Chem Final

Calculate the freezing point of a solution made from 22.0 g of octane (C8H18) dissolved in 148.0 g of benzene. Benzene freezes at 5.50°C and its Kf value is 5.12°C/m. A) -1.16°C B) 0.98°C C) 5.49°C D) 6.66°C E) 12.2°C

A) -1.16°C

Calculate the value of E°cell for the following reaction: 2Au(s) + 3Ca2+(aq) → 2Au3+(aq) + 3Ca(s) A) -4.37 V B) -1.37 V C) -11.6 V D) 1.37 V E) 4.37 V

A) -4.37 V

The number of lone electron pairs in the NH4+ ion is ___ A) 0 B) 1 C) 2 D) 3 E) 4

A) 0

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + SO32- → Mn2+ + SO42- (acidic solution) A) 3 B) 4 C) 5 D) 8 E) None of these.

A) 3

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] A) 3.97 B) 4.83 C) 4.19 D) 3.40 E) 4.41

A) 3.97

Calculate the frequency of visible light having a wavelength of 686 nm. A) 4.37 × 1014 /s B) 4.37 × 105 /s C) 6.17 × 1014 /s D) 2.29 × 10-15 /s E) 2.29 × 10-6 /s

A) 4.37 × 10^14 /s

If we take away two electrons from the outer shell of calcium, it would have the same electron configuration as what element? A) Argon B) Titanium C) Stronium D) Magnesium E) None of the above

A) Argon

25.0 mL of a 0.100 M solution of NH3 is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is: A) Basic and before the equivalence point B) Basic and after the equivalence point C) Acidic and before the equivalence point D) Acidic and after the equivalence point E) Neutral and at the equivalence point

A) Basic and before the equivalence point

35.0 mL of a 0.250 M solution of KOH is titrated with 0.150 M HCl. After 35.0 mL of the HCl has been added, the resultant solution is: A) Basic and before the equivalence point B) Basic and after the equivalence point C) Acidic and before the equivalence point D) Acidic and after the equivalence point E) Neutral and at the equivalence point

A) Basic and before the equivalence point

14. Which of the following electronic transitions is consistent with an increase in energy? A) From a 4s subshell to a 3d subshell B) From a 5p subshell to a 4d subshell C) From a 4d subshell to a 5s subshell D) From a 4f subshell to a 6s subshell E) From a 5d subshell to a 6s subshell

A) From a 4s subshell to a 3d subshell

Which of the elements listed below has the highest first ionization energy? A) He B) Ne C) Ar D) Kr E) Xe

A) He

Arrange the following ions in order of increasing ionic radius: K+, P3- , S2-, Cl- increasing radius → A) K + < Cl - < S 2 - < P 3 - B) K + < P 3 - < S 2 - < Cl - C) P 3 - < S 2 - < Cl - < K + D) Cl - < S 2 - < P 3 - < K + E) Cl - < S 2 - < K + < P 3 -

A) K + < Cl - < S 2 - < P 3 -

Which one of these salts will form a neutral solution on dissolving in water? A) NaCl B) KNO2 C) NaCN D) NH4NO3 E) FeCl3

A) NaCl

Which of the following is true concerning a galvanic cell? A) Oxidation occurs at the anode and is where anions move towards B) Oxidation occurs at the cathode and is where anions move towards C) Oxidation occurs at the anode and is where cations move towards D) Oxidation occurs at the cathode and is where cations move towards E) Reduction occurs at the anode and is where anions move towards

A) Oxidation occurs at the anode and is where anions move towards

Which of the following phase changes is endothermic? A) Sublimation B) Condensation C) Freezing D) Deposition

A) Sublimation

Which one of the following statements is true for a 0.1 M solution of a weak acid HA? A) The concentration of H+ is slightly greater than the concentration of A-. B) The pH equals 1.0.C) The concentration of H+ is exactly equal to the concentration of A-.D) The pH is less than 1.0.E) The concentration of H+ is slightly less than the concentration of A-.

A) The concentration of H+ is slightly greater than the concentration of A-.

