how would hydrogen ions and hydroxide ions be attracted to intact water molecules
Hydrogen ions (H+) and hydroxide ions (OH-) are attracted to intact water molecules through a process called hydrogen bonding. To understand this, we need to look at the structure of water.
Water molecules (H2O) are made up of two hydrogen atoms covalently bonded to an oxygen atom. Due to the large electronegativity difference between oxygen and hydrogen, the oxygen atom has a partial negative charge (δ-) while the hydrogen atoms have partial positive charges (δ+).
When a hydrogen ion (H+) is present in a solution, it is essentially a lone proton with a positive charge. This positive charge of the hydrogen ion is attracted to the partial negative charge on the oxygen atom of a water molecule. The oxygen atom serves as the electronegative partner and forms a short-lived bond with the hydrogen ion. This attraction is responsible for the acid-base properties of water and why it can act as a proton donor.
On the other hand, a hydroxide ion (OH-) consists of an oxygen atom with a negative charge and a hydrogen atom. The partial negative charge on the oxygen atom of the hydroxide ion is attracted to the partial positive charge on a nearby water molecule's hydrogen atom. Similarly, a hydrogen bond is formed between the hydroxide ion and water molecule due to this electrostatic attraction.
Overall, hydrogen ions and hydroxide ions are attracted to intact water molecules due to the dipole-dipole interactions formed through hydrogen bonding. These interactions play a crucial role in various chemical reactions and the behavior of acids and bases in aqueous solutions.