This comment is not properly reflected in Figure 2.6.1. Specifically, Figure 2.6.1 makes it appear that all n=3 electrons, whether s, p, or d, will shield at 0.35. While the table calls out that l less than the probe electron value (ie l=2 for 3d electron) receives a shielding constant of 1 (ie 3s and 3p electrons) even though the n value is the same for 3s, 3p, and 3d electrons.

In Exercise 2.6.1 I think for the 4p electron in bromine this value should be 6, not 4, as there are six electrons interacting with the probe electron in the n = 4 shell (4s2,4p5). See calculation in Example 2.6.1 for nitrogen 2p electron for reference.

I'm skeptical that the listed values for the atomic radii are correct. The van der Waals radius for fluorine is 135 pm. If you look at the covalent radius instead, it would be 70 pm (based on Fig 4.2.2.8 in this article). In addition, the atomic radius of boron should be larger than the atomic radius of beryllium because of p orbital occupation. Perhaps the figure is just mislabeled? (Also triangles is misspelled in the figure caption).

Source: https://pubchem.ncbi.nlm.nih.gov/ptable/atomic-radius/