Chemistry: Structure and Properties
1st Edition
ISBN: 9780321834683
Author: Nivaldo J. Tro
Publisher: PEARSON
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Chapter 7, Problem 85E
Interpretation Introduction
To determine:
Definition of the major bonding theories for single, double and triple bonds
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18. Explain with the help of partial molecular orbitals the difference between an acceptor
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(b)
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Chapter 7 Solutions
Chemistry: Structure and Properties
Ch. 7 - Determine the hybridization about 0 in CH3OH.Ch. 7 - Determine the hybridization about C in H2CO.Ch. 7 - According to the valance bond theory, which kind...Ch. 7 - Use molecular orbital theory to determine the bond...Ch. 7 - Use molecular orbital theory to predict which...Ch. 7 - Use molecular orbital theory to determine which...Ch. 7 - Which hybridization scheme occurs about nitrogen...Ch. 7 - Prob. 8SAQCh. 7 - Prob. 9SAQCh. 7 - Prob. 10SAQ
Ch. 7 - Which type of orbitals overlap to form the sigma...Ch. 7 - Prob. 12SAQCh. 7 - Prob. 1ECh. 7 - What is a chemical bond according to valence bond...Ch. 7 - In valence bond theory, what determines the...Ch. 7 - In valence bond theory, the interaction energy...Ch. 7 - What is hybridization? Why is hybridization...Ch. 7 - How does hybridization of the atomic orbitals in...Ch. 7 - How is the number of hybrid orbitals related to...Ch. 7 - Sketch each hybrid orbital sp sp2 sp3 sp3d sp3d2Ch. 7 - Prob. 9ECh. 7 - Name the hybridization scheme that corresponds to...Ch. 7 - What is a chemical bond according to molecular...Ch. 7 - Explain the difference between hybrid atomic...Ch. 7 - What is a bonding molecular orbital?Ch. 7 - Prob. 14ECh. 7 - What is the role of wave interference in...Ch. 7 - Prob. 16ECh. 7 - Prob. 17ECh. 7 - Prob. 18ECh. 7 - Prob. 19ECh. 7 - Prob. 20ECh. 7 - Prob. 21ECh. 7 - When applying molecular orbital theory to...Ch. 7 - In molecular orbital theory, what is a nonbonding...Ch. 7 - Write a short paragraph describing chemical...Ch. 7 - Prob. 25ECh. 7 - Prob. 26ECh. 7 - Prob. 27ECh. 7 - Prob. 28ECh. 7 - Prob. 29ECh. 7 - Prob. 30ECh. 7 - The valence electron configurations of several...Ch. 7 - The valence electron configurations of several...Ch. 7 - Draw orbital diagrams (boxes with arrows in them)...Ch. 7 - Draw orbital diagrams (boxes with arrows in them)...Ch. 7 - Prob. 35ECh. 7 - Draw orbital diagrams (boxes with arrows in them)...Ch. 7 - Which hybridization scheme allows the formation of...Ch. 7 - Which hybridization scheme allows the central atom...Ch. 7 - Write a hybridization and bonding scheme for each...Ch. 7 - Write a hybridization and bonding scheme for each...Ch. 7 - Write a hybridization and bonding scheme for each...Ch. 7 - Write a hybridization and bonding scheme for each...Ch. 7 - Write a hybridization and bonding scheme for each...Ch. 7 - Write a hybridization and bonding scheme for each...Ch. 7 - Consider the structure of the amino acid alanine...Ch. 7 - Consider the structure of the amino acid aspartic...Ch. 7 - Sketch the bonding molecular orbital that results...Ch. 7 - Sketch the antibonding molecular orbital that...Ch. 7 - Draw an MO energy diagram and predict the bond...Ch. 7 - Draw an MO energy diagram and predict the bond...Ch. 7 - Sketch the bonding and antibonding molecular...Ch. 7 - Sketch the bonding and antibonding molecular...Ch. 7 - Using the molecular orbital energy ordenng for...Ch. 7 - Using the molecular orbital energy ordering for...Ch. 7 - Apply molecular orbital theory to predict if each...Ch. 7 - Apply molecular orbital theory to predict if each...Ch. 7 - According to MO theory, which molecule or ion has...Ch. 7 - According to MO theory, which molecule or ion has...Ch. 7 - Draw an MO energy diagram for CO. (Use the energy...Ch. 7 - Draw an MO energy diagram for HCI. Predict the...Ch. 7 - Prob. 61ECh. 7 - Prob. 62ECh. 7 - Prob. 63ECh. 7 - Prob. 64ECh. 7 - Prob. 65ECh. 7 - Prob. 66ECh. 7 - For each compound, draw the Lewis structure,...Ch. 7 - For each compound, draw the Lewis structure,...Ch. 7 - Amino acids are biological compounds that link...Ch. 7 - The genetic code is based on four different bases...Ch. 7 - The structure of caffeine, present in coffee and...Ch. 7 - The structure of acetylsalicylic acid (aspirin) is...Ch. 7 - Draw a molecular orbital energy diagram for CIF....Ch. 7 - Draw Lewis structures and MO diagrams for CN+, CN,...Ch. 7 - Bromine can form compounds or ions with any number...Ch. 7 - The compound C3H4 has two double bonds. Describe...Ch. 7 - How many hybrid orbitals do we use to describe...Ch. 7 - Prob. 78ECh. 7 - In VSEPR theory, which uses the Lewis model to...Ch. 7 - The resuts of a molecular orbital calculation for...Ch. 7 - Prob. 81ECh. 7 - cis-2-Butene isomerizes (changes its structure) to...Ch. 7 - The ion CH5 + can form under very special...Ch. 7 - Neither the VSEPR model nor the hybridization...Ch. 7 - Prob. 85ECh. 7 - The most stable forms of the nonmetals in groups...Ch. 7 - Consider the bond energies of three iodine...Ch. 7 - How many atomic orbitals form a set of sp3hybrid...
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- Calculate the atomic packing factor of quartz, knowing that the number of Si atoms per cm3 is 2.66x1022 and that the atomic radii of Si and O are 0.038 and 0.117 nm.arrow_forwardChoose one or more: Draw the Lewis structure. Consider and draw alternate resonance structures. Calculate the molar mass of the compound. Leave out the lone pairs of electrons. Complete the octets of each atom (dublet for H). Determine the central atom, if possible. Determine the number of covalent bonds in the structure. Check the structure with electron bookkeeping Question: Determine which of the following procedures are steps in drawing the resonance structures of pyridine and pyrazine. Check all that apply.arrow_forward1. Draw the shapes of the various d orbitals and explain why they are split into two groups; 12g and eg in an octahedral field Draw a diagram to show how the d orbitals are split into groups with different energy in an octahedral field. Some electronic configurations may exist in both high spin and low spin arrangements in an octahedral field. Draw all of these cases, and suggest which metal ions and which ligands might give rise to each. Draw an energy level diagram to show the lifting of degeneracy of the 3d orbitals in a tetrahedral ligand field . Give the number of unpaired electrons in a strong and weak octahedral field for (a) Cr² (b) Co and (c) Fe. Calculate the CFSE and magnetic moment in each casearrow_forward
- 9. Describe and explain the Jahn teller effect in octahedral complexes of Cu² and Cr Define paramagnetism and diamagnetism. What is the difference between an inner orbital complex and an outer orbital complex? The complex [NiCN)4] is diamagnetic, but [NiCla] is paramagnetic and has two unpaired electrons, explain these observations and deduce the structures of the two complexes The complex ion [Co (NH3)6] is octahedral and diamagnetic, the complexion [CoF6] is also octahedral but paramagnetic. How does valence bond theory account for this observation? How does crystal field explain color of complexes?arrow_forward5. Show how the d orbital splitting changes as an octahedral complex undergoes tetragonal distortion and eventually becomes a square planar complex. What is the spectrochemical series and what is its importance Using crystal field theory, (a) Draw the d-orbital electronic configuration of [Cr(CN)6]³ (b) How many unpaired electrons are present? (c) Calculate the CFSE and magnetic moment of the complex ion (c) If six Br groups were substituted for the six CN groups to give [CrBr.]³ would you expect Ao to increase or decrease? Why? Describe how Ao changes as the charge on the metal changes from M² to M and how it changes between a first row, second row or third row transition element.arrow_forward15. Describe clearly how crystal field theory explains satisfactorily the magnetic moment of transition metal complexes. Which complex has the larger crystal field splitting? Give reasons for your answer. (i) [Co(CN)6] or (ii) [Co(H2O)²+ or (iii) [Co(NH)6] or [Co(NH3)6] [Co(H_O)] [Rh(NH3)]* What relationship exist between A (the crystal field splitting) and the pairing energy (P) in determining whether a given complex will be high spin or low spin.arrow_forward
- Part 1 See Periodic Table Draw the major resonance contributor for the skeletal arrangement CNNO 2 (arrangement a). Include all nonbonding electrons and all nonzero formal charges. The skeleton has been given to you. Н Ν HCNO SE F ·N—N; ☑ P Cl Br Iarrow_forward5. Show how the d orbital splitting changes as an octahedral complex undergoes tetragonal distortion and eventually becomes a square planar complex. What is the spectrochemical series and what is its importance Using crystal field theory, (a) Draw the d-orbital electronic configuration of [Cr(CN)6]³ (b) How many unpaired electrons are present? (c) Calculate the CFSE and magnetic moment of the complex ion (c) If six Br groups were substituted for the six CN groups to give [CrBr.]³ would you expect Ao to increase or decrease? Why? Describe how Ao changes as the charge on the metal changes from M² to M and how it changes between a first row, second row or third row transition element.arrow_forwardPart 1 See Periodic Table One resonance structure of CNO¯ is shown. In the first box, add two curved arrows to show the movement of electrons that result in the resonance form with a -1 formal charge on the oxygen atom. In the second box, draw this resonance form with the -1 formal charge on the oxygen atom by adding bonds, lone pairs, and non-zero formal charges. =0% → [N=C=O 1 N-C-0arrow_forward
- Draw any major resonance contributor for S2O3, assuming that the S atoms are bonded to each other, and the O atoms are bonded to S atoms. Include all nonbonding electrons and all nonzero formal charges.arrow_forwardDetermine which of the following procedures are steps in drawing the resonance structures of pyridine and pyrazine. Check all that apply. Draw the Lewis structure.Consider and draw alternate resonance structures. Calculate the molar mass of the compound. Leave out the lone pairs of electrons. Determine the central atom, if possible. Complete the octets of each atom (dublet for H). Determine the number of covalent bonds in the structure. Check the structure with electron bookkeeping.arrow_forwardDetermine which of the following procedures are steps in drawing the resonance structures of pyridine and pyrazine. Check all that apply. Draw the Lewis structure.Consider and draw alternate resonance structures.Calculate the molar mass of the compound.Leave out the lone pairs of electrons.Determine the central atom, if possible.Complete the octets of each atom (dublet for H).Determine the number of covalent bonds in the structure.Check the structure with electron bookkeeping.arrow_forward
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