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Ch.7 - Periodic Properties of the Elements
Chapter 7, Problem 25c

Using only the periodic table, arrange each set of atoms in order from largest to smallest: (c) F, O, N.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Atomic Radius

The atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electron shell. Atomic radius generally decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus. Conversely, it increases down a group as additional electron shells are added, resulting in larger atomic sizes.
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Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Key trends include atomic radius, ionization energy, and electronegativity. Understanding these trends helps in predicting the behavior of elements, such as their size, reactivity, and bonding characteristics.
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Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. While it primarily influences bonding behavior, it is also related to atomic size; smaller atoms with higher electronegativity tend to have stronger attractions for electrons. This concept is important for understanding how elements interact and form compounds.
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