Concept explainers
Explain how
Interpretation: To explain how the sigma (s) and pi (p) bonds are similar and different.
Concept introduction: A sigma bond is formed by the axial overlap of atomic orbitalsand the pi bonds are formed by the side-to-side overlap of p-orbitals.
Answer to Problem 1E
Similarities: Both sigma and pi bonds are formed by the overlapping of orbital and these bonds are covalent bonds.
Differences: Sigma bond is the strong bond whereas pi bond is weaker in comparison to sigma bond.
Pi bond is formed by the side to side overlapping of atomic orbital whereas sigma bond is formed by the linear (end to end) overlapping of atomic orbital.
Explanation of Solution
The sigma and pi both the bonds are formed by sharing of an electron pair that is both are covalent bonds. The sigma bond is formed when two orbitals overlap axially along the internuclear axis; it is strong bond as it requires very high energy to break. The sigma bonds of molecules give the shape of a molecule as per VSEPR model. The sigma bonds can rotate but the pi bonds cannot because if a pi bond is rotated it will break.
Therefore, the similarity between sigma and pi bonds are that both are formed by the overlap of orbital and both the bonds are covalent bonds that is it involves a bond pair. The difference between sigma and pi bonds are that sigma bond is the strongest bond while pi bonds are weaker as compared to sigma bond. Sigma bond is formed by linear overlap of atomic orbital while the pi bond is formed by side-to-side overlap of atomic orbital. Sigma bond gives the shape while a pi bond gives the length of a molecule. Sigma bond is free to rotate around its axis while the pi bond cannot rotate it is locked.
Similarities: Both sigma and pi bonds are formed by the overlapping of orbital and these bonds are covalent bonds.
Differences: Sigma bond is the strong bond whereas pi bond is weaker in comparison to sigma bond.
Pi bond is formed by the side to side overlapping of atomic orbital whereas sigma bond is formed by the linear (end to end) overlapping of atomic orbital.
Want to see more full solutions like this?
Chapter 8 Solutions
Chemistry by OpenStax (2015-05-04)
Additional Science Textbook Solutions
College Physics
Chemistry: A Molecular Approach (4th Edition)
Organic Chemistry (8th Edition)
Organic Chemistry
Chemistry: A Molecular Approach
Chemistry: The Central Science (13th Edition)
- hy do atoms form bonds with one another? What can make a molecule favored compared with the lone atoms?arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forwardWhat aspect of the following Lewis structure indicates that the concept of coordinate covalency is needed to explain the bonding in the molecule?arrow_forward
- Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.arrow_forwardBased on average bond enthalpies, would you expect a photon capable ofdissociating a C¬Cl bond to have sufficient energy to dissociate a C¬Br bond?arrow_forward13) The average C−C bond dissociation energy (D) is 350 kJ/mol and the average C=C bond dissociation energy is 728 kJ/mol. Based on these values, which is stronger: a σ or a π bond?arrow_forward
- Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction:2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(g)2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(g) Note that the average bond energy for the breaking of a bond in CO2CO2 is 799 kJ/molkJ/mol. Use average bond energies to calculate ΔHrxnΔHrxn for this reaction.arrow_forwardExplain Bond Dissociation Energy ?arrow_forwardHow is the partial ionic character of a bond in a diatomic molecule related to ΔEN for the bonded atoms? Why?arrow_forward
- The bond energy for C-H bond is about 413 kJ/mol in CH4 but 380 kJ/mol in CHBr3. Although these values are relatively close in magnitude, they are different. Explain why they are different. Does the fact that the bond energy is lower in CHBr3, make any sense? Why?arrow_forwardCompare the bond enthalpies of the carbon-carbon single and triple bonds. Based on this information, what is the average π-bond contribution to bond enthalpy in C≡C? Compare the bond enthalpies of the nitrogen-nitrogen single and triple bonds. Based on this information, what is the average π-bond contribution to bond enthalpy in N≡N?arrow_forwardCalculate ΔH ° for the reaction H2( g) + Br2( g)¡2 HBr( g) using the bond energy values. The ΔH °f of HBr(g) is not equal to one-half of the value calculated. Account for the difference.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning