21:36Molecular Orbital Theory - Bonding & Antibonding MO - Bond OrderThe Organic Chemistry Tutor644views1rank
Multiple ChoiceApply molecular orbital theory to predict which species has the strongest bond. a) O2 b) O2– c) O2+ d) All the bonds are equivalent 1607views1rank2comments
Multiple ChoiceUsing Molecular Orbital Theory, answer the following questions dealing with carbon mononitride, CN. 1398views1rank1comments
Multiple ChoiceWhich of the following is not consistent with the valence bond theory description of the formation of a chemical bond?330views
Textbook QuestionThe C2 molecule has a MO diagram similar to N2 (Figure 8.22a). What is the bond order of C2 and is it paramagnetic or diamagnetic? (LO 8.12) (a) Bond order = 2, diamagnetic (b) Bond order = 2, paramagnetic (c) Bond order = 0, paramagnetic (d) Bond order = 3>2, diamagnetic1018views
Textbook QuestionConsider the H2+ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H2+ ion to be stable or to fall apart?995views1rank
Textbook QuestionDraw an MO energy diagram and predict the bond order of Li2+ and Li2-. Do you expect these molecules to exist in the gas phase?2604views
Textbook QuestionUsing the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at lower energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? d. 9740views
Textbook QuestionUsing the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at lower energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? c. 8499views
Textbook QuestionUsing the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at lower energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? a. 4327views
Textbook QuestionExplain the following: (c) The O22 + ion has a stronger O—O bond than O2 itself.873views1rank
Textbook QuestionUsing the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at higher energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? d. 14676views
Textbook QuestionUsing the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at higher energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? c. 131804views
Textbook QuestionUsing the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at higher energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? a. 10457views
Textbook QuestionUse molecular orbital theory to predict if each molecule or ion exists in a relatively stable form. a. H22 -745views
Textbook QuestionApply molecular orbital theory to predict if each molecule or ion exists in a relatively stable form. a. C22+ b. Li2 c. Be22+ d. Li22-2542views
Textbook QuestionUsing Figures 9.35 and 9.43 as guides, draw the molecular orbital electron configuration for (d) Ne22 +. In each case indicate whether the addition of an electron to the ion would increase or decrease the bond order of the species.815views
Textbook QuestionIf we assume that the energy-level diagrams for homonuclear diatomic molecules shown in Figure 9.43 can be applied to heteronuclear diatomic molecules and ions, predict the bond order and magnetic behavior of (d) ClF.836views
Textbook QuestionIf we assume that the energy-level diagrams for homonuclear diatomic molecules shown in Figure 9.43 can be applied to heteronuclear diatomic molecules and ions, predict the bond order and magnetic behavior of (b) NO+.664views
Textbook QuestionAccording to MO theory, which molecule or ion has the shortest bond length? O2, O2- , O22 -1627views1rank
Textbook QuestionAccording to MO theory, which molecule or ion has the highest bond energy? O2, O2- , O22 -2288views
Textbook QuestionAccording to MO theory, which molecule or ion has the highest bond order? O2, O2- , O22 -628views
Textbook QuestionDetermine the electron configurations for CN+, CN, and CN-. (a) Which species has the strongest C¬N bond?1812views
Textbook QuestionDraw an MO energy diagram for CO. (Use the energy ordering of O2.) Predict the bond order and make a sketch of the lowest energy bonding molecular orbital.2507views1comments
Textbook QuestionDraw an energy diagram for HCl. Predict the bond order and make a sketch of the lowest energy bonding molecular orbital.1373views
Textbook QuestionDraw a molecular orbital energy diagram for ClF. (Assume that the sp orbitals are lower in energy than the p orbitals.) What is the bond order in ClF?1621views
Textbook QuestionDraw Lewis structures and MO diagrams for CN+ , CN, and CN- . According to the Lewis model, which species is most stable?1667views1comments
Textbook QuestionUse the MO energy diagram in Figure 8.22b to describe the bonding in O2+, O2, and O2-. Which of the three is likely to be stable? What is the bond order of each? Which contain unpaired electrons?976views
Textbook QuestionThe C2 molecule can be represented by an MO diagram similar to that in Figure 8.22a. (b) To increase the bond order of C2, should you add or remove an electron?1516views
Textbook QuestionCalcium carbide, CaC2, reacts with water to produce acetylene, C2H2, and is sometimes used as a convenient source of that substance. Use the MO energy diagram in Figure 8.22a to describe the bonding in the carbide anion, C22-. What is its bond order?1048views
Textbook QuestionOne of the molecular orbitals of the H2- ion is sketched below: (d) Compared to the H¬H bond in H2, the H¬H bond in H2- is expected to be which of the following: (i) Shorter and stronger, (ii) longer and stronger, (iii) shorter and weaker, (iv) longer and weaker, or (v) the same length and strength?560views
Textbook QuestionAt high temperatures, sulfur vapor is predominantly in the form of S21g2 molecules. (d) When two electrons are added to S2, the disulfide ion S22- is formed. Is the bond length in S22- likely to be shorter or longer than the bond length in S2? Explain.505views
Textbook QuestionPlace the following molecules and ions in order from smallest to largest bond order: N22+, He2+, Cl2 H2-, O22-.828views1rank
Textbook QuestionCarbon monoxide is produced by incomplete combustion of fossil fuels. (c) What is the bond order of CO? Does this match the bond order predicted by the electron-dot structure?599views
Textbook QuestionThe energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding π orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the p2p to the p*2p molecular orbital. (c) Is the C¬C bond in ethylene stronger or weaker in the excited state than in the ground state? Why?505views
Open QuestionUse the molecular orbital diagram shown to determine which of the following is most stable.1062views
Open QuestionUse molecular orbital theory to predict whether or not each of the following molecules or ions should exist in a relatively stable form.383views
Open QuestionUse the molecular orbital diagram shown to determine which of the following is least stable.351views
Open QuestionComplete the molecular orbital diagram for CN−. Note that the 1𝑠 orbitals are not shown.385views