Metals

Definition

Metals are a category of elements characterized by their ability to conduct electricity and heat, their malleability, ductility, and generally shiny appearance. They typically have high melting and boiling points, and they tend to lose electrons during chemical reactions, forming positive ions. In the periodic table, metals are primarily found on the left side and in the middle, with specific trends observed in their properties as you move across periods and down groups.

5 Must Know Facts For Your Next Test

1. Metals are typically good conductors of electricity and heat due to the presence of free-moving electrons within their structure.
2. As you move down a group in the periodic table, metallic character increases, meaning elements become more likely to lose electrons and form positive ions.
3. Metals tend to have higher densities compared to nonmetals and are often solid at room temperature, with the exception of mercury, which is a liquid.
4. The reactivity of metals generally increases as you move down a group; for example, alkali metals become more reactive from lithium to cesium.
5. Metals can be categorized into different types, including alkali metals, alkaline earth metals, transition metals, and post-transition metals, each exhibiting distinct physical and chemical properties.

Review Questions

• How do the physical properties of metals relate to their position on the periodic table?
  • The physical properties of metals, such as conductivity, malleability, and density, show clear trends based on their position in the periodic table. For instance, as you move from left to right across a period, elements tend to become less metallic in character, showing decreases in conductivity and malleability. Conversely, moving down a group generally enhances metallic properties due to increased atomic size and decreased ionization energy, making it easier for metals to lose electrons.
• Discuss how the reactivity of metals changes within a group in the periodic table and provide an example.
  • Within a group in the periodic table, the reactivity of metals tends to increase as you go down. This trend is due to the increasing atomic size which results in a greater distance between the nucleus and the outer electrons. For example, alkali metals like lithium are less reactive than cesium; while lithium reacts vigorously with water, cesium reacts explosively. This pattern is attributed to lower ionization energy for larger atoms.
• Evaluate the implications of metallic bonding on the physical properties of metals and their applications in everyday life.
  • Metallic bonding results from the attraction between metal cations and a 'sea' of delocalized electrons that move freely throughout the structure. This unique bonding contributes to key physical properties like high electrical and thermal conductivity, malleability, and ductility. These characteristics make metals essential for a variety of applications in everyday life—from electrical wiring that requires efficient conductivity to structural components in buildings that benefit from malleability and strength. Understanding these properties allows us to utilize metals effectively in technology and engineering.

Related terms

Alloys: Alloys are mixtures of two or more elements, where at least one of them is a metal, designed to enhance specific properties such as strength or resistance to corrosion.

Electronegativity:

Electronegativity is a measure of an atom's ability to attract and hold onto electrons; metals generally have lower electronegativity compared to nonmetals.

Transition Metals:

Transition metals are elements found in groups 3-12 of the periodic table that display unique properties such as variable oxidation states and the ability to form colored compounds.