Concept explainers
Interpretation:TheLewis structure, resonance form, polarity and bond order for N-O bond in
Concept Introduction: Lewis dot structure is also known as Lewis dot formula or electron dot structure. The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons.
The resonance is the phenomenon in which if all the properties cannot explain by one structure, it can be shown in two or more structures by the shifting of pi bonds or lone pair but there is no change in sigma bond and position of atoms.
In the different resonance structures, hybridization gives idea about the geometry of each atom. It can be checked with the below formula:
Hybridization = Number of sigma bonds + Number of lone pairs on bonded atoms.
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Organic Chemistry: Structure and Function
- Two compounds have the molecular formula N3H3. One of the compounds, triazene, contains an NN bond; the other compound, triaziridene, does not. (a) Write the correct Lewis structures for each compound. (b) Approximate the bond angle between the three nitrogen atoms in each compound.arrow_forwardBest Lewis Formula and Molecular Geometry A student writes the Lewis electron-dot formula for the carbonate anion, CO32, as a Does this Lewis formula obey the octet rule? Explain. What are the formal charges on the atoms? Try describing the bonding for this formula in valence bond terms. Do you have any difficulty doing this? b Does this Lewis formula give a reasonable description of the electron structure, or is there a better one? If there is a better Lewis formula, write it down and explain why it is better. c The same student writes the following resonance description for CO2: Is there something wrong with this description? (What would you predict as the geometries of these formulas?) d Is one or the other formula a better description? Could a value for the dipole moment help you decide? e Can you write a Lewis formula that gives an even better description of CO2? Explain your answer.arrow_forwardIn addition to CO, CO2, and C3O2, there is another molecular oxide of carbon, pentacarbon dioxide, C5O2, a yellow solid. (a) What is the approximate C-to-C-to-O bond angle in pentacarbon dioxide? (b) What is the approximate C-to-C-to-C bond angle in this compound?arrow_forward
- It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forwardSelenium tetrafluoride, SeF₄, is a colorless liquid that is used as a fluorinating reagent in organic synthesis. Based on your Lewis structure for SeF₄, how many electron domains are on the central atom?arrow_forwardDraw the Lewis structure for acetamide (CH3CONH2), an organic compound, and determine the geometry about each interior atom. Experiments show that the geometry about the nitrogen atom in acetamide is nearly planar. What resonance structure can account for the planar geometry about the nitrogen atom?arrow_forward
- In a hydrogen molecule, the two hydrogen atoms are held together by a single bond with a bond energy of 436 kJ/mol of hydrogen. In other words, to break the H-H bonds in one mole of molecular hydrogen requires the expenditure of 436 kJ of energy. Using the balanced chemical equation for the formation of water from oxygen and hydrogen (shown above), and interpreting the stoichiometric coefficients as mole amounts, how much energy must be expended in breaking the H-H bonds? kJarrow_forwardGive the molecular shape for the oxygen atom in H 2O and H 3O + and explain why they are different.arrow_forwardUse VSEPR to predict the geometry (including bond angles) about each interior atom of methyl azide (CH3N3) and draw the molecule. Would you expect the bond angle between the two interior nitrogen atoms to be the same or different? Would you expect the two nitrogen–nitrogen bond lengths to be the same or different?arrow_forward
- draw one of the resonance structures of CH3NO3 in its VSEPR shape and estimate all bond angles. estimate the nitrogen-oxygen bond length.arrow_forwardUse VSEPR theory to predict the geometry (including bond angles) about each interior atom of methyl azide (CH3N3), and make a sketch of the molecule. Would you expect the bond angle between the two interior nitrogen atoms to be the same or different? Would you expect the two nitrogen–nitrogen bond lengths to be the same or different?arrow_forwardPhosphorus pentachloride, a key industrial compound with annual world production of about 2 x 107 kg, is used to make other compounds. It reacts with sulfur dioxide to produce phosphorus oxychloride (POCl3) and thionyl chloride (SOCl2). Draw a Lewis structure, and name the molecular shape of each product.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: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning