Classify each statement about effective nuclear charge, Zeff, as true or false.
In a Be atom, a 1s electron has a greater Zeff than a 2s electron.
Across a period, as Zeff increases, atomic size decreases.
Electrons in a p orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge.
A 1s electron is a Be atom has a smaller Zeff than a 1s electron in a Li atom.
Effective nuclear charge decreases from left to right across a period on the periodic table.
Effective nuclear charge is dependent on the number of electrons present in an atom.
Classify each statement about effective nuclear charge, Z_eff, as true or false. In a Be atom, a 1s electron has a greater Z_eff than a 2s electron. Electrons in a p orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge. Effective nuclear charge decreases from left to right across a period on the periodic table. Across a period, as Z_eff increases, atomic size decreases. A 1s electron In a Be atom has a smaller Z_eff than a 1 s electron in a Li atom. Effective nuclear charge is dependent on the number of electrons present in an atom.
Generally speaking, as you go down a group in the periodic table, there is successively greater shielding of the outer-shell electrons by the inner-shell electrons.
Generally speaking, as you go across a period in the periodic table, the effective nuclear charge (Zeff) increases because each successive element contains more protons in the nucleus than the previous element and the outer electrons are all in the same shell as you go across a period.
Generally speaking, the lighter halogens can be predicted to exhibit greater shielding of the outer-shell electrons by the inner-shell electrons than heavier halogens.
Generally speaking, non-metallic elements have greater effective nuclear charge (Zeff) than metallic elements in the same period.
