Use the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (Electronegativity of CrCr is 1.6) Electronegativity Difference (ΔENΔEN) Bond Type Example zero (0−0.40−0.4) pure covalent Cl2Cl2 intermediate (0.4−2.00.4−2.0) polar covalent HFHF large (2.0+2.0+) ionic NaClNaCl Find the electronegativity difference between Br and Br. Express your answer using two significant
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
Use the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (Electronegativity of CrCr is 1.6)
| Electronegativity Difference (ΔENΔEN) | Bond Type | Example |
| zero (0−0.40−0.4) | pure covalent | Cl2Cl2 |
| intermediate (0.4−2.00.4−2.0) | polar covalent | HFHF |
| large (2.0+2.0+) | ionic | NaClNaCl |
Molecules that formed by the transfer of electrons from one another are called ionic bond.
Molecules that are formed by sharing of electrons are called covalent bond.
Covalent bond are further classified as polar covalent and non-polar covalent bonds.
Polar covalent bonds are formed between the atoms of different electronegativity.
Non-polar covalent bonds are formed between the atoms of same electronegativity.
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