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Carbon monoxide
molecule. The molecular orbitals of
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Chemistry
- The 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_forwardThe drawing below shows the overlap of two hybrid orbitalsto form a bond in a hydrocarbon. (a) Which of the followingtypes of bonds is being formed: (i) C¬C σ, (ii) C¬C π,or (iii) C¬H σ? (b) Which of the following could be theidentity of the hydrocarbon: (i) CH4, (ii) C2H6, (iii) C2H4, or(iv) C2H2?arrow_forwardAcetylene (C2H2) has a tendency to lose two protons (H+) and form the carbide ion (C22−), which is present in a number of ionic compounds, such as CaC2 and MgC2. (a) What is the bond order of the carbide dianion C22−? (b) For comparison, what is the bond order of C2?arrow_forward
- A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers.(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds.(c) Describe the atomic orbitals that form the π bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.arrow_forward(a) Complete the Lewis structure for the molecule shown below. How many lone pairs are there? H-C H 1 H (b) Give the hybridizations of the following atoms in the structure: (i) Ca; (ii) Ob (c) Give approximate values of the following bond angles: (i) O a-Ca-Ob; (ii) С a -О b-Сbarrow_forward(a) The nitric oxide molecule, NO, readily loses one electronto form the NO+ ion. Which of the following is the best explanationof why this happens: (i) Oxygen is more electronegativethan nitrogen, (ii) The highest energy electron inNO lies in a π*2p molecular orbital, or (iii) The π*2pMO in NOis completely filled. (b) Predict the order of the N¬O bondstrengths in NO, NO+, and NO-, and describe the magneticproperties of each. (c) With what neutral homonuclear diatomicmolecules are the NO+ and NO- ions isoelectronic(same number of electrons)?arrow_forward
- Butadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths: (a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.arrow_forward(a) The nitric oxide molecule, NO, readily loses one electronto form the NO+ ion. Which of the following is the best explanationof why this happens: (i) Oxygen is more electronegativethan nitrogen, (ii) The highest energy electron inNO lies in a p2*p molecular orbital, or (iii) The p2*p MO in NOis completely filled. (b) Predict the order of the N¬O bondstrengths in NO, NO+, and NO-, and describe the magneticproperties of each. (c) With what neutral homonuclear diatomicmolecules are the NO+ and NO- ions isoelectronic(same number of electrons)?arrow_forwardShow, if overlap is ignored, (a) that if a molecular orbital is expressed as a linear combination of two atomic orbitals in the form ψ = ψA cos θ + ψB sin θ, where θ is a parameter that varies between 0 and π, with ψA and ψB are orthogonal and normalized to 1, then ψ is also normalized to 1. (b) To what values of θ do the bonding and antibonding orbitals in a homonuclear diatomic molecule correspond?arrow_forward
- The molecular orbitals depicted below are derived from 2p atomic orbitals in F₂⁺. (a) Give the orbital designations. (b) Which is occupied by at least one electron in F₂⁺? (c) Which is occupied by only one electron in F₂⁺?arrow_forward4. (a) Draw the shape of the atomic valence orbitals formed by the overlaping of two fluoride 2p atomic orbitals. (b) Draw the molecular orbital diagrams for F2 and F2*. Identify their bond order and magnetic properties. (c) An unstable nucleus exhibit radioactivity. (i) Explain how the number of protons and neutrons in a radioactive nucleus can be used to predict its probable mode decay. (ii) Illustrate your answer in (i) with a schematic graph.arrow_forwardThe 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_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning