Suppose that any given kind of bond, such as 0-H, hasa characteristic electric dipole. That is, suppose that elec-tric dipole moments can be assigned to bonds just asbond energies can be. Both are usefully accurate approxi-mations. Consider the water moleculeH`HShow that if MOH is the dipole moment of the OH bond,then the dipole moment of water is µ(H2O) = 2µ0H cos(0/2). What is the dipole moment µoH if µ(H,O) is 1.86 D?

dipole moment of Oh bond,μ=1.86D This dipole moment of bond is due to electronegativity of…

Answered: Suppose that any given kind of bond,…

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

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 105AP

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Calculate the bond energy of C-F given that the heat of atominzation of CHFClBr is 1502 kj/mol, and that the bond energies of C--H, C--Br, and C-Cl are 413, 276 and 328 kj/mol, respectively. show the calculations
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— .
Given the bond enthalpies C=O (707), O=O (498), H—O (464), and C—H (414) in kJ/mol, compute Δ H° in kJ/mol for: CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) +259 -618 -259 -519 +618
If the bond in the AB molecule is considered 100% ionic, the absolute value  of the partial charge would be equal to the electron charge (1.602 x 10-19 C). If the distance between A and B atoms is taken as 10-10 m (1Å), the dipole moment between two elementary charges of opposite sign at atomic magnitude (1Å) distance between them is = 1.602x10-19 C x 10-10 m = 1.602 x 10- It is available in 29 Cm (or 4.8 x 10-18 esbcm). Dipole moment is given by debye (D) and 1D = 3.34x10-30 Cm (or 1D = 10-18 esbcm) (esb = electrostatic unit). 1. As can be seen, when the HCl covalent molecule is considered ionic and the bond length is 1.27x10-10 m, calculate the dipole moment. The experimental dipole moment of an HCl polar option is = 1.03 D. Calculate the value character of the H-Cl bond according to the bulletin. How many% covalent is the bond, how many% is ionic? Specify
The bond dissociation energy to break 4 C-H bond(s) in 1 mole of ethanol (CH₃CH₂OH) molecules is
Calculate ∆Hf for C2H4 2C + 2H2 ------> C2H4
Show computations for [H+], pOH, [OH-] of the following substances:
In CH3Cl, are the three hydrogen atoms equivalent (i.e., do they have identical environments with respect to the other atoms adjacent to themselves)?
Hi! Are tou sure it's not [H2O] / [CO] [H2] ?
(a) How does the structure of diborane (B2H6) differ fromthat of ethane (C2H6)? (b) Explain why diborane adoptsthe geometry that it does. (c) What is the significance ofthe statement that the hydrogen atoms in diborane aredescribed as “hydridic”?
The dipole moment (μ�) of HBrHBr (a polar covalent molecule) is 0.831D0.831D (debye), and its percent ionic character is 12.3 %% . Estimate the bond length of the H−BrH−Br bond in picometers. Note that 1 D=3.34×10−30 C⋅m1 D=3.34×10−30 C⋅m and in a bond with 100%% ionic character, Q=1.6×10−19 C�=1.6×10−19 C. Express your answer to two significant figures and include the appropriate units.
What is the dipole moment of CH4 and CCl4? What is the dipole moment of CH3OCH3 and CH3NH2? Which has a higher dipole moment, cis-CHCl=CHCl or trans-CHF=CHF, is trans usually smaller?

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