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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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In PBr3, Indicate which atoms in the species need what hybrid orbitals in order to explain the bonding in the molecule or ion.
Also, Describe each of the bonds in the species: (There is a ___ bond between the ___ atom and the ___ atom formed by the overlap of a ____ orbital on the ____ atom and the ___ orbital on the ____ atom)
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- Draw the molecular orbital (MO) electron diagram for the Be₂ molecule. Be sure your diagram contains all of the electrons in the molecule, including any core electrons. Energy X 1 Ś |arrow_forward10. Consider the peroxide ion, O22. Draw the molecular orbital diagram. Be sure to label your orbitals. Calculate the bond order. Is the peroxide ion attracted to magnetic fields or repulsed by magnetic fields? Briefly explain why or why not.arrow_forwardExplain a covalent bond involving four electrons between two atoms using quantum mechanics and valance bond theory. Group of answer choices Direct unhybridized s, p, or d electron overlap results in a sigma bond and hybridized indirect p electron overlap results in a pi bond. Direct unhybridized s, p, or d electron overlap results in a pi bond and hybridized indirect p electron overlap results in a sigma bond. Direct hybridized s, p, or d electron overlap results in a sigma bond and unhybridized indirect p electron overlap results in a pi bond. Direct s, p, or d electron overlap results in two unhybridized sigma bonds. Direct s, p, or d electron overlap results in two hybridized sigma bonds. Direct hybridized s, p, or d electron overlap results in a pi bond and unhybridized indirect p electron overlap results in a sigma bond.arrow_forward
- The molecular orbital (MO) diagram of OF is given below. Answer Questions 15 - 18. 2p. 2, 2e, OF F 15. How many electrons are in the two degenerate molecular orbitals (MOs)? A. There are three electrons with one MO being doubly occupied and the other singly occupied. B. There are two electrons with each MO being singly occupied. C. There are two electrons that occupy one of the two MOs. D. There are four electrons that occupy both * MOS. E. There is only one electron that occupies one of the two MOS. 16. What is the bond order? A. 0.5 B. 1.0 C. 1.5 D. 2.0 E. 2.5 17. The HOM0 is C. O D. E. 18. The LUMO is B. C. , D. E. .arrow_forwardIn SeO2, Indicate which atoms in the species need what hybrid orbitals in order to explain the bonding in the molecule or ion. Describe each of the bonds in the species: (There is a ___ bond between the ___ atom and the ___ atom formed by the overlap of a ____ orbital on the ____ atom and the ___ orbital on the ____ atom)arrow_forwardAccording to molecular orbital theory, in the O2* ion, how many valence electrons are in antibonding molecular orbitals? 4arrow_forward
- According to the molecular orbital theory, what is the bond order in F2? O 0.5 O 1.5 00 01 O 2 « Previousarrow_forwardPlease answer question 20 Part A, B, and Carrow_forwardWhich of the following factors contribute to the tetrahedral shape of the above molecule? Group of answer choices A. the shape of the two p orbitals in the carbon atom B. the shape of the one s orbital in the carbon atom C. the shape of the sp3 hybrid orbitals of the electrons shared between the carbon and hydrogen atoms D. hydrogen bonding configurations between the carbon and hydrogen atomsarrow_forward
- 2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew. b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.arrow_forward6. Consider the molecule sulfur dioxide. Draw the Lewis structure such that it follows the octet rule. Include any formal charges. What is the electron geometry? What is the molecular shape? What are the expected bond angles? What kind of intermolecular forces does it have? How many sigma bonds are there? How many pi bonds? What is the hybridization of the sulfur atom? In the space below, sketch the hybridized orbitals.arrow_forward
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