2.5 Electrons, bonding & structure (Spec) Flashcards
Main energy level
Determines principal quantum number
s-orbital
spherical shape
lowest energy
present in all main energy levels
1 per s sub-shell
Electron sub-shell
Group of orbitals with same shape and energy
Atomic orbital
Region of electron density holding 2 electrons of opposite spins
Electron
Cloud of relative charge -1
Relative mass 1/1836
p-orbital
dumbbell shape
second-lowest energy
present in energy levels w/ PQN 2 and above
3 per p sub-shell
d-orbital
third-lowest energy
present in energy levels w/ PQN 3 and above
5 per d sub-shell
f-orbital
highest energy
present in energy levels w/ PQN 4 and above
7 per f sub-shell
Ionic bond
Strong electrostatic attraction between oppositely charged ions, extending in all directions in giant ionic lattice.
Ionic lattice melting point
High - strong electrostatic attraction between oppositely charged ions extends in all directions, requires lots of energy to overcome, resulting in a high temperature
Ionic lattice solubility
Soluble in polar solvents (partial charges on solvent molecules weaken electrostatic attraction between ions), insoluble in non-polar solvents
Ionic lattice electrical conductivity
Solid - does not conduct as no charged particles free to move due to strength of electrostatic attraction in all directions
Molten or aqueous - conducts as ions are free to move and carry charge as electrostatic attraction between ions is overcome
Covalent bond
Strong electrostatic attraction between a shared pair of electrons and the bonded nuclei
Dative covalent bond
Both of the shared pair of electrons are donated by one atom in a covalent bond
Bond enthalpy - bond strength relationship
Increased bond enthalpy, increased bond strength
