Chemistry
12th Edition
ISBN: 9780078021510
Author: Raymond Chang Dr., Kenneth Goldsby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 10.5, Problem 5PE
Describe the bonding in the hydrogen cyanide molecule, HCN. Assume that N is sp-hybridized.
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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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- Consider the polyatomic ion IO65-. How many pairs of electrons are around the central iodine atom? What is its hybridization? Describe the geometry of the ion.arrow_forwardAspirin, or acetylsalicylic acid, has the formula C9H8O4 and the skeleton structure (a) Complete the Lewis structure and give the number of bonds and bonds in aspirin. (b) What is the hybridization about the CO2H carbon atom (colored blue)? (c) What is the hybridization about the carbon atom in the benzene-like ring that is bonded to an oxygen atom (colored red)? Also, what is the hybridization of the oxygen atom bonded to this carbon atom?arrow_forwardDescribe the hybridization around the central atom and the bonding in SCl2 and OCS.arrow_forward
- Methylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is (a) How many sigma bonds are in the molecule? (b) How many pi bonds are in the molecule? (c) What is the hybridization of the carbon atom bonded to nitrogen? (d) What is the hybridization of the carbon atom bonded to oxygen? (e) What is the hybridization of the double-bonded oxygen?arrow_forwardGamma hydroxybutyric acid, GHB, infamous as a date rape drug, is used illicitly because of its effects on the nervous system. The condensed molecular formula for GHB is HO(CH2)3COOH. (a) Write the Lewis structure for GHB. (b) Identify the hybridization of the carbon atom in the CH2 groups and of the terminal carbon. (c) Is hydrogen bonding possible in GHB? If so, write Lewis structures to illustrate the hydrogen bonding. (d) Which carbon atoms are involved in sigma bonds? In pi bonds? (e) Which oxygen atom is involved in sigma bonds? In pi bonds?arrow_forwardWhy is the concept of hybridization required in valence bond theory?arrow_forward
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- The hybridization of the two carbon atoms differs in an acetic acid, CH3COOH, molecule. (a) Designate the correct hybridization for each carbon atom in this molecule. (b) What is the approximate bond angle around each carbon?arrow_forwardCalcium cyanamide, CaNCN, is used both to kill weeds and as a fertilizer. Give the Lewis structure of the NCN2 ion and the bonded-atom lone-pair arrangement and hybridization of the carbon atom.arrow_forwardThe sulfamate ion, H2NSO3, can be thought of as having been formed from the amide ion, NH2, and sulphur trioxide, SO3. (a) What are the electron-pair and molecular geometries or the amide ion and or SO3? What are the hybridizations of the N and S atoms, respectively? (b) Sketch a structure for the sulfamate ion, and estimate the bond angles. (c) What changes in hybridization do you expect for N and S in the course of the reaction NH2 + SO3 H2NSO3? (d) Is SO3 the donor of an electron pair or the acceptor of an electron pair in the reaction with amide ion? Does the electrostatic potential map shown below confirm your prediction?arrow_forward
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