What is the primary reason for the increase in melting point as you move from so

What is the primary reason for the increase in melting point as you move from sodium to aluminum in the periodic table?

What is the primary reason for the increase in melting point as you move from sodium to aluminum in the periodic table?

Step 1: Understand that elements in the periodic table are arranged by their atomic number.
Step 2: Recognize that sodium (Na) is a metal and is located in Group 1 of the periodic table.
Step 3: Identify that aluminum (Al) is also a metal but is located in Group 13 of the periodic table.
Step 4: Learn that metals have a structure where atoms are surrounded by a 'sea' of delocalized electrons.
Step 5: Note that as you move from sodium to aluminum, the number of delocalized electrons increases.
Step 6: Understand that more delocalized electrons lead to stronger metallic bonds between the metal atoms.
Step 7: Realize that stronger metallic bonds require more energy to break, resulting in a higher melting point.

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