what is nitrogen's valence of electron?
360598
N has atomic number 7- so electronic configuration is 2,5 whish emans its has 5 valence electrons in the L shell
199784
electrons have negative charge
772133
proton-neutron-proton\nproton = positive = +\nneutron = negative = -\nits for semiconductors
852560
Sn has a valence (charge) of +3, that is also its' oxidation number.\nSn had 3 valence electrons it lost so the next lowest level would have eight. Having lost the three electrons gave it a +3 charge.  \nNormally Sn has +4 or +2 as a oxidation number. It's charge in this molecule is +3 (an odd occurrence), I think it is written incorrectly, having never seen Sn as +3.\n\nCl has a charge of -1, it gained one electrons because it had 7 valence electrons, gaining the one gave it eight. \n\nA compound must be neutral, so three Cl are needed to counter the one Sn.
575353
That is simple- Just write down the the electronic configuration of the atomic number of that element. And the number of electrons in the last shell are the valence electrons.\n\nFor eg: Na(Sodium) has the atomic number 11, now there are four shells in which the distribustion takes place- namely- K,L,M,N.These shells are also known as energy levels. \n\nThe max no of electrons in K is 2, In L is 8, M is 16 and finally in N its 32.\nAnd you cant fill the next shell till the total number is completed in one shell.\n\nThere fore for Na the configuration is: K= 2 L= 8 M= 1\nAnd hence the valence electron is 1. That is only one electron partcipates in bond formation and in chemical reactions.
778586
It's in the 6th row, so n= 6.\nIt's in the first column of the "p" block of the table, so it's highest energy electron is 6p1\n\nStarting from Xe, and following the atomic numbers, these are the orbitals that are filled :\n\n[Xe] 6s2 4f14 5d10 6p1\n\nThe valence electrons are the ones with the highest quantum numbers: 6s2 6p1.
832259
N cannot expand its outer level to more than 8 electrons, because it is in Period 2.  NF5 would require there to be 10 electrons in the outer level of N.
1124895
The NH3 molecule has an unshared pair of electrons and the H+ ion has lost the one electron in its outermost shell. This enables NH3 to readily donate its unshared pair of electrons and H+ to readily accept that pair. That way, they form a dative covalent bond, in which both H+ and NH3 act simultaneously on each other.  The NH4+ ion is formed, in which the charge is distributed over the whole structure.  It is not localised on any atom. The overall charge is +1 originating from the H+ ion.
227254
The general valence shell electronic configuration is\nns2 np3.\nAnd the elements along the group are :-\n1.Nitrogen (N)\n2.Phosphorous (P)\n3.Arsenic (As)\n4.Antimony (Sb)\n5.Bismuth (Bi)\n6.Ununpentium (Uup)\n\nCheck it out in various books above 10th grade
836131
The correct answer is 3 Nitrogen \n\n7 electrons as follows 1s2 2s2  2p3  . The sublevel 2p3 can theoretically contain  6 electrons and has only 3\n\n\nHelium and neon are noble gases. All the sublevels are filled\n\nBeryllium  has  4 electrons and  2 on shell K 2 and 2 on sublevel 2s complete
698948
1)   O::C::O  for CO2 because there are total 4 valence electrons in outermost orbit of carbon so it will share 2 with each oxygen and it has 3 resonance structures\n\n2)  H . . C three electrons shared from carbon and nitrogen N\nie on one side one electron sharing by hydrogen and carbon and on other side 3-3 electrons shared by both carbon and nitrogen\n\ni hope it helps you out
298745
The kernel of an atom is the nucleus and all of the electrons. The remaining electrons are the valence electrons, equal in number to the charge of the kernel in electronic units. This term is used when doing Lewis dot structures. The kernel is represented by the elemental symbol and the dots surrounding it represent the valence electrons.
954154
Valency number is the combining power of an atom or group of atoms and is used to work out the formulae of compounds. It used to be defined as how many hydrogen atoms am atom or group could combine with or displace. Nowadays it is the number of electrons the element or group can give, take or share. A sodium atom will give away one electron so it has a valency number of +1. Chlorine will take an electron so it has a valency of -1. When working out the formula of a compound the valency numbers must add up to zero. So in sodium chloride there is one of each atom as the +1 and -1 add up to 0. The formula is NaCl. The group sulphate SO4 has a valency number of -2 and so in sodium sulphate you would need two sodiums (each +1) for one sulphate and so the formula of sodium sulphate is Na2SO4.  Copper has a valency of +2 so copper sulphate would have one copper and one sulphate group (+2 and -2 = 0) so its formula is CuSO4. If you end up with a formula with more than one of a group - the group has to be enclosed in brackets as in Copper nitrate where the nitrate, NO3  is -1 and the copper is +2 you need 2 nitrates. The formula is Cu(NO3)2\nCarbon can share 4 electrons and hydrogen can share 1 electron. So carbon is considered as -4 and hydrogen +1. The formula for the simplest compound of carbon and hydrogen is therefore CH4 (methane).
150155
Carbon bound to Nitrogen by a triple bond.
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a the number of outer electron that will bond with other atoms to fill thei valence shells
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A valence electron is the outer most shell of electrons in an atom
851509
There are two possibilities. Follow this link for a picture of the first possibility. http://img175.imageshack.us/img175/8223/ncssh2.jpg\n\nBasically, all 3 of these elements follow the octet rule (they want 8 electrons in their outermost shell), and as you can see, they all have 8. Now, S is carrying the - sign because it's formal charge is -1. Formal charge is calculated by Formal Charge=# of electrons the element has (S brings in 6) - the # of electrons it "owns" within the bond. Sulfur "owns" 7 in this case (3 lone pairs and one in a shared covalent bond--thus (3*2)+1=7.\n\nTherefore Formal Charge of Sulfur (in this case): is -1 because\n\n6-7=-1\n\nI probably made it sound more confusing than it is. Sorry about that.\n\nBut other than that, you know that Carbon should be the central atom here because it's coming in with only 4 electrons in it's valence shell, so it's more needy than Nitrogen with it's 5 and Sulfur with it's 6. So you stick it in the middle and then pretty much trial and error. \n\nThe other possibility is here.\nhttp://img175.imageshack.us/img175/6659/ncs2wf4.jpg\n\nThis time Nitrogen is carrying the -1 formal charge, because it comes into the bond with 5 electrons in it's valence shell, but it "owns" 6 in this case (2 lone pairs and 2 electrons out of the 4 in the N=C double bond..(2*2)+2=6. So...Formal charge of -1 comes from \n\n-1=5-6\n\nEven though these two molecules look different, they are in fact the same. This is a concept called resonance. \n\nI hope this wasn't too confusing.