Explain how elements attain stability.

Elements attain stability by achieving a full outer electron shell, similar to the electron configuration of a noble gas. This can be accomplished in several ways:

  1. By losing electrons: Metals tend to lose electrons to achieve a stable configuration, forming cations.

  2. By gaining electrons: Non-metals tend to gain electrons, forming anions.

  3. By sharing electrons: Atoms can share electrons in covalent bonds to complete their outer shells.

The attainment of a stable electron configuration minimizes the atom’s energy and makes it chemically inert or reactive in a more predictable manner.

Related Questions:

  1. Describe the ways in which bonds may be formed.
  2. Describe the formation of a covalent bond between two non-metallic elements.
  3. Explain with examples single, double, and triple covalent bonds.
  4. Find the number of valence electrons in the following atoms using the periodic table:
  5. Represent the formation of cations for the following metal atoms using electron dot structures:
  6. A sample of sulfur from a volcano was analyzed to give the following composition of isotopes (Atomic No. of S = 16):
  7. An atom of an element has an atomic number of 9 and a mass number of 19:
  8. Define ionic bond and give an example.
  9. State octet and duplet rules.
  10. Explain the formation of a covalent bond between two nitrogen atoms.
  11. How does Al form a cation?
  12. Draw an electron cross and dot structure for an H₂O molecule.
  13. Describe the importance of noble gas electronic configuration.
  14. The atomic number of an element is 23, and its mass number is 56.
  15. The atomic symbol of aluminum is written as Al. What information do you get from it?
  16. Write the valence shell electronic configuration of an element present in the 3rd period and Group IIA.
  17. Define halogens.
  18. Which atom has a higher shielding effect, Li or Na?
  19. Explain why Na has higher ionization energy than K.
  20. Arrange the elements in each of the following groups in order of increasing ionization energy: