Ionic bonding: In ionic bonding, atoms achieve stability by transferring electrons to or from other atoms, resulting in the formation of positively charged ions (cations) and negatively charged ions (anions). The electrostatic attraction between the oppositely charged ions holds the ionic compound together. For example, in sodium chloride (NaCl), sodium loses one electron to chlorine, forming Na+ and Cl- ions. The strong electrostatic attraction between Na+ and Cl- ions leads to the formation of a stable ionic compound.

Covalent bonding: In covalent bonding, atoms achieve stability by sharing electrons. When atoms share electrons, they form a covalent bond. This shared electron pair is located between the nuclei of the bonded atoms, creating a region of high electron density. The attraction between the positively charged nuclei and the negatively charged electrons holds the atoms together. For example, in the covalent molecule methane (CH4), each carbon atom shares four electrons with four hydrogen atoms, forming four covalent bonds. The sharing of electrons results in a stable molecule.

Here's a table summarizing the key differences between ionic and covalent bonding:

| Property | Ionic Bonding | Covalent Bonding |

|---|---|---|

| Electron transfer | Complete transfer of electrons from one atom to another | Sharing of electrons between atoms |

| Type of bond | Electrostatic attraction between oppositely charged ions | Attraction between positively charged nuclei and negatively charged electrons shared between atoms |

| Formation of ions | Forms ions (cations and anions) | Does not form ions |

| Examples | Sodium chloride (NaCl), potassium iodide (KI), calcium oxide (CaO) | Methane (CH4), water (H2O), carbon dioxide (CO2) |