Which Chemical Species Has the Lowest Energy Based on Formal Charge?

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SUMMARY

The discussion centers on determining the chemical species with the lowest energy based on formal charge. Participants agree that the most stable structure is identified by the lowest sum of absolute values of formal charges and the largest negative formal charge on the most electronegative element. Specifically, the first structure is favored due to arsenic's ability to form multiple bonds, while oxygen's electronegativity plays a crucial role in stability assessments. The conversation highlights the importance of formal charge calculations in evaluating molecular stability.

PREREQUISITES
  • Understanding of formal charge calculations in chemistry
  • Knowledge of electronegativity and its impact on molecular stability
  • Familiarity with chemical bonding, particularly d-orbitals and double bonds
  • Basic principles of molecular structure and stability assessment
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  • Research the concept of formal charge in molecular structures
  • Study the role of electronegativity in determining molecular stability
  • Explore the bonding capabilities of elements with d-orbitals, focusing on arsenic
  • Learn about resonance structures and their impact on stability in chemical species
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Chemistry students, educators, and researchers interested in molecular stability, formal charge analysis, and chemical bonding principles.

omni
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i found the Formal charge of 3 Chemical species, now i asked to decide which one יhave the most low energy.

how can i know it, all have -3 at the sum.

i need help in this section.thanks.
 

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What do you mean by 'the lowest energy'? I can tell you which one is the most stable: the first one. Since As has d-orbitals, it is able to form more than 4 bonds. Combine this with the fact that oxygen tends to form double bonds, and it is readily seen that the first is the logical choice.

The most stable structure is the one with:
a) the lowest sum when the absolute values of the formal charges are added
b) the largest negative formal charge on the most electronegative element (when 2 or more
structures have the same lowest sum)
 

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hi thank you very much.
you really helped me :)

but i think you have a mistake if we work with the rules from what you given and since o is more electronegative than As so if we follow after rule b the most stable structure is the one in the center.
 
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