Question

what is the correct lewis structure for sicl4?
n = 40, a = 32, s = 8, bonds = 4

Explanation:

Step1: Calculate the total number of valence electrons

Silicon (Si) has 4 valence electrons, and each chlorine (Cl) has 7 valence electrons. For \(SiCl_4\), the total number of valence electrons \(A=(4)+4\times(7)=32\)

Step2: Calculate the number of shared electrons

The formula \(S = N - A\), where \(N\) is the number of electrons needed for noble - gas configurations. Si needs 8 electrons and each Cl needs 8 electrons, so \(N=(8)+4\times(8)=40\). Then \(S = 40 - 32=8\)

Step3: Determine the number of bonds

Since each bond contributes 2 electrons, the number of bonds \(=\frac{S}{2}=\frac{8}{2}=4\). Si is the central atom. Each Cl forms a single bond with Si. And after forming bonds, each Cl has 6 non - bonding electrons (3 lone pairs)

Answer:

The first structure (where Si is in the center, bonded to four Cl atoms, and each Cl has 3 lone pairs) is the correct Lewis structure for \(SiCl_4\)