Organic Chemistry
9th Edition
ISBN: 9781305080485
Author: John E. McMurry
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 2.1, Problem 3P
Use the electronegativity values shown in Figure 2-2 to rank the following bonds from least polar to most polar: H3C-Li, H3C-K, H3C-F, H3C-MgBr, H3C-OH
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Draw the resonance structure indicated by the curved arrows. Assign formal charges.
H
H/:O:
H
H-C-C-C-Ċ—H
H H
H
Draw the molecule by placing atoms on the canvas and connecting them with bonds. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of
all atoms in the correct structure.
For each full Lewis structure in question 4, draw a bond-line structure.
H H
a)
H-C-N-H
b)
H-N-C-N-H
H.
H H
O-C-C-N-H
c)
d) H-C-C-C-H
H-C-H
HICIH
HINIH
HICICIH
Directions: Complete the data table below. It is not necessary to construct any models.
Number of bonds &
number of lone pairs
around central atom
Chemical
Valence
electrons
name
Formula
Lewis structure
NCI,
N-5
3 bonds
Nitrogen
CI- 7(3)
20 lone pairs
trichloride
Si-4
S-6(2)
Sis,
Silicon
disulfide
Н-1
C- 4
HCN
N-5
C-4
CF,CI,
F-7(2)
CI-7(2)
Ge-4
Germane
GeH,
H-1(4)
C-4
CSF,
S-6
F-7(2)
Selenium
Se-6
dichloride
SeCl,
CI-7(2)
AsF,
As-5
F-7(3)
arsenic
trifluoride
C-4(2)
Br-7(2)
Dibromoacetylene
chlorine gas
Cl:
CI-7(2)
dihydrogen
monoxide
DHMO
CH,O
C-4
H-1(2)
O-6
carbon
CF,
C-4
tetrafluoride
F-7(4)
Chapter 2 Solutions
Organic Chemistry
Ch. 2.1 - Prob. 1PCh. 2.1 - Prob. 2PCh. 2.1 - Use the electronegativity values shown in Figure...Ch. 2.1 - Look at the following electrostatic potential map...Ch. 2.2 - Ethylene glycol, HOCH2CH2OH, may look nonpolar...Ch. 2.2 - Make three-dimensional drawings of the following...Ch. 2.3 - Calculate formal charges for the nonhydrogen atoms...Ch. 2.3 - Organic phosphate groups occur commonly in...Ch. 2.6 - Which of the following pairs of structures...Ch. 2.6 - Draw the indicated number of resonance forms for...
Ch. 2.7 - Nitric acid (HNO3) reacts with ammonia (NH3) to...Ch. 2.8 - Prob. 12PCh. 2.8 - Amide ion, H2N-, is a much stronger base than...Ch. 2.9 - Prob. 14PCh. 2.9 - Prob. 15PCh. 2.9 - Prob. 16PCh. 2.11 - Using curved arrows, show how the species in part...Ch. 2.11 - Prob. 18PCh. 2.12 - Of the two vitamins A and C, one is hydrophilic...Ch. 2.SE - Prob. 20VCCh. 2.SE - The following model is a representation of...Ch. 2.SE - cis-l, 2-Dichloroethylene and trans-1,...Ch. 2.SE - The following molecular models are representations...Ch. 2.SE - Predict the product(s) of the acid/base reactions...Ch. 2.SE - Use curved arrows to draw the protonated form of...Ch. 2.SE - Prob. 26MPCh. 2.SE - Double bonds can also act like Lewis bases,...Ch. 2.SE - Prob. 28APCh. 2.SE - Use the electronegativity table given in Figure...Ch. 2.SE - Which of the following molecules has a dipole...Ch. 2.SE - Prob. 31APCh. 2.SE - Phosgene, C12C=O, has a smaller dipole moment than...Ch. 2.SE - Prob. 33APCh. 2.SE - Methanethiol, CH3SH, has a substantial dipole...Ch. 2.SE - Calculate the formal charges on the atoms shown in...Ch. 2.SE - Assign formal charges to the atoms in each of the...Ch. 2.SE - Which of the following pairs of structures...Ch. 2.SE - Prob. 38APCh. 2.SE - 1, 3-Cyclobutadiene is a rectangular molecule with...Ch. 2.SE - Alcohols can act either as weak acids or as weak...Ch. 2.SE - The O-H hydrogen in acetic acid is more acidic...Ch. 2.SE - Draw electron-dot structures for the following...Ch. 2.SE - Write the products of the following acid-base...Ch. 2.SE - Rank the following substances in order of...Ch. 2.SE - Which, if any, of the substances in Problem 2-44...Ch. 2.SE - The ammonium ion (NH4+, pKa = 9.25) has a lower...Ch. 2.SE - Prob. 47APCh. 2.SE - Prob. 48APCh. 2.SE - Calculate Ka values from the following pka’s:...Ch. 2.SE - Calculate pKa values from the following Ka’s:...Ch. 2.SE - What is the pH of a 0.050 M solution of formic...Ch. 2.SE - Prob. 52APCh. 2.SE - Maleic acid has a dipole moment, but the closely...Ch. 2.SE - Assume that you have two unlabeled bottles, one of...Ch. 2.SE - Identify the acids and bases in the following...Ch. 2.SE - Which of the following pairs represent resonance...Ch. 2.SE - Draw as many resonance structures as you can for...Ch. 2.SE - Carbocations, which contain a trivalent,...Ch. 2.SE - We’ll see in the next chapter that organic...Ch. 2.SE - The azide functional group, which occurs in...Ch. 2.SE - Phenol, C6H5OH, is a stronger acid than methanol,...Ch. 2.SE - Thiamin diphosphate (TPP), a derivative of vitamin...Ch. 2.SE - Determine if each compound or ion below has a...Ch. 2.SE - Prob. 64APCh. 2.SE - Prob. 65APCh. 2.SE - Draw the conjugate base for each compound below...Ch. 2.SE - 1, 1, 1-Trichloroethanol is an acid more than 1000...
