/*! 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 131 Which of the following are non-p... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 13: Problem 131

Which of the following are non-polar? (1) \(\mathrm{SiF}_{4}\) (2) \(\mathrm{XeF}_{4}\) (3) \(\mathrm{SF}_{4}\) (4) \(\mathrm{BF}_{3}\) (5) \(\mathrm{NF}_{3}\) Select the correct answer using the code given below: (a) 1,2 and 4 (b) 3,4 and 5 (c) 2,3 and 4 (d) 1,3 and 4

Short Answer

Expert verified
Option (a) 1, 2, and 4 are non-polar.

Step by step solution

01

Understanding Molecular Geometry

For each molecule, determine its molecular geometry. Molecules with symmetric geometries are non-polar if they have identical atoms attached to the central atom. Let's list molecular geometries for the provided compounds:1. \(\mathrm{SiF}_{4}\) has a tetrahedral shape.2. \(\mathrm{XeF}_{4}\) has a square planar shape.3. \(\mathrm{SF}_{4}\) has a see-saw shape.4. \(\mathrm{BF}_{3}\) has a trigonal planar shape.5. \(\mathrm{NF}_{3}\) has a trigonal pyramidal shape.
02

Identify Symmetry in Molecular Geometry

Determine which of the molecular geometries are symmetric:- \(\mathrm{SiF}_{4}\) is symmetric (tetrahedral).- \(\mathrm{XeF}_{4}\) is symmetric (square planar).- \(\mathrm{SF}_{4}\) is not symmetric (see-saw).- \(\mathrm{BF}_{3}\) is symmetric (trigonal planar).- \(\mathrm{NF}_{3}\) is not symmetric (trigonal pyramidal).Symmetric shapes with identical external atoms tend to be non-polar.
03

Analyze Electronegativity

While symmetry is a direct way to determine polarity, consider electronegativity: - \(\mathrm{SiF}_{4}\), \(\mathrm{XeF}_{4}\), and \(\mathrm{BF}_{3}\) form symmetrical structures, helping balance out dipoles and result in non-polar molecules since fluorine atoms are identical and symmetrically arranged.
04

Determine Polar or Non-Polar Nature

Based on the analysis of symmetry:- \(\mathrm{SiF}_{4}\) is non-polar due to its symmetrical tetrahedral shape with identical bonds.- \(\mathrm{XeF}_{4}\) is non-polar due to its symmetrical square planar shape, despite any lone pairs, as the opposing dipoles cancel out.- \(\mathrm{BF}_{3}\) is non-polar due to a symmetrical trigonal planar shape with identical bonds.- \(\mathrm{SF}_{4}\) does not possess symmetry and thus result is polar.- \(\mathrm{NF}_{3}\) has an asymmetrical shape making it polar. Therefore, the non-polar molecules are 1, 2, and 4.

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.

Polarity of Molecules
The polarity of a molecule determines how it interacts with other substances. A molecule is considered polar if it has a positive end and a negative end due to an uneven distribution of electrons. This uneven distribution leads to the formation of a dipole moment, causing the molecule to react differently with electric fields and other polar substances. In contrast, non-polar molecules have an even distribution of electronic charge. Factors affecting molecular polarity include:
  • The difference in electronegativity between atoms in a bond. A large difference usually results in a polar bond.
  • The molecular geometry, which can help cancel out dipoles within the molecule if it is symmetrical.
Understanding these factors is key in determining the polarity of molecules.
Symmetric vs Asymmetric Shapes
The symmetry of a molecule plays a crucial role in its polarity. Symmetric shapes can cause dipoles to cancel each other out, resulting in a non-polar molecule. Symmetrical molecular geometries include tetrahedral, square planar, and trigonal planar forms.In symmetric molecules:
  • Identical atoms are evenly distributed around the central atom, leading to balanced forces that negate dipole moments.
  • Examples include \(\mathrm{SiF}_4\), \(\mathrm{XeF}_4\), and \(\mathrm{BF}_3\).
On the other hand, asymmetric molecules do not have this balanced distribution, leading to a net dipole moment. Asymmetric shapes, like the see-saw shape of \(\mathrm{SF}_4\), result in polar molecules since the dipoles do not cancel out. Recognizing whether a molecule's shape is symmetric or not is essential in determining whether it will behave as polar or non-polar.
Dipole Moments
Dipole moments give quantitative measures of the polarity of a molecule. They arise from differences in electronegativity between atoms in a molecule, creating a molecule with partial positive and negative charges.Dipole moments have several key characteristics:
  • They are vectors, meaning they have both magnitude and direction, represented by a dipole arrow pointing from positive to negative charge.
  • In symmetric molecules, dipole moments cancel out, leading to a net zero dipole and a non-polar characteristic.
  • In asymmetric molecules, these vectors do not entirely cancel, producing a net dipole moment. This makes the molecule polar, such as in the case of \(\mathrm{NF}_3\).
Understanding the nature of dipole moments helps predict how molecules interact with other substances, especially in chemical reactions and solubility.

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 type of bond is not present in \(\mathrm{HNO}_{2}\) molecule? (a) covalent (b) coordinate (c) ionic (d) ionic as well as coordinate

Which of the following types of bonds are present in \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} ?\) (1) electrovalent (2) covalent (3) coordinate Select the correct answer using the code given below. (a) 1 and 2 only (b) 1 and 3 only (c) 1,2 and 3 (d) 2 and 3 only

The correct order in which the O-O bond length increases in the following is (a) \(\mathrm{O}_{2}<\mathrm{H}_{2} \mathrm{O}_{2}<\mathrm{O}_{3}\) (b) \(\mathrm{O}_{3}<\mathrm{H}_{2} \mathrm{O}_{2}<\mathrm{O}_{2}\) (c) \(\mathrm{H}_{2} \mathrm{O}_{2}<\mathrm{O}_{2}<\mathrm{O}_{3}\) (d) \(\mathrm{O}_{2}<\mathrm{O}_{3}<\mathrm{H}_{2} \mathrm{O}_{2}\)

Arrange the following compounds in order of increasing dipole moment 1\. Toluene, 2\. m-dichlorobenzene 3\. o-dichlorobenzene, 4\. p-dichlorobenzene (a) \(1<4<2<3\) (b) \(4<1<2<3\) (c) \(4<1<3<2\) (d) \(4<2 \leq 1<3\)

Find the total number of pr-d \(\pi\) bonds present in \(\mathrm{XeO}_{4}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

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.