MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

Transcription

1 Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The reaction of HNO3(aq) + KOH(aq) KNO3(aq) + H2O(l) is best classified as a(n) A) precipitation reaction. B) single replacement reaction. C) oxidation-reduction reaction. D) acid-base neutralization reaction. 1) 2) Arrange the following spectral regions in order of increasing wavelength: infrared, microwave, ultraviolet, visible. A) microwave < infrared < visible < ultraviolet B) ultraviolet < infrared < visible < microwave C) microwave < visible < infrared < ultraviolet D) ultraviolet < visible < infrared < microwave 2) 3) What is the oxidation number of the sulfur atom in Li2SO4? A) +4 B) +6 C) +2 D) -2 3) 4) Based on the balanced chemical equation shown below, determine the mass percent of Fe 3+ in a g sample of iron ore, if ml of a M stannous chloride, SnCl 2 (aq), solution is 4) required to completely react with the Fe 3+ present in the ore sample. The chemical equation for the reaction is 2 Fe3+(aq) + Sn2+(aq) 2 Fe2+(aq) + Sn4+(aq) A) 6.196% B) 38.79% C) 9.697% D) 19.40% 5) What are the coefficients in front of NO3 - (aq) and Cu(s) when the following redox equation is balanced in an acidic solution: NO3 - (aq) + Cu(s) NO(g) + Cu2+(aq)? A) 2, 6 B) 3, 6 C) 3, 4 D) 2, 3 5) 6) What is the frequency of a helium-neon laser light with a wavelength of nm? The speed of light is m/s. A) s-1 B) s-1 C) s-1 D) s-1 6) 7) The absorption of light of frequency Hz is required for CO molecules to go from the lowest rotational energy level to the next highest rotational energy level. Determine the energy for this transition in kj/mol. h = J s A) 46.3 kj/mol B) 949 kj/mol C) kj/mol D) kj/mol 7) 1

2 8) The mixing of which pair of reactants will result in a precipitation reaction? A) HCl(aq) + Ca(OH)2(aq) B) NaNO3(aq) + NH4Cl(aq) C) CsI(aq) + NaOH(aq) D) K2SO4(aq) + Ba(NO3)2(aq) 8) Ch. 4 #47 (43) 9) What is the oxidation number change for the chromium atom in the following unbalanced reduction half reaction: Cr 2 O7 2- (aq) + H+(aq) Cr3+(aq) + H2O(l)? A) +6 B) -7 C) +3 D) -3 9) 10) What are the possible values of n and ml for an electron in a 5d orbital? A) n = 5 and ml = -2, -1, 0, +1, or +2 B) n = 1, 2, 3, 4, or 5 and ml = 2 C) n = 5 and ml = 2 D) n = 1, 2, 3, 4, or 5 and ml = -2, -1, 0, +1, or +2 10) 11) According to the balanced chemical equation 5 H2C2O4(aq) + 2 MnO4 - (aq) + 6 H+(aq) 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) grams of oxalic acid, H2C2O4 will react with ml of M potassium permanganate, KMnO4 solution. A) 97.2 ml B) 15.5 ml C) 38.9 ml D) 77.7 ml 11) 12) For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is nm-1. A) nm B) nm C) nm D) nm 12) 13) What is the molar concentration of sodium ions in a M Na3PO4 solution? A) 1.40 M B) 1.05 M C) M D) M 13) 14) How many orbitals are there in the seventh shell? A) 21 B) 49 C) 7 D) 6 14) 15) The number of orbitals in a given subshell, such as the 5d subshell, is determined by the number of possible values of A) l. B) n. C) ml. D) ms. 15) 16) The mixing of which pair of reactants will result in a precipitation reaction? A) Cu(NO3)2(aq) + Na2CO3(aq) B) NaClO4(aq) + (NH4)2S(aq) C) K2SO4(aq) + Cu(NO3)2(aq) D) NH4Br(aq) + NaI(aq) 16) 17) Determine the number of water molecules necessary to balance the following chemical equation Cr2O7 2- (aq) + Cl-(aq) + H+(aq) Cr3+(aq) + Cl2(g) + H2O(l). A) 3 B) 14 C) 7 D) 5 17) 2

3 18) What is the first ionization energy for a hydrogen atom in the ground state? The Rydberg constant is nm-1. A) J B) J C) J D) J 18) 19) The first vibrational level for NaH lies at J and the second vibrational level lies at J. What is the frequency of the photon emitted when a molecule of NaH drops from the second vibrational level to the first vibrational level? A) Hz B) Hz C) Hz D) Hz 19) 20) Which of the following is not a valid set of quantum numbers? A) n = 3, l = 0, ml = 0, and ms = 1/2 B) n = 2, l = 1, ml = -1, and ms = -1/2 C) n = 3, l = 2, ml = 3, and ms = 1/2 D) n = 2, l = 1, ml = 0, and ms = -1/2 20) 21) What reagent would distinguish between Ba2+ and Pb2+? A) Na2S2O3 B) NaNO3 C) NaCl D) Na2SO4 21) 22) Of the following, which atom has the largest atomic radius? A) Cl B) Br C) Na D) K 22) 23) What is the ground-state electron configuration of Co? A) [Ar]3d9 B) [Ar]4s23d7 C) [Ar]4s13d8 D) [Ar]4s24p64d1 23) 24) How many unpaired electrons are in an atom of Co in its ground state? A) 7 B) 1 C) 3 D) 2 24) 25) Which of the following have their valence electrons in the same shell? A) N, As, Bi B) K, As, Br C) He, Ne, F D) B, Si, As 25) 26) What is the general valence-electron ground-state electron configuration for neutral alkaline earth metals? A) ns2 B) 1s22s2 C) 1s22s1 D) ns1 26) 27) The symbol [Kr] represents A) 4s24p6. B) 1s22s22p63s23p64s24p6. C) 1s22s22p63s23p63d104s24p64d10. D) 1s22s22p63s23p63d104s24p6. 27) 3

