Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 9, Problem 52IL
Ethylene oxide is an intermediate in the manufacture or ethylene glycol (antifreeze) and polyester
(a) What are the bond angles in the ring? Comment on the relation between the bond angles expected based on hybridization an d the bond angles expected for a three-member ring.
(b) Is the molecule polar? Based on the electrostatic poten1ial map shown below. where do the neg-alive and positive charges lie in the molecule?
Polarity: It is a well separation of electric charge leading to a molecule or chemical compounds having an electrical dipole moment. Generally the polar molecules must contain polar bonds due to a different in electronegative between the bonded atoms.
The electrostatic potential map clearly to explain, the oxygen atom has more negative (δ–) charge and other side has less positive (δ–) charge, so this molecule is a more polar nature.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The structure of caffeine is shown below.
(a) Complete the Lewis structure.
(b) How many pi bonds are present in caffeine? How many sigma bonds?
(c) Identify the hybridization of the carbon atoms.
(d) What is the value of the O-C-N angle?
Identify and label geometry, hybridization, sigma bonds and pi bonds for any atom/group of atoms.
A structure of XanaxTM is shown here.
(a) and (b): Identify the hybridization state AND geometry of each of the indicated atoms.
(c) List the total number of pi bonds in the structure.
(d) List the total number of tetrahedral carbons.
CI
N
(a)
(b)
The structural formulas for ethanol, CH3CH2OH, and propene,
CH;CH=CH,2, are
нн
H
Н—С—С—0—н
H-C-C=C-H
нн
H H H
Ethanol
Propene
(a) Complete the Lewis structure for each molecule showing all valence
electrons.
(b) Using the VSEPR model, predict all bond angles in each molecule.
Chapter 9 Solutions
Chemistry & Chemical Reactivity
Ch. 9.2 - Use valence bond theory to describe the bonding in...Ch. 9.2 - Identify the hybridization of each underlined atom...Ch. 9.2 - Use valence bond theory to describe the bonding in...Ch. 9.2 - What is the hybridization of the S atom (the...Ch. 9.2 - 2. Which of the following is incorrect?
The...Ch. 9.2 - Prob. 3RCCh. 9.2 - Prob. 4RCCh. 9.3 - What is the electron configuration of the H2+ ion?...Ch. 9.3 - Could the anion Li2 exist? What is the ions bond...Ch. 9.3 - The cations O2+ and N2+ are formed when molecules...
Ch. 9.3 - What is the NO bond order in nitrogen monoxide,...Ch. 9.3 - Prob. 2RCCh. 9.3 - Prob. 3RCCh. 9.3 - 4. Among the known dioxygen species (O2+, O2, O2−...Ch. 9.3 - What is the empirical formula of Tynan purple?Ch. 9.3 - Butter yellow absorbs light with a wavelength of...Ch. 9.3 - Prob. 3CSCh. 9.A - Photoelectron spectroscopy is s1milar to the...Ch. 9.A - What is the energy of a photon with a wavelength...Ch. 9.A - Using the accompanying figure, state which...Ch. 9.A - The kinetic energy of an electron ejected from the...Ch. 9.A - The N2+ ions that are formed when electrons with...Ch. 9 - Draw the Lewis structure for chloroform, CHCl3....Ch. 9 - Draw the Lewis structure for NF3. What are its...Ch. 9 - Draw the Lewis structure for hydroxylamine, H2NOH....Ch. 9 - Draw the Lewis structure for 1,...Ch. 9 - Draw the Lewis structure for carbonyl fluoride,...Ch. 9 - Draw the Lewis structure for acetamide, CH3CONH2....Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Prob. 9PSCh. 9 - What is the hybrid orbital set used by each of the...Ch. 9 - Draw the Lewis structures of the acid HPO2F2 and...Ch. 9 - Draw the Lewis structures of the arid HSO3F and...Ch. 9 - What is the hybridization of the carbon atom in...Ch. 9 - What is the hybridization of the carbon atoms in...Ch. 9 - What is the electron-pair and molecular geometry...Ch. 9 - Prob. 17PSCh. 9 - For each compound below, decide whether cis and...Ch. 9 - Molecular Orbital Theory (See Examples 9.49.6.)...Ch. 9 - Give the electron configurations for the ions Li2+...Ch. 9 - Platinum hexafluoride is an extremely strong...Ch. 9 - When potassium and oxygen react, one of the...Ch. 9 - Among the following, which has the shortest bond...Ch. 9 - Consider the following list of small molecules and...Ch. 9 - Prob. 27PSCh. 9 - The nitrosyl ion. NO+, has an interesting...Ch. 9 - These questions are not designated as to type or...Ch. 9 - What is the OSO angle and the hybrid orbital set...Ch. 9 - Sketch the resonance structures for the nitrite...Ch. 9 - Sketch the resonance structures for the nitrate...Ch. 9 - Sketch the resonance structures for the N2O...Ch. 9 - Compare the structure and bonding in CO2 and CO32...Ch. 9 - Numerous molecules are detected in deep space....Ch. 9 - Acrolein, a component of photochemical smog, has a...Ch. 9 - The organic compound below is a member of a class...Ch. 9 - The compound sketched below is acetylsalicylic...Ch. 9 - Phosphoserine is a less-common amino acid. (a)...Ch. 9 - Lactic acid is a natural compound found in sour...Ch. 9 - Cinnamaldehyde ocaus naturally in cinnamon oil....Ch. 9 - The ion Si2 was reported in a laboratory...Ch. 9 - The simple valence bond picture of O2 