Final Exam Review
When the equation Fe3O4 + Al --> A1203 + Fe is correctly balanced, what is the coefficient of Fe?
9
Which equation is not balanced? a. 2H2 + 02 --> 2H2O b. 4H3 + 202 --> 4H2O C. H2+H2+O2 --> H2O+H2O d. 2H2 + 02 --> H20
D. 2H2 + O2 --> H2O
What is the formula for zinc fluoride?
ZnF2
If 114 mL of 0.008 04 M NaOH completely titrates 118 mL of H3PO4 solution, what is the molarity of the H3PO4 solution? a. 0.002 59 M c. 0.007 77 M b. 0.005 18M d. 0.0105M
a. 0.00259 M
What is the pH of a solution whose hydronium ion concentration is 5.03 x 10-1 M? a. 0.2984 c. 1.542 b. 0.5133 d. 5.031
a. 0.2984
What is the number of moles of H2 produced when 23 g of sodium react with Water according to the equation 2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2(g)? a. 0.50 mol c. 2.0 mol b. 1.0 mol d. 4.0 mol
a. 0.50 mol
What is the concentration of OH- ions in pure water? a. 10-7 M c. 55.4 M b. 0.7 M d. 107 M
a. 10-7 M
How many milliliters of a 0.171 M solution contain 1.00 g of NaCl? (molar mass of NaCl = 58.44 g/mol) a. 1 00. mL c. 171 mL b. 1000. mL d. 17.1 mL
a. 100 mL
The standard molar volume of a gas at STP is a. 22.4 L. c. g-mol wt/22.4 L. b. g/22.4 L. d. 1 L.
a. 22.4 L
What is the equation for the ionization of Water? a. 2H20(l) <--> H3O+(aq) + OH'(aq) c. 2H20(l) <--> 2H2(g) + 02(g) b. 2H2O(l) <--> H3O'(aq) + OH+(aq) d. H2O(l)<--> H'(aq) + OH,+(aq)
a. 2H2O (l) <--> H3O+(aq) + OH-(aq)
Which reaction does not occur? a. 2HF (aq) + C12(g) --> F2(g) + 2HC1(aq) b. 2Na(s) + ZnF2(aq) --> 2NaF(aq) + Zn(s) c. Fe(s) + CuCl2(aq) --> FeCl2(aq) + Cu(S) d. 2HCl(aq) + Mg(S) --> MgCl2(aq) + H2(g)
a. 2HF + Cl2 --> F2 + 2HCl
If 0.500 mol of Na+ combines With 0.500 mol of C1' to form NaCl, how many formula units of NaCl are present? a. 3.01 x 10^23 c. 6.02 X 10^24 b. 6.02 x 10^23 d. 1
a. 3.01 x 10^23
All of the following are homogeneous mixtures except a. soil. c. gasoline. b. a sugar-water solution. d. a salt-water solution.
a. soil
In the equation HCIO4 + NH3 <-->NH4+ + ClO4-; ClO4- is a weak base and HCIO4 is a a. strong acid. c. weak acid. b. strong base. d. weak base.
a. strong acid
An acid ending with the suffix -ic produces an anion with the a. suffix -ate. c. prefix hydro-. b. suffix -ite. d. suffix -ous.
a. suffix -ate
Name the compound So3. a. sulfur trioxide c. selenium trioxide b. silver trioxide d. sodium trioxide
a. sulfur trioxide
What determines the average kinetic energy of the molecules of any gas? a. temperature c. container volume b. pressure d. molar mass
a. temperature
An equation for the dissociation of an ionic solid shows a. the solid on the left side and aqueous ions on the right side. b. an aqueous solid on the left side and ions on the right side. c. aqueous ions on the left side and the solid on the right side. d. ions on the left side and an aqueous solid on the right side.
a. the solid on the left side and aqueous ions on the right side
The molar mass of Mgl2 is a. the sum of the masses of 1 mol of Mg and 2 mol of I. b. the sum of the masses of 1 mol of Mg and 1 mol of I. c. the sum of the masses of 1 atom of Mg and 2 atoms of 1. d. the sum of the masses of 1 atom of Mg and 1 atom of 1.
a. the sum of the masses of 1 mol of Mg and 2 mol of I
What is the maximum possible amount of product obtained in a chemical reaction? a. theoretical yield c. mole ratio b. percentage yield d. actual yield
a. theoretical yield
Which compound dissociates to produce the ions SO42"(aq) and NH4+(aq)? a. NH4SO4(s) c. NH4(SO4)2(s) b- (NH4)2SO4(s) d- (NH4)3(SO4)2(S)
b. (NH4)2SO4
What is the approximate freezing-point depression of nonvolatile aqueous electrolyte solutions? a. -1.86C°/m x molality of electrolyte b. -1 .86C°/m x total molality of solute particles c. -1 .86C° d. 0.52C°/m x total molality of solute particles
b. -1.86C/m x total molality of solute particles
What is the oxidation number of oxygen in most compounds? a. -8 c. 0 b. -2 d. +1
b. -2
Which expression represents the pH of a solution? a. log[H3O+] c. 1og[OH-] b. -1og[H3O+] d. -1og[OH-]
b. -log[H3O+]
What is the oxidation number of a pure element? a. -l c. +1 b. 0 d. 8
b. 0
What is the molarity of an H3PO4 solution if 358 mL is completely titrated by 876 mL of 0.0102 M Ba(OH)2 solution? a. 0.0111 M c. 0.025oM b. 0.0166M d. 0.0333 M
b. 0.0166M
What is the product of H3O+ ion and OH- ion concentrations in water? a. 10-28 c. 10-7 b. 10-14 d. 55.4
b. 10-14
What is the percentage composition of CF4? a. 20% C, 80% F c. 16.8% C, 83.2% F b. 13.6% C, 86.4% F d. 81% C, 19% F
b. 13.6% C, 86.4% F
he Word equation solid carbon + oxygen gas --> carbon dioxide gas + energy, represents a chemical reaction because a. the reaction releases energy. b. CO2 has chemical properties that differ from those of C and O. c. the reaction absorbs energy. d. CO2 is a gas and carbon is a crystal.
