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 8, Problem 31E
Draw the orbital diagram for carbon in
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Draw the orbital diagram for carbon in CO2 showing how many carbon atom electrons are in each orbital.
Depending on the protein under study, the bond angle of a drug molecule can become critical to successfully deactivating a viral protein. For this reason, chemists are frequently concerned with the 3D shape of their molecules and their bond angles.
The oxygen atom shown in the structure has a tetrahedral electronic geometry, meaning we would predict that it would have 109.5° bond angles. However, the actual structure, the bond angles are smaller than 109.5°. Explain why this compression occurs. Make sure to discuss what’s happening around/what groups are present around the oxygen atom.
Answer the questions in the table below about the shape of the fluoroform (CHF3) molecule.
How many electron groups are around the central carbon atom?
Note: one "electron group" means one lone pair, one single bond,
one double bond, or one triple bond.
What phrase best describes the arrangement of these electron
groups around the central carbon atom?
(You may need to use the scrollbar to see all the choices.)
0
(choose one)
X
8
Chapter 8 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 8 - Explain how and bonds are similar and how they...Ch. 8 - Draw a curve that describes the energy of a system...Ch. 8 - Explain why bonds occur at specific average bond...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - How many and bonds are present in the molecule...Ch. 8 - A friend tells you N2 has three bonds due to...Ch. 8 - Draw the Lewis structures for CO2 and CO, and...Ch. 8 - Why is the concept of hybridization required in...Ch. 8 - Give the shape that describes each hybrid orbital...
Ch. 8 - Explain why a carbon atom cannot form five bonds...Ch. 8 - What is the hybridization of the central atom in...Ch. 8 - A molecule with the formula AB3 could have one of...Ch. 8 - Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino...Ch. 8 - Sulfuric acid is manufactured by a series of...Ch. 8 - Two important industrial chemicals, ethene, C2H4,...Ch. 8 - For many years after they were discovered, it was...Ch. 8 - Consider nitrous acid, HNO2 (HONO). (a) Write a...Ch. 8 - Strike-anywhere matches contain a layer of KClO3...Ch. 8 - Identify the hybridization of each carbon atom in...Ch. 8 - Write Lewis structures for NF3 and PP5. On the...Ch. 8 - In addition to NF3, two other fluoro derivatives...Ch. 8 - The bond energy of a C—C single bond averages 347...Ch. 8 - For the carbonate ion, CO32, draw all of the...Ch. 8 - A useful solvent that will dissolve salts as well...Ch. 8 - For the molecule allene, H2C=C=CH2, give the...Ch. 8 - Identify the hybridization of the central atom in...Ch. 8 - Describe the molecular geometry and hybridization...Ch. 8 - For each of the following molecules, indicate the...Ch. 8 - For each of the following structures, determine...Ch. 8 - Draw the orbital diagram for carbon in CO2 showing...Ch. 8 - Sketch the distribution of electron density in the...Ch. 8 - How are the following similar, and how do they...Ch. 8 - If molecular orbitals are created by combining...Ch. 8 - Can a molecule with an odd number of electrons...Ch. 8 - Can a molecule with an even number of electrons...Ch. 8 - Why are bonding molecular orbitals lower in energy...Ch. 8 - Calculate the bond order for an ion with this...Ch. 8 - Explain why an electron in the bonding molecular...Ch. 8 - Predict the valence electron molecular orbital...Ch. 8 - Determine the bond order of each member of the...Ch. 8 - For the first ionization energy for an N2...Ch. 8 - Compare the atomic and molecular orbital diagrams...Ch. 8 - Which of the period 2 homonuclear diatomic...Ch. 8 - A friend tells you that the 2s orbital for...Ch. 8 - True or false: Boron contains 2s22p1 valence...Ch. 8 - What charge would be needed on F2 to generate an...Ch. 8 - Predict whether the MO diagram S2 would show s-p...Ch. 8 - Explain why N22+ is diamagnetic, while O24+, which...Ch. 8 - Using the MO diagrams, predict the bond order for...
Additional Science Textbook Solutions
Find more solutions based on key concepts
Q1. What is the empirical formula of a compound with the molecular formula
Chemistry: A Molecular Approach
1. Why is the quantum-mechanical model of the atom important for understanding chemistry?
Chemistry: Structure and Properties
a. Find potassium (K) in the periodic table and predict how many valence electrons it has. b. What orbital does...
Essential Organic Chemistry (3rd Edition)
58. Write full electron configurations and indicate the valence electrons and the core electrons for each eleme...
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)
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
- Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.arrow_forwardSuccessive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.arrow_forwardWhich of the following is angular molecular shaped? NO2 SO3 HCN O H2CO3 (C being the central atom) PH3arrow_forward
- Using the principles of VSEPR theory, you can predict the geometry or electron arrangement around any atom in any molecule, no matter how complex. Predict the electron arrangement geometry around the indicated atoms in the structure shown. a H-C-0-H Part 1 of 2 H Part 2 of 2 b H Atom a: (Choose one) linear trigonal planar tetrahedral Atom b: (Choose one) Xarrow_forward4. Give four neutral atoms or ions that could have the valence electron configuration shown below 2s 2p 3sarrow_forwardConsider an iodine tetrafluoride cation (IF4*): What is the elemental symbol of its central atom? How many valence electrons does this molecule contain? How many lone electron pairs surround the central atom? How many regions of electron density surround the central atom? For remaining items in this question, place the appropriate letter in the box: What is the electron geometry of this molecule? A = linear B = trigonal planar C = tetrahedral %3D D = trigonal bipyramidal E = octahedralarrow_forward
- In the given three-dimensional molecular structure, the differently colored spheres represent different types of atoms. Write a molecular formula for this molecule. molecular formula: C₁4H12 O Rotate X ❤ Rotate Y C ОН 3 Rotate Z Zoom In ПО Zoom Out A Label Atomsarrow_forwardWrite the electron configuration for Al3+. Also, identify which of these electrons are valence electrons.arrow_forward3) 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.arrow_forward
- What are the angles a and b in the actual molecule of which this is a Lewis structure? H H C H a H C ^ b C a = 11° b=0° H -H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. X 3arrow_forwardMake a table that shows all the possible molecular shapes and AXE types within each of the 5 geometries: A central atom with 6 electron groups, 5 electron groups, 4 electron groups, 3 electron groups, and 2 electron groups. • For example, a central atom with 4 electron groups has a tetrahedral electron pair geometry. It includes the following molecular shapes: tetrahedral (AX4E0), trigonal pyramidal (AX3E1), and bent (AX2E2). • For a central atom with 6 electron groups, consider the following AXE types: AX6E0, AX5E1, AX4E2, AX3E3, and AX2E4. Note: The last two are not in your textbook but can be derived from the VSEPR model.arrow_forwardC5H12 What is the electron geometry around each C? Does the geometry around any of the carbon atoms change from structure to structure? Does the overall shape of the molecule change? Describe these changes.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
General, Organic, and Biological Chemistry
Chemistry
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher: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
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