Question

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$\huge \mathfrak{question}$
⤵⤵

Explain
1. Why the first ionisation energy for Magnesium is more than that of Aluminium.

2. Why the first ionisation energy for Nitrogen is more than that of Oxygen.

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Answer 1

Hey mate ♥️♥️♥️♥️

fristly,

isonisation energy: it is the amount of energy is required to remove an electrons from outermost orbit of gases isolated atom is called isonisation energy..

Q1.this is because in magnesium has one more proton than aluminium in its nucleus to hold on electrons in 3s orbital...

Q2.when we move from left to right the atomic number increase then the nuclear charge also increases then it's becomes half field orbital .nd then due to half field orbital stability increase in 2p shell...

then increased ionisation energy increase

Answer 2

the electronic configuration of Na is (Ne) 3s1 and the that of mg (Ne) 3s2 the configuration of mg is more stable being completely filled that date of energy for the first ionization enthalpy of mg is more than that of Na

2) it is due to the fact that the electronic configuration of nitrogen atom in which 2P orbital is half filled is more stable than that of oxygen therefore ionization enthalpy of nitrogen is more than that of oxygen