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Chapter 8: Problem 27

Identify the block of the periodic table where each of the following elements is. (a) \(\mathrm{Gd}\) (b) \(\mathrm{Ir}\) (c) \(\mathrm{As}\) (d) \(\mathrm{Sc}\)

Short Answer

Expert verified
(a) f-block, (b) d-block, (c) p-block, (d) d-block.

Step by step solution

01

Understanding the Periodic Table Blocks

The periodic table is divided into four blocks: s, p, d, and f. The differentiating factor is the type of atomic orbital the outer electrons occupy. The s-block includes groups 1 and 2, the p-block comprises groups 13 to 18, the d-block consists of groups 3 to 12, and the f-block consists of the lanthanides and actinides.
02

Identify the Block for Gadolinium (Gd)

Gadolinium (\(\mathrm{Gd}\)) is an element in the lanthanide series. Elements in the lanthanide series are part of the f-block because they have their outer electrons in f-orbitals. Therefore, \(\mathrm{Gd}\) is an f-block element.
03

Identify the Block for Iridium (Ir)

Iridium (\(\mathrm{Ir}\)) is located in group 9 of the periodic table, which is within the d-block. The d-block includes transition metals where the differentiating electron enters a d-orbital. Therefore, \(\mathrm{Ir}\) is a d-block element.
04

Identify the Block for Arsenic (As)

Arsenic (\(\mathrm{As}\)) is located in group 15. The elements in groups 13 to 18 are part of the p-block since they fill p-orbitals. Thus, \(\mathrm{As}\) is a p-block element.
05

Identify the Block for Scandium (Sc)

Scandium (\(\mathrm{Sc}\)) is found in group 3, which is part of the d-block. Being in the first group of transition metals, its outer electrons occupy d-orbitals. Thus, \(\mathrm{Sc}\) is a d-block element.

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Key Concepts

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

s-block
The s-block of the periodic table is where you'll find the alkali and alkaline earth metals. These elements occupy the first two columns (groups 1 and 2) of the periodic table. The name "s-block" comes from the fact that the outermost electrons of these elements inhabit s-orbitals.

Key features of the s-block include:
  • Group 1: Alkali Metals (e.g., lithium, sodium, potassium)
  • Group 2: Alkaline Earth Metals (e.g., magnesium, calcium, strontium)
  • Highly reactive, especially group 1 elements
  • Shiny, soft, and have low melting points
The s-block plays a crucial role in many chemical reactions, given the high reactivity of these metals. Their reactivity increases as you move down the group, making them a significant focus in both chemistry education and industry applications.
p-block
The p-block elements are located on the right side of the periodic table, comprising groups 13 to 18. These elements have their outermost electrons in p-orbitals. The p-block is incredibly diverse, hosting metals, metalloids, and non-metals.

Some important characteristics:
  • Includes elements such as carbon (group 14), nitrogen (group 15), and oxygen (group 16)
  • Contains both nonmetals and metalloids
  • Encompasses a wide range of properties and reactivity
  • Houses noble gases in group 18, known for their inert behavior
The p-block elements are essential in forming various organic and inorganic compounds. They are widely used in different industries, such as silicon in technology and carbon in organic chemistry.
d-block
The d-block is positioned in the center of the periodic table and includes groups 3 to 12. Known as the transition metals, these elements have electrons filling d-orbitals. The d-block is known for its metallic characteristics and considerable industrial importance.

Distinctive features of the d-block:
  • Includes elements like iron, copper, and gold
  • Typically exhibit metallic properties: good conductors of heat and electricity
  • Often form colorful compounds
  • Have high melting and boiling points
  • Possess multiple oxidation states, making them versatile in reactions
These metals are key in various industries, ranging from construction and manufacturing to electronics and jewelry, due to their durability and conductive properties.
f-block
Hidden beneath the main body of the periodic table, the f-block contains the lanthanides and actinides. These elements are characterized by their filling of f-orbitals, resulting in the inclusion of these rare earth elements and radioactive metals.

Key points about the f-block:
  • Lanthanides commonly found from cerium ( cerium) to lutetium The lanthanides are known for their shiny, silvery appearance and are often used in products like phosphors and magnets.

  • Actinides range from thorium to lawrencium
  • Many actinides are radioactive (e.g., uranium and plutonium)
  • These elements are employed in nuclear energy applications and advanced technologies
The f-block elements have unique properties that make them valuable in high-tech and specialized uses, though they often require careful handling due to radioactivity in the actinides.

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Most popular questions from this chapter

One way to generate hydrogen gas in the laboratory is to combine a reactive metal with water. The ensuing chemical reaction produces hydrogen gas as one product. Which element would generate hydrogen gas more vigorously when combined with water: potassium or calcium? Explain your answer. Write the balanced chemical reaction for both processes.

Indicate which species in each pair has the higher ionization energy. Explain your answer. (a) Ge or \(\mathrm{Cl}\) (b) \(\mathrm{B}\) or \(\mathrm{F}\) (c) \(\mathrm{Al}^{3+}\) or \(\mathrm{Na}^{+}\)

Of the atoms with the electron configurations \(1 s^{2} 2 s^{2} 2 p^{4}\) and \(1 s^{2} 2 s^{2} 2 p^{2},\) which is smaller?

Given the following two equations, where the metals (M and \(M^{\prime}\) ) are from the second period, what are the metals, and which metal cation in the product has a larger radius? $$ \begin{array}{l} 2 \mathrm{M}+\mathrm{F}_{2} \rightarrow 2 \mathrm{MF} \\ \mathrm{M}^{\prime}+\mathrm{F}_{2} \rightarrow \mathrm{M}^{\prime} \mathrm{F}_{2} \end{array} $$

Identify the cations with a \(1+\) charge that have the following electron configurations. (a) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}\) (b) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10}\)
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