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Why there are discontinous spaces between spectrum of hydrogen?
There are spaces in the atomic spectrum of hydrogen because there are discrete energy levels that the electron in the hydrogen atom can be located in. Generally speaking the further away from the nucleus, the higher the potential energy of the electron. When hydrogen gas is excited, the electron can jump up to higher energy levels. When that electron falls back down to a lower energy level, a photon is emitted with an energy equal to the energy difference between the atomic orbital it jumped from and the one it jumped to. Since excited electrons can make a number of different jumps (ex. 4->3, 4->2, 5->3, 5->2, etc) there are a series of photons given off with discrete energies. Each one of these photons has a distinct wavelength (given by the equation E=hf, where E is the energy of the photon, h is planck's constant and f is the frequency of the photon). Each line you see on the spectrum is a photon produced from a different energy jump, with a different wavelength. We are only able to see the photons that emit a wavelength in the visible spectrum (roughly 400-700 nm).
How was Niel bohr model of an atom different from that of Rutherford model of an atom?
According to rutherford an electron jumps from one orbit to other by continueous discharge of energy ( classical thought about energy) while bohr said that electron jumps at once by discharging quanta of energy( quantum view of energy)
What does the electron do when an atom emits a photon?
Atoms actually emit light by reflecting light. I just did a science project on this and when I researched it, atoms take the sun's rays and absorb them. Darker colours, with darker atoms, such as blue, red, and black, lock in more of the sun's rays and lighter colours, with lighter atoms, such as yellow, white, and orange, reflect more of the light and the sun's rays. That's why if you put a black car and a white car next to each other in a parking lot for an hour and you come back and the black car feels hotter than the white car. Atoms also emit light in another way. The electrons in an atoms have certain values of energy, and are not all the same. Scientists think of them as occupying points on a 'ladder' of energy values. When an atom gains energy, for instance being heated such as flames, hot metal and stars, the electrons of the atom increase in energy levels. They will then drop back down the 'ladder' and emit energy as a photon - a single packet of energy. The energy of the photon is equal to the difference in energy between the electrons original energy level and its new level. The higher the drop down the 'ladder' the more energy the electron loses and so the more energy in the emitted photon. This changes it's wavelength in the electromagnetic spectrum. That's why metal first glows red, as it emits the lower red part of the spectrum, and increases to white hot, as it emits all different wavelengths. The combination of colours build up to form the colour white. Very hot stars can even glow blue, only emitting the top end of the spectrum. Each element in the periodic table emits (and absorbs, in the reverse process, reflecting photons of the wrong energy value) different parts of the spectrum, giving us the ranges of colour we see. In 1868, by looking at the parts of the spectrum emitted from the corona of the sun during a total eclipse, Helium was discovered, as it did not match any other element known to man.
What was Niels Bohr's expanation for the observation of atomic spectra?
When a gas is excited in an electrical discharge, light is emitted (this is essentially how neon lamps work). Niels Bohr looked at this emitted light using a spectrograph, which separates different wavelengths of light (just a like a simple triangular prism). Atoms, such as hydrogen or neon, emit very specific patterns of light. When you separate the wavelengths, you see a pattern of very sharp lines of light at only certain wavelengths and not others. In other words, the atoms emit only certain wavelengths of light, resulting in a series of lines when you look at the light through a spectrograph. Bohr looked at these lines and managed to figure out the pattern that determined which wavelengths were observed. He said that the light emitted was due to transitions between energy levels in the atoms, and the wavelength of light corresponded to the energy difference between the two states involved in the transition. In this way, he figured out the equation to predict the spacing between all of the energy levels of any one-electron atom or ion. His model was quite successful, and he was able to predict which lines you would see for things that hadn't even been measured yet (a good test for any theory!). Surprisingly, although he figured out the pattern so well, he didn't actually know what the patterns were really due to. In fact, he had to make assumptions that turned out to be completely false! However, despite these errors (which were corrected when quantum mechanics was developed), the Bohr model of the atom is very useful for many applications. His model does NOT work well for multi-electron atoms/ions, which unfortunately includes the large majority of atoms and ions! You need quantum mechanics for that!
