Particles+of+Elements+Sheet

Number || Atomic Mass || Number of Protons || Number of Neutrons || Number of Electrons || 1. The atomic masses given in this chart are whole numbers. How are the atomic masses in the periodic table different and why?
 * Element Name ||  || Atomic
 * Technetium ||  ||   || 98 ||   ||   ||   ||
 * Gold ||  ||   || 197 ||   ||   ||   ||
 * || Br ||  || 80 ||   ||   ||   ||
 * ||  || 40 ||   ||   || 51 ||   ||
 * ||  || 87 ||   ||   || 136 ||   ||
 * Gallium ||  ||   || 70 ||   ||   ||   ||
 * ||  || 96 || 247 ||   ||   ||   ||
 * || K ||  || 39 ||   ||   ||   ||
 * Hydrogen ||  ||   || 1 ||   ||   ||   ||
 * ||  || 8 || 16 ||   ||   ||   ||
 * || C ||  ||   ||   || 6 ||   ||
 * || H (D) ||  ||   ||   || 1 ||   ||
 * || Fe ||  ||   ||   || 30 ||   ||
 * ||  || 13 || 27 ||   ||   ||   ||
 * Uranium ||  ||   ||   ||   || 135 ||   ||

2. If the atomic mass of an element can vary, how is more than one mass accounted for in the periodic table? Give an example.

3. Electrons are so small that they don’t factor into the atomic mass of an atom. Yet, they account for most of an atom’s volume. Explain why this is so.



Hints: __ Atom Facts __ a. Atomic number = how many protons b. Atomic number determines the kind of atom c. Atomic mass = Protons + Neutrons d. Atomic mass – Protons = Neutrons e. Atomic mass – Neutrons = Protons f. Isotopes – Element with different numbers of neutrons 7. Protons (+), neutrons (0), electrons (-) /Protons have a positive charge, neutrons have no charge, and electrons have a negative charge. 8. Usually atoms have a neutral charge, because each proton will attract one electron to the atom.