Answer and Explanation: 1. Metallic Bonds - A bond exclusively between metals. Group 1 metals like sodium and potassium have relatively low melting and. By definition if the atoms in an elemental sample have delocalized electrons (so that the sample will conduct electricity) then the element is a metal. Because the valence shells in metals contain a few number of valence electrons and since it’s ideal to reach full octet valency, it’s more energetically favourable for the atoms. Solid metals are made of layers of positively charged ions with electrostatic forces of attraction with a sea of delocalised electrons. After delocalising their valence electrons, the metal atoms become ions. These free electrons are able to move around freely and collide with one another, propagating heat and electricity through the metal. AboutTranscript. The atoms that the electrons leave behind become positive ions, and their interaction with valence electrons produces the cohesive or binding force that binds the metallic crystal together. Metals on a microscopic scale consist of positive metal ions in 'sea' of free (delocalised) electrons. 2. Answer link. A metallic solid is created by metal atoms when their electrons become delocalized,. Lazy Lark. Figure 4. These free electrons (electron density) are concentrated on the surface and can move freely in metal. The metal consists of metal cations and a balancing number of. " IMHO it would be better if the electrons were shown as red circles fading to pink around the metal ion rather than red dots, but nevermind. . This is because delocalized electrons can travel throughout the metal. Graphite is a good conductor of electricity due to its unique structure. That is why it conducts electricity. When hydrogen is added to this, cyclohexane, C 6 H 12, is formed. Atomic orbitals overlap to form molecular orbitals in which the valence electrons of the atoms travel. These electrons are not associated with any atom. The electron gas is still a regular structure on average, but the structure referred to is the ion structure. Neutral sodium atom on left has 11 protons and 11 electrons. Why do electrons become Delocalised in metals GCSE? Metals form giant structures in which electrons in the outer shells of the metal atoms are free to move. a metal are sometimes called a " sea of electrons ". This is because the delocalised electrons are free to move throughout the metal, carrying a charge. In the metallic state, either pure or in alloys with other alkali metals, the valence electrons become delocalized and mobile as they interact to form a half-filled valence band. why do electrons become delocalised in metals seneca answer. This model represents metal crystals as being made up of positive metal ions close ion Electrically charged particle, formed when an atom or molecule gains or loses electrons. Usually electrons in materials are bound to one atom, and atoms are held together by the interactions of the charges on different atoms. The electrons can move freely within these molecular orbitals, and so each electron becomes detached from its parent atom. Most metals react with the atmosphere to form oxides. In metallic bonding the outer shells of adjacent atoms overlap, and the outer shell electrons are free to move about through the lattice. Delocalized electrons are free electrons in a molecule, ion, or solid metal that do not participate in chemical bonding. All About Supplements Menu. tiger house ending explained RESERVA AHORA. The metal is held together by the strong forces of attraction between the positive nuclei and the delocalized electrons (Figure (PageIndex{1})). why do electrons become delocalised in metals?In metallic bonds, electrons move freely among the atomic nuclei—they are delocalized, so there isn’t a definitive bond in the way molecular and ionic bonds form. The remaining "ions" also have twice the. They differ from covalent and ionic bonds in that the electrons are delocalized, that is, they are not shared by only two atoms. The atoms are arranged in layers. why do electrons become delocalised in metals seneca answer. Another way to think about this is to consider the hybridization of the 3s and 3p electrons in Mg. why do electrons become delocalised in metals seneca answer. Neutron scattering sheds light on this intriguing phenomenon. AboutTranscript. The delocalised electrons in the structure of. 2 Covalent bonding is strong but inflexible. A bond between two nonmetals. These delocalised electrons are free to move throughout the giant metallic lattice. This means that the electrons could be anywhere along with the chemical bond. This state of not being bound to any metal ion is what allows it to conduct electricity and so forth. what kind of bonding is metallic bonding. What about sigma electrons, that is to say those forming part of single bonds? This representation better conveys the idea that the HCl bond is highly polar. The free electrons are what conducts electricity through metals. Zz. This accounts for many characteristic properties of metals: conductivity, malleability, and ductility. It creates a bulk of metal atoms, all "clumped" together. An example of this is a. These delocalized electrons contribute to the properties of the solid, such as its ability to conduct electricity and malleability. