Smruti Bhosale

I am Smruti Bhosale. I am from Mumbai. I have Master's degree in Inorganic chemistry from Guru Nanak Khalsa College, Mumbai. I always have a passion for writing and to inspire as many willing minds through my words. Chemistry is a subject that is used by everyone in their normal lives. I want to explain the subject in the most understandable and simplest way possible. I am a creative, hard working person and passionate about learning new things. I like to read books.

N2 polar or nonpolar : Why, How, Characteristics, And Detailed Facts.

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Nitrogen gas (N2) is a diatomic molecule composed of two nitrogen atoms. When it comes to determining whether N2 is polar or nonpolar, we need to consider the electronegativity difference between the atoms and the molecular geometry. Polar molecules have an uneven distribution of charge due to the electronegativity difference between the atoms, while nonpolar molecules have an even distribution of charge. In the case of N2, the electronegativity of nitrogen is the same, resulting in a nonpolar molecule. This means that N2 has no positive or negative poles and does not exhibit dipole-dipole interactions. To further understand the polarity of N2, let’s delve into the concept of electronegativity and molecular geometry.

Key Takeaways

  • N2 is a nonpolar molecule because it has a symmetrical linear shape and equal electronegativity between nitrogen atoms.
  • Nonpolar molecules have no permanent dipole moment and do not have positive or negative poles.
  • The electronegativity difference between atoms determines whether a molecule is polar or nonpolar.
  • Understanding the polarity of molecules is important in predicting their physical and chemical properties.

N2: Polar or Nonpolar?

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Explanation of polar and nonpolar molecules

When discussing the polarity of molecules, it is essential to understand the concept of electronegativity. Electronegativity refers to an atom‘s ability to attract electrons towards itself in a chemical bond. When two atoms with different electronegativities form a bond, the shared electrons are not equally distributed. This uneven distribution creates a separation of charge, resulting in a polar molecule.

On the other hand, in nonpolar molecules, the atoms involved in the chemical bond have similar or identical electronegativities. As a result, the shared electrons are evenly distributed, leading to a molecule with no separation of charge.

Comparison with HF molecule

To better understand the polarity of N2 (nitrogen gas), let’s compare it with the HF (hydrogen fluoride) molecule. HF is a polar molecule due to the significant difference in electronegativity between hydrogen and fluorine. Hydrogen has a lower electronegativity, causing the shared electrons to be pulled closer to the fluorine atom, resulting in a partial negative charge on fluorine and a partial positive charge on hydrogen.

In contrast, N2 is composed of two nitrogen atoms, which have the same electronegativity. Therefore, the electrons in the nitrogen-nitrogen bond are shared equally, resulting in a nonpolar molecule.

Explanation of N2 as a nonpolar molecule

N2 is a diatomic molecule, meaning it consists of two nitrogen atoms bonded together. Each nitrogen atom has five valence electrons, and in the N2 molecule, these ten valence electrons are shared between the two atoms. The electron distribution in N2 is symmetrical, with each nitrogen atom contributing five electrons to the bond.

The equal sharing of electrons in the N2 molecule leads to a linear molecular shape. The two nitrogen atoms are directly bonded to each other, and the molecule has no lone pairs of electrons. This symmetrical arrangement of atoms and electrons results in a nonpolar molecule.

To determine the polarity of a molecule, we can also consider the dipole moment. The dipole moment is a measure of the separation of positive and negative charges in a molecule. In a nonpolar molecule like N2, the dipole moment is zero because there is no separation of charge.

Bond Type of N2

Nitrogen gas (N2) is a diatomic molecule composed of two nitrogen atoms. In order to understand the bond type of N2, we need to explore the nature of the bond between these atoms.

Explanation of Bond Types

When atoms come together to form molecules, they can do so through different types of bonds. The two main types of chemical bonds are covalent bonds and ionic bonds.

  1. Covalent Bonds: Covalent bonds occur when atoms share electrons. This type of bond is typically formed between nonmetal atoms. In a covalent bond, the shared electrons are attracted to both nuclei, creating a strong bond.

  2. Ionic Bonds: Ionic bonds occur when there is a transfer of electrons from one atom to another. This type of bond is typically formed between a metal and a nonmetal. In an ionic bond, one atom becomes positively charged (cation) by losing electrons, while the other atom becomes negatively charged (anion) by gaining electrons. The attraction between these opposite charges creates the bond.

Determination of N2 Bond Type

To determine the bond type of N2, we need to consider the electronegativity of nitrogen atoms and the distribution of electrons in the molecule.

  1. Electronegativity: Electronegativity is a measure of an atom‘s ability to attract electrons towards itself in a chemical bond. The difference in electronegativity between two atoms can help determine the type of bond.

In the case of N2, both nitrogen atoms have the same electronegativity value since they are the same element. Nitrogen has an electronegativity value of 3.04 on the Pauling scale.

  1. Electron Distribution: In N2, each nitrogen atom has five valence electrons. To form a stable molecule, each nitrogen atom shares three electrons with the other nitrogen atom, resulting in a triple bond.

The triple bond in N2 consists of one sigma bond and two pi bonds. The sigma bond is formed by the overlap of two atomic orbitals head-on, while the pi bonds are formed by the sideways overlap of p orbitals.

Based on the electronegativity and electron distribution, we can conclude that the bond between the nitrogen atoms in N2 is a covalent bond. Since both nitrogen atoms have the same electronegativity, the electron pair is shared equally between them, resulting in a nonpolar covalent bond.

