1 1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c Answer: E 2) The wavelength of light emitted from a traffic light having a frequency of Hz is. A) 702 nm B) 641 nm C) 674 nm D) 522 nm E) 583 nm 3) Of the following, radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared 4) The photoelectric effect is. A) the total reflection of light by metals giving them their typical luster B) the production of current by silicon solar cells when exposed to sunlight C) the ejection of electrons by a metal when struck with light of sufficient energy D) the darkening of photographic film when exposed to an electric field E) a relativistic effect
2 5) Which one of the following is considered to be ionizing radiation? A) visible light B) radio waves C) X-rays D) microwaves E) infrared radiation 6) Of the following transitions in the Bohr hydrogen atom, the transition results in the emission of the highest-energy photon. A) n = 1 n = 6 B) n = 6 n = 1 C) n = 6 n = 3 D) n = 3 n = 6 E) n = 1 n = 4 10) According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the of an electron. A) mass B) color C) momentum D) shape E) charge 11) All of the orbitals in a given electron shell have the same value of the quantum number. A) principal B) angular momentum C) magnetic D) spin E) psi 14) All of the orbitals in a given subshell have the same value of the quantum number. A) principal B) angular momentum C) magnetic D) A and B E) B and C
3 15) Which one of the following is not a valid value for the magnetic quantum number of an electron in a 5d subshell? A) 2 B) 3 C) 0 D) 1 E) -1 16) Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? A) 2d B) 2s C) 2p D) all of the above E) none of the above 18) An electron cannot have the quantum numbers n =, l =, m l =. A) 2, 0, 0 B) 2, 1, -1 C) 3, 1, -1 D) 1, 1, 1 E) 3, 2, 1 20) Which one of the following is an incorrect subshell notation? A) 4f B) 2d C) 3s D) 2p E) 3d 27) At maximum, an f-subshell can hold electrons, a d-subshell can hold electrons, and a p-subshell can hold electrons. A) 14, 10, 6 B) 2, 8, 18 C) 14, 8, 2 D) 2, 12, 21 E) 2, 6, 10
4 28) If an electron has a principal quantum number (n) of 3 and an angular momentum quantum number (l) of 2, the subshell designation is. A) 3p B) 3d C) 4s D) 4p E) 4d 30) Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, m l, m s ) for an electron in an atom? A) 2, 1, -1, 1/2 B) 2, 1, 0, 0 C) 2, 2, 0, 1/2 D) 2, 0, 1, -1/2 E) 2, 0, 2, +1/2 31) Which one of the following orbitals can hold two electrons? A) 2p x B) 3s C) 4d xy D) all of the above E) none of the above 33) Which one of the following represents an impossible set of quantum numbers for an electron in an atom? (arranged as n, l, m l, and m s ) A) 2, 1, -1, -1/2 B) 1, 0, 0, 1/2 C) 3, 3, 3, 1/2 D) 5, 4, - 3, 1/2 E) 5, 4, -3, -1/2
5 36) Which electron configuration represents a violation of the Pauli exclusion principle? A) B) C) D) E)
6 39) Which one of the following is the correct electron configuration for a ground-state nitrogen atom? A) B) C) D) E) None of the above is correct.
