Concept explainers
Interpretation:
The molecular orbital description of
Concept Introduction:
Molecular orbital theory: Molecular orbital theory explains about the bonding, non-bonding and anti-bonding orbitals present in molecule. A bond is generally formed in bonding electrons that shows the maximum presence of electrons than in anti-bonding electrons. Molecular orbital theory also explains about the magnetic properties of molecule.
To explain the molecular orbital description of
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Chapter 10 Solutions
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
- Aspirin, or acetylsalicylic acid, has the formula C9H8O4 and the skeleton structure (a) Complete the Lewis structure and give the number of bonds and bonds in aspirin. (b) What is the hybridization about the CO2H carbon atom (colored blue)? (c) What is the hybridization about the carbon atom in the benzene-like ring that is bonded to an oxygen atom (colored red)? Also, what is the hybridization of the oxygen atom bonded to this carbon atom?arrow_forwardMethylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is (a) How many sigma bonds are in the molecule? (b) How many pi bonds are in the molecule? (c) What is the hybridization of the carbon atom bonded to nitrogen? (d) What is the hybridization of the carbon atom bonded to oxygen? (e) What is the hybridization of the double-bonded oxygen?arrow_forwardDraw a Lewis diagram(s) for the ozone molecule (O3). Determine the steric number and hybridization of the central oxygen atom, and identify the molecular geometry. Describe the nature of the p bonds and give the bondorder of the O-O bonds in ozone.arrow_forward
- For each of the following molecules, write the Lewis structures, predict the electron geometry, molecular geometry, bond angles, expected hybrid orbitals on central atoms and predict the overall polarity. BRF3 ICI4arrow_forwardWhat is the hybridization state of the Beryllium in BeClBr? And is this a polar or nonpolar molecule?arrow_forward2. Use molecular orbital (MO) theory in description of the following molecules: Which of the following species has the greater bond enthalpy? These chemical species have the similar orbital structure to that of N2. CO, CO+arrow_forward
- The ionization energy of CO is greater than that of NO. Explain this difference based on the electron configurations of these two molecules.arrow_forwardUsing molecular orbital theory, determine the electronic structure of the first excited electronic state of N2. What differences are expected in the properties of the excited state of N2 compared with the same properties of the ground state?arrow_forwardThe existence of compounds of the noble gases was once a great surprise and stimulated a great deal of theoretical work. Sketch the molecular orbital energy level diagram for XeF and deduce its ground-state electron configurations. Is XeF likely to have a shorter or longer bond than XeF+?arrow_forward
- Draw Lewis structure for OPF, (P is the central atom). Write down all possible resonance structures, including formal charges. Draw the geometry of the ion. Indicate the hybridization of the central atom and type of orbitals involved in x bonding on both bonded atoms.arrow_forwardElectrons in bonds are negatively charged and therefore repel each other. If you had a molecule of formula AB 2 , with A being the central atom, what would you predict the 3D shape to be to allow maximum distance between the two B atoms bonded to A?arrow_forwardThe Lewis structure for SF6 is shown below. This sulfur S atom in this molecule has an expanded octet, and you are not expected to be familiar with the specific electron geometry and molecular geometry for expanded octets. Still, we can make some predictions with the knowledge that we have. Would you predict the electron geometry and molecular geometry for SF6 to be the same or to differ? Please briefly explain your answer.arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)