Smruti Bhosale

In this article, we are going to see precipitation reaction examples with detailed explanations.

• Silver nitrate AgNO₃ and Potassium chloride KCl
• Ferrous sulphate FeSO₄ and Sodium hydroxide NaOH
• Silver nitrate AgNO₃ and Sodium chloride NaCl
• Calcium chloride CaCl₂ and Potassium hydroxide KOH
• Magnesium hydroxide Mg(OH)₂ and Hydrochloric acid HCl
• Sodium hydroxide NaOH and Copper sulphate CuSO₄
• Strontium chloride SrCl₂ and Sodium sulphate Na₂SO₄
• Lead nitrate Pb(NO)₃ and Potassium iodide KI
• Ferric sulphate Fe₂(SO)₄  and Sodium hydroxide NaOH
• Potassium sulphide K₂S and Cadmium sulphate CdSO₄

The chemical reaction in which two ions combined to form one of the insoluble products in an aqueous solution that precipitated out. The precipitate is shown by the down arrow in the chemical reaction. It is used to check out elements present in the solution. It is a type of double displacement reaction.

Image Credits : Wikipedia

Also Read On: 15 Coordinate Covalent Bond Examples: Detailed Insight And Facts

Precipitation Reaction Examples

Silver nitrate and Potassium chloride

The insoluble salt or precipitate of silver chloride AgCl is a product of the reaction between Silver nitrate AgNO₃ and potassium chloride KCl. The silver chloride AgCl is a water-insoluble, solid, and white colour precipitate. The reaction occurs in an aqueous solution. So that ions get formed to replace each other and to form the salt.

Ferrous sulphate and Sodium hydroxide

The iron (ll) hydroxide Fe(OH)2 is an insoluble salt formed when ferrous sulphate FeSO4 and sodium hydroxide NaOH undergo a reaction. Sodium sulphate Na₂SO₄ is formed as a co-product. Iron (ll) hydroxide is a green coloured solid.

Silver nitrate and Sodium chloride

The insoluble salt or precipitate of silver chloride AgCl is a product of the reaction between Silver nitrate AgNO₃ and sodium chloride NaCl. Sodium nitrate is also formed as a co-product. The silver chloride AgCl is a water-insoluble, solid, and white colour precipitate. The reaction occurs in an aqueous solution. So that ions get formed to replace each other and to form the salt.

Calcium chloride and Potassium hydroxide

The calcium hydroxide Ca(OH)2 is precipitated out by the reaction of calcium chloride CaCl2 and potassium hydroxide KOH. The reaction takes place in an aqueous medium only. The calcium hydroxide Ca(OH)₂ is a water-insoluble, solid, and white colour precipitate.

Magnesium hydroxide and Hydrochloric acid

The magnesium chloride MgCl₂ is an insoluble salt formed when magnesium hydroxide Mg(OH)₂ and hydrochloric acid HCl react with each other. The magnesium chloride MgCl₂ is a colourless or white solid and water formed as a co-product.

Sodium hydroxide and Copper sulphate

The copper hydroxide Cu(OH)₂ is precipitated out when sodium hydroxide NaOH and copper sulphate CuSO₄ react with each other. The copper hydroxide Cu(OH)₂ is a blue colour solid and Sodium sulphate formed Na₂SO₄ as a co-product.

Strontium chloride and Sodium sulphate

The strontium sulphate SrSO₄ is water-insoluble salt, that precipitate out when strontium chloride SrCl₂ and sodium sulphate Na₂SO₄ react with each other. Sodium chloride NaCl is also formed as a co-product. The strontium sulphate SrSO₄ is a water-insoluble, solid, and white colour precipitate.

lead nitrate and Potassium iodide

The lead iodide Pbl₂ is precipitated out by the reaction of lead nitrate Pb(NO)₃ and potassium iodide KI. Potassium nitrate KNO₃ is formed as a co-product. The reaction required aqueous conditions. The lead iodide Pbl₂ is yellow coloured solid.

Ferric sulphate and Sodium hydroxide

The iron (lll) hydroxide Fe(OH)3 is an insoluble salt formed when ferric sulphate Fe2(SO)4  and sodium hydroxide NaOH undergo a reaction. Sodium sulphate Na₂SO₄ is formed as a co-product. Iron (lll) hydroxide is brown coloured solid.

Potassium sulphide and Cadmium sulphate

The cadmium sulphide CdS is formed by the reaction of potassium sulphide K₂S and cadmium sulphate CdSO₄. The potassium sulphate is formed as a co-product. Cadmium sulphide CdS is a yellow coloured solid, water-insoluble. The reaction required an aqueous medium.

Also Read On: Alkyl Halide Examples: Detailed Insights And Facts

Facts

• The chemical reaction in which two ions combined to form one of the insoluble products in an aqueous solution that precipitated out.
• The precipitate is shown by the down arrow in a reaction.
• It is a type of double displacement reaction.
• It affects by the type and size of ions, the concentration of an aqueous solution, pH of the solution, solubility etc.

Frequently Asked Questions:

Question: What is a precipitation reaction?

Answer: The precipitation reaction is,

The chemical reaction in which two ions combined to form one of the insoluble products in an aqueous solution that precipitated. The precipitate is shown by the down arrow in the chemical reaction. It is used to check out elements present in the solution. It is a type of double displacement reaction.

Question: What are the factors that affect the precipitation reaction?

Answer: Factors affecting precipitation reaction are,

Type and size of ions, the concentration of an aqueous solution, pH of the solution, solubility etc.

Question: What are examples of precipitation occur in nature?

Answer: The precipitation occurs in nature,

The most common examples of precipitation are Rain, Snowfall, hail, sleet, dew etc. 

Also Read On: 5+ Metallic Bond Examples: Explanation and detailed Facts

In this article, we are going to see what is combustion reaction, combustion examples in detail.

• Reaction of Methane and Oxygen
• Reaction of Ethane and Oxygen
• Reaction of Propane and Oxygen
• Reaction of Butane and Oxygen
• Reaction of Methyl alcohol and Oxygen
• Reaction of Naphthalene and Oxygen

Combustion reaction

The combustion reaction is defined as an exothermic chemical reaction that occurs between hydrocarbons (compounds having carbon and hydrogen) and atmospheric oxygen and results in the formation of carbon dioxide and a water molecule. It is also known as burning. General reaction:

Image Credits : wikipedia

Also Read On : Is O2 a triple bond: Why, How, Characteristics and Detailed Facts

Combustion examples :

Reaction of Methane and Oxygen

Methane is a most simple form of alkane that is hydrocarbons. it is found in natural gas. It has a burning property hence used as fuel. Methane burns in a blue flame in presence of air. When methane reacts with oxygen it results in the formation of carbon dioxide and water. As shown in above figure.

Reaction of Ethane and Oxygen

Ethane is a simple form of alkane containing two carbon atoms and six hydrogens that are hydrocarbons. It has a burning property hence used as a gaseous fuel. Ethane burns in a blue flame in presence of air. When ethane reacts with oxygen it results in the formation of four molecules carbon dioxide and six water molecules.

Reaction of Propane and Oxygen

Propane is a simple form of alkane containing three carbon atoms and seven hydrogens that are hydrocarbons. It has a burning property hence used as a gaseous fuel. It is used in fireplaces, some types of cookstoves and gas grills. Propane burns in a blue flame in presence of air. When propane reacts with oxygen it results in the formation of six molecules of carbon dioxide and seven water molecules.

Reaction of Butane and Oxygen

Butane is a simple form of alkane containing four carbon atoms and ten hydrogens that are hydrocarbons. It has a burning property hence used as fuel. It is usually found in a lighter. Butane burns in a blue flame in presence of air. When butane reacts with oxygen it results in the formation of eight molecules of carbon dioxide and ten water molecules.

Reaction of Methyl alcohol and Oxygen

Methyl alcohol also termed as wood alcohol, is a simple form of alcohol-containing one carbon atom, one oxygen and four hydrogens that are hydrocarbons. Methyl alcohol burns in a pale blue flame in presence of air. When methyl alcohol reacts with oxygen it results in the formation of two molecules of carbon dioxide and four water molecules.

Reaction of Naphthalene and Oxygen

Naphthalene, is a simple form of polycyclic aromatic hydrocarbon, containing ten carbon atoms, eight hydrogens that are hydrocarbons. Naphthalene burns in a yellow flame in presence of air. When naphthalene reacts with oxygen it results in the formation of ten molecules of carbon dioxide and four water molecules.

Also Read On: N2 polar or nonpolar: Why, How, Characteristics, And Detailed Facts

Frequently Asked Questions:

Question : Why oxygen is needed in combustion?

 Answer : The oxygen is required for the combustion because,

Oxygen reacts with substances (fuel or combustible materials)   by releasing a high amount of energy. This energy is in the form of light and heat or fire. In the combustion reaction oxygen acts as a reactant and supports burning. Hence oxygen is required for the combustion reaction.

Question : What is the difference between complete and incomplete combustion?

 Answer : The difference between complete and incomplete combustion are,

Question : What are the types of combustion?

 Answer : Combustion reactions are classified as,

Complete combustion – The hydrocarbons burned in presence of oxygen or air produce only carbon dioxide and water.

Incomplete combustion – The hydrocarbons burns in presence of oxygen or air produce not only carbon dioxide and water.

Smoldering reaction – It is a type of incomplete reaction, flame-less and slow.

Spontaneous reaction- It is shown by self-heating substances.

Rapid reaction- It is the fast reaction with the evolution of a large amount of light and heat energy.

Turbulent reaction – It shows a turbulent flame.

Micro combustion- Occur in a very small amount.

Question : What is a combustion reaction?

 Answer : The combustion reaction is,

The combustion reaction is defined as an exothermic chemical reaction that occurs between hydrocarbons (compounds having carbon and hydrogen) and atmospheric oxygen and results in the formation of carbon dioxide and a water molecule. It is also known as burning.

Also Read On : CH2CL2 Lewis Structure Why,How,When And Detailed Facts

In this article, we are going to see what are acid base reaction examples with their explanation in detail.

• Hydrochloric acid and Sodium hydroxide
• Hydrobromic acid and potassium hydroxide
• Hydrochloric acid and Ammonia
• Hydrochloric acid and potassium hydroxide
• Hydrochloric acid and magnesium hydroxide
• Hydrochloric acid and Ferric oxide
• Nitric acid and Barium hydroxide
• Phosphoric  acid and Calcium hydroxide
• Sulphuric acid and strontium hydroxide
• Hydrochloric acid and strontium hydroxide

The acids are the chemical species that give proton H+ while bases are the chemical species that accept a proton.

When base and acid undergo chemical reaction gives salt and water as a product of their reaction.

Also Read On: 5+ Metallic Bond Examples: Explanation and detailed Facts

Acid Base Reaction Example

Hydrochloric acid and Sodium hydroxide

Hydrochloric acid is a strong acid. It dissociates completely in an aqueous solution and gives arise to H+ and Cl-. The sodium hydroxide is a strong base, it dissociates in Na+ and OH-. During the course of the reaction Na+ combined with Cl- to form salt NaCl sodium chloride and H+ combined with OH- to form water.

Hydrobromic acid and potassium hydroxide

Hydrobromic acid is a strong acid. It dissociates completely in an aqueous solution and produces H+ and Br-. The potassium hydroxide is a strong base, it dissociates in K+ and OH-. During the course of the reaction K+ combined with Br- to form salt KBr, potassium bromide, and H+ combined with OH- to form water.

Hydrochloric acid and Ammonia

Hydrochloric acid dissociates completely in an aqueous solution and produces H+ and Cl-. It is a strong acid. Ammonia is not a strong base. This reaction does not follow acid-base criteria due to the only formation of salt taking place, not water. Hydrochloric acid and Ammonia react to form Ammonium chloride.

