Metals

Definition

Metals are a class of elements characterized by their shiny appearance, good conductivity of heat and electricity, and malleability. They typically form cations by losing electrons in chemical reactions and are found on the left side and in the center of the periodic table. The properties of metals, such as ductility and tensile strength, are essential for various applications in industry and technology.

5 Must Know Facts For Your Next Test

1. Metals are typically solid at room temperature, except for mercury, which is liquid.
2. Most metals have high melting and boiling points due to strong metallic bonds.
3. Metals tend to lose electrons during chemical reactions, resulting in positive ions (cations).
4. The metallic character of elements increases as you move down a group in the periodic table.
5. Alloys are mixtures of two or more metals that enhance specific properties like strength and corrosion resistance.

Review Questions

• How do the physical properties of metals contribute to their common uses in everyday applications?
  • The physical properties of metals, such as conductivity, malleability, and ductility, make them ideal for a wide range of everyday applications. For example, copper is widely used in electrical wiring due to its excellent conductivity, while aluminum is used for cans and foils because it is lightweight yet strong. The ability of metals to be shaped into wires or sheets allows them to be utilized in construction, automotive manufacturing, and electronics.
• Discuss the trends in metallic character across the periodic table and how these trends relate to reactivity.
  • As you move from right to left across a period on the periodic table, the metallic character increases. This trend is due to the decreasing electronegativity and ionization energy of elements as they become more metallic. Additionally, metallic character increases down a group because atomic size increases, making it easier for these elements to lose electrons. Consequently, alkali metals at the bottom left are more reactive than transition metals or nonmetals found higher up on the right side.
• Evaluate how the properties of transition metals differ from those of alkali metals and what implications these differences have for their uses in technology.
  • Transition metals possess unique properties compared to alkali metals due to their ability to form multiple oxidation states and complex ions. This allows transition metals like iron and copper to be used in various industrial applications such as catalysts or in producing alloys that enhance strength. In contrast, alkali metals are highly reactive and typically used in simpler applications like batteries or as reducing agents. Understanding these differences is crucial when selecting materials for specific technological purposes.

Related terms

metalloids: Elements that have properties intermediate between metals and nonmetals, often displaying a mix of metallic and nonmetallic characteristics.

alkali metals:

Highly reactive metals found in group 1 of the periodic table, known for their soft texture and low density.

transition metals:

Elements found in groups 3 to 12 of the periodic table, known for their ability to form various oxidation states and colored compounds.