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Chapter 14: Q14.9E (page 599)

Why do we hybridize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from the hybrid orbitals, σ or π? Explain.

Short Answer

Expert verified

The hybridization of atomic orbitals takes place as hybrid orbitals are more directional in nature due to which they overlap better while forming bonds and the bonds formed are stronger in nature.

Step by step solution

01

– Hybridization

Hybridization is the mixing of pure atomic orbitals to of nearly same energy to give hybrid orbitals. The number of hybrid orbitals formed is equal to the number of pure atomic orbitals combined.

The hybridization of atomic orbitals takes place as hybrid orbitals are more directional in nature due to which they overlap better while forming bonds and the bonds formed are stronger in nature.

02

– Sigma and pi bonds

$π$ bonds are formed due to side by side overlapping between unhybridized p or d orbitals. Hybrid orbitals form σ bonds.

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Most popular questions from this chapter

The diatomic molecule OH exist in the gas phase. OH plays an important role in combustion reaction and is a reactive oxidizing agent in polluted air. The bond length and bond energy have been measured to be 97.06 pm and 424.7 kJ/mol, respectively. Assume that the OH molecule is analogous to the HF molecule discussed in the chapter and that the MOs result from the overlap of p_z orbital from oxygen and 1s orbital of hydrogen. (The O-H bond lies along the z-axis)

a. Draw a picture of the sigma bonding and antibonding molecular orbitals in OH.

b. Which of the two MOs has the greater hydrogen 1s character?

c. Can the 2px orbital of oxygen form MOs with 1s orbital of hydrogen? Explain.

d. Knowing that only the 2p orbitals of oxygen interact significantly with the 1s orbital of hydrogen, complete the MO diagram for OH. Place the correct number of electrons in the energy level.

e. Estimate the bond order for OH

f. Predict whether the bond order of OH⁺ is greater than, lesser than, or the same as that of OH+. Explain.

Many important compounds in the chemical industry are derivatives of ethylene $(C_{2} H_{4})$ . Two of them are acrylonitrile and methyl methacrylate.

Complete the Lewis structures for these molecules, showing all lone pairs. Give approximate values for bond angles a through f, and give the hybridization of all carbon atoms. In acrylonitrile and methyl methacrylate indicate which atoms in each molecule must lie in the same plane. How many s bonds and how many p bonds are there in acrylonitrile and methyl methacrylate?

For each of the following chemical formulas, an NMR spectrum is described, including relative overall areas (intensities) for the various signals given in parentheses. Draw the structure of a compound having the specific formula that would give the described NMR spectrum. Hint: All of these formulas represent organic compounds. Lewis structures for organic compounds typically have all atoms in the compound with a formal charge of zero. This is the case in this problem.)

a. $C_{2} H_{3} {Cl}_{3}; NMR$ has one singlet signal.

b. $C_{3} H_{6} {Cl}_{2}; NMR$ has a triplet (4) and a quintet (2) signal.

c. $C_{3} H_{6} O_{2}$ ; NMR has a singlet (1), a quartet (2), and a triplet (3)signal.

d. $C_{5} H_{10} O$ ; NMR has a heptet (1), a singlet (3), and a doublet (6) signal.

e. $C_{3} H_{6} O; NMR$ has a triplet (3), a quintet (2), and a triplet (1) signal.

Arrange the following from lowest to highest ionization energy: $O_{1} O_{2}, O_{2}^{-}, {O_{2}}^{+}$ . Explain your answer.

The infrared spectrum of ${}^{1}{H^{79}} B r$ shows the role="math" localid="1663823566071" $v = 0 t o v = 1$ transition at $2650 c m^{- 1}$ . Determine the vibrational force constant for the HBr molecule. The atomic mass of ${}^{1}H$ is 1.0078, and the atomic mass of ${}^{79}B r$ is 78.918u.

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