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The range of electronegativity for polar nonpolar and ionic bonding will be between 1.5 and 2.1
Electronegativity is a chemical property that describes the tendency of an atom or a functional group to attract electrons toward itself.
The range of electronegativity for polar nonpolar and ionic bonding . So, the difference in electronegativity is somewhere between 1.5 and 2.1, between a polar covalent bond and an ionic bond.
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The range of electronegativity for polar nonpolar and ionic bonding is less than 0.4 and greater that 0.4, respectively.
In general there are two major categories of bonds, which are polar molecules and nonpolar molecules.
In the field of chemistry, polarity can be described as the distribution of electric charge around atoms, chemical groups, or molecules.
- When there is an electronegativity difference between the bonded atoms then polar molecules are formed. Water - [tex]H_{2}[/tex]O, Ammonia - N[tex]H_{3}[/tex] are some of the examples of polar molecules.
- And when electrons are shared equal between atoms of a diatomic molecule or when polar bonds in a larger molecule cancel out each other then non polar molecules are formed. Any of the noble gasses: He, Ne, Ar, Kr, Xe, Benzene, methane etc are some of the examples of the molecules which forms non polar bond
- And if we talk about ionic bond, which are also be called as electrovalent bond, type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound. These types of bond forms when the outermost electrons of one atom are transferred permanently to another atom.
There is no hard and fast rule but in general, a bond is considered as non polar if the difference in electronegativities is less than about 0.4, and it will be called a polar bond molecule if the difference is greater than 0.4.
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