The most common isotope has 7 neutrons.
To calculate this, look up the element on a Periodic Table, subtract the atomic number from the atomic weight, and round to the nearest whole number. Nitrogen, for example, has an atomic number of 7 and an atomic weight of 14.006. 14.006 - 7 = 7.006, which rounds to seven. Most of the low numbered elements have a number of neutrons equal to their atomic number, but the ratio starts to vary in the heavy elements.
>>M.T.<<
There are seven neutrons, seven electrons, and seven protons in a nitrogen atom.
Which isotope of nitrogen? The isotope which is most common by far has 7, but the one with 8 is also stable, and isotopes with anywhere from 3 to 18(!) neutrons are known.
A neutral nitrogen atom has 7 protons and 7 neutrons in its nucleus and 7 electrons in orbitals around the nucleus.
The Bromine atom contains: 35 protons, 35 electrons, and 45 neutrons.
14 (mass number) - 7 (number of protons) = 7 (number of neutrons)
This is an easy problem to solve if you have a Periodic Table of Elements.# protons + # neutrons = atomic number3 + 4 = 7The element with the atomic number 7 is Nitrogen.
The "atomic number" of an element is the number of protons in its atoms. The number of neutrons may be different, creating "isotopes" of the element. Altering the number of protons in an atom changes it to a different element. Since oxygen atoms contain 8 protons, losing one would create an atom of NITROGEN, containing 7 protons. Isotopes are listed by the "mass number", which is the total number of protons and neutrons in an atom. An atom of oxygen would normally be oxygen-16, with 8 protons and 8 neutrons. Losing one proton from this atom would create NITROGEN-15, a stable isotope of nitrogen with 7 protons and 8 neutrons.
7 neutrons in Nitrogen 14
7
6 neutrons
In a nitrogen-14 atom, there are 7 neutrons, where the isotopes with mass numbers with 13 and 15, have 6 and 8 neutrons respectively.
no electrons
N-14 is the most common isotope of nitrogen atom and it has 7 protons, 7 neutrons
Every nitrogen atom has 7 electrons. There are 7, 8 and 9 neutrons in nitrogen-14, nitrogen-15 and nitrogen-16 isotopes respectively.
7 protons, 7 electrons and 8 neutrons
Number of neutrons = Atomic mass of an isotope - Atomic number of the element For the most important natural stable isotope of nitrogen - 14N - the number of neutrons is 7.
there are 7 neutrons because when you take away the number of protons, which is 7 as well, from the atomic mass, which is 14 when rounded, you get 7 which is the number of neutrons in nitrogen.
Chemically there is no difference between radioactive nitrogen and stable nitrogen. Both will react the exact same way in all chemical reactions. The only difference between the two is the number of neutrons in the nucleus. This means the only difference is mass. If the nitrogen atom has too many neutrons, it will most likely give off a beta particle. The beta particle shoots out from one of its neutrons. That neutron then becomes a proton and the nitrogen becomes oxygen. If the nitrogen atom has too few neutrons, a proton in its nucleus may capture one of its own electrons and turn into a neutron. This would then turn the nitrogen atom into a carbon atom.
Nitrogen has 7 neutrons.