Organic Chemistry (6th Edition)
6th Edition
ISBN: 9781260119107
Author: Janice Gorzynski Smith
Publisher: McGraw Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 1, Problem 88P
Interpretation Introduction
(a)
Interpretation: The curved arrows that show the movement of electrons in step [1] are to be added.
Concept introduction: In the representation of a
Interpretation Introduction
(b)
Interpretation: The curved arrows that helps in the identification of structure X in the given reaction are to be drawn and the conversion of structure X into phenol and HCl is to be shown in step [3].
Concept introduction: In the representation of a chemical reaction, the movement of electrons is shown by the curved arrows. This method shows the movement of electrons of electrons in resonance structures as well.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Consider lisinopril, a drug used primarily in the treatment of high blood pressure, heart failure, and after heart attacks.
(a) Complete the Lewis structure of lisinopril, showing all valence electrons.
(b) Use the valence-shell electron-pair repulsion (VSEPR) model (Section 3.10) to predict all bond angles in lisinopril.
(c) Which is the most polar bond in lisinopril?
(d) Is lisinopril polar or nonpolar?
(e) Is lisinopril expected to possess resonance (Section 3.9)? Explain why or why not.
(f) Name the various functional groups in lisinopril.
(g) What is the molecular formula of lisinopril?
(h) What intermolecular forces are expected to exist between molecules of lisinopril in close proximity to one another (Section 5.7)?
1.- Answer the following questions:
(a) What is electronegativity?
(b) How is electronegativity measured numerically? Name the scale used and the range of values in the scale.
(c) Explain how electronegativity differences between atoms result in nonpolar covalent bonds and polar covalent bonds. Make sure you explain the difference between nonpolar covalent and polar covalent bonds as it relates to the electronegativity of the participating atoms.
answer true or flase. don't need an explanation or solution
(a) A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9.
(b) If the difference in electronegativity between two atoms is zero (they have identical electronegativ- ities), then the two atoms will not form a covalent bond.
(c) A covalent bond formed by sharing two electrons is called a double bond.
(d) In the hydrogen molecule (H2), the shared pair of electrons completes the valence shell of each hydrogen.
(e) In the molecule CH4 , each hydrogen has an electron configuration like that of helium and carbon has an electron configuration like that of neon.
(f) In a polar covalent bond, the more electronegative atom has a partial negative charge (2) and the less electronegative atom has a partial positive charge (1).
(g) These bonds are arranged in order of increasing polarity CiH , NiH , OiH.
(h) These bonds are arranged in order of increasing polarity HiF , HiCl , HiBr. (
i) A…
Chapter 1 Solutions
Organic Chemistry (6th Edition)
Ch. 1.1 - While the most common isotope of nitrogen has a...Ch. 1.2 - Label each bond in the following compounds as...Ch. 1.3 - Draw a valid Lewis structure for each species. a....Ch. 1.3 - Prob. 9PCh. 1.4 - Draw Lewis structures for each molecular formula....Ch. 1.6 - Classify each pair of compounds as isomers or...Ch. 1.6 - Prob. 12PCh. 1.6 - Prob. 13PCh. 1.6 - Prob. 14PCh. 1.6 - Prob. 16P
Ch. 1.6 - Prob. 17PCh. 1.7 - Prob. 18PCh. 1.7 - Prob. 19PCh. 1.7 - Using the principles of VSEPR theory, you can...Ch. 1.8 - Convert each condensed formula to a Lewis...Ch. 1.8 - Prob. 22PCh. 1.8 - Prob. 23PCh. 1.8 - Convert each skeletal structure to a complete...Ch. 1 - Citric acid is responsible for the tartness of...Ch. 1 - Zingerone gives ginger its pungent taste. a.What...Ch. 1 - Assign formal charges to each and atom in the...Ch. 1 - Prob. 44PCh. 1 - Prob. 46PCh. 1 - Draw all possible isomers for each molecular...Ch. 1 - 1.45 Draw Lewis structures for the nine isomers...Ch. 1 - Prob. 52PCh. 1 - Prob. 53PCh. 1 - Prob. 54PCh. 1 - Consider compounds A-D, which contain both a...Ch. 1 - Draw in all the carbon and hydrogen atoms in each...Ch. 1 - 1.61 Convert each molecule into a skeletal...Ch. 1 - Prob. 65PCh. 1 - Predict the hybridization and geometry around each...Ch. 1 - Prob. 68PCh. 1 - Ketene, , is an unusual organic molecule that has...Ch. 1 - Rank the following bonds in order of increasing...Ch. 1 - Two useful organic compounds that contain Cl atoms...Ch. 1 - Use the symbols + and to indicate the polarity of...Ch. 1 - Prob. 74PCh. 1 - Anacin is an over-the-counter pain reliever that...Ch. 1 - 1.77 Stalevo is the trade name for a medication...Ch. 1 - 1.78 and are two highly reactive carbon...Ch. 1 - 1.79 The N atom in (acetamide) is hybridized,...Ch. 1 - Prob. 83PCh. 1 - Prob. 84PCh. 1 - Prob. 85PCh. 1 - Prob. 86PCh. 1 - Prob. 87PCh. 1 - Prob. 88P
