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Draw a Lewis structure for each molecule and determine its molecular geometry. What kind

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 97P Chapter 12

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 97P

PROBLEM 97P

Draw a Lewis structure for each molecule and determine its molecular geometry. What kind of intermolecular forces are present in each substance?

(a) H2Se

(b) SO2

(c) CHCl3

(d) CO2

Step-by-Step Solution:
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Solution 97P

(a)Lewis structure of H2Se:angular geometry

Hydrogen selenide is an inorganic compound with the formula H₂Se. This hydrogen chalcogenide is the simplest and most commonly encountered hydride of selenium. H₂Se is a colorless, flammable gas under standard conditions.

Image result for h2se

 It is a selenium atom with two bonds to hydrogen atoms and two lone pairs. There is a definite polar bond here: Selenium is more electronegative than hydrogen so electrons will tend to go towards the selenium atom, causing a dipole. However, it is not polar enough to be considered a hydrogen bond. The answer is that dipole-dipole causes most of the intermolecular forces (although london dispersion forces always exist. It's just in this case they are insignificant compared to dipole-dipole).

(b)Lewis structure of SO2 :angular geometry

Sulfur dioxide is the chemical compound with the formula SO 2. At standard atmosphere, it is a toxic gas with a pungent, irritating smell. The triple point is 197.69 K and 1.67 kPa. It is released naturally by volcanic activity

Image result for so2

Dipole-dipole forces occur when polar molecules are attracted to one another due the attraction of opposite charges. Polar molecules have partial negative charge on the more electronegative atom and partial positive charge on the less electronegative atom because the more electronegative one pulls electrons from the other. The partial charges on adjacent molecules is the dipole-dipole force.

In this case, sulfur dioxide is polar because oxygen is more electronegative than sulfur. However, way more important than this is the fact that there is a partial negative charge on both oxygen atoms (see the diagram) and a partial positive charge on sulfur (see diagram), making this an extremely polar molecule.

(c)lewis structure of CHCl3:tetrahedral geometry

Chloroform, or trichloromethane, is an organic compound with formula CHCl₃. It is a colorless, sweet-smelling, dense liquid that is produced on a large scale as a precursor to PTFE. It is also a precursor to various refrigerants.

Image result for chcl3

 chloroform is a polar molecule because of the electronegative Cl's. The H is not electronegative enough to counter the electromagnetic pull of the Cl, therefore there is a dipole moment towards the Cl's. As for hydrogen bonding, the H atom can "bond" with another Cl from a different

Chloroform and then that H on the other Chloroform can bond to another Cl. So this keeps on going.

It falls under both dipole and hydrogen bonding categories.

Trichloromethane CHCL3 has a tetrahedral structure with bond angles 104.5 as the molecule is unsymmetrical its polar due to the C-CL bond where the electrons are pulled closer to the electronegative Cl atom in the covalent bond, the intermolecular attractions that exist between these molecules is permanent dipole- permanent dipole attraction as there is a permanent difference in charge density between the C-Cl bond.

(d)lewis structure of CO2:linear geometry

Carbon dioxide is a colorless and odorless gas that is vital to life on Earth. This naturally occurring chemical compound is made up of a carbon atom covalently double bonded to two oxygen atoms.

Structural formula of carbon dioxide with bond lengthImage result for co2 lewis structure

CO has two C-O bonds. The dipoles point in opposite directions, so they cancel each other out. Thus, although CO₂ has polar bonds, it is a nonpolar molecule. Therefore, the only intermolecular forces are London dispersion forces.

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Chapter 12, Problem 97P is Solved
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Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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Draw a Lewis structure for each molecule and determine its molecular geometry. What kind