Elements and Atoms
An atom is the smallest particle of an element that retains the chemical properties of that element, and an element is defined as a substance that can’t be broken down or separated into simpler substances through a chemical reaction. Elements contain just one type of atom, and each different element contains a different type of atom. Take the element sulfur (S). A pile of sulfur (a yellow, powdery or crystallized substance) sitting on a table represents a single element—sulfur—and this pile of sulfur is made up of only one type of atom—sulfur atoms.
Each atom, regardless of its identity, is made up of three types of subatomic particles.
Protons, which are positively charged and situated at the center of the atom (also known as the atomic
nucleus);
neutrons, which are electrically neutral (meaning that they have no charge) and are also in the nucleus of the atom; and
electrons, which are negatively charged and are situated outside the nucleus. The majority of the mass of an atom is contained in its nucleus: while electrons are about the same size as protons and neutrons, an electron has 1/837th the mass of protons or neutrons. You should also be aware that the nucleus of an atom is much, much smaller and more dense than the space occupied by an atom’s electrons—if an atom were the size of a football field, the nucleus would be the size of a flea on the 50-yard line!
The number of protons an atom possesses is what gives the atom its identity—all atoms of a particular element have the same number of protons in their nuclei. For example, all of the sulfur atoms in the pile of sulfur we looked at above have 16 protons in their nucleus. If they had one more proton in their nucleus, they would have a different identity—they’d be chlorine (Cl) atoms, and with one less, they’d be phosphorus (P) atoms.
Atoms of a given element can, however, differ in the number of neutrons they contain, and atoms of the same element that have different numbers of neutrons are known as isotopes. Most elements have at least two isotopes that occur naturally, although a few have just one. Now take a look at how atoms are usually symbolized:
This represents a carbon atom that has 6 protons and 6 neutrons. In this notation, the atomic number (A), which is the number of protons the atom contains, is indicated by the subscript, and the mass number (Z ), which is the number of the atom’s protons plus the number of its neutrons, is indicated by the superscript. Some relatively common isotopes of carbon can contain 5, 7, or 8 neutrons, so although their atomic numbers would all be 6, their mass numbers, respectively, would be 11 (6 + 5), 13 (6 + 7), and 14 (6 + 8). Isotopes can also be written as carbon-14, carbon-15, carbon-16, etc., or C-14, C-15, C-16, where the number represents the mass number of the atom.