Summary

Molecular Geometry of N2

The molecular geometry of a molecule refers to the arrangement of its atoms in three-dimensional space. It provides crucial information about the shape and structure of the molecule, which, in turn, affects its physical and chemical properties. In the case of N2, or nitrogen gas, understanding its molecular geometry is essential in determining its polarity.

To understand the molecular geometry of N2, we need to delve into the VSEPR theory. VSEPR stands for Valence Shell Electron Pair Repulsion, and it is a model used to predict the shapes of molecules based on the repulsion between electron pairs in the valence shell of the central atom.

According to the VSEPR theory, electron pairs around the central atom will arrange themselves in a way that minimizes repulsion, resulting in specific molecular shapes. The electron pairs can be either bonding pairs (shared between atoms) or non-bonding pairs (also known as lone pairs).

Application of VSEPR Theory to N2

In the case of N2, the central atom is nitrogen (N), and it has a total of 10 valence electrons (5 from each nitrogen atom). Since N2 is a diatomic molecule, it consists of two nitrogen atoms bonded together by a triple bond.

To determine the molecular geometry of N2, we consider the electron pairs around each nitrogen atom. Each nitrogen atom has three bonding pairs, forming the triple bond, and no lone pairs. Therefore, the electron pair arrangement around each nitrogen atom is linear.

Explanation of Linear Molecular Geometry in N2

Based on the VSEPR theory, the linear electron pair arrangement around each nitrogen atom in N2 results in a linear molecular geometry for the entire molecule. This means that the two nitrogen atoms are aligned in a straight line, with a bond angle of 180 degrees.

The linear molecular geometry of N2 can be visualized as follows:

Atom Electron Pair Arrangement
N Linear
N Linear

The linear molecular geometry of N2 has important implications for its polarity. Since the two nitrogen atoms are identical and the molecule is linear, the bond dipoles cancel each other out, resulting in a nonpolar molecule.

Electronegativity of N2

Definition of Electronegativity

Electronegativity is a fundamental concept in chemistry that refers to the ability of an atom to attract electrons towards itself in a chemical bond. It is a measure of the atom’s desire to gain electrons and form a stable electron configuration. The electronegativity of an atom is influenced by factors such as its atomic number, atomic radius, and electron configuration.

Electronegativity Value of Nitrogen

Nitrogen (N) is a nonmetallic element with an atomic number of 7. It is located in Group 15 of the periodic table and has five valence electrons. The electronegativity of nitrogen is 3.04 on the Pauling scale, which is a commonly used scale to measure electronegativity. This value indicates that nitrogen has a relatively high electronegativity compared to other elements.

Explanation of Nonpolar Nature of N2 based on Electronegativity

When considering the polarity of a molecule, it is essential to analyze the electronegativity difference between the atoms involved in the bond. In the case of nitrogen gas (N2), both nitrogen atoms have the same electronegativity value of 3.04. This means that there is no significant difference in electronegativity between the two nitrogen atoms.

Due to the equal sharing of electrons in the nitrogen-nitrogen bond, N2 is considered a nonpolar molecule. In a nonpolar covalent bond, the electrons are shared equally between the atoms, resulting in a symmetrical distribution of charge. As a result, there is no separation of positive and negative charges, and the molecule has no net dipole moment.

In the case of N2, the two nitrogen atoms share a triple bond, with each nitrogen atom contributing three electrons to form a total of six shared electrons. This sharing of electrons is equal and symmetrical, resulting in a nonpolar molecule. The Lewis structure of N2 further supports this, as it shows a linear arrangement of the atoms with no partial charges.

To summarize, the nonpolar nature of N2 can be explained by the equal electronegativity of the nitrogen atoms, leading to an equal sharing of electrons and a symmetrical distribution of charge. This absence of a net dipole moment makes N2 a nonpolar molecule.

Property N2
Electronegativity 3.04
Molecular Shape Linear
Dipole Moment 0
Lewis Structure N≡N
VSEPR Theory Linear

Force of Attraction in N2

Nitrogen (N2) is a diatomic molecule composed of two nitrogen atoms bonded together. When discussing the force of attraction in N2, we need to consider the intermolecular forces that hold the molecule together. One of the primary forces at play in N2 is the London dispersion force.

The London dispersion force, also known as the dispersion force or the Van der Waals force, is a type of intermolecular force that exists between all molecules, including nonpolar molecules like N2. This force arises due to temporary fluctuations in the electron distribution within a molecule, creating temporary dipoles.

In the case of N2, each nitrogen atom has five valence electrons. These electrons are distributed in three bonding pairs and one lone pair. The electron distribution in N2 is symmetrical, resulting in a nonpolar molecule. However, despite being nonpolar, N2 still experiences London dispersion forces.

Explanation of London Dispersion Force in N2

The London dispersion force in N2 is a result of the temporary fluctuations in the electron distribution within the molecule. Even though N2 does not have a permanent dipole moment, the movement of electrons can create temporary dipoles. These temporary dipoles induce similar temporary dipoles in neighboring N2 molecules.

As a result, the temporary dipoles in N2 molecules attract each other, leading to a weak force of attraction. While the London dispersion force is generally weaker than other intermolecular forces, such as hydrogen bonding or dipole-dipole interactions, it still plays a significant role in determining the physical properties of N2.

The strength of the London dispersion force in N2 depends on factors such as the number of electrons and the shape of the molecule. In the case of N2, the presence of 14 valence electrons (7 electrons per nitrogen atom) contributes to a relatively strong London dispersion force.

