ICl2F+2: Calculate the maximum wavelength of electromagnetic radiation that is capable of breaking the weakest bond. Express your answer in meters.
Bond energies (kJ/mol) are:
I-I (150)
F-F (160)
Cl-Cl (240)
I came up with:
EI-F = 0.5[EI-I + EF-F] + (χF – χI)2
EI-F = 0.5[1.5546+ 1.6583] + (3.98 – 2.66)2
Solving this gives
EI-F = 3.34885 eV = 323 kJ/mol
Similarly ECl-F = 265 kJ/mol and
EI-Cl = 219 kJ/mol
So to break the I-Cl bond,
Wavelength of radiation= 6.625x10^-34 Js x 3x10^8 m⁄s/2.19x10^3 J x6.023 x 10^23 = 5.47 x 10^-5 m
Not ... not sure if this is 100% correct ... the result will change depending on decimals. What was your result?
Correct answer is:
1)
E I-Cl = sqrt(150X240) + 96.3 (2.66-3.16)^2
2)
E in kJ/mole -> E in J/bond:
E I-Cl/ 6.02*10^23
3)
Wavelength = (6.626*10^(-34) X 3*10^8) / (E in J/bond)
:))
To calculate the maximum wavelength of electromagnetic radiation capable of breaking the weakest bond, we need to determine the bond with the lowest bond energy.
The bond with the lowest bond energy is the F-F bond with a bond energy of 160 kJ/mol.
Now, we can use the equation E = hc/λ, where E is the energy of a single photon, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (2.998 x 10^8 m/s), and λ is the wavelength of the radiation.
We can rearrange the equation to solve for wavelength:
λ = hc/E
First, convert the bond energy from kJ/mol to Joules per bond:
E = (160 kJ/mol) x (1000 J/1 kJ) / (6.022 x 10^23 bonds/1 mol)
E = 2.66 x 10^-19 J/bond
Now, we can substitute the values into the equation:
λ = (6.626 x 10^-34 J·s) x (2.998 x 10^8 m/s) / (2.66 x 10^-19 J/bond)
Calculating this expression will give the maximum wavelength in meters.