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The four spectral lines of the Balmer series that fall in the visible range are:
656.3 nm . . . . red
486.1 nm . . . . cyan
434.1 nm . . . . blue
410.2 nm . . . . violet
There are four more lines in the Balmer series ... all in the ultraviolet ... and
at least thirty-six observable lines altogether from the hydrogen atom.
What else can I help you with?
Is an atomic emission spectrum a continuous range of colors?
No, an atomic emission spectrum is not a continuous range of colors. It consists of discrete lines of specific wavelengths corresponding to the emission of light from excited atoms when they return to lower energy levels. Each element has a unique atomic emission spectrum due to its unique arrangement of electrons.
Why is the emission spectrum of hydrogen a line spectrum and not a continuous spectrum?
It's a line spectrum because of the quantization of energy- meaning you only see energy with levels n=1,2,3.... One would never see the energy level n=2.8 for instance- that would be the case if it were continuous rather than a line spectrum.
What is the significance of the helium lamp spectrum in the study of atomic emission spectroscopy?
The helium lamp spectrum is important in atomic emission spectroscopy because it provides a reference for identifying and calibrating the wavelengths of light emitted by other elements. By comparing the emission lines of unknown samples to the known lines of helium, scientists can determine the elemental composition of a sample.
In science what is meant by the Lyman series?
The Lyman series refers to a series of spectral lines in the ultraviolet region of the electromagnetic spectrum that are emitted by hydrogen atoms when electrons transition to the n=1 energy level. These transitions result in the emission of photons with specific wavelengths that are characteristic of the Lyman series.
The lines at the ultraviolet end of the hydrogen spectrum are known as the lyman series wich electron transitions within an atom are responsible for these lines?
The series of lines in an emission spectrum caused by electrons falling from energy level 2 or higher (n=2 or more) back down to energy level 1 (n=1) is called the Lyman series. These emission lines are in the ultra-violet region of the spectrum.
What scientist discovered a mathematical equation that allowed one to calculate the wavelengths of each of the bright lines in the hydrogen emission spectrum?
The scientist who discovered the mathematical equation to calculate the wavelengths of the bright lines in the hydrogen emission spectrum is Johann Balmer. In 1885, he formulated the Balmer series, which describes the wavelengths of the spectral lines resulting from electron transitions in hydrogen atoms. His equation allowed for the prediction of these wavelengths, significantly advancing the understanding of atomic structure and spectral lines.
What is the difference between absorption and emission spectrum?
Emission spectrum: lines emitted from an atom.Absorption spectrum: absorbed wavelengths of a molecule.
Which element did Bohr study the line emission spectrum of?
Niels Bohr studied the emission lines of Hydrogen.
What do Each of the colored lines in hydrogen's emission spectrum corresponds with?
Each colored line in hydrogen's emission spectrum corresponds to a specific transition of an electron between energy levels in the hydrogen atom. The wavelengths of these lines are unique to each transition, creating a distinct pattern that can be used to identify elements and their energy levels.
Which scientists discovered a mathematical equation that allowed one to calculate the wavelengths of each of the bright lines in the hydrogen emission spectrum?
The mathematical equation that allows one to calculate the wavelengths of each line in the hydrogen emission spectrum was discovered by Danish physicist Niels Bohr in 1913 as part of his model of the hydrogen atom. This equation is known as the Balmer equation and helped to explain the spectral lines observed in hydrogen emission spectra.
How does the spectrum of helium differ from the spectrum of white light from the Sun?
The spectrum of helium consists of distinct lines at specific wavelengths, known as emission lines, due to the transition of electrons between energy levels. In contrast, the spectrum of white light from the Sun is continuous, with all visible wavelengths present. The presence of absorption lines in the solar spectrum, caused by elements in the Sun's atmosphere absorbing specific wavelengths, further distinguishes it from the discrete emission lines of helium.
Who developed an equation used to predict the lines in the emission spectrum of hydrogen?
Rydberg
How do the emission spectra for hydrogen and helium differ from each other?
The emission spectra for hydrogen and helium differ in the specific wavelengths of light they emit. Hydrogen emits light in distinct lines corresponding to transitions of its electrons between energy levels, while helium emits a continuous spectrum of light.
What is the emission spectrum of the sun and what does this spectrum reveal about the types of elements in the sun?
The emission spectrum of the sun is primarily a continuous spectrum with dark absorption lines, known as the Fraunhofer lines, which occur at specific wavelengths where elements in the sun's atmosphere absorb light. This spectrum reveals the presence of various elements, including hydrogen, helium, calcium, and iron, as each element absorbs light at characteristic wavelengths. By analyzing these absorption lines, scientists can determine not only the composition of the sun but also its temperature, density, and other physical properties. Overall, the sun's emission spectrum serves as a crucial tool in astrophysics for understanding stellar composition and behavior.
Why does helium have more emission lines than hydrogen?
Helium has more emission lines than hydrogen because it has more electrons and energy levels, leading to more possible transitions between these levels and the emission of different wavelengths of light.
How does an emission spectrum of a gas in a discharge tube differ from a white light spectrum?
It differs by that white light spectrum is continuous and consists of light of all wavelengths. Emission spectrum is not continuous. It consists of bright lines at specific wavelengths, with complete darkness between them.
How can you Distinguish absorption spectrum from emission spectrum?
Emission spectra are bright-line spectra, absorption spectra are dark-line spectra. That is: an emission spectrum is a series of bright lines on a dark background. An absorption spectrum is a series of dark lines on a normal spectrum (rainbow) background.
