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Chapter 9: Problem 45

(a) What is meant by the term orbital overlap? (b) Describe what a chemical bond is in terms of electron density between two atoms.

Short Answer

Expert verified
(a) Orbital overlap is the interaction between the atomic orbitals of two adjacent atoms, occurring in a spatial region, leading to the formation of molecular orbitals and chemical bonds. (b) A chemical bond in terms of electron density is the region of increased electron density between two atoms due to their interaction and partial sharing of electrons, which stabilizes the system and holds the atoms together.

Step by step solution

01

(a) Orbital Overlap Definition

Orbital overlap refers to the spatial region where the wave functions (orbitals) of two adjacent atoms come together and interact. The atomic orbitals of individual atoms overlap with each other, resulting in the formation of a new type of orbital, known as a molecular orbital. The overlapping region has a higher probability of finding electrons, as they are shared between the two atoms. This interaction leads to the formation of chemical bonds in molecules.
02

(b) Chemical Bond Definition in Terms of Electron Density

A chemical bond in terms of electron density can be described as the region where the electron density is higher between two atoms, due to their interaction and partial sharing of electrons in their respective orbitals. As the atoms approach each other, their atomic orbitals start to overlap, resulting in an increase in electron density between them. This increased electron density stabilizes the system, as it reduces the potential energy between the atoms and holds them together, forming a chemical bond.

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Most popular questions from this chapter

(a) Draw Lewis structures for ethane \(\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)\), ethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\), and acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\). (b) What is the hybridization of the carbon atoms in each molecule? (c) Predict which molecules, if any, are planar. (d) How many \(\sigma\) and \(\pi\) bonds are there in each molecule?

(a) If you combine two atomic orbitals on two different atoms to make a new orbital, is this a hybrid orbital or a molecular orbital? (b) If you combine two atomic orbitals on one atom to make a new orbital, is this a hybrid orbital or a molecular orbital? (c) Does the Pauli exclusion principle (Section 6.7) apply to MOs? Explain.

In which of these molecules or ions does the presence of nonbonding electron pairs produce an effect on molecular shape? (a) \(\mathrm{SiH}_{4}\), (b) \(\mathrm{PF}_{3}\), (c) \(\mathrm{HBr}\), (d) \(\mathrm{HCN}\), (e) \(\mathrm{SO}_{2}\).

Consider the following \(\mathrm{XF}_{4}\) ions: \(\mathrm{PF}_{4}^{-}, \mathrm{BrF}_{4}^{-}, \mathrm{ClF}_{4}^{+}\), and \(\mathrm{AlF}_{4}^{-}\). (a) Which of the ions have more than an octet of electrons around the central atom? (b) For which of the ions will the electrondomain and molecular geometries be the same? (c) Which of the ions will have an octahedral electron-domain geometry? (d) Which of the ions will exhibit a see-saw molecular geometry?

The phosphorus trihalides \(\left(\mathrm{PX}_{3}\right)\) show the following variation in the bond angle \(\mathrm{X}-\mathrm{P}-\mathrm{X}: \mathrm{PF}_{3,}, 96.3^{\circ} ; \mathrm{PCl}_{3}, 100.3^{\circ}\); \(\mathrm{PBr}_{3}, 101.0^{\circ} ; \mathrm{PI}_{3}, 102.0^{\circ}\). The trend is generally attributed to the change in the electronegativity of the halogen. (a) Assuming that all electron domains are the same size, what value of the \(\mathrm{X}-\mathrm{P}-\mathrm{X}\) angle is predicted by the VSEPR model? (b) What is the general trend in the \(\mathrm{X}-\mathrm{P}-\mathrm{X}\) angle as the halide electronegativity increases? (c) Using the VSEPR model, explain the observed trend in \(\mathrm{X}-\mathrm{P}-\mathrm{X}\) angle as the electronegativity of \(\mathrm{X}\) changes. (d) Based on your answer to part (c), predict the structure of \(\mathrm{PBrCl}_{4}\).
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