b. CO2 has chemical properties that differ from those of C and 0
How do K_a Values for Weak and strong acids compare? a. Ka (Weak) = Ka (strong) c. Ka (Weak) > Ka (strong) b. Ka (weak) < Ka (strong) d. not defined for weak acids
b. Ka(weak) < Ka(strong)
What is the balanced equation for the combustion of sulfur'? a. S(s) + 02(g) --> S0(g) b- S(s) + 02(g) --> S02(g) c. 2S(s) + 3O2(g) --> SO3(s) d. S(s) + 2O2(g) --> SO42-(aq)
b. S(s) + O2(g) --> SO2(g)
What is the empirical formula for a compound that is 53.3% 0 and 46.7% Si? a. SiO c. Si2O b. SiO2 d. Si2O3
b. Si02
What is the approximate freezing-point depression of a 0.010 m aqueous CaCl2 solution? Kf = -l .86°C/m. a. -0.ol9°C c. -0.056°C b. -0.03 7°C d. -0.074°C
c. -0.056 C
The Volume of a gas is 400.0 mL when the pressure is 1.00 atm. At the same temperature, what is the pressure at which the Volume of the gas is 2.0 L? a. 0.5 atm c. 0.20 am b. 5.0 atm d. 800 atm
c. 0.20 atm
A water solution containing an unknown quantity of a nonelectrolyte solute has a freezing point of -0.665°C. What is the molal concentration of the solution if Kf= -1.86°C/m? a. 0.01om c. 0.358m b. 0.355 m d. 2.66 m
c. 0.358m
What is the solubility~product constant of magnesium hydroxide, Mg(OH)2? Its solubility is 9.0 X 10-1 g/100 g H20. The molar mass ofMg(OH)2 is 58.32 g/mol. a. 1.8 x 104 c. 1.5 x 10-11 b. 4.5 x 10-9 d. 6.2 X 10-12
c. 1.5 x 10-11
What is the solubility in mol/L of cobalt(II) sulfide, COS? Its K_sp, Value is 3.0 X 10-35. a. 5.9 x 10-10 c. 1.7 x 10-13 b. 1.7 x 10-12 d. 1.7 x 10-25
c. 1.7 x 10 -13
Which expression represents the concentration of H30' ions in solution? a. 10-14 - [OH-] c. 10-14 / [OH-] b. 10-14 x [OH-] d. [OH-] + 10-14
c. 10-14 / [OH-]
The concentration of a water solution of NaCl is 2.48 m, and it contains 806 g of water. How much NaCl is in the solution? (molar mass of NaCl = 58.44 g/mol) a.. 2.00g c. 117g b. 89.3 g d. 224 g
c. 117g
For the reaction represented by the equation 2H2 + O2 --> 2H2O, how many moles of Water can be produced from 6.0 mol of oxygen? 21. 2.0 mol . c. 12 mol b. 6.0 mol d. 18 mol
c. 12 mol
How many moles of ions are produced by the dissociation of 1 mol of NH4Br? a. 0 c. 2 mol b. 1 mol d. 5 mol
c. 2 mol
How many OH' ions are present in 3.00 mol of Ca(OH)2'? a. 3.00 c. 3.61 x 10^24 b. 6.00 d. 2.06 x 10^23
c. 3.61 x 10^24
The molar mass of NH3 is 17.03 g/mol. HOW many moles of NH3 are present in 107.1 g? a. 0.1623 mol c. 6.289 mol b. 3.614 mol d. 107.1 mol
c. 6.289 mol
A compound of low solubility a. is always a strong electrolyte. c. may be a strong or a weak electrolyte. b. is always a weak electrolyte. d. is always a nonelectrolyte.
c. may be a strong or a weak electrolyte
Which of the following is expressed in grams of solute instead of moles of solute? a. molality c. Neither (a) nor (b) b. molarity d. Both (a) and (b)
c. neither a nor b
Name the compound KClO3. a. potassium chloride c. potassium chlorate b. potassium trioxychlorite _ d. hypochlorite
c. potassium chlorate
Bases feel a. rough. c. slippery. b. moist. d. dry.
c. slippery
What is the oxidation number of sulfur in H2S04? a. -2 ' c. +4 b. 0 d. +6
d. + 6
What is the freezing~point depression of an aqueous solution of an electrolyte that produces three ions for every formula unit that dissociates if the electrolyte's concentration is 1.25 m? K_f= -1.86°C/m. a. -125°C c. -558°C b. -l.86°C d. -698°C
d. -698 C
What is the molality of a solution that contains 5.10 mol KNO3 in 4.47 kg water? (molar mass of KNO3 = 101.11 g/mol) a. 0.315 m c. 1.02 m b. 0.779 m d. 1.14 m
d. 1.14m
Calculate the ion product for mixing 300 mL of 0.000 30 M Sr(NO3)2 With 200 mL of 0.000 025 M K2S04. K_sp, for SrSO4 is 3.2 x 10-7. Does a precipitate form? a. 5.6 X 10-5; yes c. 1.8 x 10-9; yes b. 5.6 X 104; no d. 1.8 x 10-9; no
d. 1.8 x 10-9; no
The antilogarithm of a number,y, is a. the inverse of y. c. y raised to the power of 10. b. the square root of y. d. 10 raised to the power of y.
d. 10 raised to the power of y
An equilibrium mixture of So2, 02, and So3 gases at 1500 K is determined to consist of 0.344 mol/L So2, 0.172mol/L O2, and 0.56 mol/L So3. What is the equilibrium constant for the system at this temperature? The balanced equation for this reaction is 2SO2(g) + O2(g) --> 2SO3(g). a. 0.41 c. 6.7 b. 2.8 d. 15
d. 15
Which of the following is perchloric acid? a. HCIO c. HCIO3 b. HClO2 d. HClO4
d. HClO4
What is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen? a. P307 C. P203 b. PO3 d. P205
d. P205
A molecular compound has the empirical formula XY3. Which of the following is a possible molecular formula? a. X2Y3 C. X2Y5 b. XY4 d. X2Y6
d. X2Y6
In What kind of reaction do two or more substances combine to form a new compound? a. decomposition reaction c. double-displacement reaction b. combustion reaction d. synthesis reaction
d. synthesis reaction
In what kind of reaction do two or more substances combine to form a new compound? a. decomposition reaction c. double-displacement reaction b. ionic reaction d. synthesis reaction
d. synthesis reaction
In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is equal to a. 0. c. 10. b. the number of atoms in the ion. d. the charge of the ion.
d. the charge of the ion
If the rate of evaporation from the surface of a liquid exceeds the rate of condensation, a. the system is in equilibrium. b. the liquid is boiling. c. energy as heat is no longer available. d. the concentration of the vapor is increasing.
