2. The strength of a bond between two elements is 813kJ/mol. Calculate the wave length and theelectromagnetic radiation thatwould be needed to break this bond. What type of bond is this?

1. Convert Bond Energy to Joules The bond energy given is 813 kJ/mol. Convert this to joules: 813…

Answered: 2. The strength of a bond between two…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.102PAE

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These UV photons can break chemical bonds in your skin to cause sunburn- a form of radiation damage. If the 330 nm radiation provides exactly the energy to break an average chemical bond in the skin, estimate the average energy of these bonds in kJ/mol.
The molecule XZ2 is formed from the hypothetical elements Z and X. In that molecule both of the Z atoms are bonded to the X atom (and not to each other). The X-X distance in X2 is 0.136 nm and the Z-Z distance in the Z2 is 0.143 nm. What is the predicted bond length for the X-Z bond in the molecule XZ2?
Carbon-carbon bonds form the “backbone” of nearly everyorganic and biological molecule. The average bond energy of the C−C bond is 347 kJ/mol. Calculate the frequency and wave-length of the least energetic photon that can break an average C−C bond. In what region of the electromagnetic spectrum is this radiation?
Use the Born-Haber cycle to calculate the lattice energy of KF. [The heat of sublimation of K is 91.6 kJ·mol−1 and ΔfH(KF) = −567.3 kJ·mol−1. Bond enthalpy for F2 is 158.8 kJ·mol−1. Other data may be found in the Ionization Energies Table and the Electron Affinities Table.]
Chlorine and bromine are in the same group in the periodic table. The bond energy of a Cl–Cl bond is 240 kJ/mol. The bond energy of a Br–Br bond is 190 kJ/mol. Which statement best explains this difference? Bromine has more electron levels than chlorine. Bromine atoms are more likely than chlorine atoms to interact with other atoms. Chlorine atoms form a double bond, and bromine atoms form a single bond. Chlorine atoms are larger than bromine atoms.
The energy of a C-C single bond is 347 kJ/mol. What wavelength of light doesa photon need to have enough energy to break this bond? Provide your answer in nm.
For single bonds between similar types of atoms, how does the strength of the bond relate to the sizes of the atoms? Explain.
Determine the TOTAL energy to remove two electrons from 2 Br- AND form the single bond to make Br2 as described by the net reaction is 2 Br-(g) → Br2(g) + 2 e-.
Consider hypothetical elements X2 and Y2. Suppose the enthalpy of formation of the compound XY is – 84 kJ/mol, the bond energy for X2 is 105 kJ/mol, and the bond energy for Y2 is 58 kJ/mol. A)Estimate the XY bond energy, Ed, in units of kJ/mol. B)If the dissociation of a X-Y molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity required, what would be its wavelength in nm? C)Would a green-light photon (λgreen=550 nm) be able to break the above X-Y bond? Explain.
Suppose there is an element X which occurs naturally as X2(g).X2(g) + 2O2(g) → X2O4(g)ΔHof of O(g) is 249 kJ/molΔHof of X(g) is 458.5 kJ/molΔHof of X2O4(g) is 31 kJ/molThe X-X single bond energy is 116 kJ/molUse the above data to estimate the average bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.
The ionic radii of element E and a different metallic element, M, are shown in the following table: Both elements form oxides, E2O and MO. If lattice energy is defined as the energy required to separate an ionic solid into individual separate gaseous ions, would the lattice energy of MO be less than, equal to, or greater than the lattice energy of the oxide E2O? Justify your answer in terms of Coulomb's law
7.19 If the formation of chemical bonds always releases energy, why don't all elements form dozens of bonds to each atom?

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2. The strength of a bond between two elements is 813kJ/mol. Calculate the wave length and the electromagnetic radiation that would be needed to break this bond. What type of bond is this?