What element has the biggest shielding effect in its atom?

Answer 1

== == == == The screening effect, or shielding effect, is how electrons in the same atom interact with each other. In a single-electron atom (in isolation), the electron is only interacting with the proton; in a multielectron atom, the electrons are both interacting with the proton(s), but also with each other. While electrons are attracted to the protons in the nucleus, they are repelled by the other electrons. This electron-electron repulsion decreases the attractive force of the protons on the electrons.

The shielding effect changes the effective nuclear charge -- effectively decreasing the true nuclear charge. This effect causes atoms to get smaller as you across a period (row) of the Periodic Table, as well as many other periodic trends observed in the periodic table.

See the Web Links and Related Questions for more information about shielding and periodic trends.

--------------------------------------------------------------------------- keep in mind that different orbitals have varying shielding effciencies depending on their shape and symmetry from greatest effect to least s>p>d>f and the effective nuclear charge can be estimated with good approx. by the Slater's Rule where

Z_eff=Z-S Z_eff= effective nuclear charge Z=nuclear charge S=screening (or shielding) factor

the screening factor is calculated by following the directions given at this website

http://intro.chem.okstate.edu/WorkshopFolder/SlaterRule.html

Answer 2

The element with the biggest shielding effect in its atom is Francium, due to the large size of its electron cloud and the increased distance between the nucleus and the outer electrons. This leads to a stronger shielding effect that reduces the attractive force between the nucleus and the outer electrons.

Answer 3

Shielding Effect is a phenomenon observed heavy nuclei element (elements having a big atomic number & Atomic Mass).

It says that the electrons in the outer or remote shells in these elements are not attracted to the nucleus of the element with a force of attraction that is equal to the electrons in the inner shells. Hence these lesctrons are more loosely bound to the nucleus & are free to conduct electricity.

Put simply, the inner electrons 'shield' the nucleus from the outer electrons.

cheers!

Answer 4

In the larger atoms, electrons are filled in the d and f orbitals as well.

The d and f electrons have poor shielding of nuclear charge and hence the outer shell electrons are highly attracted towards the nucleus.

Hence, almost every transition and inner transition elements are of same size and

are smaller than expected.

Answer 5

Going down a column, atomic radius increases because there are more energy levels. Valence electrons feel a weaker attraction to the nuclear charge due to increased electron shielding. There is more electron shielding because there are more core electrons.

Going across a period, atomic radius decreases. Protons are increasing while electrons are added within the same energy level. There is no increase in electron shielding because there is no increase in core electrons. This increase in effective nuclear charge without at increase in electron shielding pulls electrons closer to the nucleus.

Answer 6

The shielding effect of an atom increases as the number of valence electrons become larger. Since, we can deduce that the elements in group 18 have the highest shielding effect with respect to the elements in the particular period.

Answer 7

Electrons are added to the same principal energy level.

Answer 8

more sheilding means that the electrons will not be held as tightly, so they will be farther away from the nucleus and the atmic radius will be larger

Answer 9

A greater shielding effect causes ionisation energy to decrease.

Answer 10

Due to the shielding effect the atomic radius increase down in a group of the periodic table.