Question

A nuclide of an alkaline earth metal undergoes radioactive decay by emission of the \(\alpha\) particle in succession. The group of the periodic table to which the resulting daughter element would belong is (a) Gp 14 (b) Gp 6 (c) Gp 16 (d) Gp 4

Short answer

The resulting daughter element belongs to Group 16.

Step-by-step solution

Identify the characteristics of the given element

An alkaline earth metal is in Group 2 of the periodic table. These elements have two valence electrons and are located in the second column.

Understand the effect of alpha emission

Alpha emission occurs when a nucleus emits an alpha particle, which consists of 2 protons and 2 neutrons. This process reduces the atomic number by 2 and the mass number by 4.

Apply changes to the alkaline earth metal

For an alkaline earth metal (Group 2 element) undergoing alpha decay, the atomic number will decrease by 2. Since the original element was in Group 2, subtracting 2 places it in Group 16 of the periodic table.

Key concepts

Alkaline Earth Metals

Alkaline earth metals are a fascinating group of elements that belong to Group 2 on the periodic table. They include elements like beryllium, magnesium, calcium, strontium, barium, and radium. These metals are known for their shiny appearance and high reactivity, though they are not as reactive as alkali metals. Because they have two electrons in their outermost shell, they tend to lose these electrons to achieve a stable electronic configuration. This characteristic makes them highly reactive with other elements.

• Located in Group 2 of the periodic table.
• Includes elements such as magnesium and calcium.
• Typically shiny and silvery-white in color.
• Have two valence electrons.
• Form compounds through ionic bonds.

These metals play crucial roles in various applications, from forming structural materials to being essential for biological processes in organisms. Understanding their fundamental properties provides insight into their chemical behavior and interaction with other elements.

Alpha Emission

Alpha emission is a type of radioactive decay in which a nucleus emits an alpha particle. An alpha particle is essentially a helium nucleus, consisting of two protons and two neutrons. This emission results in a reduction of both the atomic number and the mass number of the original nucleus.
When an element undergoes alpha decay, its atomic number decreases by two, while its mass number decreases by four. This change happens because the alpha particle takes away 2 protons and 2 neutrons.

• Emits an alpha particle (2 protons and 2 neutrons).
• Decreases the atomic number by 2.
• Decreases the mass number by 4.
• Translates the element to a new position on the periodic table.

The effect of alpha emission is significant in altering the identity of an element, as it moves it to a different group in the periodic table. This process is commonly observed in heavy nuclides and can result in the transformation of the element into another.

Periodic Table Groups

Understanding periodic table groups is crucial to predicting and explaining elements' chemical behavior. Each group is a vertical column on the periodic table, and elements within the same group often share similar properties due to their identical number of valence electrons.
For instance, alkaline earth metals in Group 2 have two valence electrons, leading to reactive behavior typical of this group. When an alpha emission occurs, as discussed, the reduction in atomic number results in the shifting of the element to a different group.

• Groups are vertical columns on the periodic table.
• Elements in the same group share similar properties.
• Group numbers can be associated with similar electron configurations.

In the context of the example provided, an alkaline earth metal undergoing alpha decay moves from Group 2 to Group 16. This demonstrates how changes in atomic structure due to processes like alpha emission can significantly impact an element's placement and chemical properties.