Electrovalent Compounds:
Those compounds which contain electrovalent or ionic bond are called
electrovalent compounds.
These compounds are also called ionic compounds because the bond
keeping the molecules of this compound together is ionic bond which is
formed by the complete transfer of electrons from atom of one element
to another resulting in a positively and a negatively charged ion.
These compounds are usually formed by chemical reaction between atoms
of a metal and non-metal wherein, non-metal receives an electron from
metal.
Example of such compound can be Sodium Chloride (NaCl) where Sodium
(Na) transfers 1 electron from its valence shell and becomes positively
charged Na+ ion and Chlorine (Cl) gains 1 electron and becomes Cl- ion.
A strong electrostatic force of attraction binds the two oppositely charged
ions together which greatly outweighs the force of repulsion between
similarly charged ions as each ion is surrounded by oppositely charged
ions.
A diagram of transfer of electron from Sodium to Chloride which result in
the formation of Sodium Chloride is given below:
, Sodium Chloride’s formation can also be represented by Lewis structure as
follows:
Electrovalent bond:
The bond formed which is formed by complete transfer of electron from
one atom to another is called electrovalent bond.
This transfer creates charged ions due to which it is also called ionic bond.
There exists a strong electrostatic force of attraction between the ions
which binds the atoms of the same molecule together.
Such type of bond generally exists between a metal and a non-metal.
Characteristics of Electrovalent compounds:
Physical state: Such compounds generally exists in solid state at room
temperature. It is because of the strong coulombic (electrostatic) force of
attraction between the atoms holds them in solid shape.
Melting and boiling point: These compounds have high melting and
boiling points. It is because molecules of these compounds exist in
crystalline solid structure having high lattice energy due to which a large
amount of energy is required to break the atoms which results in high
melting and boiling points.
Compound Melting Point Boiling Point
0
1. Sodium Chloride 801 C 1413oC
2. Magnesium oxide 28520C 36000C
3. Aluminum oxide 20720C 29770C
Solubility: Ionic compounds are generally soluble in polar solvents of
water and insoluble in non-polar solvents like carbon tetrachloride (CCl4).
The solubility of these compounds also depends upon the difference
between lattice energy (energy required to break 1 mole of a solid ionic
Those compounds which contain electrovalent or ionic bond are called
electrovalent compounds.
These compounds are also called ionic compounds because the bond
keeping the molecules of this compound together is ionic bond which is
formed by the complete transfer of electrons from atom of one element
to another resulting in a positively and a negatively charged ion.
These compounds are usually formed by chemical reaction between atoms
of a metal and non-metal wherein, non-metal receives an electron from
metal.
Example of such compound can be Sodium Chloride (NaCl) where Sodium
(Na) transfers 1 electron from its valence shell and becomes positively
charged Na+ ion and Chlorine (Cl) gains 1 electron and becomes Cl- ion.
A strong electrostatic force of attraction binds the two oppositely charged
ions together which greatly outweighs the force of repulsion between
similarly charged ions as each ion is surrounded by oppositely charged
ions.
A diagram of transfer of electron from Sodium to Chloride which result in
the formation of Sodium Chloride is given below:
, Sodium Chloride’s formation can also be represented by Lewis structure as
follows:
Electrovalent bond:
The bond formed which is formed by complete transfer of electron from
one atom to another is called electrovalent bond.
This transfer creates charged ions due to which it is also called ionic bond.
There exists a strong electrostatic force of attraction between the ions
which binds the atoms of the same molecule together.
Such type of bond generally exists between a metal and a non-metal.
Characteristics of Electrovalent compounds:
Physical state: Such compounds generally exists in solid state at room
temperature. It is because of the strong coulombic (electrostatic) force of
attraction between the atoms holds them in solid shape.
Melting and boiling point: These compounds have high melting and
boiling points. It is because molecules of these compounds exist in
crystalline solid structure having high lattice energy due to which a large
amount of energy is required to break the atoms which results in high
melting and boiling points.
Compound Melting Point Boiling Point
0
1. Sodium Chloride 801 C 1413oC
2. Magnesium oxide 28520C 36000C
3. Aluminum oxide 20720C 29770C
Solubility: Ionic compounds are generally soluble in polar solvents of
water and insoluble in non-polar solvents like carbon tetrachloride (CCl4).
The solubility of these compounds also depends upon the difference
between lattice energy (energy required to break 1 mole of a solid ionic
