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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins - Organic Chemistry: A Learner Centered Approach 1st Edition
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Not the one you use?Change textbook
All textbooksMullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 36a
Chapter 1, Problem 36a

For the molecules shown, indicate the direction of the dipole moment.
(a)

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1
Identify the polar bonds in the molecule by determining the electronegativity difference between the atoms in each bond. A bond is polar if the electronegativity difference is significant (generally greater than 0.4).
Determine the direction of each bond dipole moment. The dipole moment points from the less electronegative atom to the more electronegative atom. Use the periodic table to compare electronegativities.
Consider the molecular geometry to assess how the individual bond dipoles combine. If the molecule is symmetrical, the dipole moments may cancel out, resulting in no net dipole moment. If the molecule is asymmetrical, the dipole moments may add up to create a net dipole moment.
Draw the molecule's structure and use arrows to represent the direction of each bond dipole moment. The arrow should point toward the more electronegative atom, with a small cross at the tail to indicate the positive end.
Combine the bond dipoles vectorially to determine the overall direction of the molecular dipole moment. If the molecule has a net dipole moment, indicate its direction with a larger arrow pointing from the positive to the negative end of the molecule.

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Key Concepts

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

Dipole Moment

The dipole moment is a vector quantity that represents the separation of positive and negative charges in a molecule. It is calculated as the product of the charge and the distance between the charges. A molecule with a dipole moment has a positive end and a negative end, indicating the direction in which the electron density is unevenly distributed.
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Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons within a chemical bond. Atoms with higher electronegativity will pull electron density towards themselves, creating partial negative charges, while less electronegative atoms will have partial positive charges. Understanding electronegativity is crucial for predicting the direction of the dipole moment in a molecule.
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Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. The shape of a molecule influences how dipole moments add up; in symmetrical molecules, dipole moments may cancel out, resulting in a nonpolar molecule, while in asymmetrical molecules, they can reinforce each other, leading to a polar molecule. Analyzing molecular geometry is essential for determining the overall dipole moment direction.
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Related Practice
Textbook Question

Use hybrid orbitals to draw the following molecules.

(a)

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Textbook Question

For the molecules shown, indicate the direction of the dipole moment.

(b)

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Textbook Question

Hydrogen forms bonds without hybridizing. Why?

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Textbook Question

Calculate the formal charge on the non-hydrogen atoms in the molecules shown. Use the arrow-pushing formalism to 'move' an electron pair such that it is shared between two (formerly) charged atoms. Your arrow should account for the formation of the molecule on the right from the molecule on the left.

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Textbook Question

You drew the Lewis structures of the following compounds and ion in Assessment 2.32. Predict their shapes around the central atom based on the Lewis structure.

(d) CO32-

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Textbook Question

You drew the Lewis structures of the following compounds and ion in Assessment 2.32. Predict their shapes around the central atom based on the Lewis structure.

(c) HCO2H

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