Multiple Choice
As you move down a group (family) in the periodic table, how does the electronegativity of the elements typically change?
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10. Periodic Properties of the Elements
Periodic Trend: Electronegativity
Multiple Choice
Which of the following atoms has the greatest tendency to attract electrons (i.e., has the highest electronegativity)?
A
F (fluorine)
B
Cl (chlorine)
C
O (oxygen)
D
Na (sodium)
Verified step by step guidance1
Understand that electronegativity is the tendency of an atom to attract electrons towards itself when it forms a chemical bond.
Recall the general trend of electronegativity in the periodic table: it increases from left to right across a period and decreases from top to bottom down a group.
Identify the positions of the given elements in the periodic table: Na is in Group 1 (alkali metals), O and F are in Period 2, with F to the right of O, and Cl is in Period 3, below F.
Compare the elements based on their positions: since electronegativity increases across a period and decreases down a group, fluorine (F), being in the top right corner (excluding noble gases), has the highest electronegativity.
Conclude that among Na, O, Cl, and F, fluorine has the greatest tendency to attract electrons due to its position in the periodic table.
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