Atomic Structure

An updated version of this lesson is available at Visionlearning: Atomic Theory & Ions & Isotopes

Last year you learned that atoms were particles of elements, substances that could not be broken down further. In examining atomic structure though, we have to clarify this statement. An atom cannot be broken down further without changing the chemical nature of the substance. For example, if you have 1 ton, 1 gram or 1 atom of oxygen, all of these units have the same properties. We can break down the atom of oxygen into smaller particles, however, when we do the atom looses its chemical properties. For example, if you have 100 watches, or one watch, they all behave like watches and tell time. You can dismantle one of the watches: take the back off, take the batteries out, peer inside and pull things out. However, now the watch no longer behaves like a watch. So what does an atom look like inside?
Atoms are made up of 3 types of particles electrons , protons and neutrons . These particles have different properties. Electrons are tiny, very light particles that have a negative electrical charge (-). Protons are much larger and heavier than electrons and have the opposite charge, protons have a positive charge. Neutrons are large and heavy like protons, however neutrons have no electrical charge. Each atom is made up of a combination of these particles. Let's look at one type of atom:

A neutron walked into a bar and
asked how much for a drink.
The bartender replied,
"for you, no charge."

-Jaime - Internet Chemistry Jokes

The atom above, made up of one proton and one electron, is called hydrogen (the abbreviation for hydrogen is H). The proton and electron stay together because just like two magnets, the opposite electrical charges attract each other. What keeps the two from crashing into each other? The particles in an atom are not still. The electron is constantly spinning around the center of the atom (called the nucleus). The centrigugal force of the spinning electron keeps the two particles from coming into contact with each other much as the earth's rotation keeps it from plunging into the sun. Taking this into consideration, an atom of hydrogen would look like this:

A Hydrogen Atom

Keep in mind that atoms are extremely small. One hydrogen atom, for example, is approximately 5 x 10^-8 mm in diameter. First of all, the electron actually spins very far from the nucleus. If we were to draw the hydrogen atom above to scale, so that the proton were the size depicted above, the electron would actually be spinning approximately 0.5 km (or about a quarter of a mile) away from the nucleus.

In an electrically neutral atom, the positively charged protons are always balanced by an equal number of negatively charged electrons. As we have seen, hydrogen is the simplest atom with only one proton and one electron. Helium is the 2nd simplest atom. It has two protons in its nucleus and two electrons spinning around the nucleus. With helium though, we have to introduce another particle. Because the 2 protons in the nucleus have the same charge on them, they would tend to repel each other, and the nucleus would fall apart. To keep the nucleus from pushing apart, helium has two neutrons in its nucleus. Neutrons have no electrical charge on them and act as a sort of nuclear glue, holding the protons, and thus the nucleus, together.

A Helium Atom

As you can see, helium is larger than hydrogen. As you add electrons, protons and neutrons, the size of the atom increases. We can measure an atom's size in two ways: using the atomic number (Z) or using the atomic mass (A, also known as the mass number). The atomic number describes the number of protons in an atom. For hydrogen the atomic number, Z, is equal to 1. For helium Z = 2. Since the number of protons equals the number of electrons in the neutral atom, Z also tells you the number of electrons in the atom. The atomic mass tells you the number of protons plus neutrons in an atom. Therefore, the atomic mass, A, of hydrogen is 1. For helium A = 4.

Ions

So far we have only talked about electrically neutral atoms, atoms with no positive or negative charge on them. Atoms, however, can have electrical charges. Some atoms can either gain or lose electrons (the number of protons never changes in an atom). If an atom gains electrons, the atom becomes negatively charged. If the atom loses electrons, the atom becomes positively charged (because the number of positively charged protons will exceed the number of electrons). An atom that carries an electrical charge is called an ion. Listed below are three forms of hydrogen; 2 ions and the electrically neutral form.


H⁺ : a positively charged hydrogen ion	H : the hydrogen atom	H^- : a negatively charged hydrogen ion

Isotopes

Neither the number of protons nor neutrons changes in any of these ions, therefore both the atomic number and the atomic mass remain the same. While the number of protons for a given atom never changes, the number of neutrons can change. Two atoms with different numbers of neutrons are called isotopes. For example, an isotope of hydrogen exists in which the atom contains 1 neutron (commonly called deuterium). Since the atomic mass is the number of protons plus neutrons, two isotopes of an element will have different atomic masses (however the atomic number, Z, will remain the same).

Two isotopes of hydrogen


Hydrogen Atomic Mass = 1 Atomic Number = 1	Deuterium Atomic Mass = 2 Atomic Number = 1

If you would like to explore the interaction of protons and electrons further, the University of Colorado's Physics 2000 site has an interesting experiment posted on line. At the Electrical Force page, you can place an electron next to a proton and see how the electron moves. You can even try to build your own atom (and see how difficult it is)! <