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Chapter 5: Problem 16

Explain why there are 14 members of each \(f\) block series.

Short Answer

Expert verified
There are 14 members in each f-block series because the f-orbitals can accommodate 14 electrons.

Step by step solution

01

Introduction to the f-block

The f-block of the periodic table consists of two series: the lanthanides and the actinides. These elements are also known as inner transition metals. The f-block is located at the bottom of the periodic table, separated from the main table.
02

Understanding f-orbitals

The f-block elements have partially filled f-orbitals. An f-orbital can hold a maximum of 14 electrons, since it consists of seven orbital orientations, each capable of holding two electrons (one with spin-up and one with spin-down).
03

Electron Configuration

For the lanthanides and actinides, their electron configurations start to fill the 4f and 5f orbitals, respectively. Since there are 7 f-orbitals, each orbital can accommodate 2 electrons, making a total of 7 x 2 = 14 electrons.
04

Counting Elements in f-block Series

Due to the capacity of the f-orbitals (14 electrons), each f-block series, lanthanides and actinides, consists of 14 elements. Elements in these series add electrons to the f-orbital until it is filled.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

f-orbitals
The f-orbitals are a type of atomic orbital found in the f-block of the periodic table. They are characterized by having a complex shape and are less commonly discussed than s, p, and d orbitals because they only appear after the fourth energy level in atoms. Here's a breakdown of their most important points:
  • f-orbitals can hold a maximum of 14 electrons.
  • They have seven orbitals, meaning each can carry two electrons with opposite spins.
  • The orientation of f-orbitals is unique and they come into play primarily in the lanthanides and actinides.
Understanding their structure is crucial because they are responsible for the properties of f-block elements, like their magnetic and chemical behaviors.
lanthanides
The lanthanides are a series of 14 elements, from lanthanum (La) to lutetium (Lu), placed in the f-block of the periodic table. They are known for having partially filled 4f-orbitals. Key Characteristics:
  • They typically have similar properties, which is why they are often difficult to separate.
  • Their electrons fill the 4f subshell, making them part of the first of the f-block series.
  • Lanthanides are known for their high reactivity, especially with water and air.
  • They exhibit a phenomenon known as "lanthanide contraction," which influences their atomic and ionic sizes.
These elements find uses in things like catalysts, magnets, and phosphors due to their unique electronic configuration.
actinides
Actinides are the second series of 14 elements in the f-block, beginning with actinium (Ac) and ending with lawrencium (Lr). Their unique feature is having partially filled 5f-orbitals. Notable Features:
  • Most actinides are radioactive, with uranium and thorium being the most prominent due to their uses in nuclear reactors and dating techniques.
  • Actinides have complex electron setups, often forming ions with a variety of oxidation states.
  • They are generally not found naturally, except for a few like thorium and uranium.
  • These elements contribute significantly to nuclear energy and research fields due to their radioactivity.
Understanding actinides is key to exploring nuclear chemistry and synthetic element properties.

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Most popular questions from this chapter

How would the ground state electron configurations of the elements in the second row of the periodic table differ if the \(2 s\) and \(2 p\) orbitals had the same energy, as they do for a hydrogen atom?

Indicate which of the following electron configurations are ruled out by the Pauli exclusion principle: (a) \(1 s^{2} 2 s^{2} 2 p^{7}\) (b) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{3}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{12}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\)

What is meant by the term "valence electrons"?

Using the noble-gas shorthand notation, write. the ground state electron configurations for the following elements: (a) Si (b) Ni (c) Se (d) \(\mathrm{Cd}\) (e) \(\mathrm{Mg}\)

Why is the \(m_{s}\) quantum number called the "spin" quantum number? Does an electron in an atom literally spin?
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