(50 POINTS, PLEASE HELP!!) Go back and read the goals for this lesson on page 1. Form a summary statement for each goal, showing you understand and have met the goals of this lab. Be sure to explain all major concepts and relationships presented in this lab. (3-5 sentences) Goals:
Compare the sizes, charges, and relative positions of the subatomic particles: protons, neutrons, and electrons.
Relate an atom’s number of protons to its charge, name, and atomic number.
Calculate the mass number of an atom by summing the protons and neutrons.
Understand the definition of isotope.

An atom is made of up subatomic particles called protons, neutrons and electrons. The center of an atom is called the nucleus and is where the protons and neutrons are held while electrons orbit the nucleus in orbital shells. A electron has a negative charge, a proton has a positive charge, and a neutron has no charge (neutral).

The atomic number of a atom is the total amount of the atom's protons. In a neutral atom (Not an ion), the amount of electrons is the same as the protons. Therefore, the atomic number also tells the amount of electrons in the atom.

A ion is a negatively or positively charged particle due to the giving or taking of electrons with one or more atoms (Called an ionic bond). An atom that gives away electrons becomes positively charge because that atom now has more protons than neutrons. An atom that takes an electron becomes negatively charge because that atom now has more electrons than protons.

Atomic Mass is the sum of an atom proton and neutrons. To determine how many neutron an atom has, subtract the atomic mass from the atomic number. Electrons do not play a part in atomic mass as their mass is  1/1,836 of a proton's mass.

A isotope is two or more forms of the same element that contain equal amounts of protons but different amount of neutrons.