IONIC OR ELECTROVALENT BONDS:

Definition of ionic or Electrovalent bond:

It formed by electrostatic attraction between positive and negative ions, this is achieve by the transfer of single or more electrons to the atoms or atomic groups.

• Atom loses or gain electrons to gain nearest Nobel gas configuration.

• Ionic bonds are most likely to formed by when compounds have low ionization energies will react with elements have higher electronegative and electron affinity.

• Generally:

Group IA and IIA react with VI A or VII A.

• Mostly metals and non metal react to form the ionic compounds.

Reaction of sodium with chloride(example of electrovalent compounds):

Na +Cl ---->NaCl

In this reaction sodium loses a single electron to achieve neon ( Nobel gas) configuration.

The energy it required is 496kJ/mol

Where as the chlorine attain a electron and converted to chloride ion it is trying to get electronic configuration of argon .

The energy it releases is 349kJ/mol

IONIC CRYSTAL STRUCTURE:

Ionic compounds are usually solid in normal condition. The electrostatic attraction between the ion Do not have a particular direction, So it attract charged ion from the all direction. Whereas, like-charged ion will repel each other that is why compound would not exist in gas phase at normal conditions. In solid state ionic molecules do not exist in gaseous form.

LATTICE ENERGY:

The negatively and positively charged ion will be arranged in three dimensional manner in an alternating cation-anion pattern.

Energy will be released when an ionic lattice will forms from isolated gaseous ions.

X-RAY diffraction:

The crystal lattice are made up spherical ions.

UNIT CELL:

The repeated three dimensional manner of small structural unites to form the crystal lattice.

Unit cell specification:

crystal lattice can be specify by unit cell of lattice.

• The entire crystal is generated by the translation of three dimensions.

• Crystal coordinate number of ion will be indicated.

• Formula of the compound will be consistent.

CsCl Cesium Chloride Structure:

• Cation and anion are of nearly same size.

• Coordination number is 8

• Radius ratio is 0.93

• Each C’s is surrounded by 8 Cl ions

• 8 Cl are at the corners and form cubic structure.

• Body centered arrangement.

• (At the corner of the cube there will be same kind of atoms, So it is unreasonable to write it as body centered.)

CHARACTERISTICS/PROPERTIES OF IONIC or ELECTROVALENT COMPOUNDS:

1. Solubility of ionic compounds

This are soluble in the polar solvents e.g. water.

Non polar do not will have effect on ionic compound.

2. Electrical Conductivity:

Ionic compounds are poor conductor of electricity because the do not have the free electrons.

3. Room temperature:

Ionic compounds are solid at room temperature due to strong electrostatic forces and they do not have free moving electrons.

4. Non-directional:

Ionic bonds are non directional due to electrostatic forces.

5. Crystalline structure:

Definate crystalline structure due to clusters of non moving electrons.

6. Melting and boiling points:

High melting and boiling points because there are closely held ions which are forming crystal lattice.

7. Fast ionic reactions:

Some ionic reactions are fast because ions in the solvents exist as individual units.

Example:

NaCl aqueous solution added to AgNO3 solution,AgCl precipitation will be formed.

Ag + Cl --> AgCl

An electrovalent bond, also known as an ionic bond, is a type of chemical bond formed between atoms when one atom donates electrons to another atom.

Characteristics of Electrovalent bond:

Five characteristics of electrovalent compounds are high melting and boiling points, solubility in water, electrical conductivity when dissolved in water, crystal lattice structure, and strong electrostatic forces between ions. Four properties of electrovalent compounds include their brittleness, ability to conduct electricity in a molten state, the formation of crystal structures, and their often high hardness.

Formation of Electrovalent bond

The formation of an ionic bond occurs when a metal atom transfers one or more valence electrons to a nonmetal atom. For example, in the formation of sodium chloride (NaCl), sodium (Na) donates one electron to chlorine (Cl), resulting in the creation of Na+ and Cl- ions, which then attract each other through electrostatic forces.

Types of Electrovalent bond:

The two main types of ionic compounds are metal cation and nonmetal anion compounds, and nonmetal cation and nonmetal anion compounds. Ionic compounds are typically made up of metals and nonmetals, where the metal atom donates electrons to the nonmetal atom, resulting in the formation of positively charged cations and negatively charged anions.

While most ionic compounds are made up of metals and nonmetals, there are also cases where two nonmetals can form an ionic bond. In these instances, one nonmetal acts as a donor, transferring electrons to the other nonmetal, which acts as an acceptor.

Ionic bonds have several characteristics, including their strong electrostatic attraction between ions, the formation of crystal lattice structures, and their ability to conduct electricity when dissolved in water.

Examples of ionic bond:

Some common examples of ionic compounds include sodium chloride (NaCl), potassium bromide (KBr), calcium oxide (CaO), and magnesium nitride (Mg3N2).

Conclusion

In summary, electrovalent bonds, or ionic bonds, form between atoms when one atom donates electrons to another. These compounds have unique characteristics such as high melting points and solubility in water. They can be formed between metals and nonmetals or two nonmetals, resulting in the creation of cations and anions. Ionic bonds play a crucial role in the formation of various ionic compounds, many of which are essential for our everyday life and have distinct crystal lattice structures.

Ionic or Electrovalent bond (properties,/characteristics, Definition,types,structures, examples)