Atoms, Ions and Isotopes are commonly used in chemistry. While similar in some aspects, they have their differences.
An atom is the basic unit of chemical elements. It is the smallest particle of any element that still retains all of the properties of that element. Atoms are composed of three different subatomic particles: Protons, Neutrons and Electrons. Depending on the ratios of these three types of sub atomic particles, atoms can have a electrical charge. All of the atoms of an element will have the same number of protons and electrons. Changing the number of protons in an atom changes what element the atom is.
Isotopes are atoms that are of the same element that have the same atomic number but different numbers of neutrons. Carbon, as an example, is commonly found as the following isotopes: C-12, C-13, or C-14. The element of carbon still contain 6 protons, but the mass number changes due to the addition and subtraction of neutrons. Different isotopes of the same element still have the same chemical behavior
Ions are formed when atoms or groups of atoms lose or gain electrons to form electrical charges. This is caused when atoms transfer electrons between each other. When an atom loses an electron, it gains a positive charge. And the same can be said the other way. When an atom gains an electron, it also gains a positive charge. A good example of ions and ionic bonds is table salt (Sodium Chloride). The ionic charge of Sodium (Na) is positive, and the ionic charge of Chlorine (Cl) is negative. We can see these charges denoted with a positive (+) or negative (-) symbol as a superscript in the upper right hand corner.
These combine to form the neutral ion of Sodium Chloride.
As we can see, atoms, ions, and isotopes are dependent on the number of one of the three subatomic particles. The type of atom depends on the number of protons. The isotope of an element depends on the number of neutrons. And the ion depends on the electrons in an atom.
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