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The Bohr model of the atom was able to explain the Balmer series because?
The Bohr model of the atom was able to explain the Balmer series by proposing that electrons orbit the nucleus in quantized, discrete energy levels. The transition of electrons between these levels corresponds to the emission of light at specific wavelengths, which gives rise to the spectral lines observed in the Balmer series.
What technology did Bohr use to discover the electron?
The only technology Bohr needed to develop his model for the atom was a spectrometer, which, in the mid-1800s, revealed the emission lines of hydrogen. In 1885, Johann Balmer developed a mathematical formula (the Balmer Series) that fully described these lines, but nobody could explain why it worked. Neils Bohr combined the quantum ideas of Max Planck and Albert Einstein with the atomic model proposed by Ernest Rutherford, and developed an atomic model from which the Balmer Series could be derived.
If an electron in a hydrogen atom relaxes to the second energy level emitting a photon of wavelength 410.2 nm what higher energy level did it start at?
There are actually two ways to do this. I'll explain how to use Rydberg's formula, though, because it's significantly simpler to use. Rydberg's Formula states: 1/(wavelength)=R (1/n1^2-1/n2^2) R= 1.097x10^7m^-1 (this is Rydberg's constant so you can look this up) n1=nfinal (or n=2 in this problem) n2=ninitial (what we are looking to find) wavelength=lambda=3.97x10^-7m Set up the problem: 1/3.97x10^-7m=(1.097x10^7m^-1)*(1/2^2-1/n^2) .2296=1/4-1/n^2 1=.02n^2 n^2=50 n=~7 Alternatively you could have used Bohr's model but that would take two formulas and a lot more work for the same answer (using Bohr's model is simply working backwards from what it is typically used for).
What does a hydrogen atom transitioning from the 2nd to the 1st excited state produce?
A hydrogen atom transitioning from the 2nd to the 1st excited state produces a photon of ultraviolet light. This ultraviolet light has a specific wavelength corresponding to the energy difference between the two states.
Can an electron jump from sixth shell to second shell?
No, electrons cannot jump from the sixth shell to the second shell in an atom. Electrons fill shells in a specific order based on their energy levels, and they follow certain rules and restrictions regarding their movements within an atom. Jumping from the sixth shell to the second shell would violate these principles.
What color is the wavelength of light in the Balmer series that results from the transition of an electron from n 3 to n 2?
The wavelength of light in the Balmer series resulting from the transition of an electron from n=3 to n=2 corresponds to a color in the visible spectrum. Specifically, this transition emits light at a wavelength of approximately 656 nanometers, which falls within the red part of the spectrum. This transition is often referred to as the H-alpha line.
What color is the wavelength of light in the Balmer series that results from the transition of an electron to N equals 2?
There are 4 Balmer lines with wavelengths in the visible region. They are red, aqua and two shades of violet. Other Balmer lines are in the ultraviolet. The red line corresponds to the transition from n = 3 to n = 2, the subsequent ones are from the 4, 5 and 6 levels to n = 2.
What is the wavelength of the hydrogen atom in the 2nd line of the Balmer series?
The wavelength of the hydrogen atom in the 2nd line of the Balmer series is approximately 486 nm. This corresponds to the transition of an electron from the third energy level to the second energy level in the hydrogen atom.
What is the shortest wavelength radiation in balmer series?
The shortest wavelength radiation in the Balmer series is the transition from the n=3 energy level to the n=2 energy level, which corresponds to the Balmer alpha line at 656.3 nm in the visible spectrum of hydrogen.
What is the maximum wavelength of balmer series?
The Balmer series is a series of spectral lines in the hydrogen spectrum that corresponds to transitions from energy levels n > 2 to the n=2 level. The longest wavelength in the Balmer series corresponds to the transition from n = ∞ to n = 2, known as the Balmer limit, which is approximately 656.3 nm.
To which series would the emitted light belong if an electron in a hydrogen atom underwent a transition from level n 5 to level n 1?
The electron transition from n=5 to n=1 in a hydrogen atom corresponds to the Balmer series, specifically the Balmer-alpha line which is in the visible part of the spectrum.
What is ratio of maximum and minimum wavelength of balmer series?
5:9 ,i am not sure (;
Spectral lines of the Lyman and Balmer series do not overlap Verify this statement by calculating the longest wavelength associated with the Lyman series and shortest wavelength associated with the B?
Well, the different series represent different electronic transitions. But there is an important equation, the Rydberg formula which describes all of them.. I think you've learned of it since you mention the n values. This lead to the Bohr model of the hydrogen atom, which explained _why_ you had these levels.Or, almost. See, it turned out that those lines were not actually single lines, but several lines very close together.. And so they had to add more variables to describe how these levels-within-levels fit together.. and the answer to that eventually came from quantum mechanics.
What is the line spectrum of the hydrogen atom?
The line spectrum of the hydrogen atom consists of discrete lines at specific wavelengths corresponding to different electron transitions within the atom. These lines are a result of the energy differences between electron orbitals in the atom. Each line represents a specific electron transition, such as the Lyman, Balmer, and Paschen series.
What is the Balmer Series?
The Balmer series is a section of the hydrogen atomic emission line spectrum. They show the wavelengths of light emitted when electrons transition back to the n = 2 quantum level.
Is Balmer series only present in hydrogen atom?
No, the Balmer series is observed in hydrogen-like atoms, which have one electron orbiting a nucleus. It consists of the spectral lines produced when the electron transitions from higher energy levels to the second energy level. Other atoms with similar electron configurations can also exhibit Balmer-like series in their spectra.
What are the colours in the balmer series?
The Balmer series consists of visible spectral lines emitted by hydrogen atoms when electrons transition from higher to lower energy levels. The colors in the Balmer series include red (656.3 nm), blue-green (486.1 nm), and violet (434.0 nm) wavelengths.