Uses of N2

Nitrogen gas (N2) has a wide range of applications in various industries due to its unique properties. Let’s explore some of the common uses of N2 in different sectors.

Common applications of N2 in the chemical industry

In the chemical industry, nitrogen gas finds extensive use in various processes. Here are some of the common applications:

  1. Blanketing and purging: N2 is often used to create an inert atmosphere in chemical reactors and storage tanks. By displacing oxygen and moisture, it helps prevent oxidation, degradation, and contamination of sensitive chemicals.

  2. Solvent recovery: Nitrogen gas is employed in the recovery of solvents from chemical processes. It aids in the removal of volatile organic compounds (VOCs) and other impurities, allowing for the recycling and reuse of solvents.

  3. Cryogenic applications: N2 is utilized in cryogenic processes, such as freezing and cooling. Its low temperature properties make it suitable for applications like cryogenic grinding, cryopreservation, and cryogenic distillation.

  4. Chemical synthesis: Nitrogen gas is an essential component in the production of various chemicals, including ammonia, nitric acid, and urea. These chemicals serve as building blocks for fertilizers, explosives, and pharmaceuticals.

Use of N2 as a food preservative

Nitrogen gas plays a crucial role in the food industry, particularly in preserving the freshness and quality of perishable goods. Here’s how it is used:

  1. Modified Atmosphere Packaging (MAP): N2 is commonly employed in MAP, a technique used to extend the shelf life of food products. By replacing the oxygen in the packaging with nitrogen, the growth of spoilage-causing microorganisms is inhibited, thereby preserving the food’s freshness.

  2. Preventing oxidation: Nitrogen gas is used to prevent oxidative reactions in food products. It helps maintain the color, flavor, and nutritional value of packaged foods by reducing the exposure to oxygen, which can lead to spoilage.

  3. Pressurizing and propelling: Nitrogen gas is utilized in the pressurization and propelling of aerosol cans used for food products like whipped cream. It helps create the necessary pressure for dispensing the product while ensuring its safety and quality.

Other industrial uses of N2

Apart from the chemical and food industries, nitrogen gas finds applications in various other sectors. Here are some notable examples:

  1. Electronics manufacturing: N2 is used in electronics manufacturing processes, such as soldering, wave soldering, and reflow soldering. It helps create an oxygen-free environment, preventing oxidation and ensuring the quality of electronic components.

  2. Oil and gas industry: Nitrogen gas is employed in oil and gas exploration and production. It is used for well stimulation, pressure testing, and as a lifting medium in enhanced oil recovery techniques.

  3. Fire suppression systems: Nitrogen gas is utilized in fire suppression systems, particularly in areas where water-based systems may cause damage. It helps displace oxygen, effectively suppressing fires without leaving behind any residue.

  4. Tire inflation: Nitrogen gas is increasingly used for tire inflation in various industries, including automotive, aviation, and racing. It offers benefits such as improved tire life, better fuel efficiency, and enhanced safety.

Frequently Asked Questions

Is N2 polar or nonpolar?

When it comes to the polarity of N2, it is considered a nonpolar molecule.

What forces does N2 have?

N2, also known as nitrogen gas, is held together by a strong covalent bond. The forces that hold the nitrogen atoms together in N2 are called covalent forces. Covalent bonds occur when atoms share electrons, resulting in a stable molecule.

Does N2 have polar bonds?

No, N2 does not have polar bonds. A polar bond occurs when there is an unequal sharing of electrons between two atoms. In N2, the nitrogen atoms share their electrons equally, resulting in a nonpolar bond.

What is the molecular geometry of N2?

The molecular geometry of N2 is linear. This means that the two nitrogen atoms are arranged in a straight line, with a bond angle of 180 degrees.

What is the order of electronegativity of N2?

Electronegativity is a measure of an atom‘s ability to attract electrons towards itself in a chemical bond. In the case of N2, both nitrogen atoms have the same electronegativity value, which is 3.04 on the Pauling scale. Therefore, the order of electronegativity for N2 is the same for both atoms.

Why is N2 nonpolar?

N2 is nonpolar due to its linear molecular geometry and the equal sharing of electrons between the nitrogen atoms. In a nonpolar molecule, the electronegativity difference between the atoms is either very small or nonexistent. Since the nitrogen atoms in N2 have the same electronegativity, there is no separation of charge, resulting in a nonpolar molecule.

Frequently Asked Questions

Is N2 a polar or nonpolar molecule?

N2 is a nonpolar molecule.

Why is N2 nonpolar?

N2 is nonpolar because it has a linear molecular shape and the two nitrogen atoms have equal electronegativity, resulting in a symmetrical distribution of electron density.

Is N2 polar or nonpolar or ionic?

N2 is neither polar nor ionic. It is a nonpolar molecule.

Is N2 ionic, polar covalent, or nonpolar covalent?

N2 is a nonpolar covalent molecule. It consists of a covalent bond between two nitrogen atoms.

What is the bond type of N2, polar or nonpolar?

The bond in N2 is a nonpolar covalent bond.

Which atom in N2 is closest to the negative side, polar or nonpolar?

In N2, neither nitrogen atom is closer to the negative side as the molecule is nonpolar.

Is the Lewis structure of N2 polar or nonpolar?

The Lewis structure of N2 is nonpolar.

Is N2 polar or nonpolar?

N2 is a nonpolar molecule.

What is the molecular shape of N2?

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The molecular shape of N2 is linear.

What is the dipole moment of N2?

N2 has a zero dipole moment because it is a nonpolar molecule.

What is the electron distribution in N2?

