EBK CHEMISTRY
9th Edition
ISBN: 9780100453807
Author: ZUMDAHL
Publisher: YUZU
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Textbook Question
Chapter 9, Problem 21E
The space-filling models of ethane and ethanol are shown below.
Use the localized electron model to describe the bonding in ethane and ethanol.
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Which statement best captures the fundamental idea behind VSEPR theory? Explain what is wrong with the statements you do not choose.
a. The angle between two or more bonds is determined primarily by the repulsions between the electrons within those bonds and other (lone pair) electrons on the central atom of a molecule. Each of these electron groups (bonding electrons or lone pair electrons) lowers its potential energy by maximizing its separation from other electron groups, thus determining the geometry of the molecule.
b. The angle between two or more bonds is determined primarily by the repulsions between the electrons within those bonds. Each of these bonding electrons lowers its potential energy by maximizing its separation from other electron groups, thus determining the geometry of the molecule.
c. The geometry of a molecule is determined by the shapes of the overlapping orbitals that form the chemical bonds. Therefore, to determine the geometry of a molecule, you must determine…
Suppose that a molecule has four bonding groups and one lone pair on the central atom. Suppose further that the molecule is confined to two dimensions (this is a purely hypothetical assumption for the sake of understanding the principles behind VSEPR theory). Make a sketch of the molecule and estimate the bond angles.
Suppose that a molecule has four bonding groups and one lone pair on the central atom. Suppose further that the molecule is confined to two dimensions (this is a purely hypothetical assumption for the sake of understanding the principles behind VSEPR theory). Draw the molecule and estimate the bond angles.
Chapter 9 Solutions
EBK CHEMISTRY
Ch. 9 - Why do we hybtidize atomic orbitals to explain the...Ch. 9 - What hybridization is required for central atoms...Ch. 9 - Describe the bonding in H2S, CH4, H2CO and HCN...Ch. 9 - What hybridization is required for central atoms...Ch. 9 - Electrons in bonding molecular orbitals are most...Ch. 9 - What are molecular orbitals? How do they compare...Ch. 9 - Explain the difference between the and MOs for...Ch. 9 - Compare Figs. 4-47 and 4-49. Why are they...Ch. 9 - Which of the following would you expect to be more...Ch. 9 - Draw the Lewis structure for HCN. Indicate the...
Ch. 9 - Which is the more correct statement: The methane...Ch. 9 - Compare and contrast the MO model with the local...Ch. 9 - What are the relationships among bond order, bond...Ch. 9 - In the hybrid orbital model, compare and contrast ...Ch. 9 - In the molecular orbital mode l, compare and...Ch. 9 - Why are d orbitals sometimes used to form hybrid...Ch. 9 - The atoms in a single bond can rotate about the...Ch. 9 - Compare and contrast bonding molecular orbitals...Ch. 9 - What modification to the molecular orbital model...Ch. 9 - Why does the molecular orbital model do a better...Ch. 9 - The three NO bonds in NO3 are all equivalent in...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - The space-filling models of ethane and ethanol are...Ch. 9 - The space-filling models of hydrogen cyanide and...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - For each of the following molecules, write the...Ch. 9 - For each of the following molecules or ions that...Ch. 9 - Prob. 31ECh. 9 - The allene molecule has the following Lewis...Ch. 9 - Indigo is the dye used in coloring blue jeans. The...Ch. 9 - Urea, a compound formed in the liver, is one of...Ch. 9 - Biacetyl and acetoin are added to margarine to...Ch. 9 - Many important compounds in the chemical industry...Ch. 9 - Two molecules used in the polymer industry are...Ch. 9 - Hot and spicy foods contain molecules that...Ch. 9 - One of the first drugs to be approved for use in...Ch. 9 - The antibiotic thiarubin-A was discovered by...Ch. 9 - Consider the following molecular orbitals formed...Ch. 9 - Sketch the molecular orbital and label its type (...Ch. 9 - Which of the following are predicted by the...Ch. 9 - Which of the following are predicted by the...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - Consider the following electron configuration:...Ch. 9 - Using molecular orbital theory, explain why the...Ch. 9 - Using the molecular orbital model to describe the...Ch. 9 - The transport of O2 in the blood is carried out by...Ch. 9 - A Lewis structure obeying the octet rule can be...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - In which of the following diatomic molecules would...Ch. 9 - In terms of the molecular orbital model, which...Ch. 9 - Show how two 2p atomic orbitals can combine to...Ch. 9 - Show how a hydrogen 1s atomic orbital and a...Ch. 9 - Use Figs. 4-54 and 4-55 to answer the following...Ch. 9 - Acetylene (C2H2) can be produced from the reaction...Ch. 9 - Describe the bonding in NO+, NO, and NO, using...Ch. 9 - Describe the bonding in the O3 molecule and the...Ch. 9 - Describe the bonding in the CO32 ion using the...Ch. 9 - Draw the Lewis structures, predict the molecular...Ch. 9 - FClO2 and F3ClO can both gain a fluoride ion to...Ch. 9 - Two structures can be drawn for cyanuric acid: a....Ch. 9 - Give the expected hybridization for the molecular...Ch. 9 - Vitamin B6 is an organic compound whose deficiency...Ch. 9 - Aspartame is an artificial sweetener marketed...Ch. 9 - Prob. 69AECh. 9 - The three most stable oxides of carbon are carbon...Ch. 9 - Complete the following resonance structures for...Ch. 9 - Prob. 73AECh. 9 - Describe the bonding in the first excited state of...Ch. 9 - Using an MO energy-level diagram, would you expect...Ch. 9 - Show how a dxz. atomic orbital and a pz, atomic...Ch. 9 - What type of molecular orbital would result from...Ch. 9 - Consider three molecules: A, B, and C. Molecule A...Ch. 9 - Draw the Lewis structures for TeCl4, ICl5, PCl5,...Ch. 9 - A variety of chlorine oxide fluorides and related...Ch. 9 - Pelargondin is the molecule responsible for the...Ch. 9 - Complete a Lewis structure for the compound shown...Ch. 9 - Which of the following statements concerning SO2...Ch. 9 - Consider the molecular orbital electron...Ch. 9 - Place the species B2+ , B2, and B2 in order of...Ch. 9 - Consider the following computer-generated model of...Ch. 9 - Cholesterol (C27liu;O) has the following...Ch. 9 - Cyanamide (H2NCN), an important industrial...Ch. 9 - A flask containing gaseous N2 is irradiated with...Ch. 9 - Prob. 92CPCh. 9 - Values of measured bond energies may vary greatly...Ch. 9 - Use the MO model to explain the bonding in BeH2....Ch. 9 - Prob. 95CPCh. 9 - Arrange the following from lowest to highest...Ch. 9 - Use the MO model to determine which of the...Ch. 9 - Given that the ionization energy of F2 is 290...Ch. 9 - Carbon monoxide (CO) forms bonds to a variety of...Ch. 9 - Prob. 100CPCh. 9 - As the bead engineer of your starship in charge of...Ch. 9 - Determine the molecular structure and...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- What aspect of the following Lewis structure indicates that the concept of coordinate covalency is needed to explain the bonding in the molecule?arrow_forwardUse the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select model mode and S2O. What is the model bond angle? Explain whether the real bond angle should be larger or smaller than the ideal model angle.arrow_forwardA student who missed this class needs to know how to predict the bond angles and shape of amolecule from looking at its bond-line representation. Write a concise but complete explanationfor this student.arrow_forward
- The Lewis structure for SF6 is shown below. This sulfur S atom in this molecule has an expanded octet, and you are not expected to be familiar with the specific electron geometry and molecular geometry for expanded octets. Still, we can make some predictions with the knowledge that we have. Would you predict the electron geometry and molecular geometry for SF6 to be the same or to differ? Please briefly explain your answer.arrow_forward) Bean hexene is an odor compound used in cosmetics and cleaners. It is also known as leguminal. Its formula is: CH3CH2CHCHCH2CH2OCHCH2CH3 | OCH3 Please draw a Lewis structure for this compound with CORRECT GEOMETRY (use dashes and wedges!) Label all pi bonds in the molecule (if there are any) Indicate the bond angles for the red highlighted section of the molecule. (hint: you may want to keep the main carbon chain in-plane with the page for clarity) For this question, you don’t need to draw out the orbitals.arrow_forwardAccording to VSEPR theory , in which fashion will the bonds and lone pairs of electrons be arranged about the central atom in the following molecules or molecular ions? ICl3 molecule (The central atom is I.) ClO2- ion (The central atom is Cl.) AlCl3 molecule (The central atom is Al.) OPTIONS: - Linear - Octahedreal - Tetrahedral - Trigonal bipyramidal - Trigonal planararrow_forward
- Use the molecular model kit provided to build a model of the compound shown and draw the bond-line structure of that compound in the space below. Note: remember to draw the Lewis structure of the compound before building your model CH₂CHFCCCH₂CH3arrow_forwardPart A - Describing o and Bonds in a Molecule We have just arrived at a bonding description for the formaldehyde molecule. Which of the following statements about the molecule is or are true? I. Two of the electrons in the molecule are used to make the T bond in the molecule, II. Six of the electrons in the molecule are used to make the o bonds in the molecule III. The C-O bond length in formaldehyde should be shorter than that in methanol, H3COH. O Only one of the statements is true O Statements I and II are true O Statements I and III are true O Statements II and III are true O All three statements are true Submit Request Answer Provide Feedback amazon B. Word P Type here to search FULL HD - 1080- acerarrow_forwardDepending on the protein under study, the bond angle of a drug molecule can become critical to successfully deactivating a viral protein. For this reason, chemists are frequently concerned with the 3D shape of their molecules and their bond angles. The oxygen atom shown in the structure has a tetrahedral electronic geometry, meaning we would predict that it would have 109.5° bond angles. However, the actual structure, the bond angles are smaller than 109.5°. Explain why this compression occurs. Make sure to discuss what’s happening around/what groups are present around the oxygen atom.arrow_forward
- Which is true about valence bond theory? Select the correct answer below: Describes how the direction of overlap of s orbitals influences bond energy. Describes how two atoms can never overlap and share electrons. Describes how s orbitals are dumbbell shaped, they can only overlap end to end. Describes how the overlap of half-filled atomic orbitals yields a pair of shared electrons.arrow_forwardFor molecular geometry shown here, list the number of total electron groups, the number of bonding groups, and the number of lone pairs on the central atom.arrow_forwardExplain what is wrong with each molecular geometry and provide the correct molecular geometry, given the numbers of lone pairs and bonding groups on the central atom. Match the words in the left column to the appropriate blanks in the sentences on the right. a bent a trigonal bipyramidal an octahedral a trigonal planar a square planar a trigonal pyramidal a tetrahedral a seesaw a linear In structure (a), four pairs of electrons give cause lone pair-bonded pair repulsions and would have Reset electron geometry. The lone pair would molecular geometry. Help In structure (b), five pairs of electrons give electron geometry. The lone pair occupies an equatorial position to minimize lone pair-bonded pair repulsions, and the molecule would have molecular geometry. In structure (c), six pairs of electrons give electron geometry. The two lone pairs would occupy opposite positions to minimize lone pair-lone pair repulsions, and the molecule would have molecular geometry.arrow_forward
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