We're considering this carbon carbon bond. Because pylons are always made up of P orbital's for Jay. Is Pete overlapping with carbon Espy for little Both pie bonds are made up of a carbon p overlapping with another carbon piece. This carbon has also as p hybridized so the signal bond must be made up of carbon. So we have one signal bond in two pipe bombs to consider this carbon. Now we're considering the carbon carbon triple bodies. Therefore, you have an espy orbital overlapping with an s hydrogen orbital. Hydrogen on Lee has an s orbital to contribute. We have We're looking at this carbon hydrogen bond again. For the Sigma bond, the pie bond is going to be a carbon p orbital overlapped with an oxygen P orbital for H. Therefore, it is s p to hybridized so we have an S p to oxygen overlapping with an S P to high braised carbon. So it has three areas of electron density.
The oxygen has two sets of lone pairs which we should also consider when determining the hybridization of oxygen. Or you could write inversely as a carbon s p three overlapping with the carbon.
Therefore, it's a carbon ist p to orbital overlapping with a carbon s p three. This carbon is S p to hybridized This carbon is S p three hybridized. You can also write this as a carbon s p three, overlapping with the carbon Espy too for end We're talking about this carbon carbon bond. Therefore, the orbital overlap is a carbon s p to with a carbon S p three. Orbital's overlapping for e were considering this bond. So sigma is a carbon s P two overlapping with another carbon ist p to the pie is two carbon peas.
Because this carbon is also s p to hybridized for the pie bond pie bonds are always made up of p orbital's and therefore you have an overlap of a carbon p with another carbon p. The signal bond is made up of a carbon S P to orbital overlapping with another carbon S p to orbital. Now we have two bonds we have to consider. Therefore, you have a carbon espy two overlapping with a hydrogen s orbital for D. This carbon is S p to Harvard ice because there are three areas of electron density around it. So four areas of bonding This carbon is also as p three Harvard ized and therefore the overlap to form the bomb is an s p three carbon or little overlapping with a second carbon S p three orbital living Teo the second structure This carbon hydrogen bomb is the next when they're asking for again hydrogen can only contribute an s orbital. You could write this in reverse is well a hydrogen s overlapping with the carbon S p three for be the bottom Kurban here is s p three hybridized there too high Do Jin's attached to it. So the overlap is going to be a carbon s p three overlapping with a hydrogen s orbital. For instance, let's start with a This carbon is S p three hybridized and so it is contributing an s P three hybridized orbital to the overlap with hydrogen hydrogen on Lee has an s orbital to contributed. What you want to do is determine the hybridization of both atoms that are forming the overlapping bought. If there is more than one bond, you have to indicate the orbital's for each individual Bob to solve this problem. Determine what orbital's are being used to form each of the bonds.
0 kommentar(er)
