Question

draw the lewis dot structure for sif₃. then carefully compare your drawing to the answer choices and select the correct answer.

Explanation:

To determine the correct Lewis dot structure for $\ce{SiF3^-}$ (assuming it's $\ce{SiF3^-}$ or neutral $\ce{SiF3}$ with correct valence), we analyze:

1. Valence Electrons: Si has 4 valence electrons, each F has 7. For $\ce{SiF3^-}$ (if anionic), add 1 extra electron (total: $4 + 3\times7 + 1 = 26$).
2. Bonding & Lone Pairs: Si forms 3 single bonds with F (each bond uses 2 electrons), and has 1 lone pair (2 electrons) to satisfy octet (Si: 4 + 3 bonds + 1 lone pair = 8; each F: 7 + 1 bond + 6 lone pairs = 8).

Now, check the options:

• The purple card (second from top) shows Si with 3 single bonds to F, 1 lone pair (2 dots) on Si, and each F with 6 lone pairs (3 pairs) – matching the correct structure. Other options have errors (e.g., green card has too few F, orange has a double bond, yellow has extra lone pairs on Si).

Answer:

The correct Lewis dot structure is the one on the purple card (second from the top, with Si bonded to three F atoms, 2 lone electrons on Si, and each F with three lone pairs).