Why is this statement false: sp3 hybrid orbitals can form pi bonds.?

Thanks in advance!Why is this statement false: sp3 hybrid orbitals can form pi bonds.?
Because sp3 hybrid orbitals can only form sigma bonds.





蟺 bonds are formed by P orbitals which are perpendicular relatively to each other looking at a single atom. Only atoms that have Pi orbitals can form 蟺 bonds. The point of hybridisation, for sp3 hybridisation for example, is to form 4 orbitals that are the same in other to form 4 sigma bonds that are equal with other atoms. For example, carbon has configuration 1s2 2s2 2p2, so lets say in methane molecule (CH4), the carbon must have C-H sigma bonds of equal strength so in order to do that it will form 4 sp3 orbitals by taking 3 p orbitals and 1 s orbital to make sp3. The orbital that H will use is s since it has only an s bonding orbital. A 蟺 bond is weaker than a sigma bond since it is only made of Pi orbitals so in a reaction with a double bond that breaks the 蟺 bond breaks first (remember that a double bond is made of a sigma bond and a 蟺 bond).





A Carbon that is sp3 hybridised makes 4 singles bonds, 4 sigma bonds of equal length. A carbon that is sp2 hybridised makes 2 single bonds (sigma) and 1 double bond (sigma + 蟺). A carbon that is sp hybridised makes 1 single bond (sigma) and 1 triple bond (蟺 + 蟺 + sigma).





To get a picture look at the molecule of ethene (sp2 hybridised), all the sigma bonds are made of sp2 orbitals and the only 蟺 bond is an overlap between pi orbitals that are parallel to each other (one pi orbital on each carbon):


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By the way, do not get confused because of the person below that says ';The double bond has sigma electrons and pi electrons. so the statement should read, ';sp2 hybrid orbitals can form double bonds';'; In the ethene molecule, the double bond is made of a 蟺 bond + a sigma bond and ONLY the sigma bond uses the sp2 hybrid orbital NOT the entire double bond.Why is this statement false: sp3 hybrid orbitals can form pi bonds.?
sp3 carbons have 4 individual bonds to them. All single bonds are made of sigma electrons. sp2 carbons have 2 single bonds and 1 double bond. The double bond has sigma electrons and pi electrons. so the statement should read, ';sp2 hybrid orbitals can form double bonds';