S and P Block Elements

The elements in the long form of the periodic table has been divided into four blocks, namely s, p, d & f blocks. The elements of group I & II receive their last electron in s-orbital. So they are called as s – block elements.

The elements of group II are Berryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), barium (Ba) and radium (Ra) which have two electrons in their outermost shell.

All these elements are also metallic in nature and are commonly known as alkaline earth metals with the exception of beryllium. Because of their low density, alkali metals and alkaline earth metals are called lighter metals.

Both alkali and alkaline earth metals are highly reactive and hence do not occur in free state but found in combined state. Whereas alkali metals mostly occur as halides, oxides, silicates, borates and nitrates, alkaline earth metals mainly occur as silicates, carbonates, sulphates and phosphates.

Some alkali & alkaline earth metals occur abundantly in nature. Calcium is the fifth, magnesium is the sixth, sodium is seventh and potassium is eight barium is the fourteenth and strontium is the fifteenth most abundant element by weight in the earth’s crust. Sodium and magnesium are also present in sea water brine wells and few salt lakes.

Anamolous behavour of first element

The first element of a group differs considerably from the rest of the elements of the same group. This anomolous behaviour is due to

• Smaller size of their atoms

• Their higher ionization energies

• Their higher electronegativites

• Absence of vacant d – orbitals in their valence shell

• High polarizing power of its cation.

Thus Li differes from the rest of alkali metals (Na, K, Rb & Cs) and Be differs from rest of the alkaline earth metals (Mg, Ca, Sr & Ba)

Diagonal Relationships

On moving diagonally some members show similar properties with the members of next higher group which is particularly seen in the elements of second and third periods of the periodic table. However the similarities shown are far less pronounced than the similarities with in a group.

The main reasons for the diagonal relationship are

• Similarity in electropositive character: The electropositive character decreases along a period, but increases down a group. Hence on moving diagonally the two opposing trend       partially cancels out. As a result diagonally related elements have similar electropositive character and hence exhibit similar properties.

• Similarity in polarizing power: On moving along a period from left to right, the charge on the ions increases while ionic size decreases, hence polarizing power increases. On moving down the group, the ionic size increases and hence polarizing power decreases. On moving diagonally, these two trends partially cancel out. As a result thus diagonally related elements have same polarizing power and thus exhibit similar properties.

• Similarity in atomic or ionic radii: The atomic and ionic radii decrease across a period and increase in a group. Evidently on moving diagonally, the two trends partially cancel  out. As a result, diagonally related elements have similar atomic &  ionic radii and hence have similar properties.