Features
Features:

Product Tour >

Edraw AI >

Paid Plans:

Individuals >

Business >

Eduaction >
Resources
Blog

History

How-tos & Tips

Discovery

Biography

Business Analysis

Examples

AI concept Map

Free AI Mind Map Generator

Onenote Mind Map

Bcg Matrix Examples

Nike Marketing Strategy

Unilever SWOT Analysis

Make Mind Maps in Google Docs

Guide

FAQs

What's New

Resource Center
Templates
All Templates

Brain Storming Templates

Strategy and Planning Templates

Project Management Templates

Product Management Templates

Human Resources Templates

Agile Workflow Templates

Marketing Templates

Education Templates

Fun and Games Templates

User Gallery
Download
Pricing
Enterprise

S area element

This is a mind map about S-block elements. The main contents include: overview of S-block elements, elements of S-block, the particularity of lithium and beryllium, the diagonal principle, and compounds of S-block elements.

Edited at 2024-03-03 14:16:54

PlotWizard

Recent works View more works>>

S area element

PlotWizard

Recent works View more works>>

Recommended to you
Outline

S area element

Compounds of S block elements

Hydride

1. Ionic hydrides are all white crystals at room temperature. Their melting points and boiling points are higher than 9, and they can conduct electricity when melted.

2. Both can undergo violent hydrolysis reactions with water to release hydrogen.

MH H2O→MOH H2,

MH2 2H2O→M(OH)2 2H2

3. All have strong reducibility

TiCl4 4NaH→Ti 4NaCl

oxide

Normal oxide O2-

Li, Be, Mg, Ca, Sr, Ba

Peroxide O22-

Na, Ba

Superoxide O2-

(Na),K,Rb,Cs

Ozonide O3-

hydroxide

Except Be(OH)f2, which is an amphoteric hydroxide, other hydroxides are strong or medium-strong bases.

Important salts and their properties

1·Properties of salts

Crystal type - ionic crystal; Solubility - easily soluble in water; Thermal stability - high

To obtain anhydrous MgCl2, MgCl2·6H2O must be heated in a dry HCl flow to dehydrate it. CaCl2·6H2O can be directly heated for dehydration

2. Several important salts

Halide; sulfate; carbonate

The thermal stability rules of alkaline earth metal carbonates can be explained by polarizing ions. In carbonates, the smaller the cation radius, that is, the larger the z/r value, the stronger the polarization force, and the easier it is to convert CO2-

It takes oxygen from it to become an oxide and releases it at the same time

CO , shows that the thermal stability of carbonate is worse and it is easy to decompose when heated. The polarization force of alkaline earth metal ions is stronger than that of the corresponding alkali metal ions, so the thermal stability of the carbonates of alkaline earth metals is worse than that of the corresponding alkali metals. The polarizing forces of Li + and Be2 are the strongest among alkali metals and alkaline earth metals, so Li2CO3 and BeCO3 are the most unstable among the carbonates of their respective congeners.

complex

Special characteristics of lithium and beryllium Diagonal principle

Special features of lithium

Although the standard electrode potential of lithium is smaller than that of cesium, its reaction with water is not as violent as that of sodium.

This is because the sublimation enthalpy of lithium is very large and it is not easy to activate, so the reaction rate is small. In addition, the lithium hydroxide generated by the reaction has a low solubility and covers the metal surface, which also reduces the reaction rate.

Lithium's melting point and hardness are higher than other alkali metals, but its conductivity is weak. The chemical properties of lithium are inconsistent with the chemical properties of other alkali metals. The standard electrode potential E (Li/Li) of lithium is abnormally low among elements of the same family, which is related to the greater hydration heat release of Li*(g). When lithium burns in the air, it can form ordinary oxides with oxygen. Li, Q directly interacts with nitrogen to form nitrides. This is because its ionic radius is small and therefore contributes greatly to the lattice energy.

Lithium compounds are also qualitatively different from other alkali compounds. For example, the covalency of lithium compounds is more significant than that of other alkali metal compounds. LiOH decomposes when red hot, but other MOH does not decompose; LiH has higher thermal stability than other MH; LiF, Li2CO3, Li, PO4 are difficult to Dissolved in water.

Special features of beryllium

Beryllium's melting point and boiling point are higher than other alkaline earth metals, and its hardness is also the largest among alkaline earth metals, but it is brittle. Beryllium also has a large electronegativity and has a strong tendency to form covalent bonds. For example, BeCl2 is a covalent compound, while other alkaline earth metal chlorides are basically ionic. In addition, beryllium compounds have relatively poor thermal stability and are easily hydrolyzed. Beryllium hydroxide, Be (OH), is amphoteric. It is soluble in both acid and alkali.

diagonal principle

This can be roughly explained from the perspective of ion polarization. For metal ions with the same outermost electron configuration in the same period, the polarization increases as the ion charge number increases from left to right. For metal ions in the same group with the same charge number, the polarization weakens as the ion radius increases from top to bottom. Therefore, two adjacent elements located on the upper left and lower right diagonal positions in the periodic table have opposite effects of charge number and radius. Their ion polarizations are relatively similar, which makes their chemical properties have many similarities.

Elements of S block elements

physical properties

Light, soft, low melting point

Silvery white (beryllium is gray) metal with metallic luster

chemical properties

alkali metal

Alkali metals are highly reactive and can easily form a covering layer of M2CO3 in the air, so they should be stored in anhydrous kerosene. Lithium has a low density and can float on kerosene, so it is preserved in liquid paraffin. Only lithium can react with N2

rare earth metal

Alkaline earth metals are less reactive than alkali metals, and a dense oxide protective film is formed on the surface of beryllium and magnesium. Except beryllium, all can react with N2

flame reaction

Lithium (dark red) Sodium (yellow) Potassium (purple) Rubidium (red-purple) Cesium (blue) Calcium (orange-red) Strontium (dark red) Barium (green)

The reason for the flame reaction: When their atoms or ions are heated, electrons are easily excited. When the electrons transition from a higher energy level to a lower energy level, the corresponding energy is released in the form of light, producing a linear spectrum. The color of the flame often corresponds to the region of spectral lines with greater intensity

The existence of S-block elements and the preparation of elemental substances

S-block elements are active metallic elements, so they do not exist as elements in nature. These elements mostly exist in the form of ionic compounds.

Overview of S-zone elements

Element classification

Group IA (alkali metals)

Lithium sodium potassium rubidium cesium francium

Group IIA (alkaline earth metals)

beryllium magnesium calcium strontium barium

Element properties

From top to bottom, nuclear charge ↑, radius ↑, ionization energy ↑, electronegativity ↓, metallic reducibility ↑, melting and boiling point ↓, density ↑

·Except for beryllium, all elements in the S block can be dissolved in liquid ammonia to form a blue reducing solution. ·Except for beryllium and magnesium, they are all easy to react with water.

·Among the S-block elements, lithium, beryllium, rubidium, and cesium are rare metal elements. Francium and radium are radioactive elements.