Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 7, Problem 115E
Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the “real” and “model” modes. Explain the difference observed.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Please answer all parts of the question
3) Determine whether CH3CI is polar. To do this, you must: draw the
3D structure of the molecule, use arrows to indicate polar bonds, and
either use an arrow to indicate the net dipole moment or state that the
molecule is non-polar.
Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to build amolecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.
Chapter 7 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 7 - Does a cation gain protons to form a positive...Ch. 7 - Iron(III) sulfate [Fe2( SO 4)3] is composed of...Ch. 7 - Which of the following atoms would be expected to...Ch. 7 - Which of the following atoms would be expected to...Ch. 7 - Predict the charge on the monatomic ions formed...Ch. 7 - Predict the charge on the monatomic ions formed...Ch. 7 - Write the electron configuration for each of the...Ch. 7 - Write the electron configuration for the monatomic...Ch. 7 - Write out the full electron configuration for each...Ch. 7 - From the labels of several commercial products,...
Ch. 7 - Why is it incorrect to speak of a molecule of...Ch. 7 - What information can you use to predict whether a...Ch. 7 - Predict which of the following compounds are ionic...Ch. 7 - Explain the difference between a nonpolar covalent...Ch. 7 - From its position in the periodic table, determine...Ch. 7 - From its position in the periodic table, determine...Ch. 7 - From their positions in the periodic able, arrange...Ch. 7 - From their positions in the periodic table,...Ch. 7 - Which atoms can bond to sulfur so as to produce a...Ch. 7 - Which is the most polar bond? (a) CC (b) CH (c) NH...Ch. 7 - Identify the more polar bond in each of the...Ch. 7 - Which of the following molecules or ions contain...Ch. 7 - Write the Lewis symbols for each of the following...Ch. 7 - Many monatomic ions are found in seawater,...Ch. 7 - Write the Lewis symbols of the ions in each of the...Ch. 7 - Iii (he Lewis structures listed here, M and X...Ch. 7 - Write the Lewis structure for the diatomic...Ch. 7 - Write Lewis structures for the following: (a) H2...Ch. 7 - Write Lewis structures for the following: (a) O2...Ch. 7 - Write Lewis structures for the following: (a) ClF3...Ch. 7 - Write Lewis structures for the following: (a) SeF6...Ch. 7 - Write Lewis structures for: (a) PO43 (b) ICl4 (c)...Ch. 7 - Correct the following statement: The bonds in...Ch. 7 - Write Lewis structures for the following molecules...Ch. 7 - Methanol, H3COH, is used as the fuel in some race...Ch. 7 - Many planets in our solar system contain organic...Ch. 7 - Carbon tetrachloride was formerly used in fire...Ch. 7 - Identify the atoms that correspond to each of the...Ch. 7 - The arrangement of atoms in several biologically...Ch. 7 - A compound with a molar mass of about 28 g/mol...Ch. 7 - A compound with a molar mass of about 42 g/mol...Ch. 7 - Two arrangements of atoms are possible for a...Ch. 7 - How are single, double, and triple bonds similar?...Ch. 7 - Write resonance forms that describe the...Ch. 7 - Write resonance forms that describe the...Ch. 7 - Write the resonance forms of ozone, Q3, the...Ch. 7 - Sodium nitrite, which has been used to preserve...Ch. 7 - In terms of the bonds present, explain why acetic...Ch. 7 - Write the Lewis structures for the following, and...Ch. 7 - Toothpastes containing sodium hydrogen carbonate...Ch. 7 - Determine the formal charge of each element in the...Ch. 7 - Determine the formal charge of each element in the...Ch. 7 - Calculate the formal charge of chlorine in the...Ch. 7 - 54. Calculate the formal charge of each element in...Ch. 7 - Draw all possible resonance structures for each of...Ch. 7 - Based on formal charge considerations, which of...Ch. 7 - Based on formal charge considerations, which of...Ch. 7 - Based on formal charge considerations, which of...Ch. 7 - Draw the structure of hydroxylamine, H3NO, and...Ch. 