Taking into account the definition of electronegativity and polar covalent, the range of the electronegativity difference is 0.5 to 1.6.
Electronegativity is defined as the ability of an element to attract electrons that bind it to another element.
The bond dipole moment can then be defined as the magnitude of the polarity in a bond. This moment represents the distribution of electron density in a bond.
The distribution of charges is due to the fact that the atoms that form them have different electronegativity.
Then the polar bonds are established between atoms of different electronegativity. In a polar molecule there is separation between positive and negative charges. The bonds will be the more polar the greater the electronegativity difference between the bonded atoms. In a polar covalent bond the range of the electronegativity difference is 0.5 to 1.6.
On the other hand, the nonpolar covalent bond occurs between atoms of the same element or between atoms with very little difference in electronegativity. Thus, molecules or bonds that do not exhibit any polarity are characterized.
Finally, the range of the electronegativity difference is 0.5 to 1.6.
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Answer: (im guessing this is for Bonding of Atoms in Reactions Quick Check so here is the rest of the answers~if not please ignore)
1. Approximately in which range of electronegativity differences would polar covalent bonds occur?
0.5 to 1.7
2. This image shows the electronegativities of elements on the periodic table. Based on this information, which element is most likely to form a strong ionic bond and take on electrons?
fluorine (f)
3. Which option contains an example of a polyatomic ion?
KN03
4. Which statement best explains the difference between polar and nonpolar covalent bonds?
Polar covalent bonds share electrons unequally, while nonpolar covalent bonds share electrons equally.
5. Which statement describes the bonds in iron sulfate, FeSO4?
Fe and S have an ionic bond, while S and O have covalent bonds
100% correct!
