Question

Answer the following questions for the elements from scandium through zinc: (a) Are they metals or nonmetals? (b) To what general class of elements do they belong? (c) What subshell is being filled by electrons in these elements?

Short answer

(a) Metals, (b) Transition metals, (c) 3d subshell.

Step-by-step solution

Identify Elements in the Range

The elements from scandium (Sc) to zinc (Zn) are scandium, titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper, and zinc, which are the ten elements that occupy the 3d block in the periodic table.

Determine if Metals or Nonmetals

Examine each element and refer to the periodic table to determine if they are metals or nonmetals. Elements from scandium to zinc are all metals. They are characterized by their ability to conduct electricity and heat, and are typically malleable and solid at room temperature.

Classify the General Class

All the elements from scandium to zinc belong to the general class called 'transition metals.' These are elements found in groups 3-12 of the periodic table known for having d subshells being filled with electrons.

Identify the Subshell Being Filled

Look at the electronic configuration of these elements. The subshell that is being filled with electrons for scandium through zinc is the 3d subshell. This is characteristic of transition metals, which fill the d subshell during the transition from one period to the next in the periodic table.

Key concepts

Periodic Table

The periodic table is a comprehensive chart that displays all known chemical elements. It organizes these elements by increasing atomic number, effectively grouping them based on similar chemical properties.
This arrangement helps us understand patterns among elements, especially the way they interact in chemical reactions. The periodic table is divided into several blocks, with each block corresponding to a specific type of electron subshell being filled.

• The s-block includes the first two columns, mainly consisting of metals like alkali and alkaline earth metals.
• The p-block includes the last six columns, where you find nonmetals and metalloids.
• The d-block, where transition metals reside, fills the columns from group 3 to group 12.
• The f-block contains the lanthanides and actinides, which are placed separately at the bottom.

The elements from scandium (Sc) to zinc (Zn) are in the d-block, specifically in the 3d series. Understanding their placement helps clarify their physical and chemical properties.

d subshell

Subshells refer to divisions of electron shells in each atom's electron cloud. Each shell contains subshells labeled s, p, d, and f, corresponding to a specific number of electrons they can hold.
- The d subshell can hold up to 10 electrons. It plays a crucial role in giving transition metals their unique properties. For example, the d subshell allows elements to form multiple oxidation states.
For the elements ranging from scandium to zinc, it's the 3d subshell that is being filled. This means that as you move from element to element in this series, the 3d subshell gradually fills with electrons. Such filling is central to the behavior and chemistry of transition metals.
Here’s how it works:

• Electrons fill the 3d subshell following the Pauli exclusion principle and Hund's rule, which help predict electron arrangements.
• This d subshell filling gives rise to properties like magnetism and variable valency.

Grasping the concept of subshells allows a deeper understanding of why elements in the same block behave similarly.

Scandium to Zinc

From scandium (Sc) to zinc (Zn), we encounter what are known as transition metals. These 10 elements form an essential part of the periodic table in the 3d block and have unique physical and chemical properties.
These elements are recognized by certain shared characteristics:

• All are metals, exhibiting high conductivity of electricity and heat.
• They are typically dense and possess high melting points.
• Each element is capable of forming colored compounds, which is often a result of d-d electron transitions.
• These metals have the ability to assume various oxidation states, which is useful in forming a myriad of complex compounds.

Amongst them, scandium is where the 3d subshell starts to fill up its electrons, and the process continues across to zinc, making them quintessential examples of transition metals. These characteristics make them valuable in industrial applications and research in chemistry.