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The reason that metal atoms have their own unique type of bonding force is the looseness with which their valence electrons are held in the outer shell This is evident from the fact that the ionization potential of metal atoms is one-half to twothirds that of nonmetal atoms The mean radius of the valence electrons in a free (isolated) metal atom is larger than the interatomic distance of that metal in the solid crystalline state This means that the valence electrons are closer to a nucleus in the solid metal than they are in a free atom, and thus their potential energy is lower in the solid Since the valence electrons are not localized between a pair of positive ions, they are free to move through the solid.

Part II:

Thus the structure of the solid metal is a closepacked arrangement of positive ion cores (the nucleus plus the nonvalence electrons) that is permeated by an electron gas or cloud This ability of the valence electrons to move freely through the solid explains the high thermal and electrical conductivities of metals Also, the fact that the valence electrons are nondirectional (not shared by only two atoms) explains the relatively low strength and high ductility of elemental metals, since the positive ions can move relative to one another without breaking any primary bonds This mechanism is referred to as slip and is discussed in more detail in a following section on crystal structures..

FIGURE 5-2

Downloaded from Digital Engineering Library @ McGraw-Hill (www.digitalengineeringlibrary.com) Copyright 2004 The McGraw-Hill Companies. All rights reserved. Any use is subject to the Terms of Use as given at the website.

Variable items in a SQL statement (such as the table name and search condition in Figure 5-2) are shown in lowercase italics. It s up to you to specify the appropriate item value(s) each time the statement is used. Optional clauses and keywords, such as the WHERE clause in Figure 5-2, are indicated by alternate paths through the syntax diagram. When a choice of optional keywords is offered, the default choice (that is, the behavior of the statement if no keyword is specified) is UNDERLINED.

Maintain independence of applications from lower-level details, while maintaining technology awareness to promote scalability and error robustness Provide usable results over a wide bit rate, ranging from a few kilobits per second to a few megabits per second Reuse encoding tools and data from previous MPEG standards Support identification and management of digital rights Provide interactivity and hyperlinking with individual audiovisual objects simultaneously Handle natural and synthetic information, as well as real-time and non-real-time information, in an integrated fashion Provide the capability to composite and present information according to the user s interaction and needs, as in Virtual Reality

32.2.4 Molecular or van der Waals Bonds In addition to the three strong primary bonds discussed above, there are also several much weaker (and therefore called secondary) bonds which provide the interatomic attractive forces that hold some types of atoms together in a solid material. These forces are referred to as either secondary bonds, molecular bonds, or van der Waals bonds. These bonds are due to residual electrostatic fields between neutral molecules whose charge distribution is not uniform. Covalently bonded atoms frequently form molecules that behave as electric or magnetic dipoles. Although the molecule itself is electrically neutral, there is an electrical imbalance within the molecule. That is, the center of the positive charge and the center of the negative charge do not coincide, and it is this dipole that creates molecular bonding.