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Question & Answer
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The first ionization energy is lower than the second due to increased shielding from the first electron removed.
The second ionization energy is significantly higher than the first due to the removal of an electron from a fully filled subshell.
Successive ionization energies are generally constant for all elements regardless of electron configuration.
The first ionization energy is the highest due to the stability of the electron configuration after the first electron is removed.
Understanding the Answer
Let's break down why this is correct
The first electron comes from the outer 3s shell, which is not tightly held. Other options are incorrect because Shielding occurs because inner electrons block the pull of the nucleus; Successive ionization energies change with each electron removed, not stay flat.
Key Concepts
Ionization Potential
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Deep Dive: Ionization Potential
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Definition
Ionization potential is the energy required to remove an electron from an atom's outermost shell. It varies across periods and groups in the Periodic Table, influencing the element's reactivity and ability to form ions. Understanding ionization potential helps in predicting chemical behavior and bonding patterns.
Topic Definition
Ionization potential is the energy required to remove an electron from an atom's outermost shell. It varies across periods and groups in the Periodic Table, influencing the element's reactivity and ability to form ions. Understanding ionization potential helps in predicting chemical behavior and bonding patterns.
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