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-
$Z _{eff}=Z-S$
where,
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.
$Z _{eff}=Z-S=2- 0.30-1.70$
Hence, the correct option is B.