Connect 1-Semester Online Access for Principles of General, Organic & Biochemistry
2nd Edition
ISBN: 9780077633707
Author: Janice Smith
Publisher: Mcgraw-hill Higher Education (us)
expand_more
expand_more
format_list_bulleted
Question
Chapter 3, Problem 3.105CP
(a)
Interpretation Introduction
Interpretation:
The total number of valence electrons in
(b)
Interpretation Introduction
Interpretation:
The Lewis structure of
(c)
Interpretation Introduction
Interpretation:
The polar bonds in
(d)
Interpretation Introduction
Interpretation:
The shape around carbon atom has to be given.
(e)
Interpretation Introduction
Interpretation:
The polarity of
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Answer the following questions about the molecule OCS. a. How many valence electrons does OCS contain? b. Draw a valid Lewis structure. c. Label all polar bonds. d. What is the shape around the C atom? e. Is OCS a polar molecule? Explain.
Consider the compound NO3.
Is NO, a polar or nonpolar molecule?
A. Polar molecule
B. Nonpolar molecule
C. Not enough information
has been provided
or ion:
1. Draw the complete Lewis structure of the molecule or ion.
2. Determine the total number of electron groups (clouds) surrounding the
central atom.
3. Determine the electron geometry of the groups around the central atom
(linear, trigonal planar, etc.)
4. Determine the molecular shape of the molecule (linear, bent, trigonal
planar, etc.)
5. Determine the molecular polarity (polar vs, nonpolar)
6. SCN-, thiocyanate ion (carbon central atom)
Lewis structure
Total number of electron groups around
the central atom
Electron geometry
Molecular shape
Molecular polarity
Chapter 3 Solutions
Connect 1-Semester Online Access for Principles of General, Organic & Biochemistry
Ch. 3.1 - Predict whether the bonds in the following species...Ch. 3.2 - Write the ion symbol for an atom with the given...Ch. 3.2 - Prob. 3.4PCh. 3.2 - Prob. 3.5PCh. 3.2 - How many electrons and protons are contained in...Ch. 3.2 - Prob. 3.7PCh. 3.3 - Write the formula for the ionic compound formed...Ch. 3.3 - Prob. 3.9PCh. 3.4 - Prob. 3.10PCh. 3.4 - Give the symbol for each ion. a. stannous b....
Ch. 3.4 - Name each ionic compound. a. NaF b. MgO c. SrBr2...Ch. 3.4 - Name each ionic compound. a. CrCl3 b. PbS c. SnF4...Ch. 3.4 - Prob. 3.14PCh. 3.5 - List four physical properties of ionic compounds.Ch. 3.6 - Write the formula for the compound formed when K+...Ch. 3.6 - Prob. 3.17PCh. 3.6 - Name each compound. a. Na2CO3 b. Ca(OH)2 c....Ch. 3.6 - Prob. 3.19PCh. 3.7 - Use electron-dot symbols to show how a hydrogen...Ch. 3.7 - Prob. 3.21PCh. 3.8 - Draw a Lewis structure for each covalent molecule....Ch. 3.8 - Prob. 3.23PCh. 3.8 - Prob. 3.24PCh. 3.9 - Prob. 3.25PCh. 3.9 - Prob. 3.26PCh. 3.10 - Prob. 3.27PCh. 3.11 - Prob. 3.28PCh. 3.11 - Prob. 3.29PCh. 3.11 - Show the direction of the dipole in each bond....Ch. 3.12 - Prob. 3.31PCh. 3.12 - Prob. 3.32PCh. 3 - Which formulas represent ionic compounds and which...Ch. 3 - Which pairs of elements are likely to form ionic...Ch. 3 - Prob. 3.35UKCCh. 3 - Prob. 3.36UKCCh. 3 - Prob. 3.37UKCCh. 3 - Prob. 3.38UKCCh. 3 - Prob. 3.39UKCCh. 3 - Prob. 3.40UKCCh. 3 - Prob. 3.41UKCCh. 3 - Prob. 3.42UKCCh. 3 - Prob. 3.43UKCCh. 3 - Prob. 3.44UKCCh. 3 - Prob. 3.45UKCCh. 3 - Prob. 3.46UKCCh. 3 - (a) Translate each ball-and-stick model to a Lewis...Ch. 3 - Prob. 3.48UKCCh. 3 - Prob. 3.49APCh. 3 - How many protons and electrons are present in each...Ch. 3 - Prob. 3.51APCh. 3 - Prob. 3.52APCh. 3 - Prob. 3.53APCh. 3 - Give the ion symbol for each ion. a. barium ion b....Ch. 3 - Prob. 3.65APCh. 3 - Write the formula for the ionic compound formed...Ch. 3 - Prob. 3.67APCh. 3 - Prob. 3.68APCh. 3 - Name each ionic compound. a. Na2O b. BaS c. PbS2...Ch. 3 - Name each ionic compound. a. KF b. ZnCl2 c. Cu2S...Ch. 3 - Prob. 3.71APCh. 3 - Write formulas to illustrate the difference...Ch. 3 - Prob. 3.73APCh. 3 - Name each ionic compound. a. (NH4)2SO4 b. NaH2PO4...Ch. 3 - Prob. 3.75APCh. 3 - Prob. 3.76APCh. 3 - Prob. 3.77APCh. 3 - Label each statement as true or false. Correct any...Ch. 3 - Prob. 3.79APCh. 3 - Prob. 3.80APCh. 3 - Prob. 3.81APCh. 3 - Prob. 3.82APCh. 3 - Convert the 3-D model of oxalic acid into a Lewis...Ch. 3 - Convert the 3-D model of the general anesthetic...Ch. 3 - Prob. 3.85APCh. 3 - Prob. 3.86APCh. 3 - Prob. 3.87APCh. 3 - Prob. 3.88APCh. 3 - Prob. 3.89APCh. 3 - Prob. 3.90APCh. 3 - Prob. 3.91APCh. 3 - Prob. 3.92APCh. 3 - Prob. 3.93APCh. 3 - Prob. 3.94APCh. 3 - Rank the atoms in each group in order of...Ch. 3 - Prob. 3.96APCh. 3 - Prob. 3.97APCh. 3 - Prob. 3.98APCh. 3 - Prob. 3.99APCh. 3 - Which bond in each pair is more polarthat is, has...Ch. 3 - Prob. 3.101APCh. 3 - Prob. 3.102APCh. 3 - Isobutyl cyanoacrylate is used in medical glues to...Ch. 3 - Prob. 3.104APCh. 3 - Prob. 3.105CPCh. 3 - Prob. 3.106CP
