Problem: When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms that has a formula of S2Cl2. 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.

FREE Expert Solution

In drawing Lewis structures, there are general guidelines to be followed:

1. The number of valence electrons equals group number. 

The total number of valence electrons is:


2. Least electronegative element goes in the center.

Sulfur is less electronegative than chlorine and would be the central atoms.


3. Atoms share or transfer elements to obtain 8 valence shell electrons. Atoms in a covalent bond share electrons. The electrons that participate/bonding in sharing is represented by a line.


4. Non-bonding electrons are represented by Lewis dot symbols.


5. Halogens, when not in center, make one bond.


The Lewis structure of S2Cl2 is:


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Problem Details

When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms that has a formula of S2Cl2. 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.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Formal Charge concept. You can view video lessons to learn Formal Charge. Or if you need more Formal Charge practice, you can also practice Formal Charge practice problems.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.