2.2.2 Bonding and structure Flashcards
State the three main types of chemical bonds?
ionic, covalent, metallic
Define ionic bonding
Electrostatic attraction between oppositely charged ions
Define covalent bonding
Electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms
Define metallic bonding
Electrostatic attraction between positive metal ions and delocalised electrons
Explain how the conductivity of an ionic compound changes in solid and liquid state
solid - non-conductive as ions are fixed in position
liquid - conductive as ions are mobile and can carry charge
Explain why ionic compounds have high melting and boiling points
Ionic compounds have a high melting and boiling point as the electrostatic attraction between oppositely charged ions is strong and requires a lot of energy to overcome.
Explain the solubility of ionic compounds
Ionic compounds are soluble in polar solvents.
The oppositely charged ions are attracted to the slightly charged atoms of the solvent.
What is a single covalent bond?
Atoms bonded by a single pair of shared electrons
Define multiple covalent bonding
Atoms share more than one pair of electrons - double or triple bond.
Define dative covalent bond
The electrons in the shared pair are supplied by one atom
What is a lone pair?
Electrons in the outer shell that are not involved in bonding
Define average bond enthalpy
A measurement of covalent bond strength
The average energy needed to break the bond
Describe the bonding in simple molecular lattice structure
Atoms within a molecule are held by strong covalent bonds, each molecule is attracted to each other by weak intermolecular forces.
Explain the low melting point of simple molecular structures
Weak intermolecular forces require little energy to overcome
Explain the conductivity of simple molecule structures
Non-conductive
No free charged particles in the structure
Explain the solubility of simple molecular structures
Soluble in non-polar solvents
State and explain the properties of giant covalent structures e.g. graphite, silicon dioxide, diamond
High melting and boiling points - strong covalent bonds require a lot of energy to overcome
Non conductive - no free charged particles in structure (except graphite)
Insoluble - strong covalent bonds require a lot of energy to overcome
Why is graphite conductive?
Each carbon atom in graphite form three covalent bonds with other carbon atoms
The delocalised electrons are free to move
Describe linear shape and angle
2 bonding pairs, 0 lone pairs
180 degree angle
Describe trigonal planar shape and angle
3 bonding pairs, 0 lone pairs
120 degree angle
Describe tetrahedral structure and bond angle
4 bonding pairs, 0 lone pairs
109.5 degree angle
Describe trigonal bi-pyramidal shape and bond angles
5 bonding pairs, 0 lone pairs
90 and 120 degree angles
Describe octahedral shape and angle
6 bonding pairs, 0 lone pairs
90 degree angle
describe pyramidal shape, bond angle and give an example
3 bonding angles, 1 lone pair
107 degree angle
NH3