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
- For the polyatomic ion, carbonate, CO32": (A) Draw the Lewis structure of carbonate. (B) How many total valence electrons are there in the polyatomic ion? (C) What is the steric number? (D) Does carbonate have any resonance structures (yes or no)? (E) If carbonate has any resonance structures, draw them on your work sheet. (F) On your work, draw carbonate using perspective drawing (include any lone-pair electrons on the central atom that affect the shape of the molecule; do not include electrons on the surrounding atoms or draw multiple bonds if present). (G) What is the electron geometry? (H) What is the molecule shape? (1) Is carbonate polar or nonpolar?arrow_forwardUsing just a periodic table (not a table of electronegativities), decide which of these is likely to be the most polar bond. Explain your answer! (a) C-F (b) S-F (c) Si-F (d) O-Farrow_forwardConsider compounds A–D, which contain both a heteroatom and a double bond. (a) For which compounds are no additional Lewis structures possible? (b) When two or more Lewis structures can be drawn, draw all additional resonance structures.arrow_forward
- (a) Complete the Lewis structure for vinyl chloride by showing all unshared pairs of electrons. (b) Predict the H-C-H, H-C-C, and Cl-C-H bond angles in this molecule. (c) Does vinyl chloride have polar bonds? Is it a polar molecule? Does it have a dipole?arrow_forward6. a) Using bond dipole arrows, indicate the bond polarity of the bonds in red in the following molecule. b) Using partial charge notation, indicate where the partial charges reside on the atoms in blue. H O=Parrow_forwardConsider the theoretical molecule KrCl3‾. (a) Draw a valid Lewis structure for KrCl3‾. Show all lone pairs and use lines for bonds. Label all non-zeroformal charges on individual atoms and show the overall charge, if it exists, using square brackets.(b) What would you expect to be the molecular geometry for this ion? Fully explain your thought process,including all details about how successive lone pairs should be positioned within this electron geometry.(c) Draw this ion in 3-D, using hashed and wedged bonds as appropriate. Do not worry about labeling the overall or formal charge.arrow_forward
- For the polyatomic ion, carbonate, CO32": (D) Does carbonate have any resonance structures (yes or no)? (E) If carbonate has any resonance structures, draw them on your work sheet. (F) On your work, draw carbonate using perspective drawing (include any lone-pair electrons on the central atom that affect the shape of the molecule; do not include electrons on the surrounding atoms or draw multiple bonds if present). (G) What is the electron geometry? (H) What is the molecule shape? (1) Is carbonate polar or nonpolar?arrow_forwardWhat is the structural diagram of CH2ClF without lone pairs? Also what is its Electronegativity bond after you subtract the smaller from the greater value along with its bond type, total lone pairs of electrons and total bonding pairs of electrons? Lastly, is it polar or non polar (polar molecularity) ?arrow_forward3. Consider the four compounds BB33, CB14, NB13, and Br,O. Use periodic trends in bond lengths and the electronegativity table in Chang to answer the following questions: (a) Which molecule is expected to have the longest bonds? (b) Which molecule is expected to have the most polar bonds? (c) Which molecule is expected to have the least polar bonds?arrow_forward
- 2. Sulfur dioxide, SO,, is a gaseous pollutant that has two resonance structures. Draw both resonance structures below. Include proper resonance notation, lone pairs, and formal charges ... (There is a third resonance structure that involves sulfur hypervalency*, there is no need to include this resonance structure.)arrow_forwardAnswer each of the following questions for ClF3. (a) total valence electron count. (b) the Lewis structure. (c) the arrangement (or shape) of the electron grouping (includes lone pairs). (d) ideal bond angle. (e) actual molecular geometry (may be the same or different than answer (c). (f) actual bond angles (may use > or< symbols where appropriate).arrow_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_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning