Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED

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1 CHM-201 General Chemistry and Laboratory I Unit #4 Take Home Test Due December 13, 2018 Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED

3 CHM-201 General Chemistry and Laboratory I Unit #4 Take Home Test Due December 13, 2018 Directions: Complete this test and pass in the answer sheet portion on or before the due date. Please pass in ONLY the answer sheet. On the answer sheet, be sure to enter your student ID and fill in the appropriate bubbles. Record your answers unambiguously ambiguous answers are wrong. Do not cross out answers either erase/cover them completely or print a new answer sheet. Absolutely no papers will be accepted after the due date. 1. Which statement about the quantum numbers that identify an atomic orbital is not correct? a. The angular momentum quantum number,, identifies the shape of an orbital. b. The value of the angular momentum quantum number can range from 0 to n, where n is the principal quantum number for the orbital. c. Orbitals with the same value for the principal quantum number and the angular momentum quantum number are said to be in the same subshell. d. Orbitals with the same values for the principal quantum number and the angular momentum quantum number have the same energy. e. The value for the angular momentum quantum number also is designated by a letter: s = 0, p = 1, d = 2, f = 3, and so on. 2. Which subshell contains six total electrons? a. 2 d. 3 b. 1 e. 4 c A certain shell is known to have a total of 16 orbitals. Which shell is it? a. n 4 c. n 8 b. n 16 d. n 2 4. Which of the following is not an allowed value for the principal quantum number? a. 1 d. 0 b. 3 e. 2 c Which listing has the orbitals in order of increasing energy in a multielectron atom? a. 3s 3p 4s 3d 4p d. 3s 3p x 3p y 3p z b. 3s 3p 3d 4s 4p e. 2s 3s 2p 3d c. 3s 4s 3p 4p 3d 6. What is the ground state electron configuration for fluorine? a. 1s 2 2s 2 2p 5 d. [Ne]3s 2 3p 5 b. 1s 2 2s 2 2p 6 3s 2 3p 5 e. 1s 2 2s 2 2p 4 c. [He]2s 2 2p 6

4 7. Which one of the following diagrams violates the Aufbau Principle? a. c. b. d. 8. What is the ground-state electron configuration of an Ni 2+ ion? a. [Ar]3d 8 4s 2 d. [Ar]3d 10 4s 2 b. [Ar]3d 6 4s 2 e. [Ar]3d 10 c. [Ar]3d 8 9. Which one of these atoms or ions has the most unpaired electrons in its ground state? a. Sc d. S b. Sc 3+ e. P c. K 10. Which of the following electron configurations represents an excited state? a. [Ne]3s 2 3p 5 d. [Ne]3s 2 3p 6 4s 2 b. [Kr]4d 10 5s 2 5p 1 e. [Kr]4d 10 5s 1 5p 1 c. [Ar]3d 10 4s 2 4p Down a column in the periodic table, the ionization energy a. increases because the n quantum number changes. b. increases because the quantum number changes. c. decreases because the outer electrons are further from the nucleus. d. increases because the atomic number (nuclear charge) increases. e. changes little because the outer electrons are all in the same outer shell. 12. Which of the following is most likely a polar covalent bond? a. Na Cl d. K F b. H H e. Ca O c. C N

5 13. How many valence electrons does F have? a. 5 d. 9 b. 7 e. 19 c Which of the following has 13 valence electrons? a. SH d. ICl b. IO e. Cl 2 c. NO 15. Triple bonds a. involve sharing of 3 total electrons between atoms. b. involve sharing of 6 total electrons between atoms. c. always occur between 2 metal atoms. d. occur only between atoms with 3 valence electrons. e. typically occur between hydrogen and another atom. 16. Which of the following properties is typically used to identify whether a bond is polar, nonpolar, or ionic? a. electronegativity d. electron affinity b. ionization energy e. atomic mass c. atomic radius 17. Which of the following bonds is most polar? a. H O d. H C b. H N e. H F c. H B 18. Nitrite (NO 2 ) is an important nutrient in the eutrophic zone of the ocean. Which of the following is the correct set of resonance structures for this ion? a. I c. III b. II d. IV

6 19. Which of these statements correctly describes the use of formal charge in choosing between possible Lewis structures to describe a molecule? I. Formal charge on all the atoms should be zero, or at least the smallest possible value. II. The sum of the formal charges on all the atoms should equal the charge on the molecule or ion. III. The formal charge on an atom is not affected by the electronegativity of the atom. IV. In an anion containing nitrogen and oxygen, the Lewis structures with a negative charge on the nitrogen will contribute the most to the description of the bonding. a. I and II only d. I and III only b. II and III only e. II and IV only c. III and IV only 20. Which of the following compounds would have the largest enthalpy of formation? The bond energies are given in parentheses. a. H Br (366 kj/mol) d. H F (567 kj/mol) b. H I (299 kj/mol) e. H H (436 kj/mol) c. H Cl (431 kj/mol) 21. In VSEPR theory, molecular geometry is determined by a. electron proton attractive forces. b. electron electron attractive forces. c. electron electron repulsive forces. d. proton proton repulsive forces. e. electron nucleus attractive forces. 22. Which electron-pair geometry corresponds to a steric number of 3? a. linear d. trigonal bipyramidal b. trigonal planar e. octahedral c. tetrahedral 23. Which of the following molecules or ions has a linear molecular geometry? a. H 2O d. I 3 b. H 2S e. SO 2 c. ICl Which of the following molecules or ions is not polar? a. BF 3 d. NH 3 b. CHCl 3 e. SF 4 c. H 2CO 25. What is the hybridization of the oxygen in the H 3O + ion? a. sp 2 d. sp b. sp 3 e. sp 3 d 2 c. sp 3 d

General Chemistry 1 CHM201 Unit 4 Practice Test. 4. What is the orbital designation for an electron with the quantum numbers n 4, 3?

General Chemistry 1 CHM201 Unit 4 Practice Test 1. An orbital s orientation in space is determined by a. the quantum number. d. the n quantum number. b. the m l quantum number. e. both the and m l quantum