You are mistaken in your question. Silion does form multiple bonds. Glass, for example, is a silica-derived formation as is sand; both include silicon dioxide which has multiple bonds.
Carbon is a nonmetal, while silicon is a metalloid, so no.
in diamond carbon is sp3 hybridized while in graphite itz sp2 raahat
because when there is a double bond, there is a Pi bond involved. and Pi bonds are weaker than sigma bonds (which are in single bonds) WRONG. While it is true that Pi bonds are weaker than Sigma bonds, double bonds (C = C) contain BOTH Pi and Sigma bonds making double bonds stronger than single bonds (which contain only a Sigma bond) overall.
Carbon tetrachloride is nonpolar because its polar bonds are distributed in space (at the corners of tetrahedron with the carbon atom at its center) in a manner such that the the polarities of the individual bonds cancel one another out at any substantial distance from the molecule.
Silicon has covalent bonds while aluminium has metallic bonds so aluminium has the higher modulus of elsticity(E).
Carbon is a nonmetal, while silicon is a metalloid, so no.
Carbon is unique because it can form four bonds, whether they be single, double, or triple bonds, and can also make C-C bonds. Silicon, while in the same group and containing 4 valence electrons, cannot, because silicon has a much larger atomic radius it can rarely make double bonds, and when it does they are generally not stable. In addition, Si-Si bonds are not stable, and an Si-O bond is more favorable. Carbon is unique because it is so versatile in its bonding.
generally silicon forms covalent bonds. These are generally single bonds- (there are some silenes with Si-Si double bonds but these are unstable compounds.) Si -Si bonds in silanes are known but and while long chain molecules with Si-Si backbones are knwn they are not as stable as the analogous carbon chains. Silicon forms polyatomic anions- so-called silicides- an example is sodium silicide NaSi (Na4Si4) (It contains the Si44- ion which is tetrahedral and isoelectronic with the P4 molecule. This is not the only strange anion- there are others.
in diamond carbon is sp3 hybridized while in graphite itz sp2 raahat
No not at all only metallic bonds are malleable. An example of this is iron can be struck to from many shapes. While diamond which is a lattice of carbon to carbon covalent bonds though extremely hard is impossible to disform
because when there is a double bond, there is a Pi bond involved. and Pi bonds are weaker than sigma bonds (which are in single bonds) WRONG. While it is true that Pi bonds are weaker than Sigma bonds, double bonds (C = C) contain BOTH Pi and Sigma bonds making double bonds stronger than single bonds (which contain only a Sigma bond) overall.
Carbon tetrachloride is nonpolar because its polar bonds are distributed in space (at the corners of tetrahedron with the carbon atom at its center) in a manner such that the the polarities of the individual bonds cancel one another out at any substantial distance from the molecule.
Saturated fatty acids have single carbon-to-carbon bonds (which tend to act like a rigid pole) while unsaturated fatty acids have double carbon-to-carbon bonds (which can act like hinges making the molecule flexible).
Saturated fatty acids have single carbon-to-carbon bonds (which tend to act like a rigid pole) while unsaturated fatty acids have double carbon-to-carbon bonds (which can act like hinges making the molecule flexible).
Saturated fatty acids have single carbon-to-carbon bonds (which tend to act like a rigid pole) while unsaturated fatty acids have double carbon-to-carbon bonds (which can act like hinges making the molecule flexible).
Saturated fatty acids have single carbon-to-carbon bonds (which tend to act like a rigid pole) while unsaturated fatty acids have double carbon-to-carbon bonds (which can act like hinges making the molecule flexible).
Saturated fatty acids have single carbon-to-carbon bonds (which tend to act like a rigid pole) while unsaturated fatty acids have double carbon-to-carbon bonds (which can act like hinges making the molecule flexible).