According to the Bohr theory of the hydrogen atom, what is the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state?
delta E = 2.180 x 10^-18*(1/2 - 1/infinity) = ??
For whatever it's worth, 1/infinity = 0.
It should be delta E = -2.18x10^-18 J (1/(2squared) - 1/infinitysquared)
Dr. Bob is definitely not a doctor.
To find the minimum energy required to ionize a hydrogen atom from the n = 2 state using the Bohr theory, you can use the formula for the energy of an electron in an orbit:
E = - (13.6 eV) / n^2
Where E is the energy, n is the principal quantum number, and 13.6 eV is the ionization energy of a hydrogen atom.
In this case, the atom is in the n = 2 state, so plug n = 2 into the formula:
E = - (13.6 eV) / (2^2)
E = - (13.6 eV) / 4
To convert eV to Joules, remember that 1 eV is equal to 1.602 x 10^(-19) Joules. So, multiply the result by this conversion factor:
E = - (13.6 eV) / 4 * (1.602 x 10^(-19) J/eV)
After performing the calculation, you will find the minimum energy required to ionize the hydrogen atom from the n = 2 state.