Unit 1 Practice Exam 2 PDF

CH301 NAME: ______________________________________________ Unit 1 Practice Exam 2 1. Periodic Table Which of the following statements is true about group names in the periodic table? a) Group I is the alkaline earth met...

CH301 NAME: ______________________________________________ Unit 1 Practice Exam 2 1. Periodic Table Which of the following statements is true about group names in the periodic table? a) Group I is the alkaline earth metals b) Group III is the halogens c) Group VIII is the noble gases d) Group VII is the alkali metals 2. Quantum Mechanics Application – H Atom The size of an atomic orbital is determined by which quantum number? a) ml b) l c) ms d) n 3. Quantum number applications – _H atom Which of the following descriptions of a quantum number is correct? I. The quantum number, n, is a shell and defines the energy and distance from the nucleus of an electron II. The quantum number, l, is a subshell and defines the shape of an orbital III. The quantum number, ml, is an orbital and defines the orientation of the orbital a) I only b) I and II only c) I, II and III d) II and III only CH301 | 1  CH301 NAME: ______________________________________________ 4. Quantum numbers boundary conditions In an atom, what would be the maximum number of electrons having the quantum numbers n = 3 , l = 2 and ms = -1/2 a) 18 b) 10 c) 5 d) 0 5. Quantum numbers boundary conditions Which set of quantum numbers does NOT provide a satisfactory solution to the wave equation? a) n = 2, l = 0, ml = -1 b) n = 1, l = 0, ml = 0 c) n = 4, l = 2, ml = +2 d) n = 5, l = 3, ml = -3 6. Quantum numbers and periodic table Which of the following statements about the alkali metals is NOT true? a) They readily form singly charged cations b) Flame tests produce photons in the visible region of the electromagnetic spectrum. c) They have a single valence electron d) Hydrogen is an alkali metal 7. Aufbau, Hund & Pauli Theory One of the following does NOT represent the ground state electron configuration for an atom. Which one? a) [Ne] 3s2 3p5 b) [Ne] 3s1 3p3 c) [Ne] 3s1 d) [Ne] 3s2 CH301 | 2  CH301 NAME: ______________________________________________ 8. Aufbau, Hund & Pauli Theory Pauli’s rule is the reason: a) There are a maximum of two electrons in an orbital b) Electrons do not pair in subshells until all orbitals have at least one electron c) That electrons can behave as particles and waves d) None of the above. 9. Electron Configurations of atoms: no exceptions Which of the following atoms has an s2p3 valence electron configuration? a) Ga b) Ge c) As d) Se 10. Electron Configurations of atoms: no exceptions Which of the following is the valence electronic structure for a halogen? a) ns2 np5 b) ns1 c) ns2 np6 d) ns2 nd10 11. Electron configurations of ions: no exceptions How many electrons are in the 4s orbital of a Ca2+ ion? a) 0 b) 2 c) -2 d) 3 12. Electron Configurations and magnetism Based on electronic configurations, which of the following species would you predict to be most magnetic? a) Sc b) Ti c) V d) Mn CH301 | 3  CH301 NAME: ______________________________________________ 13. Periodicity theory: effective nuclear charge & shielding What is the effective nuclear charge of a valence electron in the Al+ cation? a) 2 b) 3 c) 12 d) 13 14. Periodicity theory: effective nuclear charge & shielding As you move down a family on the periodic table, the increase in atomic radius can be explained by the ______. a) increase in number of shielding electrons b) increase in effective nuclear charge c) decrease in number of shielding electrons d) decrease in effective nuclear charge 15. Ranking periodic trends without exceptions, atomic radius Rank the following atoms in terms of decreasing atomic radius. a) Na, N, O, Mg, F b) F, O, N, Na, Mg c) Na, Mg, N, O, F d) F, Mg, Na, O, N 16. Ranking periodic trends without exceptions, ionic radius Rank the following atoms and ions in order of decreasing size: Li+, Be2+, He, H-, B3+ a) H-, Li+, He, Be2+, B3+ b) B3+, Be2+, He, Li+, H- c) B3+, Be2+, Li+, He, H- d) H-, He, Li+, Be2+, B3+ CH301 | 4  CH301 NAME: ______________________________________________ 17. Ranking periodic trends, exceptions, 1st ionization energy The ionization energy of an Oxygen atom (O) is (equal to/greater than/less than) what you would predict based on simple effective nuclear charge arguments because the half-filled 2p orbital for O+ is (more/less) stable. a) equal to; less b) less than; more c) greater than; less d) less than; less 18. Ranking periodic trends, exceptions, 1st ionization energy Rank the following from least to greatest ionization energy: silicon (Si), phosphorous (P), sulfur (S). a) P < S < Si b) Si < P < S c) S < Si < P d) Si < S < P 19. Ranking electronegativity What is the difference in electronegativity between C and O atoms? a) 0.5 b) 1.0 c) 1.5 d) 0.4 20. Ranking electronegativity What is the correct order of increasing electronegativity for N, O, P, and K? a) P, K, N, O b) K, O, N, P c) K, P, N, O d) O, N, P, K CH301 | 5