Organic Chemistry
4th Edition
ISBN: 9780073402772
Author: Janice G. Smith
Publisher: MCG
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Textbook Question
Chapter 1, Problem 1.42P
Assign formal charges to each N and O atom in the given molecules. All lone pairs have been drawn in.
a.
b.
C.
d.
e.
f.
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The element sulphur has atomic number 16. Sulphur forms a molecular compound with chloride witha molecular formula SCl2. The atomic number of chlorine is 17.i. Write down the electronic configuration of a sulphur atom and a chlorine atom.ii. Draw a Lewis structure of an SCl2 molecule, by showing the electrons in the outer shells of theatoms.iii. State how many bond pairs and lone pairs of electrons are arranged around the sulphur atomsin SCl2 molecule.iv. Sketch the shape and state the molecular geometry of SCl2 molecule.v. Explain the hybridisation of the central atom in SCl2 molecule.vi. Explain the intermolecular forces exists in SCl2 molecule
A. CHF
i. Best Lewis Structure
B. HNO (H is connected to one of the O's)
i. Best Lewis Structure
ii. Electron geometry on the C atom
ii. Electron geometry on the N atom
iii. Approximate bond angles about the C atom
iii. Approximate bond angles around the N atom
v. Draw the shape with in and out wedges (as necessary) and
dipole arrows around the C atom.
v. Draw the shape with in and out wedges (as necessary) and
dipole arrows around the N atom.
vi. Is the molecule polar or nonpolar?
vi. Is the molecule polar or nonpolar?
d. H E
Assign formal charges to each carbon atom in the given species. All lone pairs have been drawn in.
H H
a. CH2-CH
b. H-C-H
c. H-C-H
нн
Chapter 1 Solutions
Organic Chemistry
Ch. 1 - While the most common isotope of nitrogen has a...Ch. 1 - Label each bond in the following compounds as...Ch. 1 - How many covalent bonds are predicted for each...Ch. 1 - Draw a valid Lewis structure for each species. a....Ch. 1 - Draw an acceptable Lewis structure for each...Ch. 1 - Prob. 1.6PCh. 1 - Draw a Lewis structure for each ion. a. CH3Ob....Ch. 1 - Draw Lewis structures for each molecular formula....Ch. 1 - Prob. 1.9PCh. 1 - Prob. 1.10P
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Draw a second resonance structure for each...Ch. 1 - Prob. 1.14PCh. 1 - Draw a second resonance structure for nitrous...Ch. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Prob. 1.19PCh. 1 - Prob. 1.20PCh. 1 - Simplify each condensed structure by using...Ch. 1 - Prob. 1.22PCh. 1 - Prob. 1.23PCh. 1 - Convert each skeletal structure to a complete...Ch. 1 - Draw in all hydrogens and lone pairs on the...Ch. 1 - Prob. 1.26PCh. 1 - What orbitals are used to form each of the CC, and...Ch. 1 - What orbitals are used to form each bond in the...Ch. 1 - Determine the hybridization around the highlighted...Ch. 1 - Classify each bond in the following molecules as ...Ch. 1 - Prob. 1.31PCh. 1 - Rank the following atoms in order of increasing...Ch. 1 - Prob. 1.33PCh. 1 - Prob. 1.34PCh. 1 - Provide the following information about...Ch. 1 - Use the ball-and-stick model to answer each...Ch. 1 - Citric acid is responsible for the tartness of...Ch. 1 - Zingerone gives ginger its pungent taste. a.What...Ch. 1 - Two radioactive isotopes of iodine used for the...Ch. 1 - Prob. 1.40PCh. 1 - Assign formal charges to each carbon atom in the...Ch. 1 - Assign formal charges to each N and O atom in the...Ch. 1 - Draw one valid Lewis structure for each compound....Ch. 1 - Prob. 1.44PCh. 1 - Prob. 1.45PCh. 1 - Prob. 1.46PCh. 1 - Draw all possible isomers for each molecular...Ch. 1 - 1.45 Draw Lewis structures for the nine isomers...Ch. 1 - Prob. 1.49PCh. 1 - Prob. 1.50PCh. 1 - Prob. 1.51PCh. 1 - Prob. 1.52PCh. 1 - Prob. 1.53PCh. 1 - Prob. 1.54PCh. 1 - Draw all reasonable resonance structures for each...Ch. 1 - Prob. 1.56PCh. 1 - Rank the resonance structures in each group in...Ch. 1 - 1.56 Consider the compounds and ions with curved...Ch. 1 - 1.57 Predict all bond angles in each...Ch. 1 - Predict the geometry around each indicated atom....Ch. 1 - Prob. 1.61PCh. 1 - Prob. 1.62PCh. 1 - Draw in all the carbon and hydrogen atoms in each...Ch. 1 - Prob. 1.64PCh. 1 - Prob. 1.65PCh. 1 - Prob. 1.66PCh. 1 - Prob. 1.67PCh. 1 - Each of the following condensed or skeletal...Ch. 1 - Prob. 1.69PCh. 1 - Prob. 1.70PCh. 1 - Prob. 1.71PCh. 1 - Prob. 1.72PCh. 1 - Prob. 1.73PCh. 1 - Prob. 1.74PCh. 1 - Two useful organic compounds that contain Cl atoms...Ch. 1 - Use the symbols + and to indicate the polarity of...Ch. 1 - Label the polar bonds in each molecule. Indicate...Ch. 1 - Answer the following questions about acetonitrile...Ch. 1 - Prob. 1.79PCh. 1 - The principles of this chapter can be applied to...Ch. 1 -
