Understanding Atoms, Ions, and Isotopes

Understanding Atoms, Ions, and Isotopes

It is important to know the difference between atoms, ions, and isotopes in chemistry. An atom is the smallest unit of a chemical element, consisting of protons, neutrons, and electrons. Ions are electrically charged atoms or molecules, with either a positive or negative charge. Isotopes are variants of a particular chemical element which have the same number of protons and electrons but differ in the number of neutrons.

Explanation

Isotope: Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons in their nuclei. This results in variations in atomic mass for isotopes of the same element.

The statement that an atom of oxygen and the ion of oxygen both have 8 protons is correct because ions are formed by the gain or loss of electrons, not protons. Meanwhile, the statement that isotopes are formed by adding or removing neutrons from the nucleus is true, as this affects the atomic mass of the element.

It is important to note that removing electrons from an atom to form an isotope is incorrect, as this would change the atomic number and, consequently, the element itself. Additionally, the calculation of atomic mass is done in the same way for metals and non-metals, so there is no difference in this regard.

Electrons are actually the least massive of the subatomic particles, with protons and neutrons being much more massive. Lastly, while the isotope of carbon has 6 protons and different numbers of neutrons, the atom of nitrogen has 7 protons in its nucleus.