Question

Name an element of Group 6 A. What does the group designation tell you about the electron configuration of the element?

Short answer

Oxygen is in Group 6A, which means it has 6 valence electrons.

Step-by-step solution

Understanding Group 6A

Group 6A of the periodic table is also known as the oxygen group or chalcogens. The group includes elements like oxygen, sulfur, selenium, tellurium, and polonium. Each of these elements shares similar chemical properties.

Selecting an Element

Choose one element from Group 6A. A common choice is oxygen, which is the first element in this group. It is a well-known element and serves as a good example to understand the properties of Group 6A.

Group Designation and Electron Configuration

Group 6A indicates that elements in this group have six electrons in their outermost shell, specifically in the p subshell. This is because Group A designations correspond to the number of valence electrons in the element excluding the transition metals. For example, oxygen has an electron configuration of \([He] 2s^2 2p^4\), showing six valence electrons.

Key concepts

Group 6A elements

The Group 6A elements in the periodic table are also known as the oxygen group or chalcogens.
This group includes the elements oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po).
These elements are known for having similar chemical properties.

• Oxygen (O): Most abundant element in Earth's crust. Vital for respiration processes in living organisms.
• Sulfur (S): Found in various forms, important for life and in industrial processes.
• Selenium (Se): Rare element, but essential in small amounts for human health.
• Tellurium (Te): Used in the electronics industry and in the production of solar panels.
• Polonium (Po): A highly radioactive element with specialized applications in science and industry.

Group 6A elements are found in the p-block of the periodic table and tend to have distinct nonmetallic characteristics. This group is highly reactive, especially with hydrogen to form hydrides, and with metals to form compounds like oxides and sulfides.

Oxygen group

The group referred to as the oxygen group showcases how similar chemical properties arise from electron configurations.
These elements typically exhibit a variety of oxidation states and play crucial roles in biological and environmental processes. Key characteristics of the oxygen group include:

• Oxidation states: These elements can manifest in multiple oxidation states, making them versatile in chemical reactions.
• Reactivity: They readily form compounds with a wide range of elements and are especially reactive with hydrogen and metals.
• Biological importance: Oxygen and sulfur are essential for cellular respiration and synthesis of amino acids, respectively.

The oxygen group elements are essential not only in industrial applications but also in vital biological processes. They help sustain life and facilitate numerous chemical reactions necessary for natural and artificial transformations.

Electron configuration

Understanding the electron configuration provides insight into the chemical behavior of the Group 6A elements. In the periodic table, electron configuration helps predict how an element will interact in chemical reactions based on its number of valence electrons.Elements in Group 6A have six electrons in their outermost shell, particularly filling the p subshell.
This results from the A-group designation which approximates the count of valence electrons excluding transition metals. Example of Electron Configuration:

• Oxygen: \( [He] 2s^2 2p^4 \). This reveals it has a total of six valence electrons.
• Sulfur: \( [Ne] 3s^2 3p^4 \). Like oxygen, it also has six valence electrons.

The electron configuration mainly dictates an element's place on the periodic table, and it is crucial for predicting the chemical bonding behavior and reactivity of the elements.