Hydrochloric acid and potassium hydroxide

Hydrochloric acid is a strong acid, that dissociates completely in an aqueous solution and gives arise to H+ and Cl-. The potassium hydroxide is a strong base, it dissociates in K+ and OH-. During the course of the reaction K+ combined with Cl- to form salt KCl potassium chloride and H+ combined with OH- to form water.

Hydrochloric acid and magnesium hydroxide

Being a strong acid, Hydrochloric acid dissociates to form H+ and Cl-. The magnesium hydroxide acts as the base. It dissociates to form Mg⁺² magnesium ion and hydroxide ion OH-.  In the reaction, magnesium chloride is formed along with water.

Hydrochloric acid and Ferric oxide

Hydrochloric acid dissociates completely in an aqueous solution and produces H+ and Cl-. It is a strong acid. Ferric oxide dissociates into Fe⁺³ and hydroxide ion OH-. Ferric chloride is the product given by the reaction of ferric oxide and hydrochloric acid.

Nitric acid and Barium hydroxide

Nitric acid dissociates into H+ and NO3- ions in the aqueous solution. Barium hydroxide dissociates Ba⁺² and OH-. During the reaction of nitric acid and barium hydroxide, the barium nitrate is formed as a product.

Phosphoric  acid and Calcium hydroxide

Phosphoric acid is a strong acid. It dissociates in an aqueous solution and produces hydronium H+, PO₄– ions. Calcium hydroxide acts as a base, dissociates in an aqueous solution to form Ca+ and OH-. The salt calcium phosphate and water are the results of the reaction.

Sulphuric acid and strontium hydroxide

Sulphuric acid dissociates completely in an aqueous solution and produces H²⁺ and SO₄²-. It is a strong acid. Strontium hydroxide is a base. The salt, strontium sulfate is formed with water as a product of the reaction between sulphuric acid and strontium hydroxide.

Hydrochloric acid and strontium hydroxide

Being a strong acid, Hydrochloric acid dissociates to form H+ and Cl-. Strontium hydroxide dissociates to form Sr+ and OH-. H+ and OH- linked to form water as well as strontium ion and chloride ion linked to form strontium chloride.

Also Read On: Is HBr Ionic or Covalent : Why? How, Characteristics and Detailed Facts

Frequently Asked Questions:

Question : What is a strong acid?

Answer : The strong acid is defined as,

The chemical species completely dissociates into an aqueous solution and produces hydronium ion or proton H+. example, sulphuric acid, nitric acid, hydrochloric acid, phosphoric acid etc.

Question : What are the examples of strong bases?

Answer : The examples of strong bases are,

Sodium hydroxide, potassium hydroxide, strontium hydroxide, lithium hydroxide, etc. dissociates completely in an aqueous solution to form hydroxide ion.

Question : What are the examples of weak acids and weak bases?

Answer: The examples of weak acids and weak bases are,

Weak acids: Partially dissociates in an aqueous solution to form protons. Eg. Benzoic acid, formic acid, oxalic acid etc.

Weak bases: Partially dissociates in an aqueous solution to form hydroxide ion. Eg. Ammonia, copper hydroxide, aluminum hydroxide, etc.

Question : What are the reaction of Phosphoric acid and Calcium hydroxide?

Answer: The reaction of Phosphoric acid and Calcium hydroxide,

Phosphoric acid is a strong acid. It dissociates in an aqueous solution and produces hydronium H+, PO₄– ions. Calcium hydroxide acts as a base, dissociates in an aqueous solution to form Ca+ and OH-. The salt calcium phosphate and water are the results of the reaction.

Also Read On: Is O2 a triple bond: Why, How, Characteristics and Detailed Facts

In this article, we are going to see, what redox reaction example is with their explanation in detail.

• Reaction of Iron and copper sulphate
• Formation of Hydrogen fluoride
• Reaction of Zinc and copper sulphate
• Reaction of Iron and Hydrogen Peroxide
• Reaction of Copper sulphate and potassium iodide
• Reaction of Hydrogen sulphide and chlorine
• Reaction of Arsenous acid and Bromate
• Reaction of Potassium permanganate and Ferrous sulphate
• Reaction of Manganese ion and Chlorine trioxide
• Reaction of Hydrogen peroxide and Perchloric acid

The word redox itself shows that there are two processes involved in the reaction. Those are Oxidation and Reduction and are going on at the same time during the course of the reaction.

Oxidation: During the reaction, some of the atoms change their oxidation number or loss of electrons takes place or there is the addition of an electronegative element or there is a gain of oxygen or loss of hydrogen, then it is called as oxidation.

Reduction: During the reaction, the gain of electrons takes place by some of the atoms or addition of electropositive element or gain of hydrogen or loss of oxygen.

Also Read On: 4 nonpolar covalent bond examples: Detailed Insights And Facts

Redox Reaction Example

Reaction of Iron and copper sulphate

In the reaction of iron and copper sulphate, the oxidation number changes from 0 to +2. Shows increases in the oxidation number of ferrous. The decrease in oxidation number is shown by copper from +2 to 0. It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants.

Formation of Hydrogen fluoride

In the above reaction, the oxidation reaction is shown by hydrogen as its oxidation number changes from 0 to +1 on the other hand reduction reaction is shown by fluorine as its oxidation number changes from +1 to 0. It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants.

Reaction of  Zinc and copper sulphate

During the reaction of Zinc and copper sulphate, the oxidation reaction is shown by zinc as its oxidation number changes from 0 to +2 on the other hand reduction reaction is shown by copper as its oxidation number changes from +2 to 0. The oxidation number of reactant species increases and others decreases therefore it’s a redox reaction.

Reaction of  Iron and Hydrogen Peroxide

In the above reaction, the oxidation number increases from +2 to +3, or loss of electrons takes place, hence its oxidation, shown by iron. The oxidation number decreases from 0 to +1 or gain of electrons taking place, is reduction shown by hydrogen peroxide.  