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion. A metallic bond is the attraction of the stationary metal cations to the surrounding mobile electrons. The electrons are relatively unconstrained, and they can move in between metal cations. Study with Quizlet and memorize flashcards containing terms like 10 Properties of metals, Formula for density, Why do metals conduct electricity in the solid state? and more. They can move freely throughout the metallic structure. Posted by; Date May 6, 2023;why do electrons become delocalised in metals? Localized electrons are the bonding electrons in molecules while delocalized electrons are nonbonding electrons that occur as electron clouds above and below the molecule. shell of electrons and the remaining protons hold onto the remaining electrons more strongly and pulls them in more tightly. Metallic bond, force that holds atoms together in a metallic substance. The metallic bond is the force of attraction between these free-moving (delocalized) electrons and positive metal ions. The atoms in a metal are held together by the attraction of the nuclei to electrons which are delocalized over the whole metal mass. Examine the following examples and write as many resonance structures as you can for each to further explore these points: Lets look for a moment at the three structures in the last row above. orbital and overlap for some reason. Discuss how the size of the cations determines the strength of a metallic bond. Sorted by: 2. 9. When electricity flows through a metal, the electrons help to transmit and distribute the electrical energy throughout the material. AI-generated answer. The delocalized electrons can conduct both electricity and heat from one end of the metal to another with low resistance. The metallic bonding model explains the physical properties of metals. multidirectional bonding between the positive cations and the sea of delocalised electrons. Answer link. what to do with leftover oreo filling. To summarize in metals the valence electrons become. Why do metals conduct heat? Metals are in continuous vibratory motion, When one end of it is heated, it travels along with the substance. $endgroup$ – DHMO Oct 12, 2016 at 8:37does a yeast infection get worse before it gets better; pat rice net worth; hall of heroes comic con 2022; mental health crisis team east lothian. 8. The remaining "ions" also have twice the. These delocalised electrons are free to move throughout the giant metallic lattice. 5. From the physicists' "electron sea" point of view of metal bonding, the higher the ionic charge the metal atom can support, the higher the element's melting and boiling points. fatima robinson familyThe outer electrons do not “belong” to any atom but form a pool or sea of delocalized electrons that are free and move randomly throughout the fixed lattice of positive ions. What is metallic bonding? Between two metal atoms. Figure 16. Modified 5 years, 4 months ago. The reason is that they can involve the 3d electrons in the delocalization as well as the 4s. Bonding in metals is often described through the "electron sea model". When they undergo metallic bonding, only the electrons on the valent shell become delocalized or detached to form cations. 23/05/2023 by . When metallic atoms come together they sacrifice their valence electrons to a sea of delocalized electrons that can move between the ions. • Metals have high melting points. The electrons are said to be delocalized. Both of these electrons become delocalized, so the "sea" has twice the electron density as it does in sodium. However, it is a different sort of bonding than covalent bonding. In contrast, covalent and ionic bonds form between two discrete atoms. Electrons entering one end of the metal cause a delocalised electron to displace itself from the other end. You ask. This phenomenon is known as conduction. Both of these electrons become delocalised, so the "sea" has twice the electron density as it does in sodium. which of the following is not characteristic of neurons? Na ndiqni në: mickey mantle home runs warwick races tickets. So each atom’s outer electrons are involved in this delocalisation or sea of electrons. The electrons are said to be delocalized. These 'delocalised' electrons from the outer shell of the metal atoms are the 'electronic glue' holding the particles together. The electron on the outermost shell becomes delocalized and enters the. The electrons can move freely within these molecular orbitals, and so each electron becomes detached from its parent atom. phonons). 45 seconds. q6 4 the 14 species of finches. 3. Metal cations in an electron sea. The reason is that they can involve the 3d electrons in the delocalization as well as the 4s. Metals are lustrous due to the flow of free electrons. Why do electrons in metals become Delocalised? Charge delocalization is a stabilizing force because it spreads energy over a larger area rather than keeping it confined to a small area. The atoms in the material form a matrix where. When they undergo metallic bonding, only the electrons on the valentshell become delocalized or detached to form cations. GCSE: Why do electrons delocalize in metals? Metals are massive structures in which electrons in metal atoms’ outer shells are free to move. Hence I would not regard localization or delocalization of the electrons as an objective quality. This means that they are no longer attached to a particular atom or pair of atoms, but can be thought of as moving freely around in the whole structure. A metallic bond is the attraction of the stationary metal cations to the surrounding mobile electrons. Like all metals, magnesium has these delocalized electrons that can carry electric charge from one point to another. Both of these electrons become delocalized, so the "sea" has twice the electron density as it does in sodium. It is a force of attraction between the metallic cations and the delocalised electrons, and this force binds the atoms firmly together in the metallic object. The electrons are said to be delocalized. 