The N—F bond is more polar than the N—H bond, but NF 3 has a smaller dipole moment than NH 3 . Explain this curious result. NF 3 μ= 0.2 D NH 3 μ = 1.5 D

Welcome back, everyone explain why of two has a smaller dile moment than H2O when the of bond is more polar than the oh bond. And we're also given the dile moments mu mu of of two is 0.3. Dubai and mu of H2O is 1.8 Dubai which essentially illustrates that the dile moment of water is larger. So let's draw the two structures of two is very similar to oh H two, right? There will be two fluorine atoms bonded to oxygen. Oxygen. According to the octet rule has two single bonds and two lone pairs. And now age 20 on the scan, we can add low pairs to oxygen for flooring. That's not so important. But of course, to be accurate, we can add those long pairs to each flooring. And now let's recall that the electron negativity of fluorine is higher than the electron negativity of oxygen because it's the most electron element in the periodic table. Now, for hydrogen, it's oxygen, that is more electron negative. So if we draw the individual diaper moments for each bond when it comes to water, we have two dile moments pointing towards oxygen and then those two lone pairs are also creating additional dile moments. What about oft we can begin with the long pairs? But now here's what's different since fluorine is more electron than oxygen, the remaining dipole moments will be pointing towards each fluorine. Now, what do we know about vector addition? Well, essentially for water, all of the vectors are additive vertically, right? Because their vertical components are all pointing up. So there will be a large net dipole moment pointing up. Now for fluorine, there are two individual dipole moments that have negative vertical components that are pointing down. So they are actually decreasing. That nut dipole moment slightly long pairs have a higher dipole moment. So we will still have a nut dipole moment pointing up, but it will be smaller because fluorine is partially canceling out the vertical component of each lump pair, right? And that's it. We understand our answer. We can say that the diapers of oft are pointing in the opposite direction of the lom pair dipole. And that's our short explanation. That's it. Thank you for watching.

Table of contents

Skip topic navigation

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Electronegativity

Organic Chemistry

1. A Review of General Chemistry

Electronegativity

Previous problemNext problem

4:10 minutes

Problem 2a

Textbook Question

The N—F bond is more polar than the N—H bond, but NF₃ has a smaller dipole moment than NH₃. Explain this curious result.
NF₃
μ= 0.2 D
NH₃
μ = 1.5 D

Verified step by step guidance

Understand the concept of dipole moment: Dipole moment (μ) is a measure of the separation of positive and negative charges in a molecule. It is a vector quantity, meaning it has both magnitude and direction.

Analyze the polarity of individual bonds: The N—F bond is more polar than the N—H bond because fluorine is more electronegative than hydrogen, leading to a greater difference in electronegativity between N and F compared to N and H.

Consider the molecular geometry: Both NF3 and NH3 have a trigonal pyramidal shape due to the presence of a lone pair on the nitrogen atom. This shape affects how the individual bond dipoles add up to give the overall dipole moment of the molecule.

Evaluate the direction of bond dipoles: In NH3, the N—H bond dipoles are directed towards the nitrogen, and the lone pair also contributes to the dipole moment in the same direction, resulting in a larger overall dipole moment.

Assess the effect of lone pairs and bond dipoles in NF3: In NF3, the N—F bond dipoles are directed towards the fluorine atoms, but the lone pair on nitrogen has a dipole moment in the opposite direction, partially canceling out the bond dipoles, leading to a smaller overall dipole moment.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above

Video duration:

Play a video:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Bond Polarity

Bond polarity refers to the distribution of electrical charge between atoms in a molecule. A bond is polar when there is a significant difference in electronegativity between the bonded atoms, causing a dipole moment. In NF3, the N—F bond is more polar than the N—H bond due to fluorine's higher electronegativity compared to hydrogen.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms within a molecule, influencing its dipole moment. NF3 and NH3 both have a trigonal pyramidal shape, but the orientation of the dipoles in NF3 leads to partial cancellation, resulting in a smaller overall dipole moment compared to NH3, where dipoles add constructively.

Dipole Moment

Dipole moment is a measure of the separation of positive and negative charges in a molecule, indicating its polarity. It depends on both the individual bond polarities and the molecular geometry. Despite NF3 having more polar bonds, its dipole moment is smaller than NH3 due to the vector sum of the bond dipoles being less effective in NF3.

Watch next

Master Differences between ionic, polar and covalent bonds with a bite sized video explanation from Johnny

Start learning

Related Videos

Related Practice

Textbook Question

The C=O double bond has a dipole moment of about 2.4 D and a bond length of about 1.23 Å.

a. Calculate the amount of charge separation in this bond.

Textbook Question

1. From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.

2. In each case, predict whether the dipole moment is relatively large (electronegativity difference >0.5) or small.

a. C—Cl

b. C—H

c. C—Li

d. C—N

e. C—O

Textbook Question

For each alkene, indicate the direction of the dipole moment. For each pair, determine which compound has the larger dipole moment

b. cis-1,2-dibromoethene or trans-2,3-dibromobut-2-ene

Textbook Question

For each alkene, indicate the direction of the dipole moment. For each pair, determine which compound has the larger dipole moment.

c. cis-1,2-dibromo-1,2-dichloroethene or cis-1,2-dichloroethene

Textbook Question

For each of the following compounds,

1. draw the Lewis structure.

2. show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. estimate whether the compound will have a large, small, or zero dipole moment.

Textbook Question

For each of the following compounds,

1. draw the Lewis structure.

2. show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. estimate whether the compound will have a large, small, or zero dipole moment.

Textbook Question

The electrostatic potential maps for ammonia and water are shown here. The structure of ammonia is shown within its EPM. Note how the lone pair creates a region of high electron potential (red), and the hydrogens are in regions of low electron potential (blue). Show how your three-dimensional structure of water corresponds with its EPM.

Textbook Question

Why are Na⁺ and K⁺ unable to form covalent bonds?

Show more practices

Download the Mobile app

Privacy

Do not sell my personal information

Accessibility

Patent notice

Sitemap

The N—F bond is more polar than the N—H bond, but NF3 has a smaller dipole moment than NH3. Explain this curious result.NF3μ= 0.2 DNH3μ = 1.5 D

Key Concepts

Bond Polarity

Molecular Geometry

Dipole Moment

Watch next

The N—F bond is more polar than the N—H bond, but NF₃ has a smaller dipole moment than NH₃. Explain this curious result.
NF₃
μ= 0.2 D
NH₃
μ = 1.5 D