The Diagonal Relationship Within S-Block Elements

The Diagonal Relationship Within S-Block Elements

A diagonal relationship in S-block elements exists between adjacent elements which are located in the second and third period of the periodic table. For example, Lithium of group 1A and second period shows similarities with the properties of magnesium which are located in the 2nd group and 3rd period. Similarly, properties of beryllium which are located in 2nd group and 2nd period show a likeness with properties of aluminum which is located in the third period and third group. The two elements which show similarities in their properties can be called a diagonal pair or diagonal neighbors. The properties of these elements vary significantly when compared to the other elements of the sub-group they belong to. The diagonal neighbors show a lot of similarities. Such a relationship is exhibited as you move left to right and down the group; the periodic table has opposing factors. For example, the electronegativity of the elements increases as we go across the period and decreases as we go down the group. Therefore when it is moved diagonally the opposite tendencies cancel out and the value of electronegativity almost remains same.

Similarities between Lithium and magnesium:

  • The hardness of lithium and magnesium is higher than the other elements in their respective groups.
  • Chlorides of lithium and magnesium have the capability to be soluble in ethanol.
  • They are lighter when compared to other elements in their groups.
  • Lithium and magnesium react gently with water. The oxides and hydroxides are less soluble.
  • In the presence nitrogen, lithium and magnesium form their respective nitrides.
  • Superoxides are not formed when lithium and magnesium react with excess oxygen.
  • Carbon dioxide and their respective oxides are formed when carbonates of magnesium and lithium are heated.

Similarities between beryllium and aluminum:

  • Aluminium hydroxide and beryllium hydroxide react with excess alkali to form their respective ions.
  • Both these elements have the capacity to withstand the acid attack due to the presence of an oxide film on the surface of the metal.
  • Both these metals have the tendency to form complexes.
  • Chlorides of both these metals possess the capacity to be soluble in organic solvents.

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Practise This Question

Which of the following is the electronic configuration of the outer most two subshells of the alkali metals