Concept explainers
(a)
Interpretation:
The electron geometries of all nonhydrogen atoms in the four listed species are to be determined.
Concept introduction:
Electron geometry around an atom is determined on the basis of the Valence Shell Electron Pair Repulsion (VSEPR) Theory. Electron geometry describes the orientation of the electron groups in an atom’s valence shell. An electron group is a lone pair or a bond between the two atoms. The bond, whether a single, double or triple, counts as just one electron group.
Since all electrons have the same charge, the electron groups repel each other. They try to move (orient themselves) as far away from each other as possible in order to minimize these repulsions. This results in a linear geometry (
The number of electron groups and geometry is determined on the basis of the Lewis structure of the molecule/ion.
(b)
Interpretation:
The hybridization of all nonhydrogen atoms in the given four species is to be determined.
Concept introduction:
The concept of hybridization of atomic orbitals is used in Valence Bond (VB) Theory to account for the electron and molecular geometry around an atom. A hybrid orbital is a combination of one or more atomic orbitals from the valence shell of an atom. It typically involves an s orbital and a number of p orbitals from the valence shell, resulting in the same total number of hybrid orbitals of the same energy and shape. In heavy atoms, those from Group 3 onward, the valence shell d orbital may also be involved if the atom has an expanded octet. The orientation of these orbitals is same as the electron geometry of the atom. The number of hybrid orbitals required is the same as the number of electron groups. If the number of electron groups is two, two hybrid orbitals are needed. These are formed by a combination of the s and one p orbital, giving
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Chapter 3 Solutions
Organic Chemistry: Principles and Mechanisms (Second Edition)
- Describe the hybridization around the central atom and the bonding in SCl2 and OCS.arrow_forwardH2CO molecules (a) use orbital hybridization theory to determine the molecular shape of h2co. (b) what bonds are formed between the c and o atoms in formaldehyde molecules?arrow_forwardButadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths: (a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.arrow_forward
- Describe the molecular geometry and hybridization of the N, P, or S atoms in each of the following compounds. (a) H3PO4, phosphoric acid, used in cola soft drinks (b) NH4NO3, ammonium nitrate, a fertilizer and explosive (c) S2Cl2, disulfur dichloride, used in vulcanizing rubber (d) K4[O3POPO3], potassium pyrophosphate, an ingredient in some toothpastesarrow_forwardDescribe the molecular geometry and hybridization of the N, P, or S atoms in each of the following compounds.(a) H3PO4, phosphoric acid, used in cola soft drinks(b) NH4NO3, ammonium nitrate, a fertilizer and explosive(c) S2Cl2, disulfur dichloride, used in vulcanizing rubber(d) K4[O3POPO3], potassium pyrophosphate, an ingredient in some toothpastesarrow_forwardThe Lewis structure of BH2Cl (a) Is the molecule polar or nonpolar? (b) What is the hybridization of the carbon atom? (c) What is the geometric shape of the molecule?arrow_forward
- Draw a Lewis electron dot diagram for each of the follow- ing molecules and ions. Formulate the hybridization for the central atom in each case and give the molecular geometry. (a) BF3 (b) BH4- (c) PH3 (d) CS2 (e) CH3+arrow_forwardDraw the molecular orbital energy diagrams for the valence electrons in the following diatomic molecules. Calculate the bond order and indicate if each of them is diamagnetic or paramagnetic. (а) В> (b) С. (c) CO (d) NO (е) Оzarrow_forward(a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forward
- 10.What is the hybridization of the central atom in each of the following? (a) BeH2 (b) SF6 (c) PO43− (d) PCl5arrow_forwardBorane (BH3) is unstable under normal conditions, but it has been detected at lowpressure.(a) Draw the Lewis structure for borane.(b) Draw a diagram of the bonding in BH3, and label the hybridization of each orbital.(c) Predict the H¬B¬H bond anglearrow_forwardWhich of the following molecules does not have a dipole moment? (a) CH3Cl (b) CH2Cl2 (c) CFCl3 (d) CHCl3arrow_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