Arrange these elements in order of increasing metallic character: Fr, Sb, In, S, Ba, Se.

Verified step by step guidance

1. Step 1: Understand that the metallic character of an element refers to its ability to lose electrons and form positive ions. It increases down a group and decreases across a period from left to right on the periodic table.
2. Step 2: Locate each of the elements on the periodic table. The elements are Francium (Fr), Antimony (Sb), Indium (In), Sulfur (S), Barium (Ba), and Selenium (Se).
3. Step 3: Compare the positions of these elements on the periodic table. Elements on the left and lower part of the periodic table have higher metallic character than those on the right and upper part.
4. Step 4: Based on their positions, arrange the elements in order of increasing metallic character. Start with the element that is furthest to the right and highest up on the periodic table, and end with the element that is furthest to the left and lowest down.
5. Step 5: The final order should be: S (furthest right and highest up), then Se, then Sb, then In, then Ba, and finally Fr (furthest left and lowest down). This is the order of increasing metallic character.

Key Concepts

Metallic Character

Metallic character refers to the set of properties associated with metals, including conductivity, malleability, ductility, and luster. It increases down a group in the periodic table and decreases across a period from left to right. Understanding this trend is essential for predicting the behavior of elements in chemical reactions and their physical properties.

Periodic Trends

Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change as you move across a period or down a group. Key trends include atomic radius, ionization energy, electronegativity, and metallic character. Recognizing these trends helps in arranging elements based on their properties, such as increasing metallic character.

Group and Period Classification

Elements in the periodic table are organized into groups (columns) and periods (rows). Groups contain elements with similar chemical properties, while periods indicate the number of electron shells. The position of an element within these classifications influences its metallic character, with elements in lower groups generally exhibiting higher metallic character due to their larger atomic size and lower ionization energies.