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.
That is quite correct. Energy added to an electron becomes potential energy, in the form of the increased distance from the nucleus. This is very similar to what happens if you lift an object to a higher altitude. The object can fall, and will release energy by falling (for example, water falling through a turbine can generate electricity). Electrons are attracted to the nucleus, so when they move closer to the nucleus, they are in effect falling to a lower energy level. Add energy and they are elevated to a higher energy level. Add enough energy and they leave the atom entirely (in other words, they are ionized).
The kinetic energy of electrons is higher in orbitals near the nucleus but potential energy of electrons is higher in orbitals far away from nucleus.
No, as electrons tend to move away from the nucleus there energy increases
No, just the opposite. The farther from the nucleus, the greater energy it has.
An electron with enough energy can break free of the nucleus and sail away
on its own.
Yes. Higher orbitals have greater energy.
Yes
"higher energy"
Going down a group, the number of valence electrons remains the same, but these electrons get farther and farther away from the nucleus. Thus, they are not as tightly held and the ionization energy decreases. Moving from left to right along a period, the electrons are the same distance from the nucleus, but the number of protons are increasing in the nucleus, thus holding those electrons more tightly. Thus, the ionization energy increases.
To determine this look at the periodic table. The larger the atom, the farther its valence electrons are from the nucleus. Therefore, potassium's valence electrons have the highest energy.
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
Electrons are arranged around the atomic nucleus forming the electron clouds.
higher energy
"higher energy"
Because as you go down a group, with each additional period, an additional energy level is added. Each additional energy level is farther from the nucleus than the previous energy level.
In general, electrons farther from the nucleus will have more energy than electrons closer in.
It is because when you move down, the number of electrons increases. When the number of electrons increases, it calls for more energy levels to fit these electrons.With each additional period, an additional energy level is occupied. This additional energy level is farther from the nucleus than the previous energy level, so the atoms increase in size.
You must be thinking of electrons in shells surrounding the nucleus. The quantity getting bigger is therefore the diameter of the electrons orbit.
Ionization energy decreases down a group because with each additional period, there is an additional energy level, so the outermost electrons are farther away from the positive charge of the nucleus, so they are not held as tightly. The further away the valence electrons are from the nucleus, the less energy is required to remove an electron, so the ionization energy decreases.
The farther an electron is from the nucleus, the greater its energy.
Going down a group, the number of valence electrons remains the same, but these electrons get farther and farther away from the nucleus. Thus, they are not as tightly held and the ionization energy decreases. Moving from left to right along a period, the electrons are the same distance from the nucleus, but the number of protons are increasing in the nucleus, thus holding those electrons more tightly. Thus, the ionization energy increases.
it has to do with quantum numbers N,L, and M
To determine this look at the periodic table. The larger the atom, the farther its valence electrons are from the nucleus. Therefore, potassium's valence electrons have the highest energy.
With each additional period, there is an additional energy level, which means that the outermost electrons are farther away from the nucleus of the atom. This means that the attractive force of the positively charged nucleus is less, so it takes less energy to remove an electron from an atom in the third energy level than it does from an atom in the second energy level. Therefore, the elements in the third period have lower ionization energies than elements in the second period.