Question

why there is sharp increase in atomic and ionic radius from boron to aluminum​

Answer 1

Answer:

Reason: As we move from Boron to aluminium ,the atomic size increases ,considerably, therefore attraction of nucleus for the electron decreases and hence electronegativity decreases. ... As a result, force of attraction of the nucleus for the electrons increases and hence the electronegativity increases from Al to Tl.

Explanation:

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Answer 2

There is a sharp increase in atomic and ionic radius from boron to aluminum due to the addition of a new shell as we move downwards in group 13 of the periodic table.

• Boron and aluminum are elements belonging to group 13 in the periodic table.
• The atomic radius is the measurement of an atom's size from the nucleus's core to the outermost electron-bearing shell.
• The distance between the nucleus and electron in an ion's outermost shell is called the ionic radius.
• The electronic structure of the elements are given below:

    1. Boron

    Number of shells = 2

    Atomic number = 5

    Ionic state = Br ³⁺

    Boron belongs to the second period in the periodic table.

    2. Aluminum

    Number of shells = 3

    Atomic number = 13

    Ionic state = Al ³⁺

    Aluminum belongs to the third period in the periodic table.

• Hence, as we move down the period or column in the periodic table there is an increase in atomic and ionic radius due to the addition of a new shell in an atom.