According to the Bohr model of a hydrogen atom, the frequency of light radiated by an electron moving from an orbit
to an orbit
corresponds to the energy level difference between
and
of
,
where
,
and where
is the electron mass,
is the atomic number,
is the magnitude of the electron charge,
is the permittivity of free space, and
is Planck's constnt divided by
. In the case of hydrogen (
)
.
Part A 

Find the frequency of light radiated by an electron moving from orbit to inside of a ion. 
Express your answer in hertz to three significant figures.
ANSWER: 
 =  9.860×10^{15}
 

Part B 

In the Bohr model of hydrogen, the radius of the orbit is defined as , where is called the Bohr radius. Find the radius of a valence orbital for a ion. Express your answer in meters to three significant figures.
ANSWER: 
 =  2.65×10^{−11}
 


In fact, the radius of the helium valence orbital is
. The discrepancy between your answer and the real value can be explained by the fact that the Bohr model is a semiclassical treatment of a quantum problem. It only works well for the hydrogen atom and, with some corrections, for helium. Bohr's model fails for larger atoms. This is due to the presence of many (more than one) electrons in those atoms. With a large number of electrons in an atom, their mutual interactions become significant and cannot be ignored, as they are in the Bohr model.
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