Comparison between Polar and Non-polar compounds for class 10 ICSE

Comparison between Polar and Non-polar compounds

Polar covalent and non polar molecules

Polar molecules	Non-polar molecules
1.      Due to the electronegativity difference between the atoms the electrons are distributed unequally which leads to charge separation.	1.  There is no charge separation since the electron pair is equally distributed between the atoms.
2.      Example: HCl, H2O , NH3 etc.	2. Example: H2, Cl2, O2, N2, CCl4, CH4 etc

 

Ø  Charge separation in Hydrogen chloride molecule:

In HCl molecule Chlorine is more electronegative than Hydrogen so the electron pair is more strongly attracted by Chlorine atom due this a slight negative charge is developed on Chlorine and a slight positive charge on Hydrogen atom. Hence it becomes a polar compound

Class 10 Chemical bonding ICSE notes

 Class 10 Chemical bonding icse notes 

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Electrovalent bond (or) Ionic bond :

The electrostatic force of attraction which binds two or more oppositely charged ions formed by the transfer of electron/s from the metal atom to the non metal atom.

Electrovalent compound: The compounds formed as a result of the transfer electrons.

Electrovalency: The number of electrons lost or gained by an atom of an element to attain stability.

The electrovalent bond is possible between a metal and a non metal. The metal atom atom loses electron/s to nonmetal atom so that the metal and the nonmetal attain stable electronic configuration.

 

Formation of Electrovalent compounds - Electron dot representation

ü  As the metal loses electron/s it is oxidized and forms a cation (positive ion).

Oxidation:

Na – e^-  -->Na⁺

Mg – 2e^- --> Mg²⁺

ü  The non metal atom accepts electron/s and it is reduced to form an anion (negative ion).

Reduction:

Cl₂ + 2e^-   -->2Cl^-

O₂ + 4e^-  --> 2O^2-

Formation of Electrovalent (Ionic) Compounds:

 

Example 1 Sodium chloride ( NaCl):

Sodium is a metal with electronic configuration 2,8,1 – has one valence electron.

Chlorine is a non metal with electronic configuration 2,8,7 – has 7 valence electrons.

 

Sodium has to lose one electron from its valence shell to attain the electronic configuration of its nearest noble gas (Neon) i.e. 2, 8.

 

Chlorine has gain one electron for the electronic configuration of its nearest noble gas (Argon) i.e 2,8,8

Hence Sodium loses its one electron from the valence shell to the chlorine atom.

Representation of Sodium Chloride using electron dot structures

 

Example 2    Magnesium Oxide (MgO)

Mg – electronic configuration is 2, 8, 2- it loses 2 electrons

O – electronic configuration is 2,6 – it has to gain two electrons.

One Magnesium atom donates two electrons to the Oxygen atom.

Example 3 Magnesium Chloride (MgCl₂)

Mg – 2,8,2 – Mg atom has to lose 2 electrons and

Cl – 2,8,7 – each Chlorine atom requires one more electron to get the stable electronic configuration.

Hence Mg atom donates one electron to each chlorine atom.

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CHEMICAL BONDING ICSE class 10 NOTES

CHEMICAL BONDING Class 10 ICSE NOTES

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