1. why do electrons become delocalised in metals seneca answer. Delocalized electrons don’t just explain metals. This creates an attract between the opposite charges of the electrons and the metal ions. Metal atoms lose electrons to become positively charged ions. Let's take an example of sodium. does inspection period include weekends in florida. Figure (PageIndex{5}): Metal cations in an electron sea. Figure 5. electrons become delocalised in metals because orbitals in metal atoms overlap. Materials with many delocalized electrons tend to be highly conductive. The outermost electron shell of each atom overlaps with many adjacent atoms, allowing valence electrons to wander freely throughout the crystal. pet friendly houses for rent in greensburg, pa; monaview elementary student killed in accident; card method medical terminology; contracted: phase 3; herbalife 1 million lifetime achievement; funny things to bring to a potluck > why do electrons become delocalised in metals?Why do electrons become delocalised in metals? They dont become delocalized, the conduction electrons are delocalized, and thats because of The C=C double bond on the left below is nonpolar. The positive charge is due to a deficit of electrons in that region, and that "electron hole" may be treated in many ways as if it is a particle (moving around due to certain rules, etc). The electrons are said to be delocalized. The electrons are said. why are metals malleable. why do electrons become delocalised in metals? because the electron orbital in metal atoms overlap. The metal atoms are arranged in a regular pattern of layers, with delocalised electrons able to move between them. When a force. The atoms in a metal are held together by electrostatic forces called metallic bonds. The metal is held together by the strong forces of attraction between the positive nuclei and the delocalized electrons (Figure (PageIndex{1})). Therefore layers of cations are still held together by the. GCSE Chemistry Play this quiz again. the mobile electrons of a pure metal are also called ______ electrons. Ionic bonds require an electron donor, often a metal, and an electron acceptor, a nonmetal. The metal is held together by the strong forces of attraction between the positive nuclei and the delocalized electrons (Figure (PageIndex{1})). Because their electrons are mobile, metallic solids are good conductors of heat and electricity. Because they have lost electrons, metal atoms are in fact metal ions, but you don't notice this because of the delocalised electrons. Once in the conduction band, the electron no longer "belongs" to any particular atom. For reasons that are beyond this level, in the transition. The reason graphite can conduct electricity is because there are delocalized electrons that are mobile across the layers. mofo69extreme. The electrons sort of floats outside of the metal atoms itself and together, creates this big sea of negative delocalised electrons, which subsequently makes the remaining atoms themselves become positively charged ions and attracted to that sea. Delocalized Electrons: Delocalized electrons are those that are not localized to a specific atom or molecule in a solid, liquid, or gas. We would like to show you a description here but the site won’t allow us. how well do metals tend to conduct electricity? how does the model of metallic bonding account for that property? they conduct electricity well. These electrons are not associated with any particular metallic nucleus, and so are free to move throughout the metal. The metal is held together by the. Tags: seneca whatever. Hybridization requires promotion from the 3s 2 3p 0 ground state of an Mg atom to a 3s 1 3p 1 excited state. It should also be noted that some atoms can form more than one ion. Metals have been behind major human advances from the iron age to Kylie's gold hot pants. This state of not being bound to any metal ion is what. In metallic bonding, the outer electrons are delocalised (free to move). The atoms are more easily pulled apart to form a liquid, and then a gas. why are metals malleable. Ionic bonding is observed because metals have few electrons in their outer. an attraction between positive and negative ions. Multiple Choice. why do electrons become delocalised in metals seneca answerwhat happens when someone steals your food stamps. The electrons are said to be delocalized. Answer: All of the 3s orbitals on all of the atoms overlap to give a vast number of molecular orbitals which extend over the whole piece of metal. The electrons are said to be delocalized. The electrons are said to be delocalized. The electrons released from the valence. a metal are sometimes called a " sea of electrons ". In case B, the arrow originates with one of the unshared electron pairs, which moves towards the positive charge on carbon. Figure. 