Chapter 3: Problem 19
Cerium \((Z=58)\) is a member of (1) s-block elements (2) p-block elements (3) d-block elements (4) f-block elements
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f-block elements
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Periodic Table Blocks
The periodic table of elements is organized into blocks based on the electron configuration of atoms. This helps in categorizing the elements according to the type of atomic orbital their valence electrons occupy. Here is a breakdown:
- **s-Block Elements:** These elements have their valence electrons in s orbitals. Examples include alkali metals (such as sodium) and alkaline earth metals (such as calcium).
- **p-Block Elements:** These elements have their valence electrons in p orbitals. Examples include elements like carbon, nitrogen, and oxygen.
- **d-Block Elements:** Their valence electrons fill d orbitals, including transition metals such as iron, copper, and gold.
- **f-Block Elements:** These elements have their valence electrons occupying f orbitals. The f-block elements are usually separated into the Lanthanide and Actinide series.
By understanding where each element falls within these blocks, you can predict its chemical properties and behaviors, which is essential in both chemistry and various applications of these elements.
- **s-Block Elements:** These elements have their valence electrons in s orbitals. Examples include alkali metals (such as sodium) and alkaline earth metals (such as calcium).
- **p-Block Elements:** These elements have their valence electrons in p orbitals. Examples include elements like carbon, nitrogen, and oxygen.
- **d-Block Elements:** Their valence electrons fill d orbitals, including transition metals such as iron, copper, and gold.
- **f-Block Elements:** These elements have their valence electrons occupying f orbitals. The f-block elements are usually separated into the Lanthanide and Actinide series.
By understanding where each element falls within these blocks, you can predict its chemical properties and behaviors, which is essential in both chemistry and various applications of these elements.
Lanthanide Series
The Lanthanide series consists of 15 metallic elements with atomic numbers from 57 to 71. These elements are often referred to as rare earth elements.
- **Physical Properties:** Lanthanides are typically shiny and silvery-white metals. They are generally soft and can be cut with a knife.
- **Chemical Properties:** Lanthanides are highly reactive, especially with water and air. They usually form +3 oxidation states.
- **Applications:** Lanthanides are used in various high-tech applications. For instance, they are critical in the manufacturing of powerful magnets, phosphors for color TV and LED screens, and various catalysts used in the petroleum industry.
Cerium (Ce), with an atomic number of 58, falls into this series. Because it's part of the Lanthanides, its chemical behavior is consistent with the properties mentioned above. Understanding the characteristics of the Lanthanide series as a whole helps in predicting the properties of Cerium.
- **Physical Properties:** Lanthanides are typically shiny and silvery-white metals. They are generally soft and can be cut with a knife.
- **Chemical Properties:** Lanthanides are highly reactive, especially with water and air. They usually form +3 oxidation states.
- **Applications:** Lanthanides are used in various high-tech applications. For instance, they are critical in the manufacturing of powerful magnets, phosphors for color TV and LED screens, and various catalysts used in the petroleum industry.
Cerium (Ce), with an atomic number of 58, falls into this series. Because it's part of the Lanthanides, its chemical behavior is consistent with the properties mentioned above. Understanding the characteristics of the Lanthanide series as a whole helps in predicting the properties of Cerium.
Atomic Orbitals
Atomic orbitals are regions around the nucleus of an atom where electrons are likely to be found. They are fundamental in defining the chemical properties of elements.
- **s Orbitals:** These are spherical in shape and can hold up to 2 electrons. The first two columns of the periodic table correspond to s orbitals.
- **p Orbitals:** These have a dumbbell shape and can hold up to 6 electrons. The p-block includes elements from groups 13 to 18.
- **d Orbitals:** These orbitals are more complex in shape and can hold up to 10 electrons. They are associated with the transition metals in groups 3 to 12.
- **f Orbitals:** These are even more complex and can hold up to 14 electrons. The Lanthanides and Actinides belong to the f-block.
Understanding these orbital types is crucial for grasping the electronic configuration of elements. For example, Cerium's valence electrons occupy the 4f orbital, situating it within the f-block and helping to explain its placement in the Lanthanide series.
- **s Orbitals:** These are spherical in shape and can hold up to 2 electrons. The first two columns of the periodic table correspond to s orbitals.
- **p Orbitals:** These have a dumbbell shape and can hold up to 6 electrons. The p-block includes elements from groups 13 to 18.
- **d Orbitals:** These orbitals are more complex in shape and can hold up to 10 electrons. They are associated with the transition metals in groups 3 to 12.
- **f Orbitals:** These are even more complex and can hold up to 14 electrons. The Lanthanides and Actinides belong to the f-block.
Understanding these orbital types is crucial for grasping the electronic configuration of elements. For example, Cerium's valence electrons occupy the 4f orbital, situating it within the f-block and helping to explain its placement in the Lanthanide series.
