Question

Use a reference book or the Internet to look up the average atomic masses and properties of silicon, Si, germanium, Ge, tin, Sn, phosphorus, P, antimony, Sb, sulfur, S, and selenium, Se. a. Organize these elements into rows and columns. b. List two properties that the elements in each column have in common.

Short answer

Group Si, Ge, and Sn in one column due to metallic characteristics; P and Sb due to non-metallic traits; S and Se as chalcogens.

Step-by-step solution

Gather Atomic Masses and Properties

Look up the average atomic masses and notable properties of the elements: silicon (Si), germanium (Ge), tin (Sn), phosphorus (P), antimony (Sb), sulfur (S), and selenium (Se). Make notes about their physical and chemical properties such as state at room temperature, color, metallic or non-metallic character, etc.

Organize Elements into Table

Identify trends and categorize the elements into rows and columns based on similar properties. For example, group silicon, germanium, and tin together as they are metalloid or metallic, whereas group phosphorus and antimony based on their non-metallic properties. Sulfur and selenium can also form another group as they share chalcogen group properties.

Draw the Periodic Connections

Place the elements in a periodic table manner to expose their similarities. This arrangement may look like forming a mini-table from the larger periodic table, with Si, Ge, and Sn possibly in one column or row, P and Sb in another, and S and Se in a third. This alignment should reflect periodic trends like increase in atomic size down a group.

Identify Common Properties

Once organized, identify and list two properties that elements in each column share. For instance, in the column containing Si, Ge, and Sn, you might note they all have metallic luster and conductivity. In the P, Sb column, they might have similar oxidation states. S and Se might share biochemical roles and similar chemical reactivity.

Key concepts

Atomic Mass

The concept of atomic mass is fundamental when studying the periodic table and the elements it includes. Atomic mass, often referred to as atomic weight, is the weighted average mass of the atoms in a naturally occurring element based on the relative abundance of each isotope. This mass is measured in atomic mass units (amu), which makes comparisons across different elements straightforward. For example, when examining elements like silicon (Si), germanium (Ge), tin (Sn), phosphorus (P), antimony (Sb), sulfur (S), and selenium (Se), atomic masses vary accordingly, reflecting their differences in isotopic composition. Silicon, for instance, has an atomic mass of approximately 28.085 amu, whereas tin, a heavier element, carries an atomic mass around 118.71 amu. These differences in atomic mass can be attributed to the varying number of protons and neutrons within the atomic nuclei of different elements. Understanding atomic mass helps in predicting how elements will react with each other. This characteristic plays a crucial role in determining the molar mass of elements and compounds, impacting calculations in chemical reactions.

Element Properties

Every element exhibits unique physical and chemical properties that define its behavior in natural and laboratory conditions. These properties can be categorized into various types, such as physical properties (like color, density, state at room temperature) and chemical properties (such as reactivity and oxidation states). For example, silicon (Si), germanium (Ge), and tin (Sn) are elements known for their metallic luster and conductivity, a property particularly significant in the electronics industry. Phosphorus (P) and antimony (Sb) are non-metals, notable for their use in compounds with distinct oxidation states that have applications in areas ranging from electronics to medicine. Sulfur (S) and selenium (Se), on the other hand, have shared characteristics as chalcogens. They display non-metallic properties and are essential in biological contexts, forming compounds like sulfuric acid or selenium-enriched substances. Recognizing these properties provides insight into the purposes and applications of these elements across various scientific fields.

Metalloids

Metalloids are important elements that display properties of both metals and non-metals, making them unique in the periodic table. This group includes elements like silicon (Si) and germanium (Ge), which are particularly known for their semi-conducting abilities. Metalloids are often found along the zig-zag line on the periodic table, separating metals from non-metals. They typically exhibit a mix of properties:

• Metallic luster
• Intermediate conductivity that increases with temperature
• Ability to gain or lose electrons to form bonds

Silicon is the most well-known metalloid, widely used in the production of silicones and electronics, due to its structural resilience and conductive properties. Germanium also finds application in transistors and diodes, capitalizing on its semi-conducting nature. The versatility of metalloids stems from their ability to bridge the gap between the conductive properties of metals and the insulating properties of non-metals.

Chalcogens

Chalcogens compose group 16 in the periodic table and include elements like sulfur (S) and selenium (Se). These elements are predominantly non-metallic and are essential for various biological and chemical processes. Chalcogens exhibit distinct properties:

• Typically form 2- charge ions in compounds
• Are able to form multiple bonds with other atoms
• Display varied states of matter (solid, gas) in natural forms

Sulfur is notable for its pungent smell in compounds like hydrogen sulfide and its role in vulcanizing rubber, while selenium is essential in trace amounts for proper enzymatic function in organisms. Their role as chalcogens implies their high reactivity, especially with metals, to form sulfides and selenides. By engaging fully in chemical reactions, chalcogens contribute significantly to natural mineral formations and industrial applications.