Types of Bonding & Properties (Test 1&2) Flashcards
Name the 4 types of bonding
Metallic, Ionic, Covalent Molecular and Covalent Network.
Atoms involved in metallic bonding
Metals
Atoms involved in covalent molecular bonding
Non-metals
Atoms involved in covalent network bonding
- Boron Nitride
- Diamond
- Silicon carbide
- Silicon dioxide
- Graphite
What is the structure of Metallic Bonding?
A 2D lattice of cations surrounded by a ‘sea’ of delocalized electrons. Held together by the electrostatic attraction between the cations and the delocalized electrons.
What is the structure of ionic bonding?
Formed when outer shell electrons are transferred from the metal to the nonmetal in order for both atoms to become stable forming ions, ions found in a 3D lattice, held together by the electrostatic attraction of the oppositely charged ions.
What is the structure of covalent molecular bonding?
Small discrete molecules formed when nonmetals share their valence electrons to become stable. Held together by this strong electrostatic attraction between the positive nucleus and the shared pair(s) of electrons within the molecule, the molecules are attracted to each other by weak intermolecular forces.
What is the structure of covalent network bonding?
Except for graphite: 3D lattice of atoms, held together by the electrostatic attraction between the positive nucleus and the shared pair(s) of electrons.
Graphite: 2D layers of atoms where 3 electrons are shared, leaving one free to move between the layers.
What is the melting/boiling point of metallic bonding?
High.
Due to the strong electrostatic attraction between the cations and the delocalized electrons, which requires a large amount of energy to disrupt.
What is the melting/boiling point of ionic bonding?
High.
Due to the strong electrostatic attraction between the oppositely charged ions, which requires a large amount of energy to disrupt.
What is the melting/boiling point of covalent molecular bonding?
Low.
Due to the weak forces of attraction between the molecules, which do not require a lot of energy to disrupt (it is the forces between the molecules that are disrupted, not the bond between the atoms).
What is the melting/boiling point of covalent network bonding?
Very high.
Due to the very strong electrostatic attraction between the positive nucleus and the shared pair(s) of electrons that requires a considerable amount of energy to disrupt (the bond between the atoms must be broken).
What is the conductivity - as (s), (l) and (aq) of metallic bonding?
Will conduct as a solid and a liquid.
The delocalized electrons are free to move within the cations’ structure, meaning that it can carry a charge.
What is the conductivity - as (s), (l) and (aq) of ionic bonding?
As a solid: will not conduct as all ions are in fixed positions.
As a liquid, or aqueous: will conduct because the ions are free to move and can carry a charge.
What is the conductivity - as (s), (l) and (aq) of covalent molecular bonding?
Will not conduct, free moving charged particles are required for a substance to conduct electricity, and all electrons are involved in bonding.
