IO4- Lewis Structure, Characteristics: 11 Facts You Should Know

Introduction to Lewis Structures and Ionic Compounds

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the distribution of electrons around them. They were developed by American chemist Gilbert N. Lewis in the early 20th century and are an essential tool in understanding chemical bonding.

Overview of Lewis Structures

Lewis structures use symbols to represent atoms and lines to represent chemical bonds. The valence electrons, which are the outermost electrons of an atom, are represented as dots around the atomic symbol. These dots are placed in pairs around the symbol, with each pair representing a single electron.

Lewis structures provide a visual representation of how atoms are connected and how electrons are shared or transferred between them. They help us understand the stability of molecules and predict their chemical behavior.

Explanation of Ionic Compounds and their Structures

Ionic compounds are formed when atoms transfer electrons to achieve a stable electron configuration. In these compounds, one or more electrons are completely transferred from one atom to another, resulting in the formation of positively charged ions (cations) and negatively charged ions (anions).

The structure of an ionic compound can be represented using Lewis structures. Let’s take the example of the iodate ion (IO4-). The iodate ion consists of one iodine atom and four oxygen atoms. The iodine atom donates one electron to each of the four oxygen atoms, resulting in the formation of four iodate ions. The iodine atom becomes positively charged (IO4+) and the oxygen atoms become negatively charged (O-).

To represent the iodate ion using a Lewis structure, we start by placing the iodine atom in the center and surrounding it with the four oxygen atoms. Each oxygen atom is connected to the iodine atom by a single bond, represented by a line. The iodine atom has three lone pairs of electrons, represented by dots, and each oxygen atom has one lone pair of electrons.

By following the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a stable configuration with eight valence electrons, we can determine the electron distribution in the iodate ion. The iodine atom has a complete octet, while each oxygen atom has a complete octet as well.

In summary, Lewis structures provide a visual representation of the bonding and electron distribution in molecules and ions. They help us understand the structure and properties of compounds, including ionic compounds like the iodate ion. By analyzing Lewis structures, we can predict the behavior of molecules and ions in chemical reactions.

Lewis Structure of Periodate Ion (IO4-)

The Lewis structure of the periodate ion (IO4-) is a visual representation of the arrangement of atoms and electrons in the molecule. It provides valuable insights into the bonding and geometry of the ion. In this section, we will explore the composition of IO4-, the steps to draw its Lewis structure, the resonance structures involved, and the characteristics of its Lewis structure.

Composition of IO4- and its Elements

The periodate ion (IO4-) is composed of one iodine atom (I) and four oxygen atoms (O). Iodine is a halogen element, while oxygen is a non-metal. The iodine atom is the central atom in the IO4- ion, surrounded by four oxygen atoms. Each oxygen atom forms a single bond with the iodine atom, resulting in a tetrahedral arrangement.

Steps to Draw the Lewis Structure of IO4-

Drawing the Lewis structure of IO4- involves a series of steps that help us determine the arrangement of atoms and electrons. Let’s go through these steps:

Determine the total number of valence electrons: For IO4-, we need to consider the valence electrons of iodine (7) and oxygen (6 each). Since there are four oxygen atoms, the total number of valence electrons is 7 + 4(6) + 1 = 32.
Identify the central atom: In IO4-, the iodine atom is the central atom due to its lower electronegativity compared to oxygen.
Connect the central atom with the surrounding atoms: Draw a single bond between the iodine atom and each oxygen atom.
Distribute the remaining electrons: Place the remaining electrons around the atoms to satisfy the octet rule. Start by placing them on the oxygen atoms, and then distribute any remaining electrons on the iodine atom.
Check for octet rule compliance: Ensure that all atoms, except hydrogen, have an octet of electrons. If any atoms lack an octet, form multiple bonds by converting lone pairs into bonding pairs.
Determine the formal charges: Calculate the formal charges on each atom by comparing the number of valence electrons with the number of electrons assigned to the atom. Minimize formal charges whenever possible.
Assign lone pairs and double bonds: If necessary, convert lone pairs into double bonds to achieve a more stable arrangement.

Resonance Structures of IO4-

Resonance structures are different representations of a molecule that can be obtained by moving electrons or electron pairs. In the case of IO4-, the presence of multiple oxygen atoms allows for the formation of resonance structures. These structures differ in the arrangement of double bonds and the distribution of electrons. The resonance structures of IO4- contribute to its stability and reactivity.

Characteristics of IO4- Lewis Structure

The Lewis structure of IO4- exhibits several characteristics worth noting:

Tetrahedral geometry: The IO4- ion adopts a tetrahedral geometry due to the arrangement of four oxygen atoms around the central iodine atom.
Multiple resonance structures: IO4- can have multiple resonance structures due to the delocalization of electrons. This contributes to its stability and reactivity.
Formal charges: The Lewis structure of IO4- allows for the distribution of formal charges to achieve a more stable arrangement. Minimizing formal charges helps to determine the most likely resonance structure.
Bond angles: The bond angles in IO4- are approximately 109.5 degrees, which is characteristic of a tetrahedral arrangement.

In conclusion, understanding the Lewis structure of the periodate ion (IO4-) provides valuable insights into its bonding, geometry, and reactivity. By following the steps outlined above, we can accurately draw the Lewis structure of IO4- and appreciate its resonance structures and characteristics.

Lewis Dot Structure of C2Cl4

Explanation of C2Cl4 and its elements

C2Cl4, also known as tetrachloroethylene or perchloroethylene, is a colorless liquid with a sweet odor. It is commonly used as a solvent in dry cleaning and metal degreasing processes. The molecule consists of two carbon atoms (C2) and four chlorine atoms (Cl4). Carbon is a nonmetal, while chlorine is a halogen. Understanding the Lewis dot structure of C2Cl4 helps us visualize the arrangement of its atoms and the distribution of valence electrons.

Steps to draw the Lewis dot structure of C2Cl4

Drawing the Lewis dot structure of C2Cl4 involves several steps:

Determine the total number of valence electrons: To do this, count the valence electrons of each atom in the molecule. Carbon has four valence electrons, and chlorine has seven. Since there are two carbon atoms and four chlorine atoms, the total number of valence electrons is (2 × 4) + (4 × 7) = 34.
Determine the central atom: In C2Cl4, carbon is the central atom because it is less electronegative than chlorine. Carbon can form multiple bonds, making it suitable for the central position.
Connect the atoms with single bonds: Start by connecting each chlorine atom to the central carbon atom with a single bond. This step ensures that each atom has a full outer shell of electrons.
Distribute the remaining electrons: After connecting the atoms with single bonds, distribute the remaining valence electrons around the atoms to satisfy the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable configuration with eight valence electrons.
Check for octets and adjust bonds if necessary: After distributing the electrons, check if each atom has an octet of electrons. If any atom does not have an octet, convert one or more of the lone pairs on adjacent atoms into bonding pairs to form double or triple bonds.

Characteristics of C2Cl4 Lewis dot structure

The Lewis dot structure of C2Cl4 reveals several important characteristics:

Carbon forms double bonds with each chlorine atom: In the Lewis dot structure of C2Cl4, carbon forms double bonds with each of the four chlorine atoms. This allows carbon to achieve an octet of electrons, while each chlorine atom has a full outer shell.
The molecule has a tetrahedral shape: The arrangement of the atoms in the Lewis dot structure of C2Cl4 results in a tetrahedral shape. The central carbon atom is surrounded by four chlorine atoms, forming a regular tetrahedron.
The molecule is nonpolar: Due to the symmetrical arrangement of the chlorine atoms around the central carbon atom, the molecule is nonpolar. This means that the electron distribution is even, and there is no separation of positive and negative charges within the molecule.

In conclusion, the Lewis dot structure of C2Cl4 helps us understand the arrangement of its atoms and the distribution of valence electrons. By following the steps outlined above, we can draw an accurate representation of the molecule and identify its key characteristics.

