Name ___________________________________________ Term 1 Final Practice Exam
1. Beaker A contains 2.06 mol of copper and beaker B contains 222 grams of silver. Which beaker contains the
larger mass?
2. Which beaker contains the larger number of atoms?
3. Fill in the table.
Isotope
Si-28
Si-29
Si-30
# of protons
# of electrons
# of neutrons
4. Rutherford’s experiment with gold foil established that
a. Atoms have mass
c. electrons have a negative charge
b. Neutrons are uncharged particles
d. the atom is mostly empty space
5.
Which particle has a charge of +1? a. electron
6. Which particle has the least mass?
a. electron
b. neutron
c. proton
b. neutron
c. proton
7. The atomic number of an element is the same as the number of
a. protons
b. neutrons
c. protons + electrons
d. protons + neutrons
8. How many neutrons are present in an atom that has an atomic number of 50 and a mass of 119?
9. What is the mass of 1.50 mol of sodium?
10. How many moles of carbon are in a 28.0 gram sample?
11. Which atom has more neutrons, potassium-40 or argon-40?
12. What is the mass of 1.20 X 1023 atoms of phosphorus?
Given the equation:
Zn + 2HCl  ZnCl2 + H2
13. If 2.5 mol of Zn are mixed with 6.0 mol of HCl, which reactant is limiting (used up)?
a.
Which reactant will be in excess and how many moles will be in excess?
b. How many moles of each product will be formed?
Given the equation:
2Fe(OH)3 + 3H2SO4  Fe2(SO4)3 + 6H2O
14. If 4.0 mol of Fe(OH)3 are mixed with 6.5 mol of H2SO4, which reactant will limit the reaction?
a. Which reactant will be in excess and how many moles will be in excess?
b. How many moles of each product will be formed?
Given the equation:
Cu + 2AgNO3  2Ag + Cu(NO3)2
15. If 2.50 mol of copper and 5.50 mol of silver nitrate are combined, which reactant will be limiting?
a. Which reactant will be in excess and how many moles will be in excess?
b. How many moles of each product will be formed?
Given the equation:
Cu + 2AgNO3  2Ag + Cu(NO3)2
16. If 2.00 grams of copper react with an excess of silver nitrate, how many grams of silver can theoretically be
produced?
17. Suppose that a student reacts 2.00 grams of copper in an excess of silver nitrate and filters and dries the
silver product. The student finds the mass of the silver to be only 6.50 grams. Why might the student’s
actual yield of silver be less than the theoretical yield of silver calculated in the previous problem (#16)?
Use the following equation to answer the next three questions.
Zn(solid) + 2HCl(liquid) 
ZnCl2 (aqueous) + H2(gas)
A student is given a small piece of zinc metal with a mass of 1.24 grams and a glass beaker with a mass of 65.46 grams.
The student places the zinc metal in the beaker and adds an excess of HCl. After the zinc bubbles and dissolves in the
acid, the student boils off the excess acid until there is only a white solid remaining in the beaker. The student finds the
mass of the beaker with the white solid in it to have a mass of 67.98 grams.
18. Calculate the theoretical yield of ZnCl2 that should be produced if the reaction goes to completion. (Show all
work!)
19. What was the actual yield of ZnCl2 produced? (Show all work!)
20. What is a logical explanation to account for the difference between the actual yield and the theoretical
yield?
When magnesium carbonate is heated above 500 ̊C it decomposes into magnesium oxide and carbon dioxide gas
according to the equation shown below.
MgCO3 (solid)

MgO (solid) + CO2 (gas)
21. Fill in the blank cells in the Data Table below
Mass of empty, dry crucible
Mass of crucible + MgCO3 (before heating)
Mass of MgCO3
Mass of crucible + MgO (after heating)
Mass of MgO
14.00 grams
15.20 grams
14.50 grams
22. Based on the amount of magnesium carbonate heated in the crucible, what theoretical mass of magnesium oxide
should have been produced?
23. What was the actual mass of magnesium oxide produced in the reaction?
24. What is a logical explanation for the difference between the theoretical mass and the actual mass of MgO?
25. When Rutherford fired positively charged alpha particles at a sheet of thin, gold foil, he found that most of the
particles went straight through, but occasionally one would bounce back. Which of the following is supported by this
observation?
a. Matter must contain negatively charged particles that are very small yet very massive
b. Matter must contain dense, positively charged particles that occupy a very small volume
c. Matter must contain positively charged particles that occupy most of the space within matter
d. Matter must contain negatively charged particles packed into a very small volume
26. Fill in the table below.
Subatomic particle
proton
electron
neutron
charge
+
Relative mass
Location in atom
Inside the nucleus
0
1
27. What element has 5 protons and 9 neutrons?
28. How many protons, electrons, and neutrons are in an atom that has an atomic number of four and a mass
number of nine?
Protons =
electrons =
neutrons =
29. How many protons, electrons, and neutrons are in Carbon-14?
protons =
electrons =
neutrons =
30. The formula for methane is CH4. How many hydrogen atoms are in one molecule of methane?
31. How many hydrogen atoms are in one mole of methane?
32. What is the mass of one mole of methane?
33. How many hydrogen atoms are in one molecule of water (H2O)?
34. How many hydrogen atoms are in one mole of water?
35. What is the mass of one mole of water?
36. How many of each type of atom are in one molecule of Al2(SO4)3?
37.What is the mass of one mole of Al2(SO4)3?
Al =
S=
O=