ap chem midterm WHOOP

Metal Hydroxides are A) Bases B) Acids

A) Bases

Which of the following lists Mg, P, and Cl in order of increasing atomic radius? A) Cl < P < Mg B) Cl < Mg < P C) Mg < P < Cl D) Mg < Cl < P E) P < Cl < Mg

A) Cl < P < Mg

Which of the following molecules has the shortest bond length? A) N2 B) O2 C) Cl2 D) Br2 E) I2

A) N2

MnO4− + 5 Fe2+ + 8 H+ Mn2+ + 5 Fe3+ + 4 H2O In the reaction represented above, the number of MnO4- ions that react must be equal to which of the following? A) One-fifth the number of Fe2+ ions that are consumed B) Eight times the number of H+ ions that are consumed C) Five times the number of Fe3+ ions that are produced D) One-half the number of H2O molecules that are produced

A) One-fifth the number of Fe2+ ions that are consumed

Based on the data in the table above, which of the following correctly predicts the relative strength of the attraction of Zn2+, Ca2+, and Ba2+ ions to water molecules in a solution, from strongest to weakest, and provides the correct reason? A) Zn2+ > Ca2+ > Ba2+ because the smaller ions have a stronger coulombic attraction to water B) Zn2+ > Ca2+ > Ba2+ because the smaller ions are more electronegative C) Ba2+ > Ca2+ > Zn2+ because the larger ions are more polarizable D) Ba2+ > Ca2+ > Zn2+ because the larger ions are less electronegative

A) Zn2+ > Ca2+ > Ba2+ because the smaller ions have a stronger coulombic attraction to water

H-C=C-H What is the hybridization of the carbon atoms in a molecule of ethyne, represented above? A) sp B) sp2 C) sp3 D) dsp2 E) d2sp

A) sp

. LiHCO3(aq) + . . . H2SO4(aq) . . . Li2SO4(aq) + . . . H2O(l) + . . . CO2(g) When the equation above is balanced and the coefficients are reduced to lowest whole-number terms, what is the coefficient of H2O(l) ? A) 1 B) 2 C) 3 D) 4 E) 5

B) 2

Which is listed in order of increasing boiling points A) Butane<propanol<acetone B) Butane<acetone<propanol C) propanol<acetone<butane D) Acetone=butane<propanol

B) Butane<acetone<propanol

______ have one more H+ than _______ A) Conjugate bases, conjugate acids B) Conjugate acids, conjugate bases

B) Conjugate acids, conjugate bases

What is the identity of the metal chloride? A) NaCl B) KCl C) CuCl D) LiCl

B) KCl

Na20=62 MgO=30.3 K2O=94.2 CaO=56.1 According to the information in the table above, a 1.00 g sample of which of the following contains the greatest mass of oxygen? A) Na2O B) MgO C) K2O D) CaO

B) MgO

NH2+HCl->NH4++Cl- the bron-low bases are A) NH3 and NH3+ B) NH3 and Cl- C) NH3 and HCl D) HCl and NH4+ E) HCl and Cl-

B) NH3 and Cl-

Which of the following could be the identity of a white crystal solid with the following properties: 1) melts at 320 2) doesnt conduct electricity as a solid 3) conducts electricity in aqueous solutions A) C6H12O6 B) NaOH C) SiO2 D) Cu(S)

B) NaOH

Resonance is most commonly used to describe the bonding in molecules of which of the following? A) CO2 B) O3 C) H2O D) CH4 E) SF6

B) O3

For which of the following molecules are resonance structures necessary to describe the bonding satisfactorily? A) H2S B) SO2 C) CO2 D) OF2 E) PF3

B) SO2

Is a polar molecule A) BeCl2 B) SO2 C) N2 D) O2 E) F2

B) SO2

Type of reaction that occurs when solid sodium acetate Na2C2H3O2(s) is added to water

Bronsted Lowry-Base Reaction

Which flask contains the sample with the greatest density? A) A B) B C) C D) D E) E

C) C

Of the following single bonds, which is the LEAST polar? A) N—H B) H—F C) O—F D) I—F E) O—H

C) O—F

Which of the following best helps to explain the deviation of the first ionization energy of oxygen from the overall trend? A) The atomic radius of oxygen is greater than the atomic radius of fluorine. B) The atomic radius of oxygen is less than the atomic radius of nitrogen. C) There is repulsion between paired electrons in oxygen's 2p orbitals. D) There is attraction between paired electrons in oxygen's 2p orbitals.

C) There is repulsion between paired electrons in oxygen's 2p orbitals.

A 360. mg sample of aspirin, C9H8O4, (molar mass 180. g), is dissolved in enough water to produce 200. mL of solution. What is the molarity of aspirin in a 50. mL sample of this solution? A) 0.0800 M B) 0.0400 M C) 0.0200 M D) 0.0100 M E) 0.00250 M

D) 0.0100 M

When a 3.22 g sample of an unknown hydrate of sodium sulfate, Na2SO4 ⋅ H2O(s), is heated, H2O (molar mass 18 g) is driven off. The mass of the anhydrous Na2SO4(s) (molar mass 142 g) that remains is 1.42 g. The value of x in the hydrate is A) 0.013 B) 1.8 C) 6.0 D) 10. E) 20.

D) 10.

For an experiment, a student needs 100.0 mL of 0.4220 M NaCl. If the student starts with NaCl(s) and distilled water, which of the following pieces of laboratory glassware should the student use to prepare the solution with the greatest accuracy? A) 25 mL volumetric pipet B) 100 mL Erlenmeyer flask C) 100 mL graduated cylinder D) 100 mL volumetric flask E) 1 L beaker

D) 100 mL volumetric flask

How many mL of 10.0 M HCl are needed to prepare 500. mL of 2.00 M HCl ? A) 1.00 mL B) 10.0 mL C) 20.0 mL D) 100. mL E) 200. mL

D) 100. mL

H2+F2->2HF What mass of HF is produced by 3x10^23 moolecules of H2 with excess F2? A) 1.0 g B) 4.0 g C) 10 g D) 20 g E) 40 g

D) 20 g

C3H8(g) + 4 Cl2(g) C3H4Cl4(g) + 4 HCl(g) A 6.0 mol sample of C3H8(g) and a 20. mol sample of Cl2(g) are placed in a previously evacuated vessel, where they react according to the equation above. After one of the reactants has been totally consumed, how many moles of HCl(g) have been produced? A) 4.0 mol B) 8.0 mol C) 20. mol D) 24 mol

D) 24 mol

A chemical supply company sells a concentrated solution of aqueous H2SO4 (molar mass 98 g mol-1) that is 50 percent H2SO4 by mass. At 25C, the density of the solution is 1.4 g mL-1. What is the molarity of the H2SO4 solution at 25C? A) 1.8 M B) 3.6 M C) 5.1 M D) 7.1 M E) 14 M

D) 7.1 M

A sample of CaCO3 (molar mass 100. g) was reported as being 30 percent Ca. Assuming no calcium was present in any impurities, the percent of CaCO3 in the sample is A) 30% B) 40% C) 70% D) 75% E) 100%

D) 75%

. . Cr2O72-(aq) + . . . H2S(g) + . . . H+(aq) . . . Cr3+(aq) + . . . S(s) + . . . H2O(l) When the equation above is correctly balanced and all coefficients are reduced to lowest whole-number terms, the coefficient for H+(aq) is A) 2 B) 4 C) 6 D) 8 E) 14

D) 8

Which of the following correctly identifies which has the higher first-ionization energy, Cl or Ar, and supplies the best justification? A) Cl, because of its higher electronegativity B) Cl, because of its higher electron affinity C) Ar, because of its completely filled valence shell D) Ar, because of its higher effective nuclear charge

D) Ar, because of its higher effective nuclear charge

Has the highest electronegativity A) Cs B) Ag C) Pb D) Br E) Se

D) Br

The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the right of the peak in the lower spectrum? A) Nitrogen atoms have a half-filled p subshell. B) There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms. C) Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p subshell of nitrogen atoms. D) Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

D) Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

During the course of the experiment, which of the following happens to the NO3- ions? A) They are oxidized by Cl- ions. B) They are reduced to NO2- ions. C) They are decomposed by reacting with M+ ions. D) They remain dissolved in the filtrate solution.

D) They remain dissolved in the filtrate solution.

A 0.20 mol sample of MgCl2(s) and a 0.10 mol sample of KCl(s) are dissolved in water and diluted to 500 mL. What is the concentration of Cl- in the solution? A) 0.15 M B) 0.30 M C) 0.50 M D) 0.60 M E) 1.0 M

E) 1.0 M

Which of the following is the electron configuration of an excited atom that is likely to emit a quantum of energy? A) 1s2 2s22p6 3s23p1 B) 1s2 2s22p6 3s23p5 C) 1s2 2s22p6 3s2 D) 1s2 2s22p6 3s1 E) 1s2 2s22p6 3s13p1

E) 1s2 2s22p6 3s13p1

Which of the following has a zero dipole moment? A) HCN B) NH3 C) SO2 D) NO2 E) PF5

E) PF5

Indicates that an atomic orbital can hold no more than two electrons

Pauli Exclusion Principle

N2 molecules absorb ultraviolet light but not visible light. I2 molecules absorb visible and UV, why?

Visible light does not produce transitions between electron energy levels in N2 but does in I2