Multiple Choice
Which of the following options correctly describes the general trends in electronegativity across the periodic table?
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10. Periodic Properties of the Elements
Periodic Trend: Electronegativity
Multiple Choice
Which of the following best helps explain why the electronegativity of sodium (Na) is less than that of chlorine (Cl)?
A
Chlorine is a metal, while sodium is a nonmetal, and nonmetals generally have lower electronegativity.
B
Sodium has a lower effective nuclear charge than chlorine, resulting in a weaker attraction for bonding electrons.
C
Sodium is located further to the right on the periodic table than chlorine, so its electronegativity is lower.
D
Sodium has more valence electrons than chlorine, making it less likely to attract additional electrons.
Verified step by step guidance1
Understand the concept of electronegativity: it is the tendency of an atom to attract bonding electrons toward itself in a chemical bond.
Recall that effective nuclear charge (Z_eff) is the net positive charge experienced by valence electrons, calculated as the actual nuclear charge (number of protons) minus the shielding effect of inner electrons.
Compare sodium (Na) and chlorine (Cl): Sodium has 11 protons and fewer valence electrons, while chlorine has 17 protons and more valence electrons, leading to a higher effective nuclear charge in chlorine.
Recognize that a higher effective nuclear charge means a stronger attraction for bonding electrons, so chlorine attracts electrons more strongly than sodium.
Conclude that the best explanation for the difference in electronegativity is that sodium has a lower effective nuclear charge than chlorine, resulting in a weaker attraction for bonding electrons.
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