Concept explainers
(a)
Interpretation:
Sigma and pi bond in
Concept Introduction:
Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.
Pi (π) bonds are the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule.
Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.
Geometry of different types of molecule with respect to the hybridizations are mentioned below,
(a)
Explanation of Solution
Given molecule is
The Lewis electron dot structure for
.
Sigma bond and pi bonds in the molecule are marked below:
(b)
Interpretation:
Sigma and pi bond in
Concept Introduction:
Refer to (a).
(b)
Explanation of Solution
Given molecule is
The Lewis electron dot structure for
.
Sigma bond and pi bonds in the molecule are marked below:
(c)
Interpretation:
Sigma and pi bond in
Concept Introduction:
Refer to (a).
(c)
Explanation of Solution
Given molecule is
The Lewis electron dot structure for
.
Sigma bond and pi bonds in the molecule are marked below:
(d)
Interpretation:
Sigma and pi bond in
Concept Introduction:
Refer to (a).
(d)
Explanation of Solution
Given molecule is
The Lewis electron dot structure for
Sigma bond and pi bonds in the molecule are marked below:
Want to see more full solutions like this?
Chapter 7 Solutions
Chemistry: The Molecular Science, Hybrid Edition (with OWLv2 24-Months Printed Access Card)
- What is the hybridization of the central phosphorus atom of PO43− ?arrow_forwardCompounds such as NaBH4, Al(BH4)3, and LiAlH4 are complexhydrides used as reducing agents in many syntheses.(a) Give the oxidation state of each element in these compounds.(b) Write a Lewis structure for the polyatomic anion in NaBH4, and predict its shape.arrow_forwardExplain chemically nonequivevalent hydrogen.arrow_forward
- what is the lewis structure of ICl4-and what is its geometry?arrow_forwardIn developing a Lewis structure for NO +, the nitroxonium ion, how many valence electrons must you account for?arrow_forwardAcetylene 1C2H22 and nitrogen 1N22 both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) Byreferring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O51g2 and of acetylene to formCO21g2 and H2O1g2. (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O51g2 is 11.30 kJ>mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning