Chemistry: An Atoms First Approach (Custom)
15th Edition
ISBN: 9781337032650
Author: UNIV.MICHIGAN
Publisher: CENGAGE L
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Textbook Question
Chapter 4, Problem 5RQ
What hybridization is required for central atoms that have a tetrahedral arrangement of electron pairs? A trigonal planar arrangement of electron pairs? A linear arrangement of e lectron pairs? How many unhybridized p atomic orbitals are present when a central atom exhibits tetrahedral geometry? Trigonal planar geometry? Linear geometry? What are the unhybridized p atomic orbitals used for? Describe the bonding in H2S, CH4, H2CO, and HCN, using the localized electron model.
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Chemistry: An Atoms First Approach (Custom)
Ch. 4 - Explain the main postulate of the VSEPR model....Ch. 4 - Explain why CF4 and Xef4 are nonpolar compounds...Ch. 4 - Consider the following compounds: CO2, SO2, KrF2,...Ch. 4 - Prob. 4RQCh. 4 - What hybridization is required for central atoms...Ch. 4 - Prob. 6RQCh. 4 - Prob. 7RQCh. 4 - What are molecular orbitals? How do they compare...Ch. 4 - Explain the difference between the and MOs for...Ch. 4 - Prob. 3ALQ
Ch. 4 - Which of the following would you expect to be more...Ch. 4 - Arrange the following molecules from most to least...Ch. 4 - Which is the more correct statement: The methane...Ch. 4 - Prob. 7ALQCh. 4 - Prob. 8ALQCh. 4 - Which of the following statements is/are true?...Ch. 4 - Give one example of a compound having a linear...Ch. 4 - In the hybrid orbital model, compare and contrast ...Ch. 4 - Prob. 13QCh. 4 - Prob. 14QCh. 4 - Prob. 15QCh. 4 - Prob. 16QCh. 4 - Compare and contrast bonding molecular orbitals...Ch. 4 - Prob. 18QCh. 4 - Why does the molecular orbital model do a better...Ch. 4 - The three NO bonds in NO3 are all equivalent in...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - Predict the molecular structure and bond angles...Ch. 4 - Prob. 24ECh. 4 - Prob. 25ECh. 4 - Two variations of the octahedral geometry (see...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - State whether or not each of the following has a...Ch. 4 - The following electrostatic potential diagrams...Ch. 4 - Which of the molecules in Exercises 21 and 22 have...Ch. 4 - Which of the molecules in Exercises 27 and 28 have...Ch. 4 - Write Lewis structures and predict the molecular...Ch. 4 - Write Lewis structures and predict whether each of...Ch. 4 - Consider the following Lewis structure where E is...Ch. 4 - Consider the following Lewis structure where E is...Ch. 4 - The molecules BF3, CF4, CO2, PF5, and SF6 are all...Ch. 4 - Two different compounds have the formula XeF2Cl2....Ch. 4 - Use the localized electron model to describe the...Ch. 4 - Use the localized electron model to describe the...Ch. 4 - Use the localized electron model to describe the...Ch. 4 - Use the localized electron model to describe the...Ch. 4 - The space-filling models of ethane and ethanol are...Ch. 4 - The space-filling models of hydrogen cyanide and...Ch. 4 - Prob. 45ECh. 4 - Prob. 46ECh. 4 - Prob. 47ECh. 4 - Give the expected hybridization of the central...Ch. 4 - For each of the following molecules, write the...Ch. 4 - For each of the following molecules or ions that...Ch. 4 - Prob. 51ECh. 4 - The allene molecule has the following Lewis...Ch. 4 - Indigo is the dye used in coloring blue jeans. The...Ch. 4 - Prob. 54ECh. 4 - Prob. 55ECh. 4 - Many important compounds in the chemical industry...Ch. 4 - Two molecules used in the polymer industry are...Ch. 4 - Hot and spicy foods contain molecules that...Ch. 4 - One of the first drugs to be approved for use in...Ch. 4 - The antibiotic thiarubin-A was discovered by...Ch. 4 - Prob. 61ECh. 4 - Sketch the molecular orbital and label its type (...Ch. 4 - Prob. 63ECh. 4 - Which of the following are predicted by the...Ch. 4 - Prob. 65ECh. 4 - Prob. 66ECh. 4 - Prob. 67ECh. 4 - Using the molecular orbital model to describe the...Ch. 4 - Prob. 69ECh. 4 - A Lewis structure obeying the octet rule can be...Ch. 4 - Using the molecular orbital model, write electron...Ch. 4 - Using the molecular orbital model, write electron...Ch. 4 - In which of the following diatomic molecules would...Ch. 4 - In terms of the molecular orbital model, which...Ch. 4 - Prob. 75ECh. 4 - Show how a hydrogen 1s atomic orbital and a...Ch. 4 - Use Figs. 