Why does ionization energy generally increase moving from left to right across a row of the periodic table?

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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. 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. 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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QuestionChemistry

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Full Solution Locked

Step 1:
I'll solve this problem by explaining the underlying atomic structure and electron configuration principles.

Step 2:
: Understanding Ionization Energy

Step 3:
: Nuclear Charge Effect

Final Answer

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