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Chapter 10: Q9CQ (page 466)

The energy necessary to break the ionic bond between a sodium ion and a fluorine ion is 4.99eV. The energy necessary to separate the sodium and fluorine ions that form the ionic NaFcrystal is 9.30eV per ion pair. Explain the difference qualitatively.

Short Answer

Expert verified

It takes more energy to separate the sodium and fluorine ions than it does to break the link per pair.

Step by step solution

01

- Concept:

Sodium is metal and fluorine is non-metal. So the bond between them can be an ionic bond. Sodium has one valence electron and fluorine is highly electronegative. Sodium needs to lose electrons and fluorine needs to lose electrons to form a chemical bond.

02

Separate the sodium and fluorine ions: 

Here not only break all sodium-fluorine connections but also separate all sodium ions from all fluorine ions in order to separate the sodium and fluorine ions that make up the NaF crystal. Distinguish ions macroscopically since they were just 10 Bohr radii apart. To separate the oppositely charged ions that attract each other requires more energy. As a result, separating the sodium and fluorine ions requires more energy than breaking the connection per pair.

Hence, it takes more energy to separate the sodium and fluorine ions than it does to break the link per pair.

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Most popular questions from this chapter

why is covalent bonding directional, while ionic bonding is not?

The diagram shows a bridge rectifier circuit. A sinusoidal input voltage is fed into four identical diodes. each represented by the standard diode circuit symbol. The symbol indicates the direction of conventional current flow through the diode. The plots show input and output voltages versus time. Note that the output voltage is strictly in one direction. Explain

(a) how this circuit produces the unidirectional output voltage it does, and

(b) what features in the output plot indicate that the band gap of the diodes is about half an electronvolt, (It might seem that about one volt is correct, but consider how many diodes are on and in series at any given instant. In fact, although not the usual habit, it might be more accurate to plot the output voltage shifted upward relative to the input.)

The accompanying diagrams represent the three lowest energy wave functions for three "atoms." As in all truly molecular states we consider, these states are shared among the atoms. At such large atomic separation, however, the energies are practically equal, so anelectron would be just as happy occupying any combination.

(a) Identify algebraic combinations of the states (for instance, 5+11/2+11/2 ) that would place the electron in each of the three atoms.

(b) Were the atoms closer together, the energies of states 1.11, and III would spread out and an electron would occupy the lowest energy one. Rank them in order of increasing energy as the atoms draw closer together. Explain your reasoning.

Question: - (a) Compare equation (10-11) evaluated at room temperature for a silicon band gap of 1.1 eV and for a typical donor-state/conduction band gap of 0.05 eV.

(b) Assuming only one impurity atom for every 10鲁 silicon atoms, do your results suggest that majority carriers, bumped up from donor levels. should outnumber minority carriers created by thermal excitation across the whole 1.1 eV gap? (The calculation ignores the difference in density of states between donor levels and bands, which actually strengthens the argument.)

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?

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