Question

Помогите, пожалуйста! Сколько наружных электронов имеют атомы металлов? Что происходит с их наружными электронами? Какой металл - натрий или магний - более активен и почему? Какой из металлов самый активный? Как устроена кристаллическая решетка металлов? Какие особые свойства имеют металлы и чем обусловлены такие свойства?

Answer 1

Правильнее сказать не наружные, а валентные :)
Металлы имеют 1, 2, 3 валентных электрона, кроме некоторых исключений
Натрий более активен, потому что он находится в группе щелочных металлов, а магний - щелочно-земельные, щелочные - активнее.
Самый активный - Франций. Кристаллическая металлическая решетка устроена так: в узлах стоят атомы или ионы, и "бегают" обобществленные электроны. Слои в решетке могут смешаться относительно друг друга, может меняться расстояние между слоями, но сами слои сохраняются. 
Свойства:
Метал. блеск из-за обобществленных электронов
Пластичность и ковкость - из-за смешения и уменьшения расстояния между слоями
Теплопроводность из-за увеличения подвижности электронов при нагревании
Электропроводность: при помещении металла в электрическое поле электроны двигаются направленно

Answer 2

Number of Valence Electrons in Metal Atoms:

Atoms of metals typically have a few valence electrons. The number of valence electrons in metal atoms is determined by their position in the periodic table. Metals are found on the left side of the periodic table, and the number of valence electrons increases from left to right within a period. For example, alkali metals like sodium (Na) have one valence electron, while alkaline earth metals like magnesium (Mg) have two valence electrons [[1]].

Behavior of Valence Electrons in Metal Atoms:

The valence electrons in metal atoms are loosely held and can move freely within the metal structure. This is due to the metallic bonding, which is a type of chemical bonding that occurs between metal atoms. In metallic bonding, the valence electrons are delocalized and form a "sea" of electrons that are shared by all the metal atoms. This delocalization of electrons allows metals to conduct electricity and heat efficiently [[2]].

Reactivity of Sodium and Magnesium:

Sodium (Na) and magnesium (Mg) are both metals, but sodium is more reactive than magnesium. This is because sodium has only one valence electron, which is easily lost to form a stable cation with a full outer electron shell. On the other hand, magnesium has two valence electrons, which require more energy to be removed. Therefore, sodium is more likely to undergo chemical reactions and form compounds compared to magnesium [[3]].

Most Reactive Metal:

The most reactive metal is francium (Fr), which is an alkali metal. Francium is located at the bottom of Group 1 in the periodic table and has only one valence electron. Due to the low ionization energy required to remove this electron, francium is highly reactive and can react explosively with water and other substances. However, francium is extremely rare and highly radioactive, making it difficult to study its reactivity in detail [[4]].

Crystal Structure of Metals:

Metals have a unique crystal structure known as a metallic lattice or metallic crystal. In this structure, metal atoms are arranged in a regular pattern, forming a three-dimensional network. The arrangement of atoms in the crystal lattice allows for the delocalization of valence electrons, which contributes to the characteristic properties of metals, such as high electrical and thermal conductivity, malleability, and ductility [[5]].

Special Properties of Metals:

Metals possess several special properties that distinguish them from nonmetals. These properties include:

1. High electrical conductivity: Metals are excellent conductors of electricity due to the presence of delocalized electrons that can move freely within the metal structure. 2. High thermal conductivity: Metals also have high thermal conductivity, allowing them to efficiently transfer heat. 3. Malleability: Metals can be easily hammered or rolled into thin sheets without breaking. 4. Ductility: Metals can be drawn into thin wires without breaking. 5. Luster: Metals have a characteristic shiny appearance due to the reflection of light by the delocalized electrons. 6. High melting and boiling points: Metals generally have high melting and boiling points compared to nonmetals, which is attributed to the strong metallic bonding between atoms.

These special properties of metals are primarily due to the presence of delocalized electrons and the metallic bonding within the crystal lattice [[6]].

I hope this information helps! Let me know if you have any further questions.