Shielding example sentences

As a result, the valence electron experiences a net positive charge which is less than the actual charge of + In general, shielding is effective when the orbitals in the inner shells are completely filled.Small decrease in ?iH from Si to Ge to Sn and slight increase in ?iH from Sn to Pb is the consequence of poor shielding effect of intervening d and f orbitals and increase in size of the atom.The effective nuclear charge experienced by a valence electron in an atom will be less than the actual charge on the nucleus because of shielding or screening of the valence electron from the nucleus by the intervening core electrons.As we go down a group, the outermost electron being increasingly farther from the nucleus, there is an increased shielding of the nuclear charge by the electrons in the inner levels.Therefore, it is easier shielding or screening of the valence electron from the nucleus by the intervening core electrons.In this case, increase in shielding outweighs the increasing nuclear charge and the removal of the outermost electron requires less energy down a group.As we go down a group, the outermost electron being increasingly farther from the nucleus, there is an increased shielding of the nuclear charge by the electrons in the inner levels.However, down the group, due to poor shielding effect of intervening d and f orbitals, the increased effective nuclear charge holds ns electrons tightly (responsible for inter pair effect) and thereby, restricting their participation in bonding.In this case, increase in shielding outweighs the increasing nuclear charge and the removal of the outermost electron requires less energy down a group.Thus, across a period, increasing nuclear charge outweighs the shielding.When we move from lithium to fluorine across the second period, successive electrons are added to orbitals in the same principal quantum level and the shielding of the nuclear charge by the inner core of electrons does not increase very much to compensate for the increased attraction of the electron to the nucleus.As a result, the valence electron experiences a net positive charge which is less than the actual charge of + In general, shielding is effective when the orbitals in the inner shells are completely filled.Thus, across a period, increasing nuclear charge outweighs the shielding.When we move from lithium to fluorine across the second period, successive electrons are added to orbitals in the same principal quantum level and the shielding of the nuclear charge by the inner core of electrons does not increase very much to compensate for the increased attraction of the electron to the nucleus.