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Chapter 13: Problem 5

Why does metallic binding usually occur with atoms having a small number of valence electrons?

Short Answer

Expert verified
Metallic bonding typically occurs with atoms having few valence electrons because those valence electrons can easily detach and spread out around the metal lattice, forming a 'sea' or cloud of delocalized electrons. This enables the formation of metallic bonds, which are characterized by the electrostatic attractive force between the positively charged metal ions and the delocalized electrons.

Step by step solution

01

Understand Metallic Bonding

Metallic bonding is a type of chemical bonding that arises from the electrostatic attractive force between conduction electrons (in the form of an electron cloud) and positively charged metal ions. It involves the sharing of many detached electrons, which belong to a 'cloud' of delocalized electrons.
02

Define and understand importance of valence electrons

Valence electrons are the electrons in the outermost shell of an atom. They are important because they are the electrons involved in chemical reactions and in bonding between atoms. The number of valence electrons can influence an atom's reactivity and its ability to form bonds.
03

Explaining Metal's tendency to have few valence electrons and form Metallic bond

Metals usually have 1-3 valence electrons. Those easily detachable valence electrons become delocalized and form a 'sea' or cloud around the metal ions, allowing them to conduct electricity and heat. This is due to the fact that for a metal atom, it is energetically beneficial to donate these few electrons to the sea of electrons and achieve a full outer electron shell.
04

The role of metallic bonding in atoms with few valence electrons

The type of bonding in metals is called metallic bonding. The valence electrons from the metal atoms detach and spread out around the metal lattice, causing the positive ions and delocalized electrons to attract. Because metals have only a few valence electrons and these can easily become delocalized, metals are conducive to the formation of metallic bonds.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Valence Electrons
Valence electrons are the electrons found in the outermost shell of an atom. They play a key role in an atom's ability to form bonds with other atoms. In chemical reactions, it is these electrons that are often gained, lost, or shared.
  • Valence electrons determine how an atom interacts with others.
  • Atoms with few valence electrons tend to easily give them up, especially in metals.
Metals generally have between one and three valence electrons. These few electrons can be easily removed, which simplifies their incorporation into a broader framework of electrons鈥攌nown as metallic bonding. This tendency to lose electrons contributes to the reactivity and properties of metal atoms.
Delocalized Electrons
Delocalized electrons are electrons that are not associated with a single atom but are free to move across multiple atoms. This concept is especially important in metals, where valence electrons leave their parent atoms and form a 'cloud' or 'sea' of electrons.
  • These electrons can move freely, making them crucial in electricity and heat conduction.
  • The electron cloud created by delocalized electrons stabilizes the metal structure.
This flexibility of electrons contributes to metals being malleable and ductile. As the electrons are not bound to any specific ion, they allow the metal to bend and reshape without breaking, while maintaining a persistent electrostatic attraction.
Chemical Bonding
Chemical bonding is the process by which atoms combine to form compounds. These bonds form because of the interactions between valence electrons of atoms.
  • Metallic bonds are a type of chemical bonding seen in metals.
  • They involve valence electrons creating a 'cloud' that binds metal ions together.
The principal difference in metallic bonding compared to other types of bonds, such as ionic or covalent, is the presence of a delocalized electron cloud. This sea of electrons allows for unique properties in metals, such as electrical conductivity and resilience.
Metal Ions
Metal ions are formed when copper, gold, or any metal losestheir valence electrons and become positively charged. These positive ions are immersed in a sea of delocalized electrons, creating a stable structure.
  • The metal ions are stabilized by the attraction to the electron cloud.
  • This attraction results in the metal's characteristic high melting and boiling points.
The orderly arrangement of metal ions allows them to slide past one another when force is applied, lending metals their malleability. This structure also means that applying heat or electricity energizes the delocalized electrons, enhancing their reactive capacities in various applications.

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Most popular questions from this chapter

A tunnel diode junction is approximated by a rectangular barrier \(100 \AA\) thick and \(3.3 \mathrm{eV}\) high. If \(1.00 \times 10^{25}\) electrons strike the barrier each second with kinetic energy \(3.1 \mathrm{eV}\), and the effective electron mass is \(0.30 m\), what current passes the junction?

Explain why the electrical conductivity of materials varies over a factor of \(10^{24}\) whereas the thermal conductivity of materials only varies over a factor of about \(10^{8}\).

Show that, according to the free-electron model, the resistance \(R\) of a length \(L\) of wire is given by $$ R=m L / n A e^{2} T $$ where \(A\) is the cross-sectional area of the wire and \(T\) is the mean time between collisions.

(a) Show that the effect of a lattice periodicity \(a\) on periodic potentials having Bloch function solutions is to modulate the free-electron solution so that \(\psi(x+a)=\psi(x) e^{i k a}\). (b) Show that \(e^{i k a}=-1\) at the Brillouin zone boundaries. Comment on the meaning of this result.

Explain why metallic binding leads to a close-packed arrangement of atoms; i.e., explain why the lowest energy in metallic binding corresponds to the greatest number density of atoms.
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