What is the acid base behavior of element oxides? Information and examples about acid base behavior of some common oxides

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Acid Base Behavior Of Element Oxides; Metals are also distinguished from nonmetals by the acid-base behavior of their oxides in water:
• Most main-group metals transfer electrons to oxygen, so their oxides are ionic. In water, these oxides act as bases, producing OH– ions and reacting with acids. Calcium oxide is an example.
• Nonmetals share electrons with oxygen, so non-metal oxides are covalent. In water, they act as acids, producing H+ ions and reacting with bases. Tetraphosphorus decaoxide is an example.
Figure on the right classifies the acid-base behavior of some common oxides, focusing once again on the elements in Group 5A, dinitrogen pentaoxide, N2O5, forms nitric acid:
Tetraphosphorus decaoxide, P4O10, forms the weaker acid H3PO4:

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The oxide of the metalloid arsenic is weakly acidic, whereas that of the metalloid antimony is weakly basic. Bismuth, the most metallic of the group, forms a basic oxide that is insoluble in water but that forms a salt and water with acid:
Note that as the elements become less metallic across a period, their oxides become more acidic. In Period 3, sodium and magnesium form the strongly basic oxides Na2O and MgO.
Some metals and many metalloids form oxides that are amphoteric: they can act as acids or as bases in water. Metallic aluminum forms amphoteric aluminum oxide (Al2O3), which reacts with acid or with base:
Silicon dioxide is weakly acidic, forming a salt and water with base:
The common oxides of phosphorus, sulfur, and chlorine form acids of increasing strength: H3PO4, H2SO4, and HClO4.
So the metallic properties decreases from left to right across a period, and increases from top to bottom within a group Most of the periodic properties of elements are summarized in below.
Comparison of Periodic Properties in Periodic Table
1 | Within period from left to right | 1 | Down a group from top to bottom |
1. | Atomic number increases. | 1. | Atomic number increases. |
2. | Mass number increases. | 2. | Mass number increases. |
3. | Atomic volume decreases. | 3. | Atomic volume increases. |
4. | lonazation energy increases. | 4. | lonazation energy decreases. |
5. | Electron affinity increases. | 5. | Electron affinity decreases. |
6. | Electron losing tendency decreases. | 6. | Electron losing tendency increases. |
7. | Metallic character decreases. | 7. | Metallic character increases. |
8. | Nonmetallic character increases. | 8. | Nonmetallic character decreases. |
9. | Acidic character of oxides increases. | 9. | Acidic character of oxides decreases. |
10. | Number of valence electrons increases. | 10. | Number of valence electrons does not change. |