Polar Covalent Bond AND Characteristics of Polar Covalent Compounds

Polar Covalent Bond

                                    In the covalent compound if one is the more is more electronegative than other atom, then shared pair of electrons is attracted towards more electronegative atom so it acquire or obtain some partial negative charge which is represented by delta negative (d-) and other atom acquire some partial positive charge which is represented by delta positive (d+) therefore polar bond is form, which is known as Polar covalent bond.

Example : Hydrogen Chloride Molecule.

In HCl molecule, Chlorine is more electronegative than Hydrogen so chlorine acquires partial negative charge and hydrogen acquire partial positive charge.

Characteristics of Polar Covalent Compounds

i.                   Polar covalent compounds are approximately 80% covalent and 20% ionic so they so characteristics of both covalent and ionic (or electrovalent) compounds.

ii.                 In solution forms, polar covalent compounds are good conductor of electricity. Example: HCl

iii.              As compared to pure non-polar covalent compounds and electrovalent compounds, the melting point and boiling point of polar covalent compound are higher.

Covalent Compounds and Types of Covalent Bonds

Covalent Compounds

                                   Compound which are formed as a result of covalent bonding and containing covalent bonds are known as Covalent Compounds.

Example: Hydrogen, Chlorine, Oxygen, Water, Ethanol etc.

Types of Covalent Bonds

Covalent Bonds are of three types which are as follows-

1.     SingleCovalent Bonds

2.   DoubleCovalent Bonds

3.     TripleCovalent Bonds

Single Covalent Bonds

                                      Bonds which are formed due to sharing of single pair of electrons between two atoms are called single covalent bond. It is represented by single line (-)

Example: Formation of H₂ molecule, Formation of Cl₂ molecule.

i.                   Formation of Hydrogen (H₂) molecule:

                                                         In the outermost shell of hydrogen atom, it have single electron, which it share with another hydrogen atom to acquire inert configuration of helium so single bond is formed between these two hydrogen atoms and this single covalent bond is represented by single line (-)

ii.                 Formation of Chlorine Molecule (Cl₂) :

In the outermost shell of chlorine atom, it have seven electrons, it share its one valence electron with another chlorine atom to form chlorine molecule by single covalent bond.

Double Covalent Bonds

                                      Bonds which are formed due to sharing of double pair of electrons between two atoms are called double covalent bond. It is represented by double line (=)

Example: Formation of O₂ molecule.

i.                   Formation of Oxygen (O₂) molecule:

                                                          In the outermost shell of oxygen atom, it have six electrons, it share its two valence electrons with another oxygen atom to form oxygen molecule by double covalent bond.

Triple Covalent Bonds

                                      Bonds which are formed due to sharing of triple pair of electrons between two atoms are called triple covalent bond. It is represented by triple lines

Example: Formation of N₂ molecule.

i.                   Formation of Nitrogen (N₂) molecule:

                                                          In the outermost shell of nitrogen atom, it have five electrons, it share its three valence electrons with another nitrogen atom to form nitrogen molecule by triple covalent bond.

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Simple Chemical Reaction and General Rule for writing Simple Chemical Reaction

Simple Chemical Reaction

                                         Chemical reaction is represented by chemical equation in brief by taking help of symbol and formula of participating substances in reaction.

General Rule for writing Simple Chemical Reaction

   1.     Reactant are written on left hand side and if more than one reactant are present than write plus (+) sign between them.

   2.     Product are written on left hand side and if more than one product are present than write plus (+) sign between them.

   3.     Arrow sign is placed between reactants and products.

Example: Zn + H₂SO₄ ( Reactants)  -----> ZnSO₄ + H₂ (Products)

 4.     To get more information from the reaction write temperature, pressure, catalyst name above or below arrow sign. 

   5.     On the right side of the gaseous substances sign and on the left side of heavy substances which precipitate sign is placed.

   6.     Reactions which absorb heat are known as endothermic reactions and (+Q) heat sign is added on reactant side.

   7.     Reactions which produce heat are known as exothermic reactions and (+Q) heat sign is added on product side.

    8.     (Aq) is written for aqueous solution substances.
    
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Electrovalent Compound and Characteristics of Electrovalent Compounds

Electrovalent Compound

                             The compounds which contain ionic or electrovalent bonds are known as Electrovalent or Ionic Compounds. Mainly electrovalent compounds are formed due to reaction between highly electropositive and highly electronegative atoms.

Characteristics of Electrovalent Compounds

1.     Crystal Structure:

                              In solid state of electrovalent compounds anions and cations are arranged in regular manner called as crystal, In which anions surrounded by definite number of cations and cations surrounded by definite number of anions.

2.     Physical Nature:

       Ionic or electrovalent compounds are generally hard and their hardness increases with increasing ionic charge and decreasing distance between ions.

3.     Solubility:

Positive ion of ionic compound attach with negative part of polar solvent and negative ion of ionic compound attach with positive part of polar solvent, so ionic or electrovalent compounds are soluble in polar solvents like water and insoluble in non polar solvents like benzene, ether, alcohol.

4.     Melting Point and Boiling Point:

Electrovalent or ionic compounds have high Melting and boiling points because they need large amount of energy to break strong ionic bonds.

5.     Electrical Conductivity:

                                    In molten and solution forms electrovalent compounds conduct electricity because ions flows in molten and solution forms.




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