7 42) The ground state electron configuration of Ga is. A) 1s 2 2s 2 3s 2 3p 6 4s 2 3d 10 4p 1 B) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 10 4p 1 C) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 1 D) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4d 1 E) [Ar]4s 2 3d 11 43) The ground-state electron configuration of the element is [Kr]5s 1 4d 5. A) Nb B) Mo C) Cr D) Mn E) Tc 45) Which one of the following configurations depicts an excited oxygen atom? A) 1s 2 2s 2 2p 2 B) 1s 2 2s 2 2p 2 3s 2 C) 1s 2 2s 2 2p 1 D) 1s 2 2s 2 2p 4 E) [He]2s 2 2p 4
8 47) Which electron configuration represents a violation of Hund's rule for an atom in its ground state? A) B) C) D) E)
9 51) The ground state configuration of tungsten is. A) [Ar]4s23d3 B) [Xe]6s24f145d4 C) [Ne]3s1 D) [Xe]6s24f7 E) [Kr]5s24d105p5 2) In which set of elements would all members be expected to have very similar chemical properties? A) P, Se, I B) Cl, Br, Na C) Si, As, Te D) Ne, Na, Mg E) Br, I, At Answer: E 3) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger in Ar. A) nuclear charge B) paramagnetism C) diamagnetism D) Hund's rule E) azimuthal quantum number 4) Screening of the nuclear charge by core electrons in atoms is. A) less efficient than that by valence electrons B) more efficient than that by valence electrons C) essentially identical to that by valence electrons D) responsible for a general decrease in atomic radius going down a group E) both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group
10 5) The effective nuclear charge of an atom is primarily affected by. A) inner electrons B) outer electrons C) nuclear charge D) electron distribution E) orbital radial probability 6) The atomic radius of main-group elements generally increases down a group because. A) effective nuclear charge increases down a group B) effective nuclear charge decreases down a group C) effective nuclear charge zigzags down a group D) the principal quantum number of the valence orbitals increases E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases 7) Atomic radius generally increases as we move. A) down a group and from right to left across a period B) up a group and from left to right across a period C) down a group and from left to right across a period D) up a group and from right to left across a period E) down a group; the period position has no effect 9) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? A) Mg > Na > P > Si > Ar B) Ar > Si > P > Na > Mg C) Si > P > Ar > Na > Mg D) Na > Mg > Si > P > Ar E) Ar > P > Si > Mg > Na 10) Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr? A) Ca > K > As > Ge > Kr B) Kr > Ge > As > K > Ca C) Ge > As > Kr > K > Ca D) K > Ca > Ge > As > Kr E) Kr > As > Ge > Ca > K
11 11) Which one of the following atoms has the largest radius? A) O B) F C) S D) Cl E) Ne 12) Of the compounds below, has the smallest ionic separation. A) KF B) K 2 S C) RbCl D) SrBr 2 E) RbF 13) is isoelectronic with argon and is isoelectronic with neon. A) Cl -, F - B) Cl -, Cl + C) F+, F - D) Ne -, Kr + E) Ne -, Ar + 18) have the lowest first ionization energies of the groups listed. A) Alkali metals B) Transition elements C) Halogens D) Alkaline earth metals E) Noble gases 19) Which equation correctly represents the first ionization of aluminum? A) Al - (g) Al (g) + e - B) Al (g) Al - (g) + e - C) Al (g) + e - Al - (g) D) Al (g) Al + (g) + e - E) Al + (g) + e - Al (g)
12 23) Which of the following correctly represents the second ionization of phosphorus? A) P + (g) + e - P 2+ (g) B) P (g) P + (g) + e - C) P - (g) + e - P 2- (g) D) P + (g) P 2+ (g) + e - E) P + (g) + e - P (g) 31) Of the following species, has the largest radius. A) Rb + B) Sr 2+ C) Br - D) Kr E) Ar Consider the following electron configurations to answer the questions that follow: (i) 1s 2 2s 2 2p 6 3s 1 (ii) 1s 2 2s 2 2p 6 3s 2 (iii) 1s 2 2s 2 2p 6 3s 2 3p 1 (iv) 1s 2 2s 2 2p 6 3s 2 3p 4 (v) 1s 2 2s 2 2p 6 3s 2 3p 5 32) The electron configuration belonging to the atom with the highest second ionization energy is. A) (i) B) (ii) C) (iii) D) (iv) E) (v) Diff: 1 Page Ref: Sec ) The electron configuration that belongs to the atom with the lowest second ionization energy is. A) (i) B) (ii) C) (iii) D) (iv) E) (v)
13 Consider the following electron configurations to answer the questions that follow: (i) 1s 2 2s 2 2p 6 3s 1 (ii) 1s 2 2s 2 2p 6 3s 2 (iii) 1s 2 2s 2 2p 6 3s 2 3p 1 (iv) 1s 2 2s 2 2p 6 3s 2 3p 4 (v) 1s 2 2s 2 2p 6 3s 2 3p 5 34) The electron configuration of the atom with the most negative electron affinity is. A) (i) B) (ii) C) (iii) D) (iv) E) (v) Answer: E Diff: 1 Page Ref: Sec ) The electron configuration of the atom that is expected to have a positive electron affinity is. A) (i) B) (ii) C) (iii) D) (iv) E) (v) 13) In which of the molecules below is the carbon-carbon distance the shortest? A) H 2 C CH 2 B) H C C H C) H 3 C CH 3 D) H 2 C C CH 2 E) H 3 C CH 2 C H 3 14) Of the atoms below, is the most electronegative. A) Si B) Cl C) Rb D) Ca E) S
14 15) Of the molecules below, the bond in is the most polar. A) HBr B) HI C) HCl D) HF E) H 2 16) Which of the following has the bonds correctly arranged in order of increasing polarity? A) Be F, Mg F, N F, O F B) O F, N F, Be F, Mg F C) O F, Be F, Mg F, N F D) N F, Be F, Mg F, O F E) Mg F, Be F, N F, O F 18) The Lewis structure of N 2 H 2 shows. A) a nitrogen-nitrogen triple bond B) a nitrogen-nitrogen single bond C) each nitrogen has one nonbonding electron pair D) each nitrogen has two nonbonding electron pairs E) each hydrogen has one nonbonding electron pair 21) In the Lewis symbol for a sulfur atom, there are paired and unpaired electrons. A) 2, 2 B) 4, 2 C) 2, 4 D) 0, 6 E) 5, 1
15 23) In the nitrite ion (NO 2 - ),. A) both bonds are single bonds B) both bonds are double bonds C) one bond is a double bond and the other is a single bond D) both bonds are the same E) there are 20 valence electrons 24) Resonance structures differ by. A) number and placement of electrons B) number of electrons only C) placement of atoms only D) number of atoms only E) placement of electrons only Answer: E 46) As the number of covalent bonds between two atoms increases, the distance between the atoms and the strength of the bond between them. A) increases, increases B) decreases, decreases C) increases, decreases D) decreases, increases E) is unpredictable 47) Of the possible bonds between carbon atoms (single, double, and triple),. A) a triple bond is longer than a single bond B) a double bond is stronger than a triple bond C) a single bond is stronger than a triple bond D) a double bond is longer than a triple bond E) a single bond is stronger than a double bond 2) ClF3 has "T-shaped" geometry. There are non-bonding domains in this molecule. A) 0 B) 1 C) 2 D) 3 E) 4 Diff: 4 Page Ref: Sec ) The electron domain and molecular geometry of BrO2 - is.
16 A) tetrahedral, trigonal planar B) trigonal planar, trigonal planar C) trigonal pyramidal, linear D) tetrahedral, bent E) trigonal pyramidal, seesaw 5) The electron-domain geometry of is tetrahedral. A) CBr 4 B) PH 3 C) CCl 2 Br 2 D) XeF 4 E) all of the above except XeF 4 Answer: E Diff: 2 Page Ref: Sec ) The O-C-O bond angle in the CO3 2- ion is approximately. A) 90 B) C) 120 D) 180 E) 60 Diff: 2 Page Ref: Sec ) Of the following species, will have bond angles of 120. A) PH 3 B) ClF 3 C) NCl 3 D) BCl 3 E) All of these will have bond angles of 120.
