Ch.6 Ionic and Molecular Compounds

Timberlake - Chemistry: An Introduction to General, Organic, and Biological Chemistry 13th Edition

Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353Not the one you use?Change textbook

Timberlake 13th Edition

Ch.6 Ionic and Molecular Compounds

Problem 69a

Chapter 6, Problem 69a

For each of the following bonds, indicate the positive end with 𝛿⁺ and the negative end with 𝛿⁻ . Draw an arrow to show the dipole for each.
a. N and F

Verified step by step guidance

Step 1: Understand the concept of electronegativity. Electronegativity is the ability of an atom to attract shared electrons in a chemical bond. The greater the difference in electronegativity between two atoms, the more polar the bond will be.

Step 2: Look up the electronegativity values of nitrogen (N) and fluorine (F). Fluorine has an electronegativity of approximately 3.98, while nitrogen has an electronegativity of approximately 3.04.

Step 3: Determine the direction of the dipole. Since fluorine has a higher electronegativity than nitrogen, it will attract the shared electrons more strongly, making fluorine the negative end (𝛿⁻) and nitrogen the positive end (𝛿⁺).

Step 4: Represent the dipole with an arrow. Draw an arrow pointing from the less electronegative atom (N) to the more electronegative atom (F). Place a small plus sign (+) at the tail of the arrow near nitrogen to indicate the positive end.

Step 5: Label the bond. Clearly mark the nitrogen atom with 𝛿⁺ and the fluorine atom with 𝛿⁻ to indicate the partial charges due to the unequal sharing of electrons.

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Key Concepts

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

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. In the context of the bond between nitrogen (N) and fluorine (F), fluorine is more electronegative than nitrogen, meaning it pulls the shared electrons closer to itself, creating a dipole moment.

Dipole Moment

A dipole moment occurs in a polar bond where there is an uneven distribution of electron density. It is represented by an arrow pointing from the positive end (𝛿⁺) to the negative end (𝛿⁻) of the bond. In the N-F bond, the dipole moment indicates that the electrons are more concentrated around fluorine, making it the negative end.

Polar vs. Nonpolar Bonds

Bonds can be classified as polar or nonpolar based on the difference in electronegativity between the two atoms involved. A polar bond, like that between N and F, has a significant difference in electronegativity, resulting in a dipole moment. In contrast, nonpolar bonds occur between atoms with similar electronegativities, leading to an even distribution of electron density.

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Complete each of the following statements for a molecule of H₂S:

c. The number of atoms attached to the central S atom is _______.

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Compare the Lewis structures of CF₄ and NF₃ Why do these molecules have different shapes?

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Textbook Question

Which electronegativity difference (a, b, or c) would you expect for a nonpolar covalent bond?

a. from 0.0 to 0.4

b. from 0.5 to 1.8

c. from 1.9 to 3.3

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d. ClNO₂ (N is the central atom)

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Choose the shape (1 to 6) that matches each of the following descriptions (a to c):

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2. bent (109°)

3. trigonal planar

4. bent (120°)

5. trigonal pyramidal

6. tetrahedral

b. a molecule with a central atom that has four electron groups and three bonded atoms

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Textbook Question

Write the formula for the polyatomic ion and name each of the following compounds:

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For each of the following bonds, indicate the positive end with 𝛿⁺ and the negative end with 𝛿⁻ . Draw an arrow to show the dipole for each.a. N and F

Verified video answer for a similar problem:

Key Concepts

Electronegativity

Dipole Moment

Polar vs. Nonpolar Bonds

For each of the following bonds, indicate the positive end with 𝛿⁺ and the negative end with 𝛿⁻ . Draw an arrow to show the dipole for each.
a. N and F