Types Of Bonding Flashcards
Define Ionic bond
Electrostatic attraction between oppositely charged ions
Regular arrangement
- ions bigger than + ions
Covalent substances
Shared pair of e
Metallic lattice structure
Metal ions surrounded by sea of delocalised e
Layered structure that slide
Strength of metallic attraction increased by:
More delocalised e per atom
Bigger + charges
Smaller sized metal ions
Explain how coordinate bond formed
Lone pair on ___ donated to ___
What makes good thermal conductor
Metal
When heated + ions vibrate as thermal energy increases
Transfer KE as they collide
delocalised e carry and transfer KE through out metal
Ionic mp vs metallic mp
Metallic mp higher than ionic mp
Key formulas of ions
CO3
NO3
SO4
NH4
CO3 2-
NO3 -
SO4 2-
NH4 +
Electrical conductivity in ionic
Solid doesn’t conduct
Aqueous can due to free moving ions
Graphite conductivity
Good good conductor
Mobile e that carry charge
Explain why graphene and graphite are good e conductors but diamond isn’t (6 marks)
• Graphene is single layer of C atoms
• with delocalised e which carry charge
• Graphite has multiple layers of C atoms bonded to 3 other C atoms
• which delocalise e which carry charge
• Diamond has tetrahedral structure and C atoms bonded to 4 other C atoms
• All outer electrons bonded so no delocalise to e to carry electrical charge
Explain why melting point in diamond and ice is different
• Both covalent bonding
• Diamond is giant macromolecule
• 4 C atoms bonded
• High mp as lost of energy required to break strong covalent bonds
• Hydrogen bonding between water molecules
• Covalent bonds strong between H and O
• Less energy needed to overcome weaker hydrogen bonding so lower mp
