Chapter 6: Problem 49
What type of energy sublevel is being filled by the transition elements?
Short Answer
Expert verified
The energy sublevel being filled by transition elements is the d sublevel.
Step by step solution
01
Understand the Periodic Table and Electron Configuration
The periodic table is divided into blocks, each representing a different type of atomic orbital that is being filled with electrons. These blocks are named after the electron sublevels: s, p, d, and f. The location of an element in the periodic table helps determine the type of sublevel that is being filled.
02
Locate Transition Elements in the Periodic Table
Transition elements are found in the d-block of the periodic table, which includes Groups 3 to 12. These elements are situated between the s-block elements on the left and the p-block elements on the right.
03
Determine the Sublevel Being Filled
For transition elements, the defining characteristic is the filling of the d sublevel. As we progress through the transition elements, electrons are added to the d orbitals of the penultimate energy level, making the d orbitals partially filled.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Transition Elements
Transition elements are fascinating components of the periodic table, known for their unique properties and widespread applications. They are metal elements that exist between Groups 3 and 12, and this particular positioning lends them certain distinct characteristics. These elements are often seen in a variety of different oxidation states, which means they can form multiple types of ions.
A key feature of transition elements is their partially filled d orbitals. This results in complex chemistry and the ability to form colorful compounds, often used in pigments and dyes. Furthermore, transition metals exhibit good conductivity of heat and electricity, and they are known for being strong and resilient, making them essential in construction materials.
- Widely used in industrial applications
- Known for forming complex compounds
- Exhibit multiple oxidation states
These attributes make transition elements integral to compounds used in catalysis, manufacturing, and even biological systems—like how iron plays a crucial role in oxygen transport in hemoglobin.
A key feature of transition elements is their partially filled d orbitals. This results in complex chemistry and the ability to form colorful compounds, often used in pigments and dyes. Furthermore, transition metals exhibit good conductivity of heat and electricity, and they are known for being strong and resilient, making them essential in construction materials.
- Widely used in industrial applications
- Known for forming complex compounds
- Exhibit multiple oxidation states
These attributes make transition elements integral to compounds used in catalysis, manufacturing, and even biological systems—like how iron plays a crucial role in oxygen transport in hemoglobin.
Periodic Table Blocks
The periodic table is an ingenious arrangement of elements that organizes them according to increasing atomic number and recurring chemical properties. Within this table, the elements are divided into blocks corresponding to electron sublevels: s-block, p-block, d-block, and f-block. Understanding these blocks is essential for grasping the concept of electron configuration.
- **s-block**: Located on the left side, this block contains elements with electrons filling an s sublevel. These include alkali metals and alkaline earth metals.
- **p-block**: Found on the right side, elements here have their last electron entering a p orbital. It contains a diverse group of elements including nonmetals, metalloids, and metals.
- **d-block**: Also known as the transition metals block, it lies at the center and involves the filling of d orbitals.
- **f-block**: Composed of the lanthanides and actinides, positioned at the bottom, and involves the filling of f orbitals.
This block organization aids in understanding the chemical behavior of elements, explains why they participate in certain types of bonding, and restricts their reactivity with other elements.
- **s-block**: Located on the left side, this block contains elements with electrons filling an s sublevel. These include alkali metals and alkaline earth metals.
- **p-block**: Found on the right side, elements here have their last electron entering a p orbital. It contains a diverse group of elements including nonmetals, metalloids, and metals.
- **d-block**: Also known as the transition metals block, it lies at the center and involves the filling of d orbitals.
- **f-block**: Composed of the lanthanides and actinides, positioned at the bottom, and involves the filling of f orbitals.
This block organization aids in understanding the chemical behavior of elements, explains why they participate in certain types of bonding, and restricts their reactivity with other elements.
D-Block Elements
D-block elements form the core region of the periodic table and are synonymous with transition metals. They represent elements where d-orbital electrons are being filled, which directly influences their chemical and physical properties.
Typically, when we move across the d-block in the periodic table, we see a gradual filling of the 3d to 6d orbitals. These elements can hold up to ten electrons in their d sublevel, yet it is the partial occupancy of these electrons that imparts characteristic properties such as variable oxidation states and color.
- **Variable oxidation states**: This arises because d and s electrons can participate in forming bonds.
- **Complex formation**: D-block elements can form complex ions that have extensive applications, especially in coordination chemistry.
- **Catalytic properties**: Many of these metals act as catalysts due to their ability to change oxidation states and form bonds with a variety of substances.
These features make d-block elements highly versatile and valuable in both chemical reactions and industrial applications.
Typically, when we move across the d-block in the periodic table, we see a gradual filling of the 3d to 6d orbitals. These elements can hold up to ten electrons in their d sublevel, yet it is the partial occupancy of these electrons that imparts characteristic properties such as variable oxidation states and color.
- **Variable oxidation states**: This arises because d and s electrons can participate in forming bonds.
- **Complex formation**: D-block elements can form complex ions that have extensive applications, especially in coordination chemistry.
- **Catalytic properties**: Many of these metals act as catalysts due to their ability to change oxidation states and form bonds with a variety of substances.
These features make d-block elements highly versatile and valuable in both chemical reactions and industrial applications.
