Metals in Periodic Table — Reading Comprehension

Metals are a group of elements that make up the majority of the periodic table. Their importance in daily life is evident in everything from coins and cooking pans to skyscrapers and smartphones. The unique properties of metals, such as luster, conductivity, malleability, and ductility, have shaped technology and society. Scientists have worked to understand why metals behave differently from other elements and how their structure leads to these remarkable traits.

Atomic Structure and Physical Properties
Metals are found on the left and center of the periodic table. They are typically solid at room temperature, except for mercury, which is a liquid. At the atomic level, metals have a structure called a metallic bond. In this bond, atoms share a 'sea' of electrons that move freely between them. This movement of electrons explains why metals conduct electricity and heat so well. For example, copper wires are used in electrical circuits because their free electrons allow electric current to flow efficiently. The same structure gives metals their shiny appearance, or luster, because light bounces off the closely packed atoms. The ability to bend and shape metals without breaking—called malleability—and to stretch them into wires—called ductility—are also results of this flexible atomic arrangement.

Examples and Applications
Different metals are chosen for specific uses based on their properties. Iron is strong and forms the backbone of buildings and bridges. Aluminum is lightweight and resists rust, making it perfect for airplane bodies and soda cans. Gold and copper are excellent conductors and are used in electronics and jewelry. Quantitatively, about 75% of the elements in the periodic table are classified as metals. This abundance allows for a wide range of alloys—mixtures of metals with other elements—to further enhance their properties. For instance, adding carbon to iron creates steel, which is even stronger and more durable.

Metals in Society and Science
The interactions between metals and their surroundings have broad implications. Conductive metals have enabled the development of power grids and advanced electronics, which are essential for modern society. However, not all metals are equally reactive. Some, like gold, resist corrosion, while others, like iron, rust easily when exposed to air and water. Understanding these differences helps engineers select the right material for specific environments, whether building a bridge or designing a smartphone.

Metals illustrate how atomic-level structures influence the observable world. Their physical properties arise from the interactions of electrons and atoms, demonstrating key principles of chemistry and physics. As new alloys and materials are developed, the study of metals continues to drive technological innovation and scientific discovery.

Interesting Fact:
Mercury is the only metal that is liquid at room temperature, making it unique among all metals on the periodic table.

Where are metals located on the periodic table?

What is the only metal that is liquid at room temperature?

Which property allows metals to be hammered into sheets without breaking?

What does conductivity mean in relation to metals?

What is a metallic bond?

Based on the passage, why are copper wires used in electrical circuits?

Why do scientists mix metals with other elements to create alloys?

If a material can be drawn into wires, it is described as:

True or False: All metals are solid at room temperature.

True or False: Gold resists corrosion better than iron.