d. the concentration of the vapor is increasing
If the temperature of a container of gas remains constant, how could the pressure of the gas increase? a. The mass of the gas molecules increase. b. The diffusion of the gas molecules increases. c. The size of the container increases. d. The number of gas molecules in the container increases.
d. the number of gas molecules in the container increases
For the reaction represented by the equation 2Na + 2H2O --> 2NaOH + H2, how many grams of hydrogen are produced if 120. g of sodium and 80. g of water are available? a. 4.5 g c. 80. g b. 45 g d. 200 g
a. 4.5 g
How many oxygen atoms are there in 0.500 mol of CO2? a. 6.02 X 10^23 c. 15.9994 b. 3.01 x 10^23 d. 11.0
a. 6.02 x 10^23
For the reaction represented by the equation CH4 +202 --> CO + 2H2O, how many moles of carbon dioxide are produced from the combustion of 100. g of methane'? a. 6.23 mol c. 12.5 mol b. 10.8 mol d. 25 mol
a. 6.23 mol
For the reaction represented by the equation N2 + 3H2 -->2NH3, how many moles of nitrogen are required to produce 18 mol of ammonia? a. 9.0 mol c. 27 mol b. 18 mol d. 36mol
a. 9.0 mol
How many molecules are there in 5.0 g of methyl alcohol, CH3OH? a. 9.4 x 10^22 c. 3.6 x 10^24 b. 3.0 x 10^24 d. 3.8 x 10^24
a. 9.4 x 10^22
In the reaction represented by the equation NH3 + H20 --> NH + OH", H20 is a(n) a. Brensted-Lowry acid. c. Brrz5nsted-Lowry base. b. Lewis base. d. Arrhenius.
a. Bronsted-Lowry acid
In the equilibrium system CH3COOH(aq) + H2O(l) <--> H3O+(aq) + CH3COO'(aq), which species is present in the highest concentration at equilibrium? a. CH3COOH b. H3O+ c. CH3COO' d. Equal concentrations of CH3COOH, H3O* and CH3COO' are present.
a. CH3COOH
Which compound is produced by a neutralization? a. H2O(l) c. Ca(OH)2(s) b. HNO3(aq) d. H3PO4(aq)
a. H2O(l)
Which of the following is not an oxyacid? a. H202 C. HClO4 b. H2SO4 d. HCIO2
a. H2O2
Which of the following is a diprotic acid? a, H2S04 C. HCl b. CH3COOH d. H3PO4
a. H2SO4
All of the following equations are statements of the ideal gas law except a. P = nRTV c. P/n = RT/V b. PV/T = nR d. R=PV/nT
a. P = nRTV
Reactions tend to run to completion if a. a gaseous product forms and escapes. b. a product in the same phase as the reactants forms. c. one product is highly ionized. d. one product is highly soluble.
a. a gaseous product forms and escapes
A standard solution always contains a. a known concentration of solute. c. a base. b. an acid. d. a primary standard.
a. a known concentration of solute
A chemical formula for a molecular compound represents the composition of a. a molecule. c. the ions that make up the compound. b. an atom. d. the crystal lattice.
a. a molecule
Which of the following is at equilibrium when undissolved solute is visible? a. a saturated solution c. a supersaturated solution b. an unsaturated solution d. All of the above
a. a saturated solution
Which of the following is a homogeneous mixture of substances in a single phase? a. a solution c. a compound b. a colloid d. a suspension
a. a solution
Which acid is found in vinegar? a. acetic acid c. phosphoric acid b. nitric acid ' d. hydrochloric acid
a. acetic acid
Bases react with a. acids to produce salts and water. c. water to produce acids and salts. b. salts to produce acids and water. d. neither acids, salts, nor water.
a. acids to produce salts and water
Which is an example of effusion? a. air slowly escaping from a pinhole in a tire b. the aroma of a cooling pie spreading across a room c. helium dispersing into a room after a balloon pops d. oxygen and gasoline fumes mixing in an automobile carburetor
a. air slowly escaping from a pinhole in a tire
As electrolyte concentration decreases, freezing-point depression a. approaches the Value calculated by assuming complete ionization. b. gets farther from the Value calculated by assuming complete ionization. c. remains exactly equal to the Value calculated by assuming complete ionization. d. approaches 0°C.
a. approaches the value calculated by assuming complete ionization
An acid-base titration determines the volumes of two solutions that a. are chemically equivalent. c. have equal mass. b. have equal molarity. d. have equal molality.
a. are chemically equivalent
In a solution, the slightly charged part of a water molecule a. attracts the ions in ionic compounds. b. forms ionic bonds with ions in ionic compounds. c. attracts nonpolar molecules. d. forms ionic bonds with other water molecules.
a. attracts the ions in ionic compounds
An insoluble gas that forms in a double-displacement reaction in aqueous solution a. bubbles out of solution. c. disassociates into ions. b. forms a precipitate. d. reacts with the water.
a. bubbles out of solution
To balance a chemical equation, it may be necessary to adjust the a. coefficients. c. formulas of the products. b. subscripts. d. number of products.
a. coefficients
A species that remains when an acid has lost a proton is a a. conjugate base. c. strong base. b. conjugate acid. d. strong acid.
a. conjugate base
In what kind of reaction does a single compound produce two or more simpler substances? a. decomposition reaction c. single-displacement reaction b. synthesis reaction d. ionic reaction
a. decomposition reaction
Nonvolatile solutes a. depress freezing point and elevate boiling point. b. elevate freezing point and depress boiling point. c. depress both freezing point and boiling point. d. elevate both freezing point and boiling point.
a. depress freezing point and elevate boiling point
The decomposition of a substance by an electric current is called a. electrolysis. c. ionization. b. conduction. d. transformation.
a. electrolysis
Which acid is produced in the stomach? a. hydrochloric acid c. nitric acid b. phosphoric acid d. sulfiiric acid
a. hydrochloric acid
If a soluble product forms, a reaction may run to completion a. if the product is only slightly ionized. b. if the product is highly soluble. c. if the product is not gaseous. d. under no circumstances.
a. if the product is only slightly ionized
Adding sodium acetate to an acetic acid, CH3COOH, solution a. increases pH and lowers [H+]. b. increases pH and raises [H+]. c. decreases pH and lowers [H+]. d. decreases pH and raises [H+].