7 - Iodine forms a series of fluorides (listed here)....Ch. 7 - Write the Lewis structure and chemical formula of...Ch. 7 - Which of the following structures would we expect...Ch. 7 - Sulfuric acid is the industrial chemical produced...Ch. 7 - Which bond in each of the following pairs of bonds...Ch. 7 - Using the bond energies in Table 7.2, determine...Ch. 7 - Using the bond energies in Table 7.2, determine...Ch. 7 - When a molecule can form two different structures,...Ch. 7 - How does the bond energy of HCl(g) differ from the...Ch. 7 - Using the standard enthalpy of formation data in...Ch. 7 - Using the standard enthalpy of formation data in...Ch. 7 - Using the standard enthalpy of formation data in...Ch. 7 - Using the standard enthalpy of formation data in...Ch. 7 - Complete the following Lewis structure by adding...Ch. 7 - Use the bond energy to calculate an approximate...Ch. 7 - Element First Ionization Energy (kJImol) Second...Ch. 7 - The lattice energy of LiF is 1023 kJ/mol, and the...Ch. 7 - For which of the following substances is the least...Ch. 7 - The reaction of a metal, M, with a halogen, X2,...Ch. 7 - The lattice energy of LiF is 1023 kJ/mol, and the...Ch. 7 - Which compound in each of the following pairs has...Ch. 7 - Which compound in each of the following pairs has...Ch. 7 - Which of the following compounds requires the most...Ch. 7 - Which of the following compounds requires the most...Ch. 7 - The lattice energy of KF is 794 kJ/mol, and the...Ch. 7 - Explain why the HOH molecule is bent, whereas the...Ch. 7 - What feature of a Lewis structure can be used to...Ch. 7 - Explain the difference between electron-pair...Ch. 7 - Why is the HNH angle in NH3 smaller than the HCH...Ch. 7 - Explain how a molecule that contains polar bonds...Ch. 7 - As a general rule, MX molecules (where M...Ch. 7 - Predict the electron pair geometry and the...Ch. 7 - Identify the electron pair geometry and the...Ch. 7 - What are the electron-pair geometry and the...Ch. 7 - Predict the electron pair geometry and the...Ch. 7 - Identify the electron pair geometry and the...Ch. 7 - Predict the electron pair geometry and the...Ch. 7 - Which of the following molecules and ions contain...Ch. 7 - Which of these molecules and ions contain polar...Ch. 7 - Which of the following molecules have dipole...Ch. 7 - Identify the molecules with a dipole moment: (a)...Ch. 7 - The molecule XF3 has a dipole moment. Is X boron...Ch. 7 - The molecule XCl2 has a dipole moment. Is X...Ch. 7 - Is the Cl2BBCl2 molecule polar or nonpolar?Ch. 7 - There are three possible structures for PCl2F3...Ch. 7 - Describe the molecular structure around the...Ch. 7 - Draw the Lewis structures and predict the shape of...Ch. 7 - A molecule with the formula AB2, in which A and B...Ch. 7 - A molecule with the formula AB3, in which A and B...Ch. 7 - Draw the Lewis electron dot structures for these...Ch. 7 - What is the molecular structure of the stable form...Ch. 7 - A compound with a molar mass of about 42 g/mol...Ch. 7 - Use the simulation...Ch. 7 - Use the simulation...Ch. 7 - Use the Molecule Shape simulator...Ch. 7 - Use the Molecule Shape simulator...Ch. 7 - Use the Molecule Shape simulator...
Additional Science Textbook Solutions
Find more solutions based on key concepts
Everyday application: Suppose a yo-yo has a center shaft that has a 0.250 cm radius and that its string is bein...
College Physics
a. Which 2+ ion has two 3d electrons? Which has eight 3d electrons? b. Which is the more likely configuration f...
Inorganic Chemistry
The indicator methyl red has a pF(.. • 495. It changes born red to yellow over the pH range from 4.4 to 6.2. a....
General Chemistry: Principles and Modern Applications (11th Edition)
83. Which solid has the highest melting point? Why?
a. Ar(s)
b.
c. LiCl(s)
d.
Introductory Chemistry (6th Edition)
A catalyst speeds up a chemical reaction by lowering the activation energy. Sketch Diagram A and draw a second ...
General, Organic, and Biological Chemistry (3rd Edition)
a. Draw the resonance forms for SO2 (bonded OSO). b. Draw the resonance forms for ozone (bonded OOO). c. Sulfur...
Organic Chemistry (9th Edition)
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
- A model for SiH4 is shown in the chem3D window. SiH4 has tetrahedral geometry. ball & stick |+ labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? If you take any three of the outer atoms, what shape do they define? | Consider the bond angles at the central atom. Do they all have the approximately the same numerical value? What is the approximate numerical value of this angle? | degrees. Are all four positions about the central atom equivalent, or is one of them different from the other three. For practice, type in the name of the geometry of the molecule: Previous Nextarrow_forwardtR-XZxj_1SoekWMaP1As1fEhnC179H4SICzl1mdWKpKlvbF3amiKazP. OF ORGANIC MOLECULES Drawing a Lewis structure for a simple organic molecule from a. GE OOD D Draw a Lewis structure of the molecule that matches the description below. All non-H atoms should have full octets, and all formal charges should be zero. Unless you're told otherwise, assume there are no rings in the molecule. Description: The molecule is composed of 10, 4H's, and 2C's and it contains a C-C single bond. Click and drag to start drawing a structure. 2021 McGraw-Hill Education All Rights Reseved Terms of Uhe Pcy Check Explanationarrow_forwardO Presentation Session E Jesselyn Palaguachi x cfr Haiti's Protests: Image x 29 Institute for Health Pr O Join n/student/tekihxcsq?gooleClassroom=true In the space below draw the display model of the following molecules: Be sure to include all bonds and unshared electrons. Show your work. HCN Pear Deck Interactive Slide Students, draw anywhere on this slide! T Slide 20/20 MacBook Pro +, Q Search Default & %23 2$ 4 5 6. 7 8. < CO # 3arrow_forward
- ) Bean hexene is an odor compound used in cosmetics and cleaners. It is also known as leguminal. Its formula is: CH3CH2CHCHCH2CH2OCHCH2CH3 | OCH3 Please draw a Lewis structure for this compound with CORRECT GEOMETRY (use dashes and wedges!) Label all pi bonds in the molecule (if there are any) Indicate the bond angles for the red highlighted section of the molecule. (hint: you may want to keep the main carbon chain in-plane with the page for clarity) For this question, you don’t need to draw out the orbitals.arrow_forwardMolecular geometry—don’t know why I’m incorrect all of a sudden. Might be one shape needed that is not given in the option choices.arrow_forward• Calculate Bond Pairs (BP.s) Calculate Lone Pairs (LP.s) • Draw Lewis Structure for the Simple Molecules and Polyatomic lons Page 228 Text Book) • VSEPR Notation (Pg. 234 T. Book) • Prediction of Molecular Shapes (Pg. 234 T. Book) • Polarity (justify your answer) Pg. 239 (T.Book) 1 H30* 2 3 4 5 CHCI3 -2 CO3 AIF4 + NO₂ 6 7 col 8 9 10 Xe Fz Xe F3+ SO₂ SO3 -2 SO4arrow_forward
- PHET Molecular Modeling https://phet.colorado.edu/sims/html/build-a-molecule/latest/build-a-molecule en.html Choose the "Playground" option to complete this modeling activity: You can drag and drop molecules to the screen and put them together then click the 3D button to see a model like the one we would make in the classroom. Make sure to check the ball & stick model mode in 3D viewer- this is important for seeing the bonds (sticks)! 1. Build the molecule (you can see different element choices by clicking the dots at the bottom of the screen) 2. Draw the Lewis structure. 3. Count the number of bonds and lone pairs on the central atom (lone pairs are not shown on the models only on your Lewis Structure) 4. Use bond and lone pair information to determine the shape of the molecule (linear, bent, trigonal planar, tetrahedral) 4. Calculate the polarity of each different bond by subtracting atom electronegativities. 5. Use the bond types and shape to determine if the molecule is polar or…arrow_forward|| Predicting deviations from ideal bond angles Consider the carbonyl fluoride (CF₂O) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the carbon-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the carbon-fluorine bonds to be ... 口。 (choose one) (choose one) about the same bigger smallerarrow_forwardCan you please do the first 3 rows of the table?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
INTRODUCTION TO MOLECULAR QUANTUM MECHANICS -Valence bond theory - 1; Author: AGK Chemistry;https://www.youtube.com/watch?v=U8kPBPqDIwM;License: Standard YouTube License, CC-BY