Click on an element to begin
Periodic Trends
Periodic trends within the element period
- Atomic Radii: As the atomic number of elements in Period 3 increases, the atomic radius decreases.
- Ionic Radii: The ionic radii makes a gradual decrease except for the noble gas that is bigger than all the rest
- Reactivity: As you go farther down the period the reactivity decreases
- Electronegativity: As the atomic number of elements in Period 3 increases, the electronegativity increases.
- Ionization Energy: As the atomic number of elements in Period 3 increases, the ionization energy generally increases.
- Valence Electrons: Going to the right on the period increases the number of valence electrons by 1
- Electron Configuration: The only difference between these elements is the number which you would use to tell the position of the element and on all of them but the first two elements on the period because they are in the S group.
- Lewis Structure: In each of the lewis structures of these elements the energy level has a gradual increase in valence electron per element.
- States (phase) of matter at room temperature or 25 C: All of the elements in period 3 are solids except for argon and chlorine which are gases.
- Boiling Point: Boiling points generally increase going from sodium to aluminium, then decrease to argon, with a bump in sulfur.
- Melting Point: Melting points generally increase going from sodium to silicon, then decrease going to argon, with a bump in sulphur.
- The metals/nonmetals, and/or metalloids in the element family and/or period: Elements to the left of Period 3 show metallic properties, elements to the right show non-metallic properties. Silicon is a semi-metal aka metalloid.
- Na, Mg, and Cl react with water while Al, Si, P, S, and Ar do not