Effective nuclear charge `(Z_(eff))` is the net attractive force on electrons under consideration and is equal to:
`Z_(eff) = Z - sigma` (nuclear charge - screening constant). `Z_(eff)` or `sigma` is calculated by Slater's formula, as given.
If one electrons is present in the outermst orbit, there will be no screening in that orbital. Each electrons contribute, `0.35` (total electrons minus one electron) present in the outermost shell.
A contribution of `0.85` for each electrons is taken in the `(n - 1)th` shell.
Which of the following statement is wrong?

Effective nuclear charge (Z_(eff)) is the net attractive force on electrons under consideration and is equal to: Z_(eff) = Z - sigma (nuclear charge - screening constant). Z_(eff) or sigma is calculated by Slater's formula, as given. If one electrons is present in the outermst orbit, there will be no screening in that orbital. Each electrons contribute, 0.35 (total electrons minus one electron) present in the outermost shell. A contribution of 0.85 for each electrons is taken in the (n - 1)th shell. The screening constant (sigma) for 4s electron of Mn (Z = 25) will be

Effective nuclear charge (Z_(eff)) is the net attractive force on electrons under consideration and is equal to: Z_(eff) = Z - sigma (nuclear charge - screening constant). Z_(eff) or sigma is calculated by Slater's formula, as given. If one electrons is present in the outermst orbit, there will be no screening in that orbital. Each electrons contribute, 0.35 (total electrons minus one electron) present in the outermost shell. A contribution of 0.85 for each electrons is taken in the (n - 1)th shell. The screening constant (sigma) for 4s electron of Mn (Z = 25) will be

Screening effect is the effect produced by intervening electron between nucleus and valence electrons. They shield the nucleus from valence electron and effective nuclear charge decreases if there is less shielding effect, the effective nuclear charge decreases. Balance electrons are attracted by nucleus and repelled by other electrons. Net attractive force on electron under consideration =Z- sigma = (Nuclear charge screening effect) which is Slater's formula for screening constant. If one electron is present in outermost orbit, there will be no screening in that orbital. Each electron contributes 0.35 (total electrons minus 1) present in outermost shell. In penultimate energy level, electrons contribute 0.85. A contribution of 1.0 is from remaining electrons (present in last but one energy level). The effective nuclear charge for 4s electrons of Zn will be

Screening effect is the effect produced by intervening electrons between nucleus and valence electrons . They shield the nucleus from valence electron and effective nuclear charge decreases if there is less shielding effect the effective nuclear charge decreases Valence electrons are attracted by nucleus and repelled by other electrons. Net effective force on electrons under consideration = Z-sigma = (Nuclear charge -screening effect ) slaters formula for screening constant. If one electron is present in outermost orbit there will be no screening in that orbital. Each electrons contributes 0.35 (total electrons minus 1) present in outermost shell. In penultimate energy level electrons contribute 0.85. A contribution of 1 is from remaining electrons (present in last but one energy level) The effective nuclear charge for 4s electrons of Zn will be

Effective nuclear charge (Z_(eff)) for a nucleus of an atom is defined as

Effective nuclear charge (Z_(eff)) for a nucleus of an atom is defined as

Z_(eff) for 4s electron in _(30)Zn I s:

According to Slater's rule , correct order of Z_("eff") on valence shell electron is :