Hydrogen Atom and Hydrogen Molecule The observed wavelengths in the line spectrum of hydrogen atom were first expressed in terms of a series by johann Jakob Balmer, a Swiss teacher. Balmer's empirical empirical formula is 1/lambda=R_(H)(1/2^(2)-1/n^(2)),"" N=3, 4, 5 R_(H)=(Me e^(4))/(8 epsilon_(0)^(2)h^(3) c)=109. 678 cm^(-1) Here, R_(H) is the Rydberg Constant, m_(e) is the mass of electron. Niels Bohr derived this expression theoretically in 1913. The formula is easily generalized to any one electron atom//ion. Determine the loest energy and the radius of the Bohr orbit of the muonic hydrogen atom. Ignore the motion of the nucleus in your calculation. The radius of the Bohr orbit of a hydrogen atom ("called the Bohr radius", a_(0)=(epsilon_(0)h^(2))/(m_(e)e^(2)prod) "is" 0.53 Å) The classical picture of an ''orbit'' in Bohr's theory has now been replaced by the quantum mechanical nation of an 'orbital'. The orbital psi 1 sigma 1s (r) for the ground state of a hydrogen atom is given by psi 1 s (r)=1/sqrt(proda_(0)^(3)) e^(r/a_(0)) where r is the distance of the electron from the nucleus and a_(0) is the Bohr radius.