Chemistry
12th Edition
ISBN: 9780078021510
Author: Raymond Chang Dr., Kenneth Goldsby Professor
Publisher: McGraw-Hill Education
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Chapter 10, Problem 10.85QP
Interpretation Introduction
Interpretation: The hybridization of 
in 
has to be found out.
Concept Introduction:
Hybridization:
Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals that have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are
The following table shows the shapes for the various hybrid orbitals.
Figure 1
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How many milliliters of 97.5(±0.5) wt% H2SO4 with a density of 1.84(±0.01) g/mL will you need to prepare 2.000 L of 0.110 M H2SO4?
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Chapter 10 Solutions
Chemistry
Ch. 10.1 - Use the VSEPR model to predict the geometry of (a)...Ch. 10.1 - Which of the following geometries has a greater...Ch. 10.2 - Does the AlCl3 molecule have a dipole moment?Ch. 10.2 - Carbon dioxide has a linear geometry and is...Ch. 10.3 - Compare the Lewis theory and the valence bond...Ch. 10.4 - Determine the hybridization state of the...Ch. 10.4 - Describe the hybridization state of Se in SeF6.Ch. 10.4 - What is the hybridization of Xe in XeF4Ch. 10.5 - Describe the bonding in the hydrogen cyanide...Ch. 10.5 - Which of the following pairs of atomic orbitals on...
Ch. 10.6 - One way to account for the fact that an O2...Ch. 10.7 - Estimate the bond enthalpy (kJ/mol) of the H2+...Ch. 10.7 - Which of the following species has a longer bond...Ch. 10.8 - Describe the bonding in the nitrate ion (NO3) in...Ch. 10 - How is the geometry of a molecule defined and why...Ch. 10 - Sketch the shape of a linear triatomic molecule, a...Ch. 10 - How many atoms are directly bonded to the central...Ch. 10 - Discuss the basic features of the VSEPR model....Ch. 10 - Prob. 10.5QPCh. 10 - Prob. 10.6QPCh. 10 - Predict the geometries of the following species...Ch. 10 - Predict the geometries of the following species:...Ch. 10 - Predict the geometry of the following molecules...Ch. 10 - Predict the geometry of the following molecules...Ch. 10 - Predict the geometry of the following molecules...Ch. 10 - Predict the geometries of the following ions: (a)...Ch. 10 - Describe the geometry around each of the three...Ch. 10 - Which of the following species are tetrahedral?...Ch. 10 - Prob. 10.15QPCh. 10 - Prob. 10.16QPCh. 10 - Prob. 10.17QPCh. 10 - The bonds in beryllium hydride (BeH2) molecules...Ch. 10 - Referring to Table 10.3, arrange the following...Ch. 10 - The dipole moments of the hydrogen halides...Ch. 10 - List the following molecules in order of...Ch. 10 - Does the molecule OCS have a higher or lower...Ch. 10 - Which of the molecules (a) or (b) has a higher...Ch. 10 - Prob. 10.24QPCh. 10 - What is valence bond theory? How does it differ...Ch. 10 - Use valence bond theory to explain the bonding in...Ch. 10 - Prob. 10.27QPCh. 10 - Prob. 10.28QPCh. 10 - What is the angle between the following two hybrid...Ch. 10 - How would you distinguish between a sigma bond and...Ch. 10 - Describe the bonding scheme of the AsH3 molecule...Ch. 10 - What is the hybridization state of Si in SiH4 and...Ch. 10 - Describe the change in hybridization (if any) of...Ch. 10 - Consider the reaction BF3+NH3F3BNH3 Describe the...Ch. 10 - What hybrid orbitals are used by nitrogen atoms in...Ch. 10 - What are the hybrid orbitals of the carbon atoms...Ch. 10 - Specify which hybrid orbitals are used by carbon...Ch. 10 - Prob. 10.38QPCh. 10 - The allene molecule H2CCCH2 is linear (the three C...Ch. 10 - Prob. 10.40QPCh. 10 - How many sigma bonds and pi bonds are there in...Ch. 10 - How many pi bonds and sigma bonds are there in the...Ch. 10 - Give the formula of a cation comprised of iodine...Ch. 10 - Give the formula of an anion comprised of iodine...Ch. 10 - What is molecular orbital theory? How does it...Ch. 10 - Sketch the shapes of the following molecular...Ch. 10 - 10.47 Compare the Lewis theory, valence bond...Ch. 10 - Explain the significance of bond order. Can bond...Ch. 10 - Explain in molecular orbital terms the changes in...Ch. 10 - The formation of H2 from two H atoms is an...Ch. 10 - Prob. 10.51QPCh. 10 - Arrange the following species in order of...Ch. 10 - Prob. 10.53QPCh. 10 - Which of these species has a longer bond, B2 or...Ch. 10 - Acetylene (C2H2) has a tendency to lose two...Ch. 10 - Compare the Lewis and molecular orbital treatments...Ch. 10 - Explain why the bond order of N2 is greater than...Ch. 10 - Compare the relative stability of the following...Ch. 10 - Use molecular orbital theory to compare the...Ch. 10 - A single bond is almost always a sigma bond, and a...Ch. 10 - In 2009 the ion N23 was isolated. 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