Atoms form bonds in order to achieve stability by filling their outermost electron shell. This is known as the octet rule, where atoms strive to have a full valence shell containing 8 electrons (2 for hydrogen). By forming bonds, atoms can share, donate, or receive electrons to attain this stable configuration.
Types of bonds include:
1. **Ionic bonds:** In ionic bonding, one atom transfers electrons to another, resulting in the formation of positive and negative ions that are attracted to each other due to their opposite charges. For example, sodium (Na) can transfer an electron to chlorine (Cl) to form sodium chloride (NaCl) – table salt.
2. **Covalent bonds:** In covalent bonding, atoms share electrons to complete their valence shells. This sharing of electrons allows each atom to achieve stability. An example is water (H₂O), where oxygen shares electrons with hydrogen to form a stable molecule.
3. **Metallic bonds:** Metallic bonding occurs in metals where electrons are delocalized and free to move throughout the material. This allows metals to conduct electricity and heat efficiently.
Overall, by forming bonds, atoms can achieve a more stable configuration, lower their energy state, and increase their likelihood of existing in a more energetically favorable state.
