(a)
Interpretation:
Hybridization of
Concept Introduction:
Hybridization is the concept of mixing of atomic orbital into hybrid orbitals that are of dissimilar shapes, energies and are appropriate for combination of electrons to form bonds in
Hybridization is calculated by the hybrid orbitals and to calculate hybrid orbitals we need to know the steric number that is given by,
The table that relates the steric number with hybridization is as follows:
(b)
Interpretation:
Hybridization of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Hybridization of
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
Hybridization of
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Chemical Principles: The Quest for Insight
- Acrylonitrile, C3H3N is the building mer Orlon. Its Lewis structure is What is the hybridization of nitrogen and of the three numbered carbon atoms?arrow_forwardWhat are the relationships among bond order, bond energy, and bond length? Which of these quantities can be measured?arrow_forwardDescribe the hybrid orbitals used by the central atom(s) and the type(s) of bonds formed in (a) FNO; (b) C2F4; (c) (CN)2.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) What is the hybridization of chlorine in Clo4 ? (Type your answer using the format sp3 for sp3.) (b) What is the hybridization of bromine in BrF5? (c) What is the hybridization of bromine in BrO2 ?arrow_forward1. Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central atom. (a) POF3 (b) XeO₂F3+ (c) BrCl₂ (d) N3 (the central atom is N; two other N's are bonded to it) (e) PF3arrow_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_forwardFor each of the following molecule: (i) draw the correct Lewis structure; (ii) determine the molecular geometry and the type of hybridization on the central atom, and (iii) predict whether the molecule is polar or nonpolar. (a) BrCl5arrow_forward1. For each of the following molecules, please provide (a) hybridization of the central atom, (b) a Lewis dot structure, (c) a sketch of the molecular structure and the name of the structural arrangement, and (d) the expected bond angles (if distorted, just indicate if the angle is smaller or larger than the ideal geometry). OSbC1₂+ OCCI+arrow_forward
- Azo dyes are organic dyes that are used for many applications,such as the coloring of fabrics. Many azo dyes arederivatives of the organic substance azobenzene, C12H10N2.A closely related substance is hydrazobenzene, C12H12N2.The Lewis structures of these two substances are given (Recall the shorthand notation used for benzene.)(a) What is the hybridization at the N atom in each of thesubstances? (b) How many unhybridized atomic orbitalsare there on the N and the C atoms in each of the substances?(c) Predict the N—N—C angles in each of thesubstances. (d) Azobenzene is said to have greater delocalizationof its π electrons than hydrazobenzene. Discussthis statement in light of your answers to (a) and (b). (e) Allthe atoms of azobenzene lie in one plane, whereas thoseof hydrazobenzene do not. Is this observation consistentwith the statement in part (d)? (f) Azobenzene is an intensered-orange color, whereas hydrazobenzene is nearly colorless.Which molecule would be a better one to use in…arrow_forward7. Nitrogen is the central atom in each of the species given. (a) Draw the Lewis electron-dot structure for each of the species. + NO₂ NO₂ NO₂ (b) List the species in order of increasing bond angle. Justify your answer. (c) For NO₂ and NO₂, give the hybridization of the nitrogen atom in it. (d) Identify the only one of the species that dimerizes and explain what causes it to do so.arrow_forwardDraw Lewis diagrams and predict the geometries of the following molecules. State which are polar and which are nonpolar. (a) ONCI (c) XeF2 (e) CHF; (b) O,NCI (d) SCl4arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning