________.
36. What is the pH of a neutral solution at 25°C? ______________.
37. A solution whose pH is less than 7 is said to be ______________ and greater than 7 is ____________.
38. Complete this acid-base neutralization reaction: H2SO4 + KOH  ___________ + ____________.
39. Write the electron configuration and noble gas notation for phosphorus.
EC: ________________________________
NGN: ______________________________
40. Write the orbital notation for phosphorus. ON: __________________________________________________
41. What is the molarity of a HCl-solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?
42. What is the molarity of a NaOH-solution if 3.47 mL is titrated by 11.1 mL of 0.0904 M HNO3?
43. Who discovered the electron and what was the name of his famous experiment? __________________________
44. Who discovered the nucleus and what was his famous experiment called? _____________________________
45. Whose definition of acids and bases emphasizes the role of protons (proton donors/acceptors)? _______
A. Brønsted-Lowery
B. Lewis
C. Bohr
D. Arrhenius
46. Reactions that split the nucleus of an atom into smaller daughter nuclei are called ______________ reactions.
47. Electronegativity values increase as one moves left/right and up/down on the periodic table. (circle)
48. Balance the following equation:
238
92
49.
239
U +
→
92U
How do you write the following particles in nuclear notation?
_______________________
Alpha Particle
____________________
Beta Particle
______________________
Positron
4|Page of 5
Name: ______________________________________________ Previous Chemistry I Teacher: _______________
50.
Chemical Formula
Mg(OH)2
Bond Type:
Ionic or Covalent
Ionic
Chemical Name
magnesium hydroxide
Al2O3
trinitrogen monoxide
sodium phosphate
N2O5
Fe2(CO3)3
SBr6
Covalent (molecular)
strontium chlorate
H3O7
Ca(NO3)2
lead (IV) sulfate
tin (IV) oxide
copper (II) sulfide
gold (III) chromate
51. A sample of fluorine gas at 45.0°C and 0.124 atm occupies a volume of 0.275 L. What volume (in liters) would this gas
occupy if the temperature is changed to -10.0°C but the pressure changes to 0.175 atm?
52. What is the pressure (in atm) of 2.55 mols of Br 2 at 150.0°C that is occupying 22.9 L of volume?
53. Determine the type of chemical reaction (right blank) and predict the products (left blank):
CH3OH + O2  ______________________________________________
_____________________
b) CaCO3  ___________________________________________________
_____________________
Sr + HCl  _________________________________________________
_____________________
d) NaOH + MgCl2  ____________________________________________
_____________________
a)
c)
---END
5|Page of 5