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The path that an electron travels around a nucleus is called an?
The "orbit" of an electron is the energy level that electron happens to be in. When we get to particles the size of electrons, the concept of electrons following a specific path begins to fall apart. We can no longer talk about an electron being somewhere and having a specific velocity; we can only talk about the PROBABILITY of an electron being at a specific place, as well as the most likely velocity at a given orbit.
What keeps an electron in motion around the nucleus to which it is attracted?
Actually, its more of a matter of why don't they fall into the nucleus and stop moving. You see, electrons are very chaotic particles that always move around because of the kinetic energy (kinetic energy is the energy of a moving object) they carry, and at a subatomic scale it is very difficult, and practically impossible, to "stop" a particle i.e. reduce its kinetic energy to zero. So you see, when electrons are bound by electrostatic forces to atomic nuclei, they can't fly away because of the attraction between the protons of the nucleus and them, but they also can't just stick to said nuclei because they still have kinetic energy which keeps them moving.A simple analogy is spinning a string with a small stone tied to the opposing end. The stone spins around the opposite end of the string because it is bound to that point by the string, but it can't fall towards it because it has a lot of kinetic energy that's trying to make it fly away.Hope this was useful.
Where does the coagulation tube fall in the order of draw if no blood cultures are needed?
First
What season is after Winter?
After Winter is Spring. There are four seasons (in cyclical order): Winter, Spring, Summer, Fall.
Why do skydivers usually fall with their arms and legs spread out?
The spreading of the arms and legs slows the fall and gives the skydiver more control of the fall.
Why doesn't the electron fall into the nucleus?
The electron does not fall into the nucleus because of the electromagnetic force. This force between the positively charged nucleus and the negatively charged electron keeps them in orbit around each other, creating a stable structure within an atom.
Why electron does not fall in nucleus to attack towards proton?
awaa
What do we mean when we say a nucleus has undergone an electron capture process?
You will recall that electrons orbit the nucleus of an atom (or in quantum mechanical terms, they surround the nucleus as a cloud). Under some circumstances, one of those orbiting electrons can fall into the nucleus, where it will react with a proton and convert it into a neutron. This is an electron capture process.
Why electrons near the nucleus having less energy as that of higher shells?
That's actually not quite how it works, you're probably going by an outdated model of the atom. It is true that the probability of finding the electron at a larger distance from the nucleus tends to be larger for electrons with higher energy... the reason why should be fairly obvious: they have more energy to overcome the electromagnetic attraction between the (negative) electron and the (positive) nucleus.
What is the force thea holds an electron to an atom?
The electromagnetic force (protons are positive and electrons are negative, so they attract), which is manifested into Coulomb's force of attraction. The reason that electrons will not fall into the nucleus is due to the electron's energy; it is moving fast enough to not collide with the nucleus.
Why does the outer most electron contain the highest energy?
Due to the fact that it's the farthest away, it has the largest (albeit absolutely tiny) distance to fall to the nucleus, making it have the most potential energy. Similar to rolling a ball off a chair or rolling it off a roof. The farther away, the more potential energy.
The path that an electron travels around a nucleus is called an?
The "orbit" of an electron is the energy level that electron happens to be in. When we get to particles the size of electrons, the concept of electrons following a specific path begins to fall apart. We can no longer talk about an electron being somewhere and having a specific velocity; we can only talk about the PROBABILITY of an electron being at a specific place, as well as the most likely velocity at a given orbit.
When electrons gain additional energy do they move farther away from the nucleus?
In general, electrons farther from the nucleus will have more energy than electrons closer in. These "outer" electrons are said to be in higher Fermi energy levels, and they have more kinetic energy than the electrons in lower orbitals. Consider that electrons give up energy to "fall into" closer orbitals, and they will, in general, have less energy than the outer electrons. A consequence of the idea that there is less energy binding outer electrons to that nucleus is that it takes less energy to remove that outer electron from an atom. These are the so called ionization energies of the atom's electrons. And when the electron is in a higher orbital, it has a lower ionization energy. It can be removed more easily. As we attempt to remove more electrons from that atom, it takes progressively more and more energy as we move inward removing electrons.
Using heisenberg's uncertainity principle prove the non existence of the electron inside the nucleus?
The Heseinberg's Uncertainty Principle states that you cannot know the position and momentum of a particle simultaneously. More rigorously stated, the product of the uncertainty of the position of a particle (Δx) and the uncertainty of its momentum (Δp) must be greater than a specified value: ∆x∆p ≥ (h/4π) Now, as the electron approaches the nucleus, it's uncertainty in position decreases (if the electron is 10nm away from the nucleus, it could be anywhere within a spherical shell of radius 10nm, but if the electron is only 0.1nm away from the nucleus, that area is greatly reduced). According to the Heisenberg uncertainty principle, if you decrease the uncertainty of the electrons position, the uncertainty in its momentum must increase. This increased momentum uncertainty means that the electron will be moving away from the nucleus faster, on average. Put another way, if we do know that at one instant, that the electron is right on top of the nucleus, we lose all information about where the electron will be at the next instant. It could stay at the nucleus, it could be slightly to the left or to the right, or it could very likely be very far away from the nucleus. Therefore, because of the uncertainty principle it is impossible for the electron to fall into the nucleus and stay in the nucleus. In essence, the uncertainty principle causes a sort of quantum repulsion that keeps electrons from being too tightly localized near the nucleus.
Why do electrons and planets spin instead of just falling into the sun or nucleus?
Electrons in orbit around a nucleus, and planets in orbit around the sun both have energy which keeps them in orbit. In the case of a planet, that energy is in the form of angular momentum. In the case of an electron the energy is a form of electromotive force. In either case, if the energy is not great enough to maintain the orbit, the planet or electron will fall out of orbit. This is not often seen in the case of planets, but is fairly common in the case of electrons; when an electron falls into the nucleus, it causes a form of radioactive decay.
Which water fall?
The one closer to you...
Why do electrons not spiral into the nucleus?
No one knows. The fact that it doesn't has been the source of much of the uncertainty principal & quantum mechanics. One thing you should know is that the electron is NOT a tiny planet spinning around the nucleus. In fact the "stuff" of electrons is NOT the "stuff" of the nucleus (quarks) ... maybe they repel each other, maybe they just can't be in the same place.
