Answer:
Carbon because of its small size and
higher electro negativity than silicon forms \[p\pi -p\pi \] double bonds with
O-atoms to form \[C{{O}_{2}}\] molecule. These molecules of \[C{{O}_{2}}\] are
held together by weak van der Waals forces of attraction which can be easily
overcome by collisions of the molecules at room temperature. Consequently,\[C{{O}_{2}}\]
is a gas.
Silicon, on the other hand, because of
its bigger size and lower electro negativity than carbon has little tendency to
form\[p\pi -p\pi \] double bonds with O-atoms. Instead, each silicon atom forms
four single covalent bonds with O-atoms which are tetrahedrally arranged around
it leading to the formation of a three-dimensional network structure (Fig.
11.18, page 11/40). To break these covalent bonds, a large amount of energy is
needed and hence \[Si{{O}_{2}}\] is a high melting solid.
You need to login to perform this action.
You will be redirected in
3 sec
