Concept explainers
(a)
Interpretation:
The hybrid-orbital picture for the hydronium ion
Concept introduction:
The atomic orbitals combine to form the new set of orbitals known as hybrid orbitals. The hybrid orbitals are obtained due to the mixing of atomic orbitals with different azimuthal quantum numbers. The hybrid orbitals have the property of directionality that is the electron density in the hybrid orbitals is directional.
(b)
Interpretation:
The
Concept introduction:
The atomic orbitals combine to form the new set of orbitals known as hybrid orbitals. The hybrid orbitals are obtained due to the mixing of atomic orbitals with different azimuthal quantum numbers. The hybrid orbitals have the property of directionality that is the electron density in the hybrid orbitals is directional.
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Organic Chemistry
- (a) Construct a Lewis structure for O2 in which each atomachieves an octet of electrons. (b) How many bondingelectrons are in the structure? (c) Would you expect theO¬O bond in O2 to be shorter or longer than the O¬Obond in compounds that contain an O¬O single bond?Explain.arrow_forward. Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?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
- Sodium azide is a shock-sensitive compound that releases N2upon physical impact. The compound is used in automobileairbags. The azide ion is N3-. (a) Draw the Lewis structure of theazide ion that minimizes formal charge (it does not form a triangle).Is it linear or bent? (b) State the hybridization of the centralN atom in the azide ion. (c) How many σ bonds and how manyπ bonds does the central nitrogen atom make in the azide ion?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_forwardIn developing a Lewis structure for NO +, the nitroxonium ion, how many valence electrons must you account for?arrow_forward
- For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. [b] The greater the orbital overlap in a bond, the shorter the bond. [c] To create a hybrid orbital, you could use the s orbital on one atom with a p orbital on another atom. [d] Nonbonding electron pairs cannot occupy a hybrid orbital.arrow_forwardConsider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.arrow_forwardThe Lewis structure of BH2Cl (a) Is the molecule polar or nonpolar? (b) What is the hybridization of the carbon atom? (c) What is the geometric shape of the molecule?arrow_forward
- Nitrogen 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_forwarda) Methane 1CH42 and the perchlorate ion 1ClO4- 2 are both described as tetrahedral. What does this indicate about their bond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forward19. :O: || :0-N- O: Which of the following statements, if true, would support the claim that the NO3 ion, represented above, has three resonance structures? (A) The NO3 ion is not a polar species. (B) The oxygen-to-nitrogen-to-oxygen bond angles are 90°. (C) One of the bonds in NO3 is longer than the other two. (D) One of the bonds in NO3¯ is shorter than the other two.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning