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NF5 (Ninja Force 5) is a highly trained ninja clan trained by Master Sensei (whose name will not be released for security reasons). Little is known about the clan except to its members (whose names will also not be released). Such events as the eighth grade formal crash of 2006 and the humiliating defeat of Mike Bolin's clan (MF4) were speculated to have been carried out by these renegade ninjas, though evidence is scarce.
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What is the formula for nitrogen pentafloride?
NF5
What is the formula for nitrogen pentafluoride?
The formula for nitrogen pentafluoride is NF5. It is a compound composed of one nitrogen atom and five fluorine atoms.
Why PF5 is known but neither NCl5 nor NF5 is known?
There are 5 outermost electrons in both phosphorus and nitrogen atoms but in nitrogen no more than three unpaired electrons are possible due to absence of d-orbitals in 2nd energy level so nitrogen may form only three covalent bonds (as NCl3 and NF3) but d-orbitals are present in 3rd energy level of Phosphorus so in excited state it may have five unpaired electrons and may form PCl5.
What makes the noble gasses so special or why do they not form compounds with any other element?
The noble gases, or "rare" gases, do not usually form compounds with other elements because they have a full valence shell. This means that to remove or add an electron requires considerable energy, so it is not favorable. However, there are a few exceptions, such as compounds involving Argon and Fluorine. Fluorine is so electronegative and has such a high (very negative) electron affinity that it can remove one of the valence electrons of Argon.Ouch... let's touch on the things wrong with this response because it is educational to see why some of what was said above is wrong. If you just want the answer, skip down to the bold text.1. Noble gases are not "rare". Argon makes up almost 1% of all gas in our atmosphere... far more than the amount of CO2.2. Elements don't just form compounds by adding or removing electrons. What the answerer said was true---it is really freaking hard to add or remove an electron from a noble gas, but that does not address covalent bonding, which involves sharing electrons (a mutual attraction of valence electrons by two nuclei).3. Fluorine CANNOT remove an electron from argon. Fluorine's electron affinity is -328 kJ/mol... the ionization energy of argon is 1521 kJ/mol. So it comes up a bit short. Fluorine's electron affinity isn't even high enough to remove an electron from sodium, but an electron does transfer because of the lattice energy that is released when you hook up an Na+ and an F-. No lattice energy is going to overcome the 1521 kJ of energy required to pull the electron off of argon.4. Only one compound has ever been formed with argon, and that is the metastable HArF. It is formed only at extremely low temperatures by breaking an H-F bond with a laser inside a frozen matrix of Ar. The reason it has to remain frozen is because if the molecules were allowed to move at all they would collide and immediately convert back into HF and Ar. Although this compound has some interesting bonding characterisitics related to the very different electronegativities of Ar, F, and H, its formation does not involve removing electrons from the argon as its presence was detected by observing Ar-F bond vibrations (covalent bond).5. Most calculations of the electronegativity of argon put it around 3.2 to 3.3, giving it the 3rd highest electronegativity of any atom on the periodic table. So it is comparable to that of fluorine.Now noble gases such as krypton and xenon (and theoretically argon) can form polar covalent bonds with elements like fluorine and oxygen (the polarity strengthens the bond).What an atom needs to form a covalent bond is space within their atomic orbitals to put shared electrons. Helium and neon have full valence shells---they have no space in their 1st shell in the case of helium or 2nd shell in the case of neon. Therefore, helium and neon CANNOT form compounds.Argon, krypton, and xenon DO have empty orbitals in their valence shells---the unoccupied d-orbitals that fill after the next shell is created. It can use those valence orbitals to share electrons and form covalent bonds. Krypton uses is 4d orbitals, xenon uses its 5d orbitals, and presumably argon used its 3d orbitals when they made HArF.Recent calculations shows that the contribution d-orbitals in the hypervalent compounds is just 2%; ie. neglegibly small. Therefore there are some predictions for NF5 (Nitrogen pentafluoride) and HHeF (Helium fluorohydride analogous to HArF). In the latter helium would use its 1s orbital for bonding with hydrogen and 2p with fluorine!. But the neon analogue HNeF was predicted to be incapable of existence! So the reactivity of noble gases follow a surprising order: Ne < He < Ar < Kr < Xe and < Rn (Very likely)
