Organic Chemistry
12th Edition
ISBN: 9781118875766
Author: T. W. Graham Solomons, Craig B. Fryhle, Scott A. Snyder
Publisher: WILEY
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Textbook Question
Chapter 1, Problem 32P
Add any unshared electrons to give each element an octet in its valence shell in the formulas below and indicate any formal charges. Note that all of the hydrogen atoms that are attached to heteroatoms have been drawn if they are present.
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Draw the Lewis structures for the following four molecules, being sure to show all steps following the methods covered in class. Structures without work shown will be marked incorrect. Also, one of these molecules has resonance structures – for this compound, make sure to include all resonance structures, indicate formal charges for each atom.
SO2 OF2 IF3 NH4+
Consider a molecule where the central atom has one lone pair of electrons and is double-bonded to two other atoms (of a different element). Draw a general diagram of the molecule. Is this molecule likely a polar or nonpolar molecule? Briefly explain your reasoning, using words and the diagram.
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Match the words in the left column to the appropriate blanks in the sentences on the right.
minus
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the number of
plus
lone pair electrons and
the number of bonding electrons. The formal charge is equal to
the number of valence electrons because there are
bonds.
one-half
two times
no
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Chapter 1 Solutions
Organic Chemistry
Ch. 1 - Prob. 1PPCh. 1 - Prob. 2PPCh. 1 - Prob. 3PPCh. 1 - Prob. 4PPCh. 1 - Prob. 5PPCh. 1 - Prob. 6PPCh. 1 - Prob. 7PPCh. 1 - Prob. 8PPCh. 1 - Prob. 9PPCh. 1 - Prob. 10PP
Ch. 1 - Prob. 11PPCh. 1 - Prob. 12PPCh. 1 - Prob. 13PPCh. 1 - Prob. 14PPCh. 1 - Prob. 15PPCh. 1 - Prob. 16PPCh. 1 - Prob. 17PPCh. 1 - Prob. 18PPCh. 1 - Prob. 19PPCh. 1 - Prob. 20PPCh. 1 - Prob. 21PPCh. 1 - Practice Problem 1.22 Which of the following...Ch. 1 - Prob. 23PPCh. 1 - Prob. 24PPCh. 1 - Practice Problem 1.25
What do the bond angles of...Ch. 1 - Prob. 26PPCh. 1 - Practice Problem 1.27
Use VSEPR theory to predict...Ch. 1 - Practice Problem 1.28 Predict the bond angles of...Ch. 1 - 1.29 Which of the following ions possess the...Ch. 1 - 1.30 Write a Lewis structure for each of the...Ch. 1 - Prob. 31PCh. 1 - Add any unshared electrons to give each element an...Ch. 1 - Prob. 33PCh. 1 - What is the molecular formula for each of the...Ch. 1 - Prob. 35PCh. 1 - Prob. 36PCh. 1 - 1.37 Write bond-line formulas for all of the...Ch. 1 - Prob. 38PCh. 1 - Prob. 39PCh. 1 - Prob. 40PCh. 1 - Prob. 41PCh. 1 - (a) Cyanic acid (HOCN) and isocyanic acid (HN=C=O)...Ch. 1 - Consider a chemical species (either a molecule or...Ch. 1 - 1.44 Consider a chemical species like the one in...Ch. 1 - 1.45 Consider another chemical species like the...Ch. 1 - Draw a three-dimensional orbital representation...Ch. 1 - Ozone (O3) is found in the upper atmosphere where...Ch. 1 - Write resonance structures for the azide ion, N3....Ch. 1 - Write structural formulas of the type indicated:...Ch. 1 - Prob. 50PCh. 1 - 1.51 In Chapter 15 we shall learn how the...Ch. 1 - Prob. 52PCh. 1 - (a) Consider a carbon atom in its ground state....Ch. 1 - Open computer molecular models for dimethyl ether,...Ch. 1 - Boron is a group IIIA element. Open the molecular...Ch. 1 - 1.56 There are two contributing resonance...Ch. 1 - Prob. 1LGPCh. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Prob. 7LGPCh. 1 - Prob. 8LGP
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- Part C Cio Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons. Show the formal charges of all atoms in the correct structure. To change the symbol of an atom, double-click on the atom, and enter the letter of the new atom.arrow_forwardFormal charge is (select all that are true) equal to the number of valence electrons minus half the number of bonding electrons minus the number of nonbonding electrons. equal to number of valence electrons minus number of bonds minus number of nonbonding electrons. the difference between the number of valence electrons of each atom and the number of electrons the atom is associated with. the charge assigned to an atom in a molecule.arrow_forwardDraw the Lewis structures for the following four molecules, being sure to show all steps following the methods covered in class. Structures without work shown will be marked incorrect. Also, one of these molecules has resonance structures – for this compound, make sure to include all resonance structures, indicate formal charges for each atom. SO2 OF2 IF3 NH4+arrow_forward
- Unshared, or lone, electron pairs play an important role in determining the chemical and phy 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 Be sure your answers are consistent with the formal charges on the formulas. 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 ALI H-A-H bH 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 isarrow_forwardQuestion: Consider a hypothetical molecule, X₄Y₃, composed of four atoms of element X and three atoms of element Y. The molecule is in a gaseous state. a) According to the octet rule, which elements are likely to form multiple bonds in this molecule? Explain your reasoning. b) Calculate the total number of valence electrons in X₄Y₃. c) Based on the total number of valence electrons, determine the formal charge on each atom in X₄Y₃.arrow_forwardWrite a Lewis structure for each of the following molecules that are exceptions to the octet rule. ClO2 Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons and nonbonding electrons. Do not include charges.arrow_forward
- Assign formal charges to each N and O atom in the given molecules. All lone pairs have been drawn in.arrow_forwardParaphrasing .ewriting Tool Car note Pirate Ship BLACKBOARD [Review Toplcs) [References) 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. The number of unshared pairs at atom a is 0 0 b c CH,-CH2-0-H a The number of unshared pairs at atom b is 3 0. The number of unshared pairs at atom c is o e. The number of unshared pairs at atom a is The number of unshared pairs at atom b is „CH2 The number of unshared pairs at atom c is Submit Answer Retry Entire Group 9 more group attempts remaining (Previous Next> FE 1 18 étv S ali Z W MacBook Air DII 888 F10 FO F3 F4 & dele 4 6. 8 { P R Y F G J K L V M command option Barrow_forwardPlease refer to the example image to answer. You must use CER, claim-evidence-reasoning. Make sure that your answer is CLEAR and explained well. Claim is your answer to the question. Evidence is from the image and reasoning is your explanation. Proper evidence for all Lewis structures include: Most electronegative atom must be in the center. Octet of electrons surrounding each atom. Total number of electrons depicted equals same total number of valence electrons from each participating atom. Make sure to refer to the example image because it shows the correct Lewis structures. The question you're answering is about the students drawing of CH20.arrow_forward
- Draw the Lewis structure created by the curved arrow. Write in formal charges wherever they are not equal to zero. H-N=c-H H-N=C-Harrow_forward(True/False) The summation of the formal charges of the atoms in a compound/ polyatomic ion is equal to the charge of the whole compound/ polyatomic ion.arrow_forwardquestion. Then draw two resonance structures for ozone, O3. The structures must show all nonbonding electron pairs and must show each nonzero formal charge on the atom with that charge.arrow_forward
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