Which of the following is the electron configuration of the iron(III) ion? A)[Ar]3d5B)[Ar]4s13d5C)[Ar]4s23d3D)[Ar]3d6E)[Ar]4s23d9

A) [Ar]3d5

The electron configuration of a ground-state Co atom is A) [Ar]4s23d7. B) 1s22s22p63s23d9. C) [Ne]3s23d7. D) [Ar]4s13d5. E) [Ar]4s24d7.

A) [Ar]4s23d7.

Which of the following characteristics indicates the presence of weak intermolecular forces in a liquid? A) a low heat of vaporization B) a high critical temperature C) a low vapor pressure D) a high boiling point E) None of the above.

A) a low heat of vaporization

The hybridization of the central nitrogen atom in the molecule N2O is A) sp. B) sp2. C) sp3. D) sp3d. E) sp3d2.

A) sp.

List the following sets of quantum numbers in order of increasing energy: I. n = 4, l = 0, m l = 0, m s = -1/2 II. n = 4, l = 2, m l = -1, m s = -1/2 III. n = 5, l = 0, m l = 0, m s = +1/2 A)I < II < IIIB)II < III < IC)III < II < ID)I < III < IIE)III < I < II

A)I < II < III or D)I < III < II

Give the number of lone pairs around the central atom and the molecular geometry of CBr4. A)0 lone pairs, square planarB)0 lone pairs, tetahedralC)1 lone pair, square pyramidalD)1 lone pair, trigonal bipyramidalE)2 lone pairs, square planar

B) 0 lone pairs, tetahedral

Calculate the pH of the solution resulting from the addition of 85.0 mL of 0.35 M HCl to 30.0 mL of 0.40 M aniline (C6H5NH2). Kb (C6H5NH2) = 3.8 x 10-10 A) 1.75 B) 0.81 C) 4.64 D) 4.19 E) 9.09

B) 0.81

. What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 4 l = 3 ml = -2 ms = +1/2 A) 0 B) 1 C) 2 D) 6 E) 10

B) 1

In an electron microscope, electrons are accelerated to great velocities. Calculate the wavelength of an electron traveling with a velocity of 7.0 × 10 3 kilometers per second. The mass of an electron is 9.1 × 10-28 g. A) 1.0 × 10-13 m B) 1.0 × 10-10 m C) 1.0 × 10-7 m D) 1.0 m

B) 1.0 × 10^-10 m

What is the maximum number of electrons in an atom that can have the following quantum numbers? n = 3 l = 2 A)18B)10C)5D)2E)1

B) 10

A sp2 hybridized central atom has what angles between its hybrid orbitals? A)145°B)120°C)109.5°D)90°E)< 90°

B) 120°

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8 × 10-5] A) 4.65 B) 4.71 C) 4.56 D) 4.84 E) 5.07

B) 4.71

What is the wavelength of radiation that has a frequency of 5.39 × 1014 s-1? A) 1.80 × 10-3 nm B) 556 nm C) 618 nm D) 6180 nm E) 1.61 × 1023 nm

B) 556 nm

Calculate the mass percent of HOCH2CH2OH in a solution made by dissolving 3.2 g of HOCH2CH2OH in 43.5g of water. A) 2.9% B) 6.9% C) 7.4% D) 22% E) 29%

B) 6.9%

Each of the three resonance structures of NO3- has how many lone pairs of electrons? A)7B)8C)9D)10E)13

B) 8

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10-10) solution. A) 5.15 B) 8.71 C) 5.85 D) 9.91 E) 13.0

B) 8.71

What is the wavelength of radiation that has a frequency of 3.4 x 1011 s-1? A) 8.8 x 10-4 nm B) 8.8 x 105 nm C) 8.8 x 10-13 nm D) 1.0 x 1011 nm E) 1.0 x 10-9 nm

B) 8.8 x 10^5 nm

The boiling points of chloromethane (CH3Cl) and dichlormethane (CH2Cl 2) are - 24 °C and 40°C respectively. The boiling point of trichloromethane (CHCl3) is predicted to be: A) < - 24 °C B) > 40.°C C) > - 24 °C and < 40.°C D) - 24 °C E) 40.°C

B) > 40.°C

. If one electron is added to the outer shell of chlorine, it would have the same electron configuration as what element? A) Sulfur B) Argon C) Bromine D) Potassium E) None of the above

B) Argon

Which one of the following is most likely to be an ionic compound? A) NCl3 B) BaCl2 C) CO D) SO2 E) SF4

B) BaCl2

In which of the following solvents would you expect KBr to be most soluble? A) C6H14 (hexane) B) CH3CH2OH (ethanol) C) C6H6 (benzene) D) CCl4 (carbon tetrachloride) E) C6H12 (cyclohexane)

B) CH3CH2OH (ethanol)

Which of the following electronic transitions is consistent with a decrease in energy? A)From a 5s subshell to a 4d subshellB)From a 4f subshell to a 5p subshellC)From a 6s subshell to a 5d subshellD)From a 5s subshell to a 5p subshellE)From a 4f subshell to a 6p subshell

B) From a 4f subshell to a 5p subshell

Which of the elements listed below has the smallest first ionization energy? A)CB)GeC)PD)OE)Se

B) Ge

What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution? A) H+ + H2O → H3O+ B) H+ + OCl- → HOCl C) HOCl → H+ + OCl- D) H+ + HOCl → H2OCl+ E) HCl + HOCl → H2O + Cl2

B) H+ + OCl- → HOCl

Which one of these net ionic equations represents the reaction of a strong acid with a weak base? A) H+(aq) + OH-(aq) → H2O(aq) B) H+(aq) + CH3NH2(aq) → CH3NH3+(aq)C) OH-(aq) + HCN(aq) → H2O(aq) + CN-(aq)D) HCN(aq) + CH3NH2(aq) → CH3NH3+ (aq)+ CN-(aq)

B) H+(aq) + CH3NH2(aq) → CH3NH3+(aq)

According to the VSEPR theory, which one of the following species is linear? A) H2S B) HCN C) BF3 D) H2CO E) SO2

B) HCN

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2-9.3? A) CH3COONa / CH3COOH (Ka = 1.8 × 10-5) B) NH3 / NH4Cl (Ka = 5.6 × 10-10)C) NaOCl / HOCl (Ka = 3.2 × 10-8)D) NaNO2 / HNO2 (Ka = 4.5 × 10-4)E) NaCl / HCl

B) NH3 / NH4Cl (Ka = 5.6 × 10-10)

Which one of the following equations represents the ionization of a weak base in water? A) NH3(aq) + H2O(l)NH2+(aq) + H3O+(aq) B) NH3(aq) + H2O(l)NH4+(aq) + OH-(aq)C) NH3(aq) + H2O(l)NH4 - (aq) + OH +(aq)D) NH3(aq) + OH-(aq)NH2- (aq) + H2O(l)E) NH3(aq) + H3O+(aq)NH4+(aq) + H2O(l)

B) NH3(aq) + H2O(l)NH4+(aq) + OH-(aq)

The Lewis structure reveals a double bond in which of the following molecules? A) Br2 B) O2 C) N2 D) H2 E) CH4

B) O2

Which of the atoms listed below has the smallest radius? A) Al B) P C) As D) Te E) Na

B) P

Arrange the elements F, P, and Cl in order of increasing electronegativity. A) F < P < Cl B) P < Cl < F C) Cl < P < F D) P < F < Cl E) Cl < F < P

B) P < Cl < F

Which element has the following ground-state electron configuration? [Kr]5s24d105p3 A) Sn B) Sb C) Pb D) Bi E) Te

B) Sb

Complete the following statement: A catalyst A) increases the activation energy. B) alters the reaction mechanism. C) increases the average kinetic energy of the reactants. D) increases the concentration of reactants. E) increases the collision frequency of reactant molecules.

B) alters the reaction mechanism.

Which element has the following ground-state electron configuration? [Ar]4s23d104p5 A)arsenicB)bromineC)iodineD)seleniumE)tellurium___C___20. The electron

B) bromine

A possible set of quantum numbers to describe an electron in a 4s subshell is A) n = 4, l = 0, m l = 1 , m s = +1/2 B) n = 4, l = 0, m l = 0, m s = - 1/2 C) n = 4, l = 1, m l = 1, m s = +1/2 D) n = 3, l = 1, m l = 1, m s = - 1/2 E) n = 3, l = 0, m l = 0, m s = +1/2

B) n = 4, l = 0, m l = 0, m s = - 1/2

What is the hybridization on the central atom in NO3-? A) sp B) sp2 C) sp3 D) sp3d E) sp3d2

B) sp2

A liquid boils when its A) vapor pressure is exactly 1 atmosphere. B) vapor pressure is equal to, or greater than, the external pressure pushing on it. C) temperature is equal to 273 K (standard temperature). D) temperature is greater than room temperature.

B) vapor pressure is equal to, or greater than, the external pressure pushing on it.

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution? A) 0.03097 M B) 0.4133 M C) 0.4646 M D) 1.590 M E) 3.097 M

C) 0.4646 M

Give the number of lone pairs around the central atom and the geometry of the ion ClO3 -. A)0 lone pairs, trigonalB)1 lone pair, bentC)1 lone pair, trigonal pyramidalD)2 lone pairs, T-shapedE)2 lone pairs, trigonal

C) 1 lone pair, trigonal pyramidal

What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m? A) 2.70 × 10-43 J B) 5.43 × 10-33 J C) 1.63 × 10-24 J D) 4.07 × 10-10 J E) 2.46 × 109 J

C) 1.63 × 10^-24 J

The vapor pressure of ethanol is 400 mmHg at 63.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is the vapor pressure of ethanol, in mmHg, at 34.9°C? A) 0.0099 mmHg B) 4.61 mmHg C) 100 mmHg D) 200 mmHg E) 1,510 mmHg

C) 100 mmHg

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water. The density of water is 0.997 g/mL. A) 1.51 % B) 7.57 % C) 13.3 % D) 15.2 % E) None of these

C) 13.3 %

The heat capacity of liquid water is 4.18 J/g·°C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must be provided to convert 1.00 g of liquid water at 67°C into 1.00 g of steam at 100°C? A) 40.8 J B) 2.2 kJ C) 2,400 J D) 22.7 kJ E) 40.8 kJ

C) 2,400 J

The activation energy for the reaction CH3CO →CH3 + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170°C than at 150°C? A) 0.40 B) 1.1 C) 2.5 D) 4.0 E) 5.0

C) 2.5

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. A) 1.82 × 10-19 /s B) 9.13 × 1013 /s C) 2.74 × 1014/s D) 3.65 × 1014 /s E) 1.64 × 1015 /s

C) 2.74 × 10^14/s

The number of resonance structures for the nitrate ion that satisfy the octet rule is A)1B)2C)3D)4E)None of these

C) 3

A ground-state atom of vanadium has ___ unpaired electrons and is _____. A) 0, diamagnetic B) 2, diamagnetic C) 3, paramagnetic D) 5, paramagnetic E) 4, diamagnetic

C) 3, paramagnetic

Which of the following wavelengths of electromagnetic radiation has the highest energy? A) 450. nm B) 225 nm C) 3.50 x 10-9 m D) 8.40 x 10-7 m E) 2.50 x 10-5 m

C) 3.50 x 10^-9 m

How many 3d electrons does the manganese(II) ion, Mn2+, have? A)3B)4C)5D)6E)7

C) 5

How many orbitals are allowed in a subshell if l = 2? A) 1 B) 3 C) 5 D) 7 E) 9

C) 5

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8 × 10-5). A) 2.87 B) 4.98 C) 5.12 D) 7.00 E) 11.12

C) 5.12

The cobalt(III) ion, Co3+, has how many 3d electrons? A) 0 B) 7 C) 6 D) 5 E) 4

C) 6

Calculate the frequency of visible light having a wavelength of 486 nm. A) 2.06 × 1014 /s B) 2.06 × 106 /s C) 6.17 × 1014 /s D) 1.20 × 10-15 /s E) 4.86 × 10-7 /s

C) 6.17 × 10^14 /s

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [Ka(HOCl) = 3.2 × 10-8] A) 0.39 B) 3.94 C) 6.58 D) 7.49 E) 8.40

C) 6.58

Which of the following molecules has polar bonds but is a nonpolar molecule? A) PCl3 B) NCl3 C) BF3 D) HF E) OCl2

C) BF3

Which of the following yields an acidic solution when dissolved in water? I. NO2 II. NH4Cl III. NaCl IV. HNO2 A) I and IV B) II and III C) I, II, and IV D) I and III E) I, II, III, and IV

C) I, II, and IV

List the following sets of quantum numbers in order of increasing energy: I. n = 4, l = 1, ml = 1, ms = +1/2 II. n = 3, l = 2, ml = -1, ms = +1/2 III. n = 4, l = 0, ml = 0, ms = +1/2 A) I < II < III B) II < III < I C) III < II < I D) I < III < II E) III < I < II

C) III < II < I

Which of the following constants is/are needed to calculate the amount of energy required to heat 12.0g of H2O(l) at 30.0°C to H2O(l) at 85.0°C? I. ΔHfus (H2O) II. ΔHvap (H2O) III. specific heat of H2O(s) IV. specific heat of H2O(l) V. specific heat of H2O(g) A) I and IV B) II and IV C) IV only D) I, II, and IV E) IV and V

C) IV only

What type of chemical bond holds the atoms together within a water molecule? A)Ionic bondB)Nonpolar covalent bondC)Polar covalent bondD)Coordinate covalent bond

C) Polar covalent bond

Which one of the following ions has the largest radius? A) Cl- B) K+ C) S2- D) Na+ E) O2-

C) S^2-

The electron configuration of a ground-state vanadium atom is A) [Ar]4s24d3. B) [Ar]4s24p3. C) [Ar]4s23d3. D) [Ar]3d5.

C) [Ar]4s23d3.

Which of the following is the electron configuration for the bromide ion? A) [Ar] B) [Ar]4s23d104p7 C) [Kr] D) [Kr]5s24d105p7 E) [Xe]

C) [Kr]

Which of the following properties indicates the presence of strong intermolecular forces in a liquid? A) a low heat of vaporization B) a low critical temperature C) a low vapor pressure D) a low boiling point E) None of the above.

C) a low vapor pressure

Predict the molecular geometry and polarity of the SO2 molecule. A)linear, polarB)linear, nonpolarC)bent, polarD)bent, nonpolarE)None of the above

C) bent, polar

In general, to calculate the activation energy for an elementary step given the rate constants at two different temperatures, which equation should be used? A) ln([A]t/[A]o) = - kt B) t1/2 = ln2/k C) ln(k1/k2) = Ea/R((T1 - T2)/T1T2) D) 1/[A]t = kt + 1/[A]o E) Rate = k[A]

C) ln(k1/k2) = Ea/R((T1 - T2)/T1T2)

A possible set of quantum numbers to describe an electron in a 3d subshell is A)n = 3,l = 0, ml = 0 , ms = +1/2B)n = 3,l = 1, ml = 0, ms = - 1/2C)n = 3,l = 2, ml = 1, ms = +1/2D)n = 3,l = 3, ml = 1, ms = - 1/2E)n = 2,l = 0, ml = 0, ms = +1/2

C) n = 3, l = 2, m l = 1, m s = +1/2

According to the VSEPR theory, the geometry of the SO3 molecule is A) pyramidal. B) tetrahedral. C) trigonal planar. D) distorted tetrahedron (seesaw). E) square planar.

C) trigonal planar.

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. A)2.07 × 10-29 JB)2.25 × 10-18 JC)2.04 × 10-18 JD)3.27 × 10-17 JE)2.19 × 105 J

C)2.04 × 10^-18

For the reaction Ni2+(aq) + 2Fe2+(aq) → Ni(s) + 2Fe3+(aq), the standard cell potential E°cell is A) +2.81 V. B) +1.02 V. C) +0.52 V. D) -1.02 V. E) -2.81 V.

D) -1.02 V.

Estimate the enthalpy change for the reaction 2CO + O2→ 2CO2 given the following bond energies. BE(C≡O) = 1074 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol A) +2380 kJ/mol B) +1949 kJ/mol C) +744 kJ/mol D) -561 kJ/mol E) -744 kJ/mol

D) -561 kJ/mol

The Arrhenius equation is k = Ae -Ea/RT. The slope of a plot of ln k vs. 1/T is equal to A)-kB)kC)EaD)-Ea /RE)A

D) -Ea /R

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed? A) 0.10M H2CO3 and 0.050M HCl B) 0.10M H2CO3 and 0.10M KOH C) 0.10M H2CO3 and 0.10M HCl D) 0.10M H2CO3 and 0.050M KOH E) 0.10M K2CO3 and 0.050M KOH

D) 0.10M H2CO3 and 0.050M KOH

Which solution will have the lowest pH? A) 0.25 M HClO B) 0.25 M HClO2 C) 0.25 M HClO3 D) 0.25 M HClO4 E) 0.25 M NaClO4

D) 0.25 M HClO4

In how many grams of water should 25.31 g of potassium nitrate (KNO3) be dissolved to prepare a 0.1982m solution? A) 250.0 g B) 792.0 g C) 1000. g D) 1,263 g E) 7,917 g

D) 1,263 g

Calculate the molality of a 20.0% by mass ammonium sulfate (NH4)2SO4 solution. The density of the solution is 1.117 g/mL. A) 0.150 m B) 1.51 m C) 1.70 m D) 1.89 m E) 2.10 m

D) 1.89 m

The bond angles in CO32- are expected to be A)a little less than 109.5°.B)109.5°.C)a little less than 120°.D)120°.E)a little more than 120°.

D) 120°.

The total number of valence electrons in the molecule CO2 is A) 4. B) 10. C) 14. D) 16. E) 20.

D) 16

Complete and balance the following redox equation using the set of smallest whole-number coefficients. What is the sum of the coefficients? HI + HNO3 → I2 + NO (acidic solution) A) 5 B) 7 C) 14 D) 17 E) None of these.

D) 17

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. A)9.18 × 10-20 nmB)4.45 × 10-20 nmC)2.16 × 10-6 nmD)2.16 × 103 nmE)1.38 × 1014 nm

D) 2.16 × 10^3 nm

How many grams of sucrose (C12H22O11, 342.3 g/mol) would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L·atm/K·mol) A) 0.57 g B) 6.8 g C) 2.0 × 10 2 g D) 4.9 × 10 2 g E) 5.8 × 10 3 g

D) 4.9 × 10^2 g

A ground-state atom of manganese has ___ unpaired electrons and is _____. A) 0, diamagnetic B) 2, diamagnetic C) 3, paramagnetic D) 5, paramagnetic E) 7, paramagnetic

D) 5, paramagnetic

What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: Cr2O72-(aq) + 6Fe2+(aq) + 14H+(aq) → 2Cr3+(aq) + 6Fe3+(aq) + 7H2O(l) A) 1 B) 2 C) 3 D) 6 E) 12

D) 6

The vapor pressure of water at 45.0 °C is 71.93 mmHg. What is the vapor pressure of water over a solution prepared from 75.0 g of citric acid (C6H8O7) in 0.420 kg of water at this temperature? A) 1.22 mmHg B) 42.3 mmHg C) 43.0 mmHg D) 70.7 mmHg E) 73.2 mmHg

D) 70.7 mmHg

Which of the following compounds should be soluble in CCl4? A) NaCl B) H2O C) NaOH D) C8H18 E) None of these

D) C8H18

Which one of the following molecules has tetrahedral geometry? A)XeF4B)BF3C)AsF5D)CF4E)NH3

D) CF4

. Arrange the acids HBr, H2Se, and H3As in order of increasing acid strength. A) HBr < H2Se < H3As B) HBr < H3As < H2Se C) H2Se < H3As < HBr D) H3As < H2Se < HBr E) H3As < HBr < H2Se

