What occurs when metals and non-metals react may be on your mind. Ionic chemicals are created when they establish ionic bonds. An electrical force of attraction between two atoms with opposing charges is known as an ionic bond. An electron is transferred from a metal to a non-metal to form an ionic connection. Between cations and anions, an ionic connection forms. 

Cations have a positive charge, whereas anions are negative-charged ions. We will cover all of the vocabulary and ideas related to ionic compounds, so don't worry if you don't know them. This page will teach you about the ionic compound, including its production, structure, and often asked questions. 

 

What is an Ionic Compound?

You have to understand that every atom has a certain number of protons, neutrons, and electrons, making it unique. An atom is typically equal to the number of protons and electrons. An atom's proton count never varies, as doing so would result in the atom becoming a completely new element. An atom's electron count, however, is subject to vary. 

Thus, an ion might result from an atom gaining or losing an electron. The addition or removal of one electron from an atom modifies its charge since the electrons already have a net negative charge. It occurs as a result of the electron count becoming out of phase with the positively charged protons.

In the case of ions, it is true that opposites attract. Ionic compounds are made up of opposing charges—positive and negative—holding each other together through ionic bonds. It is only an ion-based molecule, as the name would imply. One atom's gain or loss is equal to the other's gain or loss. Thus, the atom forms a pair with the atom that requires its electron donated by the other atom.

Ions can be thought of as a two-bar magnet. The north and south ends of the various magnets resist one another when you try to connect them together. However, if you rotate one of the magnets, the north end and the sound end will come together quickly. Ions behave similarly; an ionic compound is created when two positive and one negative ion combine. 

Sodium Chloride, also generally known as common salt, is a well-known ionic compound.

 

Download Mathematics notes

 

Cation

A cation has a net positive charge because there are fewer electrons than protons in it. An element must lose one or more electrons in order to form a cation, and these electrons may be drawn by an element with a great affinity for them. A cation is indicated by the symbol '+'. Mg₂⁺, for instance

Anion

An anion is a particle with a net negative charge because it has more electrons than protons. An element must acquire one or more electrons in order to form an anion; these electrons might be lost by an element with a lower affinity for them. A cation is indicated by the symbol '-'. O₂⁺ is one example.

 

Properties of the Ionic Compound

Physical Properties: Because positive and negative ions are strongly attracted to one another, ionic compounds are solid and challenging to break. But when pressure is applied, they fracture, which is why they are fragile.

Melting and Boiling Points: There is a strong affinity between ionic compounds. Thus, a significant amount of energy is needed to break the ionic bonds that hold the atoms together. Ionic compounds have a higher melting and boiling point because of this.

Solubility: Ionic chemicals have the ability to dissolve in polar liquids. Among the polar solvents are formamide, methanol, and water. Moreover, ionic chemicals have a low solubility or no solubility in non-polar solvents such as hydrocarbons and chloroform.

Electric Conductivity: Ionic substances exhibit electrical conductivity when melted, but not when they are solid. You are aware that the transfer of charge from one point to another is a necessary component of electricity conduction.

Ionic substances are not electrically conductive because ions cannot travel when they are solid. Nonetheless, when ionic compounds are melted, the heat generated overcomes their electrostatic forces of attraction, allowing the compounds to conduct electricity.  

 

Ionic Compound Structure 

A polar covalent bond's ionic nature is determined by how much charge separation there is. Determining the disparity between the two atoms' electronegativity is helpful.

Δχ = χB - φA

Bond polarity and ionic nature both grow with increasing electronegativity difference.

 

Download Question Bank

 

For instance:

When chlorine and magnesium combine,

Because magnesium contains two electrons in its outermost orbit, it loses those two electrons, or two electrons from the M shell are taken out, making the outermost orbit of the L shell. It therefore creates a stable octet. With just 10 electrons and 12 protons, magnesium now has a positive charge, creating Mg₂⁺.

Comparably, the outermost orbit of chlorine has seven electrons. As a result, Cl now requires one electron to finish its stable octet. From the Mg ion, Cl receives one electron. However, since Cl only requires one electron and Mg has released two, the two Cl atoms unite with one Mg atom in this instance. As a result, Cl generates Cl⁻, a negative charge. This process produces MgCl₂.

 

Applications of ionic compounds

1. Sodium chloride, or NaCl, is an ingredient in regular tablets.

2. The toothpaste we use to clean our teeth includes sodium fluoride or NaF.

3. A ubiquitous cooking ingredient, sodium bicarbonate, or NaHCO3, is usually used to make cakes, idlis, and other baked foods.

4. Potassium phosphate, or KPO₂, is added to meals.

5. The wood is further preserved with the addition of ionic chemicals. Oxides and boric acid are often utilized.

 

CBSE Class 10 NCERT Science Topics for a Strong Foundation

Chapter Name	Metals and Non-metals
Topic Number	Topic
3.1	Properties of Metals and Non-metals
3.2	Reactivity Series
3.3	Formation and Properties of Ionic Compounds
3.4	Basic Metallurgical Processes
3.5	Corrosion and its Prevention

 

List of CBSE Class 10 Science Chapter

Chapter Number	Chapter Name
Chapter 1	Chemical Reactions and Equations
Chapter 2	Acids, Bases and Salts
Chapter 3	Metals and Non-metals
Chapter 4	Carbon and its Compounds
Chapter 5	Life Processes
Chapter 6	Control and Coordination
Chapter 7	How do Organisms Reproduce?
Chapter 8	Heredity
Chapter 9	Light – Reflection and Refraction
Chapter 10	The Human Eye and the Colourful World
Chapter 11	Electricity
Chapter 12	Magnetic Effects of Electric Current
Chapter 13	Our Environment

 

List of CBSE Class 10 Mathmetics  Chapter

Chapter Number	Chapter Name
Chapter 1	Real Numbers
Chapter 2	Polynomials
Chapter 3	Pair of Linear Equations in Two Variables
Chapter 4	Quadratic Equations
Chapter 5	Arithmetic Progressions
Chapter 6	Triangles
Chapter 7	Coordinate Geometry
Chapter 8	Introduction to Trigonometry
Chapter 9	Some Applications of Trigonometry
Chapter 10	Circles
Chapter 11	Areas Related to Circles
Chapter 12	Surface Areas and Volumes
Chapter 13	Statistics
Chapter14	Probability

 

FAQs

Que1. Which is an ionic compound?

Ans. Ionic compounds include sodium chloride (NaCl), which is the chemical name for table salt.

Que2. What are the common ionic compounds?

Ans. Common ionic compounds include sodium chloride (table salt, NaCl), calcium carbonate (chalk, CaCO3), potassium iodide (KI), magnesium sulfate (Epsom salt, MgSO4), and calcium chloride (CaCl2).

Que3. What is the ionic bond example?

Ans. An example of an ionic bond is the bond formed between sodium (Na) and chlorine (Cl) to create sodium chloride (NaCl), commonly known as table salt.

Que4. Is MgO an ionic compound?

Ans. Yes.

Que5. What are the 2 parts of an ionic compound?

Ans. Ions are the building blocks of an ionic substance. Cations are positively charged ions, whereas anions are negatively charged ions.