Reactivity Lab Report By: Veronica Campoverde Introduction: Elements on the periodic table are organized by increasing atomic number. As atomic numbers increases, so does the number of electrons. Electrons, and specifically valence electrons, are important in determining how an atom interacts with other atoms. The elements in a vertical “group” have similar properties because they have the same number of valence electrons and similar electron configurations. Thus this leads to smoothly varying trends in properties such as ionization energy, electronegativity, ionization energy, and atomic radius as one moves both down the groups and across the periods. Thus, the organization of the periodic table is useful for making predictions about an element based on its position in the table. The reactivity of the elements also follow well-defined …show more content…
Lithium- gives off hydrogen gas Sodium- sound is louder hydrogen gas is produced Potassium-lit on fire Rubidium -blew up Cesium- blew up and glass broke Francium- Will explode Stated and explained why reactivity increases or decreases down a group in terms of shielding because it’s easier to give off because of the higher atomic number. Explained why alkali metals are more reactive than the alkaline earth metals because there easier to give away (give and take). Experiment: several chemical reactions were examined. From the observations a list of 6 elements in their order of activity beginning with the most active element down to the least active element were constructed. Materials: Copper, metal strip Cu Copper sulfate, CuSO4, 0.1 M, 1mL Lead metal strip, Pb Lead nitrate , Pb (No3)2, 0.1 M, 1mL Magnesium, metal strip, Mg Magnesium sulfate, MgSO4, 0.1 M,1mL Silver nitrate, AgNO3,0.1 M, 1 mL Sulfuric acid, H2SO4, 5 M, mL Zinc, metal strip, Zn Zinc sulfate, ZNSO4, 0.1 M, 1mL Beral pipets,