Question

Calculate the energy, frequency, and wavelength required to remove the electron from the H atom, if the electron is in the n=2 energy level. Is the transition visible?

Answer #1

**for Hydrogen,**

**En = -13.6/n^2 ev**

**So, energy for n=2 is,**

**E = -13.6/2^2 = -3.4 eV**

**1)**

**Energy required = 3.4 eV**

**E = 3.4 eV**

**= 3.4*1.602*10^-19 J**

**= 5.45*10^-19 J**

**Answer: 5.45*10^-19 J**

**2)**

**use:**

**E = h*f**

**5.45*10^-19J =(6.626*10^-34 J.s)*f**

**f = 8.225*10^14 Hz**

**Answer: 8.225*10^14 Hz**

**3)**

**use:**

**E = h*c/lambda**

**5.45*10^-19J =(6.626*10^-34 J.s)*(3.0*10^8
m/s)/lambda**

**lambda = 3.647*10^-7 m**

**Answer: wavelength = 3.647*10^-7 m**

**4)**

**wavelength = 3.647*10^-7 m**

**wavelength = 365 nm**

**wavelength of visible light is 400 nm to 700
nm**

**This is not in this range**

**Answer: no**

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