Answered: (a)Complex forming agents can be used…

(a)Complex forming agents can be used to determine hardness of water how? Explain with the help of following points. (i) Principle (ii) Chemical reactions (iii) Structure (iv) Calculations.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 66AP: Calcium carbide (CaC2) is an intermediate in the manufacturing of acetylene (C2H2) . It is the...

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Antibonding molecular orbitals can be used to make bonds to other atoms in a molecule. For example, metal atoms can use appropriate d orbitals to overlap with the T, orbitals of the carbon monoxide molecule. This is called d – T backbonding. (a) Draw a coordinate axis system in which the y -axis is vertical in the plane of the paper and the x -axis horizontal. Write ªM" at the origin to denote a metal atom. (b) Now, on the x -axis to the right of M, draw the Lewis structure of a CO molecule, with the carbon nearest the M. The CO bond axis should be on the x -axis. (c) Draw the CO T, orbital, with phases (see the "Closer Look" box on phases) in the plane of the paper. Two lobes should be pointing toward M. (d) Now draw the dy orbital of M, with phases. Can you see how they will overlap with the T, orbital of CO? (e) What kind of bond is being made with the orbitals between Mand C, o or n?(f) Predict what will happen to the strength of the CO bond in a metal-CO complex compared to CO…
Many compounds of the transition-metal elements contain direct bonds between metal atoms. We will assume that the z-axis is defined as the metal–metal bond axis. (a) Which of the 3d orbitals (Figure 6.23) can be used to make a σ bond between metal atoms? (b) Sketch the bonding and σ3d* antibonding MOs.(c)With reference to the “Closer Look” box on the phases of orbitals, explain why a node is generated in the σ3d* MO. (d) Sketch the energy-level diagram for the Sc2 molecule, assuming that only the 3d orbital from part (a) is important. (e)What is the bond order in Sc2?
(a) Sketch the molecular orbitals of the H2- ion and draw itsenergy-level diagram. (b) Write the electron configuration ofthe ion in terms of its MOs. (c) Calculate the bond order inH2-. (d) Suppose that the ion is excited by light, so that anelectron moves from a lower-energy to a higher-energy molecularorbital. Would you expect the excited-state H2- ion to bestable? (e) Which of the following statements about part (d) is correct: (i) The light excites an electron from a bonding orbitalto an antibonding orbital, (ii) The light excites an electronfrom an antibonding orbital to a bonding orbital, or (iii)In the excited state there are more bonding electrons thanantibonding electrons?
Many compounds of the transition-metal elements containdirect bonds between metal atoms. We will assumethat the z-axis is defined as the metal–metal bond axis.(a) Which of the 3d orbitals (Figure 6.23) is most likely tomake a σ bond between metal atoms? (b) Sketch the s3dbonding and σ*3d antibonding MOs. (c) With reference tothe “Closer Look” box on the phases of orbitals, explain whya node is generated in the σ*3d MO. (d) Sketch the energyleveldiagram for the Sc2 molecule, assuming that only the3d orbital from part (a) is important. (e) What is the bondorder in Sc2?
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2. Draw MO energy level diagrams for each of the following diatomic molecules are molecular ions. All contributing atomic orbitals and the resulting molecular orbitals must be labeled properly showing the electrons (as arrows) in the atomic orbitals and in the molecular orbitals. All orbitals should be drawn to show their relative energy relationships. Calculate the bond order for each and label each as either diamagnetic or paramagnetic. (a) BO‒ (b) CN (c) FCl (d) Cl2‒
The following sketches show the atomic orbital wave functions(with phases) used to construct some of the MOs ofa homonuclear diatomic molecule. For each sketch, determinethe type of MO that will result from mixing theatomic orbital wave functions as drawn. Use the same labelsfor the MOs as in the “Closer Look” box on phases.
Use the References to access important values if needed for this question. Consider the fluorine molecule and the F," molecular ion: (a) Give the bond order of each species. If a fraction is needed, use a decimal number. Bond order F2 Bond order F2= (b) Predict which species should be paramagnetic. Is F2 paramagnetic? | Is F2 paramagnetic? (c) Predict which species has the greater bond dissociation energy. The species with the largest bond dissociation energy is: a. F2 b. F2
The following is part of a molecular orbital energy-level diagramfor MOs constructed from 1s atomic orbitals. (a) What labels do we use for the two MOs shown? (b) Forwhich of the following molecules or ions could this be theenergy-level diagram:H2, He2, H2+, He2+, or H2-?(c) What is the bond order of the molecule or ion? (d) If anelectron is added to the system, into which of the MOs will itbe added? [
(a) If these three balloons are all the same size, what angleis formed between the red one and the green one? (b) If additionalair is added to the blue balloon so that it gets larger,will the angle between the red and green balloons increase,decrease, or stay the same? (c) Which of the following aspectsof the VSEPR model is illustrated by part (b): (i) Theelectron-domain geometry for four electron domains is tetrahedral.(ii) The electron domains for nonbonding pairs arelarger than those for bonding pairs. (iii) The hybridizationthat corresponds to a trigonal planar electron-domain geometryis sp2.
(a) If these three balloons are all the same size, what angleis formed between the red one and the green one? (b) If additionalair is added to the blue balloon so that it gets larger,will the angle between the red and green balloons increase,decrease, or stay the same? (c) Which of the following aspectsof the VSEPR model is illustrated by part (b): (i) Theelectron-domain geometry for four electron domains is tetrahedral.(ii) The electron domains for nonbonding pairs arelarger than those for bonding pairs. (iii) The hybridizationthat corresponds to a trigonal planar electron-domain geometryis sp2. [Section 9.2]
3.) Carbon and graphite are allotropes of Carbon. Between graphite and diamond, which one is a good conductor of electricity and which one is not? Support answer with an explanation. (Limit answer to not more than 4 sentences)