객관식
Which of the following correctly describes the Lewis dot structure for the ion Ni^{3+}?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
객관식
Determine the Lewis Dot Structure for the following ion: O22–.
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검증된 단계별 안내1
Step 1: Determine the total number of valence electrons for the O\_2\(\textsuperscript{2-}\) ion. Each oxygen atom has 6 valence electrons, and the 2- charge adds 2 extra electrons. So, total electrons = 6 \(\times\) 2 + 2 = 14 electrons.
Step 2: Draw a skeletal structure with two oxygen atoms connected by a single bond initially. Place the remaining electrons as lone pairs around the atoms to satisfy the octet rule.
Step 3: Calculate the formal charges on each oxygen atom to check the stability of the structure. The formal charge formula is: \(\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}\).
Step 4: Adjust the bonding between the oxygen atoms if necessary to minimize formal charges. For O\_2\(\textsuperscript{2-}\), a single bond with lone pairs on each oxygen typically results in the most stable structure with formal charges close to zero.
Step 5: Enclose the entire structure in brackets and indicate the 2- charge outside the brackets to represent the ion correctly.
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