a. increases pH and lowers [H+]
Arrhenius theorized that an acid is a chemical compound that a. increases the concentration of hydrogen ions when dissolved in water. b. increases the concentration of hydroxide ions when dissolved in water. c. decreases the concentration of hydrogen ions when dissolved in water. d. decreases the concentration of hydroxide ions when dissolved in water.
a. increases the concentration of hydrogen ions when dissolved in water
The law of combining Volumes applies only to gas volumes a. measured at constant temperature and pressure. b. that equal 1 L. c. that equal 22.4 L. d.' measured at STP.
a. measured at constant temperature and pressure
If an acid is added to a solution of a Weak base and its salt, a. more water forms and more weak base ionizes. b. the hydronium ion concentration decreases. c. more hydroxide ions form. d. more nonionized weak base forms.
a. more water forms and more weak base ionizes
Solubilities, expressed as grams/100. g of water, a. must be determined experimentally. b. can be easily predicted. c. vary directly with the rate at which solids dissolve. d. do not vary with temperature.
a. must be determined experimentally
Predict what happens When zinc is added to water. a. No reaction occurs. c. Zinc oxide forms. b. Steam is produced. d. Hydrogen is released.
a. no reaction occurs
Predict What happens when nickel is added to a solution of potassium chloride. a. No reaction occurs. c. Potassium nickel chloride forms. b. Nickel chloride forms. d. Hydrochloric acid forms.
a. no reaction occurs.
In a conjugate acid-base pair, the acid typically has a. one more proton than the base. b. one fewer proton than the base. c. two fewer protons than the base. d. the same number of protons as the base.
a. one more proton than the base
Which of the following is soluble in water? A a. potassium nitrate C. benzene b. silver d. carbon tetrachloride
a. potassium nitrate
An active metal and a halogen react to form a(n) a. salt. c. acid. b. hydroxide. d. oxide.
a. salt
Which of the following is an electrolyte? a. sodium chloride c. pure water b. sugar d. glass
a. sodium chloride
For the reaction represented by the equation 3F e + 4H3O --> Fe3O4 + 4H2, how many moles of iron(II) oxide are produced from 500. g of iron in an excess of H20? a. 1.04 mol c. 8.95 mo b. 2.98 mol d. 12.98 mol
b. 2.98 g
What is the net ionic equation for the precipitation reaction between silver nitrate solution and sodium sulfide solution'? a. 2Ag+(aq) + 2NO3'(aq) + 2Na+(aq) + S3'(aq) --> Ag2S(s) + 2Na+(aq) + 2NO3"(aq) b. 2Ag+(aq) + S3'(aq) --> Ag2S(s) c. Na+(aq) + NO3'(aq) --> NaNO3(s) d. 2Ag+(aq) + 2NO3*(aq) + 2Na+(aq) + S2'(aq) -->Ag2S(s) + 2NaNO3(s)
b. 2Ag+ + S2- --> Ag2S
For the reaction represented by the equation 2F e + O2 -->9 2FeO, how many grams of iron(iI) oxide are produced from 8.00 moi of iron in an excess of oxygen? a. 71.8g c. 712g b. 575g d. 1310g
b. 575 g
How many Mg2+ ions are found in 1.00 mol of MgO? a. 3.01 x 10^23 c. 12.04 x 10^23 b. 6.02 x 10^23 d. 6.02 X 10^25
b. 6.02 x 10^23
What is the solubility in mol/L of silver iodide, Agl? Its K_sp value is 8.3 x 10-17. a. 4.9 X 10-11 C. 8.6 x 10-7 b. 9.1 x 10-9 d. 5.5 x 10-7
b. 9.1 x 10-9
Which of the following is the right side of the equation for dissolving Al(NO3)3? a. Alt + (No3); c. Al3+ + No: b. Al3+(aq) + 3No;(aq) d. Ai3~(ag)'+ 3No;(ag)
b. Al3 + 3NO
Which reaction describes an anion hydrolysis reaction? a. B+(aq) + H2O(l) <--> HB(aq) + OH+(aq) b. B'(aq) + H2O(l) <--> HB(aq) + OH'(aq) c. HB(aq) + H20(l) <--> H30+(aq) + B-(aq) d. B*(aq) + H2O(l) <--> BOH(aq) + H"(aq)
b. B-(aq) + H2O(l) <--> HB (aq) + OH-(aq)
A compound contains 27.3 g of C and 72.7 g of 0. What is the empirical formula for this compound? a. CO c. C20 b. CO2 d .C204
b. C02
In the reaction represented by the equation CH3 COOH + H20 <--> H30+ + CH3COO-, the conjugate acid CH3COO' is a. C. H3O+. b. CH3COOH. cl. not shown.
b. CH3COOH
When energy as heat is applied to a liquid-vapor system at equilibrium, a new equilibrium state will have a. a higher percentage of liquid. c. equal amounts of liquid and vapor. b. a higher percentage of vapor. d. all liquid.
b. a higher percentage of vapor
Which of the following is a hydrated proton? a. a hydrogen ion c. a water molecule b. a hydronium ion d. a hydrogen chloride molecule
b. a hydronium ion
How would you classify HCl, in the equation below? HCl(ag) +H2O(Z) --> H30+ (aq) + C1-(aq) a. a weak acid c. a weak base b. a strong acid d. a strong base
b. a strong acid
When the chemical equilibrium expression is written, coefficients from the equation for the reaction a. appear as coefficients. c. appear as subscripts. b. appear as exponents. d. do not appear.
b. appear as exponents
An element in the activity series can replace any element a. in the periodic table. c. above it on the list. b. below it on the list. d. in its group.
b. below it on the list
The particles in both gases and liquids a. consist only of atoms. b. can change positions with other particles. c. can only vibrate in fixed positions. d. are packed closely together.
b. can change positions with other particles
Aqueous solutions of bases a. contain only two different elements. c. have Very high boiling points. b. carry electricity. d. cannot be prepared.
b. carry electricity
What unknown quantity can be calculated after performing a titration? a. volume c. mass b. concentration d. density
b. concentration
The reaction represented by the equation 2KClO3(s) --> 2KCl(s) + 3O2(g) is a(n) c. combustion reaction. d. ionic reaction. a. synthesis reaction. b. decomposition reaction.
b. decomposition reaciton
The equation AX --> A + X is the general equation for a a. synthesis reaction. c. combustion reaction. b. decomposition reaction. d. single-displacement reaction.
b. decomposition reaction
As temperature increases, solubility of gases in liquids a. increases. c. can increase or decrease. b. decreases. d. is not affected.
