MODELO ATÔMICO DE BOHR | Resumo de Química para o Enem

📚 Free e-book with the most frequently tested topics in Math and Natural Sciences on the ENEM exam: http://bit.ly/35OYaeg 🎓 Free ENEM Course: https://goo.gl/2rebsa 📑 Complete Summary: https://goo.gl/9pyV72 ✔️ Practice Test on Atomic Models: https://bit.ly/3kX56f4 Subscribe to the channel to receive everything about the ENEM exam 100% FREE https://bit.ly/37WGBZi /// ABOUT THE VIDEO The model proposed by Rutherford was unable to elucidate an important question: how could negatively charged electrons move around a positive nucleus without losing energy and colliding with it? (at that time it was already known that charges of opposite signs attract each other). Niels Bohr's ideas, supported by Rutherford, resulted in an improved model for the structure of the atom. Let's see what the fundamental principles of this model were: • Electrons occupy specific energy levels or electron shells; • An electron cannot have zero energy, that is, be stationary in the atom; • In each shell, the electron has constant energy: the closer to the nucleus, the lower the electron's energy relative to the nucleus, and the farther away, the higher its energy; • To move from a lower energy level to a higher one, the electron absorbs an appropriate amount of energy. When making the reverse journey, it releases energy. The amount absorbed or released by an electron corresponds exactly to the difference between one energy level and another. In this lesson, Professor Sobis explains Bohr's atomic model in more detail. Questions? Leave them in the comments. ;) ⏱ TIMESTAMPS / TOPICS 00:21 to 1:09 - Rutherford's atomic model had a problem: it stated that the nucleus was positive and the electrons negative. If opposites attract, how come the electrons didn't collide with the nucleus? It was Bohr who solved this problem. 1:10 to 2:17 - By studying some quantum physics, proposed by Max Planck, Bohr realized that there were energy levels around the nucleus. Each level had a defined energy, which held the electron. He called the levels letters, from K to Q. 2:18 to 4:29 - The electron could also jump from one level to another. If an electron is in the M level, for example, and wants to move to the outermost level (N), it must absorb energy. Upon reaching the N shell, it will be very energetic and will not want to remain there; that is, it will want to return to the M shell. Upon returning, it releases the absorbed energy in the form of a photon. Depending on the wavelength of the emitted photon, there is a color to the light generated. An example of this is fireworks. 4:30 to 5:06 - He also discovered how many electrons fit in each shell. K = 2; L = 8; M = 18; N = 32; O = 32; P = 18; Q = 8. 🔴 ALSO WATCH Dalton's Atomic Model https://bit.ly/3aJcru1 Thomson's Atomic Model https://bit.ly/3aHK6UZ Rutherford's Atomic Model https://bit.ly/3hAeHGO ❤️ SOCIAL MEDIA INSTA @cursoenemgratuito TWITTER @enemgratuito FACE /cursoenemgratuito/ /// SO, WHAT IS THE FREE ENEM COURSE? We are a channel with completely free classes on the topics that most frequently appear on the ENEM and university entrance exams. We emerged to democratically share content and information about the ENEM, helping you get into the college of your dreams ♥ We also have a website with written lessons, questions, and a study plan to help you organize yourself! Let's study together? 🎓 ACCESS OUR 100% FREE COURSE FOR THE ENEM EXAM https://goo.gl/2rebsa Intro music: "Summer" - Royalty Free Music from Bensound