In N2, the electron distribution is symmetrical due to the linear molecular shape and equal electronegativity of the nitrogen atoms.

What is the electronegativity of N2?

The electronegativity of N2 is equal for both nitrogen atoms since they are the same element.

9+ Ionic Bond Examples: Explanation And Detailed Facts

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ionic bond

In this article, we are going to see what is an ionic bond, its characteristics, facts along with some ionic bond examples in detail.

When the attractive force binds unlike ions together then this is known as an ionic bond. An ionic bond is also termed an electrovalent bond. Compounds having this type of bonding are called ionic compounds. Some examples are given as follows.

Some elements of the periodic table could acquire a noble gas configuration by losing or gaining electrons. Those elements that lose an electron and acquire a positive charge are called cations, while those that gain an electron and acquire a negative charge are called anions.

AB  image 26 A+ +  B–         A is a cation with a positive charge and B is an anion with a negative charge.

Characteristics

  • An ionic bond is also termed an electrovalent bond.        
  • A strong electrostatic force of attraction held Positive and Negative ions together.
  • Ionic compounds are hard and brittle.
  • Usually have e high melting point.
  • In the solid-state ionic compounds is a bad conductor of electricity while they are a good conductor of electricity when melted or dissolved in solvents.
  • Ionic compounds are soluble in polar solvents and insoluble in non-polar solvents.
  • Ionic bond forms between metal and non-metal.

Ionic Bond Examples

Sodium Chloride NaCl

Sodium Chloride, Sodium atom has 1 valence electron and Chlorine atom has 7 valence electrons. Chlorine atom need one electron to complete its octet. Na atom loses its electron and acquires a positive charge while Chlorine atom gains an electron and acquires a negative charge. Hence Na and Cl form an ionic bond.

ionic bond example
Fig 1: Sodium Chloride NaCl

Image Credits: Cloudfront

Sodium Bromide NaBr

In Sodium Bromide, the Sodium atom has one electron in its valence shell and the Bromine atom has 7 electrons.  Na loses one electron which is gained by Br to complete its octet. Ionic compound NaBr is formed.

image 9
Fig 2: Sodium Bromide NaBr

Image Credits: Study

Sodium Fluoride NaF

In Sodium Fluoride NaF, to complete octet state Fluorine atom need only 1 electron, which is given by the sodium atom. Na acquires positive [Na]+and F acquire negative charge [F]–, forming an ionic bond.                                                      

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Fig3: Sodium Fluoride NaF

Image Credits: Studiousguy

Potassium Chloride KCl

In Potassium Chloride KCl, the Potassium atom has one electron in its valence shell and the Chlorine atom has seven electrons. Chlorine atom need one electron to complete its octet state. K loses its electron and becomes positively charged by gaining this electron Cl becomes negatively charged. The Formation Ionic bond takes place between K and Cl.

image 11
Fig 4: Potassium Chloride KCl

Image Credits: Blogspot

Potassium Iodide KI

In Potassium Iodide KI, the Iodine atom has seven valence electrons in its valence shell to get its octet state complete, it requires one electron. Potassium loses one electron, acquires a positive charge while iodine takes this electron and acquires a negative charge forming an ionic bond.

image 12
Fig 5: Potassium Iodide KI

Image Credits: Chem.libretexts

Potassium Bromide KBr

In Potassium Bromide KBr, Potassium has 1 electron in its valence shell whereas Bromine has seven electrons. Hence K loses its electron becomes K+ and Br gains this electron becomes Br–. The ionic bond formed between K and Br.

image 13
Fig 6: Potassium Bromide KBr

Image Credits: Study

 Potassium Fluoride KF

In Potassium Fluoride KF, the Fluorine atom has seven electrons and the Potassium atom has one electron in its valence shell. To get a stable configuration Fluorine needed one electron. Potassium transfers its valence electron to Fluorine forming an ionic bond.

image 14
Fig 7: Potassium Fluoride KF

Image Credits: Slideplayer

Lithium Iodide LiI

In this ionic compound, the Iodine atom has seven electrons in its valence shell to complete its stable electronic configuration it requires one electron. Lithium has a valency of one electron. Li loses its electron acquires a positive charge and by gaining of electron I acquire a negative charge.  

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Fig 8: Lithium Iodide LiI

Image Credits: Gstatic

Lithium Oxide Li2O

In Lithium Oxide Li2O, Each Lithium has one electron in its outermost shell and oxygen has six electrons. To attain an octet state oxygen need two electrons. Both lithium atoms lose electrons becomes positively charged while oxygen gains those electrons and becomes negatively charged. The ionic bond formed.

image 16
Fig 9: Lithium Oxide Li2O

Image Credits: Socratic

Calcium Oxide CaO

In Calcium oxide, Calcium has two valence electrons while oxygen has six valence electrons in its valence shell. To complete its octet oxygen requires two more electrons. Calcium loses its electrons and acquires +2 charge and oxygen gains those electrons, acquires 2- charge. 

image 17
Fig 10: Calcium Oxide CaO

Image Credits: Gstatic

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

Frequently Asked Questions:

Question: Is CaCl2 an ionic compound?

Answer: The CaCl2 is an ionic compound,

In CaCl2, Calcium has two valence electrons and each Chlorine has one electron. Ca loses both the electrons which are gained by each Cl and complete its octet. Calcium acquires +2 while each Chlorine acquires -1 charged. Due to this unlike charges ionic bond formed in the CaCl2 compound.

Question: What is an ionic bond?

