Explain, in terms of subatomic particles, the difference
between S-32 and S-34
S-32 has 16 electrons, 16 protons, 16 neutrons.
S-34 has 16 electrons, 16 protons, 18 neutrons.
For neutral atoms, #protons = #electrons.
mass number (in this case either the 32 or 34) = #protons + #neutrons.
The mass of S-34 is greater than the mass of S-32
To understand the difference between S-32 and S-34, we need to delve into the world of subatomic particles. S stands for sulfur, while the numbers 32 and 34 represent the atomic mass of the isotopes.
Isotopes are atoms of the same element that have the same number of protons but differ in the number of neutrons. Protons carry a positive charge, while neutrons have no charge. Together, they make up the nucleus of an atom.
In the case of sulfur, S-32 refers to an isotope that contains 16 protons and 16 neutrons, while S-34 has 16 protons and 18 neutrons. Atomic mass is the sum of protons and neutrons in an atom.
The primary difference between S-32 and S-34 is that they have different atomic masses due to the varying number of neutrons. This variation in atomic mass can affect the behavior of the isotopes in terms of stability, chemical reactivity, and radioactive decay.