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Gajan1234
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Why is it easier to remove an electron from p orbital than s orbital. I thought P orbital have higher energy so more energy is require to remove a electron from P orbital.
Gajan1234 said:Why is it easier to remove an electron from p orbital than s orbital. I thought P orbital have higher energy so more energy is require to remove a electron from P orbital.
Electron arrangement refers to the specific distribution of electrons in an atom's energy levels or orbitals. It determines the atom's chemical and physical properties and is responsible for the formation of chemical bonds.
Ionisation energy is the minimum amount of energy required to remove an electron from an atom. The electron arrangement of an atom determines its ionisation energy, as it reflects the stability of the atom and the strength of its attraction to its electrons.
The electron arrangement of an atom is influenced by the number of electrons, the number of energy levels, and the electron shielding effect from inner levels. Additionally, the type of element and its position on the periodic table can also affect electron arrangement.
Ionisation energy generally increases across a period on the periodic table. This is because as you move from left to right, the number of protons and electrons increases, leading to a stronger attraction between the nucleus and the outermost electrons. As a result, more energy is required to remove an electron.
Ionisation energy decreases down a group on the periodic table because the outermost electrons are further away from the nucleus due to the addition of more energy levels. This leads to a weaker attraction between the nucleus and the outermost electrons, making it easier to remove an electron and resulting in a lower ionisation energy.