Answer: Ionic bond is defined as

When the attractive force binds unlike ions together then this is known as an ionic bond. An ionic bond is also termed an electrovalent bond.

Question: What are the differences between ionic and covalent bonds?

Answer: The difference between ionic and covalent bonds :

Ionic bond Covalent bond
When the attractive force binds unlike ions together then this is known as an ionic bond. When two atoms get stabilized by sharing of electrons then this is known as a covalent bond.
Forms between electropositive and electronegative atoms. Forms between the same or different atoms.
It is a non-directional bond. It is a directional bond.
Has high melting and boiling points. Has low melting and boiling points.
Ionic compounds are soluble in polar solvents and insoluble in non-polar solvents.   Covalent compounds are insoluble in polar solvents and soluble in non-polar solvents.

Also Read:

15 Coordinate Covalent Bond Examples: Detailed Insight And Facts

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coordinate covalent bond

In this article we are going to see what is a coordinate covalent bond, its characteristics are facts along with some coordinate covalent bond examples in detail.

During the bond formation sharing of electron pair takes place by only one atom, it is called a coordinate covalent bond. Only one atom in a molecule shares both the electrons to form a bond. This type of bonding is seen in following examples.

The coordinate covalent bonds are also entitled as a dipolar bond or dative bond. In a coordinate covalent bonding, both electrons are shared by an individual atom, another one is the electron acceptor. Denoted by arrow ‘→’, pointing towards atom who accepts electrons.

 A → B       A gives electron pair or two electrons, termed as Donor atom

                 B accepts electron pair or electrons, termed as Acceptor atom.  

The coordinate covalent bond differs from a covalent bond only in the way it is formed, once formed it is exactly like a covalent bond. The coordinate covalent bond may form when one of the combining atoms has an unused lone pair of electrons besides its completed octet.     

Characteristics

  • Electron pair or both the electrons of a bond given by only one atom.
  • Also called dipolar bond or dative bond.
  • Coordinate covalent bonds are shown as ‘→‘.  
  • Compounds containing this type of bonding are called coordinate covalent compounds.
  • Sharing of electrons leads to the stabilization of all the atoms.
  • The donor atom acquires a slight positive charge and a slight negative charge acquired by the acceptor atom.

Coordinate Covalent Bond Examples

Formation of Ammonium boron trifluoride NH3→BF3

In the NH3 molecule, Nitrogen has 5 electrons in its valence shell. N has a complete octet by the formation of three bonds with three hydrogen atoms. But it is still left with a pair of unused electrons. This lone pair of electrons may be donated to the B atom in BF3, which is electron-deficient forming a coordinate covalent bond. Due to this Boron atom also completes its octet.

Coordinate Covalent Bond Examples
Figure 1: Ammonium boron trifluoride NH3→BF3

Image credits : Wikipedia

Formation of Ammonium ion NH4+

In the NH3 molecule, the Nitrogen atom has lone pair of electrons after completing its octet. This lone pair of electrons share with the H+ ion of HCl. The coordinate covalent bond formed between N and H, which leads to the formation of Ammonium ion NH4+.

image 69
Figure 2: Formation of Ammonium ion NH4+

Image Credits: Staticflickr

Formation of Hydronium ion H3O+

During the formation of hydronium ions, water molecules act as donor atoms.  The oxygen atom present in H2O has lone pair of electrons which is used to form a coordinate covalent bond with the hydrogen atom present in HCl.

image 70
Figure 3: Formation of Hydronium ion H3O+

Image Credits: Brainkart

Formation of tetrafluroboron BF4–

Fluorine atoms share lone pair of electrons with Boron. Fluorine act as a donor atom and boron act as an acceptor. The formation of tetrafluroboron takes place by a coordinate covalent bond.

image 71
Figure 4: Formation of tetrafluroboron BF4–

Image Credits: Redchemistry

Formation of Aluminium chloride AlCl6

Aluminium has three electrons in its valence shell, hence it forms three bonds with Chlorine. Chlorine has 7 electrons from which one is used for bond formation rest act as lone pair. Chlorine share one lone pair of electrons with another aluminium atom forming a coordinate covalent bond.

image 72
Figure 5: Aluminium chloride AlCl6

Image Credits: Redchemistry

Sulphur dioxide SO2

In sulphur dioxide molecule sulphur has 6 valence electrons hence act as donor atom and oxygen acts as an acceptor. Sulphur form a double bond with one of the oxygen and shares one lone pair with other oxygen.

image 73
Figure 6: Sulphur dioxide SO2

Image Credits: Redchemistry

Sulphur trioxide SO3

After the formation of a double bond with oxygen, Sulphur shares two lone pairs of electrons with two oxygen atoms by a coordinate covalent bond.

image 74
Figure 7: Sulphur trioxide SO3

Image Credits: Redchemistry

Sulphuric acid H2SO4

Sulphur present in sulphuric acid forms two coordinate covalent bonds with two different oxygen atoms. Sulphur has two lone pairs.

image 75
Figure 8: Sulphuric acid H2SO4

Image Credits: gstatic.com

Nitrogen pentaoxide N2O5

Nitrogen has 5 electrons in its valence shell, out of which three electrons are used to form one single and one double bond with oxygen. The remaining electrons act as lone pairs. This lone pair was utilized to form a coordinate covalent bond with the oxygen atom.

image 76
Figure 9: Nitrogen pentaoxide N2O5

Image Credits: encrypted-tbn0.gstatic.com

Nitromethane

In nitromethane, Nitrogen atoms form coordinate covalent bonds with oxygen atoms. Nitrogen forms a double bond with one oxygen and a single bond with a carbon atom of the methyl group and completes its octet.

