why does water after evaported not turn to H+ ions.
is it be cause of the intermolecurar and intramolecuar forces?
When water evaporates, it undergoes a phase change from a liquid to a gas, but it does not turn into H+ ions. This is because H+ ions, also known as hydrogen ions, are formed when water molecules dissociate in an aqueous solution, such as in an acidic or alkaline solution.
In pure water, the majority of water molecules exist as intact H2O molecules. These water molecules are held together by strong intramolecular forces such as covalent bonding between hydrogen and oxygen atoms within each molecule. These covalent bonds are very stable and do not break during evaporation.
The process of water evaporation is driven by intermolecular forces, specifically hydrogen bonding. Hydrogen bonding occurs between the positively charged hydrogen atoms of one water molecule and the negatively charged oxygen atoms of neighboring water molecules. This bonding is relatively weaker than the intramolecular forces within each water molecule.
As the temperature of the water increases, the kinetic energy of the water molecules also increases. Some of the water molecules acquire enough energy to overcome the intermolecular forces and escape from the liquid phase into the gas phase, forming water vapor. During evaporation, the intact H2O molecules are released as a gas, without breaking apart to form H+ ions.
So, the reason why water does not turn into H+ ions during evaporation is primarily due to the nature of the intramolecular and intermolecular forces that hold water molecules together and the conditions under which evaporation occurs.