Question

Which corresponds to the most electropositive character? (a) \([\mathrm{Xe}] 6 \mathrm{~s}^{1}\) (b) \([\mathrm{Xe}] 6 \mathrm{~s}^{2}\) (c) \([\mathrm{He}] 2 \mathrm{~s}^{1}\) (d) \([\mathrm{He}] 2 \mathrm{~s}^{1}\)

Short answer

The most electropositive element is francium, so option (a) \\([ ext{Xe}] 6  ext{s}^1\\) corresponds to the most electropositive character.

Step-by-step solution

Understand Electronegativity vs. Electropositivity

Electropositivity refers to the tendency of an atom to donate electrons and form positive ions, and is typically exhibited by elements on the left side of the periodic table, particularly metals. Electronegativity, conversely, is the tendency to attract electrons.

Identify Element Configurations

Review the given electronic configurations: - Option (a), \([ ext{Xe}] 6  ext{s}^1\): Corresponds to francium (Fr)- Option (b), \([ ext{Xe}] 6  ext{s}^2\): Corresponds to radium (Ra)- Option (c) and (d), \([ ext{He}] 2  ext{s}^1\): Both correspond to lithium (Li).

Analyze Electropositive Character by Position

Francium (Fr) and radium (Ra) belong to the alkali and alkaline earth metals, known for their electropositive nature. However, among them, the alkali metals show greater electropositivity compared to alkaline earth metals, and as elements proceed down a group in the periodic table, they typically become more electropositive. This makes francium, the heaviest alkali metal, highly electropositive.

Compare to Determine the Most Electropositive

Li (Lithium) while electropositive, is less so compared to the heavier alkali and alkaline earth metals. Francium stands out as the most electropositive due to its position as the heaviest alkali metal, even more so than radium.

Key concepts

Periodic Table

The Periodic Table is an organized chart of chemical elements. Each element is arranged based on its atomic number, electron configuration, and recurring chemical properties. This systematic arrangement helps predict how elements behave and interact with each other.

• Elements in the same column, known as groups or families, possess similar chemical behaviors.
• The rows, called periods, highlight the filling of electrons in various electron shells.

Aside from its fluent organization, the Periodic Table reveals trends such as electronegativity and electropositivity. Electropositive elements, often metals, generally reside on the left side, exhibiting a tendency to lose electrons. This table is essential for identifying elemental characteristics and foreseeing chemical reactions.

Alkali Metals

Alkali metals make up Group 1 of the Periodic Table. These elements include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). They have a single electron in their outer shell, which they easily lose to form a stable electron configuration.

• These metals are soft and highly reactive, especially with water.
• As you move down the group, their reactivity and electropositive character increase.

Francium is known as the most electropositive of all alkali metals, highlighting its tendency to donate its outer electron. This characteristic makes francium extremely reactive, though it is rarely encountered in chemical studies due to its radioactivity and scarcity.

Alkaline Earth Metals

Occupying Group 2 of the Periodic Table, the alkaline earth metals consist of beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). These elements have two electrons in their outer shell.

• They are less reactive than the alkali metals but are still more electropositive than non-metals.
• These metals are typically found in compounds rather than in pure form due to their reactivity.

As we descend within this group, the electropositive character and reactivity generally increase, due to the decreased attraction between the nucleus and the outer electrons. Radium, being the heaviest and last in the alkaline earth metals, manifests more electropositive character compared to lighter elements in the group.