Concept explainers
Interpretation: Determine the reason for the fact that the number of atomic orbitals combined is always the same as that of the hybrid orbitals formed.
Concept Introduction: The mathematical process where the standard atomic orbitals are joined to make new atomic orbitals is called hybridization. The new atomic orbitals so formed are called hybrid orbitals which are localized on individual atoms. However, they have distinctive shapes and energies when compared to those of the standard atomic orbitals. They are important in valence bond hypothesis since they relate all the more intently to actual electron distribution that exists in
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- 7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?arrow_forward7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals?arrow_forwardLets look more closely at the process of hybridization. (a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them? (b) Do hybrid atomic orbitals form between different p orbitals without involving 5 orbitals? (c) What is the relationship between the energy of hybrid atomic orbitals and the atomic orbitals from which they are formed?arrow_forward
- Aspartame is a compound that is 200 times sweeter than sugar and is used extensively (under the trade name NutraSweet) in diet soft drinks. The skeleton structure of the atoms in aspartame is (a) Complete the Lewis structure and give the number of and bonds in aspartame. (b) What is the hybridization about each carbon atom that forms a double bond with an oxygen atom? (c) What is the hybridization about each nitrogen atom?arrow_forward7.88 The N5+ cation has been synthesized and studied. Consider the possible Lewis structure below. Indicate the hybridization expected for each nitrogen atom and the expected bond angles. Assuming that the structure shown above is correct, how many of the five nitrogen atoms would always lie in the same plane?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
- 7.96 Consider the hydrocarbons whose structures are shown below. Which of these molecules would be planar, meaning that all of the atoms must lie in the same plane? Explain your answer in terms of orbital hybridizations.arrow_forwardIn each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.arrow_forwardHow many and bonds are present in the molecule HCN?arrow_forward
- What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?arrow_forwardWhy is it important to understand the concept of orbital hybridization?arrow_forwardConsider the following forms of oxygen species: 0, 02, 02, and 0₂ a) Provide the orbital diagrams and show the correct electron configurations for the four species? b) Calculate the bond order in each case. c) Order the species from lowest to highest ionization energy. Explain your answer.arrow_forward
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