Multiple choice study guide
Cumulative portion:
1. Describe the structure of an atom.
2. Atomic number is the number of ______________ an atom has.
3. What are valence electrons?
4. An element’s outermost energy level is determined by its __________________ on the periodic
table.
5. The number of valence electrons an atom has is determined by its __________________ on the
periodic table.
6. Determine which groups correspond to the following electron orbitals:
s = _______________________
p = _________________________
d= _________________________
7. Describe the difference between a chlorine atom, Cl, and a chlorine ion Cl-.
8. Describe the difference between a potassium atom, K, and a potassium ion K+.
9. Describe how atomic radius changes moving across the periodic table from the upper right corner to
the lower left corner.
10. Describe how electronegativity changes moving from the upper right corner to the lower left corner.
11. How does reactivity change moving down a group on the periodic table?
12. Metals tend to form _________________ (+ or -) ions and nonmetals tend to form
_______________ (+ or -) ions.
13. What is the difference between a homogeneous mixture and a heterogeneous mixture?
14. Compare and contrast properties of ionic compounds with properties of molecular (covalent)
compounds.
Review (chapters 12-18)
15. Draw label the following graphs describing the gas laws:
a. pressure vs volume
b. pressure vs temperature
c. volume vs temperature
16. What is meant by Avogadro’s Principle?
17. Differentiate between an endothermic and exothermic reaction. Draw graphs of each.
18. How does increasing the concentration of reactants influence the direction of a reaction?
Increasing the concentration of the products?
A + B
C+D
19. What factors increase reaction rate?
20. How do catalysts alter activation energy and affect the rate of a reaction?
21. What is enthalpy and how is it calculated?
22. What is chemical equilibrium?
23. What factors increase the solubility of solids in liquids?
24. What factors increase the solubility of gases in liquids?
25. What is the equilibrium expression for the following hypothetical equation?
3A + 2 B
C + 5D
26. What is a solubility curve diagram and what does it illustrate?
Final study guide (short answers)
Name:_______________________________
1. Draw a graph illustrating the change in temperature of water as it changes from a solid to a liquid to a
gas.
2. How does the change in temperature of water during a phase change differ from the change in
temperature in between phase changes?
3. A sample of butane occupies 150L at 120kPa. At constant temperature, find the volume at 59 torr,
4. A gas has an original temperature of 20oC and an original pressure of 450 torr. If the volume is held
constant and the pressure of the gas changes to 710 torr, what is the new temperature?
5. a. How many molecules are in 30L of CH4 gas at STP.
b. Find the volume of 12.3g NO2 gas at STP.
c. How many grams of CO gas are in 160 ml at STP?
6. A gas has a pressure of 730 torr, a volume of 525L and is at a temperature of 30oC. Use the Ideal Gas
Law to find how many moles of gas are in this sample.
7. Use the following hypothetical reaction to answer the next question:
4A +
3B
7C +
9D
If 300 ml of gas B reacted, find the volume of:
A:
C:
D:
8. How many grams of glucose (C6H6O6) would you have to add to prepare 5L of 3.2 Molar glucose
solution?
9. Solution (I) is 170 ml 0.13M HCl and solution (2) is 270ml 0.16M HNO3.
a. Find the pH of each solution separately.
b. Find the pH of the mixture of solution 1 and 2.
10. After performing a titration, you must find the molarity of HNO3 if 93 ml of a 0.3M solution of NaOH
just titrates 76ml of a solution of nitric acid (HNO3) with an unknown molarity.
a. Complete and balance the neutralization equation: HNO3 + NaOH
b. Find the moles of the unknown solution.
c. Determine the molarity of HNO3.
11. What is a solubility curve? What does it illustrate?