Final answer:
The Lewis structure for O₂ is depicted with a double bond between the two oxygen atoms. SeO is not a recognized diatomic molecule so a Lewis structure is not provided for it, but analogous structures were provided for similar substances, such as SO and SeO₂.
Step-by-step explanation:
The student has been asked to draw the Lewis structures for two diatomic molecules, SeO, and O₂. Lewis structures are a way to represent the valence electrons in a molecule and how they are shared between atoms to form covalent bonds.
For the oxygen molecule (O₂), the Lewis structure is relatively straightforward due to oxygen's well-known propensity to form a double bond when paired with another oxygen atom. Thus, the Lewis structure for O₂ is:
:O::O:
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O O
Unfortunately, SeO is not a commonly recognized diatomic molecule, and it may be misprinted or misunderstood. However, if we consider a molecule such as SO (sulfur monoxide) or SeO₂ (selenium dioxide), we could then provide a Lewis structure for that molecule. Since selenium and sulfur are in the same group, their bonding behaviors are somewhat similar.
For SO, the structure would feature a double bond between sulfur and oxygen:
:S::O:
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S O
For SeO₂, it would similarly feature double bonds:
:O::Se::O:
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O Se O
Note that the Lewis structure for SeO is not provided as SeO is not a recognized diatomic molecule. SeO₂ is a compound with known characteristics, so its Lewis structure can be inferred.