An atom of Boron-10 (B10) contains 5 protons and 5 neutrons.
Understanding the Composition of Boron-10
Every atom is defined by its number of protons, which is known as its atomic number. Boron (B) is element number 5 on the periodic table, meaning any atom of Boron will always have 5 protons.
The "10" in B10 represents the mass number of this specific isotope. The mass number is the total count of protons and neutrons in an atom's nucleus.
To determine the number of neutrons, you subtract the number of protons from the mass number:
- Mass Number (10) - Number of Protons (5) = Number of Neutrons (5)
Therefore, a B10 atom consists of 5 protons and 5 neutrons. For a neutral atom, the number of electrons is equal to the number of protons, meaning a 10B atom also contains 5 electrons.
Breakdown of a B10 Atom
Here's a quick summary of the subatomic particles in a neutral Boron-10 atom:
| Particle | Count | Location | Charge |
|---|---|---|---|
| Protons | 5 | Nucleus | +1 |
| Neutrons | 5 | Nucleus | 0 |
| Electrons | 5 | Electron Cloud | -1 |
The Concept of Isotopes
While the number of protons defines an element, the number of neutrons can vary, leading to different isotopes of the same element. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons, and thus different mass numbers.
Consider the following:
- Adding a proton to 10B: If a proton were added to 10B, it would result in the symbol 10C. This would no longer be Boron, but Carbon, as the element identity changes with the number of protons.
- Adding a neutron to 10B: If a neutron were added to 10B, it would result in the symbol 11B. This atom would still be Boron (because it still has 5 protons), but its mass number would increase to 11. The atom 11B is an isotope of 10B because they both have the same atomic number (5 protons) but different mass numbers (10 vs. 11).
This distinction highlights that while atoms of the same element always have the same number of protons, their neutron count can vary, leading to different isotopes with slightly different masses.
