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Which of the following elements has the fewest valence electrons available for bonding?
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10. Periodic Properties of the Elements
Valence Electrons of Elements
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Which of the following elements can expand its valence shell to accommodate more than eight electrons?
A
Phosphorus (P)
B
Carbon (C)
C
Nitrogen (N)
D
Fluorine (F)
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Recall the octet rule, which states that atoms tend to form bonds until they are surrounded by eight electrons in their valence shell, achieving a noble gas configuration.
Understand that elements in period 3 or higher of the periodic table have access to d orbitals, allowing them to expand their valence shell beyond eight electrons.
Identify the elements given: Carbon (C), Nitrogen (N), Fluorine (F) are all in period 2, so they cannot expand their valence shells beyond eight electrons because they lack available d orbitals.
Phosphorus (P) is in period 3, which means it has empty 3d orbitals that can be used to accommodate more than eight electrons, allowing it to expand its valence shell.
Therefore, the element that can expand its valence shell to accommodate more than eight electrons is Phosphorus (P).
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