image 87
Figure 10: Nitromethane

Image Credits: Brainkart

Hexammine Cobalt (lll) chloride Co(NH3)6Cl3

In Hexammine Cobalt (lll) chloride complex, Six Nitrogen atoms of the ligand, Ammonia NH3 shares lone pair of electrons with central metal Cobalt.

image 78
Figure 11: Hexammine Cobalt (lll) chloride Co(NH3)6Cl3

Image Credits: Wikipedia

Hexaaquo cobalt (ll) chloride Co(H2O)6Cl2

In Hexaaquo cobalt (ll) chloride, Six water H2O molecules are the ligands, act as donor atoms. Central metal atom Cobalt act as an acceptor atom. The oxygen atom of H2O has lone pair of electrons that share with Cobalt forming a coordinate covalent bond.

image 79
Figure 12: Hexaaquo cobalt (ll) chloride Co(H2O)6Cl2

Image Credits: encrypted-tbn0.gstatic.com

Tetracarbonyl Nickel Ni(CO)4

In Tetracarbonyl Nickel, Ni acts as acceptor, and CO acts as a donor atom. Four oxygen atoms of ligand share lone pair with Nickel forming a coordinate covalent bond.

image 80
Figure 13: Tetracarbonyl Nickel Ni(CO)4

Image Credits: Wikimedia

Hexaaquo Aluminium (lll)

In this complex, the oxygen atoms of H2O shares lone pair with the central metal atom Aluminium. 

image 81
Figure 14: Hexaaquo Aluminium (lll)

Image Credits: Chemguide

Ozone

The oxygen atom has 6 electrons in its valence shell. Two electrons are utilized to form a double bond with one oxygen and one lone pair is used to form a coordinate covalent bond with another oxygen.

image 82
Figure 15: Ozone

Image Credits: Redchemistry

Read on :SN2 Examples: Detailed Insights And Facts

Frequently asked questions:

1)Question: What is meant by a dative bond?

Answer: Dative bond is defined as

During the bond formation sharing of electron pair takes place by only one atom, it is called a coordinate covalent bond. Also called dipolar bond or dative bond.

2)Question: What are the differences between coordinate and covalent bonds?

Answer: Difference between a coordinate and covalent bond

Coordinate bond Covalent bond
Only one atom in a molecule shares both the electrons to form a bond. Both the atoms of the molecule share electrons to form a bond.
A minimum of one lone pair of electrons is required. It does not require any lone pair of electrons.
Should not have unpair electrons Should have unpair electrons
Empty orbital should be present in the acceptor atom. Empty orbital does not require.
It is a polar bond. It may be polar or non-polar depending on atoms forming a bond.
Represented by arrow → Represented by a dash –

3) Question: Is the coordinate bond directional?

Answer: Coordinate bond is directional,

The coordinate bond form when both the electrons are shared by only one atom, the donor atom hence coordinate bond is directional. Also represented by an arrow → pointing towards the acceptor atom.

Also Read:

Alkyl Halide Examples: Detailed Insights And Facts

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In this article, we are going to see what are the alkyl halides, their insights, and facts in detail with some alkyl halide examples.

Alkyl Halide Examples

NO. CLASSIFICATION STRUCTURE NAME EXPLANATION
1 Primary Screenshot 2021 12 05 140107 Bromoethane In the structure of ethane one hydrogen gets replaced by halogen i.e Bromine.
2 Primary Screenshot 2021 12 05 140017 1- Iodo propane This is a three-carbon structure, propane. In this one hydrogen atom gets replaced by Iodine, which is attached to the carbon, having a bond with another carbon.
3 Primary Screenshot 2021 12 05 140301 1-Chloro butane   In the four carbons chain of alkane, one hydrogen gets replaced by Chlorine. Which is attached to a primary carbon.
4PrimaryFluoroethaneIn the structure of ethane one hydrogen get replaced by Fluorine. which is attached with carbon having a bond with another carbon.
5 Secondary Screenshot 2021 12 05 140559 2-Bromo butane In the structure of butane, one of the hydrogen atoms of the second carbon gets replaced by Bromine.
6 Secondary Screenshot 2021 12 05 142009 2- Iodo propane In the structure of propane, one of the hydrogen atoms of second carbon gets replaced by Iodine.
7Tertiary2- Iodo-2-methyl propaneIn the structure of propane one hydrogen gets replaced by Iodine. which is attached with carbon having bonds with another three carbons.
8 Tertiary Screenshot 2021 12 05 141801 2-Bromo-2-methyl butane In the structure of butane, hydrogen atoms of second carbon gets replaced by Iodine and methyl group.
9 Tertiary Screenshot 2021 12 05 142620 2-Chloro-2-methyl pentane This is a five-carbon structure, pentane. In this one hydrogen atom gets replaced by Chlorine, which is attached to the carbon, having a bond with another three carbons.
10 Secondary Screenshot 2021 12 05 140228 2-Iodo butane In the structure of butane, one hydrogen gets replaced by Iodine. which is attached with carbon having bonds with another two carbons.
11 Secondary Screenshot 2021 12 05 142021 2-Chloro propane In the structure of propane, one of the hydrogen atoms of second carbon gets replaced by Chlorine.
12 Secondary Screenshot 2021 12 05 142712 2-Bromo-3-ethyl hexane This is a six carbons structure, hexane. In this one hydrogen atom of second carbon gets replaced by Bromine, which is attached to the carbon, having a bond with another two carbons. An ethyl group is attached at third carbon.
13Primary1- Bromo-2,2-dimethyl propaneIn the structure of propane one hydrogen gets replaced Bromine. Two methyl groups are attached to the second carbon.
14 Secondary Screenshot 2021 12 05 142118 3- Chloro pentane In the structure of pentane, one of the hydrogen atoms of the third carbon gets replaced by Chlorine.
15 Primary Screenshot 2021 12 05 141917 1-Bromo-2-methyl butane In the structure of butane, one of the hydrogen atoms of first carbon get replaced by Bromine, a methyl group is attached at second carbon.
16 Secondary Screenshot 2021 12 05 141658 2-Iodo-3-methyl butane In the structure of butane, one of the hydrogen atoms of second carbon gets replaced by Iodine. Methyl group is boned with third carbon.
17 Primary Screenshot 2021 12 05 142427 1- Bromo-2,3-dimethyl butane In the structure of butane, one of the hydrogen atoms of first carbon gets replaced by Bromine. Two Methyl groups are boned with second and third carbon.
18 Secondary Screenshot 2021 12 12 200516 2- Fluoro butane In the structure of butane, one of the hydrogen atoms of second carbon gets replaced by Fluorine.
19 Primary Screenshot 2021 12 05 142451 1-Chloro-2,2-dimethyl propane In the structure of propane one hydrogen gets replaced Chlorine .two methyl groups are attached to the second carbon.
20 Secondary Screenshot 2021 12 05 140518 1 2-Chloro butane In the structure of butane, one of the hydrogens gets replaced by Chlorine. which is attached with carbon having bonds with another two carbons.