Reaction of  Copper sulphate and potassium iodide

In the reaction of Copper sulphate and potassium iodide, oxidation and reduction take place at the same time it is a redox reaction. Oxidation half-reaction is shown by iodide while reduction half-reaction is shown by copper.

Reaction of  Hydrogen sulphide and chlorine

During the reaction of Hydrogen sulphide and chlorine, the loss of hydrogen is called oxidation, is shown by H2S and gain of hydrogen is called reduction is shown by chlorine. As the reduction and oxidation reactions take place at the same time it is considered as a redox reaction.

Reaction of  Arsenous acid and Bromate

In the above reaction the oxidation no, of As changes by +3 to +5 and the oxidation number of Br changed from +5 to -1. It is a redox reaction as the Oxidation number of one reactant species increases while the other decreases.

Reaction of  Potassium permanganate and Ferrous sulphate

In the reaction of Potassium permanganate and Ferrous sulphate, the oxidation number changes from +2 to +3. Shows increases in the oxidation number of ferrous. The decrease in oxidation number is shown by manganese from +7 to +2.

Reaction of  Manganese ion and Chlorine trioxide

This reaction required an acidic medium. Oxidation number changes from +2 to +4 of one reactant species while others decrease from +5 to +4. It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants.

Reaction of  Hydrogen peroxide and Perchloric acid

In the above reaction oxidation number changes from -1 to 0. It shows an increase by 1. The oxidation number of chlorine trioxide is decreasing from +7 to +3 It is a redox reaction because the Oxidation number shows an increase and decrease of the reactants. This reaction required an acidic medium.

Also Read On: Is O2 a triple bond: Why, How, Characteristics and Detailed Facts

Frequently Asked Questions:

Question: What are oxidizing agents?

Answer: The oxidizing agents are,

A substance or a reagent that causes oxidation of another substance or species and itself undergoes reduction are termed an oxidizing agent or oxidant. It is an electron acceptor species.

Question: What are reducing agents?

Answer: The reducing agents are,

A substance or a reagent which cause the reduction of another substance or species and itself undergoes oxidation are termed a reducing agent or reductant. It is an electron donor species.

Question: What are the examples of oxidizing and reducing agents?

Answer: The examples of oxidizing and reducing agents are as follows,

Oxidizing agents:  O₂, O₃, H₂SO₄, HNO₃, KMnO₄, H₂O₂ etc.

Reducing agents: LiH, LiAlH_4, NaH, CaH₂ etc.

Question: What are the types of redox reactions?

Answer: The four types of redox reactions :

Combination reactions

Disproportion reactions

Decomposition reactions

Displacement reactions.

Also Read On: Is HBr Acid : Weak or strong, Why, How and Detailed Facts

In this article, we are going to see about hydrogen bonding, intermolecular hydrogen bond examples with facts in detail.

Following are the examples of intermolecular hydrogen bond.

• Alcohols
• Ammonia (NH₃)
• Carboxylic Acid
• Hydrogen fluoride (HF)
• Water (H₂O)

The term hydrogen bond is used when there is a covalent bond present between the hydrogen atom and an electronegative atom, another electronegative atom having lone pair attracts an electropositive hydrogen atom by electrostatic dipole-dipole interactive force. The covalent bond is represented as a dashed line and the hydrogen bond is shown by a dotted line.

Hydrogen bonding shows two types of bonding:

1. Intermolecular hydrogen bonding: When the hydrogen bond is formed in between more than one molecule.
2. Intramolecular hydrogen bonding: The hydrogen bond is present in the identical molecule.

Intermolecular hydrogen bond

When a hydrogen bond is present between more than one different molecule, it is called an intermolecular hydrogen bond. The electronegative atoms like oxygen, fluorine, nitrogen, etc. formed a covalent bond with the electropositive hydrogen atom. Due to the presence of an electrostatic dipole-dipole interactive force, the compounds having this type of hydrogen boding show high melting and boiling point, solubility

Also Read On: 4 Hydrogen Bond Examples : Detailed Insights And Facts

Intermolecular hydrogen bond examples

Alcohols

In organic chemistry, alcohols have –OH, as a functional group. The hydrogen atom formed a covalent bond with the oxygen atom. The oxygen atom is electronegative having lone pair of electrons that has a partial negative charge. Which attracts the electropositive hydrogen atom of another alcohol molecule. An example of the intermolecular hydrogen bond is shown in the figure below.

Ammonia (NH₃)

In the Ammonia molecule, The electronegative nitrogen atom linked with three hydrogen atoms . The nitrogen atom has lone pair hence it acquires a partial negative charge and attracts an electropositive hydrogen atom of another ammonia molecule with the help of electrostatic dipole-dipole interaction force. Thus, the intermolecular hydrogen bond get formed as shown in figure below.

Carboxylic Acid

In the carboxylic acid molecule, the carbon atom is bonded with oxygen and hydroxide group, having –COOH as a functional group. Both the oxygen atoms have lone pairs. They are electronegative in nature, acquire a partial negative charge. They attract hydrogen atoms having a partial positive charge of another carboxylic acid molecule and forms intermolecular hydrogen bonds.

Hydrogen fluoride (HF)

In the hydrogen fluoride (HF) molecule, the fluorine atom is highly electronegative compared to the electropositive hydrogen atom. The hydrogen atom had a partial positive charge on the other hand fluorine atom had a partial negative charge. It attracts the hydrogen atom of another H₂S molecule and forms an intermolecular hydrogen bond.

Water (H₂O)

In a water (H₂O) molecule, the oxygen atom is linked with hydrogen atoms. The hydrogen is more electropositive than Oxygen, had a partial positive charge, while oxygen had a partial negative charge. Due to the presence of dipole-dipole interactive force, it attracts hydrogen atoms, having a partial positive charge of the separate water molecule. Hence water has a high boiling point.