D) H3As < H2Se < HBr

Which one of these equations represents the reaction of a weak acid with a weak base?A) H+(aq) + OH-(aq) → H2O(aq) B) H+(aq) + CH3NH2(aq) → CH3NH3+(aq)C) OH-(aq) + HCN(aq) → H2O(aq) + CN-(aq)D) HCN(aq) + CH3NH2(aq) → CH3NH3+(aq) + CN-(aq)

D) HCN(aq) + CH3NH2(aq) → CH3NH3+(aq) + CN-(aq)

Arrange the following substances in order of increasing boiling point: CH3OH, He, CH3Cl, and N2 A) CH3OH < He < CH3Cl < N2 B) He < N2 < CH3OH < CH3Cl C) N2 < He < CH3OH < CH3Cl D) He < N2 < CH3Cl < CH3OH E) CH3Cl < He < N2 < CH3OH

D) He < N2 < CH3Cl < CH3OH

Which of the following is not true with regard to water? A) Water has a high heat capacity. B) Water has an unusually high boiling point. C) Water can form hydrogen bonds. D) Ice is more dense than liquid water. E) Water is a polar molecule.

D) Ice is more dense than liquid water.

Which of the following elements has the smallest first ionization energy? A)ClB)NaC)BeD)KE)As

D) K

29. Which of the elements listed below has the highest first ionization energy? A) C B) Ge C) P D) O E) Se

D) O

Which of the atoms listed below has the largest radius? A)ClB)IC)PD)SbE)Se

D) Sb

Which of the following would be expected to have the highest vapor pressure at room temperature? A) ethanol, bp = 78°C B) methanol, bp = 65°C C) water, bp = 100°C D) acetone, bp = 56°C

D) acetone, bp = 56°C

A saturated solution A) contains more solute than solvent. B) contains more solvent than solute. C) contains equal moles of solute and solvent. D) contains the maximum amount of solute that will dissolve in that solvent at that temperature. E) contains a solvent with only sigma bonds and no pi bonds (i.e. only single bonds, with no double or triple bonds).

D) contains the maximum amount of solute that will dissolve in that solvent at that temperature.

Which one of the following sets of quantum numbers represents an electron with the highest energy? A) n = 2, l = 1, m l = 0, m s = +1/2 B) n = 3, l = 0, m l = 0, m s = -1/2 C) n = 2, l = 0, m l = 0, m s = +1/2 D) n = 3, l = 2, m l = 1, m s = -1/2 E) n = 3, l = 1, m l = 1, m s = +1/2

D) n = 3, l = 2, m l = 1, m s = -1/2

How many orbitals are allowed in a subshell if l = 3? A)1B)3C)5D)7E)9

D)7

The formal charge on the bromine atom in BrO3- drawn with three single bonds is A) -2. B) -1. C) 0. D) +1. E) +2.

E) +2.

What is the freezing point of a solution that contains 10.0 g of glucose (C6H12O6) in 100.g of H2O? Kf for water is 1.86°C/m. A) +0.10°C B) +0.186°C C) -0.10°C D) -0.186°C E) -1.03°C

E) -1.03°C

Which of the following frequencies of light has the highest energy? A)2.5 x 1010 s-1B)7.0 x 1013 s-1C)2.3 x 1014 s-1D)5.0 x 1014 s-1E)1.4 x 1015 s-1

E) 1.4 x 10^15 s -1

What is the energy in joules of one photon of x-ray radiation with a wavelength of 0.120 nm? A) 2.50 x 109 J B) 1.66 x 10-24 J C) 1.66 x 10-33 J D) 2.50 x 1018J E) 1.66 x 10-15J

E) 1.66 x 10^-15J

35.00 mL of a 0.30 M HCl solution is titrated with 0.35 M NaOH. What is the pH of the solution after 40.00 mL of the NaOH has been added? A) 2.46 B) 11.54 C) 7.00 D) 12.72 E) 12.67

E) 12.67

The bond angles in ICl2- are expected to be A) a little less than 109.5°. B) 109.5°. C) a little more than 109.5°. D) 120°. E) 180°.

E) 180°.

