Elements forming ionic compounds attain noble gas configuration by either gaining or losing electrons from their outermost shells. Give reason to explain why carbon cannot attain a noble gas configuration in this manner to form its compounds. Name the type of bonds formed in ionic compounds and in the compounds formed by carbon. Also, give a reason why carbon compounds are generally poor conductors of electricity.
Elements forming ionic compounds attain noble gas configuration by either gaining or losing electrons from their outermost shells. Give reason to explain why carbon cannot attain a noble gas configuration in this manner to form its compounds. Name the type of bonds formed in ionic compounds and in the compounds formed by carbon. Also, give a reason why carbon compounds are generally poor conductors of electricity.
The atomic number of Carbon () is six. In the outermost shell, it has four electrons. So, a very high energy is needed to eject four electrons from carbon to form .
Carbon cannot gain four electrons to form as it has six protons so, it is difficult to hold ten electrons. Therefore, carbon cannot attain a noble gas configuration.
Two types of bonds are formed in the carbon compounds.
(i) Covalent bonds
(ii) Ionic/Electrovalent bonds
Covalent compounds are those compounds in which the atoms share one or more pairs of electrons present in their valence shells.
The atoms in covalent compounds are held together by covalent bonds.
Example: Hydrogen chloride HCl is a covalent compound containing one chlorine atom.
Electrovalent compounds or ionic are those compounds in which the complete transfer of electrons takes place from one atom to another atom.
These compounds contain an ionic bond between their atoms.
Example: Sodium chloride NaCl and magnesium chloride MgCl2 are electrovalent compounds.
Ionic compounds are formed by the reaction of metals with non-metals.
In the formation of an ionic compound, metals lose their electron to complete octets and non-metals accept electrons to complete their octet.
Ionic compounds are held together by ionic bonds because metal and non-metal ions react to form ionic compounds.
Example: NaCl
In the carbon compounds, all the electrons are shared, and charged particles are not formed.
So, due to a lack of free electrons, carbon compounds are generally poor conductors of electricity.
Example: Diamond is a non-conductor of electricity.
The atomic number of Carbon () is six. In the outermost shell, it has four electrons. So, a very high energy is needed to eject four electrons from carbon to form .
Carbon cannot gain four electrons to form as it has six protons so, it is difficult to hold ten electrons. Therefore, carbon cannot attain a noble gas configuration.
Two types of bonds are formed in the carbon compounds.
(i) Covalent bonds
(ii) Ionic/Electrovalent bonds
Covalent compounds are those compounds in which the atoms share one or more pairs of electrons present in their valence shells.
The atoms in covalent compounds are held together by covalent bonds.
Example: Hydrogen chloride HCl is a covalent compound containing one chlorine atom.
Electrovalent compounds or ionic are those compounds in which the complete transfer of electrons takes place from one atom to another atom.
These compounds contain an ionic bond between their atoms.
Example: Sodium chloride NaCl and magnesium chloride MgCl2 are electrovalent compounds.
Ionic compounds are formed by the reaction of metals with non-metals.
In the formation of an ionic compound, metals lose their electron to complete octets and non-metals accept electrons to complete their octet.
Ionic compounds are held together by ionic bonds because metal and non-metal ions react to form ionic compounds.
Example: NaCl
In the carbon compounds, all the electrons are shared, and charged particles are not formed.
So, due to a lack of free electrons, carbon compounds are generally poor conductors of electricity.
Example: Diamond is a non-conductor of electricity.
