Chemistry Regents Practice Test

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Prepare for the Chemistry Regents Exam with essential questions and detailed explanations. Study via flashcards and multiple-choice questions to ensure exam readiness!

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Which atom demonstrates the weakest attraction for electrons when bonded to hydrogen?

Oxygen
Nitrogen
Sodium
S atom

The correct answer is: S atom

When considering the attraction of an atom for electrons in a bond with hydrogen, the concept of electronegativity is critical. Electronegativity is a measure of how strongly an atom attracts electrons in a chemical bond. In this context, sulfur (S) has a lower electronegativity compared to oxygen, nitrogen, and sodium. Oxygen is the most electronegative element among the choices, followed closely by nitrogen. Sodium, being a metal, has a very low electronegativity and tends to lose electrons rather than attract them. However, sulfur's electronegativity is still lower than that of hydrogen and is less than that of oxygen and nitrogen, making it less capable of attracting bonding electrons compared to those elements. Thus, when sulfur forms a bond with hydrogen, it exerts the weakest attraction for the shared electrons in comparison to the other elements listed. This is why sulfur is identified as demonstrating the weakest attraction for electrons when bonded to hydrogen.