#Q.1# Calculate the frequency of #e^-# in the first Bohr orbit of H-atom?
1 Answer
You should get the Rydberg constant in reciprocal wavelength units as your answer.
Well, the energy levels of a hydrogen-like atom are given by:
#E_n = -(mu Z^2 e^4)/(8epsilon_0^2 h^2 n^2)# ,where:
#mu = (m_em_p)/(m_e + m_p) = 9.104425135 xx 10^(-31) "kg"# is the reduced mass of the electron + proton.#m_e = 9.10938356 xx 10^(-31) "kg"# is the rest mass of the electron.#m_p = 1.672621898 xx 10^(-27) "kg"# is the rest mass of the proton.#Z# is the atomic number.#e# is the elementary charge,#1.60217662 xx 10^(-19) "C"# .#epsilon_0 = 8.854187817 xx 10^(-12) "C"^2cdot"s"^2"/kg"cdot"m"^3# is the vacuum permittivity.#h = 6.62607004 xx 10^(-34) "kg"cdot"m"^2"/s"# is Planck's constant.#n# is the principal quantum number.
So, the ground-state energy, i.e. the energy in the so-called "first Bohr orbit", is:
#ul(E_1) = -((9.104425135 xx 10^(-31) "kg")(1^2)(1.60217662 xx 10^(-19) cancel("C"))^cancel(4))/(8 cdot (8.854187817 xx 10^(-12) cancel("C"^2)cdot"s"^2"/"cancel"kg"cdot"m"^(cancel(3)^(2)))^cancel(2)(6.62607004 xx 10^(-34) cancel"kg"cdotcancel("m"^2)"/"cancel("s"))^cancel(2)(1^2))#
The remaining units are as expected,
#= ul(-2.17868577 xx 10^(-18) "J")#
I recall the energy should be
#E_1 = -2.17868577 xx 10^(-18) cancel"J" xx "1 eV"/(1.60217662 xx 10^(-19) cancel"J")#
#= -"13.60 eV"#
Close enough. If you used the approximation that
#E = hnu# ,
so by noting that frequencies are always nonnegative... the electron would need an input of
#color(blue)(nu_1) = |E_1|/h = (2.17868577 xx 10^(-18) cancel"J")/(6.62607004 xx 10^(-34) cancel"J"cdot"s")#
#= color(blue)(3.288051226 xx 10^(15))# #color(blue)("s"^(-1))#
Or, perhaps a more useful unit is the
#color(blue)(R_H) = nu_1 / (2.99792458 xx 10^(10) "cm/s") = color(blue)("109677.58 cm"^(-1))#
which is, would you look at that, pretty much the Rydberg constant in