The effective nuclear charge experienced by a 1s electron in helium is +1.70.
The effective nuclear charge ##Z_”eff”## is the net positive charge experienced by an electron in a multi-electron atom.
A given electron does not experience a full nuclear charge because the other electrons are sometimes between it and the nucleus and shield it from the nucleus.
The formula for effective nuclear charge is
##Z_”eff” = Z – S##
##Z## is the number of protons in the nucleus, and
##S## is the shielding constant, the average number of electrons between the nucleus and the electron in question.
The American physicist John Slater derived a number of rules to determine the shielding constant.
He found that for electrons in a 1s orbital, the second electron shields the first by 0.30 units.
##Z_”eff” = Z – S = 2 – 0.30 = 1.70##
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