Draw the Lewis structures and predict the hybridization (sp, sp2, sp3), geometry (linear, trigonal, tetrahedral) and bond angles (180°, 120°, 109.5°) for the central atoms in the following compounds. a. Cin CH3CCH b. C & O in CH3OCH3 c. C & N in CH3CHNCH3
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Kindly answer the following questions from 1 to 3. As per your guidelines, only solve the first three questions.
1. Draw the Lewis structures and predict the hybridization (sp, sp2, sp3), geometry (linear, trigonal, tetrahedral) and bond angles (180°, 120°, 109.5°) for the central atoms in the following compounds.
2. Give the systematic (IUPAC) name for each of the following
3. Given the IUPAC name, draw the structure of the following compounds.
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- Which atomic orbitals overlap to form the carbon-carbon σ and π bonding molecular orbitals of ethene, H2C=CH2? A. C2sp3 + C2sp3, and C2p + C2p B. C2sp2 + C2sp2, and C2sp2 + C2sp2 C. C2sp2 + C2sp2, and C2p + C2p D. C2sp3 + C2sp3, and C2sp2 + C2sp2Specify the hybridization (sp, sp2, sp3, sp2d, sp3d, spd2 etc.) of the circled atoms in the structures below a. Hybridization of the circled carbon is _______________; of the circled nitrogen is b.Hybridization of the circled (C=O) oxygen is _____________; of the circled (C-N-C) nitrogen is ______________; of the circled sulfur is c.Hybridization of the circled carbon on the left of C≡C is _____________;of the circled (CH2) carbon is ______________; of the circled (Si=O) silicon is______________; of the circled (C=O) oxygen isall of the orbital overlaps in NCO ‒---- Which of the following statements is TRUE? Select one: Pi bonds are stronger than sigma bonds. The sp2 hybridization scheme for carbon allows for the formation of two pi bonds. A carbon-carbon triple bond consists of one π bond. Pi bonds can hold 4 electrons: 2 above the bond axis, and 2 below the bond axis. A molecule with the VSEPR class AX4E2 will have a central atom that is sp3d2 hybridized.
- What kind of hybridization do you expect for each carbon atom in the following molecules? (a) Propane, CH3CH2CH3 (b) 2-Methylpropene, (c) But-l-en-3-yne, H2C=CHa€"Ca%ojCH (d) Acetic acid,Harry creates a compound that contains only 1 pi (π) bond in total. The central atom has 4s2, 3d10, and 4p5. There are only 3 surrounding atoms with the electron configuration: 1s2 2s2 2p5. What is the formula and VSEPR shape for this compound? Explain how this is possible with respect to hybridized orbitals and how electrons are moved around to create this compound.In the hydrocarbon: (a) What is the hybridization at each carbon atom in themolecule? (b) How many σ bonds are there in the molecule?(c) How many π bonds? (d) Identify all the 120° bond anglesin the molecule.
- Represent the bonding in each molecule or ion by drawing the orbitals (hybridized and unhybridized) of each atom in the bond. Label the σ and π bonds and label each bond by the orbitals that it is made from. For instance, the C–H bond in CH4 would be made from the overlap of: C (sp3) – H (1 s). You may draw the hybridized sigma orbitals as sticks and the unhybridized p-orbitals as lobes for clairity and ease. a. HONO b. CH3 CCH c. C3 H4 d. C2 O4 2-Draw orbital diagrams (boxes with arrows in them) to represent the electron configurations—without hybridization—for all the atoms in PH3. Circle the electrons involved in bonding. Draw a three-dimensional sketch of the molecule and show orbital overlap. What bond angle do you expect from the unhybridized orbitals? How well does valence bond theory agree with theexperimentally measured bond angle of 93.3°?how many sp2 hybridized carbon?
- 1. a) Draw the dominant Lewis structure for the allene molecule (1,2-propyl diene, CH2CCH2 ) and use VSEPR theory to determine the molecule's geometry. In specifying the geometry give all bond angles and specify which nuclei lie in the same plane. b) Propose a hybridization and bonding scheme for the atoms in allene. That is, specify how each of the atoms is hybridized, which atomic orbitals overlap to form bonding molecular orbitals, and the nature (i.e., 0", 7f, etc.) of these molecular orbitals. c) Draw a plausible valence molecular orbital level diagram for allene (include only bonding MOs) based on the results from (b). d) Based on the work from (c) deduce the valence electronic configuration of the ground state of allene. e) Is the molecule planar or nonplanar? Explain your answer1. a) Draw the dominant Lewis structure for the allene molecule (1,2-propyl diene, CH2CCH2 ) and use VSEPR theory to determine the molecule's geometry. In specifying the geometry give all bond angles and specify which nuclei lie in the same plane. b) Propose a hybridization and bonding scheme for the atoms in allene. That is, specify how each of the atoms is hybridized, which atomic orbitals overlap to form bonding molecular orbitals, and the nature (i.e., sigma", pi, etc.) of these molecular orbitals. c) Draw a plausible valence molecular orbital level diagram for allene (include only bonding MOs) based on the results from (b). d) Based on the work from (c) deduce the valence electronic configuration of the ground state of allene. e) Is the molecule planar or nonplanar? Explain your answer Answer subparts c, d, and eBiotin is being studied in a lab. a. What is the IMF(s) of biotin (C10H16N2O3S)? b. What are the sigma/pi bondings and bond angles of biotin? c. What are the resonance functional groups?