1- Use the molecular orbital model to predict the bond order and magnetism of each of the following molecules.a- COb- CO+c- CO2+ 2- Compare and contrast bonding molecular orbitals with antibonding molecularorbitals. 3- Consider the following electron configuration:(σ3s)2(σ3s*)2(σ3p)2(π3p)4(π3p*)4Give four species that, in theory, would have this electron configuration. 4- Predict which substance in each of the following pairs would have the greaterintermolecular forces.I. CO2 or OCSII. SeO2 or SO2III. CH3CH2CH2NH2 or H2NCH2CH2NH2IV. CH3CH3 or H2COV. CH3OH or H2CO 5- Explain why water forms into beads on a waxed car finish. 6- At which temperature does water have its greatest density? 7- At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is solid. This is because of what?
1- Use the molecular orbital model to predict the bond order and magnetism of each of the following molecules.a- COb- CO+c- CO2+ 2- Compare and contrast bonding molecular orbitals with antibonding molecularorbitals. 3- Consider the following electron configuration:(σ3s)2(σ3s*)2(σ3p)2(π3p)4(π3p*)4Give four species that, in theory, would have this electron configuration. 4- Predict which substance in each of the following pairs would have the greaterintermolecular forces.I. CO2 or OCSII. SeO2 or SO2III. CH3CH2CH2NH2 or H2NCH2CH2NH2IV. CH3CH3 or H2COV. CH3OH or H2CO 5- Explain why water forms into beads on a waxed car finish. 6- At which temperature does water have its greatest density? 7- At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is solid. This is because of what?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter10: Molecular Geometry And Chemical Bonding Theory
Section: Chapter Questions
Problem 10.22QP
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1- Use the molecular orbital model to predict the bond order and magnetism of each of the following molecules.
a- CO
b- CO+
c- CO2+
2- Compare and contrast bonding molecular orbitals with antibonding molecular
orbitals.
3- Consider the following electron configuration:
(σ3s)2
(σ3s*)2
(σ3p)2
(π3p)4
(π3p*)4
Give four species that, in theory, would have this electron configuration.
4- Predict which substance in each of the following pairs would have the greater
intermolecular forces.
I. CO2 or OCS
II. SeO2 or SO2
III. CH3CH2CH2NH2 or H2NCH2CH2NH2
IV. CH3CH3 or H2CO
V. CH3OH or H2CO
5- Explain why water forms into beads on a waxed car finish.
6- At which temperature does water have its greatest density?
7- At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is solid. This is because of what?
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