Q1: Find the frequency of revolution of the electron in the classical model of the hydrogen atom.In what region of the spectrum are electromagnetic waves of this frequency?? Q2:A beam of 13.o electrons is used to bombared gaseous hydrogen.What series of wavelengths will be emitted?
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To find the frequency of revolution of the electron in the classical model of the hydrogen atom, you can use the formula:
f = (v / 2πr) (Equation 1)
where f represents the frequency, v is the velocity of the electron, and r is the radius of the electron's orbit.
However, in the classical model of the hydrogen atom, the electron does not revolve in a circular orbit like in the Bohr model. Instead, it moves in elliptical orbits, making the question invalid in the classical context.
Moving on to the second question, when a beam of electrons is used to bombard gaseous hydrogen, it excites the hydrogen atoms, causing them to transition to higher energy states. These excited atoms then emit radiation as they return to lower energy states. The wavelengths emitted during this process fall into specific series called the spectral lines.
The most well-known spectral series in hydrogen is the Balmer series, which corresponds to electron transitions involving the second energy level (n = 2). The Balmer series emits visible light, which ranges from approximately 400 to 700 nanometers (nm).
Thus, the wavelengths emitted by the hydrogen atoms upon bombardment by a beam of 13.0 electrons will fall within the visible spectrum, specifically in the Balmer series.