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Chapter 10: 7CQ (page 413)

For the four kinds of crystal binding – covalent, ionic, metallic, and molecular- how would the destiny of valence electrons vary throughout the solid? Would it be constant, centered on the atoms, or largest between the atoms? Or would it alternate, with a net charge density positive at one atom and negative at the next?

Short Answer

Expert verified

The valence electrons are strongly linked to the atoms in a molecular solid. As a result, the valence electron density will be concentrated around the atoms.

Step by step solution

01

Definitions of crystal bindin

All valence electrons are bound into bonds between neighboring atoms in a covalent solid. As a result, the valence electron density will be the highest among the atoms.

02

The destiny of valence electrons

Electrons are held from one side to the other in an ionic solid. When the ions with different signs alternate, the lowest energy state is reached. As a result, the density of valence electrons will alternate, with a positive net charge density on one ion and a negative charge density on its closest neighbors.

All atoms in a metallic solid share valence electrons. They combine to create an electron gas. As a result, the valence electron density remains constant.

The valence electrons are strongly linked to the atoms in a molecular solid. As a result, the valence electron density will be concentrated around the atoms.

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Most popular questions from this chapter

Question: The critical temperature lead is 7.2 K. What is the binding energy of its Cooper pairs at zero temperature?

Electron affinity is a property specifying the "appetite" of an element for gaining electrons. Elements, such as fluorine and oxygen that lack only one or two electrons to complete shells can achieve a lower energy state by absorbing an external electron. For instance, in uniting an electron with a neutral chlorine atom, completing its n = 3 shell and forming a CI ion, 3.61 eV of energy is liberated. Suppose an electron is detached from a sodium atom, whose ionization energy is 5.14 eV.Then transferred to a (faraway) chlorine atom.

(a) Must energy on balance be put in by an external agent, or is some energy actually liberated? If so How much?

(b) The transfer leaves the sodium with a positive charge and the chlorine with a negative. Energy can now be extracted by allowing these ions to draw close forming a molecule. How close must they approach to recover the energy expended in part (a)?

(c)The actual separation of the atoms in a NaCl molecule is 0.24 nm. How much lower in energy is the molecule than the separated neutral atoms?

Upon what definitions do we base the claim that the Ψ2px and Ψ2py states of equations 10−1 are related to x and y just as Ψ2pz is to z.

The effective force constant of the molecular “spring” in HCL is 480 N/m, and the bond length is 0.13 nm.

(a) Determine the energies of the two lowest-energy vibrational states.

(b) For these energies, determine the amplitude of vibration if the atoms could be treated as oscillating classical particles.

(c) For these energies, by what percentages does the atomic separation fluctuate?

(d) Calculate the classical vibrational frequencyωvh=k/μand rotational frequency for the rotational frequencyωrot=L/I, assume that L is the its lowest non zero value, 1(1+1)hand that the moment of inertia Iis μa2.

(e) Is is valid to treat the atomic separation as fixed for rotational motion while changing for vibrational?

Section 10.2 gives the energy and approximate proton separation of the H2+ molecule. What is the energy of the electron alone?
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