Concept explainers
(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
(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.
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Chapter 1 Solutions
CNCT ORG CHEM 6 2020
- 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.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_forwardFor 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_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_forward
- What 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_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_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
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning