Arrange the atoms in Exercise 86 in order of increasing...

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Key Concepts

Atomic Radius

The atomic radius is the distance from the nucleus of an atom to the outer electron shell. It is inversely related to ionization energy; as the atomic radius increases, the outer electrons are further from the nucleus and less tightly held, thus requiring less energy to remove.

Effective Nuclear Charge

Effective nuclear charge refers to the net positive charge experienced by an electron in an atom after accounting for electron shielding. A higher effective nuclear charge typically increases the ionization energy by pulling electrons closer to the nucleus, making them harder to remove.

Periodic Trends

Periodic trends are patterns in the properties of elements that occur in a systematic manner across periods and down groups in the periodic table. Specifically, first ionization energy generally increases across a period and decreases down a group due to changes in effective nuclear charge and electron shielding.

First Ionization Energy

This is the minimum amount of energy required to remove the outermost electron from a neutral atom in the gaseous state. Understanding first ionization energy is crucial for predicting an element's reactivity and its chemical behavior, particularly in forming ions.

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