Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 3, Problem 6CTQ
Interpretation Introduction
Interpretation: The reason behind each orbital of
Concept introduction: Two or more of orbitals undergo redistributions of their different energies so as to form mathematically averaged orbitals in terms of energy although they may differ in shape and orientation. The energy and orientation of the new hybrid orbital depends upon by the kind and number of orbitals used in the hybridization.
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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.
Out of p-orbital and sp-hybrid orbital which has greater directional character and Why?
2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew.
b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.
Chapter 3 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 3 - Prob. 1CTQCh. 3 - What neutral atom is represented by the electron...Ch. 3 - Prob. 3CTQCh. 3 - Consider any one of the four identical hybrid...Ch. 3 - Prob. 5CTQCh. 3 - Prob. 6CTQCh. 3 - Prob. 7CTQCh. 3 - Prob. 8CTQCh. 3 - Prob. 9CTQCh. 3 - Prob. 10CTQ
Ch. 3 - On the left side of Figure 3.6, label the areas...Ch. 3 - Prob. 12CTQCh. 3 - Prob. 13CTQCh. 3 - Prob. 14CTQCh. 3 - Prob. 15CTQCh. 3 - Now consider the fully formed molecule on the...Ch. 3 - Prob. 1ECh. 3 - Explain why the two molecules below cannot...Ch. 3 - Prob. 3ECh. 3 - Consider the incomplete orbital representation of...Ch. 3 - Consider the following orbital representation of...Ch. 3 - Summarize how one determines the hybridization...Ch. 3 - Explain what is wrong with each of the following...Ch. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Complete the following tables, and memorize their...Ch. 3 - Draw orbital representations of bonding in water...Ch. 3 - Draw electron configuration diagrams for carbon in...Ch. 3 - Prob. 13E
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- Give the shape that describes each hybrid orbital set: (a) sp2 (b) sp3d (c) sp (d) sp3d2arrow_forwardThere are two compounds with the molecular formula HN3. One is called hydrogen azide; the other is cyclotriazene. (a) Write the Lewis structure for each compound. (b) Designate the hybridization of each nitrogen in hydrogen azide. (c) What is the hybridization of each nitrogen in cyclotriazene? (d) How many sigma bonds are in hydrogen azide? In cyclotriazene? (e) How many pi bonds are in hydrogen azide? In cyclotriazene? (f) Give approximate values for the N-to-N-to-N bond angles in each molecule.arrow_forwardIn 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?arrow_forward
- 9. How many hybrid orbitals does a carbon atom have in an SP3 hybrid state? Draw the shape of the hybrid orbital.arrow_forwardIndicate what kind of bonding orbital is formed when the following atomic or hybridized atomic orbitals are combined as shown for each pair of orbitals described below. Please write out your answers using words (options: sigma, pi, or no bond formed). A: an sp3 orbital and an s orbital B: two pz orbitals in a side-to-side fashion C: two px orbitals in a head-to-head fashion D: a px orbital and a pz orbitalarrow_forward2. Complete the table for the indicated compounds Molecule C2H2 SF5- NO3- Lewis structure include lone pairs & formal charges on each atom Resonance structures don't have to include lone pairs; write N/A if there are none Electron Geometry Hybridization on central atom Overlapping orbitals include value of n in the orbital name (e.g. 1s, not s). Write N/A if that kind of bond is not present in the molecule T: Molecular Geometry Bond angle(s) include < as necessary 3D structure and polarity don't have to include lone pairs; draw the |dipole arrow on the molecule or write "non- polar"arrow_forward
- The pyridine molecule C5H5N has a planar geometry. What is the hybridization of each atom in the ring? Draw a diagram to show all the hybrid orbitals (in one color) and the pz orbitals (in a different color) contributing to the pi MO. Is the molecule aromatic? The thiophene molecule is also planar. What is the hybridization of each atom in the ring? Draw a diagram to show all the hybrid orbitals (in one color) and the pz orbitals (in a different color) contributing to the pi MO. Is the molecule aromatic?arrow_forward4. Silicon is an interesting atom because it behaves similarly to carbon. There is speculation in the scientific field that aliens could be made of silicon structures rather than carbon. The following structures are silicon versions of important carbon signaling molecules in our body. 1.) What is the electron geometry and hybridization for each of these structures? H-Si-H H-H Silane Silanone Silicon Dioxide e geometry: e geometry: hybridization: e geometry: hybridization: hybridization: 2.) Based on what you have described above, match the orbital diagram below with the correct molecule above:arrow_forwardRecall that for a lone pair to be involved in resonance, it must be in a p orbital, which requires the atom it is on to be sp² or sp hybridized. This means that for a situation with resonance, the actual hybridization of the atom is determined from the resonance structure where that atom has the lowest steric number (so it can use the required number of p orbitals to form pi bonds as shown in some of its resonance structures). This could be the situation in your initial drawing, or in one of the resonance structures you draw from it. All of the oxygens in the following molecules are sp² hybridized except one. Which of the following structures has an sp³ hybridized oxygen atom? НО. (A) (B) (D)arrow_forward
- According to valence bond theory, what is the total number of sp2 hybridized orbitals on all the atoms in formaldehyde, CH2O? Sketch and explain why. According to valence bond theory, how many lone pairs of electrons reside in sp hybridized orbitals in formaldehyde? explain why?arrow_forwardGive the shape that describes each hybrid orbital set.arrow_forwardWhich atomic orbitals from carbon hybridize to form the bonds in CH4? А) 1s, 2рх, 2p_у, 2p_z В) 2s, 2px, 2p_у, 2р_z С) 3s, Зрх, 2р_у, 2р_z D) 2s, 2px, 2p_yarrow_forward
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