Lewis Structure of C2H4

Ethene, also known as ethylene, is a chemical compound with the molecular formula C2H4. In this section, we will explore the Lewis structure of C2H4, which provides a visual representation of how the atoms are bonded together in the molecule.

Composition of C2H4 and its Elements

C2H4 consists of two carbon (C) atoms and four hydrogen (H) atoms. Carbon is a versatile element that forms the backbone of many organic compounds, while hydrogen is the simplest and most abundant element in the universe. The combination of these elements in C2H4 gives rise to its unique properties and reactivity.

Steps to draw the Lewis structure of C2H4

Drawing the Lewis structure of C2H4 involves a series of steps that help us understand the bonding and electron distribution within the molecule. Here’s a step-by-step guide to drawing the Lewis structure of C2H4:

Determine the total number of valence electrons: To do this, add up the valence electrons of each atom in the molecule. Carbon has four valence electrons, while hydrogen has one valence electron. In C2H4, we have 2 carbon atoms (2 × 4 = 8 valence electrons) and 4 hydrogen atoms (4 × 1 = 4 valence electrons), giving us a total of 12 valence electrons.
Identify the central atom: In C2H4, one carbon atom will act as the central atom, while the other carbon atom and the hydrogen atoms will be bonded to it.
Connect the atoms with single bonds: Start by connecting the central carbon atom to the other carbon atom and the hydrogen atoms using single bonds. Each single bond represents two electrons.
Distribute the remaining electrons: After connecting the atoms with single bonds, distribute the remaining electrons around the atoms to satisfy the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.
Check for octets and adjust: Once you have distributed the electrons, check if all atoms (except hydrogen) have achieved an octet. If any atom is short of electrons, form double or triple bonds as needed to complete the octet.
Determine the formal charges: Formal charges are used to determine the most stable Lewis structure. To calculate the formal charge of an atom, subtract the number of lone pair electrons and half the number of shared electrons from the number of valence electrons. Aim for a Lewis structure with minimal formal charges.

Characteristics of C2H4 Lewis Structure

The Lewis structure of C2H4 reveals several important characteristics about the molecule:

Double bond: The central carbon atom in C2H4 forms a double bond with the other carbon atom. This double bond consists of two shared electron pairs, contributing to the overall stability of the molecule.
Unshared electrons: Each carbon atom in C2H4 has two unshared (or lone pair) electrons. These electrons are not involved in bonding and are located in regions of high electron density around the carbon atoms.
Linear geometry: The Lewis structure of C2H4 shows that the molecule has a linear geometry. This means that the carbon atoms and hydrogen atoms are arranged in a straight line, with a bond angle of approximately 180 degrees.
Nonpolar molecule: Due to its linear geometry and symmetrical distribution of electrons, C2H4 is a nonpolar molecule. This means that the electron density is evenly distributed, resulting in no significant positive or negative charges at different regions of the molecule.

In conclusion, the Lewis structure of C2H4 provides valuable insights into the bonding and electron distribution within the molecule. By following the steps outlined above, we can accurately depict the arrangement of atoms and electrons in C2H4, allowing us to better understand its chemical properties and behavior.

Understanding Ionic Structures

Ionic compounds are an essential part of chemistry, playing a crucial role in various chemical reactions and processes. In this section, we will explore the definition and properties of ionic compounds, how ionic bonding works, and the importance of understanding ionic structures.

Definition and Properties of Ionic Compounds

Ionic compounds are formed through the transfer of electrons between atoms. They consist of positively charged ions, known as cations, and negatively charged ions, known as anions. These ions are held together by electrostatic forces, creating a strong bond.

One key property of ionic compounds is their high melting and boiling points. This is due to the strong electrostatic forces between the ions, which require a significant amount of energy to break. Additionally, ionic compounds are typically solid at room temperature and have a crystalline structure.

Another important property of ionic compounds is their ability to conduct electricity when dissolved in water or melted. This is because the ions are free to move and carry electric charge. However, in their solid state, ionic compounds are not conductive as the ions are held in fixed positions.

