Carbon (diamond) is much harder and stronger
Because silicon is a metalloid/semi-metal and carbon is a nonmetal, the bond is covalent.
No, diamond is a covalent compound as it is made from carbon which forms covalent bonds.
There is generally a lack of free electrons to conduct electricty. For example diamond (an allotrope of carbon) and silicon dioxide, which are very poor conductors. . Some network covalent t are semiconductors- like silicon- which mean that they can conduct but poorly.
a covalent bond
These are giant molecular lattice structures. This implies that strong covalent bonding holds their atoms together in a highly regular extended network. The bonding between the atoms goes on and on in three dimensions. Melting requires the separation of the species comprising the soild state, and boiling the separation of the species comprising the liquid state. Because of the large amount of energy needed to break huge numbers of covalent bonds, all giant covalent network structures have high melting points and boiling points and are insoluble in water. Diamond, graphite (allotropes of carbon) and quartz (silicon(IV) oxide, SiO2) are examples.
Because silicon is a metalloid/semi-metal and carbon is a nonmetal, the bond is covalent.
No, diamond is a covalent compound as it is made from carbon which forms covalent bonds.
There is generally a lack of free electrons to conduct electricty. For example diamond (an allotrope of carbon) and silicon dioxide, which are very poor conductors. . Some network covalent t are semiconductors- like silicon- which mean that they can conduct but poorly.
a covalent bond
Silicon (like carbon) can form covalent bonds, it forms a giant molecule with the diamond structure. Silicon dioxide is also a giant structure with polar covalent bonds. Silica reacts with basic oxides to form silicates- and these are generally giant structures, polar covalent bonds again, that form a very large proportion of the minerals in the earths crust.
These are giant molecular lattice structures. This implies that strong covalent bonding holds their atoms together in a highly regular extended network. The bonding between the atoms goes on and on in three dimensions. Melting requires the separation of the species comprising the soild state, and boiling the separation of the species comprising the liquid state. Because of the large amount of energy needed to break huge numbers of covalent bonds, all giant covalent network structures have high melting points and boiling points and are insoluble in water. Diamond, graphite (allotropes of carbon) and quartz (silicon(IV) oxide, SiO2) are examples.
Diamond and Graphite are allotropes of Carbon [chemical symbol: C]The chemical symbol of Silicon is Si.
Diamond is a covalent substance in which every carbon atom is linked with four other carbon atoms tetrahedraly through covalent (sigma) bonds.
The diamond is a crystallized, allotrope form of pure carbon.
The carbon to carbon bonding in Diamond is a covalent bonding.
The strongest chemical bond is the ionic bond. Ionic bond strengths are greater than covalent bond strengths.answer 2it is known that covalent bond is stronger.
Silicon is most likely to form covalent bonds because it has four valence electrons and will share electrons rather than give them away.