When 24.0 g of glucose (a nonelectrolyte) is dissolved in 500. g of water, the solution has a freezing point of -0.47°C. What is the molar mass of glucose? Kf of water is 1.86°C/m. A) 41.9 g/mol B) 47.5 g/mol C) 54.9 g/mol D) 178 g/mol E) 190. g/mol

E) 190. g/mol

Which of the following elementary steps is bimolecular? A) 2A + B → A2B B) 3B → B2 + B C) A + B + C → AB + C D) A2 → 2A E) 2A → A2

E) 2A → A2

Give the number of lone pairs around the central atom and the molecular geometry of XeF2. A) 0 lone pairs, linear B) 1 lone pair, bent C) 2 lone pairs, bent D) 3 lone pairs, bent E) 3 lone pairs, linear

E) 3 lone pairs, linear

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. A)1.35 × 10-51 /sB)1.03 × 108 /sC)2.06 × 1014 /sD)8.22 × 1014 /sE)3.08 × 1015 /s

E) 3.08 × 10^15 /s

Which one of the following molecules has an atom with an incomplete octet? A)NF3B)H2OC)AsCl3D)GeH4E)BF3

E) BF3

Which one of the following elements forms a stable 2+ cation? A)KrB)IC)SeD)AlE)Ba

E) Ba

Which one of the following substances is expected to have the highest melting point? A) CH4 B) CCl4 C) CO D) CO2 E) C(diamond)

E) C(diamond)

For which of the following species are the dispersion forces strongest? A) C4H10 B) C5H12 C) C6H14 D) C7H16 E) C8H18

E) C8H18

Which one of the following substances should exhibit hydrogen bonding in the liquid state? A) SiH4 B) H2 C) H2S D) CH4 E) CH3NH2

E) CH3NH2

Which ion is isoelectronic with Ar? A)Fe2+B)F-C)Br-D)Ga3+E)Ca2+

E) Ca2+

Which of the following liquids would have the highest viscosity at 25°C? A) CH3OCH3 B) CH2Cl2 C) C2H5OH D) CH3Br E) HOCH2CH2OH

E) HOCH2CH2OH

Which one of the following elements forms a stable 1- anion? A) K B) Be C) Al D) O E) I

E) I

The intermolecular forces present in C6H6 include which of the following? I. dipole-dipole II. ion-dipole III. dispersion IV. hydrogen bonding A) I, II, III, and IV B) I and III C) I, III, and IV D) I and II E) III only

E) III only

Which one of the following pairs are isoelectronic? A) Mn2+ and Ar B) Zn2+ and Cu2+ C) Na+ and K+ D) Cl- and S E) K+ and Cl-

E) K+ and Cl-

Which one of the following substances should exhibit hydrogen bonding in the liquid state? A) PH3 B) H2 C) H2S D) CH4 E) NH3

E) NH3

. Which one of the following sets of quantum numbers represents an electron with the highest energy? A) n = 3, l = 2, ml = -2, ms = +1/2 B) n = 4, l = 1, ml = 0, ms = -1/2 C) n = 4, l = 0, ml = 0, ms = +1/2 D) n = 5, l = 0, ml = 0, ms = +1/2 E) n = 4, l = 2, ml = -1, ms = -1/2

E) n = 4, l = 2, ml = -1, ms = -1/2

The geometry of the hybrid orbitals about a central atom with sp3d2 hybridization is: A)linearB)trigonal planarC)tetrahedralD)trigonal bipyramidalE)octahedral

E) octahedral

The geometry of the hybrid orbitals about a central atom with sp3d hybridization is: A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal bipyramidal

E) trigonal bipyramidal

1 Select True or False: The following set of quantum numbers is correct. n = 3, l = 3, ml = 0, ms = +1/2 ⊚ true ⊚ false

F

Select True or False: An electron in a 3p orbital could have a value of 2 for its angular momentum quantum number (l).

F

Select True or False: A neon atom in its ground state will be diamagnetic. ⊚ true ⊚ false

T

Select True or False: There is nothing wrong with the following set of quantum numbers: n = 3, l = 1, ml = 0, ms = +1/2

T