* Electronegativity: Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. The higher the electronegativity, the stronger the attraction.

* Periodic Trends: Electronegativity increases as you move:

* Across a period (left to right): This is because the number of protons in the nucleus increases, pulling the electrons more strongly.

* Up a group (top to bottom): This is because the outermost electrons are closer to the nucleus, making the attraction stronger.

Let's look at the elements:

* Boron (B): Located in Group 13 (3A) and Period 2

* Oxygen (O): Located in Group 16 (6A) and Period 2

* Sulfur (S): Located in Group 16 (6A) and Period 3

Conclusion:

* Oxygen (O) has the greatest attraction for electrons. It's in the same period as Boron but further to the right, meaning it has more protons and a stronger pull on electrons.

* Sulfur (S) is in the same group as Oxygen but a period lower. This means it has a weaker attraction for electrons compared to Oxygen.

Therefore, Oxygen (O) has the greatest attraction for electrons among Boron, Oxygen, and Sulfur.