Multiple Choice
As you move from left to right across a period (row) on the periodic table, how does electronegativity generally change?
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10. Periodic Properties of the Elements
Periodic Trend: Electronegativity
Multiple Choice
Which of the following best explains why smaller atoms can more easily attract electrons in a chemical bond?
A
Smaller atoms have more electron shells, which shield the nucleus and increase attraction.
B
Their outer electrons are farther from the nucleus, making it easier to attract additional electrons.
C
They have more protons, which always increases electronegativity regardless of atomic size.
D
Their valence electrons are closer to the nucleus, resulting in a stronger electrostatic pull on bonding electrons.
Verified step by step guidance1
Understand that electronegativity is the ability of an atom to attract electrons in a chemical bond.
Recognize that atomic size affects electronegativity because the distance between the nucleus and the valence electrons influences the strength of the electrostatic attraction.
Recall that smaller atoms have fewer electron shells, so their valence electrons are closer to the nucleus, which means the nucleus exerts a stronger pull on electrons involved in bonding.
Note that more electron shells increase shielding, which reduces the effective nuclear charge felt by valence electrons, making it harder to attract additional electrons.
Conclude that the key reason smaller atoms attract electrons more easily is that their valence electrons are closer to the nucleus, resulting in a stronger electrostatic pull on bonding electrons.
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