Hydrogen Spectrum Lab Report
Lab 3: Hydrogen Spectrum
Abstract
When white light is viewed through a diffraction grating, we can see each component that makes up the light. However, when in an excited state, a gaseous element produces bright light of specific wavelengths rather than a continuous spectrum of colors. This phenomenon ultimately lead to the Neils Bohr model of the atom in 1913.
Introduction
In the middle of the 19th century, Robert Bunsen and Gustav Kichoff observed that gases emit spectral lines specific to each element. This made it possible for the composition of these gases to be analyzed by using a spectroscope to identify the wavelengths of the emitted spectral lines. In 1885, Johann Balmer created a formula for the spectral lines for the hydrogen atom, which was later found to be a special case of the Rydberg formula.
Theory …show more content…
These light rays then become diffracted upon hitting the diffraction grating and can be observed by a telescoping lens that is fixed upon a rotating axis to the collimating lens. By observing the angle at which the spectral lines are visible, we can determine the wavelengths using Balmer's formula:
where λ is the wavelength, h is a constant = 3.6456 x 10-7 m, n = 2, and m is an integer such that m > n. One can also determine the the Rydberg constant for hydrogen using Rydberg's formula:
where λ is the wavelength, n1 and n2 are integers such that n1 > n2, and RH is the Rydberg constant for hydrogen.
No one understood why these formulas worked until Neils Bohr created the first quantum model for the binding energy of the electrons in a hydrogen atom.:
where k = 8.988 x 109 Nm2/C2, and aB is the Bohr radius. The observed light is produced by photon emission when an electron changes energy levels. This change in energy can be shown as:
where h = 6.626 x 10-37 m2kg/s.
Abstract
When white light is viewed through a diffraction grating, we can see each component that makes up the light. However, when in an excited state, a gaseous element produces bright light of specific wavelengths rather than a continuous spectrum of colors. This phenomenon ultimately lead to the Neils Bohr model of the atom in 1913.
Introduction
In the middle of the 19th century, Robert Bunsen and Gustav Kichoff observed that gases emit spectral lines specific to each element. This made it possible for the composition of these gases to be analyzed by using a spectroscope to identify the wavelengths of the emitted spectral lines. In 1885, Johann Balmer created a formula for the spectral lines for the hydrogen atom, which was later found to be a special case of the Rydberg formula.
Theory …show more content…
These light rays then become diffracted upon hitting the diffraction grating and can be observed by a telescoping lens that is fixed upon a rotating axis to the collimating lens. By observing the angle at which the spectral lines are visible, we can determine the wavelengths using Balmer's formula:
where λ is the wavelength, h is a constant = 3.6456 x 10-7 m, n = 2, and m is an integer such that m > n. One can also determine the the Rydberg constant for hydrogen using Rydberg's formula:
where λ is the wavelength, n1 and n2 are integers such that n1 > n2, and RH is the Rydberg constant for hydrogen.
No one understood why these formulas worked until Neils Bohr created the first quantum model for the binding energy of the electrons in a hydrogen atom.:
where k = 8.988 x 109 Nm2/C2, and aB is the Bohr radius. The observed light is produced by photon emission when an electron changes energy levels. This change in energy can be shown as:
where h = 6.626 x 10-37 m2kg/s.