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Answered 2011-02-05 21:59:38

Valence electrons are the outermost ring of electrons that are shared between atoms to form covalent bonds or exchanged to form ionic bonds

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they serve a very important roll , bonding is based off them. covalent bonds share valence electrons in order to have a complete electron shell. ionic bonds are also between the valence, where one atom gives another electrons in order to complete it.


Electrons, specifically valence electrons.


To help the particle such as chlorine which has 7 valence electrons in the outermost shell to obtain a stable octet structure, which has 8 valence electrons to become stable and less reactive, the valence electron will undergo covalent bonding to bond with another chlorine atom to obtain a chlorine molecule that is stable and less reactive.


Electrons play a major role in many chemical bonds. There is one type of bonding called electrovalent bonding (ionic) where an ion from one atom is transferred to another atom. It is an even trade, creating two ions. The second type of bonding is called covalent bonding. Electrons are actually shared between two or more atoms in a cloud. Both types have specific advantages and weaknesses.


The valence electron are involved in the sharing of electrons with the other atoms to form ionic bonds.


In chemical bonding electrons are involved.


IDK that is why i asked it!!The electrons in the valence shell form chemical bonds with other atoms in order to form compounds.


Metals have metal bonds. valence electron make bonds with metal ions.


Valence electrons are electrons on the outermost "level". And depending on its electron configuration, it plays a role in which if the atom requires to gain or lose electrons in order to become "stable", it can accept or give electrons to another atom in a chemical reaction.



According to the Octet Rule, the most valence electrons any atom can have is 8. Atoms naturally want to meet this rule either by losing or gaining enough electrons to have a total of 8 valence electrons. The nobel gases have exactly 8 valence electrons. The neither need to lose or gain any and therefore do not play well with others. The losing or gaining of valence electrons determines the stability and reactivity of the element.


Valence electrons are the electrons on the outer most shell of a neutral atom; they are used when forming chemical bonds with other atoms. Because of the octet rule - which is a chemical bonding theory based on the assumption that in the formation of compounds, atoms exhibit a tendency for their valence shells to either be empty or a full 8 electrons (octet) - atoms that do not have an octet need to either get rid of their electrons or gain more electrons. Atoms combine with other atoms in order to stabilize themselves. For example if sodium and chlorine were to combine sodium would need to lose 1 valence electron while chlorine would need to gain 1 valence electron. Na + Cl ------> NaCl FYI NaCl, sodium chloride, is table salt. *NB* All elements react in order to become stable and either get an octet or empty their shell. They are all attempting to be like the noble gases, which are hellium, neon, argon, krypton..etc. FYI noble gases are all stable and have 8 valence electrons.


Electrons are in design made to balance out protons, because electrons, being negative, will even out the positive charge of the protons. Additionally they play a big part in the electrovalent and covalent chemical bonds.


Someone else answered this with :O=O-Al-Al=O:, but since 26 electrons are available, and Al doesn't have full octets, i think it's wrong. Or, just possibly, I am. There are 24 valence electrons available. The stable oxygen ion will move to the electron configuration of the noble gas neon to gain 2- electrons. While Aluminum loss or transfer its 3+ valence electrons to also become the noble gas neon. The Octets Rule is now is play for the 24 valence electrons. :Ö =O=Al=Al=Ö:


They play a HUGE role. This is because this is the most fundamental principle that governs chemical reactions. For example, the classic tablesalt compound. Sodium (Na) has a single valence electron, while Chlorine (Cl) has seven valence electrons. Elements of this size (atomic mass) usually want to have a total of 8 valence electrons. Well guess what? Sodium wants to get rid of that bothersome electron to have a complete shell rather than another incomplete shell. Chlorine wants to fill its shell so it happily takes it. Now Sodium has a filled shell and so does Chlorine. This means that sodium is positive and the chlorine is negative and so they bond from the difference in charge. Voila we have tablesalt. This is just one of many examples showing the importance of valence electrons in chemistry. This was an example of an ionic bond because an electron was completely given and not shared like in a covalence electron. The term "covalence" implies that the valence electrons will co-exist between the atoms, like in water (H20).


iron ion will have the same number of protons as iron atom because while bonding there is loss of electrons only and protons play no role. thus, the number of protons will be same..


electrons are what creates the bond, the type and the force. compounds are either held by the static electricity and are just attracted to each other (Ionic bond) or they are held by the actual sharing of an electron to "fill a shell" Some elements desperately want electrons, and some easily give them away. (Covalent Bond)


Chemistry is mostly concerned with nothing smaller than the protons, neutrons, and electrons when dealing with atoms. Photons do play a part in some disciplines of chemistry, but are mentioned less often. The bonding of atoms into molecules is also a key idea in chemistry, which is concerned with the transfer or sharing of electrons.


The trend for atomic radius, and most other trends on the periodic table, can be explained by the amount of attraction between the positively charged nucleus and the negatively charged electrons. Other factors that come into play are the number of electrons in the outer energy level (valence shell) and the distance between the outer electrons and the nucleus (number of energy levels.)


all you have 2 do is get an item for bonding and play with it for 34 times.


Electronegativity (EN) is a property calculated from Ionization Energy and Electron Affinity. If EN difference is more than 1.7 , it is considered IONIC bond and less than that it is categorized as COVALENT bond. Again, it is not a phenomenon that is observed that plays a role but a value calculated. HOpe this helps.


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The role electrons play in stabilizing an atom is they balance out the charge of the protons. If an element has more protons than electrons, it has a positive, not neutral, charge, and vice versa. Unpaired electrons can cause an element to be chemically reactive and/or radioactive. Hope this helps!


Basically, the Electron shells in an insulator are complete, they are not prone to accepting external electrons or donating any of theirs. As such they aren't waystations for electrons looking to move (conduct). There is a need to slip away from what's going on with individual atoms when looking at conductivity (which can be used to sort out insulators from conductors). When a whole bunch of atoms or molecules are put together, a number of other opportunities or places for electrons to exist are created. The valence band of a given atom is subordinated and another type of "valence band" is set up. This new valence band (we are assigning a new definition) does not have a given energy level (like it would for a given atom) but, rather, has a range of allowable energy levels. This is because the many different atoms and molecules when combined to make up whatever it is we are making provide other places (energy levels) in which electrons can hang out. (Let's give Fermi, Schrödinger, Bloch and Brillouin the day off to keep from running off the page.) We have our newly defined valence band as a range of energy levels which an electron can occupy. (These were not available in a single atom of the material.) In a conductor, the band of energies in which an electron must be to support current flow actually are so low that they overlap part of the valence band. That means electrons in the material can support conduction and play musical electrons. In an insulator, there is a gap between the valence band (that group of energy levels allowed by the material as a whole) and the conduction band. Electrons cannot support conduction because they cannot reach the higher energy bands necessary to support it.


In photosynthesis electrons play a important role for example; NADP grabs a hydrogen atom to form NADPH



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