Can someone explain the shielding effects The inner core electrons are being att
ID: 716385 • Letter: C
Question
Can someone explain the shielding effectsThe inner core electrons are being attracted by the nucleus,(energy is spent form the protons to bind that electron in that particular space?) so as we go to the outmost shell’ the electron that’s residing in that shell will receive far less of a pull from the nucleus, why is that?
Is it because the energy is reduced because the energy that is being emitted from the nucleus has been reduced by the core electrons, so their will be less of a net attraction from the outer electrons?
Can someone explain the shielding effects
The inner core electrons are being attracted by the nucleus,(energy is spent form the protons to bind that electron in that particular space?) so as we go to the outmost shell’ the electron that’s residing in that shell will receive far less of a pull from the nucleus, why is that?
Is it because the energy is reduced because the energy that is being emitted from the nucleus has been reduced by the core electrons, so their will be less of a net attraction from the outer electrons?
The inner core electrons are being attracted by the nucleus,(energy is spent form the protons to bind that electron in that particular space?) so as we go to the outmost shell’ the electron that’s residing in that shell will receive far less of a pull from the nucleus, why is that?
Is it because the energy is reduced because the energy that is being emitted from the nucleus has been reduced by the core electrons, so their will be less of a net attraction from the outer electrons?
Explanation / Answer
The shielding effect describes the balance between the pull of the protons on valence electrons and the repulsion forces from inner electrons.
Electrons in an atom can shield each other from the pull of the nucleus. This effect, called the shielding effect, describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. The more electron shells there are, the greater the shielding effect experienced by the outermost electrons.
In hydrogen-like atoms, which have just one electron, the net force on the electron is as large as the electric attraction from the nucleus. However, when more electrons are involved, each electron (in the n-shell) feels not only the electromagnetic attraction from the positive nucleus but also repulsion forces from other electrons in shells from 1 to n-1. This causes the net electrostatic force on electrons in outer shells to be significantly smaller in magnitude. Therefore, these electrons are not as strongly bound as electrons closer to the nucleus.
The shielding effect explains why valence shell electrons are more easily removed from the atom. The nucleus can pull the valence shell in tighter when the attraction is strong and less tight when the attraction is weakened. The more shielding that occurs, the further the valence shell can spread out. As a result, atoms will be larger.