Quiz #1 Fall 2010
DEPARTMENT OF MINING AND MATERIALS ENGINEERING
MIME 261 – Structure of materials Quiz n.1 – October 4th, 2011 – version C Duration of the test: 35 min Examiner: Marta Cerruti Instructions 1. This is a closed book test. 2. You can consult only the periodic table provided along with this quiz. 3. Write your answers on the question paper. 4. There is only one correct answer for each multiple‐choice question. 5. Each question counts for one point unless otherwise specified. The total is 29 points. 6. The grade from this quiz counts for 10% of your course grade.
Family name ____________________________________________________ (Please print)
Given name(s) ___________________________________________ (Please print)
Student ID __________________________________________________ 1
2
1. Give three examples of molecular solids. 2. How many d orbitals are there? a. 1 b. 3 c. 7 d. 5 3. The energy of the 1s orbital in Li is a. Incomparable with the energy of the 1s orbital in H b. Lower (more negative) than the 1s orbital in H c. Same as the 1s orbital in H d. Higher (more positive) than the 1s orbital in H 4. What are the two strongest types of weak bonds? 5. What kinds of bonds hold a crystal of CaCO3 together? 6. In a semiconductor like Ge: a. No band structure is observed b. Bonding and antibonding bands are not separate, rather form a continuous band c. We can distinguish a bonding and an antibonding band separated by a small energy gap d. We can distinguish a bonding and an antibonding band separated by a large energy gap 7. Energy bands are obtained when a. Many metallic elements interact b. Many heavy elements interact c. Many light elements interact d. Many atomic orbitals interact 3
8. Metallic bonds a. Permit easy electron transfer b. Are maintained at the liquid state c. Act between both identical and different atoms d. All of the above 9. The quantum number ml is related to a. The energy of the orbital b. The spin of an electron in the orbital c. The shape of the orbital d. The orientation of the orbital 10. What is the most common ion formed by Rb? 11. Why is the boiling point of propane higher than that of methane? 12. An anti‐bonding molecular orbital has energy a. Equal to the atomic orbitals that combine to form it b. Lower than the atomic orbitals that combine to form it c. Higher than the atomic orbitals that combine to form it d. Incomparable with that of the atomic orbitals that combine to form it 13. The electron density in a molecular orbital is a. Concentrated on the largest one of the nuclei involved b. Concentrated between the nuclei involved c. Concentrated above and below the plane containing the nuclei involved d. Concentrated on both of the nuclei involved 3 14. sp orbitals are a. Hybrid atomic orbitals arranged in a tetrahedral geometry b. Hybrid molecular orbitals arranged in a tetrahedral geometry c. Hybrid atomic orbitals arranged in a square planar geometry d. Hybrid molecular orbitals arranged in a square planar geometry 15. How many valence electrons does Br have? a. 1 b. 17 c. 5 d. 7 4
16. What is the hybridization of the C atoms in graphite? 17. Write the electronic configuration for Bi (Z=83) 18. Write the ground state configuration for Ne2 19. Which of the following statements about bonds is true: a. Metallic and covalent bonds are directional, ionic bond is non‐directional b. Ionic and covalent bonds are directional, metallic bond is non‐directional c. Ionic and metallic bonds are non‐directional, covalent bond is directional d. None of the above 20. What geometry do you predict for BeF2? 21. Orbitals with the same principal quantum number n a. Have a different energy for the H atom and the same energy for heavier atoms b. Have the same energy for the H atom but not for heavier atoms c. Have the same energy d. None of the above 22. Band overlap is greater for a. Ions b. Heavier elements c. Lighter elements d. Liquids 23. The energy of the 2p orbital in Li is a. Incomparable with the energy of the 2s orbital in Li b. Higher (more positive) than the energy of the 2s orbital in Li c. Same as the 2s orbital in Li d. Lower (more negative) than the energy of the 2s orbital in Li 5
24. What’s the bond order of Ne2? 25. What are atomic orbitals? a. Wave functions characterized by a specific energy and a set of quantum numbers b. Wave functions related to the probability of finding electrons in specific regions around the nucleus c. Wave functions solutions of Schroedinger’s equation d. All of the above 26. What is the hybridization of the O atom in the water molecule? 27. The bond in O2 can be described as a. One covalent bond b. One covalent bond and two covalent bonds c. One covalent bond and one covalent bond d. One covalent bond and one ionic bond 28. Consider the following electron configuration: ‐‐‐‐‐ ‐‐‐‐‐ ‐‐‐‐‐ 2p ‐‐‐‐‐ 2s ‐‐‐‐‐ 1s a. Which atom has this as its ground electronic configuration? b. What are the four quantum numbers that describe the electron indicated with a star?
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MIME 261 – Structure of materials Quiz n.1 – October 4th, 2011 – version C Duration of the test: 35 min Examiner: Marta Cerruti Instructions 1. This is a closed book test. 2. You can consult only the periodic table provided along with this quiz. 3. Write your answers on the question paper. 4. There is only one correct answer for each multiple‐choice question. 5. Each question counts for one point unless otherwise specified. The total is 29 points. 6. The grade from this quiz counts for 10% of your course grade.
Family name ____________________________________________________ (Please print)
Given name(s) ___________________________________________ (Please print)
Student ID __________________________________________________ 1
2
1. Give three examples of molecular solids. 2. How many d orbitals are there? a. 1 b. 3 c. 7 d. 5 3. The energy of the 1s orbital in Li is a. Incomparable with the energy of the 1s orbital in H b. Lower (more negative) than the 1s orbital in H c. Same as the 1s orbital in H d. Higher (more positive) than the 1s orbital in H 4. What are the two strongest types of weak bonds? 5. What kinds of bonds hold a crystal of CaCO3 together? 6. In a semiconductor like Ge: a. No band structure is observed b. Bonding and antibonding bands are not separate, rather form a continuous band c. We can distinguish a bonding and an antibonding band separated by a small energy gap d. We can distinguish a bonding and an antibonding band separated by a large energy gap 7. Energy bands are obtained when a. Many metallic elements interact b. Many heavy elements interact c. Many light elements interact d. Many atomic orbitals interact 3
8. Metallic bonds a. Permit easy electron transfer b. Are maintained at the liquid state c. Act between both identical and different atoms d. All of the above 9. The quantum number ml is related to a. The energy of the orbital b. The spin of an electron in the orbital c. The shape of the orbital d. The orientation of the orbital 10. What is the most common ion formed by Rb? 11. Why is the boiling point of propane higher than that of methane? 12. An anti‐bonding molecular orbital has energy a. Equal to the atomic orbitals that combine to form it b. Lower than the atomic orbitals that combine to form it c. Higher than the atomic orbitals that combine to form it d. Incomparable with that of the atomic orbitals that combine to form it 13. The electron density in a molecular orbital is a. Concentrated on the largest one of the nuclei involved b. Concentrated between the nuclei involved c. Concentrated above and below the plane containing the nuclei involved d. Concentrated on both of the nuclei involved 3 14. sp orbitals are a. Hybrid atomic orbitals arranged in a tetrahedral geometry b. Hybrid molecular orbitals arranged in a tetrahedral geometry c. Hybrid atomic orbitals arranged in a square planar geometry d. Hybrid molecular orbitals arranged in a square planar geometry 15. How many valence electrons does Br have? a. 1 b. 17 c. 5 d. 7 4
16. What is the hybridization of the C atoms in graphite? 17. Write the electronic configuration for Bi (Z=83) 18. Write the ground state configuration for Ne2 19. Which of the following statements about bonds is true: a. Metallic and covalent bonds are directional, ionic bond is non‐directional b. Ionic and covalent bonds are directional, metallic bond is non‐directional c. Ionic and metallic bonds are non‐directional, covalent bond is directional d. None of the above 20. What geometry do you predict for BeF2? 21. Orbitals with the same principal quantum number n a. Have a different energy for the H atom and the same energy for heavier atoms b. Have the same energy for the H atom but not for heavier atoms c. Have the same energy d. None of the above 22. Band overlap is greater for a. Ions b. Heavier elements c. Lighter elements d. Liquids 23. The energy of the 2p orbital in Li is a. Incomparable with the energy of the 2s orbital in Li b. Higher (more positive) than the energy of the 2s orbital in Li c. Same as the 2s orbital in Li d. Lower (more negative) than the energy of the 2s orbital in Li 5
24. What’s the bond order of Ne2? 25. What are atomic orbitals? a. Wave functions characterized by a specific energy and a set of quantum numbers b. Wave functions related to the probability of finding electrons in specific regions around the nucleus c. Wave functions solutions of Schroedinger’s equation d. All of the above 26. What is the hybridization of the O atom in the water molecule? 27. The bond in O2 can be described as a. One covalent bond b. One covalent bond and two covalent bonds c. One covalent bond and one covalent bond d. One covalent bond and one ionic bond 28. Consider the following electron configuration: ‐‐‐‐‐ ‐‐‐‐‐ ‐‐‐‐‐ 2p ‐‐‐‐‐ 2s ‐‐‐‐‐ 1s a. Which atom has this as its ground electronic configuration? b. What are the four quantum numbers that describe the electron indicated with a star?
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