CHEMISTRY COMMUNITY

Question: Can you please explain to me why (CH3)2Be has a hybridization of sp rather than sp3? Is it because Be has an empty p orbital and lone pairs do not effect it?

Answer: Be is in group 2 and forms two bonds, one to each CH3. Placing Be in the center forms a linear molecule with two single bonds.Therefore Be is sp hybridization.

Can you please explain why we can put Be in the middle? thanks

The central atom is always the one with the lowest electronegativity. Be is lower than C so it is in between the two carbons

On number 4.19, it says that (CH3)2BE is tetrahedral - how is that right if it's VSEPR is sp?

Please read things carefully.

The solution manual says the shape is a tetrahedral about the carbon atoms.

However, as a whole, the molecule is linear. Meaning with respect to the central Be atom in (CH₃)₂Be.

Chem_Mod wrote:Please read things carefully.

The solution manual says the shape is a tetrahedral about the carbon atoms.

However, as a whole, the molecule is linear. Meaning with respect to the central Be atom in (CH₃)₂Be.

So to better understand, if the question were to ask of the shape in respect to the carbon atoms then the shape would be tetrahedral and if in respect to Be then the shape would be linear? Since the question doesnt specify would you just assume Be and just specify in the answer what your bond angle is refering to ?

Your statement is correct. You can also ask for clarification if it appears on the exam

Is the VSPER shape tetrahedral? If so, why?