4 28) For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l? 28) A) n = 4 and l = 0 B) n = 4 and l = 3 C) n = 4 and l = 2 D) n = 4 and l = 1 29) The phosphorus atom in PCl3 would be expected to have a A) 3+ charge. B) partial negative (δ-) charge. C) 3- charge. D) partial positive (δ+) charge. 29) 30) The Cl Cl bond energy is 243 kj/mol. Therefore the formation of a single bond between chlorine atoms A) should require the absorption of 243 kj per mole of Cl2 formed. B) should result in the release of 486 kj per mole of Cl2 formed. C) should result in the release of 243 kj per mole of Cl2 formed. D) should require the absorption of 486 kj per mole of Cl2 formed. 30) 31) Of the following elements, which has the highest electronegativity? A) Sc B) P C) S D) As 31) 32) How many electrons are in the valence shell of I in IF4 -? A) 14 B) 12 C) 10 D) 8 32) 33) How many lone pairs of electrons are on the P atom in PF3? A) 2 B) 1 C) 0 D) 3 33) 34) Which element can expand its valence shell to accommodate more than eight electrons? A) He B) O C) P D) C 34) 35) Which is the most acceptable electron dot structure for N2H2? 35) A) B) C) D) 4

5 36) The molecule SO2 would be expected to have A) two identical bonds intermediate between a single and a double bond. B) two single bonds. C) two double bonds. D) one single and one double bond. 36) 37) Which one of the following is expected to exhibit resonance? A) CO2 B) NH4 + C) HCN D) NO2-37) 38) The electronegativity is 2.1 for H and 1.8 for Si. Based on these electronegativities, SiH4 would be expected to A) be ionic and contain H + ions. 38) B) be ionic and contain H - ions. C) have polar covalent bonds with a partial negative charges on the H atoms. D) have polar covalent bonds with a partial positive charges on the H atoms. 39) Which of the following should be nonplanar? 39) A) I and III B) only III C) only II D) only I 40) What is the molecular geometry of AsCl3? A) tetrahedral B) trigonal pyramidal C) trigonal planar D) T-shaped 40) 41) What geometric arrangement of charge clouds is expected for an atom that has five charge clouds? A) tetrahedral B) trigonal bipyramidal C) octahedral D) square planar 41) 42) How many lone pairs of electrons are on the Xe atom in XeF6? A) 0 B) 3 C) 2 D) 1 42) 43) Which molecule contains a triple bond? A) HCN B) F2 C) O3 D) H2CO 43) 44) How many lone pairs are on the Br atom in BrF2 -? A) 2 B) 3 C) 0 D) 1 44) 5

6 45) How much heat is absorbed when g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation? 5 C(s) + 2 SO2(g) CS2(l) + 4 CO(g) ΔH = kj A) kj B) kj C) kj D) 1439 kj 45) 46) Which orbital hybridization is associated with a tetrahedral charge cloud arrangement? A) sp B) sp3d2 C) sp3 D) sp2 46) 47) What is the molecular geometry of BrF4 -? A) square planar B) square pyramidal C) seesaw D) tetrahedral 47) 48) What orbital hybridization is expected for the central atom in a molecule with a square planar geometry? A) sp3d B) sp3 C) sp2 D) sp3d2 48) 49) What is the smallest bond angle in SF6? A) B) 60 C) 120 D) 90 49) 50) A triple bond is generally composed of A) one π bond and two σ bonds. B) two π bonds and one σ bond. C) three σ bonds. D) three π bonds. 50) 51) The orbital hybridization on the carbon atom in HCN is A) sp3d2. B) sp2. C) sp. D) sp3. 51) 52) It takes 11.2 kj of energy to raise the temperature of 145 g of benzene from 25.0 C to 70.0 C. What is the specific heat of benzene? A) 5.41 J/(g C) B) 3.48 J/(g C) C) 1.10 J/(g C) D) 1.72 J/(g C) 52) 53) How much heat is absorbed/released when g of NH3(g) reacts in the presence of excess O 2 (g) to produce NO(g) and H2O(l) according to the following chemical equation? 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(l) ΔH = kj A) kj of heat are absorbed. B) kj of heat are released. C) 1372 kj of heat are released. D) 1372 kj of heat are absorbed. 53) 6

7 Answer Key Testname: SU_06_E2_REVIEW 1) D 2) D 3) B 4) B 5) D 6) D 7) D 8) D 9) D 10) A 11) B 12) D 13) B 14) B 15) C 16) A 17) C 18) A 19) A 20) C 21) C 22) D 23) B 24) C 25) B 26) A 27) D 28) D 29) D 30) C 31) C 32) B 33) B 34) C 35) B 36) A 37) D 38) C 39) B 40) B 41) B 42) D 43) A 44) B 45) C 46) C 47) A 48) D 49) D 7

8 Answer Key Testname: SU_06_E2_REVIEW 50) B 51) C 52) D 53) A 8