Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Chapter 6, Problem 30P
The molecular ion
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The average bond energy (enthalpy) for a C=C double bond is 614 kJ/molkJ/mol and that of a C−C single bond is 348 kJ/molkJ/mol. If it takes
4.42×10−19
J/molecule
to break the C=C double bond. What is the longest wavelength λ of light that will provide photons of sufficient energy to break the π bond and cause the isomerization?
Express your answer numerically in nanometers.
There are two main types of covalent bond breakage. In ho-molytic breakage , each atom in the bond gets one of the shared electrons. In some cases, the electronega-tivity of adjacent atoms affects the bond energy. In heterolytic breakage, one atom gets both electrons and the other gets none;thus, a cation and an anion form. (a) Why is the C−C bond in H₃C−CF₃(423 kJ/mol) strongerthan that in H₃C−CH₃(376 kJ/mol)?(b) Use bond energy and any other data to calculate the heat ofreaction for the heterolytic cleavage of O₂.
The molecular ion HeH1 has an equilibrium bond length of 0.774 Å. Draw an electron correlation diagram for this ion, indicating the occupied MOs. Is HeH+ paramagnetic? When HeH+ dissociates, is a lower energy state reached by forming He+H+ or He+ + H?
Chapter 6 Solutions
Principles of Modern Chemistry
Ch. 6 - Determine the number of nodes along the...Ch. 6 - Determine the number of nodes along the...Ch. 6 - Sketch the shape of each of the molecular...Ch. 6 - Sketch the shape of each of the molecular...Ch. 6 - Compare the electron density in the 1g and 1u*...Ch. 6 - Explain why 1g is the ground state for H2+ . By...Ch. 6 - Prob. 7PCh. 6 - Predict the ground electronic state of the He22+...Ch. 6 - Prob. 9PCh. 6 - Prob. 10P
Ch. 6 - Without consulting tables of data, predict which...Ch. 6 - Without consulting tables of data, predict which...Ch. 6 - Without consulting tables of data, on the same...Ch. 6 - Without consulting tables of data, on the same...Ch. 6 - Suppose we supply enough energy to H2 to remove...Ch. 6 - Suppose we supply enough energy to He2+ to remove...Ch. 6 - Prob. 17PCh. 6 - When one electron is added to an oxygen molecule,...Ch. 6 - Predict the valence electron configuration and the...Ch. 6 - Predict the valence electron configuration and the...Ch. 6 - Prob. 21PCh. 6 - For each of the following valence electron...Ch. 6 - For each of the electron configurations in Problem...Ch. 6 - For each of the electron configurations in Problem...Ch. 6 - Following the pattern of Figure 6.21, work out the...Ch. 6 - Following the pattern of Figure 6.21, work out the...Ch. 6 - The bond length of the transient diatomic molecule...Ch. 6 - The compound nitrogen oxide (NO) forms when the...Ch. 6 - What would be the electron configuration for a HeH...Ch. 6 - The molecular ion HeH+ has an equilibrium bond...Ch. 6 - Prob. 31PCh. 6 - Predict the ground state electronic configuration...Ch. 6 - The bond dissociation energies for the species NO,...Ch. 6 - The ionization energy of CO is greater than that...Ch. 6 - Photoelectron spectra were acquired from a sample...Ch. 6 - Photoelectron spectra were acquired from a sample...Ch. 6 - Prob. 37PCh. 6 - From the n=0 peaks in the photoelectron spectrum...Ch. 6 - The photoelectron spectrum of HBr has two main...Ch. 6 - The photoelectron spectrum of CO has four major...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Both the simple VB model and the LCAO method...Ch. 6 - Both the simple VB model and the LCAO method...Ch. 6 - Write simple valence bond wave functions for...Ch. 6 - Write simple valence bond wave functions for...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Formulate a localized bond picture for the amide...Ch. 6 - Formulate a localized bond picture for the...Ch. 6 - Prob. 51PCh. 6 - Draw a Lewis electron dot diagram for each of the...Ch. 6 - Describe the hybrid orbitals on the chlorine atom...Ch. 6 - Describe the hybrid orbitals on the chlorine atom...Ch. 6 - The sodium salt of the unfamiliar orthonitrate ion...Ch. 6 - Describe the hybrid orbitals used by the carbon...Ch. 6 - Describe the bonding in the bent molecule NF2 ....Ch. 6 - Describe the bonding in the bent molecule OF2 ....Ch. 6 - The azide ion (N3) is a weakly bound molecular...Ch. 6 - Formulate the MO structure of (NO2+) for localized...Ch. 6 - Discuss the nature of the bonding in the nitrite...Ch. 6 - Discuss the nature of the bonding in the nitrate...Ch. 6 - The pyridine molecule (C5H5N) is obtained by...Ch. 6 - For each of the following molecules, construct the...Ch. 6 - (a) Sketch the occupied MOs of the valence shell...Ch. 6 - Calcium carbide (CaC2) is an intermediate in the...Ch. 6 - The B2 molecule is paramagnetic; show how this...Ch. 6 - The Be2 molecule has been detected experimentally....Ch. 6 - Prob. 69APCh. 6 - The molecular ion HeH+ has an equilibrium bond...Ch. 6 - The MO of the ground state of a heteronuclear...Ch. 6 - The stable molecular ion H3+ is triangular, with...Ch. 6 - According to recent spectroscopic results,...Ch. 6 - trans-tetrazene (N4H4) consists of a chain of four...
