1. By Carl Lyman © September 2001
Jeopardy Template
By Carl Lyman
© September 2001

2. Kinetics/Equilibrium
Jeopardy
Bonding
Kinetics/Equilibrium
Solutions
Acid/Base
100
200
300
400
500

3. Credits
That’s all folks.
Exit

4. Given the balanced equation: I + I → I2
Which statement describes the process represented by this equation?
A.) A bond is formed as energy is absorbed.
B.) A bond is formed and energy is released.
C.) A bond is broken as energy is absorbed.
D.) A bond is broken and energy is released.

5. Given the balanced equation: I + I → I2
Which statement describes the process represented by this equation?
A.) A bond is formed as energy is absorbed.
B.) A bond is formed and energy is released.
C.) A bond is broken as energy is absorbed.
D.) A bond is broken and energy is released.

6. Which atom will form an ionic bond with a Br atom?
B.) Li
C.) O
D.) C

7. Which atom will form an ionic bond with a Br atom?
Ionic Bond: Metal and a Nonmetal
Bromine is a nonmetal
A.) N
B.) Li
C.) O
D.) C

8. In which compound do atoms form bonds by sharing electrons?
A.) H2O
B.) Na2O
C.) CaO
D.) MgO

9. In which compound do atoms form bonds by sharing electrons?
Sharing = Covalent = 2 nonmetals
A.) H2O
B.) Na2O
C.) CaO
D.) MgO

10. Conductivity in a metal results from the metal atoms having
A.) high electronegativity
B.) high ionization energy
C.) highly mobile protons in the nucleus
D.) highly mobile electrons in the valence shell

11. Conductivity in a metal results from the metal atoms having
“Sea of Mobile Electrons”
A.) high electronegativity
B.) high ionization energy
C.) highly mobile protons in the nucleus
D.) highly mobile electrons in the valence shell

12. Which formula represents a polar molecule?
A.) Cl2
C.) CH4
B.) CO2
D.) NH3

13. Which formula represents a polar molecule?
Symmetric = nonpolar, Asymmetric = polar
A.) Cl2
C.) CH4
B.) CO2
D.) NH3

14. Which arrow represents the activation energy?
B.) 2
C.) 3 E
D.) 4
E.) 5

15. Which arrow represents the activation energy? What are the others?
Is it endothermic or exothermic?
A.) 1
Activation Energy
B.) 2
PE Reactants
C.) 3
PE Act. Complex E
D.) 4
PE Products
E.) 5
Heat of Reaction
Endothermic

16. A chemical reaction between iron atoms and oxygen molecules can only occur if
A.) the particles are heated
B.) the atmospheric pressure decreases
C.) there is a catalyst present
D.) there are effective collisions between the particles

17. A chemical reaction between iron atoms and oxygen molecules can only occur if
A.) the particles are heated
B.) the atmospheric pressure decreases
C.) there is a catalyst present
D.) there are effective collisions between the particles
Proper orientation and sufficient kinetic energy

18. At equilibrium, what is the rate of production of reactants compared with the rate of production of products?
A.) much higher
B.) higher
C.) the same
D.) lower

19. At equilibrium, what is the rate of production of reactants compared with the rate of production of products?
A.) much higher
Dynamic Equilibrium:
Rates equal,
Concentrations constant
B.) higher
C.) the same
D.) lower

20. What is the effect of adding more water to the following equilibrium reaction?
CO2 + H2O ↔ H2CO3
A.) More H2CO3 is produced.
B.) CO2 concentration increases.
C.) The equilibrium is pushed in the direction of reactants.
D.) There is no effect.

21. What is the effect of adding more water to the following equilibrium reaction?
CO2 + H2O ↔ H2CO3
Shift right, causing an increase in product concentration
A.) More H2CO3 is produced.
B.) CO2 concentration increases.
C.) The equilibrium is pushed in the direction of reactants.
D.) There is no effect.

22. If a system is left to change spontaneously, in what state will it end?
A.) the same state in which it began
B.) the state with lowest possible energy
C.) the state with the maximum disorder
D.) the state with the lowest possible energy consistent with the state of maximum disorder

23. If a system is left to change spontaneously, in what state will it end?
A.) the same state in which it began
B.) the state with lowest possible energy
C.) the state with the maximum disorder
D.) the state with the lowest possible energy consistent with the state of maximum disorder

24. At STP, which of these substances is most soluble in H2O?
A.) CCl4
C.) HCl
B.) CO2
D.) N2

25. At STP, which of these substances is most soluble in H2O?
Water is polar
like dissolves like
A.) CCl4
C.) HCl
asymmetric
polar
symmetric
nonpolar
B.) CO2
D.) N2
symmetric
nonpolar
symmetric
nonpolar

