What is the atomic number, protons, neutrons and electrons of iodine
The correct answer and explanation is:
The atomic number of iodine is 53. This means that iodine has 53 protons in its nucleus. The atomic number also determines the number of electrons in a neutral atom. Therefore, iodine has 53 electrons.
The number of neutrons in an atom is determined by subtracting the atomic number from the atomic mass. The most common isotope of iodine has an atomic mass of approximately 127. Therefore, the number of neutrons in iodine can be calculated as follows:
Number of neutrons = Atomic mass – Atomic number
Number of neutrons = 127 – 53 = 74
Thus, iodine has 74 neutrons in its most common isotope.
In summary, for a neutral iodine atom:
- Atomic number: 53
- Protons: 53
- Electrons: 53 (since the atom is neutral)
- Neutrons: 74 (for the most common isotope)
These fundamental particles contribute to the overall properties of iodine. The number of protons defines its chemical behavior and place on the periodic table, while the number of neutrons influences its isotopic form and stability. Electrons, found in the electron cloud around the nucleus, are responsible for chemical bonding and interactions with other elements.