Electron-sea model, of metals

The physical properties of metals are attributed to the electron sea model of metallic bonds shown on the right. Metals conduct heat and electricity because electrons are not associated with the bonding between two specific atoms and they are able to flow through the material. They are called delocalized electrons. Metals are lustrous because electrons at their surface reflect light at many different wavelengths. 

The physical properties of metals are attributed to the electron sea model of metallic bonds shown on the right. Metals conduct heat and electricitybecause... 

A Figure 12.20 Electron-sea model of metallic bonding. The valence electrons delocalize to form a sea of mobile electrons that surrounds and binds together an extended array of mefal ions. 

Bonding in Solids I The Electron-Sea Model of Metallic Bonding... 

The electron-sea model of metallic bonding pictures metal atom cores aligned in a "sea" of delocalized electrons. The model accounts for phase changes, mechanical behavior, and electrical and thermal conductivity of metals. 

Bonding in Solids 1 The Electron-Sea Model of Metallic Bonding 382 Bonding in Solids II Band Theory 382 CHAPTER REVIEW GUIDE 385 PROBLEMS 386... 

I The electron-sea model of metallic bonding is described briefly in Section 9.7 see Figure 9.18. 

The electron-sea model of metals is a simplified view that accounts in only a qualitative way for properties of a metal such as electrical conductivity. Molecular orbital theory gives a more detailed picture of the bonding in a metal and other solids as well. ... 

The electron sea model of metallic bonding is a simple model of metallic bonding, but a more detailed and realistic way of describing metallic bonding is band theory (Chapter 24 on the accompanying website). This is based on molecular orbital theory (Chapter 14), which describes bond formation via the overlapping and merging of atomic orbitals. 

We can use Figures 19.1(b) and 19.6 as a starting point to help you form your mental movie about how electron-transfer reactions occur at the particulate level. Look back and refamiliarize yourself with this figure, a Zn/Zn " and Cu VCu voltaic cell. Now recall the electron-sea model of metallic bonding (Section 12.8), by which a metal is pictured as a crystal structure of metal ions immersed in a sea of electrons. Imagine the metallic zinc electrode in this way zinc ions in a sea of electrons. 

Figure 9.1 Id illustrates a simple model of bonding in metals known as the electron-sea model. The metallic crystal is pictured as an array of positive ions, for example, Na+, Mg2+. These are anchored in position, like buoys in a mobile sea of electrons. These electrons are not attached to any particular positive ion but rather can wander through the crystal. The electron-sea model explains many of the characteristic properties of metals ...

In the electron-sea model, a metal crystal is viewed as a three-dimensional array of metal cations immersed in a sea of delocalized electrons that are free to move throughout the crystal (Figure 21.6). The continuum of delocalized, mobile valence electrons acts as an electrostatic glue that holds the metal cations together. 

FIGURE 21.6 Two- dimensional representation of the electron-sea model of a metal. An ordered array of cations is immersed in a continuous distribution of delocalized, mobile valence electrons. The valence electrons do not belong to any particular metal ion but to the crystal as a whole. 

Describe the electron-sea model of the bonding in cesium metal. Cesium has a body-centered cubic structure. 

The electron sea model for metals postulates a regular array of cations in a "sea" of valence electrons, (a) Representation of an alkali metal (Group 1A) with one valence electron, (b) Representation of an alkaline earth metal (Group 2A) with two valence electrons. 

Discuss the electron sea model for metals. How does this model account for the fact that metals are very good conductors of electricity ... 

FIGURE 18.6 Electron sea" model of bonding in metals. The positively charged metal atom nuclei are surrounded by a sea" of negatively charged electrons. 0- Positive metal ions 0 - ... 

A Figure 23.13 Schematic illustration of the electron-sea model of the electronic structure of metals. Each sphere is a positively charged metal ion. 

The special properties of a metal result from its delocalized bonding, in which bonding electrons are spread over a number of atoms. In this section, we will look first at the electron-sea model of a metal and then at the molecular orbital theory of bonding in metals. 

Figure 12.15 The electron-sea model of a metallic crystal. The monatomic ions formed by the metal remain fixed in a definite crystal pattern, but the highest-energy valence electrons are relatively free to move, which explains the high electrical conductivity... 

Metallic Crystals Aluminum is an example of a metallic crystal (Fig. 15.29). A simple model of bonding in a metal consists of a crystal of positive ions through which valence electrons move freely. This so-called electron sea model of a metallic crystal is illustrated in Figure 12.11. Positively charged ions form the backbone of the crystal the electrons surrounding these ions are not tied down to any particular ion and therefore are not restricted to a particular location. It is because of these freely moving electrons that metals are excellent conductors of electricity. 

A FIGURE 11.55 The Electron Sea Model In the electron sea model for metals, the metal cations exist in a sea of electrons. 

In Chapter 9, we considered a simple picture of metallic bonding, the electron-sea model The molecular orbital approach leads to a refinement of this model known as band theory. Here, a crystal of a metal is considered to be one huge molecule. Valence electrons of the metal are fed into delocalized molecular orbitals, formed in the usual way from atomic... 

The electron-sea model affords a simple qualitative explanation for the electrical and thermal conductivity of metals. Because the electrons are mobile, they are free to move away from a negative electrode and toward a positive electrode when a metal is subjected to an electrical potential. The mobile electrons can also conduct heat by carrying kinetic energy from one part of the crystal to another. Metals are malleable and ductile because the delocalized bonding extends in all... 

Two bonding models are used for metals. The electron-sea model pictures a metal as an array of metal cations... 

How does the electron-sea model account for the malleability and ductility of metals ... 

What properties of metals are better explained by band theory than by the electron-sea model ... 

The electron sea model (see Figure 6.2) for metal bonding proposes a theory that explains observed metal properties. In this model, we can envision that metal bonds are formed when a uniform array of metal cations, positively charged metal ions, are surrounded by a sea of electrons. 

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