As you move across a period (row) in the periodic table from left to right, how does the electronegativity of the elements generally change?

• A. Electronegativity decreases
• B. Electronegativity increases
• C. Electronegativity first increases, then decreases
• D. Electronegativity remains constant

Answer: (B)

Verified step by step guidance

1. Understand that electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond.
2. Recall that as you move across a period from left to right, the number of protons in the nucleus increases, which increases the effective nuclear charge experienced by the valence electrons.
3. Recognize that the increased effective nuclear charge pulls the electrons closer to the nucleus, making the atom more effective at attracting electrons from other atoms.
4. Note that the atomic radius generally decreases across a period, which also contributes to the stronger attraction for bonding electrons.
5. Conclude that due to the increasing effective nuclear charge and decreasing atomic radius, electronegativity generally increases as you move from left to right across a period.