Two stable ones, 10 & 11. Several unstable.
isotopes are just things of the same element without one or more nuetrons
Boron is both: Isotopes with mass numbers of 10 and 11 occur naturally, and isotopes with mass numbers of 8, 9, 12, and 13 have been synthesized.
There are several isotopes of Boron, which have different levels of abundance. I don't know the accurate numbers, but say like 25% of Zu-isotopes are 1 amu, and 75% of Zu-isotopes is 2, it would be 1.75 amu for the Atomic mass. Relating Zu to B of course, what I mean is Boron's different isotopes appear in different abundances and have different masses. 14% of boron may be about 6.882 amu, but just think about it like the above analogy of Zu, where Zu either weighs 1 or 2, but never 1.75. By the way, to find amu for an element: (%1*Iso1)+(%2*Iso2)+[...]
It's an average number allowing for the relative abundances of different isotopes.
There is 13 isotopes in the element boron. xD
Boron-11 (80%) and boron-10 (20%).
Two stable ones, 10 & 11. Several unstable.
There are no radioactive isotopes of boron that are ordinarily found in nature. All elements have synthetic radioactive isotopes, however.
isotopes are just things of the same element without one or more nuetrons
1 and 3
Boron is both: Isotopes with mass numbers of 10 and 11 occur naturally, and isotopes with mass numbers of 8, 9, 12, and 13 have been synthesized.
Boron is both: Isotopes with mass numbers of 10 and 11 occur naturally, and isotopes with mass numbers of 8, 9, 12, and 13 have been synthesized.
Boron has 5 protons and 5 electrons Boron has two stable isotopes, one with 5 neutrons and 6 neutrons.
There are two isotopes of boron: boron-10 and boron-11 Both have 5 protons and 5 electrons per atomBoron-10 has 5 neutrons and boron-11 has 6 neutronsOverall this gives an atomic weight of 10.8 gmol-1
This is very simple, just look at the periodic table. Boron has the atomic number of 5, meaning that it has five protons and five electrons. As for the neutrons, most chemicals have isotopes, which means that one atom of an element may have a slightly lower or higher neutron count of an atom of the same element. In boron's case, it has two isotopes. Boron-10 would have 5 neutrons, and Boron-11 would have 6 neutrons, although boron-11 makes up somewhere in the range of 80% of known boron atoms.
Zero. There are NO boron atoms with a mass of 10.81 amu. The value of 10.81 is an average of the masses of the isotopes of boron.There are two stable isotopes of boron: boron-10 and boron-11, with masses of 10.012 amu and 11.009 amu. B-10 has a relative abundance of 19.9% and B-11 has a relative abundance of 80.1%.Do the math:10.012 x 0.199 + 11.009 x 0.801 = 10.81 amu