bonding Flashcards
what crystalline structure does diamond have?
macromolecular/ giant covalent
what is the structure of diamond?
tetrahedral
does diamond have a high or low melting and boiling point? why?
high m.p and b.p due to the strong covalent bonds present
why does diamond have a strong, stable structure?
due to the strong tetrahedral structure and that there are no delocalised electrons that can flow throughout the structure
why is diamond a poor conductor?
there are no delocalised electrons that can carry a charge throughout the structure
what crystalline structure does ice have?
simple molecular
describe the bonding and structure in ice
- ice has hydrogen bonds
- forms a 3D crystalline structure
- every H2O molecule is bonded to 4 other H2O molecules forming a regular lattice by hydrogen bonds
why does ice have a low melting and boiling point?
weak molecular forces between molecules
why does ice not conduct any electricity?
as there are no delocalised electrons and no free ions that can carry charge
what is the crystalline structure for iodine?
simple molecular
describe the bonding and the structure of iodine
I2 atoms are bonded by strong covalent bonds forming a lattice structure held together by intermolecular forces
why does iodine have a low melting and boiling point?
due to the weak intermolecular forces
can solid iodine conduct electricity and why?
no, as there are no free ions present that can carry a charge
when reacted in a solvent or when molten, can iodine conduct electricity and why?
yes, as ions are free to move and can carry a charge throughout the structure
what is the crystalline structure for magnesium?
metallic
describe the bonding and structure for magnesium
there is a strong electrostatic attractive between Mg ion and the delocalised electrons tightly packed in hexagonal arrangement
why does magnesium have a high melting and boiling point?
due to the strong electrostatic forces between metal ion and delocalised electrons
can magnesium conduct electricity and why?
yes, due to the delocalised electrons which can carry charge throughout the structure
is magnesium malleable and why?
yes, as the size of atoms in the lattice are identical in size meaning that they can slide over eachother
what is the crystalline structure for graphite?
macromolecular
what is the structure for graphite?
layers of hexagonal rings
what is the bonding for graphite?
each carbon atom is bonded 3x with other carbon atoms leaving with a delocalised electron
is graphite malleable and why?
yes, as the delocalised electron can move in between the layers disrupting the weak intermolecular forces
does graphite have a high melting and boiling point and why?
yes, due to the strong covalent bonds
