Arrange these elements in order of decreasing metallic character: Sr, N, Si, P, Ga, Al.

Key Concepts

Metallic Character

Metallic character refers to the set of properties associated with metals, including conductivity, malleability, ductility, and luster. It generally increases as you move down a group in the periodic table and decreases across a period from left to right. This trend is due to the increasing atomic size and decreasing ionization energy, which make it easier for atoms to lose electrons.

Periodic Trends

Periodic trends are predictable patterns observed in the periodic table, such as atomic radius, electronegativity, and ionization energy. Understanding these trends helps in predicting the behavior of elements, including their metallic character. For instance, elements on the left side of the periodic table tend to exhibit more metallic properties compared to those on the right.

Group and Period Position

The position of an element in the periodic table, defined by its group (vertical column) and period (horizontal row), significantly influences its properties. Elements in the same group share similar characteristics, while those in the same period show a gradual change in properties. For example, alkaline earth metals like strontium (Sr) are highly metallic, while nonmetals like nitrogen (N) are not.