s Item 3: Question Unshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs. Use the structural formulas below to determine the number of unshared pairs at each designated atom. Be sure your answers are consistent with the formal charges on the formulas. H H₂C H H₂ Submit b H b st tts, Amherst, MA USA с H Skip to Previous CH3 The number of unshared pairs at atom a is The number of unshared pairs at atom b is The number of unshared pairs at atom c is The number of unshared pairs at atom a is The number of unshared pairs at atom b is The number of unshared pairs at atom c is Submit and Next O: Mark this question for later review. V V V Skip to Next

s Item 3: Question Unshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs. Use the structural formulas below to determine the number of unshared pairs at each designated atom. Be sure your answers are consistent with the formal charges on the formulas. H H₂C H H₂ Submit b H b st tts, Amherst, MA USA с H Skip to Previous CH3 The number of unshared pairs at atom a is The number of unshared pairs at atom b is The number of unshared pairs at atom c is The number of unshared pairs at atom a is The number of unshared pairs at atom b is The number of unshared pairs at atom c is Submit and Next O: Mark this question for later review. V V V Skip to Next

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Specify the local electron geometries about the atoms labelled a-d. Unshared electron pairs affect local geometry and are included in the structural formula. For each atom enter one of the following: tetrahedral, square planar, trigonal planar, trigonal pyramidal, or linear. H H H. H H a C-H H. (а) (b) (c) (d)
Place the following molecular ions in order from smallest tolargest bond order: C22 + , N2-, O2-, and F2-.(a) C22+ 6 N2- 6 O2- 6 F2-(b) F2- 6 O2- 6 N2- 6 C22 +(c) O2- 6 C22 + 6 F2- 6 N2-(d) C22 + 6 F2- 6 O2- 6 N2-(e) F2- 6 C22 + 6 O2- 6 N2-
II. Answer the following items as required. А. (a) overlapping of orbitals (b) bond axis & electron density Hint: s can overlap with p, along the Given set of orbitals (c) sigma or pi 1. s + P, у-аxis 2. P, + dx²-y? Hint: the two orbitals can overlap along the x axis. 3. py + dxy
A) Explain why BrF4 with a negative charge on top is square planar, whereas BF4 with negative charge on top is tetrahedral? B) How could you expect H_X_H bond to vary in the series H2O , H2Se? Explain your answer
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Specify the local electron geometries about the atoms labelled a-d. Unshared electron pairs affect local geometry and are included in the structural formula. For each atom enter one of the following: tetrahedral, square planar, trigonal planar, trigonal pyramidal, or linear. (a) (b) (c) (d) HH H
23. Given AH+ [(NF3(g)] = -132 kJ mol-¹ and the bond enthalpy (D) data, D(N₂) = 946 kJ mol-¹ and D(F2) = 159 kJ mol-, which of the following statements is/are FALSE? The average N-F bond enthalpy in NF3 is 281 kJ mol-¹. AH+ [(NF3(g)] > AH+ [(NF3(1)] AH+ [(F(8)] = 159 kJ mol-¹ CEE
Consider the valence bond description of the covalent bonding in N2H2.(a) Draw the Lewis structure for N2H2. [3 pts](b) Identify the hybridization scheme for the two N atoms. [3 pts](c) Using the same techniques shown in class, sketch the valence bond model for N2H2
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