Question

Наиболее ярко выражены металлические свойства у атома Mg Rb AL Na ​

Answer 1

Ответ:

Rb, Na

Объяснение:

обусловлено низкой ионизацие энергии.

Answer 2

At the atomic level, metallic properties are primarily determined by the arrangement and behavior of electrons in the outermost energy level or valence shell of an atom.

Magnesium (Mg), rubidium (Rb), aluminum (Al), and sodium (Na) are all elements found in the periodic table. These elements are all metals and exhibit similar metallic properties to varying degrees. Here's an explanation of how each of these elements demonstrates metallic characteristics:

1. Magnesium (Mg): Mg is a highly reactive metal known for its strong and lightweight properties. It has two valence electrons in its outermost energy level, which allows it to lose those electrons easily and form a stable 2+ cation. This ability to lose electrons readily makes Mg a good conductor of electricity and heat. Additionally, Mg has metallic luster and is malleable and ductile, meaning it can be hammered into thin sheets or drawn into wires without breaking.

2. Rubidium (Rb): Rb is a highly reactive alkali metal. It has only one valence electron, which makes it highly likely to donate that electron and form a stable 1+ cation. Like other metals, Rb is a good conductor of electricity and heat due to the ability of its valence electron to move freely in the metallic lattice structure. Rb is also lustrous, malleable, and ductile.

3. Aluminum (Al): Aluminum is a lightweight metal with a variety of applications. It has three valence electrons, allowing it to lose these electrons and form a 3+ cation. Aluminum demonstrates excellent thermal and electrical conductivity due to the movement of these delocalized electrons. It is also corrosion-resistant because of its ability to form a protective oxide layer on its surface. Aluminum is malleable and ductile.

4. Sodium (Na): Sodium is an alkali metal known for its reactivity and low melting point. It has only one valence electron, which it readily donates to form a stable 1+ cation. As a result, sodium exhibits metallic properties such as good electrical and thermal conductivity. It is also malleable, ductile, and has a shiny appearance due to its ability to reflect light.

In summary, all these elements (Mg, Rb, Al, Na) demonstrate metallic properties due to the presence of valence electrons that can easily move within the atomic structure. These valence electrons are responsible for the excellent thermal and electrical conductivity, lustrous appearance, and malleable and ductile nature of these metals.