17 11) The bond angles marked a, b, and c in the molecule below are about,, and, respectively. A) 90, 90, 90 B) 120, 120, 90 C) 120, 120, D) 109.5, 120, E) 109.5, 90, 120 Diff: 2 Page Ref: Sec ) The central iodine atom in the ICl 4 - ion has nonbonded electron pairs and bonded electron pairs in its valence shell. A) 2, 2 B) 3, 4 C) 1, 3 D) 3, 2 E) 2, 4 Answer: E Diff: 1 Page Ref: Sec ) Of the molecules below, only is polar. A) SbF 5 B) AsH 3 C) I 2 D) SF 6 E) CH 4 Diff: 2 Page Ref: Sec ) Of the molecules below, only is nonpolar. A) CO 2 B) H 2 O C) NH 3 D) HCl
18 E) TeCl 2 Diff: 1 Page Ref: Sec ) According to valence bond theory, which orbitals overlap in the formation of the bond in HBr? A) 1s on H and 4p on Br B) 1s on H and 4s on Br C) 1s on H and 3p on Br D) 2s on H and 4p on Br E) 2s on H and 3p on Br Diff: 1 Page Ref: Sec ) The electron-domain geometry of a carbon-centered compound is tetrahedral. The hybridization of the central carbon atom is. A) sp B) sp 2 C) sp 3 D) sp 3 d E) sp 3 d 2 Diff: 2 Page Ref: Sec ) Of the following, only has sp 2 hybridization of the central atom. A) PH 3 B) CO 3 2- C) ICl 3 D) l 3 - E) PF 5 Diff: 1 Page Ref: Sec ) Of the following, the central atom is sp 3 d 2 hybridized only in. A) PCl 5 B) XeF 4 C) PH 3 D) Br 3 - E) BeF 2 Diff: 1 Page Ref: Sec. 9.5
19 58) There are unhybridized p atomic orbitals in an sp2-hybridized carbon atom. A) 0 B) 1 C) 2 D) 3 E) 4 Diff: 1 Page Ref: Sec ) When three atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed? A) one B) six C) three D) four E) five Diff: 1
20 64) A typical double bond. A) is stronger and shorter than a single bond B) consists of one σ bond and one π bond C) imparts rigidity to a molecule D) consists of two shared electron pairs E) All of the above answers are correct. Answer: E Diff: 1 Page Ref: Sec ) A typical triple bond. A) consists of one σ bond and two π bonds B) consists of three shared electrons C) consists of two σ bonds and one π bond D) consists of six shared electron pairs E) is longer than a single bond Diff: 1 Page Ref: Sec ) In a polyatomic molecule, "localized" bonding electrons are associated with. A) one particular atom B) two particular atoms C) all of the atoms in the molecule D) all of the π bonds in the molecule E) two or more σ bonds in the molecule Diff: 1 Page Ref: Sec ) There are σ bonds and π bonds in H3C CH2 CH CH CH2 C CH. A) 14, 2 B) 10, 3 C) 12, 2 D) 13, 2 E) 16, 3 Answer: E Diff: 4 Page Ref: Sec. 9.6
21 68) Which of the following molecules or ions will exhibit delocalized bonding? SO 2 SO 3 SO 3 2- A) SO 2, SO 3, and SO 3 2- B) SO 3 2- only C) SO 2 and SO 3 D) SO 3 and SO 3 2- E) None of the above will exhibit delocalized bonding. Diff: 1 Page Ref: Sec ) A typical triple bond consists of. A) three sigma bonds B) three pi bonds C) one sigma and two pi bonds D) two sigma and one pi bond E) three ionic bonds Diff: 1 Page Ref: Sec ) In comparing the same two atoms bonded together, the the bond order, the the bond length, and the the bond energy. A) greater, shorter, greater B) greater, greater, greater C) greater, longer, greater D) greater, greater, smaller E) smaller, greater, greater Diff: 4 Page Ref: Sec ) Based on molecular orbital theory, the bond order of the H H bond in the H 2 + ion is. A) 0 B) 1/2 C) 1 D) 3/2 E) 2 Diff: 4 Page Ref: Sec. 9.7
22 94) Molecular Orbital theory correctly predicts paramagnetism of oxygen gas, O 2. This is because. A) the bond order in O 2 can be shown to be equal to 2. B) there are more electrons in the bonding orbitals than in the antibonding orbitals. C) the energy of the π 2p MOs is higher than that of the σ 2p MO D) there are two unpaired electrons in the MO electron configuration of O 2 E) the O O bond distance is relatively short 97) Based on molecular orbital theory, there are unpaired electrons in the OF + ion. A) 0 B) 3 C) 1 D) 2 E) 1/2 Diff: 3 Page Ref: Sec ) Based on molecular orbital theory, the bond order of the N N bond in the N 2 molecule is. A) 0 B) 1 C) 2 D) 3 E) 5 Diff: 4 Page Ref: Sec. 9.8
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