The higher the valency of a metal element, the stronger the electron loss ability

No. The higher the valency of the metal elements in the same period, the weaker the metallicity, and the weaker the ability to lose electrons, such as Na, Mg, and Al The ability to lose electrons is weakened.

The valency increases, loses electrons in the reaction, is oxidized, acts as a reducing agent, in the periodic table.

The more left and lower the elements, the stronger the metallicity, the easier it is to lose electrons, and it is often used as a reducing agent in the reaction; In the same way, the more elements are on the upper right, the stronger the non-metallic properties, the easier it is to get electrons, and they are often used as oxidizing agents in reactions.

Valence is a chemical bond between one atom of an element and the atoms of another element.

quantity. An atom is made up of atomic nuclei.

and the outer electrons, which move in layers around the nucleus, and the individual atoms of the compound are bonded with as many valencies as the valence.

interconnected. The valence electrons around the element form a covalent bond.

A monovalent atom can form a covalent bond, and a bivalent atom can form two bonds or a bond plus a bond. Valency is the number of electrons gained or lost by atoms in a substance, or the number of shifts in shared electron pairs. Valency is also a property exhibited by an element in the formation of a compound.

The oxidation number, also known as the oxidation state, is based on the valency theory and the electronegativity of the element.

A chemical concept developed on the basis of a concept, which to a certain extent marks the combined state of an element in a compound. When leveling the redox reaction equation according to the rise and fall of valency and electron transfer, it is often difficult to determine the valency number of elements for other substances except simple ionic compounds. For some complex compounds or clusters of atoms, it is more difficult to determine their electron transfer in the reaction, and thus it is difficult to represent the valence state of the elements in the substance.

No. The ability of atoms of metal elements to lose electrons is generally related to the atomic radius and the electron configuration outside the nucleus.

In the table of metal activity sequences, the higher the left side is, the more likely it is to lose electrons, and from left to right, the ability to lose electrons gradually decreases.

Junior high) potassium, K calcium, ca sodium, magnesium, mg, aluminum, al, zn, zn, iron, fe, tin, sn, lead, pb (hydrogen, h), copper, cu, mercury, hg, silver, ag, platinum, pt, gold, au, and weakened sequentially.

Summary. Pro, the strength of a metallic bond is closely related to the electronic structure, so as the number of valence electrons increases, the strength of the metallic bond also increases accordingly. Specifically, atoms in metals are often surrounded by clouds of electrons that form so-called "metallic bonds".

Pro, the strength of a metallic bond is closely related to the electronic structure, so as the number of valence electrons increases, the strength of the metallic bond also increases accordingly. Specifically, the atoms in a metal are usually surrounded by a telemeter cloud that forms so-called "metal bonds".

These electron clouds can move freely, forming an ocean-like electron gas. When there are more valence electrons between the metal atoms, these electrons will fill the electron cloud, making the electron cloud more dense, compact, and tough.

The structure of this electron cloud also leads to a decrease in the repulsive force between the clusters of metals, which further enhances the strength of the metal bonds. Therefore, in a metal, if it has more valence electrons, then its metallic bonds will be more stable and strong.

The valency of a metal element is generally equal to the number of electrons in the outermost shell, such as +1 valence for sodium and +2 valence for magnesium.

The negative valency of non-metallic elements = = the number of electrons in the outermost shell - 8, such as oxygen has 6 electrons in the outermost shell, the valency is -2 valence, and the outermost shell of nitrogen has 5 electrons and the negative valence is -3 valence.

The highest positive valency of non-metallic elements = = the outermost electron number, such as sulfur is +6 valence, nitrogen is +5 valence, special oxygen has no +6 valence, and fluorine has no positive valence.

For metal ions that have lost their electrons, they should be oxidizing.

Only metal elements are reducible under certain circumstances (such as the well-known aluminum, which is very reducible at high temperatures) and is prone to electron loss and ionization.

In this topic, if we talk about the relationship between the electron loss and the reducibility of the atom of the metal element, if there are multiple positive valences of the same metal, theoretically speaking, the less electrons are lost, the stronger the reduction (electron loss ability), such as the ability of iron atoms to become Fe2+ is stronger than the ability of Fe3+ (it is necessary to use a strong oxidant to make metal iron directly become Fe3+), but because the substances composed of low-valent metal ions are often unstable, such as Fe2+ is easy to be oxidized, so Fe3+ is more common, If it is a different kind of metal, it is directly related to the activity of the metal, such as various alkali metals (potassium, sodium, etc.), alkaline earth metals (calcium, barium, etc.), its metal elemental reduction is definitely stronger than that of metals such as iron or copper, theoretically the stronger the metal activity, the stronger the reduction.

