- #1
meemoe_uk
- 125
- 0
Hello.
Covalent bonding molicules, right, are usually in lower quantum energy states. e.g. for a typical dihydrogen mol at air temp, the 2 electrons are often in the first or second lowest quantum state.
But, natch, the molicule can still exist with the electron at higher quantum states.
In air, there is a practical limit to how high up the quantum states the electrons can go before the molicule splits.
But how high can the electrons go in theory and still preserve the molicule?
In a very low energy enviroment, I don't see why high energy electron orbits i.e. the classical orbits, could not be exist and be stable.
If 'classical' covalent bonding is possible under such circumstances, isn't it true that most particles in the universe are subject this long range covalent bonding, it's just the attractive force is so weak as to be negligable?
Covalent bonding molicules, right, are usually in lower quantum energy states. e.g. for a typical dihydrogen mol at air temp, the 2 electrons are often in the first or second lowest quantum state.
But, natch, the molicule can still exist with the electron at higher quantum states.
In air, there is a practical limit to how high up the quantum states the electrons can go before the molicule splits.
But how high can the electrons go in theory and still preserve the molicule?
In a very low energy enviroment, I don't see why high energy electron orbits i.e. the classical orbits, could not be exist and be stable.
If 'classical' covalent bonding is possible under such circumstances, isn't it true that most particles in the universe are subject this long range covalent bonding, it's just the attractive force is so weak as to be negligable?