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

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

Credits That’s all folks. Exit

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.

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.

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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.

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.

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

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

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

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

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

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

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 0.010 M solution? A.) 0.015 B.) 0.15 C.) 1.5 D.) 15

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 0.010 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

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

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

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

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

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

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)

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

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

Which pH indicates a basic solution?

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

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

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

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

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