QQuestionChemistry
QuestionChemistry
Why does ionization energy generally increase moving from left to right across a row of the periodic table?
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Answer
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Step 1:I'll solve this problem by explaining the underlying atomic structure and electron configuration principles.
Step 2:: Understanding Ionization Energy
Ionization energy is the energy required to remove the most loosely bound electron from a neutral atom in its ground state. The trend of increasing ionization energy across a period is related to several key atomic properties.
Step 3:: Nuclear Charge Effect
Z_{effective} = Z_{nuclear} - \sigma_{shielding}
As you move from left to right across a period: - The number of protons in the nucleus increases - The nuclear charge becomes more positive - Electrons are added to the same principal energy level
Step 4:: Electron Shielding
- Inner electrons partially shield outer electrons from nuclear attraction - However, the shielding effect remains relatively constant across a period - The nuclear charge increases more significantly than shielding
Step 5:: Atomic Radius Decrease
- As nuclear charge increases, electrons are pulled closer to the nucleus - Atomic radius decreases across the period - Electrons become more tightly bound to the nucleus
Step 6:: Electrostatic Attraction
E_{ionization} \propto \frac{Z_{effective}}{r_{atomic}}
The increasing nuclear charge creates stronger electrostatic attraction between the nucleus and outer electrons, making electron removal more difficult.
Final Answer
Ionization energy increases across a period due to increasing nuclear charge, decreasing atomic radius, and stronger electrostatic attraction between the nucleus and outer electrons, which makes removing an electron progressively more energy-intensive.
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