Chemistry

Chemistry

Problem

Use the numerical values provided to answer the following for a hydrogen atom. (i) Calculate the radius of the first stationary orbit. (ii) Using the radius obtained in part (i), determine the total energy of the electron in this orbit in electron-volts. Take e=1.60×10−19 C,  m=9.11×10−31 kg,  h=6.63×10−34 J s,  ε0=8.85×10−12 C2N−1m−2,  1 eV=1.60×10−19 Je=1.60\times10^{-19}\,\text{C},\; m=9.11\times10^{-31}\,\text{kg},\; h=6.63\times10^{-34}\,\text{J\,s},\; \varepsilon_0=8.85\times10^{-12}\,\text{C}^2\text{N}^{-1}\text{m}^{-2},\; 1\,\text{eV}=1.60\times10^{-19}\,\text{J}. a. (i) Calculate the radius of the first stationary orbit of hydrogen using the given constants. b. (ii) Determine the total energy of the electron in this orbit and express the answer in electron-volts.

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