Knowledge Booster
Similar questions
- What is the most polar bond in the molecule?arrow_forwardDetermining Molecular Polarity Determine whether each molecule is polar: a.HBrb.IClc.I2d.COarrow_forwardThe images below are models of different types of bonding. C Which figure represents a polar molecule? OA. A because polar molecules evenly share electrons. OB. C because polar molecules unevenly share electrons and make partial positive and negative charges. B because polar molecules transfer electrons creating a positive cation and negative anion. OD. A and B because polar molecules share electrons.arrow_forward
- 1. The electron pair in a H - Cl bond could be considered... a. closer to H because Hydrogen has a larger radius and thus exerts greater control over the shared electron pair b. closer to Cl because Chlorine has a higher electronegativity than Hydrogen c. closer to H because Hydrogen has a lower electronegativity than Chlorine d. an inadequate model since the bond is ionic 2. It is important to know the geometry of a molecule because the geometry _______. a. will give the Lewis structure of the molecule b. affects the physical and chemical properties of the substance c. will determine whether the molecule is ionic or covalent d. Both B, and Carrow_forwardWhich of the following statements is INCORRECT? a. Polar covalent bonds can be present in a nonpolar molecule.b. Polar covalent bond is present if the electronegativity difference between atoms is equal or less than 0.4.c. Polarity of bond and molecular geometry are the two factors that affect the polarity of molecules. d. Polar bonds forms when electrons are unequally shared by two atoms in a compound.arrow_forwardionic character of the bond is less than 51% percent so the bond is covalent. (Think and check the periodic table) Multiple Choice. 20. In the molecule models of HF, HCI, and HBr on page 10, the respective numbers (1.0cm, 1.2 cm, and 1.5 cm) represent the a. protons in the atom c. repulsive force between the atoms b. molecular distance between nuclei d. actual distance between atoms 21. The halogen element that has the most attraction for the hydrogen electron is a. fluorine b. chlorine c. brominearrow_forward
- Consider the Lewis structure shown below. The A-B bonds are polar. Is this molecule polar or nonpolar? Why? B A B 1. This molecule is nonpolar. 2. This molecule is polar. Because 3. The bond dipoles point in opposite directions and cancel each other out. 4. The molecule contains polar bonds. 5. The bond dipoles add together, leaving an overall molecular dipole.arrow_forwardQuestion 48 48. Which of the following statements are true? 1. 11. III. IV. The electrons in each molecule tend to orient themselves around the most electronegative element. Each molecular drawing follows the localized electron model. Both HF and CO₂ are linear molecules and therefore polar. The bond angles of NH3 are slightly less than 109.5° because the lone pair compresses the angles between the bonding pairs. a. I, III, IV b. I, II, IV c. I, II, III d. II, IV e. All of the above statements are correct. C B esc E Q @ 2 W # 3 E $ 4 * R % 5 T < 6 Y & 7 8 Uarrow_forwardDraw a Lewis structure for NH3 and answer the following questions based on your drawing. 1. For the central nitrogen atom: The number of lone pairs The number of single bonds = The number of double bonds= 2. The central nitrogen atom A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet. =arrow_forward
- Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules and ions. Draw a Lewis structure for NH,* and answer the following questions based on your drawing. 1. For the central nitrogen atom: The number of lone pairs The number of single bonds = The number of double bonds= 2. The central nitrogen atom A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet.arrow_forwardWhich statement A-D about VSEPR theory is not correct? Select one: a. The molecular shape or geometry can differ from the electron-pair geometry. b. In VSEPR theory, the shape or geometry of a molecule is determined by electron-electron repulsion. c. The steric number of a central atom is the sum of the number of bonded atoms and lone pairs around the central atom. d. The steric number has five values from 2 to 6. e. Statements A-D are all correct. Clear my choicearrow_forwardWhich description below correctly describes polar molecules? a. Have polar bonds present. b. The polar bonds are arranged so that they do not cancel. c. Lone pairs on the central atom are arranged so that they do not cancel. d. Lone pairs on the central atom are arranged so that they can be cancelled out.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER