To answer the following question, draw the Molecular Orbital Energy Diagrams for the diatomic molecules, O2, OF and F2. Which of the following statement is (are) true? (Select all that apply.)
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- Draw the Molecular Orbital Energy Diagrams for the diatomic molecules, O2, OF and F2. Which of the following statement is (are) true? (Select all that apply.) Of these three molecules, O2 has the highest stability None of these statements are true. O2 and OF are paramagnetic and F2 is diamagnetic. Of these three molecules, F2 has the longest bond. The bond order of OF is 1.5. Of these three molecules, F2 has the highest bond order.Draw the Molecular Orbital Energy Diagram for the diatomic molecule, CO. Which of the following statement is (are) true? (Select all that apply.) The highest energy molecular orbital that contains electrons is T2p. The bond order is 3. None of these statements are true. CO is paramagnetic. The lowest energy molecular orbital that contains no electrons is T*20. CO is diamagnetic. The bond order is 2.Which of the following statements are TRUE for covalent pi bonds? (Choose as many as apply. Hint: There are 4 correct answers!) Pi bonds arise from head-on overlap of two orbitals. Pi bonds arise from sideways overlap of two orbitals. The electron density in a pi bond is found above and below the axis between the two bonded nuclei. The electron density in a pi bond is found in between the two bonded nuclei. A pi bond can exist independently; not every pi bond is accompanied by an associated o bond. Pi bonds always exist in conjunction with an associated o bond; they can never exist independently. The pi bonds in a molecule determine the shape of the molecule. There can be more than one pi bond between two nuclei. Every covalent bond contains at least one pi bond.
- Consider a molecule AB, where element A has 6 valence electrons and B has 7 valence electrons. If the AEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity.Consider the ring cation, called "cyclopentadienyl cation".... one of five possible resonance structures that can be drawn for it is shown below. In the actual ring cation, what is the charge on any one carbon atom, and what is the bond order of any one C,C bond? 4? charge on one C = ? bond order of C,C bond ? Select one: O A. +2/5; 4/3 OB. + 1/6; 1.5 O C. + 2/5; 7/5 OD. + 1/5; 6/5 O E. + 1/5; 7/5Describe the orbitals that are mixing to make the bond that the thicker arrow is pointing to. (formatting is shown for the C:O double bond pointed to by the thinner arrow)
- Question 2: The hypofluoride ion, OF', can be observed with difficulty. a) Prepare a molecular orbital energy level diagram for this ion. b) What is the bond order, and how many unpaired electrons are in this ion?Look at the Lewis structure below and determine the bond angle (See Table at end of problem). What are the bond angles at position 1 and 2 What is the hybridization for the central atom at positions 1 and 2 H. Look at the Lewis structure below. What is the bond angle at position 1 hybridization for the central atom at positions 1 and 2 ? What is the and 2 H 2 and 2 ? What is the Look at the Lewis structure below. What is the bond angle at position 1 hybridization for the central atom at positions 1 and 2 H. 1 ... ... H. .. 2 The possibilities for bond angle and hybridization are given in this table. Bond Angles < 90 90 <109.5 109.5 <120 120 180 Hybridization sp sp² sp³ sp³d sp³d²Indicate whether each statement is true or false. (a) s orbitalscan only make s or s* molecular orbitals. (b) The probabilityis 100% for finding an electron at the nucleus in a p* orbital.(c) Antibonding orbitals are higher in energy than bondingorbitals (if all orbitals are created from the same atomic orbitals).(d) Electrons cannot occupy an antibonding orbital.
- | Constants | Periodic Submit Previous Answers v Correct The highest energy electron is in an antibonding orbital for Lig Part C Use the MO diagrams to calculate the bond order for Lig+ and Lig Express the bond order for Liz+ followed by the bond order for Li2 separated by a comma. V ΑΣφ ? bondJorder for Lig+, Li2 = Your submission doesn't have the correct number of answers. Answers should be separated with a comma. No credit lost. Try again. Submit Previous Answers Request Answer Part D Which do you expect to exist in the gas phase. P Pearson 21 Pearson Education Inc. All rights reserved. Terms of Use l Privacy Policy Permissions| Contact Us | 5:29 PM 61% 84°F Sunny 11/13/20 Home End Insert Delete F10 F11 F12 Backspace NumLocka) Draw the molecular orbital diagram of the given compounds, predict the bond order, and une comment on whether the molecule can exist or not. F₂ Be₂ b) Is CN¯diamagnetic or paramagnetic? c) Would you expect the bond in CN to be stronger or weaker than in the F₂ molecule? why? CN "harks People Tab Window Help nd Tap Cengage Learning Use The Molecular OrbitalEne: X + evo/index.html?deploymentld%3D55750828934189288909969212&elSBN=97813056... INDTAP Use the References to access important values if needed for this question. What atomic or hybrid orbitals make up the T bond between C, and C, in propyne, CHCCH3? (C, is the first carbon in the formula as written.) orbital on C+ orbital on C2 How many o bonds does C, have in CHCCH3? How many TI bonds does C, have?