/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 189 Which one of the following pairs... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 13: Problem 189

Which one of the following pairs of molecules will have permanent dipole moments for both members? [2003] (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{NO}_{2}\) (b) \(\mathrm{NO}_{2}\) and \(\mathrm{CO}_{2}\) (c) \(\mathrm{NO}_{2}\) and \(\mathrm{O}_{3}\) (d) \(\mathrm{SiF}_{4}\) and \(\mathrm{CO}_{2}\)

Short Answer

Expert verified
Option (c) NO鈧� and O鈧� both have permanent dipole moments.

Step by step solution

01

Understanding Dipole Moments

A permanent dipole moment occurs in a molecule when there is an uneven distribution of electron density. This often happens when there are polar bonds and the molecular shape does not allow for these dipoles to cancel out.
02

Analyzing Molecular Structures

We need to determine the geometry and electron distribution in the given molecules: 1. **SiF鈧� (silicon tetrafluoride)**: It has a tetrahedral shape and is symmetrical, leading to the cancellation of dipole moments. 2. **NO鈧� (nitrogen dioxide)**: It is a bent molecule, causing the polar bonds to create a net dipole moment. 3. **CO鈧� (carbon dioxide)**: Although it has polar bonds, it is linear, leading to dipole cancellation. 4. **O鈧� (ozone)**: It has a bent shape, resulting in a net dipole moment.
03

Identifying Pairs with Permanent Dipoles

By applying the previous analysis: - - (a) SiF鈧� has no dipole, but NO鈧� does. - (b) CO鈧� has no dipole, but NO鈧� does. - (c) NO鈧� and O鈧� both have a bent geometry and possess permanent dipole moments. - (d) Both SiF鈧� and CO鈧� have balanced structures with no net dipole moments.
04

Conclusion on Pairs with Permanent Dipoles

The only pair which has permanent dipole moments in both molecules is option (c): NO鈧� and O鈧�.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molecular Geometry
Molecular geometry refers to the 3D arrangement of atoms within a molecule. It is a critical factor in determining various physical and chemical properties, such as polarity and dipole moments. The geometry of a molecule depends on the number of electron pairs (bonding and non-bonding) around the central atom. For instance:
  • Tetrahedral Geometry: Seen in structures like \(\text{SiF}_4\), with bond angles of approximately 109.5掳, leading to symmetrical electron distribution.
  • Bent Geometry: Exhibited by molecules like \(\text{NO}_2\) and \(\text{O}_3\), usually causing an angle less than 120掳, resulting in uneven charge distribution.
  • Linear Geometry: Present in \(\text{CO}_2\), with a bond angle of 180掳, often causing dipole cancellation due to symmetry.
The spatial arrangement of atoms is influenced by the types of bonds and the presence of lone pairs, which repel each other and shape the molecule accordingly.
Polarity
Polarity in molecules arises from the separation of charge across the molecule, due to differences in electronegativity between bonded atoms. A molecule is polar if it has a net dipole moment, resulting from an uneven electron distribution. Factors contributing to polarity include:
  • Electronegativity Difference: Atoms with larger differences in electronegativity form polar bonds, as electrons are drawn more towards one atom.
  • Molecular Geometry: Even if a molecule contains polar bonds, its geometry can offset them. For example, despite polar bonds, \(\text{SiF}_4\) is nonpolar because its symmetrical tetrahedral shape causes dipole cancellation.
  • Presence of Lone Pairs: Leads to bent shapes, as with \(\text{NO}_2\) and \(\text{O}_3\), often resulting in a net dipole moment.
Understanding polarity is crucial because it affects solubility, boiling points, and interaction with other molecules.
Electron Distribution
Electron distribution refers to how electrons are allocated within a molecule, influencing its chemical properties. Electron clouds are distributed around atomic nuclei, creating areas of partial positive or negative charge. This distribution is critical for predicting:
  • Reactivity: Molecules with unequal electron distribution are often more reactive, as they can attract or repel electrons from other reactants.
  • Dipole Moments: The unequal electron distribution in polar bonds like \(\text{NO}_2\) contributes to a dipole moment, where one part of the molecule is more negatively charged.
  • Bond Polarity: Described as the difference in electron density between bonded atoms, influencing the strength and type of bonds.
The way electrons are distributed within a molecule not only affects molecular shape but also dictates how a molecule interacts with others through intermolecular forces.
Chemical Bonding
Chemical bonding involves the interactions that hold atoms together in a molecule, formed through shared or transferred electrons. The main types of chemical bonds are:
  • Covalent Bonds: Atoms share electron pairs, creating a stable balance of attractive and repulsive forces. For example, in \(\text{O}_3\), the atoms are connected by polar covalent bonds.
  • Ionic Bonds: Involves the transfer of electrons from one atom to another, leading to the formation of ions with opposite charges and a resultant electrostatic attraction.
  • Metallic Bonds: Where electrons are delocalized across a lattice of metal atoms, providing a sea of electrons that accounts for conductivity.
Chemical bonds determine the molecule's stability and are essential for understanding the molecule's physical properties and behavior during chemical reactions.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which one of the following compounds has the smallest bond angle in its molecule? \(\quad\) [2003] (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{H}_{2} \mathrm{~S}\) (d) \(\mathrm{NH}_{3}\)

In which of the following pairs of molecules/ions, both the species are not likely to exist? (a) \(\mathrm{H}_{2}^{2+}, \mathrm{He}_{2}\) (b) \(\mathrm{H}_{2}, \mathrm{H}_{2}^{2+}\) (c) \(\mathrm{H}_{2}^{+}, \mathrm{He}_{2}^{2-}\) (d) \(\mathrm{H}_{2}^{-}, \mathrm{He}_{2}^{2-}\)

In which of the following molecules/ions all the bonds are unequal? [2006] (a) \(\mathrm{SF}_{4}\) (b) \(\mathrm{SiF}_{4}\) (c) \(\mathrm{XeF}_{4}\) (d) \(\mathrm{BF}_{4}-\)

The speces in which the atom is in a state of sphybridization is? (a) \(\mathrm{NO}_{2}^{-}\) (b) \(\mathrm{NO}_{3}^{-}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{NO}_{2}^{+}\)

In \(\mathrm{NO}_{3}^{-}\)ion, number of bond pair and lone pair of electron on nitrogen atom are? (a) 2,2 (b) 3,1 (c) 1,3 (d) 4,0
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.