above period 3 elements

[tRNA]

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I know that since Si is in period 3 it has more than just 4 valance electrons available for bonding, but how do you know how many more electrons are available for bonding???

for example: C and Si are in the same group, C can form up to 4 bonds, Si can form up to how many bonds??? is there a way to tell?

plz help

 

[169745]

I know that since Si is in period 3 it has more than just 4 valance electrons available for bonding, but how do you know how many more electrons are available for bonding???

for example: C and Si are in the same group, C can form up to 4 bonds, Si can form up to how many bonds??? is there a way to tell?

plz help

resonance structures? i'm not really sure if that answers your question. all of the atoms should have the least formal charge, that structure is the one that contributes most to the composite molecule. if there must be a negative formal charge it best fits on the mots electronegative atoms (N, O, F). also, all period 1 and 2 molecules never expand their octet to form more than 4 bonds while elements in period 3 and higher are able to expand their octet because they have access to the d, f, etc. orbitals.

 

[Nirvrex]

I am pretty sure that the reason si can bond more than carbon can is because Si has a principal quantum number 👎 of 3. That being said its L value would be 0,1,2. Therefore it has S, P and D orbitals. These empty D orbitals allow it to expand its octet. Carbon on the otherhand only has S and P orbitals and therefore cant do this. This is similar to why sulfur can have more bonds than oxygen can, because once again, it has the empty D orbitals to use, while oxygen does not. Hope that helps, I am currently studying to take the test on the 8th, so hopefully if I am wrong someone will correct me before then. : )

Oh and on a sidenote, does anyone know why it is willing to use these d orbitals? I know that a d10 configuration is quite stable, but no idea why it would want to hyperdize its d orbitals.

 

[tRNA]

I am pretty sure that the reason si can bond more than carbon can is because Si has a principal quantum number 👎 of 3. That being said its L value would be 0,1,2. Therefore it has S, P and D orbitals. These empty D orbitals allow it to expand its octet. Carbon on the otherhand only has S and P orbitals and therefore cant do this. This is similar to why sulfur can have more bonds than oxygen can, because once again, it has the empty D orbitals to use, while oxygen does not. Hope that helps, I am currently studying to take the test on the 8th, so hopefully if I am wrong someone will correct me before then. : )

Oh and on a sidenote, does anyone know why it is willing to use these d orbitals? I know that a d10 configuration is quite stable, but no idea why it would want to hyperdize its d orbitals.

thanks forgot about that 3d subshell, for your question i guess it would depend on how many atoms it needs to form bonds with, ie. if it needs the d orbitals it will use them,