Chemical Bonding Flashcards
ionic bonding
Mutual strong electrostatic force of attraction between 2 oppositely charged ions
Name of ionic structure
Giant ionic crystal lattice structure
Name and description of ionic structure
Giant ionic crystal lattice structure, 3D structure (exists only in solid state) consisting of positive and negative ions
Electrical conductivity of ionic structure in aqueous and molten state
In the aqueous or molten state, the ionic structure is a good conductor of electricity. The ions in the lattice are mobile (Can move arnd freely) in this state and hence can conduct electricity (it only has the 3D structure in solid state)
Melting and boiling point of ionic structure
Due to the strong electrostatic forces of attraction between oppositely charged ions in the giant ionic crystal lattice, a large amount of energy is required to overcome these strong forces. Hence ionic structures have a high melting and boiling point and are solids at room temperature.
Electrical conductivity of ionic structure in solid state
In the solid state, ionic structures cannot conduct electricity. Ions in the lattice in the solid state can only vibrate about in fixed positions. Hence, the ions in the lattice are not mobile and cannot conduct electricity in the solid state.
Hardness of ionic structure
Ionic compounds are hard and brittle.
HARDNESS:
- The strong electrostatic forces of attraction between oppositely charged ions make ionic compounds resistant to deforming
- The attractive forces cause ions to resist motion
BRITTLE:
- When enough force is applied, ions moved away from their lattice positions and ions of the same charge approach each other.
- The repulsive forces between ions of similar charges becomes greater than the attractive forces, causing the lattice structure to shatter.
Hence the ionic structure is hard but brittle.
Solubility of ionic structure
Most ionic compounds are soluble in water and insoluble in organic solvent. When ionic compounds are dissolved in water, they are in the AQUEOUS state.
Description of metallic bonding
Strong electrostatic force of attraction between positive cation and sea of delocalised electrons
Name and description of metallic structure
Giant metallic lattice structure, held together by a sea of mobile (delocalised) electrons. The free movement of electrons amongst the evenly distributed metal ions is the most important difference between metallic bonding and other types of bonding.
Melting and boiling point of metallic structure
Electronegativity
Ability of the atoms in a covalent bond to attract electrons to itself
