Less
The addition of electron shells results in more shielding of electrons from the nucleus.
As you move down a group in the periodic table, shielding increases because there are more electron shells surrounding the nucleus. These additional electron shells act as a barrier, reducing the attraction between the nucleus and outer electrons, thus increasing shielding.
•The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. •It is also referred to as the screening effect or atomic shielding. •Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons. They are called "shielding" electrons because they "shield" the valence electrons from the force of attraction exerted by the positive charge in the nucleus. Also, it has trends in the Periodic Table
Electrons are found in electron shells surrounding the nucleus of an atom. They move rapidly within these shells, which are composed of energy levels that determine the electron's distance from the nucleus.
The effective nuclear charge of an atom is primarily affected by the number of protons in the nucleus and the shielding effect of inner electron shells. As electrons in inner shells shield outer electrons from the full attraction of the nucleus, the effective nuclear charge felt by the outer electrons is reduced.
The addition of electron shells results in more shielding of electrons from the nucleus.
less
As you move down a group in the periodic table, shielding increases because there are more electron shells surrounding the nucleus. These additional electron shells act as a barrier, reducing the attraction between the nucleus and outer electrons, thus increasing shielding.
•The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. •It is also referred to as the screening effect or atomic shielding. •Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons. They are called "shielding" electrons because they "shield" the valence electrons from the force of attraction exerted by the positive charge in the nucleus. Also, it has trends in the Periodic Table
An electron in a phosphorus atom would experience the greatest shielding in the 3s orbital. This is because electrons in inner shells provide greater shielding than those in outer shells, and the 3s orbital is closer to the nucleus compared to the higher energy orbitals.
Electrons surround the nucleus of an atom in patterns called electron shells.
Electrons are found in electron shells surrounding the nucleus of an atom. They move rapidly within these shells, which are composed of energy levels that determine the electron's distance from the nucleus.
Shielding actually reduces ionization energy. Let's look at some atomic structure and see why. Electrons form shells around an atomic nucleus. The inner electrons shells shield the outer electrons shells and reduce the affect of the nuclear "pull" on those outer electrons. The shielding provided by the inner electrons means it will take less energy to free outer electrons from their orbitals, and thus the ionization energy of an outer electron is reduced by the effects of shielding.
The effective nuclear charge of an atom is primarily affected by the number of protons in the nucleus and the shielding effect of inner electron shells. As electrons in inner shells shield outer electrons from the full attraction of the nucleus, the effective nuclear charge felt by the outer electrons is reduced.
The K shell is closest to the nucleus and has the lowest energy level of all electron shells. Electrons in the K shell experience a stronger electrostatic attraction to the positively charged nucleus, which results in better shielding of the nucleus compared to electrons in higher energy shells.
The electrons in the atom surround the nucleus, and the higher the atomic number of the element the more electrons there are. Unless it is ionised, there will be an equal number of protons in the nucleus and electrons surrounding the atom. Ideas of how the electrons are arranged have evolved from imagining them to be in orbit around the nucleus, like a small solar system, to modern ideas of quantum physics where it is best to imagine them as an electron 'cloud'. However the idea of electron shells is still useful, this is as imagined by Bohr in the twenties of the last century, where concentric shells contain fixed numbers of electrons according to strict rules on their composition. Your query on 'electron shielding' is probably to do with these electron shells, and the more shells there are determines the effective size of the atom. You can read more in the link below
Electron shells, orbitals, and sub-orbitals.