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# Calculate the largest wavelength which can remove the electron from 1 Bohr's orbit. Given $E_1$ = 13.6 eV

$(a)\;813.4 \overset{\circ}{A}\qquad(b)\;672.4 \overset{\circ}{A}\qquad(c)\;912.24\overset{\circ}{A} \qquad d)\;734 \overset{\circ}{A}\qquad$

The photon capable of removing electron from I Bohr's orbit must posses energy
= 13.6 eV
= $13.6\times1.602\times10^{-19}$J
= $21.787\times10^{-19}$ J
E = $\large\frac{h\times c}{\lambda}$
$21.787\times10^{-19}$ = $\large\frac{6.625\times10^{-34}\times3.0\times10^8}{\lambda}$
$\lambda = 912.24\times10^{-10}$ m
= 912.24 $\overset{\circ}{A}$
edited Mar 19, 2014