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Delocalisation is when electrons are not associated with one atom but are spread over several atoms.
So the electrons are not directly bonded with any atoms but effectively 'float' above and below the molecule in electron clouds.
What else can I help you with?
Is aluminuim a conductor?
Yes ,because it has delocalised electron
Do alkali metals conduct heat and electricity?
Yes, they are metals- good conductivity is a characteristic of metals that have delocalised electron clouds.
What is basicity of furan?
furan though has a lone pair of electron which is not delocalised but due to high electronegetivity of oxygen it is not a available for donation hence has weak basic proerty
Does NH4 have delocalized electron?
No, NH4 does not have delocalized electrons. NH4+ is a cation composed of a nitrogen atom bonded to four hydrogen atoms, and the electrons are localized around the individual atoms involved in the bonds.
Which electron arrangement is that of a metallic element?
The electron arrangement of metallic elements typically involves one or two electrons in the outermost shell, which allows them to easily lose electrons and form positive ions. This electron arrangement gives metallic elements their characteristic ability to conduct electricity and heat well.
Which type of bond occurs between atoms in which the electrons are able to move around?
Metallic bonds and delocalised covalent bonds. Electrons move around in all types of bonds, its a question of degree. In straightforward covalent bonds with an electron pair- the electron moves in a small volume along the bond axis. In delocalised covalent bonds such as that in sheet graphene electrons are free to move along the plane. In metallic bonds electrons are free to move around the lattice. This ability to move is associated with electrical conductivity.
Does a metallic bond always lose an electron?
They don't lose electrons to start with. A metallic bond has delocalised electrons which bond the cations with the electrons unless a sufficient amount of force breaks them. For example tearing aluminium foil Hope this helps
Why is metal wire is a conductor?
Any metal object, whether it is a wire, a spanner or even a radiator, conducts electricity. This is because of the way metal atoms bond. Positive metal ions are formed when one electron from each of the atoms becomes delocalised, and not specifically associated with any one nucleus. These ions are surrounded by what is described as a sea of delocalised electrons, which attracts the positive ions, thus binding them in a metal object. Metal objects can conduct electricity because charge carriers can be made to move along the structure in a particular direction. In this case the charge carriers are the delocalised electrons.
What type of bonding involves de-localized electrons?
Metallic bonding involves delocalised electrons, which can transfer heat and electricity across the metal. Also, graphite and benzene contains delocalised electrons.
Why don't all forms of carbon conduct electricity?
It has do to with a phenomenon known as electron delocalisation. Graphite is the only form of carbon (and one of the only non-metals) to conduct electricity. Graphite is arranged in sheets of 6-membered rings, and these sheets have delocalised electrons, which means that electrons are spread evenly throughout the sheet and are free to move, and therefore carry electrical charge throughout the sheet. Other forms of carbon, such as diamond, do not have delocalised electrons, and are insulators.
What does delocalized mean?
DelocalisedThe term 'delocalised' refers to an electron which is not 'attached' to a particular atom. For example, in metals, some of the outer electrons are delocalised and are free to move around the whole metal solid. This is why metals conduct electricity. Another example of delocalised electrons is in benzene (C6H6), a cyclic molecule composed of a ring of bonded carbons, with one hydrogen attached to each. In benzene, the electrons in the C-C pi-bonds (basically the double bonds) are delocalised the whole molecule. If you look at the location of these pi-bonding electrons, they are found evenly distributed in a ring around the entire molecule. In this case, the delocalisation can be explained by something called 'resonance forms.' Often, molecules with alternating double bonds show delocalised bonding.However, to truly understand the concept of delocalisation, some basic quantum mechanics must be used, and delocalised bonding in molecules is best explained by molecular orbital theory. In reality, all electrons are somewhat delocalised and are never associated with exactly one bond (in molecules with more than 2 atoms). Some are more localised than others (specific electrons stay mostly with specific bonds), while some are more delocalized (electrons are very free to move about many different bonds in the molecule)
What is the arrangement of electrons in a covalent bond?
usulally they are shared and are localised around the 2 atoms being bonded. In 3 center 2 electron bonds as in B2H6 they are across 3 atoms. Also there are delocalised covalent bonds , delocalised across more than two atoms- examples graphite, benzene.
