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- < Complete the following structural formula for a neutral molecule by adding H atoms to complete the valence of each atom. Do not introduce any double or triple bonds. Then complete the Lewis diagram by adding any unshared electron pairs needed, so that each atom except H has a complete octet. [Review Topics] [References] Use the References to access important values if needed for this question. Br Br C—C— Write the molecular formula in the order CHX, where X stands for Cl or Br. Submit Answer The number of unshared pairs in the Lewis diagram unshared pair(s). Retry Entire Group 9 more group attempts remaining Previous Email Instructor Next Save and EState whether each of these statements is true or false. (a)A carbon–carbon triple bond is shorter than a carbon–carbonsingle bond. (b) There are exactly six bonding electrons inthe O2 molecule. (c) The C—O bond in carbon monoxide islonger than the C—O bond in carbon dioxide. (d) The O—Obond in ozone is shorter than the O—O bond in O2. (e) Themore electronegative the atom, the more bonds it makes toother atoms.(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?
- Refer to the structure given below and answer the given questions: CI 18 H 5 13 1 10 15 16 17 19 2 12 14 9 11 20 1 6 ОН О 2 8. 5 Red numbers for Carbon Blue numbers for Nitrogen Green numbers for Oxygen (1) What is the Molecular Formula of the given structure? (2) Which bond is the most polar (specify number if pertaining to C,N, or O) Provide your calculation for the electronegativity difference which was the basis for your answer. (3) What is the total number of lone pairs present in the structure? 6.The partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one?Fill in the blank with the appropriate numbers for bothelectrons and bonds (considering that single bonds arecounted as one, double bonds as two, and triple bonds asthree).(a) Fluorine has valence electrons and makesbond(s) in compounds.(b) Oxygen has valence electrons and makesbond(s) in compounds.(c) Nitrogen has valence electrons and makesbond(s) in compounds.(d) Carbon has valence electrons and makesbond(s) in compounds.
- Consider 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.The partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one? [Sections 8.3and 8.8]Which of these statements correctly describes the relationship between the displayed molecules? -Only one of these represents a valid Lewis Structure -They do not have the same molecular formula -They are isomers -They are the same molecule
- 22. Draw the Lewis diagram for each molecule. C (a) water, H,O (b) carbon dioxide, CO2 (c) ethane, C,H,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)?Which of the following Lewis dot structures is a valid Lewis structure? H +YF H H-P None of these : Si= CI are H- H. plausible/valid. H. :F: H