does not...Ch. 9 - Nitrogen, N2, can ionize to form N2+ or add an...Ch. 9 - Which of the homonuclear, diatomic molecules of...Ch. 9 - Which of the following molecules or ions are...Ch. 9 - Prob. 47GQCh. 9 - The structure of amphetamine, a stimulant, is...Ch. 9 - Menthol is used in soaps, perfumes, and foods. It...Ch. 9 - Prob. 50GQCh. 9 - Suppose you carry out the following reaction of...Ch. 9 - Ethylene oxide is an intermediate in the...Ch. 9 - The sulfamate ion, H2NSO3, can be thought of as...Ch. 9 - The compound whose structure is shown here is...Ch. 9 - Prob. 55ILCh. 9 - Carbon dioxide (CO2), dinitrogen monoxide (N2O),...Ch. 9 - Draw the two resonance structures that describe...Ch. 9 - Draw a Lewis structure for diimide, HNNH. Then,...Ch. 9 - Prob. 59SCQCh. 9 - Consider the three fluorides BF4, SiF4, and SF4....Ch. 9 - When two amino acids react with each other, they...Ch. 9 - What is the connection between bond order, bond...Ch. 9 - When is it desirable to use MO theory rather than...Ch. 9 - Show how valence bond theory and molecular orbital...Ch. 9 - Three of the four molecular orbitals for...Ch. 9 - Lets look more closely at the process of...Ch. 9 - Borax has the molecular formula Na2B4O5(OH)4. The...Ch. 9 - A model of the organic compound allene is shown...Ch. 9 - Prob. 69SCQCh. 9 - Prob. 70SCQCh. 9 - Bromine forms a number of oxides of varying...Ch. 9 - Prob. 72SCQCh. 9 - Urea reacts with malonic acid to produce...
Knowledge Booster
Learn more about
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
- H2CO molecules (a) use orbital hybridization theory to determine the molecular shape of h2co. (b) what bonds are formed between the c and o atoms in formaldehyde molecules?arrow_forwardBond energy : 4. (a) Draw the Lewis structure of NH,BCI, and name the bond between N and B. (b) State the type of orbital hybridization of N in NH3 and in NH3BCI3. NH3: NH;BCI3:arrow_forward(a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forward
- For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. [b] The greater the orbital overlap in a bond, the shorter the bond. [c] To create a hybrid orbital, you could use the s orbital on one atom with a p orbital on another atom. [d] Nonbonding electron pairs cannot occupy a hybrid orbital.arrow_forwardindicate the approximate values for the indicated bond angles in the following molecules. 1 (a) H 0-N=ö 2. Н 4 H. (b) H C-c=0 H H H (c) H-N-O–H . H. (d) H-C-C=N: H.arrow_forwardConsider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.arrow_forward
- The molecule shown below is called furan. It is represented intypical shorthand way for organic molecules, with hydrogenatoms not shown, and each of the 4 vertices representing acarbon atom. (a) What is the molecular formula for furan? (b) How manyvalence electrons are there in the molecule? (c) What isthe hybridization at each of the carbon atoms? (d) Howmany electrons are in the π system of the molecule? (e) TheC¬C¬C bond angles in furan are much smaller than thosein benzene. The likely reason is which of the following: (i) Thehybridization of the carbon atoms in furan is different fromthat in benzene, (ii) Furan does not have another resonancestructure equivalent to the one above, or (iii) The atoms in afive-membered ring are forced to adopt smaller angles than ina six-membered ring.arrow_forwardChloral (Cl₃C—CH=O) forms a monohydrate, chloralhydrate, the sleep-inducing depressant called “knockout drops”in old movies. (a) Write two possible structures for chloral hy-drate, one involving hydrogen bonding and one that is a Lewis adduct. (b) What spectroscopic method could be used to identify the real structure? Explain.arrow_forwardH genistein HO, H H : ОН HO, H (a) Is the hybridization of each C in the right-most ring the same? Explain. (b) Is the hybridization of the O atoms in/on the center ring the same as that of the O atoms in the OH groups? Explain. (c) How many carbon-oxygen o-bonds are there in genistein? How many carbon-oxygen n-bonds? (d) Do all the lone pairs on the oxygens occupy the same type of hybrid orbital? Explain by labeling the hybridization of each oxygen atom in genistein.arrow_forward
- (b) Draw the Lewis structure of the following molecule including its proper geometry. CH2CHC(O)CH3 a) Draw a complete orbital picture of the molecule.arrow_forwardButadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths: (a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.arrow_forward3) Which statement best describe the structure of a carbonate anion C02- ? A) The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are 120°. There is a n-bond formed between a non-hybridized "C" p-orbital overlapping with an "O" p-orbital. C) The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are 120°. There is a 7-bond formed between a non-hybridized “C" p-orbital overlapping with an “O" p-orbital.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
INTRODUCTION TO MOLECULAR QUANTUM MECHANICS -Valence bond theory - 1; Author: AGK Chemistry;https://www.youtube.com/watch?v=U8kPBPqDIwM;License: Standard YouTube License, CC-BY