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How can the Bohr model be used to explain the line spectrum for hydrogen?
Niels Bohr explained the line spectrum of the hydrogen atom by assuming that the electron moved in circular orbits and that orbits with only certain radii were allowed. The orbit closest to the nucleus represented the ground state of the atom and was most stable; orbits farther away were higher-energy excited states.
How does the Bohr model explain that each element has a unique emission spectrum?
In the Bohr model, electrons can exist only in certain energy levels surrounding the atom. When electrons jump from a higher energy level to a lower one, they emit light at a wavelength that corresponds to the energy difference between the levels. The energy levels in each atom are unique.
What did the Bohr model explain?
In 1913 Bohr proposed his quantized shell model of the atom to explain how electrons can have stable orbits around the nucleus. The energy of an electron depends on the size of the orbit and is lower for smaller orbits. Radiation can occur only when the electron jumps from one orbit to another.
How does the Bohr model explain different colors of light being emitted by different elements when heated in a flame?
The Bohr model says that electrons exist only at certain allowed energy levels. When you heat an atom, some of its electrons are “excited* to higher energy levels. The different mix of energy differences for each atom produces different colours. Each metal gives a characteristic flame emission spectrum.
Why do hydrogen atoms have line spectrum?
Any given element therefore has both a characteristic emission spectrum and a characteristic absorption spectrum, which are essentially complementary images. Figure 7.3. 6 Absorption and Emission Spectra. Absorption of light by a hydrogen atom.
What do you mean by line spectrum of hydrogen?
The emission spectrum of hydrogen or line spectrum of hydrogen is produced when hydrogen gas is taken in the discharge tube and the light emitted on passing electric discharge at low pressure is examined with a spectroscope. It is found to consist of a large number of lines that are grouped into different series.
How did Bohr explain the line spectrum of hydrogen?
To explain the line spectrum of hydrogen, Bohr assumed that electrons in hydrogen atoms move in circular orbits around the nucleus, but this assumption posed a problem. According to classical physics, a charged particle (such as an electron) moving in a circular path should continuously lose energy.
What is Bohr’s model of the atom?
Here is an illustration of Bohr’s atomic model; As n gets larger, the size of the orbit and the energy of the electron gets larger as well, but the energy of the electron is restricted to certain energy levels called the principal quantum number, n.
What are the limitations of the Bohr model?
Limitations of the Bohr Model Although the Bohr model explains the line spectrum of the hydrogen atom, it cannot explain the spectra of other atoms, except in a crude way. Bohr also avoided the problem of why the negatively charged electron would not just fall into the positively charged nucleus by simply assuming it would not happen.
What is the origin of the atomic line spectrum?
• electrons are allowed to higher orbit with an input in energy. What is the origin of the Atomic Line spectrum? The line emission line spectrum results from electrons dropping from higher energy level to lower energy levels.