Find the hybrid orbital type for each atom, the carbon-carbon-oxygen bond angle, the molecular geometry of oxygen, and the number of sigma and pi bonds in the molecule.
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- A student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.In Chapter 6, we study a group of organic cations called carbocations. Following is the structure of one such carbocation, the tert-butyl cation. (a) How many electrons are in the valence shell of the carbon bearing the positive charge? (b) Using VSEPR, predict the bond angles about this carbon. (c) Given the bond angle you predicted in (b), what hybridization do you predict for this carbon?Using cartoon representations, draw a molecular orbital mixing diagram for a CO bond. In your picture, consider the relative energies of C and O and how this changes the resulting bonding and antibonding molecular orbitals relative to a CC bond.
- The molecule shown below is called furan. It is represented intypical shorthand way for organic molecules, with hydrogenatoms not shown, and each of the 4 vertices representing acarbon atom.(a) What is the molecular formula for furan? (b) How manyvalence electrons are there in the molecule? (c) What isthe hybridization at each of the carbon atoms? (d) Howmany electrons are in the p system of the molecule? (e) TheC¬C¬C bond angles in furan are much smaller than thosein benzene. The likely reason is which of the following: (i) Thehybridization of the carbon atoms in furan is different fromthat in benzene, (ii) Furan does not have another resonancestructure equivalent to the one above, or (iii) The atoms in afive-membered ring are forced to adopt smaller angles than ina six-membered ring.PLS REFER TO THE PICTURE BELOW 1. How many covalent bonds are in the picture? 2. How mant type/s of covalent bond/s forming your double bond do you see? 3. What is/are the types of covalent bond/s forming your double bond do you see? 4. What type of hybrid orbital is the sigma bond? 5. Which electron configuration will you expect the highest energy needed to remove a valence electron?How many sp, sp2, and sp3 carbons are present in a Capsaicin? What is the hybridization around N atom? How many pi bonds are present over the whole molecule (Capsaicin)? sp: sp2: sp3: N: pi bonds: Note: The image below contains a Capsaicin Lewis Structure for the question above. Thank you.
- Draw the following molecule and answer the questions below. H3CCHCHC(O)CH2CCH What is the hybridization/bonding orbital of the bolded atom? What is the hybridization of the bonded atom?For each of the following molecules (in which the central atom is underlined), classify it according to the AXnEm nomenclature of the VSEPR theory, draw the 3-dimensional structure, showing all valence shell electrons of all atoms, draw the net dipole moment vector (if one exists) on the structure diagram, name the hybrid atomic orbitals used by the central atom for σ bonding and name the orbitals used by the central atom for π bonding (if applicable). Molecule or Ion SbOCl3 ArOF4 a. AXE formula b. 3-dimensional structure c. Indicate the net dipole moment vector (if any) on this diagram. d. σ- bonding orbitals used by the central atom e. π-bonding orbitals used by the central atomGiven the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule. SF6* XeF2* SnCl4 A=Bonding electronsB= Sigma-bondsC =Nonbonding electron pairsD= Hybrid orbitals havingnonbonding electron pairsE =Hybrid orbitals usedF= 3-D structure (NAME)G =Polar (P) or nonpolar (NP) MOLECULE OR ION LEWIS STRUCTURE A B C D E F G
- This bond is made of an sp3 orbital from a carbon atom to a 1s orbital from the H atom. The correct orbital overlap is sp3-s. What type(s) of orbital overlap is(are) indicated on the following structure: -sp3-sp -sp2-s -sp3-s -p-p -sp3-sp2Draw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. ??3??2??) give the structure around the bold atom.In the molecule shown label the indicated bonds with either their hybridization (sp,sp2,sp3) or the type of bond present (sigma, pi )