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Which phrase best describes a metallic bond?
A metallic bond is one where delocalized valence electrons of the metal are attracted to any of the metal cations. The electrons are delocalized meaning they do not stay with any particular nucleus. The bonds are held together by electrostatic interaction between the delocalized electrons and the positive cations.
How many valence electrons are found in a krypton atom?
There are 8 Valence Electrons.
Which electrons from the metal make up the delocalized electrons?
In a metallic bond, the electrons which make up the 'sea' of delocalised electrons are all of those from the outermost shell from the atoms. The other shells stay unaltered.
The electrons that occupy the outermost filled shell are called?
Outer energy level electrons, or valence electron.
What are the electrons in the outer shell?
Those electrons are the valence electrons. They are the electrons which mostly take part in exchange of electrons or sharing of electrons. Hence, valence shell electrons are a very important part of chemistry since all the reactions due to them only.
Why metal are good electrical conductivity?
Delocalized valence electrons
What do delocalised valence electrons moving between nuclei do?
Delocalized valence electrons moving between nuclei become detached from their parent atom. The metal is held together by the strong forces of attraction between the delocalized electrons and positive nuclei.
What are free electrons or delocalized electrons?
Not sure, but maybe you are referring to "lone pair" of electrons.
What happens to the valence electrons of atoms in metallic bond?
Metals have metal bonds. valence electron make bonds with metal ions.
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
Which phrase best describes a metallic bond?
A metallic bond is one where delocalized valence electrons of the metal are attracted to any of the metal cations. The electrons are delocalized meaning they do not stay with any particular nucleus. The bonds are held together by electrostatic interaction between the delocalized electrons and the positive cations.
Delocalized valence electrons are typical of ionic compounds?
I do not think so. It should be metallic compound. Electrons could move freely between the positive ions.
What happens to a valence electron in a metallic bond?
Valence electrons in a metallic bond are delocalized and can move freely within the metal atoms. This gives metals their malleability and luster.
Does hcooh have delocalized electrons?
No.
Characteristics of metallic bonds?
The valence electrons of all the metal atoms go into delocalized bonds which cover the entire crystal lattice. These electrons are free to move around and give metals their special properties such as good electrical and thermal conduction. This situation is sometimes pictured as a regular array of metal ions floating in a 'sea' of electrons. Some of the characteristics of metallic bonding are that the substance will be very hard, made of some sort of metal, usually a gray or silver color, and most likely it will be somewhat shiny. Electrons move freely among many metal nuclei.
Why are the valance electrons of metallic bonds different from other bonds?
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.To summarize in metals the valence electrons become delocalized, in other bonds the valence electrons stay local.
What does the term free moving electrons mean?
delocalized electrons
