Explain the position and properties of alkali metals and halogens in the periodic table. Why do they react so easily with each other?

Alkali metals, found in Group 1 of the periodic table, are highly reactive, soft metals with low melting points. They have one electron in their outermost shell, which they easily lose to form positive ions (cations). Examples include lithium (Li), sodium (Na), and potassium (K). Halogens, found in Group 17, are highly reactive nonmetals with seven electrons in their outer shell, making them eager to gain one electron to form negative ions (anions). Examples include fluorine (F), chlorine (Cl), and bromine (Br).

Alkali metals and halogens react easily with each other because of their complementary electron configurations. Alkali metals readily lose their single outer electron, while halogens readily gain an electron. This electron transfer results in the formation of ionic compounds, such as sodium chloride (NaCl) or potassium bromide (KBr), in which the alkali metal becomes positively charged, and the halogen becomes negatively charged, leading to a stable ionic bond.

Related Questions:

  1. Arrange the elements in each of the following in order of decreasing shielding effect:
  2. Specify which of the following elements you would expect to have the greatest electron affinity: S, P, Cl
  3. Electronic configurations of some elements are given below. Group the elements in pairs that would represent similar chemical properties:
  4. Arrange the elements in groups and periods from Q. No. 6:
  5. For normal elements, the number of valence electrons of an element is equal to the group number. Find the group number of the following elements:
  6. Write the valence shell electronic configuration for the following groups:
  7. Write the valence shell electronic configuration of the atoms of the following elements:
  8. In which block, group, and period in the periodic table would you place each of the following elements with the given electronic configurations?
  9. Explain the trends of atomic size, ionization energy, and electron affinity in the periodic table with suitable examples.
  10. Describe the significance of Mendeleev’s periodic law and how it helped in the development of the modern periodic table.
  11. Write the valence shell electronic configuration of an element present in the 3rd period and Group IIA.
  12. Define halogens.
  13. Which atom has a higher shielding effect, Li or Na?
  14. Explain why Na has higher ionization energy than K.
  15. Alkali metals belong to the S-block in the periodic table. Why?
  16. Arrange the elements in each of the following groups in order of increasing ionization energy:
  17. Why does atomic radius decrease across a period from left to right?
  18. Why do noble gases have high ionization energy?
  19. Why are alkali metals highly reactive?
  20. What is periodicity in the periodic table?