The ionization energy increases from left to right in a period due to increase in?
Correct answer: A. Nuclear charge
- A. Nuclear charge
- B. Number of electrons
- C. Atomic number
- D. All of these
Explanation
In general, ionization energy increases across a period and decreases down a group. Across a period, effective nuclear charge increases as electron shielding remain constant. The increased distance weakens the nuclear attraction to the outer-most electron and is easier to remove (requires less energy).
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About Periodic Properties and Trends
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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