Ch.22 - Chemistry of the Nonmetals
Chapter 22, Problem 45
Complete the exercises below. Write the Lewis structure for each of the following species, and indicate the structure of each: a. SeO₃²⁻; b. S₂Cl₂; c. chlorosulfonic acid, HSO₃Cl (chlorine is bonded to sulfur).
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for each species. For SeO₃²⁻, calculate the valence electrons from Se and O, and add 2 for the charge. For S₂Cl₂, sum the valence electrons from S and Cl. For HSO₃Cl, sum the valence electrons from H, S, O, and Cl.
Step 2: Draw the skeletal structure for each species. For SeO₃²⁻, place Se in the center with O atoms around it. For S₂Cl₂, place the S atoms in the center with Cl atoms bonded to them. For HSO₃Cl, place S in the center with O, Cl, and H atoms bonded to it, ensuring Cl is bonded to S.
Step 3: Distribute the valence electrons around the atoms to satisfy the octet rule, starting with the outer atoms. For SeO₃²⁻, distribute electrons to the O atoms first. For S₂Cl₂, distribute electrons to the Cl atoms. For HSO₃Cl, distribute electrons to the O and Cl atoms.
Step 4: Check for formal charges and adjust the structure if necessary to minimize them. For SeO₃²⁻, consider forming double bonds between Se and O to reduce formal charges. For S₂Cl₂, ensure the formal charges are minimized. For HSO₃Cl, adjust bonds to minimize formal charges, especially around S.
Step 5: Verify that all atoms have complete octets (or duets for hydrogen) and that the total number of electrons used matches the total number of valence electrons calculated in Step 1.
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 help visualize the arrangement of electrons and the connectivity of atoms, allowing chemists to predict molecular geometry and reactivity. Each dot represents a valence electron, while lines indicate covalent bonds between atoms.
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Formal Charge
Formal charge is a concept used to determine the distribution of electrons in a molecule. It is calculated by taking the number of valence electrons of an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. This helps in assessing the most stable Lewis structure, as structures with formal charges closest to zero are generally preferred.
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Resonance Structures
Resonance structures are different Lewis structures that represent the same molecule but differ in the arrangement of electrons. They are used when a single Lewis structure cannot accurately depict the electron distribution. The actual structure of the molecule is a hybrid of these resonance forms, which helps explain properties such as bond lengths and strengths that are intermediate between those predicted by individual structures.
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