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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 49
Chapter 10, Problem 49

Determine whether each molecule in Exercise 35 is polar or nonpolar. a. PF3 b. SBr2 c. CHCl3 d. CS2

Verified step by step guidance
1
Determine the molecular geometry of each molecule using VSEPR theory.
Identify the electronegativity of each atom in the molecules to assess the polarity of each bond.
For each molecule, evaluate the symmetry of the molecular geometry to determine if the dipole moments cancel out.
Consider the presence of lone pairs on the central atom, as they can affect the overall polarity of the molecule.
Conclude whether each molecule is polar or nonpolar based on the molecular geometry and bond polarity.

Key Concepts

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

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The shape of a molecule is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the distribution of charge. Understanding molecular geometry is crucial for predicting whether a molecule is polar or nonpolar.
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Molecular Geometry with Two Electron Groups

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. Differences in electronegativity between bonded atoms can lead to polar covalent bonds, where electrons are shared unequally. This concept is essential for determining the polarity of a molecule, as polar bonds contribute to an overall dipole moment.
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Electronegativity Trends

Dipole Moment

A dipole moment is a vector quantity that represents the separation of positive and negative charges in a molecule. It arises when there is an uneven distribution of electron density due to differences in electronegativity. Molecules with a net dipole moment are considered polar, while those with symmetrical charge distribution are nonpolar, making this concept key in assessing molecular polarity.
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Related Practice
Textbook Question

Determine whether each molecule is polar or nonpolar. a. SiCl4 b. CF2Cl2 c. SeF6 d. IF5

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Textbook Question

Determine the geometry about each interior atom in each molecule and sketch the molecule. (Skeletal structure is indicated in parentheses.) c. NH2CO2H (H2NCOOH both O atoms attached to C)

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Textbook Question

Determine the geometry about each interior atom in each molecule and sketch the molecule. (Skeletal structure is indicated in parentheses.)

a. CH3NH2 (H3CNH2)

b. CH3CO2CH3 (H3CCOOCH3 One O atom attached to 2nd C atom; the other O atom is bonded to the 2nd and 3rd C atom)

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Textbook Question

Determine whether each molecule is polar or nonpolar. a. SCl2 b. SCl4

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Textbook Question

Determine whether each molecule in Exercise 36 is polar or nonpolar. a. CF4 b. NF3 c. OF2 d. H2S

1825
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Textbook Question

CH3F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules. Explain.

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