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Why are the valance electrons of metallic bonds different from other bonds?
Wiki User
∙ 6y ago
- In a metal the valence electrons delocalize into the conduction band, becoming an "electron gas" that fills the metal's bulk volume.
- In covalent bonds the valence electrons are shared between local pairs of atoms.
- In ionic bonds the valence electrons leave the "metal" and move to the "nonmetal" creating a pair of separate oppositely charged ions.
- In resonance bonds the valence electrons oscillate between being shared between two nearby local pairs of atoms.
- etc.
Wiki User
∙ 6y ago
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What kind of atoms form metallic bonds?
A positive metal ion and the electrons surrounding it.
What are some common properties of calcium gold iron and sodium?
The elements calcium, gold, iron and sodium are all metals. They all have a tendency to donate their valance electrons, rather than acquiring additional valance electrons. They all form metallic bonds, in the form of a shared electron cloud. They all have the electrical conductivity and metallic luster which comes with metallic bonds.
Why are the valence electrons found in metallic bonds different from other bonds because of what?
their valence electrons are free-roaming they allow for the conductivity of electricity APEX :) <3 JAmie
How is metallic bond different from ionic and covalent bonds?
they share all of their valence electrons
Why metals are flexible?
The formation of metallic bonds causes them to be flexible and strong. Metallic bonds become strong because positive and negative charged electrons have a strong force of attraction. Metallic bonds are flexible because of their malleability.
What kind of atoms form metallic bonds?
A positive metal ion and the electrons surrounding it.
What are some common properties of calcium gold iron and sodium?
The elements calcium, gold, iron and sodium are all metals. They all have a tendency to donate their valance electrons, rather than acquiring additional valance electrons. They all form metallic bonds, in the form of a shared electron cloud. They all have the electrical conductivity and metallic luster which comes with metallic bonds.
Why are the valence electrons found in metallic bonds different from other bonds because of what?
their valence electrons are free-roaming they allow for the conductivity of electricity APEX :) <3 JAmie
How is metallic bond different from ionic and covalent bonds?
they share all of their valence electrons
Why metals are flexible?
The formation of metallic bonds causes them to be flexible and strong. Metallic bonds become strong because positive and negative charged electrons have a strong force of attraction. Metallic bonds are flexible because of their malleability.
Which particles of the atom participate in the formation of chemical bonds?
electrons. More specifically, valance electrons
Elcetrons used to form chemical bonds?
These are the outer electrons of the atom called valance electrons.
How is metaic bonding different from ionic bonding?
Free metal atoms form metallic bonds, and a significant feature of metallic bonds is the existence of a 'sea of electrons' . This is different from ionic compounds, where ions of opposite charges attract one another electrostatically and there are no free electrons.
How are metallic bonds different to covalent bonds?
Metallic bonds are bonds between metals. They consist of valence electrons in delocalized bonds covering the whole crystal. These electrons can move freely and are responsible for the special properties of metals such as electrical conductivity. Covalent bonds are electrons being shared and are usually between non-metals. They are localized to the atoms which are sharing them, resulting in individual molecules.
A key distinctive feature of metallic bonds is that they?
are formed by electrons that are delocalized throughout the object bonded by the metallic bonds.
What is the shape of metallic bonds?
Metallic bonds don't really have a shape. They are sometimes described as a cloud or sea of electrons.
How is the position of electrons involved in metallic bonding different from the position of electrons that form ionic and covalent bonds?
the electrons involved in metallic bonding are delocalised - they are free to move which accounts for electrical conductivity. In ionic bonds the electrons are tightly bound to individual atoms. Generally covalent bonds have localised electrons, in pairs in individual bonds. However there are delocalised electrons in some situations - take graphite extensive pi bonds allow for delocalisation and electrical conductivity.
