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Chapter 13: Problem 5

What is the likely formula for a molecule composed of hydrogen atoms and one sulfur atom? Draw the Lewis structure for this molecule.

Short Answer

Expert verified
The likely formula for a molecule composed of hydrogen atoms and one sulfur atom is \(H_2S\). The Lewis structure for this molecule features a sulfur atom at the center, connected to two hydrogen atoms, with two lone pairs of electrons on the sulfur atom.

Step by step solution

01

Determine the Molecule's Formula

First, let's determine the molecule's formula. In compounds, sulfur typically forms two bonds, and hydrogen forms one bond. Therefore, the probable formula for a molecule with one sulfur atom and hydrogen atoms is \(H_2S\). This formula suggests that two hydrogen atoms bond with one atom of sulfur.
02

Identify the Central Atom

After determining the molecule's formula, the next step is to identify the central atom for drawing the Lewis structure. In a \(H_2S\) molecule, the sulfur (S) atom serves as the central atom, with each hydrogen atom (H) attached to it.
03

Determine the Valence Electrons

The total number of valence electrons in a \(H_2S\) molecule determines its Lewis structure. Sulfur has six valence electrons, as it is in the oxygen family (Group 16 in the periodic table), and each hydrogen atom has one valence electron (Group 1 in the periodic table). Therefore, a \(H_2S\) molecule has a total of eight valence electrons.
04

Draw the Lewis Structure

To draw the Lewis structure, first, draw sulfur (S) as the central atom, then draw two hydrogen atoms (H) attached to the sulfur atom. Next, use valence electrons to form bonds between sulfur and each hydrogen atom. A line between sulfur and hydrogen represents a bond (two electrons). After creating bonds, distribute the remaining electrons around sulfur. In this case, four electrons (two lone pairs) are left on sulfur. The final Lewis structure for \(H_2S\) looks like this: \n H-S-H with two pairs of dots on the sulfur atom.
05

Check the Formal Charges

Checking the formal charges helps confirm the Lewis structure. A proper Lewis structure generally has formal charges closest to zero. In this case, each hydrogen has a formal charge of zero because it shares one electron with sulfur, and sulfur has a formal charge of zero because it owns four of its original six electrons and shares the other two electrons with hydrogen. The sum of all formal charges is zero, aligning with the charge of most molecules. Thus, this is the correct Lewis structure for \(H_2S\).

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Most popular questions from this chapter

For \(\mathrm{N}_{2}\), is the sum of the bonding electrons and nonbonding electrons around each nitrogen atom consistent with the Lewis model?

Given the shell model of the atom, suggest a possible reason that Lewis proposed a maximum of two electrons for hydrogen and a maximum of eight for carbon, nitrogen, oxygen, and fluorine atoms?

Without attempting to draw a Lewis structure, calculate the total number of valence electrons in each of these molecules: a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)

Give the Lewis representation for each of the following atoms. a) iodine b) calcium c) phosphorus

For \(\mathrm{H}_{2} \mathrm{CO}\) : a) Is the sum of the bonding electrons and lone pair electrons around the carbon atom consistent with the Lewis model? b) Is the sum of the bonding electrons and lone pair electrons (nonbonding electrons) around the oxygen atom consistent with the Lewis model?
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