a. What is the hybridization of each N atom in...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. 1.85PCh. 1 - Prob. 1.86PCh. 1 - Prob. 1.87PCh. 1 - Prob. 1.88PCh. 1 - Prob. 1.89PCh. 1 - Prob. 1.90P
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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
- In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.arrow_forwardDecide whether the proposed Lewis structure below is reasonable. proposed Lewis structure Is this a reasonable structure? H. Ves H. O No H. H. H. O Yes O No H. H. H. O Yes ONo H. H. H. Yes H. O No H. H. H.arrow_forwardTo answer the questions, interpret the following Lewis diagram for SO42- . 1. For the central sulfur atom: ... The number of non-bonding electrons = The number of bonding electrons = The total number of electrons = 2. The central sulfur atom fill in the blank 4 ... A. obeys the octet rule. B. has more than an octet. C. has less than an octet.arrow_forward
- Draw in all the hydrogen atoms and nonbonded electron pairs in each ion. a. b. d. ENHarrow_forward9. Indicate whether each statement below is true or false. a. The core electrons are called valence electrons. b. lonic bonds are formed by the attraction between cations and anions. c. Ionic bonds are formed from atoms by a transfer of electrons. d. In a Lewis symbol, the chemical symbol represents the nucleus of the atom. e. An ion written as a Lewis symbol has brackets outside the electrons. f. Two electrons involved in a bond produce a double bond. g. If the AEN value is very large the bond is polar covalent. h. The central atom is typically the atom with the highest electronegativity. i. An expanded octet has larger electron clouds. j. A nonpolar molecule can have polar bonds.arrow_forwardDraw a Lewis structure for SO2 that obeys the octet rule if possible and answer the following questions based on your drawing. 1. For the central sulfur atom: - The number of lone pairs = ? - The number of single bonds = ? - The number of double bonds = ? 2. The central sulfur atom a. obeys the octet rule. b. has an incomplete octet. c. has an expanded octet.arrow_forward
- The element sulphur has atomic number 16. Sulphur forms a molecular compound with chloride with a molecular formula SCl2. The atomic number of chlorine is 17. a. Write down the electronic configuration of a sulphur atom and a chlorine atom. b. Draw a Lewis structure of an SCl2 molecule, by showing the electrons in the outer shells of the atoms. c. State how many bond pairs and lone pairs of electrons are arranged around the sulphur atoms in SCl2 molecule. d. Sketch the shape and state the molecular geometry of SCl2 molecule. e. Explain the hybridisation of the central atom in SCl2 molecule. f.Explain the intermolecular forces exists in SCl2 molecule.arrow_forward9. Indicate whether each statement below is true or false. d. In a Lewis symbol, the chemical symbol represents the nucleus of the atom. e. An ion written as a Lewis symbol has brackets outside the electrons. f. Two electrons involved in a bond produce a double bond.arrow_forwardDecide whether the proposed Lewis structure below is reasonable. proposed Lewis structure Is this a reasonable structure? O Yes O No H. H. H. OYes O No H. H. Yes H. O No H. H. H. H. H. O No H. H. HICarrow_forward
- Draw a reasonable Lewis structure for each of the following formulas. a. H2S b. CHBr3 c. NF3 d. Br2O e. H2CO3 f. H2S2 g. HOCl h. BBr3 i. CH3CH2CHCH2arrow_forwardCarbon ring structures are common in organic chemistry. Draw a Lewis structure for each carbon ring structure, including any necessary resonance structures. a. CHg b. CH4 c. CH12 d. C,H.arrow_forwardNow, illustrate the various bond combinations each element can form. Refer to Carbon for the example. Take note that one bond is represented by a line. Nitrogen 3 single b. 1 single, 1 double c. 1 triple Oxygen 2 single b. 1 double Carbon 4 single a. а. а. b. 2 double c. 2 single & 1 double d. 1 single & 1 triple а. a. 4 single bonds а. -C b. b. b.arrow_forward
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