What is the BEST explanation for why ionization energy generally increases left to right across the periodic table?

Electrons are found in different shells as the atomic number increases across a period.

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More electrons are added to atoms as the atomic number increases across a period, increasing the electron-electron repulsions.

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Electron affinity increases as the atomic number increases in a period.

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There are more protons as the atomic number increases in a period, increasing the effective nuclear charge.

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Solution

The correct option is D There are more protons as the atomic number increases in a period, increasing the effective nuclear charge.
The statement of option D correctly explains the reason for increase of IE towards right in a period. As the effective nuclear charge increases the electrons are strongly attracted and hence more energy is needed to remove them, hence IE is higher. Thus answer is option D

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Q. Statement I: Atomic radius generally increases as you move across the periodic table from left to right.
Statement II: The atomic number is increasing from left to right as you move across the periodic table.

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Q. Choose the correct answer:
With reference to the variation of properties in the Periodic Table, which of the following is generally true?
(a) Atomic size increases from left to right across a period.
(b) Ionisation potential increases from left to right across a period.
(c) Electron affinity increases going down a group.
(d) Electronegativity increases going down a group.

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