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Chapter 11: Problem 7

For each of the following species, identify the central atom(s) and propose a hybridization scheme for those $\operatorname{atom}(\mathrm{s}):(\mathrm{a}) \mathrm{CO}_{2} ;(\mathrm{b}) \mathrm{HONO}_{2} ;(\mathrm{c}) \mathrm{ClO}_{3}^{-} ;(\mathrm{d}) \mathrm{BF}_{4}^{-}$

Short Answer

Expert verified
The central atom and its hybridization for the given species are: (a) CO2: Central atom is C, hybridization is sp. (b) HONO2: Central atom is N, hybridization is sp2. (c) ClO3^-: Central atom is Cl, hybridization is sp3. (d) BF4^-: Central atom is B, hybridization is sp3.

Step by step solution

01

Identify the Central Atom

For each molecule or ion, identify the central atom(s):(a) In CO2, the central atom is C (Carbon).(b) In HONO2, the central atom is N (Nitrogen).(c) In ClO3^-, the central atom is Cl (Chlorine).(d) In BF4^-, the central atom is B (Boron).
02

Determine the Hybridization

Next, determine the hybridization of each central atom:(a) In CO2, Carbon is double bonded to two Oxygen atoms which leads to a sp hybridization.(b) In HONO2, Nitrogen is bonded to three different groups (one hydrogen, one oxygen double bonded, one O-NO2 group), which is a trigonal planar arrangement and therefore it has sp2 hybridization.(c) In ClO3-, Chlorine is bonded to three oxygen atoms and has one lone pair of electrons which leads to a sp3 hybridization.(d) In BF4^-, Boron is bonded to four Fluorine atoms and so has a sp3 hybridization.

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Most popular questions from this chapter

Describe the molecular geometry of \(\mathrm{CCl}_{4}\) suggested by each of the following methods: (a) Lewis theory; (b) valence-bond method using simple atomic orbitals; (c) VSEPR theory; (d) valence-bond method using hybridized atomic orbitals.

A conjugated hydrocarbon has an alternation of double and single bonds. Draw the molecular orbitals of the \(\pi\) system of 1,3,5 -hexatriene. If the energy required to excite an electron from the HOMO to the LUMO corresponds to a wavelength of \(256 \mathrm{nm},\) do you expect the wavelength for the corresponding excitation in 1,3,5,7 -octatetraene to be a longer or shorter wavelength?

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Which of these diatomic molecules do you think has the greater bond energy, \(\mathrm{Li}_{2}\) or \(\mathrm{C}_{2} ?\) Explain.

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