(b) What would you expect for the magnitude and direction of the bond dipoles in this series?

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insert step 1: Identify the series of molecules or bonds in question.

insert step 2: Determine the electronegativity of each atom involved in the bonds.

insert step 3: Compare the electronegativity values to predict the direction of the bond dipoles, which points from the less electronegative atom to the more electronegative atom.

insert step 4: Assess the difference in electronegativity to estimate the magnitude of the bond dipoles; a larger difference indicates a stronger dipole.

insert step 5: Consider the molecular geometry to understand how individual bond dipoles contribute to the overall molecular dipole moment.

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Key Concepts

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

Bond Dipole

A bond dipole is a measure of the polarity of a chemical bond between two atoms. It arises due to the difference in electronegativity between the bonded atoms, resulting in an uneven distribution of electron density. The dipole is represented as a vector pointing from the less electronegative atom to the more electronegative atom, indicating the direction of the partial positive and negative charges.

Electronegativity

Electronegativity is the ability of an atom to attract electrons in a chemical bond. It is a key factor in determining the polarity of a bond; atoms with higher electronegativity will pull electron density closer to themselves. The difference in electronegativity between two bonded atoms helps predict the bond's dipole moment, with larger differences leading to stronger dipoles.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The shape of a molecule influences how bond dipoles interact and combine, affecting the overall molecular dipole moment. Understanding the geometry is crucial for predicting the direction and magnitude of bond dipoles, as symmetrical arrangements can lead to cancellation of dipoles, while asymmetrical shapes can result in a net dipole.

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Textbook Question

Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle. (a)

(b)

(c)

Textbook Question

(a) Which geometry and central atom hybridization would you expect in the series BH₄^-, CH₄, NH₄⁺?

Textbook Question

(a) Draw a picture showing how two p orbitals on two different atoms can be combined to make a σ bond. (b) Sketch a π bond that is constructed from p orbitals.

Textbook Question

(d) Can two s orbitals combine to form a p bond? Explain.