Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 7, Problem 7.81PAE
Interpretation Introduction
Interpretation:
To find out the types of hybrid orbital’s using the single bond, double bond,and triple bond formation.
Concept introduction: According to
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7. Nitrogen is the central atom in each of the species given.
(a) Draw the Lewis electron-dot structure for each of the species.
+
NO₂ NO₂ NO₂
(b) List the species in order of increasing bond angle. Justify your answer.
(c) For NO₂ and NO₂, give the hybridization of the nitrogen atom in it.
(d) Identify the only one of the species that dimerizes and explain what causes it to do so.
Complete the following table based on the structure of the given
molecules or ions. (Note: Lewis structure will not be graded)
Electron Pair
Geometry
Molecular
Geometry
Hybridization
of the Central
Atom
Molecule/lon
Resonance
Structures
(Yes/No)
(a) Chlorine
trifluoride
(CIF3)
(b) Nitrite ion
(NO2')
Consider the reaction BF3 + NH3 -> F3B-NH3
(a) Describe the changes in hybridization of the B and N atoms as a result of this reaction.
(b) Describe the shapes of all the reactant molecules with their bond angles.
(c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms.
(d) What is the name of the bond between B and N.
(e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.
Chapter 7 Solutions
Chemistry for Engineering Students
Ch. 7 - List some factors influencing the biocompatibility...Ch. 7 - • use electron configurations to explain why...Ch. 7 - • describe die energy changes in the formation of...Ch. 7 - • define electronegativity and state how...Ch. 7 - • identify or predict polar, nonpolar, and ionic...Ch. 7 - • write Lewis electron structures for molecules or...Ch. 7 - • describe chemical bonding using a model based on...Ch. 7 - • explain how hybridization reconciles observed...Ch. 7 - • predict the geometry of a molecule from its,...Ch. 7 - • use models (real or software) to help visualize...
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 - Prob. 7.3PAECh. 7 - Prob. 7.4PAECh. 7 - Prob. 7.5PAECh. 7 - Prob. 7.6PAECh. 7 - Why is the ion not found in nature?Ch. 7 - Why do nonmetals tend to form anions rather than...Ch. 7 - Prob. 7.9PAECh. 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 - 7.13 Figure 7-2 depicts the interactions of an ion...Ch. 7 - 7.14 Describe the difference between a covalent...Ch. 7 - 7.15 Covalently bonded compounds tend to have much...Ch. 7 - Prob. 7.16PAECh. 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 - Prob. 7.32PAECh. 7 - 7.33 In each group of three bonds, which bond is...Ch. 7 - Prob. 7.34PAECh. 7 - 7.35 Which one of the following contains botb...Ch. 7 - Prob. 7.36PAECh. 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 - Prob. 7.39PAECh. 7 - 7.40 Why is it impossible for hydrogen to be the...Ch. 7 - Prob. 7.41PAECh. 7 - 7.42 Draw resonance structure for (a) (b) and (c)Ch. 7 - Prob. 7.43PAECh. 7 - Prob. 7.44PAECh. 7 - Prob. 7.45PAECh. 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 - 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 - Prob. 7.58PAECh. 7 - 7.59 What type of hybrid orbital is generated by...Ch. 7 - 7.60 What type of hybridization would be expected...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 - Prob. 7.65PAECh. 7 - Prob. 7.66PAECh. 7 - Prob. 7.67PAECh. 7 - 7.68 Give approximate values for the indicated...Ch. 7 - 7.69 Propene has the chemical formula Describe the...Ch. 7 - Prob. 7.70PAECh. 7 - Prob. 7.71PAECh. 7 - 7.72 How does an MSN differ from amorphous silica...Ch. 7 - Prob. 7.73PAECh. 7 - 7.74 In a lattice, a positive ion is often...Ch. 7 - 7.75 Use the concept of lattice energy to...Ch. 7 - Prob. 7.76PAECh. 7 - Prob. 7.77PAECh. 7 - Prob. 7.78PAECh. 7 - Prob. 7.79PAECh. 7 - Prob. 7.80PAECh. 7 - Prob. 7.81PAECh. 7 - Prob. 7.82PAECh. 7 - Prob. 7.83PAECh. 7 - 7.84 Which of the following molecules is least...Ch. 7 - 7.85 Consider the molecule whose structure is...Ch. 7 - 7.86 Nitrogen triiodide, NI3(s) , is unstable and...Ch. 7 - 7.87 Nitrogen is capable of forming single,...Ch. 7 - 7.88 The N5+ cation has been synthesized and...Ch. 7 - Prob. 7.89PAECh. 7 - Prob. 7.90PAECh. 7 - 7.91 A Lewis structure for the oxalate ion is...Ch. 7 - Prob. 7.92PAECh. 7 - 7.93 An unknown metal M forms a chloride with the...Ch. 7 - Prob. 7.94PAECh. 7 - Prob. 7.95PAECh. 7 - 7.96 Consider the hydrocarbons whose structures...Ch. 7 - 7.97 Consider the structure shown below for as...Ch. 7 - Prob. 7.98PAECh. 7 - Prob. 7.99PAECh. 7 - Prob. 7.100PAECh. 7 - 7.101 Lead selenide nanocrystals may provide a...Ch. 7 - Prob. 7.102PAECh. 7 - Prob. 7.103PAECh. 7 - 7.104 Hydrogen azide, HN3 , is a liquid that...Ch. 7 - Prob. 7.105PAECh. 7 - Prob. 7.106PAECh. 7 - 7.107 How do the Lewis symbols for C, Si, and Ge...Ch. 7 - Prob. 7.108PAECh. 7 - Prob. 7.109PAE
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- In each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.arrow_forward7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals?arrow_forward• identify sigma and pi bonds in a molecule and explain the difference between them.arrow_forward
- Considering only s and p atomic orbitals, list all the possible types of hybrid orbitals that can be used in the formation of (a) single bonds, (b) double bonds, and (c) triple bonds.arrow_forwardIt is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forwardWhat hybrid orbitals would be expected for the central atom in each of the following molecules or ions?arrow_forward
- Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.arrow_forwardLets look more closely at the process of hybridization. (a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them? (b) Do hybrid atomic orbitals form between different p orbitals without involving 5 orbitals? (c) What is the relationship between the energy of hybrid atomic orbitals and the atomic orbitals from which they are formed?arrow_forwardWhy is the concept of hybridization required in valence bond theory?arrow_forward
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