Organic Chemistry-Package(Custom)
4th Edition
ISBN: 9781259141089
Author: SMITH
Publisher: MCG
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Textbook Question
Chapter 1, Problem 1.77P
Label the polar bonds in each molecule. Indicate the direction of the net dipole (if there is one).
a.
e. f.
b.
c.
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Label the polar bonds in each molecule, and then decide if the molecule is polar or nonpolar. a. HCl b. C 2H 6 c. CH 2F 2 d. HCN e. CCl 4
8. For each molecular fomula, detem ine the electron pair geom etry (EPG), make a 3-dimensional
representation, and determ ine the molecular geometry. Determine whether the molecule is polar or non-
polar. All of these have central atoms surounded by term inal atom s/one pairs only.
Formula
A. CHF3
Lewis structure
EPG
3-D drawing
Mol Geom.
Polar molecule?
B. SF2
1. Draw the complete Lewis Structure for each. Then determine the electron pair geometry (EPG), make a
3-dimensional representation (drawing), and determine the molecular geometry (MG) for all of them.
Determine whether each molecule is polar or non-polar.
Formula
Lewis structure
EPG
3-D drawing
MG
polar?
a. PF3
b. CH;F2
Cl3
d. SC4
e. XeF4
Chapter 1 Solutions
Organic Chemistry-Package(Custom)
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
- a Carbonyl fluoride, COF2, is an extremely poisonous gas used in organofluorine synthesis. Give the valence bond description of the carbonyl fluoride molecule. (Both fluorine atoms are attached to the carbon atom.) b Nitrogen, N2, makes up about 80% of the earths atmosphere. Give the valence bond description of this molecule.arrow_forwardDraw a valid Lewis structure for each molecule. a. HI b. CH 2F 2 c. H 2Se d. C 2Cl 6arrow_forward4. CHCl3 a. Lewis structure Electronic geometry_ C. d. Molecular shape_ e. Bond angle? b. Draw the different bonds and label their polarity. inorpelt b Soigns broff 02 8arrow_forward
- 16.0 g of a lead containg sample was dissolved water and an excess of sodium sulfate was added to this solution. The mass of lead (II) sulfate (PbSO4) that precipitated was 308.88 mg. Determine the mass percent of lead present in the sample? 1.51% 1.32% 1.06% 1.76% 1.17%arrow_forwardMolecular Geometry 1. NCl₃ 2. CCl2F2 3. CH2F2 4. CH2O 5. HNCarrow_forwardo=c=0 ö-s=ö 10. Lewis electron dot diagrams for CO2 and SO2 are given above. Which of the following is true regarding the molecular geometry and the polarity for both substances? A. they are both linear because they only have two non-central atoms B. they are both polar molecules due to the polar bonds between the central atom and oxygen C. the lone pair of electrons on the S atom in SO, make it a polar bent molecule D. they are both nonpolar because the formal charge on each atom is zero 150 to 140 130arrow_forward
- 1) What is the type of molecule? a. AX2E3 b. AX3E2 c. AX5 d. AX2E2 2) What is the molecular geometry of GL2-? a. Linear b. Trigonal Bypyramidal c. Bent or v-shaped d. Seesaw 3) What is the approx bond angle formed by L-G-L bond if the correct molecular geometry is followed? a. 180° b. 120° c. 109.5° d. 90° 4) Considering that L is more electronegative than G, and the en difference is 0.2, is the molecular polar? 5) What is the formal charge of G? 6) What is the formal charge of the labeled atom? (refer to the blue arrow)arrow_forward2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule before identifying the shape of the molecule? 3. Draw the Lewis structure of ozone, O3. Describe why ozone has a bent shape instead of a linear shape.arrow_forwardProvide the lewis structure and the 3D structure and the polarity of the moleculesarrow_forward
- Which bond is most polar? ОА. О—Н O B. F-H O C. N-H O D. C H IIarrow_forward5. SO42- a. Lewis structure c. Electronic geometry_ d. Molecular shape_ e. Bond angle? b. Draw the different bonds and label their polarity. qaria salupolulMarrow_forwardIndicate whether each of the following molecules is polar or nonpolar. The molecular geometry is given in parentheses. a. PH2Cl (trigonal pyramidal with P at the apex) b.SO3 (trigonal planar with S in the center position) c.CH2Cl2 (tetrahedral with C in the center position) d.CCl4 (tetrahedral with C in the center position)arrow_forward
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