PX0311-0709 1. What is the wavelength of a photon having a frequency of 4.50 10 14 Hz? (, ) A) 667 nm B) 1.50 10 3 nm C) 4.42 10 31 nm D) 0.0895 nm E) 2.98 10 10 nm 2. When a particular metal is illuminated with photons, one electron is observed for each absorbed photon. What effect would decreasing the wavelength and number of photons have on the electrons leaving the surface? A) There would be more electrons leaving the surface. B) They would have higher kinetic energy. C) The electron velocity would be lower. D) The kinetic energy of the electrons would be lower. E) Two photons might be required to eject the electrons. 3. In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus, A) energy is absorbed. B) light is emitted. C) energy is emitted. D) no change in energy occurs. E) none of these 4. When an electron in an atom makes a transition from n = 6 to n = 4, which of the following statements is/are correct? I. Energy is emitted. II. Energy is absorbed. III. The electron loses energy. IV. The electron gains energy. V. The electron cannot make this transition. A) I and III B) I and IV C) II and IV D) II and III E) III 5. Which of the following statements concerning quantum mechanics is/are true? 1. The behavior of submicroscopic particles can sometimes be described as waves.
2. Quantum mechanics limits us to making statistical statements about the location of an electron in an atom. 3. The uncertainty principle is important only for particles of very small mass, such as the electron. A) 1 only B) 2 only C) 3 only D) 2 and 3 E) 1, 2, and 3 6. Which of the following statements is a valid conclusion from the Heisenberg uncertainty principle? A) The square of the wave function is proportional to the probability of finding a particle in space. B) Particles can exhibit wavelike behavior. C) The orbits proposed by Bohr s model of the atom are correct. D) An electron in a 2p orbital is always closer to the nucleus than an electron in a 3p orbital. E) The act of measuring a particle's position changes its momentum, and vice versa. 7. Which of the following sets of quantum numbers (n, l, m l, m s ) is not permissible? A) 3 3 3 + 1 2 B) 2 1 1 + 1 2 C) 1 0 0 + 1 2 D) 3 2 2 1 2 E) 4 0 0 1 2 8. Which of the following is a representation of a 3d xz orbital? A) B) C)
D) E) 9. Which of the following statements is incorrect? A) Stern and Gerlach discovered electron spin by passing silver atoms through a magnetic field. B) Hund s rule states that electrons are placed in the orbitals of a subshell in such a way as to give a maximum number of unpaired electrons. C) The Pauli exclusion principle states that each electron in an atom must have its own unique set of quantum numbers. D) Valence electrons consist of those electrons not contained within a noble-gas core or a pseudo-noble-gas core. E) The building-up principle states that electrons are added to atoms in order of increasing principal quantum number. 10. Which of the following electron configurations represents an excited state of the indicated atom? A) Ne: 1s 2 2s 2 2p 6 B) N: 1s 2 2s 2 2p 3 C) P: 1s 2 2s 2 2p 6 3s 2 3p 2 4s 1 D) Na: 1s 2 2s 2 2p 6 3s 2 3p 2 3s 1 E) He: 1s 2 11. The ground-state valence-shell configuration of a particular atom is. The element to which this atom belongs is a A) noble gas. B) inner transition element. C) p-block main-group element. D) transition element. E) s-block main-group element. 12. Which of the following statements is incorrect? A) A p-block main-group element belonging to period n has a completely filled (n 1)d subshell. B) All noble gases have completely filled shells. C) All s-block main-group elements have only one or two valence electrons. D) Carbon and silicon have the same number of valence electrons. E) All elements in the n = 4 period have a partially or completely filled n = 4 shell.
13. Which of the following statements is true concerning the electron configuration [Ne]3s 1 3p 1? A) It may represent a ground-state electron configuration of a Al + cation. B) It may represent an excited-state electron configuration of a Mg atom. C) It may represent an excited-state electron configuration of a Ne anion. D) It may represent a ground-state electron configuration of a Mg + cation. E) It may represent a ground-state electron configuration of a Na + cation. 14. An element that has the same ground state valence-shell electron configuration as indium is A) boron. B) silicon. C) krypton. D) lithium. E) barium. 15. An atom of which of the following elements is not diamagnetic in the ground state? A) Ca B) Rn C) All are diamagnetic. D) Cd E) Pt 16. The ground-state electron configuration of a. Therefore, is A) paramagnetic with four unpaired electrons. B) diamagnetic. C) paramagnetic with one unpaired electron. D) paramagnetic with five unpaired electrons. E) paramagnetic with three unpaired electrons. 17. Which of the following atoms is paramagnetic in its ground state? A) tin (Sn) B) barium (ba) C) cadmium (Cd) D) ytterbium (Yb) E) argon (Ar) 18. Which of the following species would be expected to have chemical properties most similar to those of the nitrogen atom? A) nitride ion B) nitrite ion C) phosphate ion D) phosphide ion E) phosphorus atom 19. In general, atomic radii A) decrease from left to right in a period and increase down a group. B) increase from left to right in a period and decrease down a group. C) do not change across a period or a group. D) decrease from left to right and decrease down a group.
E) increase from left to right in a period and increase down a group. 20. An atom of which of the following elements has the largest atomic radius? A) Cl B) P C) Na D) S E) Si 21. An atom of which of the following elements has the largest atomic radius? A) Ge B) K C) Cl D) Ca E) As 22. Below are data on the first four ionization energies for a fictitious element X. First ionization energy = 500 kj/mol Second ionization energy = 2000 kj/mol Third ionization energy = 3500 kj/mol Fourth ionization energy = 25000 kj/mol From the data, which of the following statements is incorrect? A) The third ionization energy is greater than the second ionization energy because X 2+ has a bigger charge than X +. B) X could belong to Group IIIA. C) X could belong to Group IIIB. D) X could belong to group VA. E) The fourth ionization energy is much greater than the third ionization energy because X 3+ consists of a noble-gas core or a pseudo-noble-gas core. 23. An atom of which of the following elements has the smallest first ionization energy? A) Sn B) Pb C) Ge D) C E) Si 24. The change in energy for which of the following processes corresponds to the electron affinity of iodine? A) B) C) D) E) 25. Which element forms the most acidic oxide?
A) B B) Tl C) Al D) In E) Ga 26. A few atoms of the new element 113 were created in 2004 by a team of Russian and American scientists. It has been given the temporary name "ununtrium" and the temporary symbol "Uut." Based on ununtrium's position on the periodic table, what type of oxide(s) should it form? A) Ununtrium should form a basic oxide with the formula Uut 2 O 3. B) Ununtrium should form an amphoteric oxide with the formula UutO. C) Ununtrium should form an acidic oxide with the formula Uut 2 O 3. D) Ununtrium should form two acidic oxides having the formulas Uut 2 O and Uut 2 O 3. E) Ununtrium should form two basic oxides having the formulas Uut 2 O and Uut 2 O 3. 27. The element antimony is in the same group as phosphorus. Which of the following is the formula of antimonous acid? A) B) C) D) E) 28. When the cations Na +, K +, Rb +, Cs + are combined with chloride ion in the gas phase to form ion pairs, which pair formation releases the greatest amount of energy? A) KCl B) All release the same amount of energy. C) RbCl D) NaCl E) CsCl 29. Which of the following statements concerning lattice energy is false? A) MgO has a larger lattice energy than NaF. B) The lattice energy for a solid with 2+ and 2 ions should be two times that for a solid with 1+ and 1 ions. C) MgO has a larger lattice energy than LiF. D) Lattice energy is often defined as the change in energy that occurs when an ionic solid is separated into isolated ions in the gas phase. E) All of these are true. 30. Which of the following compounds would be expected to have the lowest melting point? A) AlF 3 B) RbF C) NaF D) MgF 2 E) CaF 2 31. Which of the following is the Lewis dot structure for the rubidium ion?
