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Chemistry for Engineering Students

3rd Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781285199023

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BuyFindarrow_forward

Chemistry for Engineering Students

3rd Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781285199023
Chapter 7, Problem 7.35PAE
Textbook Problem
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7.31 Why is a bond between two atoms with different electronegativities called a polar bond?

Interpretation Introduction

Interpretation:

Determine why a bond between two atoms with different electronegativities is called a polar bond.

Concept Introduction:

Bond polarity is a concept used to describe the sharing of electrons between atoms. When the electrons are shared equally among the atoms, the bond so formed is called non-polar covalent bond. When the attraction for an electron is larger in one atom than the other one, the bond so formed is a polar covalent bond. The bond is said to be ionic if the relative attraction is too large. 'Electronegativity' is a term used to analyze a given bond and find out whether it is an ionic bond, non-polar covalent bond or a polar covalent bond.

Explanation of Solution

Two atoms will share an electron pair in a covalent bond. But, the electrons are not always shared in equal numbers between them. If two atoms with the same electronegativity form a covalent bond, then that bond is non-polar, because o...

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Chapter 7 Solutions

Chemistry for Engineering Students
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Ch. 7 - • explain the formation of multiple bonds in terms...Ch. 7 - • identify sigma and pi bonds in a molecule and...Ch. 7 - Define the term biocompatibility.Ch. 7 - List some properties associated with biomaterials...Ch. 7 - Describe how PMMA functions as bone cement. How...Ch. 7 - The formulas of sodium phosphate and sodium...Ch. 7 - Why do biomedical engineers sometimes need to use...Ch. 7 - Use the concept of polarity of water and the base...Ch. 7 - Why is the ion not found in nature?Ch. 7 - Why do nonmetals tend to form anions rather than...Ch. 7 - Select the smaller member of each of the following...Ch. 7 - 7.10 Arrange the members of each of the following...Ch. 7 - 7.11 Arrange the following sets of anions in order...Ch. 7 - 7.12 Which pair will form a compound with the...Ch. 7 - In a lattice, a positive ion is often surrounded...Ch. 7 - Use the concept of lattice energy to rationalize...Ch. 7 - 7.13 Figure 7-2 depicts the interactions of an ion...Ch. 7 - Mat type of bond is likely to form between one...Ch. 7 - 7.14 Describe the difference between a covalent...Ch. 7 - 7.16 Considering the potential energy of...Ch. 7 - Sketch a graph of the potential energy of two...Ch. 7 - When a covalent bond forms, is energy absorbed or...Ch. 7 - 7.17 Coulombic forces are often used to explain...Ch. 7 - 7.18 In terms of the strengths of the covalent...Ch. 7 - 7.19 If the formation of chemical bonds always...Ch. 7 - 7.20 Draw the Lewis dot symbol for each of the...Ch. 7 - 7.21 Theoretical models for the structure of...Ch. 7 - 7.22 Use Lewis dot symbols to explain why chlorine...Ch. 7 - 7.23 Define the term lone pair.Ch. 7 - 7.24 How many electrons are shared between two...Ch. 7 - 7.25 How does the bond energy of a double bond...Ch. 7 - 7.26 How is electronegativity defined?Ch. 7 - 7.27 Distinguish between electron affinity and...Ch. 7 - 7.28 Certain elements in the periodic table shown...Ch. 7 - 7.29 When two atoms with different...Ch. 7 - 7.30 The bond in HF is said to be polar, with the...Ch. 7 - 7.31 Why is a bond between two atoms with...Ch. 7 - 7.32 Based on the positions in the periodic table...Ch. 7 - 7.33 In each group of three bonds, which bond is...Ch. 7 - 7.34 Considering the trends in electronegativity...Ch. 7 - Can fluorine atoms ever carry a partial positive...Ch. 7 - 7.35 Which one of the following contains botb...Ch. 7 - Using only halogen atoms, what would be the most...Ch. 7 - 7.36 Suppose that you wanted to make a diatomic...Ch. 7 - 7.37 Draw the Lewis structure for each of the...Ch. 7 - 7.38 Draw a Lewis structure for each of the...Ch. 7 - 7.39 Write Lewis structures for these molecules,...Ch. 7 - 7.40 Why is it impossible for hydrogen to be the...Ch. 7 - 7.41 In the context of Lewis structures, what us...Ch. 7 - 7.42 Draw resonance structure for (a) (b) and (c)Ch. 7 - 7.43 How does the structure of a molecule that...Ch. 7 - 7.44 Draw the Lewis structure of two resonance...Ch. 7 - 7.45 How does the existence of resonance...Ch. 7 - 7.46 Consider the nitrogen-oxygen bond lengths in...Ch. 7 - 7.47 Which of the species listed has a Lewis...Ch. 7 - 7.48 Identify what is incorrect in the Lewis...Ch. 7 - 7.49 Identify what is incorrect in the Lewis...Ch. 7 - 7.50 Chemical species are said to be isoelectronic...Ch. 7 - 7.51 Explain the concept of wave interference in...Ch. 7 - Distinguish between constructive and destructive...Ch. 7 - How is the concept of orbital overlap related to...Ch. 7 - 7.52 How does orbital overlap explain the buildup...Ch. 7 - 7.53 How do sigma and pi bonds differ? How are...Ch. 7 - 7.54 CO , CO2 , CH3OH , and CO32 , all contain...Ch. 7 - 7.55 Draw the Lewis dot structure of the following...Ch. 7 - 7.56 Draw the Lewis dot structures of the...Ch. 7 - 7.57 What observation about molecules compels us...Ch. 7 - 7.58 The number of hybrid orbitals formed must...Ch. 7 - 7.59 What type of hybrid orbital is generated by...Ch. 7 - Considering only s and p atomic orbitals, list all...Ch. 7 - 7.61 What hybrid orbitals would be expected for...Ch. 7 - 7.62 What type of hybridization would you expect...Ch. 7 - 7.63 What physical concept forms the premise of...Ch. 7 - 7.64 Predict the geometry of the following...Ch. 7 - 7.65 Predict the shape of each of the following...Ch. 7 - 7.66 Predict the shape of each of the following...Ch. 7 - 7.67 Which of these molecules would be linear?...Ch. 7 - 7.68 Give approximate values for the indicated...Ch. 7 - 7.69 Propene has the chemical formula Describe the...Ch. 7 - Describe why a central atom with four bonding...Ch. 7 - Describe what happens to the shape about the...Ch. 7 - 7.70 Describe why treatments like chemotherapy for...Ch. 7 - 7.71 Use the fundamental structure of mesoporous...Ch. 7 - 7.72 How does an MSN differ from amorphous silica...Ch. 7 - 7.73 Draw a schematic picture of an MSN being used...Ch. 7 - In 1999, chemists working for the Air Force...Ch. 7 - The following molecules have similar formulas, but...Ch. 7 - 7.90 Consider the Lewis structure below. Is this...Ch. 7 - 7.91 A Lewis structure for the oxalate ion is...Ch. 7 - 7.92 Methyl cyanoacrylate, is the compound...Ch. 7 - 7.93 An unknown metal M forms a chloride with the...Ch. 7 - 7.94 Nearly all of the other elements form binary...Ch. 7 - 7.95 Although we often classify bonds between a...Ch. 7 - 7.96 Consider the hydrocarbons whose structures...Ch. 7 - 7.97 Consider the structure shown below for as...Ch. 7 - 7.98 Electrical engineers often use lithium...Ch. 7 - 7.99 One of the “grand challenges” for engineering...Ch. 7 - 7.100 Another “grand challenge” for engineering is...Ch. 7 - 7.101 Lead selenide nanocrystals may provide a...Ch. 7 - 7.102 Both ozone O 3and oxygen, O 2absorb UV light...Ch. 7 - 7.103 Nitrogen is the primary component of our...Ch. 7 - 7.104 Hydrogen azide, HN3 , is a liquid that...Ch. 7 - 7.105 If leads are attached to the opposite sides...Ch. 7 - 7.106 How does electronegativity relate to the...Ch. 7 - 7.107 How do the Lewis symbols for C, Si, and Ge...Ch. 7 - 7.108 Use Lewis symbols to describe how free...Ch. 7 - 7.109 When free radical polymerization occurs, how...

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