Represent the formation of cations for the following metal atoms using electron dot structures:

When metals form cations, they lose electrons. This is because metals tend to have fewer electrons in their outer shell and can achieve a more stable configuration by losing those electrons. Here’s how the cations for the given metals are formed:

  • (a) Barium (Ba): Barium is in Group 2, so it has 2 valence electrons. To form a cation, barium loses these 2 electrons, resulting in a Ba²⁺ ion. The electron dot structure for Ba before and after ionization is:

    Before: [Ba] → 2 valence electrons in the outer shell

           After: [Ba²⁺] → No valence electrons (lost both electrons)

  • (b) Aluminum (Al): Aluminum is in Group 13, so it has 3 valence electrons. When aluminum forms a cation, it loses these 3 electrons, resulting in an Al³⁺ ion. The electron dot structure for Al before and after ionization is:

    Before: [Al] → 3 valence electrons in the outer shell

    After: [Al³⁺] → No valence electrons (lost all 3 electrons)

  • (c) Strontium (Sr): Strontium is in Group 2, so it has 2 valence electrons. Strontium loses these 2 electrons to form a Sr²⁺ ion. The electron dot structure for Sr before and after ionization is:

    Before:[Sr] → 2 valence electrons in the outer shell

    After: [Sr²⁺] → No valence electrons (lost both electrons)

In all of these examples, the metals lose electrons because they have relatively few electrons in their outer shells and can achieve a stable electron configuration by losing them. As a result, they become positively charged cations.

Related Questions:

  1. Explain how elements attain stability.
  2. Describe the ways in which bonds may be formed.
  3. Describe the formation of a covalent bond between two non-metallic elements.
  4. Explain with examples single, double, and triple covalent bonds.
  5. Find the number of valence electrons in the following atoms using the periodic table:
  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: