There are many Lewis structures you could draw for sulfuric acid, H2SO4 (each H is bonded to an O). (b) What Lewis structure(s) would you draw to minimize formal charge?

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Identify the total number of valence electrons: Calculate the total number of valence electrons available for the Lewis structure by adding the valence electrons of each atom in H2SO4.

Determine the central atom: Sulfur (S) is typically the central atom in H2SO4 because it is less electronegative than oxygen (O) and can form more bonds.

Draw a skeletal structure: Connect the central sulfur atom to four oxygen atoms. Each hydrogen (H) atom is bonded to an oxygen atom.

Distribute remaining electrons: Place the remaining valence electrons around the oxygen atoms to satisfy the octet rule, starting with the outer atoms.

Minimize formal charges: Adjust the structure by forming double bonds between sulfur and two of the oxygen atoms to minimize formal charges, ensuring that the formal charges on all atoms are as close to zero as possible.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and the number of bonds. It helps in determining the most stable Lewis structure by minimizing the formal charges across the molecule, ideally keeping them as close to zero as possible.

Resonance Structures

Resonance structures are different Lewis structures that represent the same molecule, differing only in the arrangement of electrons. They are used when a single Lewis structure cannot accurately depict the electron distribution. For sulfuric acid, considering resonance can help in identifying the most stable structure with minimized formal charges.

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(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe¬O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in part (a) yields the most favorable formal charges for the molecule?

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Some chemists believe that satisfaction of the octet rule should be the top criterion for choosing the dominant Lewis structure of a molecule or ion. Other chemists believe that achieving the best formal charges should be the top criterion. Consider the dihydrogen phosphate ion, H₂PO₄^-, in which the H atoms are bonded to O atoms. (b) What is the predicted dominant Lewis structure if achieving the best formal charges is the top criterion?

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State whether each of these statements is true or false. e. Energy is stored in chemical bonds.