Question 18 of 39In the molecule below, predict the geometry and hybridization of the circled atom.A) sp and tetrahedralH.HB) sp' and trigonal planarC) sp and tetrahedralH3CCH3D) sp and trigonal planarE) sp and trigonal planar

Hybridization :- The hypothetical intermixing of atomic orbitals of slightly different energies and…

Answered: In the molecule below, predict the…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

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Problem 82CWP: Pelargondin is the molecule responsible for the red color of the geranium flower. It also...

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7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals?
Pelargondin is the molecule responsible for the red color of the geranium flower. It also contributes to the color of ripe strawberries and raspberries. The structure of pelargondin is: How many and bonds exist in pelargondin? What is the hybridization of the carbon atoms marked 14?
Two important industrial chemicals, ethene, C2H4, and propene, C3H6, are produced by the steam (or thermal) cracking process: 2C3H8(g)C2H4(g)+C3H6(g)+H2(g) For each of the four carbon compounds, do the following: (a) Draw a Lewis structure. (b) Predict the geometry about the carbon atom. (c) Determine the hybridization of each type of carbon atom.
Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O. Assuming its empirical and molecular formulas are the same, draw a Lewis structure of the molecule and specify the hybridization of the central atom (O). (b) Another oxide is unstable BrO. Assuming the molecular orbital diagram in Figure 9. 16 applies to BrO, write its electron configuration (where Br uses 45 and 4p orbitals). What is the highest occupied molecular orbital (HOMO) for the molecule?
Identify the hybridization of each carbon atom in the following molecule. (The arrangement of atoms is given; you need to determine how many bonds connect each pair of atoms.)
Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. KCIO3 contains the ClO3 ion. P4S3 is an unusual molecule with the skeletal structure. (a) Write Lewis structures for P4S3 and the ClO3 ion. (b) Describe the geometry about the P atoms, the S atom, and the Cl atom in these species. (c) Assign a hybridization to the P atoms, the S atom, and the Cl atom in these species. (d) Determine the oxidation states and formal charge of the atoms in P4S3 and the ClO3 ion.
Numerous molecules are detected in deep space. Three of them are illustrated here. (a) Are these compounds isomers? (b) Indicate the hybridization of each C atom in each molecule. (c) What is the value of the HCH angle in each of the three molecules? (d) Which of these molecules is/are polar? (e) Which molecule should have the strongest carbon-carbon bond? The strongest carbon-oxygen bond?
Why are d orbitals sometimes used to form hybrid orbitals? Which period of elements does not used orbitals for hybridization? If necessary, which d orbitals (3d, 4d, 5d, or 6d) would sulfur use to form hybrid orbitals requiring d atomic orbitals? Answer the same question for arsenic and for iodine.
Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.39.
In propene CH3CH=CH2, the first carbon has sp3 hybrid orbitals and the second carbon has sp2 hybrid orbitals. These orbitals interact to make a bond. Why are these hybrid orbitals not orthogonal?
What hybridization is required for central atoms that have a tetrahedral arrangement ofelectron pairs? A trigonal planar arrangement of electron pairs? A linear arrangement ofelectron pairs? How many unhybridized p atomic orbitals are present when a centralatom exhibits tetrahedral geometry? Trigonal planar geometry? Linear geometry? Whatare the unhybridized p atomic orbitals used for?
In the hydrocarbon(a) What is the hybridization at each carbon atom in themolecule? (b) How many s bonds are there in the molecule?(c) How many p bonds? (d) Identify all the 120° bond anglesin the molecule. [Section 9.6]

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In the molecule below, predict the geometry and hybridization of the circled atom. A) sp and tetrahedral B) sp* and trigonal planar C) sp and tetrahedral D) sp and trigonal planar E) sp and trigonal planar