Create your Smart Home App in the Free Webinar on Home Automation. Register Now
One of our academic counsellors will contact you within 1 working day.
Click to Chat
1800-1023-196
+91-120-4616500
CART 0
Use Coupon: CART20 and get 20% off on all online Study Material
Welcome User
OR
LOGIN
Complete Your Registration (Step 2 of 2 )
Free webinar on App Development Learn to create your own Smart Home App
16th Jan @ 5:00PM for Grade 1 to 10
Sit and relax as our customer representative will contact you within 1 business day
We know that diamond is the hardest naturally occurring substance and so it is much much stable as compared to the other allotrope of carbon i.e graphite as per their structure apparently .But,why then then the bond order of graphite(1.5) is greater than diamond(1).As we know Bond Order is directly proportional to stability.
Graphite has sp2 bonded carbon in planar sheets, whereas Diamond has sp3 bonded carbons.sp2 has a higher bond energy. Diamond has a greater melting point because of the structure of diamond where each carbon is bonded to four other carbon atoms. In graphite each carbon is bonded to only three carbon atoms in a flat plane. The planes are weakly bound by what amount to London dispersion forces.
Post Question
Dear , Preparing for entrance exams? Register yourself for the free demo class from askiitians.
points won -