Also Read On: 5 Polar Covalent Bond Examples: Detailed Insights And Facts

Facts

1. Hydrogen bond forms due to the dipole-dipole interactive force of attraction.
2. Two types: 1)Intermolecular hydrogen bonding         2)Intramolecular hydrogen bonding.
3. Intermolecular hydrogen bonding: when the hydrogen bond is formed in between more than one molecule.
4. Intramolecular hydrogen bonding: The bond exits in the identical molecule.
5. Hydrogen bonding is not stronger in comparison to covalent and ionic bonding.
6. The compounds which have hydrogen bonding, show high melting and boiling points.
7. The compounds with hydrogen bonds show properties like surface tension, solubility, viscosity etc.

Also Read On: 15 Coordinate Covalent Bond Examples: Detailed Insight And Facts

Frequently Asked Questions:

1) Question: What is hydrogen bonding?

Answer: The term hydrogen bonding is used,

When there is a covalent bond present between the hydrogen atom and an electronegative atom, another electronegative atom having lone pair attracts an electropositive hydrogen atom by electrostatic dipole-dipole interactive force.

2) Question: Do hydrogen bonds share electrons?

Answer: No, hydrogen bonds don’t share electrons.

The electronegative atoms having a partial negative charge attract electropositive hydrogen atoms. Both oppositely charged atoms move closer to each other but the sharing of electrons does not take place.

3) Question: How do hydrogen bond forms in water?

Answer: The hydrogen bond is present in the H₂O molecule,

In a water (H₂O) molecule, the oxygen atom is linked with hydrogen atoms. The hydrogen is more electropositive than Oxygen, had a partial positive charge, while oxygen had a partial negative charge. Due to the presence of dipole-dipole interactive force, it attracts hydrogen atoms, having a partial positive charge of the separate water molecule. Hence water has a high boiling point.

4) Question: What is the intermolecular hydrogen bond?

Answer: The intermolecular hydrogen bond is,

When a hydrogen bond is present between more than one different molecule, it is called an intermolecular hydrogen bond The electronegative atoms like oxygen, fluorine, nitrogen, etc. formed a covalent bond with the electropositive hydrogen atom. Due to the presence of an electrostatic dipole-dipole interactive force, the compounds having this type of hydrogen boding show high melting and boiling point, solubility.

In this article, we are going to see is covalent stronger than ionic bond, why, how and detailed facts.

The ionic bond is not as strong as a covalent bond. The covalent bond is formed by the sharing of electrons while the ionic bond forms when there is a strong force of attraction present between two different ions. Since the bond strength depends upon many conditions and factors.

Covalent bond

When two atoms share their electrons with each other to complete octet or stable electronic configuration then this type of bonding is term as covalent bonding.

Three kinds of covalent bonds:

Single bond: Only one bond exists between two atoms. It consists of a sigma bond. Axial overlapping of orbitals leads to form a sigma bond.

Double bond: Two bonds exist between two atoms. It includes a sigma and a pi bond. Lateral overlapping of orbitals leads to form a pi bond.

Triple bond: There are three bonds that exist between two atoms. It includes two pi bonds and one sigma bond.

Image Credits: wikipedia

Read More On: 15 Coordinate Covalent Bond Examples: Detailed Insight And Facts

Ionic bond

When there is a strong force of attraction present between two different ions that are positively charged cation and negatively charged anion.  Usually, the ionic bond exists between metal and non-metals.

Image Credits: wikipedia

Read More On: 10 Ionic Bond Examples: Explanation And Detailed Facts

Metallic bond

When a strong force of attraction is present between negatively charged moving electrons present in the crystal lattice and positively charged metal ions, then it is termed metallic bonding.

Image Credits: wikipedia

Read More On: 5+ Metallic Bond Examples: Explanation and detailed Facts

Why is covalent stronger than ionic?

The ionic bond is not as strong as a covalent bond because,

The covalent bond is made up of sharing of electrons. There is an atomic orbital overlapping occurring in two bond-forming atoms and a sigma bond is formed.

The bond length is small, hence the influence of attractive force is greater and atoms get closer with each other. The single and double bonds are weaker than triple bonds and required high energy to cleave the bond.

The covalent bond can be formed between atoms having the same or different electronegativity values. There is a direct sharing of electrons.

Whereas, the ionic bond is formed when there is a strong force of attraction present between two different ions that are positively charged cation and negatively charged anion. Hence there is an electronegativity difference.

The polarity of the bond decreases as an increase in covalent character with bond strength. Therefore an ionic bond is not strong as that of a covalent bond.

Are polar covalent bonds stronger than ionic bonds?

Yes, Polar covalent bonds are stronger compared to ionic bonds.

When a covalent bond is formed by unequal sharing of electrons, atoms acquire partial positive and negative charges. Then it is defined as a polar covalent bond. Though it consists of polarity in bond, it has a more covalent character compared to an ionic bond.

As covalent character increases bond strength also increases, hence polar covalent bonds are stronger than ionic bonds.

Read More On: 5 Polar Covalent Bond Examples: Detailed Insights And Facts

Is covalent is stronger than metallic bonds?

Yes, the covalent bond is stronger compared to the metallic bond.

When atoms share their electrons with each other, a covalent bond is formed. There is an atomic orbital overlapping, the bond length is small, great attractive force, atoms are closer and has a covalent character.

On the other hand, when a strong force of attraction is present between negatively charged moving electrons present in the crystal lattice and positively charged metal ions, the metallic bond is formed. The atomic orbital overlapping does not take place, comparatively less attractive force and atoms are not close to each other.

Why covalent bond is stronger than a metallic bond?

When two atoms share their electrons with each other to complete octet or stable electronic configuration then this type of bonding is term as covalent bonding. When a strong force of attraction is present between negatively charged moving electrons present in the crystal lattice and positively charged metal ions, then it is termed metallic bonding.

The covalent bond is formed by sharing of electrons. There is an atomic orbital overlapping occurring in two bond-forming atoms and a sigma bond is formed.

The bond length is small, hence the influence of attractive force is greater and atoms get closer with each other. The single and double bonds are weaker than triple bonds and required a high amount of energy to cleave the bond.

But in metallic bonding, positively charged metal ions formed bonds with negatively charged moving electrons. These mobile electrons are exits in a space lattice of a crystal. Hence the influence of attractive force is less and atoms are not close to each other. The atomic orbital overlapping does take place.

Hence metallic bond is weaker than a covalent bond.

Factors influencing Bond strength

• Number of electrons
• Bond length
• Bond energy
• Orbital overlapping
• Covalent character
• Atomic size

Frequently Asked Questions:

• Question: Which is the strongest bond?

Answer: The covalent bond is the strongest bond.

The covalent bond is consists of sigma bonding which is considered the strongest bond among all other chemical bonds.

• Question: Why is covalent stronger than ionic bonds?

Answer: The covalent bond is stronger than the ionic bond.

The covalent bond is formed by sharing of electrons. There is an atomic orbital overlapping occurring in two bond-forming atoms and a sigma bond is formed. The bond length is small, hence the influence of attractive force is greater and atoms get closer. On the other hand, the ionic bond is formed when there is a strong force of attraction present between two oppositely charged ions. Hence there is an electronegativity difference. The polarity of the bond decreases as an increase in covalent character with bond strength. Hence covalent bond is stronger than an ionic bond.

• Question: What is the order of bond strength of chemical bonds?

Answer: The order of bond strength of chemical bonds is as follows,

Covalent bond > Polar covalent bond > Ionic bond > Metallic bond.

In this article, we are going to see what is double replacement reaction examples in detail.

• Reaction of sodium bicarbonate and acetic acid
• Reaction of Hydrofluoric acid and sodium hydroxide
• Reaction of Barium chloride and sodium sulfate
• Reaction of Silver nitrate and sodium chloride
• Reaction of Potassium iodide and lead nitrate
• Reaction of Barium hydroxide and sulphuric acid
• Reaction of Hydrochloric acid and sodium sulfide
• Reaction of Hydrochloric acid and sodium hydroxide
• Reaction of Potassium carbonate and ammonium iodide
• Reaction of Sodium hydroxide and cesium sulfide

When two complex molecules react with each other resulting in the formation of other complex molecules, in which positive ions and negative ions replace each other, then it is termed as double replacement reaction. ‘Metathesis’ and ‘double displacement reaction’ are other terms referred to as double replacement reactions. As the name suggested both cation and anion show displacement in the reaction.

The double replacement reactions are of three types:

Gas formation: The reactions in which the resultant product is in a gas state.

Precipitation: The water-soluble ionic compounds undergo a reaction to form a water-insoluble product then it is termed as a precipitation reaction.

Neutralization: Usually acids and bases show this type of reaction The salt and water are formed as products by the reaction of acid – base.

Also Read On: 15 Coordinate Covalent Bond Examples: Detailed Insight And Facts

Double replacement reaction examples

Reaction of sodium bicarbonate and acetic acid

The sodium bicarbonate reacts with acetic acid it resulting in the formation of carbonic acid sodium acetate and carbonic acid. As positively charged hydrogen, sodium ions and negatively charged carbonic and carboxyl group exchange in the products. Hence, an example of a double replacement reaction.

Reaction of Hydrofluoric acid and sodium hydroxide

The hydrofluoric acid and sodium hydroxide undergo reaction to form sodium fluoride along with water. The cation and anion show replacement with other identically charged ions. It is a neutralization reaction.

Reaction of Barium chloride and sodium sulfate

In the reaction of Barium chloride and sodium sulfate, positively charged Barium and sodium ion replaces each other on the other hand negatively charged chloride and sulfide ions replace each other.

Reaction of Silver nitrate and sodium chloride

The Silver nitrate and sodium chloride undergo a reaction to form sodium nitrate along with silver chloride. The cation and anion show replacement with other identically charged ions. It is a precipitation reaction, as a water-insoluble precipitate of silver chloride formed.

Reaction of Potassium iodide and lead nitrate

The potassium iodide and lead nitrate undergo a chemical reaction and potassium nitrate and lead iodide are formed as products. As positively charged potassium, lead ions and negatively charged nitrate, iodide ions are exchanged in the products.

Reaction of Barium hydroxide and sulphuric acid

The barium hydroxide and sulphuric acid undergo a reaction to form barium sulfate along with water. The cations barium and hydronium ion replace each other as well as anions hydroxide and sulfide shows replacement.

Reaction of Hydrochloric acid and sodium sulfide

The hydrochloric acid reacts with aqueous sodium sulfide it resulting in the formation of hydrogen sulfide gas and sodium chloride. As positively charged hydrogen, sodium ions and negatively charged chloride, sulfide ions exchange in the products.

Reaction of Hydrochloric acid and sodium hydroxide

The salt and water form as a product when acid and base undergo a chemical reaction. The positively charged ions of one molecule form a bond with negatively charged ions of another molecule and vice versa. Sodium chloride and water are formed by the reaction of hydrochloric acid and sodium hydroxide.

Reaction of Potassium carbonate and ammonium iodide

In the reaction of potassium carbonate and ammonium iodide, positively charged potassium and ammonium ion replace each other on the other hand negatively charged carbonium and iodide replace each other.

Reaction of Sodium hydroxide and cesium sulfide

The Sodium hydroxide reacts with aqueous cesium sulfide resulting in the formation of sodium sulfide gas and cesium hydroxide. As positively charged cesium, sodium ions and negatively charged hydroxide, sulfide ions exchange in the products.

Also Read On: 10 Ionic Bond Examples: Explanation And Detailed Facts

Frequently asked questions:

1) Question: What is double replacement reaction?

Answer: A double replacement reaction is defined as,

When two complex molecules react with each other resulting in the formation of other complex molecules, in which positive ions and negative ions replace each other, then it is termed as double replacement reaction. Metathesis and double displacement reaction are other terms that are used for double replacement reaction. As the name suggested both cation and anion show displacement in the reaction.

2) Question: What are the types of double replacement reactions?

Answer: The types of double replacement reactions are,

Gas formation: The reactions in which the resultant product is in a gas state.

Precipitation: The water-soluble ionic compounds undergo a reaction to form a water-insoluble product then it is termed as a precipitation reaction.

Neutralization: Usually acids and bases show this type of reaction. The salt and water are formed as products by the reaction of the acid – base.

3) Question: How do you know if a double replacement reaction will occur?

Answer: To figure out whether a double replacement reaction will occur,

The double replacement reaction occurs when ionic compounds react in aqueous solutions resulting in the formation of other ionic compounds. In this reaction, ions show replacement. By tracking the positions of cations and anions in reactants and products one can find whether the double displacement reaction occurs or not.

4) Question: Can a double displacement reaction takes place when the products are highly soluble?

Answer: The double replacement reaction does not take place.

The double displacement reactions can be performed only in aqueous solutions. It requires compounds having partial solubility which leads to forming ions. So that cations and anions can replace each other. Hence when the products are highly soluble, a double displacement reaction can not take place.

Also Read On: 5+ Double Bond Examples: Detailed Insights And Facts

In this article, we are going to see what are the examples of ionic covalent bond types, facts and detailed insights.

• Sodium hydroxide NaOH
• Sodium nitrate NaNO₃
• Ammonium chloride NH₄Cl
• Calcium carbonate CaCO₃
• Potassium cyanide KCN
• Potassium nitrite KNO₂
• Potassium sulphate K₂SO₄
• Barium cyanide Ba(CN)₂

Some compounds contain both ionic bonds and covalent bonds in their molecular structure. They are also termed polyatomic compounds. To attain stabilization some molecules form more than one type of bonding. Here we are going to see some molecules which are ionic covalent bond types examples .

Ionic Bond

An Ionic bond is defined as two different ions, cations and anions attract each other and form a bond. Electrovalent bond is another term used for ionic bonding. Ionic compounds show this type of bonding in their atomic structure. This type of bond is formed in Metal and Non-metals.

Characteristics

• An electrovalent bond is another term attributed to the ionic bond.    
• A strong electrostatic force of attraction is used to combine anions and cations together.
• They have a high melting point.
• They are a good conductor of electricity in a molten state or dissolved in solvents, but in the solid state, they are a bad conductor of electricity.
• They can be dissolved in polar solvents and did not dissolve in non-polar solvents.

Read More On : 10 Ionic Bond Examples: Explanation And Detailed Facts

Covalent bond

The covalent bond is determined as two atoms sharing their equal valence electrons to gain a stable electronic configuration. Covalent compounds contain this kind of bonding in their molecular structures.

Characteristics

• The bond is formed between the same or different atoms.
• It is further classified based on the electronegativity of atoms as a polar and non-polar covalent bond.
• They have a property of low melting and boiling point.
• They are unable to conduct electricity.
• They are can be dissolved in solvents that are non-polar and do not dissolve in water which is a polar solvent.

Read More On : 4 Single Covalent Bond Examples : Detailed Insights And Facts

Ionic Covalent bond types Examples

Sodium hydroxide NaOH

Sodium hydroxide, Oxygen atom and Hydrogen atom show the formation of a covalent bond by sharing electrons. Hydroxide ion has a negative charge and sodium ion has a positive charge. These two ions OH^– and Na⁺ attract each other forms an ionic bond.

Sodium nitrate NaNO₃

In Sodium nitrate, the Nitrogen atom forms a bond with three oxygen atoms. The bond formed between Nitrogen and oxygen is termed as a covalent bond. Nitrite ion NO₃ has a negative charge while sodium ion Na has a positive charge. Na⁺ and NO₃^– ions form ionic bonds. Hence this is an example of a molecule having an ionic and covalent bond.

Ammonium chloride NH₄Cl

In the Ammonium chloride molecule, the Nitrogen atom forms four covalent bonds with four different hydrogen atoms. NH₄ acquires a positive charge. This ammonium ion combines with negatively charged chloride ion. NH₄⁺ and Cl^– ions form an ionic bond.

Calcium carbonate CaCO₃

In Calcium carbonate, the covalent bonds form between the three Oxygen atoms and a Carbon atom. Carbonate ions acquire a negative charge and combine with positively charged Calcium metal ions. Ca⁺ and CO₃^– form an ionic bond.

Potassium cyanide KCN

In Potassium cyanide, the Carbon atom is combined with the Nitrogen atom covalently. The carbon atom and Nitrogen atom shares three electrons with each other. Cyanide CN is more electronegative than potassium. It acquires a negative charge. Potassium has a positive charge. K⁺ and CN^– form an ionic bond.

Potassium Nitrite KNO₂

In the Potassium Nitrite molecule, the Nitrogen atom forms two covalent bonds with two different oxygen atoms. Positively charge potassium ion K⁺ and negatively charged nitrate ion NO₂^– forms an ionic bond. KNO₂ has both ionic and covalent bonding.

Potassium Sulphate K₂SO₄

In Potassium Sulphate, the Sulphur atom shares electrons with four Oxygen atoms. Sulphur forms an ionic bond with Potassium metal ions. Negatively charged SO₄^-2 ion and Positively charged K⁺² ion forms bond.

Barium cyanide Ba(CN)₂

In Barium cyanide, the Carbon atom and Nitrogen atom share three electrons with each other. Negatively charged cyanide ion forms an ionic bond with Positively charged Barium ion. CN^– and Ba⁺² form ionic bonds.

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Facts

• Chemical bonding is consists of both ionic as well as covalent bonding.
• Both the bonds provide stability to the compounds.
• Some compounds are completely soluble in water and some of them are sparingly soluble in water.
• Most of these compounds are salts.
• They can conduct electricity in a molten state.
• In an aqueous solution, they separated to form cations and anions.

Frequently asked questions:

Question: How is KCN ionic and covalent?

Answer: KCN has both ionic and covalent bonds.

In Potassium cyanide, the Carbon atom is combined with the Nitrogen atom covalently. The carbon atom and Nitrogen atom shares three electrons with each other. Cyanide CN is more electronegative than potassium. It acquires a negative charge. Potassium has a positive charge. K⁺ and CN^– form an ionic bond.

Question: NH4S has ionic and covalent bonds?

Answer: NH₄S has both bonds.

In ammonium sulphide, nitrogen is combined with four hydrogen atoms covalently. The electronegativity difference leads to form an ionic bond between ammonium ion and sulphur. Hence NH₄S not only have an ionic but also have covalent bonding.

Question: CaCO3 is ionic or covalent?

Answer: CaCO₃ is considered an ionic compound.

In Calcium carbonate, the three oxygen atoms form three covalent bonds with a Carbon atom. Carbonate ions acquire a negative charge and combine with positively charged Calcium metal ions. Ca⁺ and CO₃^– form an ionic bond.

In this article, we are going to see about metallic bonding, its characteristics and facts along with some metallic bond examples in detail.

The metallic bond can be described as the attractive force present between negatively charged mobile electrons and positively charged metallic ions. This force of attraction is used to hold the metal atoms together in the metallic crystal. Metallic bond examples are:

• Sodium
• Aluminium
• Magnesium
• Copper
• Iron

In one of the geometrical arrangements like body central cubic arrangement, hexagonal close-packed or face central cubic close-packed arrangements, metal consists of positive ions. Negatively charged delocalized electrons hold positively charged ions together in the crystal lattice. Hence, positive and negative charges get balanced.

According to electron cloud theory, the metallic bond is electrostatic forces of attraction between positively charged metal ions embedded in a sea of negatively charged mobile electrons. As shown in a figure.

Image Credits : wikimedia

Characteristics of metallic bond

• Metals can conduct heat through them. When one end of the metal is heated, mobile electrons absorb heat energy and move rapidly towards another end hence metal shows thermal conductivity.
• Metals are also good conductors of electricity as free electrons are present which carries current.
• Metals are opaque and they also have metallic clusters.
• Metals are ductile and malleable.
• Metals show the property of luster, as mobile electrons absorb and emit visible light radiations.
• The metallic bond occurs in the solid state of matter.
• Metals required high temperatures to cleave bonds between them, hence having high melting points and boiling points.

Read more on: 5+ Double Bond Examples: Detailed Insights And Facts

Metallic bond Examples

Sodium (Na)

A sodium atom has one electron in its valence shell. When more than one sodium atom get arranged in a crystal lattice (bcc), Electrons present in the outermost shell share interstitial space with another sodium atom, molecular orbital get formed. The valence electrons which are present in the outermost shell of the atom get distributed in the space lattice of the metal. This is a metallic bond example.

 The positively charged Sodium metal ions and negatively charged electrons get bonded together forming metallic bonds.

Image Credits : chemistrylearner

Aluminium (Al)

The aluminium atom has three electrons in its valence shell. When Aluminium atoms get arranged in a crystal lattice (fcc), electrons present in the outermost shell shares interstitial space with other aluminium atoms and molecular orbitals get formed. These electrons are delocalized in space lattice.  As the number of valence electrons increases the more free electrons get available. This is a metallic bond example. The metallic bond formed between positively charged aluminium metal ions and electrons.

Image Credits: chemistrylearner

Magnesium (Mg)

The magnesium atom has two valence electrons. When magnesium atoms get arranged in a crystal lattice (hcp), electrons present in the valence shell shares space with other Magnesium atoms and molecular orbitals get formed. The electrons which are present in the valence shell are free to move in the crystal. The metallic bond formed between positively charged Magnesium metal ions (2⁺) and electrons. hence it is a metallic bond example.

Image Credits: chemistrylearner

Copper (Cu)

One electron is present in the outermost shell of the copper atom. When more than one copper atom gets arranged in a crystal lattice (fcc), Electrons present in the outermost shell share interstitial space with another copper atom, molecular orbital get formed. The electrons present in the valence shell get distributed in the interstitial space of the metal crystal. They are free to move. This is a metallic bond example. As the metallic bond formed between Copper metal ions and electrons.

Iron (Fe)

The iron atom has eight electrons in its electron shell. When Iron atoms get arranged in a crystal lattice (bcc and fcc), electrons present in the outermost shell shares interstitial space with other iron atoms and molecular orbitals get formed. The delocalization of these electrons takes place in interstitial space.  The more electrons which are not associated with atoms get available as the number of valence electrons increases. This is a metallic bond example. The metallic bond formed between positively charged iron metal ions and electrons.

Read more on : 15 Coordinate Covalent Bond Examples: Detailed Insight And Facts

Frequently Asked Questions:

Question 1. What is metallic bonding?

Answer: Metallic bonding can be defined as

The attractive force is present between negatively charged mobile electrons and positively charged metallic ions. This force of attraction is used to hold the metal atoms together in the metallic crystal.

Question 2 . Are metallic bonds soluble in water?

Answer: The water solubility of metallic bonds

Metallic bonds are not soluble in water but some alkali metals Sodium and Potassium are soluble in water.

Question 3. Are metallic bonds are strong bonds?

Answer: Yes, Metallic bonds are not weak bonds.

As metals require high temperatures to melt and boil. A large amount of energy is needed to cleave the bonds between metal atoms, hence they are considered strong bonds.

Read more on : Triple Bond Examples: Detailed Insights And Facts

Question 4. What is the difference between a Metallic and Covalent bond?

Answer: The difference between Metallic and Covalent bonds are as follows:

Read more on : 4 nonpolar covalent bond examples: Detailed Insights And Facts