Concept explainers
Interpretation: The hybridisation of central O atom in O3 has to be given; also, the bonding in
Concept Introduction: Molecular orbitals are formed by the combination of the atomic orbitals of the atoms in the molecule. The properties of the newly formed molecular orbital will be different from their individual atomic orbitals. In molecular orbital theory, electrons shared by atoms in a molecule reside in the molecular orbitals.
Delocalized molecular orbitals are extended over two or more atoms, these are not confined to adjacent bonding atoms. Therefore, the electrons are free to move around the entire molecule.
The structures that arise due to delocalization of electrons or charges is called as resonance structures or canonical structures. If a species can be represented in resonance structures, the
To Discuss: The hybridisation of central
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Chapter 7 Solutions
CHEMISTRY:ATOMS FIRST (LL)>CUSTOM PKG.<
- Describe the hybridization around the central atom and the bonding in SCl2 and OCS.arrow_forwardThe sulfamate ion, H2NSO3, can be thought of as having been formed from the amide ion, NH2, and sulphur trioxide, SO3. (a) What are the electron-pair and molecular geometries or the amide ion and or SO3? What are the hybridizations of the N and S atoms, respectively? (b) Sketch a structure for the sulfamate ion, and estimate the bond angles. (c) What changes in hybridization do you expect for N and S in the course of the reaction NH2 + SO3 H2NSO3? (d) Is SO3 the donor of an electron pair or the acceptor of an electron pair in the reaction with amide ion? Does the electrostatic potential map shown below confirm your prediction?arrow_forwardAspirin, or acetylsalicylic acid, has the formula C9H8O4 and the skeleton structure (a) Complete the Lewis structure and give the number of bonds and bonds in aspirin. (b) What is the hybridization about the CO2H carbon atom (colored blue)? (c) What is the hybridization about the carbon atom in the benzene-like ring that is bonded to an oxygen atom (colored red)? Also, what is the hybridization of the oxygen atom bonded to this carbon atom?arrow_forward
- Sketch the resonance structures for the N2O molecule. Is the hybridization of the N atoms the same or different in each structure? Describe the orbitals involved in bond formation by the central N atom.arrow_forwarda Nitrogen trifluoride, NF3, is a relatively unreactive, colorless gas. How would you describe the bonding in the NF3 molecule in terms of valence bond theory? Use hybrid orbitals. b Silicon tetrafluoride, SiF4, is a colorless gas formed when hydrofluoric acid attacks silica (SiO2) or glass. Describe the bonding in the SiF4 molecule, using valence bond theory.arrow_forwardWhat is the hybridization of the central atom in each of the following? (a) BeH2 (b) SF6 (c) PO43 (d) PCl5arrow_forward
- Consider the polyatomic ion IO65-. How many pairs of electrons are around the central iodine atom? What is its hybridization? Describe the geometry of the ion.arrow_forwardWhat is the hybridization of the central phosphorus atom of PO43− ?arrow_forwardUse the Molecular Orbital Theory to indicate the bond order, and paramagnetism or diamagnetism of O2, O2+, and O2-.arrow_forward
- What is the state of hybridization of boron and oxygen atoms in boric acid?arrow_forwardWhat is the hybridization of the central atom in the iodite (IO2- ) anion ?arrow_forwardIn ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another. (a)What is the best choice of hybridization scheme for the atoms of ozone? (b) For one of the resonance forms of ozone, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons? (c) Which of the orbitals can be used to delocalize the π electrons? (d) How many electrons are delocalized in the π system of ozone?arrow_forward
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