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From the Periodic Table, you can see that nitrogen has three unpaired electrons in its outer (valence) shell. It needs to gain three more electrons to pair with the three already in the shell in order to reach a stable configuration. Another way to get to the answer is to see that nitrogen has five valence electrons total (paired and unpaired). The outer shell needs eight electrons total to be like a noble gas, so the addition of three electrons will fulfill the octet rule.
Nitrogen has 5 valence electrons. In order to achieve the electron configuration for the nearest noble gas (neon), it must gain 3 more. Once it does this, it has the 1s22s22p6 configuration, which is the same as neon's. *Note: nitrogen does not become neon; it just gains electrons.
Nitrogen has 5 valence electrons, so it needs to gain another 3. This gets it to the noble gas configuration, which is stable.
it has to gain 3 electrons
Nitrogen has to gain three electrons
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Since nitrogen is a non-metal with five electrons in its valence shell, it will gain three electrons to attain a stable electronic configuration. So its valency is -3.
Sulfur has six valence electrons and can therefore attain an inert gas configuration in two different ways: by accepting two electrons to attain the electron configuration of argon or donating or sharing six electrons to attain the electron configuration of neon. In combination with the much less electronegative element sodium, sulfur accepts one electron from each of two sodium atoms to form the ionic compound Na2S, but in combination with the more electronegative element fluorine, sulfur shares its six valence electrons with each of six fluorine atoms to form six polar covalent bonds with fluorine.
Lithium is in group 1 of the Periodic How_many_electrons_must_the_lithium_atom_give_up_to_become_stable, so it must lose one electron for it to attain a full outermost energy level and become stable.The charge will then be positive (+).
iodine has 7 electrons in the valence shell. and needs one more electron to attain stable noble gas configuration. So it gains one electron and forms iodide ion with charge of -1.
Generally, atoms would want to fulfill the octet rule: 8 electrons in the valence shell. This gives the atom a noble gas configuration and is seen as stable. Since the Chlorine atom is in group 7 of the periodic table, it "prefers" to gain one electron instead of losing 7 to attain the stable octet configuration.
nitrogen should give 5 electrons (or better gain 3 electrons) to attain noble gas configuration.
three
Calcium loses two electrons to obtain a noble-gas electron configuration.
Since nitrogen is a non-metal with five electrons in its valence shell, it will gain three electrons to attain a stable electronic configuration. So its valency is -3.
two electrons lost
true, just not for Boron witch tries to gain 6 electrons for a stable arrangement
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It loses 2 electrons and becomes a +2 ion.
aluminium should lose three electrons to attain noble gas configuration
This is because in nitrogen the 2p subshells are filled by 3 electrons which is half filled electronic configuration. But oxygen has to lose an electron to attain the half filled electronic electronic configuration. Hence nitrogen is more stable than oxygen.
Krypton is a noble gas and need not lose electrons. It is already stable.