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Chapter 3: Problem 135

When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms that has a formula of \(\mathrm{S}_{2} \mathrm{Cl}_{2}\). The Lewis structure of this compound has a formal charge of zero on all elements in the compound. Draw the Lewis structure for the vile-smelling orange liquid.

Short Answer

Expert verified
The Lewis structure for the vile-smelling orange liquid S2Cl2 is drawn by following these steps: 1. Count the total number of valence electrons (26); 2. Determine the central atoms (2 sulfur atoms); 3. Place the remaining atoms around the central atom (2 chlorine atoms); 4. Distribute the electrons among the atoms to satisfy the octet rule: .. .. :Cl-S-S-Cl: .. .. 5. Check the formal charge: all atoms have a formal charge of zero, thus confirming that the Lewis structure is correct.

Step by step solution

01

Count the total number of valence electrons

Sulfur has 6 valence electrons (group 16) and chlorine has 7 (group 17). Since there are 2 sulfur atoms and 2 chlorine atoms in the compound, the total number of valence electrons is (6 x 2) + (7 x 2) = 12 + 14 = 26.
02

Determine the central atom

In this compound, sulfur is the central atom, as it can form more bonds than chlorine and is also less electronegative. We will be placing the 2 sulfur atoms in the center with the 2 chlorine atoms surrounding them.
03

Place the remaining atoms around the central atom

We place the chlorine atoms around the two central sulfur atoms. The two sulfur atoms will bond together as well. S - S | | Cl Cl
04

Distribute the electrons among the atoms to satisfy the octet rule

Distribute the remaining 22 electrons (26 provided minus 2 electrons in the S-S bond and 2 electrons in each S-Cl bond) to the chlorine atoms and the central sulfur atoms to satisfy the octet rule: .. .. :Cl-S-S-Cl: .. .. The octet rule is satisfied for each chlorine atom with a single bond to Sulfur of 2 shared electrons and 3 lone pairs (6 electrons). The octet rule is also satisfied for each sulfur atom with 2 shared electrons in the S-S bond, 2 electrons in each S-Cl bond, and 1 lone pair (2 electrons).
05

Check the formal charge

Now, let's verify that all the atoms in our drawn structure have a formal charge of zero. The formal charge is given by the formula: Formal charge = (number of valence electrons) - (number of non-bonding electrons) - 0.5 x (number of bonding electrons) For sulfur: Formal charge = (6) - (2) - 0.5 x (6) = 0 For chlorine: Formal charge = (7) - (6) - 0.5 x (2) = 0 All the atoms have a formal charge of zero, so our Lewis structure is correct.

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