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Chapter 23: Problem 53

Sodium does not naturally occur as a free element. Why?

Short Answer

Expert verified
Sodium is highly reactive due to its single valence electron, causing it to readily form compounds instead of existing as a free element.

Step by step solution

01

Understand Sodium's Reactivity

Sodium (Na) is an alkali metal found in Group 1 of the periodic table. Alkali metals have one electron in their outermost shell, making them highly reactive because they readily lose this electron to attain a stable noble gas configuration.
02

Electronegativity and Reaction Tendency

The low electronegativity of sodium means it easily loses its single valence electron. This makes sodium very reactive, especially with non-metals like oxygen and chlorine.
03

Formation of Compounds

Because of its high reactivity, sodium readily combines with other elements forming compounds such as sodium chloride (NaCl) and sodium oxide (Na2O). When exposed to air, sodium reacts quickly, forming these compounds, preventing it from existing as a free element.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

alkali metals
Alkali metals are found in Group 1 of the periodic table and include elements like lithium, sodium, and potassium. They are known for being highly reactive, primarily due to their single valence electron in the outermost shell. This single electron is easily lost in chemical reactions, allowing alkali metals to quickly form positive ions. Alkali metals are also characterized by their soft texture and low melting points. In nature, they rarely exist as free elements because they readily react with other substances.
electronegativity
Electronegativity refers to an atom's ability to attract and hold onto electrons. Sodium has a low electronegativity value, meaning it does not hold its valence electron tightly. This characteristic makes sodium highly reactive, particularly with non-metals, which have higher electronegativities. When sodium interacts with elements like chlorine or oxygen, it easily loses its valence electron. This loss results in the formation of compounds, because the valence electron moves to the more electronegative atom, bonding the two elements together.
compound formation
Due to its high reactivity, sodium is seldom found as a free element in nature. Instead, it frequently forms compounds such as sodium chloride (NaCl) and sodium oxide (Na2O). When sodium encounters other elements, its tendency is to lose its single valence electron. This forms a positive sodium ion (Na鈦�), which then quickly attracts negative ions such as chloride (Cl鈦�) or oxide ions (O虏鈦�). These ionic bonds lead to the formation of compounds, which are more stable than the free, reactive sodium element.
noble gas configuration
Atoms tend to lose, gain, or share electrons to attain a stable electron configuration similar to noble gases. Sodium, which has one electron in its outermost shell, strives to achieve the electron configuration of neon (Ne), the nearest noble gas. When sodium loses its one valence electron, it reaches a stable, noble gas configuration with a full outer shell. This drive for stability is the primary reason behind sodium's high reactivity. Once it forms a compound by losing its electron, sodium achieves a state that is energetically more favorable and less reactive.

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