Polar And Nonpolar Covalent Bonds: Easy Explanation With Examples - Chemistry Basics

The video explains the concept of polarity in covalent bonds using the analogy of polar bears sharing ice cream. It discusses how electronegativity differences between atoms determine whether a bond is polar or non-polar. A polar bond occurs when electrons are shared unequally due to differing electronegativities, while a non-polar bond involves equal sharing. The video also highlights the exception of the carbon-hydrogen bond, which is considered non-polar despite slight electronegativity differences. Examples of chlorine and carbon-oxygen bonds illustrate these concepts.

What is the main factor that determines whether a covalent bond is polar or non-polar?

• The temperature at which the bond forms

• The number of electrons shared

• The difference in electronegativity between the atoms

• The size of the atoms involved

How does electronegativity affect the sharing of electrons in a covalent bond?

• It alters the temperature of the bond

• It changes the size of the atoms

• It affects the strength with which an atom pulls on electrons

• It determines the number of electrons shared

Which of the following is an example of a non-polar covalent bond?

• Chlorine-chlorine bond

• Carbon-oxygen bond

• Oxygen-hydrogen bond

• Carbon-hydrogen bond

Why is the bond between carbon and hydrogen considered non-polar?

• Because they form ionic bonds

• Because the difference in electronegativity is negligible

• Because carbon and hydrogen have identical electronegativities

• Because hydrogen is much larger than carbon

What happens to the electrons in a polar covalent bond between carbon and oxygen?

• They spend more time around oxygen due to its higher electronegativity

• They are shared equally between carbon and oxygen

• They are shared equally between two oxygen atoms

• They are completely transferred to oxygen