Question

electronic structure and chemical bonding interconverting wavelength, frequency and photon energy try again your answer is wrong. the number of significant digits cant be determined. it takes 146. kj/mol to break an oxygen - oxygen single bond. calculate the maximum wavelength of light for which an oxygen - oxygen single bond could be broken by absorbing a single photon. round your answer to 3 significant digits.

Explanation:

Step1: Convert energy per mole to energy per photon

First, convert the energy required to break an oxygen - oxygen single bond from kJ/mol to J/photon. We know that 1 mole = $6.022\times10^{23}$ photons and 1 kJ = 1000 J.
$E=\frac{146\times1000\ J/mol}{6.022\times10^{23}\ photons/mol}\approx2.424\times 10^{-19}\ J/photon$

Step2: Use the energy - wavelength formula

The energy of a photon is given by the formula $E = h
u=\frac{hc}{\lambda}$, where $h = 6.626\times10^{-34}\ J\cdot s$ (Planck's constant), $c = 3.0\times10^{8}\ m/s$ (speed of light) and $\lambda$ is the wavelength.
We can re - arrange the formula to solve for $\lambda$: $\lambda=\frac{hc}{E}$.
Substitute the values of $h$, $c$ and $E$ into the formula:
$\lambda=\frac{6.626\times10^{-34}\ J\cdot s\times3.0\times10^{8}\ m/s}{2.424\times 10^{-19}\ J}\approx8.19\times10^{-7}\ m$

Step3: Convert the wavelength to nm

Since 1 m = $10^{9}$ nm, then $\lambda = 8.19\times10^{-7}\ m\times10^{9}\ nm/m = 819\ nm$

Answer:

$819\ nm$