Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Textbook Question
Chapter 3, Problem 7E
Explain what is wrong with each of the following statements.
a. “A
b. “A
c. “A
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a. One of the two known binary compounds of xenon and oxygen is XeO3. A Lewis structure is shown here, which may or may not be complete. How many lone pairs should be present on the central Xe atom?
b. What is the electron pair geometry around the Xe?
c. What is the molecular geometry of XeO3?
d. What hybrid orbitals does the Xe atom use?
Which statement is true concerning molecular orbital (MO) theory?
A. Atomic orbitals overlap to form bonds
B. Atomic orbitals combine to form both bonding and anti-bonding orbitals
C. Atomic orbitals through VSEPR can determine the geometric shapes of molecules
D. Atomic orbitals on the same atom combine with each other to make hybrid orbitals.
Which one of the following statements about molecular orbitals for homonuclear diatomic molecules is incorrect?
a. Pi orbitals are symmetric to rotation about the internuclear axis.
b. Sigma orbitals have a symmetrical distribution of electron density around the two nuclei.
c. Sigma* orbitals are higher in energy than their corresponding sigma orbitals.
d. Sigma orbitals can be formed from the overlap of s or p atomic orbitals.
e. Pi orbitals have a planar node along the internuclear axis.
Chapter 3 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 3 - Prob. 1CTQCh. 3 - What neutral atom is represented by the electron...Ch. 3 - Prob. 3CTQCh. 3 - Consider any one of the four identical hybrid...Ch. 3 - Prob. 5CTQCh. 3 - Prob. 6CTQCh. 3 - Prob. 7CTQCh. 3 - Prob. 8CTQCh. 3 - Prob. 9CTQCh. 3 - Prob. 10CTQ
Ch. 3 - On the left side of Figure 3.6, label the areas...Ch. 3 - Prob. 12CTQCh. 3 - Prob. 13CTQCh. 3 - Prob. 14CTQCh. 3 - Prob. 15CTQCh. 3 - Now consider the fully formed molecule on the...Ch. 3 - Prob. 1ECh. 3 - Explain why the two molecules below cannot...Ch. 3 - Prob. 3ECh. 3 - Consider the incomplete orbital representation of...Ch. 3 - Consider the following orbital representation of...Ch. 3 - Summarize how one determines the hybridization...Ch. 3 - Explain what is wrong with each of the following...Ch. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Complete the following tables, and memorize their...Ch. 3 - Draw orbital representations of bonding in water...Ch. 3 - Draw electron configuration diagrams for carbon in...Ch. 3 - Prob. 13E
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- This question is related to valence bond theory. a. Explain the assumptions made in bonding models under valence bond theory. What best describes bonding under these models? b. Draw the Lewis structure of SO2. Identify bonds in the moldule as either sigma or pi bonds. Draw orbital diagrams for ground state S and O atoms. Use these orbital diagrams determine the geometry of SO2 using valence bond theory (hint: SO2 must be descried using hybrid atomic orbitals. In other words, which orbitals on which atoms overlap to give rise to which bonds? C. d. Explain why valence bond theory does not adequately describe the bonding in SO2, even though it accurately predicts the geometry/bond angle.arrow_forwardFour sp3 hybrid orbitals has what kind of arrangement of electron pair .A Octahedral Tetrahedral .B .C Linear .D Trigonal planararrow_forward11. What is the electron-domain geometry of water molecule (H2O)? a. bent b. tetrahedral c. trigonal planar d. linear 12. Write the correct Lewis dot structure for O2. Which statement correctly describes the structure of the whole molecule? a. There is a double bond and four lone pairs. b. There is a double bond and six lone pairs. c. There is a single bond and six lone pairs. d. There is a single bond, a double bond, and six lone pairs. 13. If there are four (4) electron pairs around the central atom of a molecule, these electron pairs are in a/n a. trigonal planar b. trigonal pyramidal arrangement. C. octahedral d. tetrahedral 14 The molecular geometry of the molecule NF3 is a. linear b. trigonal pyramidal c. tetrahedral d. trigonal planar 15 Which of the following species will exhibit tetrahedral molecular geometry? d. PCI5 a. CCI4 b. CO2 C. O3arrow_forward
- List the correct electron and molecular geometries that correspond to each set of electron groups around the central atom of a molecule.a. four electron groups overall; three bonding groups and onelone pairb. four electron groups overall; two bonding groups and two lone pairsc. five electron groups overall; four bonding groups and one lone paird. five electron groups overall; three bonding groups and two lone pairse. five electron groups overall; two bonding groups and three lone pairsf. six electron groups overall; five bonding groups and one lone pairg. six electron groups overall; four bonding groups and two lone pairsarrow_forwarda.An s orbital and a p orbital can combine to form molecular orbitals in a couple different ways. Draw a sketch of the overlap between these two atomic orbitals that would produce each of the following molecular orbitals. A. a sigma bonding MO B. a sigma antibonding MO b. For each of the following molecules, make a list of the molecules that are (i) polar, (ii) nonpolar and (iii) ionic. A. NH 3 B. H2 O C. CH3 CH2 CH3 D. NH4 Cl E. Na2 SO 4 F. CH3 Cl G. C6H6OH H. CH3COOH I. LiNO3arrow_forwardWhich of the following descriptions of a sigma bond (according to valence bond theory) is NOT CORRECT? Select one: OA. A sigma bond is formed when two adjacent, parallel p orbitals overlap along their sides. O B. When a sigma bond is formed, a shared electron pair lies on the bond axis of adjacent, bonded atoms. OC. A sigma bond is formed between adjacent atoms when hybrid orbitals, co-linear with the bond axis, overlap. O D. A sigma bond is formed when an s orbital overlaps with a hybrid orbital.arrow_forward
- Which of the following correctly describes a pi bond according to valence bond theory? Select one: O A. A pi bond is formed between adjacent atoms when two p orbitals, co- linear with the bond axis, meet "head on". O B. A pi bond is formed when an s orbital overlaps with a hybrid orbital. O C. A pi bond is formed between adjacent atoms when hybrid orbitals, co- linear with the bond axis, overlap. O D. A pi bond is formed when two adjacent, parallel p orbitals overlap along their sides.arrow_forwardIf an electron is added to H2 it would go into a A. σ*1s molecular orbital and strengthen the H—H bond. B. σ1s molecular orbital and strengthen the H—H bond. C. σ1s molecular orbital and weaken the H—H bond. D. σ*1s molecular orbital and weaken the H—H bond. AND How many molecular orbitals are produced in the valence shell when two fluorine atoms bond to form the F2 molecule?arrow_forwardAccording to the valence bond theory, which kind of orbitals overlap to form the P-Cl bond?arrow_forward
- The central atom of a compound has 4 electron domains. Which of the following statement is FALSE. a. Its molecular geometry can be tetrahedral, trigonal pyramidal, or bent. b. Its electron-pair geometry can be tetrahedral or linear c. It contains sp hybrid orbitals. d. Its molecular geometry is the same with its electron-pair geometry when there is no lone pair of electrons.arrow_forward24. This is a type of covalent bond in carbon which has the greatest bond energy. A. Triple bond B. Double bond C. Single bond D. Pi bond 25. It is a molecular orbital which exhibits symmetry along the internuclear axis. A. Sigma orbitals B. Bonding orbitals C. Antibonding orbitals D. Piorbitalsarrow_forwardWhich of the following correctly describes a pi bond according to valence bond theory? Select one: O A. A pi bond is formed between adjacent atoms when two p orbitals, co- linear with the bond axis, meet "head on". OB. A pi bond is formed when an s orbital overlaps with a hybrid orbital. OC. A pi bond is formed between adjacent atoms when hybrid orbitals, co- linear with the bond axis, overlap. OD. A pi bond is formed when two adjacent, parallel p orbitals overlap along their sides.arrow_forward
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