Alkyl halides are compounds that contain halogens as one of their constituents along with alkanes. In alkane, when one or more hydrogen atoms get substituted by halogen atoms it is termed an alkyl halide. They also called as Haloalkane.

Halogens are group seventeen elements, electronegative. Fluorine, chlorine, bromine, iodine are the halogens, Represented by ‘X’. Hence, the alkyl halides are expressed as R-X.

Where , R- Alkyl group or carbon chain and X- Halogens as F, Cl, Br, I.

Alkyl halides are classified as

On account of several carbon atoms having bonded with the carbon atom, which is attached to the halogen atom, alkyl halides are classified as primary, secondary, tertiary alkyl halides.

Primary alkyl halides (1°)

When one carbon atom had a bond with the carbon atom which is attached to the halogen atom it is known as Primary alkyl halide or 1° alkyl halide.

Usually primary alkyl halides undergo SN2 reaction mechanism.

Secondary alkyl halides (2°)

When two carbon atoms had a bond with the carbon atom which is attached to the halogen atom it is known as Secondary alkyl halides or 2° alkyl halides.

Secondary alkyl halides undergo both SN1 and SN2 reaction mechanisms.

Tertiary alkyl halides (3°)

When three carbon atoms had a bond with the carbon atom which is attached to the halogen atom it is known as Tertiary alkyl halides or 3° alkyl halides.

Tertiary alkyl halide undergo SN1 reaction mechanism.

Alkyl halide examples
Figure1 : Classification of Alkyl halides

Alkyl halides are used as Solvents. They are also used as Refrigerants, Propellants, Fire retardants. Alkyl halides like Chloroform, are used as medical Anesthetic.

Read more on List of 20 Examples of Unbalanced Force

Frequently Asked Questions :

Question: What is alkyl halide example ?

Answer: Some examples of alkyl halides are given below,

Alkyl halides are classified as primary, secondary, tertiary alkyl halides. 2- Iodo-2-methyl propane (3°) , 2-Chloro propane (2°) , 1-Bromo-2-methyl butane (1°) etc. are the examples of haloalkane.

Question: What is primary alkyl halide?

Answer: The term primary alkyl halide is use

When, one ( Primary) carbon atom is attached to the carbon atom which is bonded with the halogen atom it is known as Primary alkyl halide or 1° alkyl halide. Represented as R-CH2-X.

Question: What is the formula for alkyl halides?

Answer: The formula for alkyl halide

In alkane, when one or more hydrogen atoms get substituted by halogen atoms it is termed an alkyl halide. The alkyl halides are represented as R-X. Where , R- Alkyl group or carbon chain and X- Halogens as F, Cl, Br, I.

Question: What is 3 alkyl halide?

Answer: The term 3 alkyl halide is use

When three carbon atoms had a bond with the carbon atom which is attached to the halogen atom it is known as Tertiary alkyl halides or 3° alkyl halides.

Question: What are the types of alkyl halide?

Answer: The alkyl halides are classified as

On account of several carbon atoms having bonded with the carbon atom, which is attached to the halogen atom, alkyl halides are classified as Primary alkyl halide, Secondary alkyl halide, Tertiary alkyl halides.

When one carbon atom had a bond with the carbon atom which is attached to the halogen atom it is known as Primary alkyl halide or 1° alkyl halide. When two carbon atoms had a bond with the carbon atom which is attached to the halogen atom it is known as Secondary alkyl halides or 2° alkyl halides. When three carbon atoms had a bond with the carbon atom which is attached to the halogen atom it is known as Tertiary alkyl halides or 3° alkyl halides.

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Stereoselective vs Stereospecific: Detailed Insights and Facts

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Fig 1.1 N 300x72 1

In this article, we are going to see the facts about stereoselective vs stereospecific reactions in detail.