A) B) C) D) E) 32. All of the following species have ground-state noble-gas electron configurations except A) Ge 4+ B) K + C) Kr D) I E) P 3 33. All of the following species are isoelectronic except A) S 2 B) K + C) Na + D) Ar E) Cl 34. All of the following species are isoelectronic except A) O B) Ne C) N 3 D) Mg 2+ E) F 35. For which of the following pairs of species is the difference in radius the greatest? A) C and F B) K + and Br C) Li + and I D) Na and Mg E) O 2 and F 36. Which of the following is the best explanation for a covalent bond?
A) electrons simultaneously attracted by more than one nucleus B) an interaction between outer electrons C) the overlapping of unoccupied orbitals of two or more atoms D) the overlapping of two electron-filled orbitals having different energies E) a positive ion attracting negative ions 37. During the formation of a chemical bond between two hydrogen atoms, which of the following statements is always true? A) Energy is released during the formation of the bond. B) A polar covalent bond is formed. C) Electrons always are between the nuclei of the atoms. D) One of the hydrogen atoms is ionized. E) Resonance stabilizes the bond. 38. An atom of which of the following elements has the highest electronegativity? A) K B) As C) Ba D) Si E) Br 39. The concept of resonance describes molecular structures A) that have several different geometric arrangements. B) that have delocalized bonding. C) that are formed from hybridized orbitals. D) that have different molecular formulas. E) that have electrons resonating. 40. All the following statements about resonance are true except A) A single Lewis formula does not provide an adequate representation of the bonding. B) Resonance describes a more stable situation than does any one contributing resonance formula. C) Resonance describes the oscillation and vibration of electrons. D) The contributing resonance formulas differ only in the arrangement of the electrons. E) Resonance describes the bonding as intermediate between the contributing resonance formulas. 41. Which one of the following species is best described by writing three equivalent Lewis formulas? A) SO 3 B) SF 4 C) SO 4 2 D) SO 3 2 E) SOF 4 42. For each of the following species except, the electronic structure may be adequately described by two resonance formulas.
A) O 3 B) SO 3 2 C) NO 2 D) C 6 H 6 E) SO 2 43. Which of the following are two appropriate resonance formulas for the acetate ion, CH 3 CO 2? A) B) C) D) E) 44. The Lewis formula of which species does not represent an exception to the octet rule? A) SiF 5 - B) SCl 6 C) SF 4
D) BF 3 E) CF 3-45. Which of the following has an incomplete octet in its Lewis structure? A) SO 2 B) F 2 C) NO 2 D) ICl E) CO 2 46. Which of the following Lewis structures best describes BF 3? A) B) C) D) E) 47. As the number of bonds between two carbon atoms increases, which of the following decrease(s)? A) only the bond length B) only the bond energy C) only the number of electrons between the carbon atoms D) all of these E) none of these 48. Which of the following species has the shortest bond distance? A) F 2 B) Cl 2 C) Br 2 D) I 2 E) H 2 49. Consider the reaction 2HCl(g) H 2 (g) + Cl 2 (g); DH = 185 kj
Which of the following statements is false? A) The reaction is endothermic. B) HCl(g) has a negative enthalpy of formation. C) The products have more enthalpy than the reactants. D) The HCl bond is longer than either the H 2 bond or the Cl 2 bond. E) The bond order of each of the products is one. 50. Using bond-energy data, what is DH for the following reaction? CH 4 (g) + 2Cl 2 (g) CCl 4 (g) + 2H 2 (g) Bond Bond Energy (kj/mol) C-H 413 H-H 432 Cl-Cl 242 C-Cl 328 A) 40 kj B) 150 kj C) 40 kj D) 1415 kj E) 150 kj
PX0311-0709 Answer Section 1. ANS: A PTS: 1 DIF: easy REF: 7.1 OBJ: Relate the wavelength, frequency, and speed of light. (Examples 7.1 and 7.2) TOP: atomic theory light KEY: electromagnetic radiation 2. ANS: B PTS: 1 DIF: difficult REF: 7.2 OBJ: Describe the photoelectric effect. TOP: atomic theory light KEY: quantum effects and photons photoelectric effect 3. ANS: A PTS: 1 DIF: easy REF: 7.3 OBJ: State the postulates of Bohr's theory of the hydrogen atom. TOP: atomic theory light KEY: Bohr theory Bohr's postulates 4. ANS: A PTS: 1 DIF: easy REF: 7.3 OBJ: Relate the energy of a photon to the associated energy levels of an atom. TOP: atomic theory light 5. ANS: E PTS: 1 DIF: easy REF: 7.4 OBJ: Define Quantum mechanics. TOP: atomic theory quantum mechanics 6. ANS: E PTS: 1 DIF: moderate REF: 7.4 OBJ: State Heisenberg's uncertainty principle. TOP: atomic theory quantum mechanics KEY: wave functions Heisenberg's uncertainty principle 7. ANS: A PTS: 1 DIF: easy REF: 7.5 OBJ: Apply the rules for quantum numbers. (Example 7.6) TOP: atomic theory quantum mechanics KEY: quantum numbers 8. ANS: A PTS: 1 DIF: easy REF: 7.5 OBJ: Describe the shapes of s, p, and d orbitals. TOP: atomic theory quantum mechanics 9. ANS: E PTS: 1 DIF: easy REF: 8.2 OBJ: Define building-up principle. TOP: atomic theory electronic structure of atoms KEY: electron configuration aufbau principle 10. ANS: C PTS: 1 DIF: moderate REF: 8.2 OBJ: Define building-up principle. TOP: atomic theory electronic structure of atoms KEY: electron configuration aufbau principle 11. ANS: C PTS: 1 DIF: easy REF: 8.2 OBJ: Define main-group element and (d-block and f-block) transition element. TOP: atomic theory electronic structure of atoms KEY: electron configuration and the periodic table 12. ANS: E PTS: 1 DIF: moderate REF: 8.2 OBJ: Define main-group element and (d-block and f-block) transition element. TOP: atomic theory electronic structure of atoms KEY: electron configuration and the periodic table 13. ANS: B PTS: 1 DIF: difficult REF: 8.3
OBJ: Determine the configuration of an atom using the building-up principle. (Example 8.2) TOP: atomic theory electronic structure of atoms KEY: electron configuration and the periodic table writing electron configurations using the periodic table 14. ANS: A PTS: 1 DIF: easy REF: 8.3 OBJ: Determine the configuration of an atom using the period and group numbers. (Example 8.3) TOP: atomic theory electronic structure of atoms 15. ANS: E PTS: 1 DIF: easy REF: 8.4 OBJ: Define paramagnetic substance and diamagnetic substance. TOP: atomic theory electronic structure of atoms KEY: electron configuration magnetic properties of atoms 16. ANS: A PTS: 1 DIF: easy REF: 8.4 OBJ: Define paramagnetic substance and diamagnetic substance. TOP: atomic theory electronic structure of atoms KEY: electron configuration magnetic properties of atoms 17. ANS: A PTS: 1 DIF: easy REF: 8.4 OBJ: Define paramagnetic substance and diamagnetic substance. TOP: atomic theory electronic structure of atoms 18. ANS: E PTS: 1 DIF: easy REF: 8.6 OBJ: State the periodic law. KEY: periodicity in main group elements group VA elements 19. ANS: A PTS: 1 DIF: easy REF: 8.6 OBJ: State the general periodic trends in size of atomic radii. KEY: periodic properties atomic radius 20. ANS: C PTS: 1 DIF: easy REF: 8.6 OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5) KEY: periodic properties atomic radius 21. ANS: B PTS: 1 DIF: moderate REF: 8.6 OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5) KEY: periodic properties atomic radius 22. ANS: D PTS: 1 DIF: difficult REF: 8.6 OBJ: State the general periodic trends in ionization energy. KEY: periodic properties ionization energy 23. ANS: B PTS: 1 DIF: easy REF: 8.6 OBJ: Determine relative ionization energies from periodic trends. (Example 8.6) KEY: periodic properties ionization energy 24. ANS: B PTS: 1 DIF: easy REF: 8.6 OBJ: Define electron affinity. KEY: periodic properties electron affinity
25. ANS: A PTS: 1 DIF: easy REF: 8.7 OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going through any main group of elements. KEY: periodicity in main group elements group IIIA elements 26. ANS: E PTS: 1 DIF: easy REF: 8.7 OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going through any main group of elements. KEY: periodicity in main group elements group IIIA elements 27. ANS: D PTS: 1 DIF: moderate REF: 8.7 OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going through any main group of elements. KEY: periodicity in main group elements group VA elements 28. ANS: D PTS: 1 DIF: difficult REF: 9.1 OBJ: Describe the energetics of ionic bonding. TOP: bonding ionic bonding KEY: properties of ionic substance 29. ANS: B PTS: 1 DIF: moderate REF: 9.1 OBJ: Define lattice energy. TOP: bonding ionic bonding KEY: Born-Haber cycle 30. ANS: B PTS: 1 DIF: easy REF: 9.1 OBJ: Describe some general properties of ionic substances. TOP: bonding ionic bonding KEY: properties of ionic substance 31. ANS: E PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) TOP: bonding ionic bonding KEY: Lewis electron-dot symbol 32. ANS: A PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) TOP: bonding ionic bonding KEY: electron configurations of ions ions of the main-group elements 33. ANS: C PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. TOP: bonding ionic bonding 34. ANS: A PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. TOP: bonding ionic bonding 35. ANS: C PTS: 1 DIF: moderate REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4) TOP: bonding ionic bonding KEY: ionic radii 36. ANS: A PTS: 1 DIF: moderate REF: 9.4 OBJ: Describe the formation of a covalent bond between two atoms. TOP: bonding covalent bonding 37. ANS: A PTS: 1 DIF: moderate REF: 9.4 OBJ: Describe the formation of a covalent bond between two atoms. TOP: bonding covalent bonding
38. ANS: E PTS: 1 DIF: easy REF: 9.5 OBJ: State the general periodic trends in the electronegativity. TOP: bonding covalent bonding KEY: electronegativity 39. ANS: B PTS: 1 DIF: easy REF: 9.7 OBJ: Define resonance description. TOP: bonding covalent bonding KEY: resonance 40. ANS: C PTS: 1 DIF: easy REF: 9.7 OBJ: Define resonance description. TOP: bonding covalent bonding KEY: resonance 41. ANS: A PTS: 1 DIF: difficult REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 42. ANS: B PTS: 1 DIF: easy REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 43. ANS: A PTS: 1 DIF: easy REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 44. ANS: E PTS: 1 DIF: easy REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding 45. ANS: C PTS: 1 DIF: moderate REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding 46. ANS: C PTS: 1 DIF: easy REF: 9.8 OBJ: Note exceptions to the octet rule in Groups IIA and Group IIIA elements. TOP: bonding covalent bonding KEY: exceptions to the octet rule 47. ANS: A PTS: 1 DIF: easy REF: 9.10 OBJ: Explain how bond order and bond length are related. (Example 9.12) TOP: bonding covalent bonding KEY: bond length 48. ANS: E PTS: 1 DIF: moderate REF: 9.10 OBJ: Explain how bond order and bond length are related. (Example 9.12) TOP: bonding covalent bonding KEY: bond length 49. ANS: D PTS: 1 DIF: easy REF: 9.11 OBJ: Define bond energy. TOP: bonding covalent bonding KEY: bond energy 50. ANS: A PTS: 1 DIF: easy REF: 9.11 OBJ: Estimate delta H from bond energies. (Example 9.13) TOP: bonding covalent bonding KEY: bond energy