Concept explainers
Carbon monoxide is produced by incomplete combustion of fossil fuels.
(a) Give the electron configuration for the valence molecular orbitals of CO. The orbitals have the same energy order as those of the
(b) Do you expect CO to be paramagnetic or diamagnetic?
(c) What is the bond order of CO? Does this match the bond order predicted by the electron-dot structure?
(d) CO can react with
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CHEMISTRY-TEXT
- 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_forward(a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forwardNitrogen trifluoride (NF3) is used in the electronics industry to clean surfaces. NF3 is also a potent greenhouse gas. (A) Draw the Lewis structure of NF3 and determine its molecular geometry. (B) BF3 and NF3 both have three covalently bonded fluorine atoms around a central atom. Do they have the same dipole moment? (C) Could BF3 also behave as a greenhouse gas? Explain why or why not.arrow_forward
- The structure of caffeine is shown below. (a) Complete the Lewis structure. (b) How many pi bonds are present in caffeine? How many sigma bonds? (c) Identify the hybridization of the carbon atoms. (d) What is the value of the O-C-N angle?arrow_forward2(a) Provide the Lewis structures for both CH3OH and C2H3Cl. 2(b) What is the largest bond angle among all the bond angles in CH3OH and C2H3Cl? Listthe three atoms making this largest bond angle, and estimate the value of the angle.2(c) What intermolecular forces are present(i) between CH3OH molecules?(ii) between C2H3Cl molecules?arrow_forwardThe sulfate ion can be represented with four S-O bonds or with two S-O and two So=O bonds.(a) Which representation is better from the standpoint of formal charges?(b) What is the shape of the sulfate ion, and what hybrid orbitals of S are postulated for the σ bonding?(c) In view of the answer to part (b), what orbitals of S must be used for the π bonds? What orbitals of O?(d) Draw a diagram to show how one atomic orbital from S and one from O overlap to form a π bond.arrow_forward
- Draw the molecular orbital energy diagrams for the valence electrons in the following diatomic molecules. Calculate the bond order and indicate if each of them is diamagnetic or paramagnetic. (а) В> (b) С. (c) CO (d) NO (е) Оzarrow_forwardIf an electron is removed from a fluorine molecule, an F+2molecular ion forms.(a) Give the molecular electron configurations for F2 and F+2 (for the MOs constructed from valence AOs).(b) Give the bond order of each species.(c) Predict which species should be paramagnetic.(d) Predict which species has the greater bond dissociation energy.arrow_forward(a) Draw the best Lewis structure(s) for the nitrite ion, NO2-.(b) With what allotrope of oxygen is it isoelectronic?(c) What would you predict for the lengths of the bondsin NO2- relative to N¬O single bonds and doublebonds?arrow_forward
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- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning