That's actually not quite how it works, you're probably going by an outdated model of the atom.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.
Because the nucleus attraction is more to the nearer electrons as the distance of seperation is less. but in higher shells the distance between the electron and the nucleus is more comparitively.Hence they possess high energy i.e. they are more unstable.
Because it requires more energy for an electron to orbit farther away from the nucleus, losing energy makes the electron fall closer to the nucleus since it does have the energy required to stay in its previous, higher-level energy shell.
That has to do with potential energy. It is for the same reason that an object nearer to Earth has less gravitational potential energy. In the case of the atom, the attracting force is the electrostatic force.
because its closer to the nucleus and since theres more protons in the nucleus theyre doesnt need to be more close to it
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"higher energy"
Electrons are arranged around the atomic nucleus forming the electron clouds.
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.
the electrons moving closer to the nucleus have lower energy level.why?AnswerWhen atoms absorb energy, electrons move into higher energy levels, and these electrons lose energy by emitting light when they return to lower energy levels.It's like a sea saw, you go up, you get energy, go back down, lose it.please recommend me :D
The 2s and2p orbitals are on the same energy because for higher elements more protons in the nucleus and hence electrons go closer to the nucleus and as the distance decreases the magnitude of energy increases.
higher energy
"higher energy"
Electrons are arranged around the atomic nucleus forming the electron clouds.
It depends on your definition of high energy. Electrons close to the nucleus have a high positive energy and will require a lot of energy to elevate them to higher orbitals. Electrons far away from the nucleus have the potential to give off a lot of energy falling to inner orbitals.
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.
Antibonding is a bonding in which the electrons are away from the nucleus and which is higher in energy.
No. The electrons nearest the nucleus have the lowest energy. The highestenergy electron is one that's out on its own, not bound to any nucleus.
No. Lower energy levels and their electrons are closer to the nucleus than higher energy levels and their electrons.
the electrons moving closer to the nucleus have lower energy level.why?AnswerWhen atoms absorb energy, electrons move into higher energy levels, and these electrons lose energy by emitting light when they return to lower energy levels.It's like a sea saw, you go up, you get energy, go back down, lose it.please recommend me :D
yes, because they are more attracted to the positively charged protons
farther from the nucleus Answer2: Electrons nearer the nucleus have a higher velocity and thus higher energy EP= -Ze2zc/2r = Zalpha ch/r = -vh/r This is similar to planets nearer the sun move faster mv2=mGM/r.
It's convenient with the atomic model to think of electrons having a certain amount of energy. The amount of energy is quantized, and each orbital has a specific amount of energy associated with it. To go to a lower energy level or orbital an electron would have to give up energy; to get to a higher energy level they would have to absorb a certain amount of energy. Since the nucleus with its positive charge attracts negatively charged electrons it takes work (added energy) to move them away from it. A simplistic view of why they don't collide with the nucleus is that they have too much energy to just spontaneously fall into the nucleus, and that the orbital they occupy is stable in terms of its spatial extents, which do not coincide with the location of the nucleus.