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
First off, it's important to remember that electronegativity is an atomic property within a molecule, not in its free form. If you think of it like that, it makes complete sense that the further an atom's valence electrons are from the nucleus, the weaker the electromagnetic bond between it and the nucleus, and therefore the less likely it will want to take in another electron, ie., lower electronegativity. The valence electron's own electromagnetic field repulses other electrons, and the further they are from the nucleus, the stronger the repulsive force is compared to the nucleus' attractive force.
The negative ionic radius is larger than the neutral atomic radius
The atomic radius is the distance from the nucleus of an atom to the outermost orbital of electron.
C.their atomic radius is small D.layers of electron shells shield the protons' attractive force fewer layers of electron shells create less shielding of the protons' attractive force
the positive ionic radius is smaller than the neutral atomic radius
Lithium has a larger atomic radius than hydrogen.
In rubidium, having a larger atomic radius, the attraction force between the atomic nucleus and and the electron from outermost shell is lower.
The negative ionic radius is larger than the neutral atomic radius
The atomic radius is the distance from the nucleus of an atom to the outermost orbital of electron.
The relation between electron affinity and atomic radius is inversely proportional.
C.their atomic radius is small D.layers of electron shells shield the protons' attractive force fewer layers of electron shells create less shielding of the protons' attractive force
the positive ionic radius is smaller than the neutral atomic radius
Atomic Radius means the size of the atoms, the distance from the atomic nucleus to the outermost electron orbital.
The shielding effect is when nearer electrons block farther electrons from getting closer to the protons, and hence, the nucleus. If the farthest electrons were able to get closer, the atomic radius would decrease because those electrons wouldn't be as far out as they originally were.
Lithium has a larger atomic radius than hydrogen.
The element krypton's atomic radius is 189 pm. This is a measurement of its atom sizes or the distance between the electron cloud and the nucleus.
This is because of the fact atomic radius is the distance of the outermost electron to the nucleus thus as more electrons are added the distance increase (which cause atomic radius to change)
The atomic radius of cation is smaller than its parent atom.This is because of the removal of electron from the parent atom.