Organic Chemistry (8th Edition)
8th Edition
ISBN: 9780134042282
Author: Paula Yurkanis Bruice
Publisher: PEARSON
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Textbook Question
Chapter 1.7, Problem 28P
Explain why a σ bond formed by overlap of s orbital with an sp3 orbital of carbon is stronger than a σ bond formed by overlap of an s orbital with a p orbital of carbon.
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Explain why a s bond formed by overlap of an s orbital with an sp3 orbital of carbon is stronger than a s bond formed by overlap of an s orbital with a p orbital of carbon.
Explain why a o bond formed by overlap of an s orbital with an sp orbital of carbon is stronger than a o bond formed by overlap of an s orbital with a p orbital of carbon.
Because s orbital of carbon is more symmetrical than p orbital of carbon atom.
The electron density of the large lobe of an sp orbital is less than the electron density of a lobe of a p orbital. Therefore, the overlap of an s orbital with an sp orbital forms a weaker bond than the overlap of an
orbital
with
ap orbital.
The electron density of the large lobe of an sp orbital is less than the electron density of a lobe of a p orbital. Therefore, the overlap of an s orbital with an sp3 orbital forms a stronger bond than the overlap of an s orbital
with a p orbital.
The electron density of the large lobe of an sp orbital is greater than the electron density of a lobe of ap orbital. Therefore, the overlap of an s orbital with an sp orbital forms a stronger bond than the overlap of an s
orbital with ap orbital.
In O=C-O, the sigma bonds arise from the overlap of
Half-filled p orbitals
Half-filled hybridized orbitals
Completely filled p orbitals
O Completely filled hybridized orbitals
Chapter 1 Solutions
Organic Chemistry (8th Edition)
Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - a. How many protons do the following species...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 4PCh. 1.2 - a. Write the ground-state electronic configuration...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar? a. b. c. d.Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...
Ch. 1.3 - Explain why HCL has a smaller dipole moment than...Ch. 1.3 - After examining the potential maps for LiH, HF,...Ch. 1.4 - An atom with a formal charge does not necessarily...Ch. 1.4 - Prob. 16PCh. 1.4 - a. Draw two Lewis structure for C2H6O. b. Draw...Ch. 1.4 - Draw the lone-pair electrons that are not shown in...Ch. 1.4 - Prob. 20PCh. 1.4 - Which of the atoms in the molecular models in...Ch. 1.4 - Prob. 22PCh. 1.4 - Prob. 23PCh. 1.5 - Draw the following orbitals: a. 3s orbital b. 4s...Ch. 1.6 - Prob. 25PCh. 1.6 - Indicate the kind of molecular orbital (, , , or )...Ch. 1.7 - What orbitals are used to form the 10 sigma bonds...Ch. 1.7 - Explain why a bond formed by overlap of s orbital...Ch. 1.9 - Put n number in each of the blanks: a. __ s...Ch. 1.9 - For each of the given species: a. Draw its Lewis...Ch. 1.11 - Predict the approximate bond angles in a. the...Ch. 1.11 - According to the potential map for the ammonium...Ch. 1.12 - Prob. 35PCh. 1.13 - a. What are the relative lengths and strengths of...Ch. 1.13 - Prob. 38PCh. 1.14 - Describe the orbitals used in bonding and the bond...Ch. 1.15 - Which of the bond in a carbon-oxygen double bond...Ch. 1.15 - Would you expect a CC bond formed by sp2sp2...Ch. 1.15 - Caffeine is a natural insecticide found in the...Ch. 1.15 - a. What is the hybridization of each of the carbon...Ch. 1.15 - Predict the approximate bond angles for a. the CNC...Ch. 1.16 - What of the following molecules would you expect...Ch. 1.16 - Account for the difference in the shape and color...Ch. 1.16 - If the dipole moment of CH3F is 1.847 D and the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 50PCh. 1 - What is the hybridization of all the atoms (other...Ch. 1 - Draw the condensed structure of a compound that...Ch. 1 - Predict the approximate bond angles: a. the CNH...Ch. 1 - Prob. 54PCh. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - What is the hybridization of each of the carbon...Ch. 1 - Rank the bonds from most polar. a. CO, CF, CN b....Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 59PCh. 1 - What is the hybridization of the indicated atom in...Ch. 1 - Predict the approximate bond angles for the...Ch. 1 - Prob. 62PCh. 1 - Draw the missing lone-pair electrons and assigns...Ch. 1 - a. Which of the indicated bonds in each molecule...Ch. 1 - For each of the following molecules, indicate the...Ch. 1 - Draw a Lewis structure for each of the following:...Ch. 1 - Prob. 67PCh. 1 - Rank the following compounds from highest dipole...Ch. 1 - In which orbitals are the lone pairs in nicotine?Ch. 1 - Prob. 70PCh. 1 - Prob. 71PCh. 1 - a. Which of the species have bond angles of 109.5?...Ch. 1 - Prob. 73PCh. 1 - Which compound has a larger dipole moment: CH3Cl...Ch. 1 - Prob. 75PCh. 1 - Explain why CH3Cl has a greater dipole moment than...Ch. 1 - a. Draw a Lewis structure for each of the...Ch. 1 - There are three isomers with molecular formula...
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- For which of the following compounds is the lone pair on nitrogen in a p-orbital? ( it can be more than 1 compound)arrow_forwardCharacterize the labeled bonds: give the atom and the orbital (atomic orbitals and/or hybridized atomic orbitals used to create each bond. HA C=C CH3 C=c_ H 2)arrow_forward11. In the structure shown, which of the following characterizations regarding the bonds is false? H-CEC-N=N-H A. The C-C triple bond contains two π-bonds formed from the overlap of sp-hybridized orbitals. B. The C-C triple bond contains two π-bonds formed from the overlap of p-orbitals. C. The C-C triple bond contains one σ-bond formed from the overlap of sp-hybridized orbitals D. The N-N double bond contains one σ-bond formed from the overlap of sp²-hybridized orbitals.arrow_forward
- What is the electron geometry and hybridization of the carbon atoms in H,C=CH,? O The electron geometry of the 2 carbons is trigonal planar with a sp hybridization. O The electron geometry of the 2 carbons is trigonal planar with a sp3 hybridization. The electron geometry of the 2 carbons is trigonal planar with a sp2 hybridization.arrow_forwardHyperconjugation is the interaction of electrons in the bonding sigma orbital with the empty p orbital of positively charged carbon. True or falsearrow_forwardAccording to valence bond theory, which description is TRUE for the carbon atom of formaldehyde (CH₂O)? H 910 H Three sp³ hybridized orbitals and an unhybridized p orbital Three sp2 hybridized orbitals and an unhybridized p orbital Two sp2 hybridized orbitals and one sp orbital Three sp3 hybridized orbitals There are three sp² hybridized orbitalsarrow_forward
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