How Ionic Bonding Works

Ionic bonding occurs when there is a large difference in electronegativity between two atoms. Electronegativity is a measure of an atom’s ability to attract electrons towards itself. In an ionic bond, one atom, usually a metal, donates electrons to another atom, typically a nonmetal.

Let’s take the example of the iodate ion (IO4-). The iodate ion consists of one iodine atom and four oxygen atoms. Iodine has a lower electronegativity compared to oxygen, resulting in the transfer of electrons from iodine to oxygen.

The iodine atom loses one electron to form a cation with a +1 charge (IO4+), while each oxygen atom gains one electron to form an anion with a -1 charge. The resulting ions are attracted to each other due to their opposite charges, forming an ionic bond.

Importance of Ionic Structures

Understanding ionic structures is crucial for various reasons. Firstly, it allows us to predict the properties and behavior of ionic compounds. By knowing the arrangement of ions in a crystal lattice, we can determine factors such as melting point, solubility, and conductivity.

Additionally, knowledge of ionic structures is essential for studying chemical reactions involving ionic compounds. The arrangement of ions in a crystal lattice affects the ease with which ions can move and react with other substances. This understanding is vital in fields such as materials science, electrochemistry, and pharmaceutical research.

Furthermore, understanding ionic structures helps in explaining the formation of different types of compounds. By analyzing the electron transfer and the resulting ionic bonds, we can comprehend why certain elements tend to form specific types of compounds and how their structures influence their properties.

In conclusion, ionic structures play a fundamental role in chemistry. They provide insights into the properties and behavior of ionic compounds, facilitate the understanding of chemical reactions, and explain the formation of various compounds. By delving into the intricacies of ionic bonding and structures, we can unlock a deeper understanding of the world of chemistry.

Finding Lewis Structures

Lewis structures are diagrams that represent the arrangement of atoms and electrons in a molecule or ion. They provide a visual representation of the valence electrons and help us understand the bonding and geometry of a molecule. In this section, we will discuss the general steps to find Lewis structures and provide examples to illustrate the process.

General Steps to Find Lewis Structures

Finding the Lewis structure of a molecule or ion involves a systematic approach. Here are the general steps to follow:

Determine the total number of valence electrons: Valence electrons are the electrons in the outermost energy level of an atom. To find the total number of valence electrons in a molecule or ion, add up the valence electrons of each atom. For example, in IO4-, we have one iodine atom (group 7A) and four oxygen atoms (group 6A), giving us a total of 32 valence electrons (7 + 4(6) + 1 = 32).
Identify the central atom: The central atom is usually the least electronegative atom in the molecule or ion. In IO4-, iodine (I) is the central atom.
Connect the atoms: Draw a skeletal structure by connecting the atoms with single bonds. In IO4-, iodine is connected to each oxygen atom with a single bond.
Distribute the remaining electrons: Distribute the remaining electrons around the atoms to satisfy the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons. Start by placing the remaining electrons around the outer atoms, and then distribute the remaining electrons around the central atom.
Check for octet rule fulfillment: After distributing the electrons, check if all atoms have achieved an octet (except hydrogen, which can have a duet). If any atoms do not have an octet, try forming multiple bonds or expanding the octet of the central atom if necessary.
Assign formal charges: Formal charges are used to determine the most stable Lewis structure. To calculate the formal charge of an atom, subtract the number of lone pair electrons and half the number of shared electrons from the number of valence electrons. Aim for the structure with the lowest formal charges on the atoms.

Examples of Lewis Structures

Let’s apply the general steps to find the Lewis structure of IO4- and illustrate the process:

Determine the total number of valence electrons: Iodine (group 7A) has 7 valence electrons, and each oxygen atom (group 6A) has 6 valence electrons. Therefore, IO4- has a total of 32 valence electrons.
Identify the central atom: Iodine (I) is the central atom in IO4-.
Connect the atoms: Connect iodine to each oxygen atom with a single bond.
Distribute the remaining electrons: Place the remaining electrons around the oxygen atoms, satisfying the octet rule. Distribute the remaining electrons around the central iodine atom.
Check for octet rule fulfillment: After distributing the electrons, we find that all atoms have achieved an octet.
Assign formal charges: Calculate the formal charges on each atom to determine the most stable Lewis structure.

