Chapter 6: Problem 22
Identify the group number corresponding to each of the following families of elements: (a) boron group (b) oxygen group (c) nickel group (d) copper group
Short Answer
Expert verified
Boron Group - 13; Oxygen Group - 16; Nickel Group - 10; Copper Group - 11.
Step by step solution
01
Understand the Periodic Table
The Periodic Table is organized into groups and periods. Groups are the vertical columns, numbered from 1 to 18. Elements in the same group share similar chemical properties.
02
Identify the Boron Group
The boron group consists of elements in Group 13 of the Periodic Table. This group includes Boron (B), Aluminum (Al), Gallium (Ga), Indium (In), and Thallium (Tl).
03
Identify the Oxygen Group
The oxygen group is in Group 16, known as the chalcogens. This group includes Oxygen (O), Sulfur (S), Selenium (Se), Tellurium (Te), and Polonium (Po).
04
Identify the Nickel Group
The nickel group is part of the transition metals, located in Group 10. This includes Nickel (Ni), Palladium (Pd), and Platinum (Pt).
05
Identify the Copper Group
The copper group is found in Group 11, often called coinage metals. This group comprises Copper (Cu), Silver (Ag), and Gold (Au).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Boron Group
The Boron Group, also known as Group 13 of the Periodic Table, is home to a fascinating collection of elements that play crucial roles in various applications. This group includes Boron (B), Aluminum (Al), Gallium (Ga), Indium (In), and Thallium (Tl). One of the key characteristics of Group 13 elements is that they have three electrons in their outermost shell, which influences their chemical reactivity and bonding characteristics.
These elements often display a tendency to form +3 oxidation states, though Boron, being unique, usually does not form simple ionic compounds. Boron itself is a metalloid, displaying properties intermediate between metals and non-metals, which contributes to its versatility in forming complex structures, such as borosilicates used in glass manufacturing.
Aluminum is perhaps the most well-known member of this group, famous for its lightweight and resistance to corrosion. Despite being the third most abundant element in Earth's crust, Aluminum never occurs naturally in its pure metal form, due to its high reactivity. The other elements in the group, such as Gallium, Indium, and Thallium, are less abundant but find applications in electronic devices and alloys.
These elements often display a tendency to form +3 oxidation states, though Boron, being unique, usually does not form simple ionic compounds. Boron itself is a metalloid, displaying properties intermediate between metals and non-metals, which contributes to its versatility in forming complex structures, such as borosilicates used in glass manufacturing.
Aluminum is perhaps the most well-known member of this group, famous for its lightweight and resistance to corrosion. Despite being the third most abundant element in Earth's crust, Aluminum never occurs naturally in its pure metal form, due to its high reactivity. The other elements in the group, such as Gallium, Indium, and Thallium, are less abundant but find applications in electronic devices and alloys.
Oxygen Group
The Oxygen Group, positioned in Group 16 of the Periodic Table, is commonly referred to as the chalcogens. These elements include Oxygen (O), Sulfur (S), Selenium (Se), Tellurium (Te), and Polonium (Po). The chalcogens are pivotal in both biological systems and industrial processes.
Oxygen, a vital component of air, is essential for respiration and combustion. It is highly reactive and forms oxides with almost all elements. Sulfur, another member of this group, is well-known for its role in vulcanizing rubber and as a component in fertilizers.
In terms of electronic configuration, chalcogens all have six electrons in their outer shells, which leads to their common oxidation state of -2. This capability allows them to form a variety of chemical compounds, such as H₂O, SO₄²⁻, and PO₄³⁻. The heavier elements in the group, like Selenium and Tellurium, are critical in semiconductor technology, while Polonium is radioactive and used in certain specialized applications.
Oxygen, a vital component of air, is essential for respiration and combustion. It is highly reactive and forms oxides with almost all elements. Sulfur, another member of this group, is well-known for its role in vulcanizing rubber and as a component in fertilizers.
In terms of electronic configuration, chalcogens all have six electrons in their outer shells, which leads to their common oxidation state of -2. This capability allows them to form a variety of chemical compounds, such as H₂O, SO₄²⁻, and PO₄³⁻. The heavier elements in the group, like Selenium and Tellurium, are critical in semiconductor technology, while Polonium is radioactive and used in certain specialized applications.
Transition Metals
Transition metals, found in the central block of the Periodic Table (Groups 3-12), include elements such as Iron, Copper, and Nickel. These metals are characterized by their ability to form positively charged ions with different oxidation states. This flexibility results from the presence of partially filled d-orbitals, which are energetically close to the s and p orbitals involved in bonding.
The transition metals are renowned for their distinct properties, such as high melting points and electrical conductivity. They also have the ability to form colored compounds, which is why they are often used in pigments and dyes. Industrially, these metals are indispensable; for example, Iron is the backbone of steel, while Copper is integral in electrical wiring due to its excellent conductivity.
Furthermore, transition metals are often catalysts in chemical reactions. Their ability to lend and take electrons easily facilitates many industrial and biological chemical processes, making them critical for manufacturing and biochemistry.
The transition metals are renowned for their distinct properties, such as high melting points and electrical conductivity. They also have the ability to form colored compounds, which is why they are often used in pigments and dyes. Industrially, these metals are indispensable; for example, Iron is the backbone of steel, while Copper is integral in electrical wiring due to its excellent conductivity.
Furthermore, transition metals are often catalysts in chemical reactions. Their ability to lend and take electrons easily facilitates many industrial and biological chemical processes, making them critical for manufacturing and biochemistry.
Coinage Metals
The Coinage Metals comprise the Group 11 elements, which include Copper (Cu), Silver (Ag), and Gold (Au). Historically, these metals have been utilized to mint coins due to their resistance to corrosion and ease of workability. Their name originates from this historical use.
These metals are notable for their excellent thermal and electrical conductivity. Copper is extensively used in electrical wiring and electronics. Silver, with its superior conductivity, is used in high-frequency equipment and soldering.
Gold, prized for its malleability and resistance to tarnish, finds applications in jewelry, electronics, and as a standard for monetary systems. Unlike metals in other groups, coinage metals typically occur in nature in metallic forms due to their low reactivity, which is why they remain shiny and untarnished over time.
Their chemical reactivity is uniquely low among metals, leading to a tendency to form a +1 oxidation state. This property enhances their stability and resistance to corrosion, making them valuable for various industrial applications.
These metals are notable for their excellent thermal and electrical conductivity. Copper is extensively used in electrical wiring and electronics. Silver, with its superior conductivity, is used in high-frequency equipment and soldering.
Gold, prized for its malleability and resistance to tarnish, finds applications in jewelry, electronics, and as a standard for monetary systems. Unlike metals in other groups, coinage metals typically occur in nature in metallic forms due to their low reactivity, which is why they remain shiny and untarnished over time.
Their chemical reactivity is uniquely low among metals, leading to a tendency to form a +1 oxidation state. This property enhances their stability and resistance to corrosion, making them valuable for various industrial applications.
