covalent bonding

Question 1

covalent bonding

Answer 1

electrostatic attraction between shared pair of electrons and the positively charged nuclei of atoms

Question 2

giant covalent structures

Answer 2

contain uncharged atoms
bonds are strong
high melting points
don’t conduct electricity 
insoluble in water

Question 3

diamond

Answer 3

strong covalent bonds
each carbon atoms uses all 4 electrons to form 4 bonds with other carbons
jewellery, drilling, cutting
solid
high melting point - 4,726*C
does not conduct electricity- no free electrons
tetrahedral structure
very hard

Question 4

graphite

Answer 4

strong covalent bonds
each carbon is bonded only to 3 carbon atoms- 3 electrons used 1 is free
4th electron is delocalised throughout structure (1 electron from each carbon atom)
4300K—>4127*C
does conduct electricity due to delocalised electron flowing freely
solid
weak intermolecular forces between layers
used in pencils- layers slide over each other (slippery) due to weak intermolecular forces - lubricant

Question 5

fullerene

Answer 5

covalent bonding
high melting and boiling points
60 carbon atoms bonded to 3 others by 2 single bonds and are double bonds
buckminster fullerene
doesn’t conduct electricity
nanotechnology- use of structure (10-9 metre) drug delivery

Question 6

silicon dioxide

Answer 6

isn’t allotrope of carbon as it doesn’t have carbon atoms (silicon, oxygen)
known as sand, makes glass (silica)
SiO2
sim to diamond
covalent bonding, giant covalent structure 
very hard
high melting and boiling points
doesn’t conduct electricity 
insoluble

Question 7

covalent bonding occurs between…?

Answer 7

two non-metals