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
- Figure A. B. C. CH₂ 시-10 -Ö: Î 0-17 0: :0:arrow_forward1) Classify each bond below as ionic, non-polar covalent, or polar covalent. For the polar covalent compounds, indicate the direction of the dipole. Na-Br H-CI H3C-CH,CH, H,CO-H Br-Br H-OH H,C-CF, H-CH, F-CI H,C-OH Br-Mg -Br Li-CH,CH3 2) Determine the formal charge on each of the bold atoms below. Lone pairs have been drawn in for you. Hc- ー4 H,C-cEc: Hy .C H,C CH, Hc-C OH2 H. 3) Determine the formal charge on each of the bold atoms below. You must draw in lone pairs as appropriate. H C=CH HC CH N. H. HC PH H,C CH H,C H CH, H.arrow_forwardBased on the atom connectivity shown bellow,evaluate the four resonance structure for the thiosulfate ion S2O3 ^2-. Use curved arrows to indicate how you get from one resonance structure to another. Assign formal changes to all atoms and determine which of these resonance structure is the most stable based on a formal charge analysis Explain your answer thoroughly. Look at the picture.arrow_forward
- 4. The following are valid Lewis structures for CH3SOCH3. Label the formal charges and circle the best Lewis structure. H :ö: H H :0 H a) H-C=S-C-H b) Н—С—S— С-н H. H. H. H. Н :0: Н H :ö: H d) H-C=$-C-H c) Н—С—$—С-н H. H. H Harrow_forwardDraw the Lewis structure created by the curved arrow. Write in formal charges wherever they are not equal to zero. H + IH Η HIN Η H Click and drag to start drawing a structure. CT Xarrow_forwardArrange the following bonds from the least polar to the most polar bond: N-O, Ca-O, Si-O, O-O What information do I need to arrange the bonds from the least polar to the most polar bond?arrow_forward
- Calculating Formal Charge: Formal charge is calculated for each atom in a structure. It provides information about the stability and reactivity of the atom in the molecule. Formal Charge = Valence Electrons - 1/2 Bonding Electrons - Non-bonding Electrons For example, the formal charge on the carbon of methane is calculated here. Carbon has 4 valence electrons. There are 8 bonding electrons around it. Formal Charge4- 12 (8) -0 Calculate the formal charge on the circled atoms in the following structures. formal charge: Incorect formal charge: formal charge: 1 Incomectarrow_forwardWhat is the formal charge on the atom the arrow points to? CI CI Al- CI- CH, CI O+2 O+1 O-2arrow_forward-draw the possible resonance structures of IO3^2- ion. -the experimental bond length of P and O bond in PO4^3- ion is in between the bond lengths of P=O and P-O.what is the reason behind this?. -draw the possible resonance structures of C3h3^- ion and on each sructure assign formal charge on each atom.arrow_forward
- The purple pathway: the oxygen - flow to the C-O bond, then from the C=C bond to the carbon atom, then the water molecule. I do not understand why cant the electrons flow from the oxygen - to the water directly AND why cant electrons flow from C=c to the water molecule , but have to land on a carbon atom first before flowing to water.arrow_forwardEthyl acetate, C4H;O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is (Figure 1). Figure 1 of 1 :Ö: H H-C-C-O-C-C-H нн H. ннarrow_forwardBased on trends in electronegativity, Rank the following polarity of the bonds. Use numbers 1, 2, 3, 4 to fill in the ranking. 1 represents the MOST polar, 4 represents the LEAST polar! Molecule Н- СІ H - N Н-F Н-С H-CI [ Choose H-N [ Choose ] H-F [ Choose ] Н-С [ Choose ]arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning
General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9781305580350
Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher:Cengage Learning
General, Organic, and Biological Chemistry
Chemistry
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:Cengage Learning
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY