Consider a class of students wherein two kids, apparently not related to each other through bloodlines, share strikingly similar characteristics, which stand as a class apart. The best way to explain the diagonal relationship is by using this analogy between beryllium and aluminium in the periodic table. Although beryllium, marked by the symbol Be, and aluminium, marked by the symbol Al, come from Group 2 and Group 13, respectively, they share some similarities in their chemical properties that are deviations from what would be expected in their respective groups.
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General Concepts and Definitions
The diagonal relationship is the relationship between pairs of elements that are diagonal across each other in the table of elements. It goes from the second period to the third period. This phenomenon could easily be best described by the conduct of beryllium and aluminium, as they are of approximately the same electronegativities and have values for ionization energy that are nearly the same, while the atomic radii are also the same. These two elements combined are in separate groups but possess a very similar chemical behaviour. Beryllium has the atomic number 4 and is one of the light metals, also placing it in Group 2: alkaline earth metals. Due to the balancing ability of elements, while they move diagonally across the periodic table, aluminium bears an atomic number of 13 and appears just below boron in Group 13 of the periodic table.
Several aspects of beryllium and aluminium are the same, such as being amphoteric, the formation of covalent compounds, and resistance to acid attacks. The two elements form an oxide layer on their surface that offers them protection from corrosion. As such, beryllium hydroxide, Be(OH)2, and aluminium hydroxide, Al(OH)2, form amphoteric oxides; thus, they react with both acids and bases. The property is very crucial for various industrial uses of the two elements. Also, beryllium and aluminium combine to form some covalent compounds with certain elements. For instance, beryllium chloride, BeCl2, and aluminium chloride, AlCl2, are formed, which presents yet another piece of evidence of the chemical similarity between these elements.
The ionic radius of Be2+ is estimated to be 31 pm; the charge/radius ratio is nearly the same as that of the Al3+ ion. Hence beryllium resembles aluminium in some ways. Some of the similarities are:
Some of the important implications of the diagonal relationship between beryllium and aluminium in theory and applications are that it helps students and researchers in academics identify and explain the diverse properties of these and other elements.
Some Solved Examples
Example 1
Question: Be and Al show a diagonal relationship, hence both have:
Solution:
The oxides of both Be and Al are amphoteric in nature. The polarising power of Be2+ and Al3+ ions is high. Consequently, the compounds develop a covalent nature. The electronegativity values of both elements are the same.
Hence, the answer is option (4) - All the above.
Example 2
Question:
Be and Al exhibits many properties which are similar. But the two elements differ in:
Solution:
Be shows a maximum covalency of four while Al shows a maximum covalency of six.
Hence, the answer is option (3) - Exhibiting maximum covalency in compounds.
Example 3
Question:
Beryllium shows a diagonal relationship with:
Solution:
Be shows a diagonal relationship with Al.
Hence, the answer is option (2) - Al.
Conclusion
The diagonal relationship between beryllium and aluminium has this exciting interplay with periodic trends that casts them into almost similar chemical properties despite being placed in different groups. How these elements can warrant such similarities through an analysis of their definitions, key properties, and examples drawn from applications in real-life scenarios will be discussed. This will not only enrich our knowledge of chemistry but also have practical implications for various industries. This periodic system is so great that, through diagonal relationships, it offers definite further study and probing of chemistry. Therefore, all rules of the periodic table are mutual and supported by other rules.
The diagonal relationship will hold for those elements that are diagonally placed in the periodic table because they will exhibit similar properties between the second and third periods. For example, beryllium will have some similar chemical properties to aluminium. They both have close values of electronegativity, ionization energy, and atomic radius.
The reason why beryllium and aluminium behave almost alike results from a balance between an enhanced nuclear charge traversed across the period and that of atomic size by going down each group. The same sets of electronegativities and ionization energies are thereby obtained, hence similar chemical behaviour.
Some of the common properties between beryllium and aluminium are their amphoteric nature, the formation of covalent compounds, and their non-corrosive nature due to the formation of a protective oxide layer. Beryllium and aluminium also readily react with acids like base metals and metals (alkalis) with bases. The reason for this is the covalent compound formation of beryllium chloride (BeCl2) and aluminium chloride (AlCl2).
However, the industry exploits this diagonal relationship for its various applications. On account of its high strength-to-weight ratio, beryllium finds its way into aerospace and military uses, while aluminium does so due to its unique properties in construction, packaging, and transport. These members further find applications in chemical processes via corrosion resistance and covalent compounds.
The study of the diagonal relationship is very important since it helps in understanding and predicting properties for elements moving forward and across a periodic table. This allows for advanced qualitative and separation techniques and fully appreciating periodic trends through an enriched study of chemistry.
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