Chemistry
12th Edition
ISBN: 9780078021510
Author: Raymond Chang Dr., Kenneth Goldsby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 10, Problem 10.66QP
Explain why the symbol on the left is a better representation of benzene molecules than that on the right.
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3) Determine whether CH3CI is polar. To do this, you must: draw the
3D structure of the molecule, use arrows to indicate polar bonds, and
either use an arrow to indicate the net dipole moment or state that the
molecule is non-polar.
For the following molecule, indicate the positive and negative ends of the dipole, using the
symbol →→→→→→→. Refer to a table of the Pauling electronegativity scale as needed. Select the single best
answer.
CO
The arrow points to the left.
The arrow points to the right.
A model for SiH4 is shown in the chem3D window. SiH4 has tetrahedral geometry.
ball & stick
|+ labels
Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom?
If you take any three of the outer atoms, what shape do they define? |
Consider the bond angles at the central atom. Do they all have the approximately the same numerical value?
What is the approximate numerical value of this angle?
| degrees.
Are all four positions about the central atom equivalent, or is one of them different from the other three.
For practice, type in the name of the geometry of the molecule:
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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. Use a molecular...Ch. 10 - The following potential energy curve represents...Ch. 10 - Prob. 10.63QPCh. 10 - Prob. 10.64QPCh. 10 - Prob. 10.65QPCh. 10 - Explain why the symbol on the left is a better...Ch. 10 - Determine which of these molecules has a more...Ch. 10 - Nitryl fluoride (FNO2) is very reactive...Ch. 10 - Describe the bonding in the nitrate ion NO3 in...Ch. 10 - Prob. 10.70QPCh. 10 - Which of the following species is not likely to...Ch. 10 - Draw the Lewis structure of mercury(II) bromide....Ch. 10 - Sketch the bond moments and resultant dipole...Ch. 10 - Although both carbon and silicon are in Group 4A,...Ch. 10 - Acetaminophen is the active ingredient in Tylenol....Ch. 10 - Caffeine is a stimulant drug present in coffee....Ch. 10 - Predict the geometry of sulfur dichloride (SCl2)...Ch. 10 - Antimony pentafluoride, SbF5, reacts with XeF4 and...Ch. 10 - Draw Lewis structures and give the other...Ch. 10 - Predict the bond angles for the following...Ch. 10 - Briefly compare the VSEPR and hybridization...Ch. 10 - Describe the hybridization state of arsenic in...Ch. 10 - Draw Lewis structures and give the other...Ch. 10 - Which of the following molecules and ions are...Ch. 10 - Prob. 10.85QPCh. 10 - The N2F2 molecule can exist in either of the...Ch. 10 - Cyclopropane (C3H6) has the shape of a triangle in...Ch. 10 - The compound 1,2-dichloroethane (C2H4Cl2) is...Ch. 10 - Does the following molecule have a dipole moment?...Ch. 10 - So-called greenhouse gases, which contribute to...Ch. 10 - The bond angle of SO2 is very close to 120, even...Ch. 10 - 3-azido-3-deoxythymidine, shown here, commonly...Ch. 10 - The following molecules (AX4Y2) all have...Ch. 10 - The compounds carbon tetrachloride (CCl4) and...Ch. 10 - Prob. 10.95QPCh. 10 - What are the hybridization states of the C and N...Ch. 10 - Use molecular orbital theory to explain the...Ch. 10 - Referring to the Chemistry in Action essay...Ch. 10 - Which of the molecules (a)(c) are polar?Ch. 10 - Prob. 10.100QPCh. 10 - The stable allotropic form of phosphorus is P4, in...Ch. 10 - Referring to Table 9.4, explain why the bond...Ch. 10 - Use molecular orbital theory to explain the...Ch. 10 - The ionic character of the bond in a diatomic...Ch. 10 - Prob. 10.105QPCh. 10 - Prob. 10.106QPCh. 10 - Aluminum trichloride (AlCl3) is an...Ch. 10 - The molecules cis-dichloroethylene and...Ch. 10 - Prob. 10.109QPCh. 10 - Prob. 10.110QPCh. 10 - The molecule benzyne (C6H4) is a very reactive...Ch. 10 - Assume that the third-period element phosphorus...Ch. 10 - Consider a N2 molecule in its first excited...Ch. 10 - Prob. 10.114QPCh. 10 - Prob. 10.116QPCh. 10 - Draw the Lewis structure of ketene (C2H2O) and...Ch. 10 - TCDD, or 2,3,7,8-tetrachlorodibenzo-p-dioxin, is a...Ch. 10 - Write the electron configuration of the cyanide...Ch. 10 - Prob. 10.120QPCh. 10 - The geometries discussed in this chapter all lend...Ch. 10 - Prob. 10.122QPCh. 10 - Which of the following ions possess a dipole...Ch. 10 - Given that the order of molecular orbitals for NO...Ch. 10 - Shown here are molecular models of SX4 for X = F,...Ch. 10 - Based on what you have learned from this chapter...Ch. 10 - How many carbon atoms are contained in one square...
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- How many valence electrons are in this molecule? SOCl2, thionyl chloridearrow_forward1. Draw the Lewis dot structure for HCOOH. (Hint: make the atom atom connectivity H-C-O-H, put in extra O on C) Based on your structure answer the following questions around the C. what is the electronic geometry? what is the molecular geometry? 2. Draw the Lewis dot structure for CH3NH2. (Hint: make the atom atom connectivity C-N-H) Based on your structure answer the following questions around the N. what is the electronic geometry? what is the molecular geometry?arrow_forwardwhat molecule is thisarrow_forward
- Select only individual atoms, and not the bonds between them. Double bonds may be conjugated, meaning that there is one single bond between them. Identify all the atoms in the structure below that must lie in the same plane.arrow_forwardConsider the molecule of furan. Its Lewis structure is shown. H X Is furan polar? If yes, consider which side of the molecule has partial negative charge and which - partial positive. Then, indicate the direction of the dipole moment relative to the molecule as shown. Non-polar, zero dipole moment. Polar, the dipole vector points along one of the C-O bonds. Polar, the dipole vector points along one of the C-H bonds. Polar, the dipole vector points along the vertical axis. Polar, the dipole vector points along the horizontal axis.arrow_forwardPART B: SHORT ANSWER AND PROBLEM SOLVING. For the following short answer questions, please show all your work in how you got your answers 1. For the molecule, ethene, CH₂ = CH₂ Write the complete electron diagram for the ethene showing all hybridize electrons and label all pi and sigma bonds.arrow_forward
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