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- Light of appropriate wavelength can break chemical bonds. Light having λ < 240 nm can dissociate gaseous O2. It requires light with λ < 819 nm to dissociate gaseous H2O2 to 2 OH. Assume that all of the photon energy is used solely for these dissociations. (a) Calculate the energy required to dissociate (i) O2 and (ii) H2O2. (b) Consider the results of part (a). How well do they correlate with the Lewis structures of O2 and H2O2? Explain your answer.arrow_forwardThe bond energy of C2 is 599 kJ/mol, the bond distance is 110 pm. Take a rough estimate of the Coulomb repulsion in doubly ionized C2 (i.e., C22+). How far would the C-C bond have to stretch for the Coulomb repulsion to be less than the bond energy in neutral C2? Do you think that the C22+ molecule will still be stable?arrow_forwardTwo useful organic compounds that contain Cl atoms are vinyl chloride(CH2=CHCl) and chloroethane (CH3CH2Cl). Vinyl chloride is the startingmaterial used to prepare poly(vinyl chloride), a plastic in insulation,pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic.Why is the C–Cl bond in vinyl chloride stronger than the C–Cl bond inchloroethane?arrow_forward
- Two useful organic compounds that contain Cl atoms are vinyl chloride (CH2=CHCl) and chloroethane (CH3CH2Cl). Vinyl chloride is the starting material used to prepare poly(vinyl chloride), a plastic in insulation, pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic. Why is the C–Cl bond in vinyl chloride stronger than the C–Cl bond in chloroethane?arrow_forwardThe dipole moment of gaseous Ag – Cl is ? = 6.08 D, and the bond distance is r(Ag − Cl) = 228. 1 pm. Calculate the percent ionic character for this bond in the gas phase. In solid form it is however, found the following values for the two silver halides Ag − CL and Ag − F: See image Explain why solid silver chloride is sparingly soluble in water, while solid silver fluoride is moderately soluble B) Explain why solid silver chloride is sparingly soluble in water, while solid silver fluoride is moderately soluble Given extra information: Formal charge: ?? = ??? – (??? + ???); where ??? = valence electrons in free atom, ???= free-pair electrons, ??? = number of bonds to the atom. The elementary charge: ? = 1.6022 × 10−19 C.1 Debye (?)= 3.3356 × 10−30 C × m. The dipole moment has definition: ? = ? × ?, where ? is partialcharge in Coulomb (?), ? is the bond distance (?). Picometer: 1 ?? = 1 × 10−12arrow_forwardWhich of the following bonds is most polar: S¬Cl, S¬Br, Se¬Cl,or Se¬Br?arrow_forward
- The bond angles in antimony trifluoride are 87°. Describe the bonding in SbF3, including a picture of the orbital overlap interaction that creates the Sb-F bonds. ✓orbitals from the inner atom. An outer halogen atom always uses one of ✓valence orbitals, and fluorine has n = vvalence orbitals, Bond angles near 90° signal interactions of valence its valence ✓orbitals to form a bond. Antimony has n = so each of the three bonds in SbF3 can be described as resulting from overlap between a orbital from F. There are three vorbital from Sb and a bonds that point at near-right angles to one another.arrow_forwardWrite the ground-state electron configuration for each atomand ion pair-Zr, Zr2+, Co, Co2+, Tc, Tc3+, Os, Os4+?arrow_forward5.a. Explain how the lattice energy of an ionic compound such as KCI can be determined using the Born-Haber cycle. On what law is this procedure based? How do the ionization energy and the electron affinity determine whether atoms of elements will combine to form ionic compounds? b. Explain in molecular orbital terms the changes in H-H inter-nuclear distance that occurs as the molecular H2 is ionized first to H2* and then to H2²*. Explain why the bond order of N2 is greater than that of N2*, but the bond order of 02 is less than that of O2*.arrow_forward
- An carbon-to-oxygen single bond (i.e. C-O) has a bond energy of 358 kJ/mol and an carbon-to-oxygen double bond (i.e. C=O) has a bond energy of 749 kJ/mol. Estimate the value of the carbon-to-oxygen bond energy in the carbonate anion, CO32— . Hint: draw the Lewis structure of CO32— , consider resonance and determine which type of bonds it has. Because of the resonance, the bond between C and O will be somewhere in between the single and double bond. Group of answer choices 1107 kJ/mol 358 kJ/mol 488 kJ/mol 928 kJ/mol 1465 kJ/mol 618 kJ/mol 749 kJ/mol 554 kJ/molarrow_forwardThe bond dissociation energies for AA, BB, and AB are 6.17, 7.69, and 7.28 eV, respectively. Calculate the difference the electronegativities of A and B on the Pauling scale. Select one:arrow_forward“Inert” xenon actually forms several compounds, especially with the highly electronegative elements oxygen and fluorine. The simple fluorides XeF2, XeF4, and XeF6 are all formed by direct reaction of the elements. As you might expect from the size of the xenon atom, the Xe-F bond is not a strong one. Calculate the Xe-F bond energy in XeF6, given that the enthalpy of formation is - 402 kJ/mol.arrow_forward
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