A carbon atom that forms four single covalent bonds (sp3 hybridised), as seen in methane, has which type of molecular geometry around it?
In ethene (CH2=CH2), each carbon atom involved in the double bond is best described as:
sp2 hybridised with trigonal planar geometry
Not hybridised at all
sp3 hybridised with tetrahedral geometry
sp hybridised with linear geometry
In ethyne (HC≡CH), each carbon atom involved in the triple bond is best described as:
sp2 hybridised with trigonal planar geometry
Not hybridised at all
sp hybridised with linear geometry
sp3 hybridised with tetrahedral geometry
Why does carbon generally form covalent bonds rather than ions like C4+ or C4-?
Carbon atoms are too large to form ions
Removing or adding four electrons requires a very large amount of energy, making ion formation difficult
Carbon has no valence electrons available
Carbon does not obey the octet rule