4-54 and 4-55 to answer the following...Ch. 4 - The diatomic molecule OH exists in the gas phase....Ch. 4 - Prob. 79ECh. 4 - Describe the bonding in NO+, NO, and NO, using...Ch. 4 - Describe the bonding in the O3 molecule and the...Ch. 4 - Prob. 82ECh. 4 - Prob. 83AECh. 4 - Vitamin B6 is an organic compound whose deficiency...Ch. 4 - Two structures can be drawn for cyanuric acid: a....Ch. 4 - Prob. 86AECh. 4 - What do each of the following sets of...Ch. 4 - Aspartame is an artificial sweetener marketed...Ch. 4 - Prob. 89AECh. 4 - The three most stable oxides of carbon are carbon...Ch. 4 - Prob. 91AECh. 4 - Which of the following molecules have net dipole...Ch. 4 - The strucrure of TeF5 is Draw a complete Lewis...Ch. 4 - Complete the following resonance structures for...Ch. 4 - Prob. 95AECh. 4 - Describe the bonding in the first excited state of...Ch. 4 - Using an MO energy-level diagram, would you expect...Ch. 4 - Show how a dxz. atomic orbital and a pz, atomic...Ch. 4 - What type of molecular orbital would result from...Ch. 4 - Consider three molecules: A, B, and C. Molecule A...Ch. 4 - Prob. 101CWPCh. 4 - Predict the molecular structure, bond angles, and...Ch. 4 - Draw the Lewis structures for SO2, PCl3, NNO, COS,...Ch. 4 - Draw the Lewis structures for TeCl4, ICl5, PCl5,...Ch. 4 - A variety of chlorine oxide fluorides and related...Ch. 4 - Pelargondin is the molecule responsible for the...Ch. 4 - Complete a Lewis structure for the compound shown...Ch. 4 - Prob. 108CWPCh. 4 - Consider the molecular orbital electron...Ch. 4 - Place the species B2+ , B2, and B2 in order of...Ch. 4 - The compound NF3 is quite stable, but NCl3 is very...Ch. 4 - Predict the molecular structure for each of the...Ch. 4 - Prob. 113CPCh. 4 - Cholesterol (C27liu;O) has the following...Ch. 4 - Cyanamide (H2NCN), an important industrial...Ch. 4 - As compared with CO and O2, CS and S2 are very...Ch. 4 - Prob. 117CPCh. 4 - Use the MO model to explain the bonding in BeH2....Ch. 4 - Prob. 119CPCh. 4 - Arrange the following from lowest to highest...Ch. 4 - Prob. 121CPCh. 4 - Prob. 122CPCh. 4 - Carbon monoxide (CO) forms bonds to a variety of...Ch. 4 - The space-filling model for benzoic acid, a food...Ch. 4 - As the bead engineer of your starship in charge of...Ch. 4 - A flask containing gaseous N2 is irradiated with...Ch. 4 - Determine the molecular structure and...
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- Lets 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_forwardFClO2 and F3ClO can both gain a fluoride ion to form stable anions. F3ClO and F3ClO2 will both lose a fluoride ion to form stable cations. Draw the Lewis structures and describe the hybrid orbitals used by chlorine in these ions.arrow_forwardFor each of the following molecules, state the bond angle (or bond angles, as appropriate) that you would expect to see on the central atom based on the simple VSEPR model. Would you expect the actual bond angles to be greater or less than this? a CCl4 b SCl2 c COCl2 d AsH3arrow_forward
- In terms of the molecular orbital model, which species in each of the following two pairs will roost likely be the one to gain an electron? Explain. a. CN or NO b. O22+ or N22+arrow_forward7.91 A Lewis structure for the oxalate ion is shown below. (One or more other resonance forms are also possible.) What is the correct charge on the oxalate ion? What type of orbital hybridization is expected for each of the carbon atoms in this structure? How many sigma bonds and how many pi bonds does the structure contain?arrow_forwardPredict the molecular structure (including bond angles) for each of the following. (See Exercises 115 and 116.) a. ICl5 b. XeCl4 c. SeCl6arrow_forward
- What is the OSO angle and the hybrid orbital set used by sulfur in each of the following molecules or ions? (a) SO2 (b) SO3 (c) SO32 (d) SO42 Do all have the same value for the OSO angle? Does the S atom in all these species use the same hybrid orbitals?arrow_forwardMethylcyanoacrylate 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_forwardElectrons in bonding molecular orbitals are most likely to be found in the region between the two bonded atoms. Why does this arrangement favor bonding? In a antibonding orbital, where are the electrons most likely to be found in relation to the nuclei in a bond?arrow_forward
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