What does potential and kinetic energy have to do with paper airplanes?
It all started when a guy named ken base jumped off a cliff with a flying fox
What is the relationship between the light emitted by an atom and the energies of the electrons in the atom?
Light Energy increases as you move down the period table among the alkali group.
When An electron jumps from energy level 1 to level 2 by absorbing 8 eV what is it when it goes back to energy level 1?
There are no handling or re-stocking charges, and the loan is interest-free. The energy it needed in order to climb from level-1 to level-2 is exactly the same energy it returns to the bank when it goes back to level-1 As it falls back to energy-level-1, it spits out a photon with energy of 8 eV, whereupon everything is back to normal, and energy is conserved.
State in which electrons have jumped to a higher energy level?
state in which electrons have absorbed energy and "jumped" to a higher energy level
What changes happen to the body when it jumped?
ITS An ENERGY CHANGEin this the body gets kinetic energy
Where can we see the potential energy in skydiving?
From the altitude of the airplane when you jumped out.
Why there are discontinous spaces between spectrum of hydrogen?
There are spaces in the atomic spectrum of hydrogen because there are discrete energy levels that the electron in the hydrogen atom can be located in. Generally speaking the further away from the nucleus, the higher the potential energy of the electron. When hydrogen gas is excited, the electron can jump up to higher energy levels. When that electron falls back down to a lower energy level, a photon is emitted with an energy equal to the energy difference between the atomic orbital it jumped from and the one it jumped to. Since excited electrons can make a number of different jumps (ex. 4->3, 4->2, 5->3, 5->2, etc) there are a series of photons given off with discrete energies. Each one of these photons has a distinct wavelength (given by the equation E=hf, where E is the energy of the photon, h is planck's constant and f is the frequency of the photon). Each line you see on the spectrum is a photon produced from a different energy jump, with a different wavelength. We are only able to see the photons that emit a wavelength in the visible spectrum (roughly 400-700 nm).
What type of energy existed before the boy jumped off the platform?
Gravitational potential energy.
How was Niel bohr model of an atom different from that of Rutherford model of an atom?
According to rutherford an electron jumps from one orbit to other by continueous discharge of energy ( classical thought about energy) while bohr said that electron jumps at once by discharging quanta of energy( quantum view of energy)
What is the past tense of jumped?
I jumped You jumped He/She/It jumped We jumped They jumped
Why do atoms emit only certain wavelengths of light?
The electrons in an atom's "electron shell" all have specific energy levels. If you add energy to an atom, the atom will absorb a specific amount of energy, and the electron will jump up to a higher energy level. Each different element has its own energy levels, and it can only absorb energy in specific amounts. (When you add a lot of energy to the atom, the atom becomes ionized, as one or more electrons absorb enough energy to break free of the atom completely, leaving the atom with an unbalanced positive electrical charge.) When those "excited" or jumped-up electrons release the energy, the electron drops back to its previous level, and the atom (or more specifically, the electron) emits a photon, which is a particle of light. Each photon has a frequency or energy that is distinctive to the element and the energy level. Electrons cannot have intermediate energies; they absorb and release exact "packets" or "quanta" of energy. This is how a mass spectrometer works; the operator ionizes a sample of the material that he wants to analyze, and watches the resulting spectrum. Each wavelength of light emitted by the sample corresponds to one specific element.
I just had to have my car jumped. Does using the heat drain the car battery after it has just been jumped?
If it was your car that has been "jumped" then the energy went from your "friends" battery to yours. Your friends battery lost some charge, whilst yours gained some charge. Once the cables were detached - no energy was transferred. No, as long as you do not have the blower motor running.
What is the present perfect tense of jumped?
I/You/We/They have jumped. He/She/It has jumped. she is jumped up and down.