26. 100 grams of water is saturated with NH4Cl at 50oC
100 grams of water is saturated with NH4Cl at 50oC. If the temp is lowered to 10oC, how much NH4Cl will precipitate?
A.) 5.0 g
B.) 17 g
C.) 30. g
D.) 50. g

27. 100 grams of water is saturated with NH4Cl at 50oC
100 grams of water is saturated with NH4Cl at 50oC. If the temp is lowered to 10oC, how much NH4Cl will precipitate?
51g - 34g
A.) 5.0 g
B.) 17 g
C.) 30. g
D.) 50. g

28. What is the total number of grams of NaI(s) needed to make 1
What is the total number of grams of NaI(s) needed to make 1.0 liter of a M solution?
A.) 0.015
B.) 0.15
C.) 1.5
D.) 15

29. What is the total number of grams of NaI(s) needed to make 1
What is the total number of grams of NaI(s) needed to make 1.0 liter of a M solution?
A.) 0.015
Molarity = moles solute
Liters solution
0.010 M = X 1L
B.) 0.15
C.) 1.5
0.010mol x 150g =
1mol
D.) 15

30. How many milliliters of 12
How many milliliters of 12.0 M HCl(aq) must be diluted with water to make exactly 500. mL of 3.00 M hydrochloric acid?
A.) 100. mL
B.) 125. mL
C.) 200. mL
D.) 250. mL

31. How many milliliters of 12
How many milliliters of 12.0 M HCl(aq) must be diluted with water to make exactly 500. mL of 3.00 M hydrochloric acid?
A.) 100. mL
MV = MV
(12.0M)V = (3.00M)(500mL)
B.) 125. mL
C.) 200. mL
D.) 250. mL

32. At standard pressure when NaCl is added to water, the solution will have a
A.) higher freezing point and a lower boiling point than water
B.) higher freezing point and a higher boiling point than water
C.) lower freezing point and higher boiling point than water
D.) lower freezing point and a lower boiling point than water

33. At standard pressure when NaCl is added to water, the solution will have a
A.) higher freezing point and a lower boiling point than water
B.) higher freezing point and a higher boiling point than water
C.) lower freezing point and higher boiling point than water
D.) lower freezing point and a lower boiling point than water

34. An aqueous solution of an ionic compound turns red litmus blue, conducts electricity, and reacts with an acid to form a salt and water. This compound could be
A.) HCl
B.) NaI
C.) KNO3
D.) LiOH

35. BOTH: Conduct electricity (are electrolytes)
D) LiOH Statement describes a base and they end with OH
ACIDS
BASES
Start with H*
Example HCl(aq)
Taste sour
Turn blue litmus red
Clear in phenolphthalein
React with active metals to form H2 gas
React with carbonates to produce CO2 gas
pH < 7
End in OH*
Example NaOH(aq)
Taste bitter
Turn red litmus blue
Pink in phenolphthalein
Feel slippery
pH > 7
BOTH: Conduct electricity (are electrolytes)

36. The two Brönsted-Lowry acids are
H2O + CO3-2  OH- + HCO-3
The two Brönsted-Lowry acids are
A.) H2O and OH-
B.) H2O and HCO-3
C.) CO3-2 and OH-
D.) CO3-2 and HCO-3

37. The two Brönsted-Lowry acids are
H2O + CO3-2  OH- + HCO-3
The two Brönsted-Lowry acids are
A.) H2O and OH-
B.) H2O and HCO-3
Acids donate H+
C.) CO3-2 and OH-
D.) CO3-2 and HCO-3

38. Which pH indicates a basic solution?

39. Which pH indicates a basic solution?
pH < 7, acidic
pH = 7, neutral
pH > 7, basic
A.) 1
B.) 5
C.) 7
D.) 12

40. What is the pH of a 0.01 M solution of HNO3?
B.) 2
C.) 13
D.) 14

41. What is the pH of a 0.01 M solution of HNO3?
HNO3 dissociates to produce H+(H3O+) ions
A.) 1
B.) 2
This problem is saying [H3O+] = 0.01 M
C.) 13
pH = -log[H3O+]
pH = -log[0.01]
D.) 14

42. How many milliliters of 1 M NaOH are needed to exactly neutralize 100 milliliters of 1 M H2SO4?
A.) 50 mL
B.) 100 mL
C.) 200 mL
D.) 400 mL

43. How many milliliters of 1 M NaOH are needed to exactly neutralize 100 milliliters of 1 M H2SO4?
A.) 50 mL
Moles H+ = Moles OH-
MV = MV
2(1M)(100mL) = (1M)V
B.) 100 mL
C.) 200 mL
D.) 400 mL