Alkali metals properties, [PART II].

INTRODUCTION.

The behavior of alkali metals is related to their atomic radius. Because as the atomic radius increases, the interaction between the last electron (layer nS1) and the atomic nucleus decreases which is due to the principle of the electrostatic force. This principle indicates that when a negative particle (-) approaches or moves away from a particle (+) the force of attraction that each one exerts on the other will increase or decrease respectively, that is to say that the electrostatic force will depend on the distance between the particles, in our case this distance would be the atomic radius.

So we can then explain, why the alkali metals react at higher speed as it descends in group 1. This happens because as the atomic radius is higher the last electron will be released more easily. This characteristic implies that its first ionized energy is lower therefore the capacity of the element to oxidize and form its characteristic ion will be greater.

METHODOLOGY.

• Reaction of alkali metals with water and alcohol (generation of hydroxides):
  A porcelain crucible was used where a small amount of distilled water was added, then a small piece of Sodium (Na) was taken, which was dried and introduced into the crucible with water, where it reacted and immediately added to the obtained solution a drop of universal indicator, then the solution was neutralized with HCl. This process was repeated with Potassium (K), then instead of water was used ethanol and the same experiment was carried out.

RESULTS AND DISCUSSION.

When the alkali metals (Na and K) were added to the water, it was observed that a "violent" reaction occurs with small explosions, in addition the level of reaction increased as it decreased in group I, that is, the reaction was more "violent" when potassium K was added to the water. A drop of universal indicator was added to the solution obtained, turning the solution into a purple color, indicating that the solution had a basic pH. This pH level was originated because the alkali metals react with water to produce the corresponding metal hydroxide and gaseous hydrogen as shown in the following reactions:

2Na(s) + 2H2O(l) ----> 2NaOH(ac) + H2 (g) ΔG°= -364KJ/mol.

2K(s) + 2H2O(l) ----> 2KOH(ac) + H2 (g) ΔG°= -405,14KJ/mol.

Figure 1. Indicator added to the solution obtained

The difference between the level of reaction of sodium and potassium can be explained because as it descends in group I the atomic radius of the elements increases and the attraction between the electron of the last layer of valence and the atomic nucleus decreases , So it is easier to liberalize the last electron, as it happens with potassium K which reacts more violently with water than Na sodium. Another important aspect to highlight is the ionization energy of each element, which decreases as it descends in the group, which likewise influences the speed of the reaction.