Here, we provided to Metallic Bonding Hand Written Note For BSC. 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 of delocalized electrons) and positively charged metal ions. It may be described as the sharing of free electrons among a structure of positively charged ions (cations). Free download PDF Metallic Bonding Hand Written Note For BSC.
Metallic bonding accounts for many physical properties of metals, such as strength, ductility, thermal and electrical resistivity, and conductivity, opacity, and luster. Free download PDF Metallic Bonding Hand Written Note For BSC.
Metallic bonding is not the only type of chemical bonding a metal can exhibit, even as a pure substance. For example, elemental gallium consists of covalently-bound pairs of atoms in both liquid and solid-state—these pairs form a crystal structure with metallic bonding between them. Another example of a metal-metal covalent bond is a mercurous ion. Free download PDF Metallic Bonding Hand Written Note For BSC.
Both metallic and covalent bonding can be observed in some metal samples. For example, covalently bonded gallium atoms tend to form crystal structures that are held together via metallic bonds. The mercurous ion also exhibits metallic and covalent bonding. Free download PDF Metallic Bonding Hand Written Note For BSC.
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BOOK NAME – METALLIC BONDING HAND WRITTEN NOTE FOR BSC
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What is the Metallic Bond?
‘Metallic bond’ is a term used to describe the collective sharing of a sea of valence electrons between several positively charged metal ions. Metallic bonding is a type of chemical bonding and is responsible for several characteristic properties of metals such as their shiny luster, their malleability, and their conductivities for heat and electricity. Free download PDF Metallic Bonding Hand Written Note For BSC.
Both metallic and covalent bonding can be observed in some metal samples. For example, covalently bonded gallium atoms tend to form crystal structures that are held together via metallic bonds. The mercurous ion also exhibits metallic and covalent bonding. Free download PDF Metallic Bonding Hand Written Note For BSC.
The factors that affect the strength of a metallic bond include:
- A total number of delocalized electrons.
- The magnitude of the positive charge held by the metal cation.
- The ionic radius of the cation
Properties Attributed by Metallic Bonding
Metallic bonds impart several important properties to metals that make them commercially desirable. Some of these properties are briefly described in this subsection. Free download PDF Metallic Bonding Hand Written Note For BSC.
Electrical Conductivity
Electrical conductivity is a measure of the ability of a substance to allow a charge to move through it. Since the movement of electrons is not restricted in the electron sea, any electric current passed through the metal passes through it, as illustrated below.
When a potential difference is introduced to the metal, the delocalized electrons start moving towards the positive charge. This is the reason why metals are generally good conductors of electric current. Free download PDF Metallic Bonding Hand Written Note For BSC.
Thermal Conductivity
The thermal conductivity of a material is a measure of its ability to conduct/transfer heat. When one end of a metallic substance is heated, the kinetic energy of the electrons in that area increases. These electrons transfer their kinetic energies to other electrons in the sea via collisions.
The greater the mobility of the electrons, the quicker the transfer of kinetic energy. Due to metallic bonds, the delocalized electrons are highly mobile, and they transfer the heat through the metallic substance by colliding with other electrons.
Malleability and Ductility
When an ionic crystal (such as a sodium chloride crystal) is beaten with a hammer, it shatters into many smaller pieces. This is because the atoms in the crystals are held together in a rigid lattice that is not easily deformed. The introduction of a force (from the hammer) causes the crystal structure to fracture, resulting in the shattering of the crystal. Free download PDF Metallic Bonding Hand Written Note For BSC.
In the case of metals, the sea of electrons in the metallic bond enables the deformation of the lattice. Therefore, when metals are beaten with a hammer, the rigid lattice is deformed and not fractured. This is why metals can be beaten into thin sheets. Since these lattices do not fracture easily, metals are said to be highly ductile.
Metallic Luster
When light is incident on a metallic surface, the energy of the photon is absorbed by the sea of electrons that constitute the metallic bond. The absorption of energy excites the electrons, increasing their energy levels. These excited electrons quickly return to their ground states, emitting light in the process. This emission of light due to the de-excitation of electrons attributes a shiny metallic luster to the metal. Free download PDF Metallic Bonding Hand Written Note For BSC.
High Melting and Boiling Points
As a result of powerful metallic bonding, the attractive force between the metal atoms is quite strong. In order to overcome this force of attraction, a great deal of energy is required. This is the reason why metals tend to have high melting and boiling points. The exceptions to this include zinc, cadmium, and mercury (explained by their electron configurations, which end with ns2).
The metallic bond can retain its strength even when the metal is in its melt state. For example, gallium melts at 29.76oC but boils only at 2400oC. Therefore, molten gallium is a nonvolatile liquid. Free download PDF Metallic Bonding Hand Written Note For BSC.
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