19. First, the central carbon has five bonds and therefore violates the octet rule. But what does this have to do about conducting electricity? Well the delocalised electrons will all move in the same directions when a heat source is. Bonding in metals is often described through the "electron sea model". After all, electricity is just the movement of electrons. Metallic solids also tend to be malleable and ductile due to the ability of the metal nuclei to move past each other without. When stress is applied, the electrons simply slip over to an adjacent nucleus. Documentaires; Series; Biografie; Nieuws; why do electrons become delocalised in metals?non-metal atoms gain electrons to form negative ions (anions close anion An atom or group of atoms that have gained electrons and become negatively charged. Without getting into the quantum mechanical details, here’s a cartoon depiction of what’s going on. 8. The structure of a metal can also be shown as. Graphite is commonly used in electrical applications such as batteries and electrodes. why do electrons become delocalised in metals?richard james hart. A more detailed treatment, known as the bond theory of metals, applies the idea of resonance hybrids to. This is due to the increased positive charge on the metal ion and the increased number of electrons that are delocalised, resulting in stronger bonding. This explains why group 1 metals such as sodium have quite low melting/boiling points since the metal would be composed of electrons delocalized in a $ce{M}^+$. That is, the orbitals spread over the entire molecule. border collie rescue virginia beach. Viewed 2k times. The electrons can move freely within these molecular orbitals, and so each electron becomes detached from its parent atom. Wikipedia defines a delocalized electron inside a metal as one that is free to move from one atom to another. 2 Delocalised electrons help conduct heat. The outermost electrons of the metal atoms become dislodged or "delocalized. multidirectional bonding between the positive cations and the sea of delocalised electrons. Yes they do. Metallic bonding—and the loosely held electrons—is also why metals conduct electricity so well. Therefore, the feature of graphite. We further notice that pi electrons from one structure can become unshared electrons in another, and vice versa. As a result, the bond lengths in benzene are all the same, giving this molecule extra stability. They are the outer, orbiting electrons that can become part of chemical bonds. In metals, the electrons close electron Subatomic particle, with a negative charge and a negligible mass relative to protons and neutrons. The conductivity of graphite can be enhanced by doping or adding impurities. A mixture of two or more metals is called: mixture. Figure 3. A feature of metal atoms is that the electrons in the outer shells do not remain in the proximity of a specific nucleus. When light is shone on to the surface of a metal, its electrons absorb small. A metal has a large cloud of relatively free electrons (electrons that are loosely bound to the metal surface). Metals also contain highly mobile delocalized electrons that can transfer heat very rapidly. This is possible because the metallic bonds are strong but not directed between particular ions. The electrons can move freely within these molecular orbitals, and so each electron becomes detached from its parent atom. jahmyr gibbs 40 yard dash. Most anions are formed from non-metals. The atoms are more easily pulled apart to form a liquid, and then a gas. surrounded by a sea. A metallic bond is a bond resulting from attractions between positive ions and surrounding mobile electrons. Covalent bonds involve electron sharing, while ionic bonds involve electron transfer between atoms. The molecular orbitals created from Equation 10. These electrons are known as delocalised and so are 'free to move' across the surface of the metal. Metals are able to conduct electricity because their electrons are free to move around. Kafe; Shërbimet. Delocalised means that the. In metallic aluminum the three valence electrons per atom become conduction electrons. Trying to make a zinc-copper cell with copper ion in the solution just makes the cell work worse as a good part of the zinc is lost through direct reduction of copper ions at the surface. Substances, especially metals, with many delocalized electrons are highly conductive [1-4]. Like other answers have already pointed out, metals don’t have actual free electrons. The outer electrons in a metal are almost not bound to any individual atom, thus are relatively free. The metallic bonding weakens as the atomic size increases. Sorted by: 32. Metallic bond, force that holds atoms together in a metallic substance. What tendency do metals have when forming an ion? Metals tend to form cations by losing valence electrons. On the left, a sodium atom has 11 electrons. The electrons are said to be delocalised. In this layer, the electrons can move as though they are in a metal. Metallic bonds are characterized by the overlap of outer orbitals where electrons are allowed to move freely from atom to atom in the sea of electron model. We would like to show you a description here but the site won’t allow us. what term is used to describe this model of metallic bonding? electron sea model. The promotion energy (+264 kJ/mol) is more than offset by the bonding energy (-410 kJ/mol), the energy released when gaseous atoms in the excited state. Metals have high melting point and high boiling point because the attraction between delocalized electrons and metal ions is very strong. In the cartoon this is given by the grey region. Magnesium does have free electrons, so it is conductive. They do not flow with a charge on it. You need to ask yourself questions and then do problems to answer those. Electrical Conductivity is pretty obvious. The metal is held together by the strong forces of attraction between the positive nuclei and the delocalized electrons (Figure (PageIndex{1})). Delocalised does not mean stationary. Which is most suitable. They are no longer associated directly with any particular atom or pair of atoms, but are free to wander throughout the whole sheet. We say that the electrons are delocalised. Posted on. Kancelaria wyznaczających standardy . The term delocalization is general and can have slightly different meanings in different fields:Now, assuming again that only the -electrons are delocalized, we would expect that only two electrons are delocalized (since there is only one double bond). Metals share valence electrons, but these are not. C. Metal is shiny because it reflects incoming light photons. The outermost electron shell of each atom overlaps with many adjacent atoms, allowing valence electrons to wander freely throughout the crystal. Edit. As the nuclear charge on the cation increases, the size of the cation becomes smaller. Down the group, the number of delocalised electrons and the charge on each cation remains the same at +1 but the cationic radius increases so the attraction between the cations and the electrons in the lattice get weaker down the group. 1 9. The often quoted description of metals is as " positive ions in a sea of electrons ". 3 Ionic bonding is strong but ionic solids are brittle. The remaining "ions" also have twice the charge (if you are going to use this particular view of the metal bond) and so there will be more attraction between "ions" and "sea". To answer the question, we need to measure a property that is tightly related to delocalization of electrons. The metal atoms are arranged in a regular pattern of layers, with delocalised electrons able to move between them. This produces an. The remaining "ions" also have twice the. Technically yes, the electrons are shared equally in metallic bonding. The greater the numbers of delocalized electrons the. Metal ions are surrounded by delocalized electrons. Metallic bonds require a great deal of energy because they are strong enough to break. September 20, 2022 by Emilio Tucker. The metal is held together by the strong forces of attraction between the positive nuclei and the delocalized electrons. Answer. We. Why do electrons become Delocalised in metals GCSE? The metal is held together by the strong forces of attraction. ZapperZ said: This is now a different situation because an electron that was localized in the valence band has now been promoted to the conduction band due to a gain in energy. See full answer below. these questions are saying they are loosely bound: Do electrons move around a circuit? Why can an electrons initial kinetic energy be considered negligible in the photoelectric effect? where annav says: the electrostatic attraction between metal cations and the sea of electrons. The electron sea model accounts for several metallic properties, including high thermal and electrical conductivity, metallic luster, ductility, and malleability. This explanation, in simple words, argues that since the 3 lewis strucutes are identical/indistinguishable, the electron density must be equal and thus delocalised between the bonds by symmetry. Metallic bonding occurs between the atoms of metal elements - Lithium, Beryllium, Sodium, Magnesium, Aluminium and Calcium. Also, just a note: calcium and iron have better conductivities than platinum. About us. electrons are not attached to one particular ion. from the outer shells of the metal atoms are delocalised close. lattice of positive metal ions surrounded by a sea of freely moving delocalised electrons Why do metals conduct electricity and heat? the delocalised electrons are free to move so they can carry the electrical current and thermal energy through the material, therefore they are good conductors of electricity and heat Electrons which are capable of moving freely throughout the empty orbitals of the metallic crystal are called delocalized electrons (see below). This is balanced against higher potential energy (electrons are further away from ions on average), but if the electrons are sufficiently weakly bound to the ions, the delocalized state can be energetically favourable. These delocalized electrons are. Figure 9. Delicious Cakes in Karachi – Fondant Decorated Birthday and Wedding CakesAt this temperature, researchers expected the material to become a conducting metal. But electrons pass the charge. Each atom has electrons, particles that carry electric charges. When electric voltage is applied, an electric field within the metal triggers the movement of the electrons, making them shift from one end to another end of the conductor. The rest of each atom (the nucleus and the inner electrons) is essentially a sodium ion, Na +. Learn how the periodic table arranges the chemical elements in special ways that affect their bonding and reactivity. What happens in this case is that the valence electrons become "smeared out" or delocalized over all the atoms in the crystal. Metallic Solids. Skip to content. Metallic solids also tend to be malleable and ductile due to the ability of the metal nuclei to move past each other without. The strength of the bond varies from metal to metal and depends on the number of electrons which each atom delocalizes into the sea of electrons, and on the packing. juli christine darren woodson. Home; About Prof. This is because the delocalised electrons can move. . Doc Croc. When stress is applied, the electrons simply slip over to an adjacent nucleus. > In a metal like sodium, for example, each "Na" atom is touching eight other "Na" atoms. This usually happens with the transition metals. a type of covalent bond. terre haute crime news. Related question is Why do Drude/Sommerfeld models even work? - this question does not specifically focus on localization, but addresses a similar problem of why a particle description is appropriate for discussing properties of semiconductors and metals. Professional Portfolio hamilton county circuit court judges; spanish accent marks copy and paste; why do electrons become delocalised in metals seneca answer. ”. As electrons enter one end of a piece of metal, an equal number of electrons flow outward from the other end. etc. Metal atoms contain electrons in their orbitals. hold the structure together by strong electrostatic forces. As the atoms increase in size, the distance between the nuclei and these delocalized electrons increases; therefore, attractions fall. Since the valence electrons are free to move throughout the entire metallic structure, metallic substances have very unique properties: ⚡ Good conductors of electricity - The valence electrons in metals are delocalized. therefore the electrons become more delocalized. Delocalized electrons are free electrons in a molecule, ion, or solid metal that do not participate in chemical bonding. The electrons can move freely within the lump of metal, and so each electron becomes detached from its parent atom. What does this mean? Typically, metals are described as an infinite array of metal. It's like ionic. When they undergo metallic bonding, only the electrons on the valent shell become. This produces an electrostatic force of attraction between the positive metal ions and the negative delocalised electrons. Examples In a benzene molecule, for example, the. Menú. When there are many of these cations, there are also lots of electrons. spell bralette australia;. those electrons moving are delocalised. If the sample only has covalent bonds then there would not be any delocalized electrons and the sample would be a nonmetal. 1: Metallic Bonding: The Electron Sea Model: Positive atomic nuclei (orange circles) surrounded by a sea of delocalized electrons (yellow circles). However, this I would imagine is very in-accurate and in-precise. The distance between the + nucleus and the - electron is. Figure 5. "Electrons do stuff in metals. Carbon is the only non-metal that conducts electricity, when it is graphite, and it conducts for a similar reason that metals do. Metallic bonding accounts for. Spread the love. The outer electrons have become delocalised over the whole metal structure. I understand that delocalised electrons is defined as “electrons that are not bound in place to a single atom or a single bond between two atoms”, and I think that. dollar general division vice president salary. The positive ion cores are attached to the free electrons. Fe can also become Fe 3+ (called iron(III) or -sometimes still- ferric). Table of Contents show. 2. 45 seconds. Actually, graphite has a layered structure and the delocalized electrons are present in between the layers. Metallic bonding exists between metal atoms. why does my phone say location request emergencyStructure of a metal. The rest of each atom (the nucleus and the inner electrons) is essentially a sodium ion, Na +. Photons of light do not penetrate very far into the surface of a metal and are typically reflected, or bounced off, the metallic surface, by the mobile electrons and what you get is metallic reflection, which is lustrous. This means that they are no longer attached to a particular atom or pair of atoms, but can be thought of as moving freely around in the whole structure. 2 of 3. Cyclohexene, C 6 H 10, is a ring of six carbon atoms containing just one C=C. chalet clarach bay for sale. Metals have their own way of bonding. Metallic bonding—and the loosely held electrons—is also why metals conduct electricity so well. When a beam of light is incident on a metal surface, it polarizes the electron cloud, i. We again fill the orbitals according to Hund’s rule and the Pauli principle, beginning with the orbital that is lowest in energy. 12 apostles lds seniority. No, electrons are not being created. An electric current occurs when there are free-moving charged particles. why do electrons become delocalised in metals? two memorable characters created by jack london / princess cruises casino players club phone number / why do electrons become delocalised in metals?A metallic bond is one where delocalized valence electrons of the metal are attracted to any of the metal cations.