Explain the difference in acidity of MgO dissolved in water and of P4O10 in water in terms of position of the element in the periodic table and bonding.
I found MgO is basic and P4O10 is acidic
The difference in acidity between MgO and P4O10 in water can be explained in terms of their positions in the periodic table and the nature of their chemical bonding.
MgO is a metal oxide, where magnesium (Mg) belongs to Group 2 (or alkaline earth metals) and oxygen (O) belongs to Group 16 (or chalcogens) of the periodic table. In this case, MgO is considered a basic oxide. Group 2 metals are known to form basic oxides because they have a tendency to donate their two valence electrons to oxygen, resulting in the formation of an ionic compound. In the case of MgO, magnesium donates its two electrons to oxygen, forming Mg2+ cations and O2- anions. When MgO is dissolved in water, it forms hydroxide ions (OH-) by reacting with water molecules. The presence of hydroxide ions gives a basic pH to the solution, making MgO basic.
On the other hand, P4O10 is a nonmetal oxide. Phosphorus (P) belongs to Group 15 (or pnictogens) in the periodic table. P4O10 is considered an acidic oxide. Unlike Group 2 metals, Group 15 nonmetals do not readily donate electrons. Instead, they have a greater tendency to accept electrons to achieve a stable electron configuration. In the case of P4O10, phosphorus accepts oxygen atoms to form a compound with a covalent framework. This compound is known as diphosphorus pentoxide. When P4O10 is dissolved in water, it reacts with water molecules to form phosphoric acid (H3PO4), which dissociates into H+ ions, giving an acidic pH to the solution.
To summarize, the difference in acidity between MgO and P4O10 can be attributed to their positions in the periodic table and the type of bonding they exhibit. MgO, being a basic oxide, forms hydroxide ions when dissolved in water, resulting in a basic pH. P4O10, being an acidic oxide, forms phosphoric acid when reacted with water, leading to the formation of H+ ions and an acidic pH.
To understand the difference in acidity of MgO and P4O10, we need to consider the position of the elements in the periodic table and the nature of their bonding.
MgO is the chemical formula for magnesium oxide, which consists of one magnesium (Mg) atom and one oxygen (O) atom. Magnesium is located in Group 2, also known as the alkaline earth metals, while oxygen is in Group 16, the chalcogens. Magnesium has two valence electrons, while oxygen has six.
When MgO dissolves in water, it undergoes hydrolysis, where water molecules react with the ions formed in the solution. In this case, magnesium oxide reacts with water to produce magnesium hydroxide (Mg(OH)2) ions. This reaction occurs because magnesium is an alkaline earth metal, which tends to form basic solutions by releasing hydroxide ions (OH-) into the water. The basic nature of MgO arises from the ability of magnesium to readily donate its valence electrons.
On the other hand, P4O10 is the chemical formula for tetraphosphorus decaoxide. It consists of four phosphorus (P) atoms and ten oxygen (O) atoms. Phosphorus is located in Group 15, the pnictogens, while oxygen is in Group 16, as mentioned earlier. Phosphorus has five valence electrons.
When P4O10 dissolves in water, it reacts with water to form phosphoric acid (H3PO4). This reaction occurs because phosphorus pentoxide is a highly acidic oxide. Phosphorus pentoxide is an acidic oxide because it easily accepts water molecules, releasing hydrogen ions (H+) into the solution. This acidity arises from the ability of phosphorus to attract electrons due to its higher electronegativity compared to oxygen.
In summary, the difference in acidity between MgO and P4O10 can be explained by their positions in the periodic table and the nature of their bonding. MgO is basic because of the alkaline earth metal characteristics of magnesium, while P4O10 is acidic due to the ability of phosphorus to form highly acidic oxides.