The reactions in which a more favorable reaction pathway is responsible for the formation of the stereoisomers of the product and gives multiple product which are stereoisomers are called stereoselective reactions. In stereospecific reactions stereochemistry of the starting material controls the stereochemistry of the product, give only one specific product.

Stereochemistry is concerned with the three-dimensional assembly of the atoms in the molecule. The term stereoisomer is defined as the molecules having the same composition but their arrangement is different. These stereoisomers are classified as diastereomers and enantiomers. Enantiomers are the reflections or clone images of each other and diastereomers are vary in their orientation.

In organic chemistry, the stereochemical outcomes of the reactions are described by stereoselective and stereospecific reactions.

Stereoselective vs stereospecific reactions–

Stereoselective Reaction Stereospecific Reaction
A more favorable reaction pathway is responsible for the formation of the stereoisomers of the product Stereochemistry of starting materials controls the stereochemistry of the product
Gives more than one product, major and minor. Gives only one specific product.  
All stereospecific reactions are also stereoselective.   All stereoselective reactions are not stereospecific
Reaction pathway forming product depends upon electronic effect, steric effect. The stereochemistry of the product leans on the stereochemistry of the reactant.

Stereoselective reactions

Some chemical reactions give more than one products, which are stereoisomers of each other, but one of the products is major while the other is minor.

The structural orientation of the reactants influences the stereoselectivity of the reaction.

In this type of reaction, the more favorable reaction pathway is responsible for the formation of the stereoisomers of the product, which are called stereoselective reactions.

One of the stereoisomers is formed rapidly showing dominancy on another, which leads to the formation of the major product.

When the outcomes of the reaction are enantiomers, the reaction is also called an enantioselective reaction.

When the products are diastereomers of each other, the reaction is also termed a diastereoselective reaction.

The reaction pathway forming product depends upon electronic effect, steric effect.

Examples,

Fig 1.1 N
Figure 1: Epoxidation

This reaction does not show any major or minor product, so it’s not a stereoselective reaction.

stereoselective vs stereospecific
Figure 2: Hydride reduction of cyclic ketone

This reaction is selective toward one of the products, forming major product 92% and minor product 8%. Hence it is a stereoselective reaction.     

Fig 4
Figure 3: Stereoselective dehydrohalogenation

When 2-iodo-butane undergo dehydrohalogenation 60% trans 2-butene and 20% cis-butene is formed. It is a diastereoselective reaction.

Stereospecific reaction

In some reactions, the stereochemistry of starting materials controls the stereochemistry of the products. A certain reactant gives only a specific product.

One stereoisomer of a particular starting material produces one stereoisomer of a particular outcome material while a different stereoisomer of the same starting material produces different stereoisomers of the same outcome materials.

The best example of a stereospecific reaction is the SN2 substitution reaction. In this type of reaction, always an inversion of the configuration takes place at the product side.

The R reactants give the products of S configuration and the S reactant gives the product of R configuration.

Examples,

Fig 5.1
Figure 4: SN2 substitution reaction

Stereoselective reactions are concerned with the reaction pathway and not with the stereochemistry of reactant, on the other hand, stereospecific reactions are only concerned with the stereochemistry of reactant and not with the favorable reaction pathway. Hence, stereospecific reactions become a subset of stereoselective reactions. Therefore all stereospecific reactions are stereoselective, but all stereoselective reactions are not stereospecific reactions.

Read more on Why Chemical Changes are Irreversible: Detailed Analysis

Frequently Asked Questions:

Question: What do you mean by the stereoselective reaction?

Answer: The stereoselective reaction means

The reactions in which more favorable reaction pathway is responsible for the formation of the stereoisomers of the product and gives more than one product, one of the product is major while other is minor which are stereoisomers of each other are called stereoselective reactions.

Question: What do you mean by the stereospecific reaction?

Answer: The stereospecific reaction means

The reactions in which stereochemistry of the starting material or reactant controls the stereochemistry of the product, gives only one specific product, are called stereospecific reactions.

Question: How can you tell if a reaction is stereoselective or stereospecific?

Answer: one can tell the reaction is stereoselective or stereospecific.

If the reaction shows the possibility of the formation of more than one or multiple products, but only one is produced in excess as a major product, then it is a stereoselective reaction.

If the stereoisomer of a different product is given by a different stereoisomer of the reactant, then it is a stereospecific reaction. If a starting material gives identical products in equal ratio then it is not a stereospecific reaction.

Question: Can a stereoselective and stereospecific reaction be both?

Answer: The reaction can be both stereoselective and stereospecific.

In stereoselective reaction, the more favorable reaction pathway is responsible for the formation of the stereoisomers of the product. In the case of stereospecific reaction stereochemistry of starting materials regulate the stereochemistry of the products. These terms describe different aspects of the reaction, it can be both stereoselective and stereospecific. Example,

Fig 6.1 N
Figure 5: Catalytic Hydrogenation

Question: Why all stereospecific reactions are stereoselective?

Answer: All stereospecific reactions are stereoselective.

As we know stereoselective reaction concerns only with the reaction pathway, on the other hand, stereospecific reactions are only concerned with the stereochemistry of the reactant and not with the favorable reaction pathway. Hence, stereospecific reactions become a subset of stereoselective reactions. Therefore all stereospecific reactions are stereoselective.

Question: Which reactions are stereoselective?

Answer: Following are the stereoselective reactions,

  1. Enantioselective hydride reduction of carbonyl compounds.
  2. Nucleophilic addition to a homochiral cyclic ketone.
  3. Nucleophilic addition to a racemic cyclic ketone.

 

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