(a) Does CS 2 have a dipole moment? If so, in which direction does the net dipole point? (b) Does SO 2 have a dipole moment? If so, in which direction does the net dipole point?

Welcome back everyone. We need to identify if dia chloral, di floor, methane has a dipole moment. So we're going to begin by noting down the electro negativity values for the atoms that make up this compound. Beginning with carbon recall that from our textbooks. Carbon has an electro negativity of 2.5. And for the election negativity of chlorine recall that in our textbooks it's a value of 3.0 and then for flooring we have an electro negativity of 4.0 recall that flooring is the most electro negative element on the periodic table. We next want to consider the election negativity difference between our bonds making up our molecule. So we have carbon chlorine bonds versus our election. Sorry, electro negativity difference between our carbon fluorine bonds making up the molecule. And we want to recall that whenever we have an electro negativity difference represented as Delta E. In that is greater than a value of .5. Then that means that our molecule is a polar molecule. And so looking at our bond between carbon chlorine, we're going to take the difference where for chlorine we have the higher value being 3.0 minus carbons. Election negativity value of 2.5. This difference gives us an election negativity difference of 0.5 for the carbon chlorine bond and recognize that because chlorine is more election negative than carbon with its higher election negativity value as you know as we stated for chlorine will have a die pool towards the chlorine atoms in our molecule represented by the plus sign towards the carbon here and the end of our arrow pointing towards our more negative atom being chlorine. Then we have our election negativity difference between our carbon fluorine bond. So beginning with Florence election negativity being 4.0 we would take the difference between carbon of 2.5 and this difference gives us a value of 1.5. And so we would see that we have a higher election negativity difference than sorry, in our carbon fluorine bond than in our carbon chlorine bond. And here yet again we have a die pool towards the more election negativity adam being flooring. So we would say that our carbon chlorine bond is less electro negative than our carbon fluorine bond. And because the election activity difference between carbon flooring is 1.5 we therefore have a higher di pole for our carbon flooring bonds in the molecule. And because we have a higher di pole for these bonds, we would say therefore yes, there is a net dipole, sorry, a net dipole moment in our day chloral, floral, methane molecule. And so this would be our final answer to complete this example corresponding to choice a as the correct choice. So I hope this made sense. And let us know if you have any questions

Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 37a,b

Chapter 9, Problem 37a,b

(a) Does CS₂ have a dipole moment? If so, in which direction does the net dipole point? (b) Does SO₂ have a dipole moment? If so, in which direction does the net dipole point?

Verified step by step guidance

Identify the molecular geometry of CS_2. CS_2 is a linear molecule because it consists of a central carbon atom double-bonded to two sulfur atoms.

Consider the electronegativity of the atoms involved. Carbon (C) has an electronegativity of 2.55, while sulfur (S) has an electronegativity of 2.58.

Determine the direction of the bond dipoles. Since the electronegativity difference between carbon and sulfur is very small, the C-S bonds are nearly nonpolar.

Analyze the symmetry of the molecule. In a linear molecule like CS_2, any small dipole moments in the C-S bonds will cancel each other out due to the molecule's symmetry.

Conclude whether there is a net dipole moment. Since the bond dipoles cancel out, CS_2 does not have a net dipole moment.

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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 positions of its atoms and the presence of lone pairs of electrons, which can affect bond angles and overall symmetry. Understanding the geometry of CS2 (carbon disulfide) is crucial for determining its polarity and dipole moment.

Polarity and Dipole Moment

Polarity in molecules arises from differences in electronegativity between bonded atoms, leading to uneven distribution of electron density. A dipole moment is a vector quantity that represents the separation of positive and negative charges in a molecule. If a molecule has a net dipole moment, it indicates that it is polar, which is essential for understanding the behavior of CS2 in different environments.

Symmetry and Nonpolar Molecules

Symmetry plays a critical role in determining whether a molecule is polar or nonpolar. A molecule can have polar bonds but still be nonpolar overall if its shape is symmetrical, allowing the dipole moments to cancel each other out. In the case of CS2, its linear geometry results in a symmetrical distribution of charge, leading to the conclusion that it does not have a net dipole moment.