1. Bond Formation:
* Ionic: Formed through the transfer of electrons from a metal to a nonmetal. This creates ions with opposite charges that attract each other strongly, forming an electrostatic bond.
* Covalent: Formed through the sharing of electrons between two nonmetals. These shared electrons create a stable, more balanced electron configuration for both atoms.
2. Physical Properties:
* Ionic: Typically solids at room temperature with high melting and boiling points. This is because the strong electrostatic forces require a lot of energy to overcome. They are often brittle due to the rigid structure of the crystal lattice.
* Covalent: Can exist as solids, liquids, or gases at room temperature, depending on the specific compound. Generally have lower melting and boiling points than ionic compounds. They can be flexible due to the weaker nature of the bonds.
3. Solubility:
* Ionic: Often soluble in water due to the polar nature of water molecules being able to interact with the charged ions.
* Covalent: Vary in solubility, with some being soluble in water (e.g., sugars) and others being insoluble (e.g., oils). The solubility depends on the polarity of the molecule and the ability of the water molecules to form hydrogen bonds.
In summary: Ionic compounds are formed by the transfer of electrons, are usually solid and strong, and dissolve well in water. Covalent compounds are formed by the sharing of electrons, can exist in various states, have weaker bonds, and show varying solubility in water.
