bonding
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covalent
shared electrons
strength of covalent bond
energy required to break molecules into constituent atoms
single covalent bond energy
150-350
double c. bond energy
greater
Ionic bonding
regular array of cations and anions via electrostatic interactions
repulsion
the attractive interaction between the ions overide the repulsion force of alike ions.
in covalent bonds the
electrostative interactions are not directional
strength of ionic bond
it is calculated by taking solid ionic and separating them into infinity. (lattice energy)
metallic bonding
cations held together by a sea of electron
dispersion interaction
electron density fluctuates over time. it may become unsymetrical creating partial charges. it geneates electron density to change in other molecules as if it is slightly positive, the electron density changes. etc
the larger the induce dipole
the stronger the interaction
the size of the dipole depends on
how much a given electric field will be disorted by the electron distribution
the more polarizable
the greater the induced dipole
if the bonds are strong the polarisation is
low
covalent bonds are
directional
covalent character in ions
t arguments can be refined using Fajan’s Rules. Ostensibly they give an empirical measure of polarisability, which is a measure of how easily an electron cloud is distorted by an electric field It weighs up 2 factors: 1. Size of the ion: Smaller cation, and larger anion, give greater covalent character. 2. The charge of cation: Greater the charge of cation, greater is the covalent character of the bond. Some versions of Fajans Rules quot