8th Edition

ISBN: 9780134042282

Author: Paula Yurkanis Bruice

Publisher: PEARSON

Concept explainers

Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be ne…

Polarity Of Water

In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in t…

Valence Bond Theory Vbt

Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the forma…

Videos

Textbook Question

Chapter 1.16, Problem 46P

What of the following molecules would you expect to have a dipole moment of zero? To answer parts g and h, you may need to review the Problem Solving Strategy on p. 39.

a. CH₃CH₃

Chapter 1.16, Problem 46P, What of the following molecules would you expect to have a dipole moment of zero? To answer parts g , example 1

b. CH₂Cl₂
c. NH₃

Chapter 1.16, Problem 46P, What of the following molecules would you expect to have a dipole moment of zero? To answer parts g , example 2

Chapter 1.16, Problem 46P, What of the following molecules would you expect to have a dipole moment of zero? To answer parts g , example 3

d. BeCl₂
e. BF₃

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 1.15, Problem 45P

Chapter 1.16, Problem 47P

Students have asked these similar questions

None

JON Determine the bund energy for UCI (in kJ/mol Hcl) using me balanced chemical equation and bund energies listed? का (My (9) +36/2(g)-(((3(g) + 3(g) A Hryn = -330. KJ bond energy и-н 432 bond bond C-1413 C=C 839 N-H 391 C=O 1010 S-H 363 б-н 467 02 498 N-N 160 N=N 243 418 C-C 341 C-0 358 C=C C-C 339 N-Br 243 Br-Br C-Br 274 193 614 (-1 214||(=olin (02) 799 C=N 615 AAL

Determine the bond energy for HCI ( in kJ/mol HCI) using he balanced cremiculequecticnand bund energles listed? also c double bond to N is 615, read numbets carefully please!!!! Determine the bund energy for UCI (in kJ/mol cl) using me balanced chemical equation and bund energies listed? 51 (My (9) +312(g)-73(g) + 3(g) =-330. KJ спод bond energy Hryn H-H bond band 432 C-1 413 C=C 839 NH 391 C=O 1010 S-1 343 6-H 02 498 N-N 160 467 N=N C-C 341 CL- 243 418 339 N-Br 243 C-O 358 Br-Br C=C C-Br 274 193 614 (-1 216 (=olin (02) 799 C=N 618

Chapter 1 Solutions

Organic Chemistry (8th Edition)

Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - a. How many protons do the following species...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 4P Ch. 1.2 - a. Write the ground-state electronic configuration...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar? a. b. c. d.Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...

Ch. 1.3 - Explain why HCL has a smaller dipole moment than...Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...Ch. 1.4 - Prob. 16P Ch. 1.4 - a. Draw two Lewis structure for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 20P Ch. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 22P Ch. 1.4 - Prob. 23P Ch. 1.5 - Draw the following orbitals: a. 3s orbital b. 4s...Ch. 1.6 - Prob. 25P Ch. 1.6 - Indicate the kind of molecular orbital (, , , or )...Ch. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.7 - Explain why a bond formed by overlap of s orbital...Ch. 1.9 - Put n number in each of the blanks: a. __ s...Ch. 1.9 - For each of the given species: a. Draw its Lewis...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 35P Ch. 1.13 - a. What are the relative lengths and strengths of...Ch. 1.13 - Prob. 38P Ch. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Which of the bond in a carbon-oxygen double bond...Ch. 1.15 - Would you expect a CC bond formed by sp2sp2...Ch. 1.15 - Caffeine is a natural insecticide found in the...Ch. 1.15 - a. What is the hybridization of each of the carbon...Ch. 1.15 - Predict the approximate bond angles for a. the CNC...Ch. 1.16 - What of the following molecules would you expect...Ch. 1.16 - Account for the difference in the shape and color...Ch. 1.16 - If the dipole moment of CH3F is 1.847 D and the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 50P Ch. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Draw the condensed structure of a compound that...Ch. 1 - Predict the approximate bond angles: a. the CNH...Ch. 1 - Prob. 54P Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - What is the hybridization of each of the carbon...Ch. 1 - Rank the bonds from most polar. a. CO, CF, CN b....Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 59P Ch. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 62P Ch. 1 - Draw the missing lone-pair electrons and assigns...Ch. 1 - a. Which of the indicated bonds in each molecule...Ch. 1 - For each of the following molecules, indicate the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 67P Ch. 1 - Rank the following compounds from highest dipole...Ch. 1 - In which orbitals are the lone pairs in nicotine?Ch. 1 - Prob. 70P Ch. 1 - Prob. 71P Ch. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 73P Ch. 1 - Which compound has a larger dipole moment: CH3Cl...Ch. 1 - Prob. 75P Ch. 1 - Explain why CH3Cl has a greater dipole moment than...Ch. 1 - a. Draw a Lewis structure for each of the...Ch. 1 - There are three isomers with molecular formula...

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.

What of the following molecules would you expect to have a dipole moment of zero? To answer parts g and h, you may need to review the Problem Solving Strategy on p. 39. a. CH 3 CH 3 b. CH 2 Cl 2 c. NH 3 d. BeCl 2 e. BF 3

Solution Summary: The author explains that the zero dipole moment among the following compounds should be determined.

Concept explainers

Videos

Want to see the full answer?

Chapter 1 Solutions