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Questions and Answers
In nonpolar covalent bonds, atoms share electrons equally due to similar electronegativities.
True
Polar covalent bonds occur when electrons are shared unequally between atoms.
True
Nonpolar covalent compounds result in charge separation due to uneven distribution of shared electrons.
False
Polar covalent bonds favor one side over another in terms of electrical attraction.
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Hydrogen sulfide (H2S) is an example of a nonpolar covalent compound.
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Methane (CH4) is an example of a nonpolar covalent compound.
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Study Notes
Covalent bonding is one of the main types of chemical bonds found between atoms. It occurs when nonmetallic elements share electrons with each other, creating a shared electron pair. This sharing can take two forms: either both atoms contribute equally to the bond (nonpolar), or they do so unequally, creating what's known as a polar covalent bond. Let's explore these different types further.
Nonpolar Covalent Bonds
When atoms have similar electronegativities—their ability to attract shared electrons—they form symmetrical bonds where the shared electrons are evenly distributed around the molecule. As a result, there isn't any charge separation, leading to nonpolar bonds. In essence, this means the force holding the atoms together doesn't favor one side over another in terms of electrical attraction. Some examples of nonpolar covalent compounds include hydrogen sulfide (H2S) and methane (CH4).
Polar Covalent Bonds
In contrast, some pairs of atoms don't share their electrons equally because they differ in their electronegativity. When this happens, the shared electrons tend to be more attracted by the atom with the higher electronegativity, resulting in a partial transfer of electrons from the less electronegative atom to the more electronegative atom. This leads to a shift in the distribution of electrons within the molecule, causing the formation of a dipole moment, with one end of the bond having slightly more positive charges and the other end having slightly more negative charges. These differences create polarity. Examples of polar covalent compounds include water (H2O), ammonia (NH3), and alcohols like ethanol (C2H5OH).
Understanding the difference between polar and nonpolar covalent bonds helps chemists understand how atoms interact with each other and predict properties such as boiling points, solubility, and reactivity.
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Description
Test your knowledge on nonpolar and polar covalent bonds, where nonmetallic elements share electrons to form shared electron pairs. Explore how symmetrical bonds with equal electron distribution create nonpolar compounds, while asymmetrical bonds with partial electron transfer lead to polarity in molecules like water and ethanol.
