Order the following atoms according to increasing atomic radius: S, F, O.

Verified step by step guidance

1. Identify the periodic trend for atomic radius: Atomic radius generally increases as you move down a group and decreases as you move across a period from left to right.
2. Locate the elements on the periodic table: Sulfur (S), Fluorine (F), and Oxygen (O) are all in the same period (Period 2).
3. Compare the positions of the elements: In Period 2, the order from left to right is O, F, S.
4. Apply the periodic trend: Since atomic radius decreases from left to right across a period, the order of increasing atomic radius is F, O, S.
5. Conclude the order: Therefore, the order of increasing atomic radius is F < O < S.

Key Concepts

Atomic Radius

Atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electron shell. It can vary based on the atom's position in the periodic table, influenced by factors such as nuclear charge and electron shielding. Generally, atomic radius increases down a group and decreases across a period.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. For atomic radius, as you move from left to right across a period, the radius decreases due to increased nuclear charge attracting electrons more strongly. Conversely, as you move down a group, the radius increases due to the addition of electron shells.

Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. It is closely related to atomic radius; smaller atoms with higher electronegativity tend to have a stronger pull on electrons. In the context of the question, understanding electronegativity helps explain why fluorine, being the most electronegative and smallest atom among S, F, and O, has the smallest atomic radius.