Question

draw the correct lewis structure of scl₂. be sure to include all lone pair electrons and non - zero formal charges.

Explanation:

Step1: Determine valence electrons

Sulfur (S) has 6 valence electrons and each chlorine (Cl) has 7 valence electrons. So total valence electrons = 6 + 2×7 = 20.

Step2: Identify central atom

Sulfur is the central atom as it is less electronegative than chlorine.

Step3: Connect atoms and distribute electrons

Connect S to each Cl with a single - bond (using 4 electrons). Then distribute the remaining 16 electrons as lone - pairs. Each Cl gets 3 lone - pairs and S gets 2 lone - pairs.

Step4: Calculate formal charges

Formal charge of S = 6 - 2 - 4 = 0. Formal charge of each Cl = 7 - 6 - 1 = 0.

Answer:

The Lewis structure has a sulfur atom in the center, single - bonded to two chlorine atoms. Each chlorine atom has 3 lone - pairs of electrons and the sulfur atom has 2 lone - pairs of electrons. There are no non - zero formal charges.