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How do metallic bonds differ from ionic and covalent bonds?

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Metallic bonding is the bonding within metals. It involves the delocalized sharing of free electrons between a lattice of metal atoms. Thus, metallic bonds may be compared to molten salts.

e.g. Iron (Fe)... Why is it so strong? Of course, metallic bonding.

Metal atoms typically contain a small amount of electrons in their valence shell compared to their period or energy level. These become delocalised and form a Sea of Electrons surrounding a giant lattice of positive ions.

Metals seem to have higher boiling and melting points which might suggest stronger bonds between the atoms.

Metallic bonding, as with covalent bonding is non-polar, in that there is no (for pure elemental metals) or very little (for alloys) electronegativity difference among the atoms participating in the bonding interaction, and the electrons involved in that interaction are delocalized across the crystalline structure of the metal.

The metallic bond accounts for many physical characteristics of metals, such as strength, malleability, ductility, conduction of heat and electricity, and luster. See also chemical bond.

Metallic bonding is the electrostatic attraction between the metal atoms or ions and the delocalised electrons. This is why atoms or layers are allowed to slide past each other, resulting in the characteristic properties of malleability and ductility.

Metallic bond are different from chemical bonds. Ionic and covalent bonds are chemical bonds.

Covalent bonding is a common type of bonding, in which the electronegativity difference between the bonded atoms is small or non-existent. In the latter case, the bond is sometimes referred as purely covalent. See sigma bonds and pi bonds for current LCAO-explanation of non-polar bonds.
e.g. CH4 (methane)

Ionic bonding is type of electrostatic bond between atoms which have an electronegativity difference of over 1.6 (this limit is a convention). These form in a solution between two ions after the excess of the solvent is removed.
e.g. NaCl (common salt)

Hey, I tried to draw the structures of NaCl and methane molecules but this Yahoo! made it impossible. I hope you know the structurel.


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  • Elif answered 9 months ago
    Metallic bond
    1- In a metallic bond, valence electrons are spread all over the crystal, more or less uniformly. Therefore, metallic bond is non-directional in character.
    2- Since valence electrons are mobile, they are weakly by the nuclei, hence metallic bonds are weaker. Because of this heat of vaporization per mole of metal to free atoms is small.
    Covalent bond
    1- In a covalent bond, the valence electrons are localized; hence it has a directional character.
    2- Valence electrons are attached strongly towards the nuclei of the atoms; hence covalent bonds are quite stronger. Because of this heat of vaporizstin per mole of a covalent substance (i.e. graphite) is quite high.
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  • nashtn answered 9 years ago
    There are three types of primary chemical bonds; ionic, covalent and metallic. Ionic bonds result from a non-directional electrostatic attraction between positive and negative ions . Covalent bonds involve the sharing of electrons and have directionality related to the position of the outer shell electron orbitals. Metallic bonds are typified by delocalized valence electrons and a non-directional character. Weaker secondary bonds are van der Waals, permanent dipoles, fluctuating dipoles, and hydrogen bonding. The three classes of materials, (metals, ceramics and polymers) can be characterized by their chemical bonding. Metals have metallic bonds owing to weakly bound outer shell valence electrons. Metallic materials can either be pure elemental metals or alloys which are mixtures of more than one metallic element and/or metals and non-metals (e.g., brass CuZn or plain carbon steel Fe-C). Ceramics which are typically compounds of metals and non-metals are held together by a mixed ionic and covalent bond character. The hydrogen and carbon atoms in polymers have strong covalent bonds with weaker secondary bonding typically between molecular chains.
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  • Bash Share answered 2 weeks ago
    you're nerd
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  • How do metallic bonds differ from ionic and covalent bonds?
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