b. decreases
The separation of ions that occurs when an ionic compound dissolves is called a. ionization. c. precipitation. b. dissociation. d. oxidation.
b. dissociation
Which of the following releases energy? a. overcoming solute-so1ute attraction c. overcoming solvent-so1vent attraction b. forming solute-solvent attraction d. All of the above
b. forming solute-solvent attraction
What is the sum of the atomic masses of all the atoms in a formula for a compound? a. molecular mass c. atomic mass b. formula mass d. actual mass
b. formula mass
If the temperature of a liquid-vapor system at equilibrium increases, the new equilibrium condition will a. have a lower concentration of Vapor. b. have an increased vapor pressure. c. not have equal rates of condensation and evaporation. d. be larger in volume.
b. have an increased vapor pressure
If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal originally in the solution is a. a halogen. c. not on the activity series. b. higher on the activity series. d. unreactive.
b. higher on the activity series
Active metals react with certain acids, such as hydrochloric acid, to yield a metal compound and a. oxygen. c. chlorine. b. hydrogen. d. sodium.
b. hydrogen
Dyes with pH-sensitive colors are used as a. primary standards. c. titrants. b. indicators. d. None of the above
b. indicators
Substances whose water solutions conduct electricity easily a. require carbon to decompose in water. b. ionize in water. e. do not dissolve inwater. d. contain neutral solute~molecules.
b. ionize in water
A water solution whose pH is 10 a. is always neutral. c. is always acidic. b. is always basic. d. might be neutral, basic, or acidic.
b. is always basic
Why is freezing-point depression a colligative property? a. It is inversely proportional to the molal concentration of a solution. b. It is directly proportional to the molal concentration of a solution. c. It does not depend on a molal freezing-point constant for each solvent. d. It depends on the properties of an electrolyte in a solvent.
b. it is directly proportional to the molal concentration of a solution
The common-ion effect is a consequence of a. Boyle's law. c. AVogadro's principle. b. Le Chatelier's principle. d. chemical kinetics.
b. le chatelier's principle
Whose acid definition is the broadest'? a. Arrhenius c. Brensted-Lowry b. Lewis d. Faraday
b. lewis
The reaction represented by the equation Ag+(aq) + 2NH3(aq) --> [Ag®H3)2]+(aq) is a(n) a. traditional acid-base reaction. c. Br@nsted-Lowry acid-base reaction. b. Lewis acid-base reaction. d. None of the above
b. lewis acid-base reaction
According to Graham's law, two gases at the same temperature and pressure will have different rates of effusion because they have different a. Volumes. c. kinetic energies. b. molar masses. d. condensation points.
b. molar masses
The attraction of water molecules overcomes the strength of covalent bonds in a. all molecular substances. b. molecular substances that are electrolytes. c. molecular substances that are not electrolytes. cl. None of the above
b. molecular substances that are electrolytes
If a base is added to a solution of a Weak acid and its salt, a. more of the nonionized Weak acid forms. b. more of the nonionized acid ionizes. c. precipitation occurs. d. the hydronium ion concentration decreases.
b. more of the nonionized acid ionizes
During an acid-base titration, a very rapid change in pH a. occurs when the first addition of the known solution is made. b. occurs when the amounts of H3O+ ions and OH' ions are nearly equivalent. c. occurs at several points during the titration. d. does not occur during titration.
b. occurs when the amounts of H30+ ions and OH- ions are nearly equivalent
An acid-base titration is carried out by monitoring a. temperature. c. pressure. b. pH. d. density.
b. pH
The coefficients in a chemical equation represent the a. masses, in grams, of all reactants and products. b. relative numbers of moles of reactants and products. c. number of atoms in each compound in a reaction. d. number of valence electrons involved in the reaction.
b. relative numbers of moles of reactants and products
Acids taste a. sweet. c. bitter. b. sour. d. salty.
b. sour
The equilibrium vapor pressure of Water is a. constant at all temperatures. b. specific for any given temperature. c. unrelated to temperature. d. inversely proportional to the temperature.
b. specific for any given temperature
Pressure is the force per unit a. volume. c. length. b. surface area. d. depth. T
b. surface area
If the percentage yield is equal to 100%, then a. the actual yield is greater than the theoretical yield. b. the actual yield is equal to the theoretical yield. c. the actual yield is less than the theoretical yield. d. there was no limiting reactant.
b. the actual yield is equal to the theoretical yield
Which of the following would not be studied in the branch of chemistry called stoichiometry? a. the mole ratio of aluminum and chlorine in aluminum chloride b. the amount of energy required to break the ionic bonds in calcium fluoride c. the mass of carbon produced when a known mass of sucrose decomposes d. the number of moles of hydrogen that reacts completely with a known quantity of oxygen
b. the amount of energy required to break the ionic bond in calcium flouride
The kinetic-molecular theory explains the properties of solids, liquids, and gases in terms of the energy of the particles and a. gravitational forces. c. diffusion. b. the forces that act between the particles. d. the mass of the particles.
b. the forces that act between the particles
A chemical equation is balanced When the a. coefficients of the reactants equal the coefficients of the products. b. same number of each kind of atom appears in the reactants and in the products. c. products and reactants are the same chemicals. d. subscripts of the reactants equal the subscripts of the products.
b. the same number of each kind of atom appears in the reactants and in the products
According to Graham's law, the rates of effusion of two gases at the same temperature and pressure are inversely proportional to a. their volumes. c. their compressibilities. b. the square roots of their molar masses. d. their rates of vaporization.
b. the square roots of their molar masses
What happens to the volume of a gas during compression? a. The volume increases. b. The volume decreases. c. The volume remains constant. p d. It is impossible to tell because all gases are different.
b. the volume decreases
Which of the following is an example of a nonpolar solvent? a. water c. Both (a) and (b) b. toluene d. Neither (a) nor (b)
b. toluene
When Gay-Lussac's law of combining Volumes holds, which of the following can be expressed in ratios of small whole numbers? a. pressure before and pressure after reaction b. Volumes of gaseous reactants and products c. temperatures of gaseous reactants and products d. 1 molar masses of products and reactants
b. volumes of gaseous reactants and products
The conjugate of a strong base is a a. strong acid. c. strong base. b. Weak acid. d. weak base.
b. weak acid
Basic solutions are generally formed by hydrolysis of anions of salts of a. weak acids and Weak bases. c. strong acids and Weak bases. b. Weak acids and strong bases. d. strong acids and strong bases.
b. weak acids and strong bases
Many organic compounds, such as codeine, that contain nitrogen are a. strong bases. c. strong acids. b. weak bases. d. weak acids.
b. weak bases
When titrating a weak acid with a strong base, the equivalence point a. will be below a pH of7.0. c. will be at a pH of 7:0. g b. will be above a pH of 7.0. d. cannot be determined by pH.
b. will be above a pH of 7.0
Chlorine is produced by the reaction 2HC1(g) -->H2(g) + Cl2(g). How many grams of HCl (36.5 g/mol) must be used to produce 10.0 L of chlorine at STP? a. 15.8 g c. 32.6 g b. 30.2 g d. 36.5 g
c. 32.6 g
Diethyl ether's boiling point is about 35°C at 1 atm. At l.5 atm, What Will be ether's approximate boiling point'? a. -l 0°C c. 40°C b. 20°C d. 100°C
c. 40 C
Convert the pressure 0.75 atm to mm Hg. a. lol.325mmHg c. 57ommHg b. 430 mm Hg d. 760 mm Hg
c. 570 mmHg
For the reaction represented by the equation 2HNO3 + Mg(OH)2 -->Mg(NO3)2 + 2H2O, how many grams of magnesium nitrate are produced fiom 8.00 moi of nitric acid, HNO3, and an excess of Mg(OH)2? a. 148 g c. 593 g b. 445 g d. 818 g
c. 593 g
The molar mass of CCI4 is 153.81 g/mol. How many grams of CC14 are needed to have 5.000 mol? a. 5 g c. 769.0 g b. 30.76 g d. 796.05 g
c. 769.0g
What is the solubility in mol/L of copper(I) sulfide, Cu2S'? Its Ksp Value is 2.5 x 10-18. a. 4.1 x 10-14 c. 8.5 X 10-17 b. 6.2 x 10-15 d. 1.8 x 10-24
c. 8.5 x 10-17
What is the pH of a 10-5 M KOH solution? a. 3 c. 9 b. 5 d. 1 1
c. 9
For the reaction represented by the equation Cl2 + 2KBr -->; 2KCl + Br2, calculate the percentage yield if 200. g of chlorine react with excess potassium bromide to produce 410. g of bromine. a. 73 .4% c. 91 .0% b. 82.1% d. 98.9%
c. 91.0%
In which solution does adding hydrogen chloride promote precipitation? 8.. H2S04 C. AgNO3 b. KBr d. NaH
c. AgNO3
Which is a Lewis acid but not a Bronsted-Lowry acid? a. HCI c. BF3 b. NH3 d. None of the above
c. BF3
A compound's empirical formula is CH3. If the formula mass is 30 amu, What is the molecular formula? a. CH3 C. C2H5 b. CH4 d. C3H9
c. C2H5
The molecular formula for Vitamin C is C6H8O6. What is the empirical formula? a. CHO c. C3H4O3 b. CHZO d. C2H4O2
c. C3H4O3
Which compound dissociates to produce the ions Ca2+(aq) and NO3*(aq)? a. CaNO3(s) c. Ca(NO3)3(s) b). Ca2NO3 d. Ca2(NO3)3
c. Ca(NO3)3
Which of the following is a binary acid? a.. H2SO4 C. HBr b. CH3COOH . d. NaOH
c. HBr
Which of the following is chloric acid? a.. HClO c. HCIO3 b. HClO2 d. HC1O4
c. HClO3
In the reaction represented by the equation HCIO3 +NH3 <--> NH4+ + Cl03-; the conjugate acid of NH3 is a. HCIO3. c. NH4+ b. C10; d. not shown.
c. NH4+
A chemical formula Written over the arrow in a chemical equation signifies a. a by-product. c. a catalyst for the reaction. b. the formation of a gas. d. an impurity.
c. a catalyst for the reaction
An arnphoteric species is one that reacts as a(n) a. acid only. c. acid or base. b. base only. d. None of the above
c. acid or base
Two gases have the same temperature but different pressures. The kinetic-molecular theory does not predict that a. molecules in both gases have the same average kinetic energies. b. molecules in the low-pressure gas travel farther before they collide with other molecules. c. both gases have the same densities. d. all collisions of the molecules are elastic.
c. both gases have the same densities
Which of these best describes vaporization? a. the process by which a liquid changes to a gas b. the process by which a solid changes to a gas c. Both (a) and (b) d. Neither (a) nor (b)
c. both the process by which a liquid changes to a gas and the process by which a solids changes to a gas
Stirring increases the rate of dissolution because it a. raises the temperature. b. lowers the temperature. c. brings fresh solvent into contact with the solute. d. decreases the surface area of the solute.
c. brings fresh solvent into contact with the solute
If a solution is not agitated while it is being made, dissolved solute tends to a. mix uniformly. c. build up in the solvent near the solute. b. build up in the solvent far from the d. raise the temperature of the solvent. solute.
c. build up in the solvent near the solute
If a reaction system has come to equilibrium, it can be made to run to completion a. only if it is not reversible. c. by removing a product. b. only if the temperature is low enough. d. under no circumstances.
c. by removing a product
The formation of solid-liquid solutions a. always releases energy as heat. b. always absorbs energy as heat. c. can either absorb or release energy as heat. d. neither absorbs nor releases energy as heat.
c. can either absorb or release energy as heat
Above the critical temperature, a substance a. does not have a vapor pressure. c. cannot exist in the liquid state. b. sublimes. d. is explosive.
c. cannot exist in the liquid state
The pH of a basic solution is a. less than 0. c. greater than 7. b. less than 7. d. greater than 14.
c. greater than 7
Name the compound H20 using the Stock system. a. Water c. hydrogen(I) oxide b. hydrogen dioxide d. hydrogen(lI) oxide
c. hydrogen (I) oxide
Pure water partially breaks down into charged particles in a process called a. hydration. c. self-ionization. b. hydrolysis. d. dissociation.
c. hydrolysis
Actual freezing-point depressions of electrolyte solutions are slightly lower than the calculated values because of a. ion repulsion. b. more complete ionization than is expected. c. ion attraction. d. higher-than-expected effective concentration.
c. ion attraction
A solute crystal is dropped into a solution containing dissolved solute. It falls to the bottom of the beaker and does not dissolve after vigorous stirring. What does this indicate about the solution? a. It is probably unsaturated. c. It is probably saturated. b. It is probably supersaturated. d. It is not at equilibrium.
c. it is probably saturated
Enthalpy of solution is generally expressed in a. kilocalories. b. moles of solute per kilogram. c. kilojoules per mole of solute at a specified temperature. d. moles of solute in a specified amount of solvent per kiloj oule.
c. kilojoules per mole of solute at a specified temperature
Whenever ammonia donates an electron pair to form a covalent bond, it acts as a(n) a. Bronsted-Lowry base. c. Lewis base. b. Lewis acid. d. Arrhenius acid.
c. lewis base
A very low value of K indicates that a. equilibrium is reached slowly. ' c. reactants are favored. b. products are favored. d. equilibrium has been reached.
c. reactants are favored
A value of K near 1 indicates that at equilibrium probably a. only products are present. b. only reactants are present. c. significant quantities of both products and reactants are present. d. the reactions occur at a moderate rate.
c. significant quantities of both products and reactants are present
To What degree does water ionize? a. completely c. slightly b. to a large extent d. not at all
c. slightly
The empirical formula for a compound shows the symbols of the elements with subscripts indicating the a. actual numbers of atoms in a molecule. b. number of moles of the compound in lOO g. c. smallest whole-number ratio of the atoms. d. atomic masses of each element.
c. smallest whole-number ratio of the atoms
During the dissolving process, which particles interact? a. solute only c. solute and solvent b. solvent only d. None of the above
c. solute and solvent
Why does the air pressure inside the tires of a car increase when the car is driven? a. Some of the air has leaked out. A b. The air particles collide with the tire after the car is in motion. c. The air particles inside the tire increase their speed because their temperature rises. d. The atmosphere compresses the tire.
c. the air particles inside the tire increase their speed because their temperature rises
When pressure, volume, and temperature are known, the ideal gas law can be used to calculate a. the chemical formula. C. molar amount. b. the ideal gas constant. d. rate of efiision.
c. the molar amount
If the temperature and surface area of a liquid remain constant, a. the liquid is not in equilibrium with its vapor. b. no further evaporation occurs. c. the rate of evaporation remains constant. d. the rate of condensation is greater than the rate of evaporation.
c. the rate of evaporation remains constant
Molecules at the surface of a liquid can enter the vapor phase only if a. equilibrium has not been reached. b. the concentration of the vapor is zero. c. their energy is high enough to overcome the attractive forces in the liquid. d. condensation is not occurring.
c. their energy is high enough to overcome the attractive forces in the liquid
Why would a camper near the top of Mt. Everest find that Water boils at less than 100°C? a. There is greater atmospheric pressure than at sea level. b. The flames are hotter at that elevation. c. There is less atmospheric pressure than at sea level. d. The atmosphere has less moisture.
c. there is less atmospheric pressure than at sea level
Which of the following does not increase the rate of dissolving a solid in water'? a. raising the temperature of the water b. stirring the solution c. using larger pieces of solid d. crushing the solid
c. using larger pieces of solid
Which quantity is directly measured in a titration? a. mass _. c. volume b. concentration d. density
c. volume
Iron(1V) oxide, FeO2, is produced by the reaction Fe + O2 --> FeO2 (87.8 g/mol). How many grams of FeO2 can b< produced from 50.0 L of 02 at STP? a. 19.5 g c. 50 g b. 37.8 g d. 196. g
d. 196 g
Which coefficients correctly balance the formula NH4NO2 --> N2 +H2O? a. 1,2,2 c. 2,1,1 b. 1,1,2 d. 2,2,2
d. 2, 2, 2
If [H3O+] = 1.7 x 10-3 M, what is the pH of the solution'? a. 1 .8 1 c. 2 .42 b. 2.13 7 d. 2.77
d. 2.77
For the reaction represented by the equation C + 2H2 --> CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4? a. 2 mol c. 10 mol b. 4 mol d. 20 mol
d. 20 mol
A 1.00 L sample of a gas has a mass of 1.25 g at STP. What is the mass of 1.00 mol of this gas? a. 0.855 g c. 22.4 g b. 1.25 g d. 28.0 g
d. 28.0 g
Which equation is not balanced? a. 2H2+O2 --> 2H2O c. H2+H2+O2 --> H2O+H2O b. 4H2 +202 --> 4H2O d. 2H2 + O2 +H20
d. 2H2 + O2 + H2O
Ozone, O3, is produced by the reaction represented by the following equation: No2(g) +02(g) -->NO(g) +03(g) What mass of ozone will form from the reaction of 2.0 g of No2 in a car's exhaust and excess oxygen? a. 1.1gO3 c. 2.1gO3 b. 1.8g03 d. 4.2gO3
d. 4.2 g O3
A 1.00 L sample of a gas has a mass of 1.92 g at STP. What is the molar mass of the gas? a. 1.92 g/mol c. 22.4 g/mol b. 19.2 g/mol d. 43.0 g/mol
d. 43.0 g/mol
What is the percentage composition of CuCl2? a. 33% Cu, 66% Cl c. 65.50% Cu, 34.50% Cl b. 50% Cu, 50% Cl d. 47.27% Cu, 52.73% Cl
d. 47.27% Cu, 52.73% Cl
The molar mass of CS2 is 76.15 g/mol. How many grams of CS2 are present in 10.00 mol? a. 0.13 g c. 10.00 g b. 7.614 g d. 761.5 g
d. 761.5 g
he molar enthalpy of fusion for Water is 6.008 kl/mol. What quantity of energy is released when 253 g of liquid Water freezes? (Molar mass of Water is 18.02 g/mol.) a. 759 kJ c. 2.33 kl b. 0.429 kl d. 84.4 kl
d. 84.4 kJ
Which reaction tends to run to completion? a. N2(g) + O2(g) -->2NO(g) b. H3O+(aq) + OH'(aq) -->2H2O(l) c. Na+(aq) +Br'(aq) --> NaBr(s) d. H2(g) + CO(g) --> C(s) + H2O(g)
d. H2(g) + CO(g) --> C(s) + H2O(g)
Which reaction tends to run to completion? a. N2(g) + 3H2(g) --> 2NH3(g) b. Na+(aq) + Cl'(aq) -->NaCl(s) c. 2CO(g) + 02(g) --> 2CO2(g) d- H2CO3 -->H20(l) + CO2(g)
d. H2CO3 --> H20 + C02
Which of the following is arnphoteric? 8.. H2S04 C. H+ b. SO4 (2-) d. HSO4-
d. HSO4-
What is the formula for dinitrogen trioxide? a. Nl203 c. N206 b. No3 d. N203
d. N2O3
General Solubility Guidelines 1. Most sodium, potassium, and ammonium compounds are soluble in water. 2. Most nitrates, acetates, and chlorates are soluble. 3. Most chlorides are soluble, except those of silver, mercury(l), and lead. Lead(lI) chloride is soluble in hot Water. 4. Most sulfates are soluble, except those of barium, strontium, and lead. 5. Most carbonates, phosphates, and silicates are insoluble, except those of sodium, potassium, and ammonium. 6. Most sulfides are insoluble, except those of calcium, strontium, sodium, potassium, and ammonium. 148. Which of the following pairs of solutions produces a precipitate when combined? a. KOH and NH4Cl ' c. Na2SO4 and KCl b. Fe(NO)3 and KCl d. NH4Cl and AgNO3
d. NH4Cl and AgNO3
A foam is a colloidal dispersion of a. two liquids. c. a solid and a liquid. b. two solids. d. a gas and a liquid.
