Multiple Choice
Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl_2 when constructing its Lewis dot structure?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Exceptions
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Which of the following elements should never have expanded octets in their Lewis dot structures?
A
Carbon (C)
B
Phosphorus (P)
C
Chlorine (Cl)
D
Sulfur (S)
Verified step by step guidance1
Understand what an expanded octet means: it occurs when an atom has more than 8 electrons around it in its Lewis structure, which is possible for elements in period 3 or below because they have d orbitals available for bonding.
Identify the period of each element: Carbon (C) is in period 2, Phosphorus (P), Chlorine (Cl), and Sulfur (S) are in period 3.
Recall that elements in period 2, like Carbon, cannot have expanded octets because they lack accessible d orbitals to accommodate extra electrons beyond the octet.
Recognize that elements in period 3, such as Phosphorus, Chlorine, and Sulfur, can have expanded octets due to the availability of 3d orbitals, allowing them to hold more than 8 electrons.
Conclude that Carbon should never have expanded octets in its Lewis dot structures, while the others can.
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