![]() We can go ahead and plug in m times v squared over r. We know that the centripetal acceleration is equal to V squared over r. This will be the centripetal acceleration since we're talking aboutĪ centripetal force. ![]() Force is equal to mass times acceleration using Newton's second law. Same magnitude of charge as the proton but it's negative. q2 I said was the charge in the electron, and the electron has the We'll say is e for now, so elemental charge. q1 I said was the charge on the proton, and the charge in the proton Q2, which we'll say is the charge on the electron. This is Coulomb's law, the electric force is equal to K, which is a constant, times q1, which is one of the charges. We can find the electricįorce by using Coulomb's law. This is the electricįorce that's causing the electron to move in a circle. In this case we're talkingĪbout the electric force. This negatively chargedĮlectron is gonna feel a force towards the center of the circle. It's going to be attracted to the nucleus. The velocity of thatĮlectron at this point is tangent to the circle. Going back to the electron here, let's say the electron is going around counter-clockwise. What we're going to calculate in this video. If you don't like physics youĬan jump to the next video where I show you the result of But I should warn you that this is a lot of physics in this video as well. We're actually gonnaĭo that in this video. It's useful to calculate, say for example we can calculate Even though the Bohr model is not reality it is useful for a concept of the atom. So I draw in a positive charge here and a negatively chargedĮlectron orbiting the nucleus, so kind of like the In the Bohr model of the hydrogen atom we have one proton in the nucleus. Rather than take a Ptolemy approach and add more and more conditions onto the hypothesis to explain the more complicated cases, the Bohr model was replaced with a fuller quantum explanation, in a sense like Copernicus replace the Ptolemaic hypotheses of a geocentric system. It still provides a good basis for understanding effects, but in more complex atoms it did not work out. Like many hypotheses, it worked very well to describe the phenomena in a set of instances, but it failed to explain the in the broader and more general cases. He needed to express it mathematically and compare that mathematical result with the observations of the energy emissions. It was an ingenious insight, but a hypothesis is an educated guess based on the observations. So his hypothesis involved asserting that the electrons were in an orbital distance of 1 radius, or 2 radii or 3 radii from the nucleus. So, based on these he took an insightful hypothesis that the orbits that the electrons were in were orbits that were in incremental, or quantum if you prefer, steps. He and his mentor, Rutherford, had already conceived of the "orbital model" of atoms (as opposed to the earlier plum pudding model where all electrons and and protons are mixed together in the nucleus like raisins in a pudding). Bohr and the science community at the time already knew that energy from the H atom was emitted at specific, discrete values (referred to as the wavelength or frequency of the emitted light energy).
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