Comparison of physical properties of elements in Group 2 and Group 14.
Answers
Answer:
What are Group 14 Elements?
The group 14 elements are the second group in the p-block of the periodic table. It is also called the carbon group. The members of this group are:
Carbon (C)
Silicon (Si)
Germanium (Ge)
Tin (Sn)
Lead (Pb)
Flerovium (Fl)
Table of Content
Electronic Configuration
Oxidation States
Anomalous Behaviour of Carbon
Chemical Properties
Physical Properties
Compounds of Group 14 Elements
Electronic Configuration of Group 14 Elements
The group 14 elements have a general electronic configuration of ns2np2. These elements have 2 electrons in the outermost p orbitals. The electronic configuration of these elements is shown below:
Group 14 Elements
Period
Element
Atomic No.
Electronic Configuration
2nd Carbon (C) 6 [He]2s2 2p2
3rd Silicon (Si) 14 [Ne]3s2 3p2
4th Germanium (Ge) 32 [Ar]3d10 4s2 4p2
5th Tin (Sn) 50 [Kr]4d10 5s2 5p2
6th Lead (Pb) 82 [Xe]4f14 5d10 6s2 6p2
As all the elements in group 14 have 4 electrons in the outermost shell, the valency of group 14 elements is 4. They use these electrons in the bond formation in order to obtain octet configuration.
Oxidation States and Inert pair Effect of Group 14 Elements
The general oxidation states exhibited by the group 14 elements are +4, and +2.
As we go down the group, the tendency to form +2 ion increases. This is due to inert pair effect. This effect is exhibited by p-block elements.
This can be explained using the inert pair effect. It is the non-participation of the s-orbital during bonding due to the poor shielding of the intervening electrons.
⇒ Check: List of all periodic table elements
For elements like Sn and Pb, d and f orbitals are filled with electrons. Since the shielding ability of d and f orbitals are very poor, the nuclear charge that seeps through attracts the s orbital closer to the nucleus. This makes the s orbital reluctant to bond, thereby only the p electrons involved in bonding.
Therefore, Pb4+ is a very good oxidizing agent.
⇒ Also Read:
Silicon
Germanium
Tin
Lead
Flerovium
Anomalous Behaviour of Carbon
Carbon exhibits different behaviour from the rest of the group due to,
Small Size
High Electronegativity
High Ionization Enthalpy
Absence of d-orbital in the Valance Shell
Chemical Properties of Group 14 Elements
Covalent Radii
The radii of group 14 elements are lesser than that of group 13 elements. This can be explained by the increase in the effective nuclear charge.
The increase in the radii from C to Si is considerable, after which the increase in the radii is less. This can be attributed to the poor shielding of d and f orbitals, which increase the effective nuclear charge,