Metal ions that have lost electrons, their oxidation is just the opposite, the weaker the metal activity, the stronger the oxidation of the cation (the ability to gain electrons), such as the electron-gaining ability of gold ions (Au3+) is the strongest among all metal ions, for the same kind of metal ions, the oxidation of more electrons is stronger, such as Fe3+, the oxidation is definitely stronger than Fe2+ (in fact, it is stronger than Cu2+, so the aqueous solution containing Fe3+ can react with copper metal to form Fe2+ and Cu2+)

The reducing agent loses electrons and the valency increases; The oxidizing agent gets electrons and the valency decreases.

Such a reaction is a redox reaction.

Oxidation-reduction reaction is a type of reaction in which the oxidation number of an element changes before and after a chemical reaction. The essence of a redox reaction is the gain or loss of electrons or the shift of shared electron pairs. Redox reaction is one of the three basic reactions in chemical reactions (the other two are (Lewis) acid-base reaction and free radical reaction).

Combustion, respiration, photosynthesis, chemical batteries in production and life, metal smelting, rocket launches, etc. are all closely related to redox reactions in nature. The study of redox reactions is of great significance to the progress of mankind.

Before and after the redox reaction, the oxidation number of the element changes. Depending on the increase or decrease in the oxidation number, the redox reaction can be split into two half reactions: the half reaction with the increased oxidation number is called the oxidation reaction; The reaction with a decrease in oxidation number is called a reduction reaction.

Oxidation and reduction reactions are interdependent and cannot exist independently, and together they constitute redox reactions.

In the reaction, the substances that undergo oxidation reactions, called reducing agents, produce oxidation products; A substance that undergoes a reduction reaction, called an oxidant, produces a reduction product. Oxidation products are oxidizing but weaker than oxidants; The reducing product is reducing, but weaker than the reducing agent.

Whether a chemical reaction is a redox reaction can be judged according to whether the reaction has an increase in oxidation number, or whether there is electron gain, loss and transfer.

The determination of redox reactions in organic chemistry is usually based on whether the oxidation number of carbon changes: if the oxidation number of carbon increases, the reaction is an oxidation reaction; When the oxidation number of carbon decreases, this reaction is a reduction reaction. Since in the vast majority of organic matter, hydrogen always presents a positive valence state, and oxygen always presents a negative valence state, so the reaction of organic matter to obtain hydrogen and lose oxygen is generally called reduction reaction, and the reaction of oxygen loss and hydrogen loss is called oxidation reaction.

1. Strength and weakness law: oxidation: oxidant oxidation product; Reducibility: Reducing agent" reducing product.

2. Valence law: the element is in the most advanced state and only has oxidation; The element is in the lowest valence state and is only reductive; It is in the intermediate valence state, which is both oxidizing and reducing.

3. Transformation law: when the centering reaction occurs between different valence states of the same element, the oxidation number of the element is only close but not crossed, and the maximum value of the same element reaches the same valence state.

4. Priority law: For the same oxidant, when there are multiple reducing agents, it usually reacts with the most reducible reducing agent first.

5. Conservation law: The number of electrons obtained by the oxidant is equal to the number of electrons lost by the reducing agent.

Electrons are lost, valency increases, it is reducible, it is a reducing agent, it is oxidized, and an oxidation reaction occurs.

When electrons are obtained, the valency decreases, it has oxidizing properties, it is an oxidizing agent, it is reduced, and a reduction reaction occurs.

a. For the same periodic element, the smaller the atomic radius, the stronger the non-metallic property, the easier it is to gain electrons, and the more difficult it is to lose electrons, so a is wrong; b. For elements of the same main group, the larger the atomic radius, the stronger the metallicity, the stronger the reduction, and the weaker the oxidation, so B is wrong; c. The elemental formed by group A elements, similar in structure, are all molecular crystals, the larger the relative molecular mass, the higher the melting point of the element, so the melting point of the elemental increases with the increase of the atomic number of the element, so C is wrong; d. From top to bottom, the non-metallic property of the same main group is weakened, and the stronger the non-metallic property, the more stable the hydroxide is, so from top to bottom, the hydride stability formed by group A elements gradually weakens, so D is correct; Therefore, choose D

The lower the number of electrons in the outermost shell, the more electron layers there are, the stronger the metallicity.

Metallity refers to the ability of a metallic element to lose electrons in a chemical reaction. The stronger the electron-losing particle, the more metallic the element belongs; The weaker it is.

So the metallicity is not proportional to the number of electrons lost, for example: sodium loses one electron in the reaction, magnesium loses two electrons, but sodium is more metallic than magnesium.

Metallicity judgment is based on 1The ease and intensity of the reaction between metal and water under certain conditions. In general, the easier and more intense the reaction with water, the stronger its metallicity.

2.The ease and intensity of the reaction with the same concentration of acid at room temperature. In general, the easier and more intense the reaction with the acid, the stronger its metallicity.

3.According to the alkalinity of the most ** oxide hydrate. The more alkaline it is, the more metallic it is.

4.Displacement reactions between metal elements.

5.Oxidation of metal cations. The stronger the oxidation, the weaker the metallicity.