Understanding Polar Covalent Bonds

This video tutorial explains polar covalent bonds, focusing on the uneven sharing of electrons between atoms. It introduces the concept of electronegativity, developed by Linus Pauling, and how it determines the type of bond formed. The video covers how to calculate the difference in electronegativity (Delta E) to classify bonds as non-polar, polar, or ionic. It also discusses dipole moments and partial charges in polar bonds, using HCl as an example. Finally, it explains how molecular symmetry can result in non-polar molecules despite having polar bonds, illustrated with carbon tetrafluoride.

What is the main idea behind polar covalent bonds?

• No sharing of electrons

• Complete transfer of electrons

• Uneven sharing of electrons

• Even sharing of electrons

What does electronegativity measure?

• The number of protons in an atom

• The ability of an atom to attract electrons

• The size of an atom

• The mass of an atom

Who developed the scale of electronegativity?

• Albert Einstein

• Linus Pauling

• Marie Curie

• Isaac Newton

What is the Delta E value for a non-polar bond?

• 0 to 0.4

• 0.5 to 1.8

• 1.9 to 2.5

• Greater than 2.5

What type of bond is formed when Delta E is greater than 1.8?

• Non-polar covalent bond

• Polar covalent bond

• Ionic bond

• Metallic bond

What does a dipole moment indicate in a polar bond?

• Complete transfer of electrons

• No sharing of electrons

• Unequal sharing of electrons

• Equal sharing of electrons

In a polar bond, which element does the dipole moment arrow point towards?

• The element with less protons

• The less electronegative element

• The element with more protons

• The more electronegative element

What charge does the more electronegative element in a polar bond acquire?

• Completely positive

• Neutral

• Partially negative

• Partially positive

What determines if a molecule with polar bonds is non-polar?

• The number of bonds

• The size of the molecule

• The symmetry of the molecule

• The mass of the molecule

Why is carbon tetrafluoride considered a non-polar molecule?

• It is asymmetrical

• It is symmetrical

• It has an ionic bond

• It has no polar bonds