Chapter 21: Problem 3

For \(\mathrm{HF}\), why is \(\delta_{\mathrm{F}}=-\delta_{\mathrm{H}}\) ?

Short Answer

Expert verified

In a dipole moment, charges in the bond are distributed according to the electronegativity of the atoms. The arrow of the dipole moment points from the positively charged atom (with lower electronegativity, Hydrogen here) towards the negatively charged atom (with higher electronegativity, Fluorine here). Hence, Fluorine has negative 'delta' and Hydrogen has positive 'delta', so \(\delta_{F} = -\delta_{H}\).

Step by step solution

Understand the concept of dipole moment

In a molecule, the dipole moment measures the charge separation in a system of charges which is equivalent to a dipole. It is given by the product of a charge (which is partial when the bond is covalent) and the distance between the charges. In a diatomic molecule, the dipole moment is directed from the less electronegative atom to the more electronegative one.

Study the Fluorine-Hydrogen bond

In a Fluorine-Hydrogen bond, Fluorine is more electronegative than Hydrogen which means it will more strongly attract the bonding electron pair. Therefore, Fluorine will have a partial negative charge and Hydrogen will have a partial positive charge. The dipole moment will point from Hydrogen to Fluorine.

Define 'delta'

In this context, 'delta' refers to the partial charge on the atoms in a polar covalent bond. Its value depends on the electronegativity difference between the two atoms. 'delta' is positive for the less electronegative atom (Hydrogen) and negative for the more electronegative atom (Fluorine). This is why \(\delta_{F} = -\delta_{H}\).

Unlock Step-by-Step Solutions & Ace Your Exams!

Full Textbook Solutions
Get detailed explanations and key concepts
Unlimited Al creation
Al flashcards, explanations, exams and more...
Ads-free access
To over 500 millions flashcards
Money-back guarantee
We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

For \(\mathrm{HF}\), why is \(\delta_{\mathrm{F}}=-\delta_{\mathrm{H}}\) ?

Short Answer

Step by step solution

Understand the concept of dipole moment

Study the Fluorine-Hydrogen bond

Define 'delta'

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Nuclear Chemistry

Organic Chemistry

Inorganic Chemistry

Chemical Reactions

Chemistry Branches

Study anywhere. Anytime. Across all devices.