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Hi, for question 2 I had to find the most stable lewis structure for TiCl4. I thought I had did it right because of the formal charges but it was wrong. Could someone please explain the answer?
The answer is titanium connected to 4 chlorines by a single bond. The question tells you that the molecule must be neutral (sum of formal charges is 0), which means that it is highly likely that all chlorine atoms have 3 lone pairs and one bond. 4 chlorines with 7 valence electrons and 1 titanium with 4 valence electrons give you a structure that looks like this https://www.mjlphd.net/blog/on-the-use- ... rachloride except with lone pairs around the chlorine. Let me know if you need anything else
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