what is the correct lewis structure for sicl4? n = 40, a = 32, s = 8, bonds = 4
what is the correct lewis structure for sicl4? n = 40, a = 32, s = 8, bonds = 4
Answer
Explanation:
Step1: Determine valence - electrons
Silicon (Si) has 4 valence electrons and each chlorine (Cl) has 7 valence electrons. So for SiCl₄, the total number of valence electrons $A=4 + 4\times7=32$.
Step2: Identify the central atom
Si is the central atom as it is less electronegative than Cl.
Step3: Form bonds
Si forms 4 single - bonds with 4 Cl atoms, using 8 electrons. Each bond represents 2 electrons, so the number of bonds is 4.
Step4: Distribute remaining electrons
After forming 4 bonds, we have $32 - 8=24$ electrons left. We distribute these 24 electrons as lone - pairs on the Cl atoms. Each Cl atom gets 3 lone - pairs (6 electrons). The correct Lewis structure is the one where Si is in the center, bonded to 4 Cl atoms and each Cl atom has 3 lone - pairs of electrons. Looking at the given structures, the first one is correct as it has the correct number of bonds and lone - pairs.
Answer:
The first structure (where Si is in the center, bonded to 4 Cl atoms and each Cl has 3 lone - pairs of electrons)