d. a gas and a liquid
A salt is not a. - an ionic compound composed of a metal cation from a base. b. an ionic compound composed of an anion from an acid. c. a product of neutralization. d. a proton donor.
d. a proton donor
A substance that ionizes nearly completely in aqueous solutions and produces H3O+ is a a. weak base. c. weak acid. b. strong base. d. strong acid.
d. a strong acid
What is the measured amount of a product obtained from a chemical reaction? a. mole ratio c. theoretical yield b. percentage yield d. actual yield
d. actual yield
The formula for carbon dioxide, CO2, can represent a. one molecule of carbon dioxide. b. 1 mol of carbon dioxide molecules. c. the combination of 1 atom of carbon and 2 atoms of oxygen. d. all of the above.
d. all of the above
The name of a binary acid a. has no prefix. c. ends with the suffix -ouS. b. begins with the prefix bz'-. d. begins with the prefix hydro-.
d. begins with the prefix hydro
A determination of the masses and number of moles of sulfur and oxygen in the compound sulfur dioxide Would_ be studied in a. reaction stoichiometry. c. chemical equilibrium. b. chemical kinetics. d. composition stoichiometry.
d. composition stoichiometry
The standard molar volume of a gas is all of the following except a. the volume occupied by 1 mol of a gas at STP. b. equal for all gases under the same conditions. c. 22.4 L at STP. d. dependent upon the size of the molecules.
d. dependent upon the size of the molecules
If more CO(g) is added to the system 2CO(g) + O2(g) <-->CO2 (g) at constant temperature, K a. increases. c. increases or decreases. b. decreases. d. does not change.
d. does not change
The equation AX + BY --> AY + BX is the general equation for a a. synthesis reaction. c. single-displacement reaction. b. decomposition reaction. d. double-displacement reaction.
d. double-displacement reaciton
What is the process by which molecules of a gas randomly encounter and pass through a small opening? container? a. diffusion c. distillation b. osmosis d. effusion
d. effusion
Which reactant controls the amount of product formed in a chemical reaction? a. excess reactant c. composition reactant b. mole ratio d. limiting reactant
d. limiting reactant
If a base is added to a solution of a Weak base and its salt, a. the hydronium ion concentration increases. b. more of the Weak base ionizes. c. more hydroxide ions form. d. more Water and nonionized base forms.
d. more water and nonionized base forms
The value of K for a system a. can be calculated from the molar masses of products and reactants. b. can be calculated from the enthalpies of the forward and reverse reactions. c. can be calculated from the chemical properties of products and reactants. d. must be measured by experiment.
d. must be measured by experiment
Besides the K_sp, Value of a compound, what other information is needed to calculate solubility in moles per liter? a. molar mass c. solubility in grams b. density of the solid d. no other information
d. no other information
In water solutions of HCl, the free H+ ion is a. present in very large quantities. c. present in small quantities. b. present in moderate quantities. d. not present.
d. not present
Which of the following will dissolve most rapidly? a. sugar cubes in cold water c. powdered sugar in cold Water b. sugar cubes in hot water d. powdered sugar in hot water
d. powdered sugar in hot water
If a substance has a greater tendency to give up protons, its conjugate has a a. great tendency to give up protons. c. slight tendency to give up protons. b. great tendency to attract protons. d. slight tendency to attract protons.
d. slight tendency to attract protons
The intermolecular forces between particles are a. weaker in solids than in liquids. b. stronger in gases than in solids. c. equal in strength in gases and in liquids. d. stronger in liquids than in gases.
d. stronger in liquids than in gases
Which acid is manufactured in largest quantity? a. hydrochloric acid c. nitric acid b. phosphoric acid d. sulfuric acid
d. sulfuric acid
Which acid is used in batteries? a. hydrochloric acid c. nitric acid b. phosphoric acid d. sulfuric acid
d. sulfuric acid
The ideal gas law is equivalent to Boyle's law when a. the number of moles and the pressure are constant. b. R equals zero. c. the pressure is 1 atm. d. the number of moles and the temperature are constant.
d. the number of moles and the temperature are constant
To determine the limiting reactant in a chemical reaction involving known masses of A and B, one could first calculate a. the mass of 100 mol of A and B. b. the masses of all products. c. the bond energies of A and B. 'd. the number of moles of B and the number of moles of A available.
d. the number of moles of B and the number of moles of A available
In a solution at equilibrium, a. no dissolution occurs. b. the rate of dissolution is less than the rate of crystallization. c. the rate of dissolution is greater than the rate of crystallization. d. the rate of dissolution and the rate of crystallization are equal.
d. the rate of dissolution and the rate of crystallization are equal
Which of the following is not correct about crystalline solids? a. They can maintain a definite shape without a container. b. They can exist as single crystals. c. Their particles are held in relatively fixed positions. d. They are geometrically irregular.
d. they are geometrically irregular
Which of the following statements about ionic crystals is not correct? a. Their structure consists of positive and negative ions arranged in a regular pattern. b. The strong binding forces between the positive and negative ions in their structure give them certain properties. c. Their ions can be monatomic or polyatomic. d. They consist of molecules held together by intermolecular forces.
d. they consist of molecules held together by intermolecular forces
When a binary compound decomposes, what is produced? a. an oxide c. a tertiary compound b. an acid d. two elements
d. two elements
In the equation HI + H20 --> H3O+ + I', HI is a strong acid and I' is a a. strong acid. c. weak acid. b. strong base. d. weak base.
d. weak base
