Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 2, Problem 9CTQ
Interpretation Introduction
Interpretation : The Lewis structure of carbon dioxide in Model 2 best fit for the experiments indicating that both carbon to oxygen bonds are identical should be discussed.
Concept Introduction : A legitimate Lewis structure is an electron dot and line bond representation in which the total number of valence electrons is indicated. Number of valence electrons around hydrogen is two. Number of valence electrons around carbon, nitrogen, oxygen, fluorine atom is eight. This is called the octet rule.
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The structure at the right is a skeleton of an anion having the overall formula C6H,NO¯. The hydrogen
atoms are not shown.
(a) Draw a complete Lewis structure in which the -1 formal charge is on N. Include all H atoms and
C.
valence electrons.
(b) Do the same for a Lewis structure with the -1 formal charge on O.
(c) Do the same for a Lewis structure with the -1 formal charge on the C atom that is bonded to three other C atoms.
ClO2F2+(a) Draw all of the possible Lewis structures (including reasonance structures) of the following compounds.(b) Label the formal charge for each atom.(c) Determine which resonance structure(s) is(are) the better/best and briefly explain.
Question 5. Finish the questions regarding the molecule/ion in Question 4 above. (a) Draw the best Lewis structure with a three-dimensional fashion by using dash and solid wedges.(b) Name the electron geometry and molecular geometry of the molecules. Identify the bond angles.
Note: For the non-standard bond angels, use “<” or “>” to suggest the deviation of the bond angles from the standard bond angel.
(c) Determine wether the molecule is molecule is polar or non-polar. Briefly explain.
(No:) on
A student proposes the following Lewis structure for the nitronium
ion.
..
0=N=0
Assign a formal charge to each atom in the student's Lewis structure.
atom
formal charge
left O
right O
Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 2 - Prob. 1CTQCh. 2 - The valence shell of an atom in a legitimate Lewis...Ch. 2 - Prob. 3CTQCh. 2 - Prob. 4CTQCh. 2 - Prob. 5CTQCh. 2 - It is impossible to draw a legitimate Lewis...Ch. 2 - Describe how to calculate the total number of...Ch. 2 - Prob. 8CTQCh. 2 - Prob. 9CTQCh. 2 - Prob. 10CTQ
Ch. 2 - Prob. 11CTQCh. 2 - Prob. 12CTQCh. 2 - A complete Lewis structure must show all nonzero...Ch. 2 - Prob. 14CTQCh. 2 - Prob. 15CTQCh. 2 - Prob. 16CTQCh. 2 - Prob. 17CTQCh. 2 - Prob. 18CTQCh. 2 - Complete the rest of the table for N, O or X by...Ch. 2 - Prob. 20CTQCh. 2 - Prob. 21CTQCh. 2 - Make a checklist that can be used to determine if...Ch. 2 - Prob. 2ECh. 2 - Prob. 3ECh. 2 - Draw the Lewis structure of a neutral molecule...Ch. 2 - Prob. 5ECh. 2 - For each element, predict (and draw a Lewis...Ch. 2 - Predict which of the following species is least...Ch. 2 - The molecules BH3 and SF6 and the ion SO42 exist...Ch. 2 - These are NOTlegitimate Lewisstructures (and...Ch. 2 - Fill in missing formal charges where needed (all...Ch. 2 - Below each structure in the previous question is a...Ch. 2 - Prob. 12ECh. 2 - Carbon monoxide (CO) is an example of an overall...Ch. 2 - Explain why this Lewis structure for CO is not as...Ch. 2 - Prob. 15ECh. 2 - Prob. 16ECh. 2 - Prob. 17ECh. 2 - Prob. 18ECh. 2 - Prob. 19E
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- 2. (B) What is wrong with the following Lewis structure? Please explain. H H. H--- C --- C= Cl Harrow_forwardDraw all possible resonance structures for SO2, S0,, and SO. Use the resonance structures to solve the problems below. (a) Arrange these species in order of increasing S-O bond length (shortest bond first). O SO O SO O SO2 O SO2 O so;²- O SO O So3? O SO2 (b) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an S atom and an O atom bonded to this S atom. (Hint: Average the number of bonds between S and an attached oxygen atom in a particular position using all of your resonance structures for the species that you are working on.) SO: -Select-v bonds between S and 0. -Select--- v bonds between S and O. SO2: Select-v bonds between S and O. (c) Match each species with the correct formal charge on the central S atom. SO: Select- charge on S. SO2: Select--v charge on S. SO32:-Select-vcharge on S. (d) Match each species with the average formal charge on an outside oxygen atom predicted by Lewis structures. so: -Select-vaverage charge on…arrow_forwards please answer allarrow_forward
- Calculate the formal charge on each of the atoms in the Lewis structure given. Be sure to answer all parts. H: N: O (of OH): O: Nitrous acidarrow_forward[ 3rd ITEM ] Instructions: Kindly provide complete and correct solution. I won't like it if it is incomplete and incorrect. Please answer some of my questions I've posted here too! I still have tons of questions to postarrow_forwardDecide whether the Lewis structure proposed for each molecule is reasonable or not. Note: If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.arrow_forward
- ent1 - Word Search (Alt+Q) lings Review View Help AaBbCcDd AaBbCcDd AaBbC AaBbCcD 1 Normal 1 No Spac. Heading 1 Heading 2 Paragraph Styles Draw at least two plausible resonance contributors for the nitrite ion (NO2). 2. (b) Assign formal charges to each atom in the resonance structures of the nitrite ion (NO2). ! (c) How many double bonds are present in the experimental (true) structure of the nitrite ion (NO2')? Write one sentence to justify your answer. !!! ilarrow_forwardII. Please expand each of the following bond-line formulas to the corresponding standard Lewis structure, be sure to show all the bonds and unshared electron pairs as well as formal charges, if it applies. 0: (a) (c) O Br | Br-B-Br -N- (b) HO: NO₂ 0: blos ohsup?arrow_forwardGiven the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?arrow_forward
- 3-31 Why does electronegativity generally increase going from left to right across a row of the Periodic Table?arrow_forwardCarbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).arrow_forwardHow come there are two major resonance structure? Wouldn't the structure with the positive charge on the nitrogen be the only major structure, as it is less electronegative than oxygen?arrow_forward
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