By following these steps, we find that the Lewis structure of IO4- has four oxygen atoms bonded to the central iodine atom, with each oxygen atom having a single bond and a lone pair of electrons. The iodine atom has a formal charge of -1, and each oxygen atom has a formal charge of 0.

In summary, Lewis structures provide a valuable tool for understanding the bonding and geometry of molecules and ions. By following the general steps outlined above, we can determine the Lewis structure of a given molecule or ion.

Lewis Dot Structure of IO3-

The Lewis dot structure is a way to represent the valence electrons of atoms in a molecule or ion. In this section, we will explore the Lewis dot structure of IO3- (iodate ion) and understand its elements, the steps to draw its structure, and its characteristics.

Explanation of IO3- and its elements

IO3- is an ion formed by iodine (I) and oxygen (O). It is a polyatomic ion, meaning it consists of multiple atoms bonded together. In the case of IO3-, it consists of one iodine atom bonded to three oxygen atoms, with an overall negative charge of -1.

Iodine is a halogen element and is located in Group 17 of the periodic table. It has seven valence electrons. Oxygen, on the other hand, is a nonmetal element and is located in Group 16 of the periodic table. It has six valence electrons.

Steps to draw the Lewis dot structure of IO3-

Drawing the Lewis dot structure of IO3- involves the following steps:

Determine the total number of valence electrons: To do this, add up the valence electrons of each atom in the ion. In IO3-, iodine contributes 7 valence electrons, while each oxygen contributes 6 valence electrons. Since there are three oxygen atoms, the total number of valence electrons is 7 + (6 x 3) = 25.
Determine the central atom: In IO3-, the iodine atom is the central atom since it is bonded to the oxygen atoms.
Connect the atoms: Draw a single bond between the central iodine atom and each oxygen atom.
Distribute the remaining electrons: Place the remaining electrons around the atoms to satisfy the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.
Check for octet rule fulfillment: Count the total number of electrons around each atom and ensure that they have achieved an octet, except for hydrogen and helium, which follow the duet rule.

Characteristics of IO3- Lewis dot structure

The Lewis dot structure of IO3- has the following characteristics:

The central iodine atom is bonded to three oxygen atoms.
The iodine atom has a formal charge of 0, while each oxygen atom has a formal charge of -1.
The overall charge of the ion is -1, indicated by the negative superscript.
The Lewis dot structure shows the arrangement of valence electrons in the ion, allowing us to understand its bonding and geometry.

In summary, the Lewis dot structure of IO3- provides a visual representation of the valence electrons in the iodate ion. By following the steps mentioned above, we can draw an accurate structure that helps us understand the bonding and characteristics of IO3-.

Thioformaldehyde Lewis Structure

Thioformaldehyde, also known as methylene sulfide, is a chemical compound with the formula CH2S. It is an organic molecule that consists of a carbon atom bonded to two hydrogen atoms and a sulfur atom. In this section, we will explore the composition of thioformaldehyde and its elements, the steps to draw its Lewis structure, and the characteristics of its Lewis structure.

Composition of Thioformaldehyde and its Elements

Thioformaldehyde is composed of three elements: carbon (C), hydrogen (H), and sulfur (S). Carbon is a nonmetal, hydrogen is a diatomic nonmetal, and sulfur is a polyatomic nonmetal. These elements play a crucial role in determining the properties and behavior of thioformaldehyde.

Steps to Draw the Lewis Structure of Thioformaldehyde

Drawing the Lewis structure of thioformaldehyde involves a series of steps that help us understand the arrangement of atoms and electrons in the molecule. Here’s a step-by-step guide to drawing the Lewis structure of thioformaldehyde:

Determine the total number of valence electrons: To do this, add up the valence electrons of each atom in the molecule. Carbon contributes 4 valence electrons, hydrogen contributes 1 valence electron per atom, and sulfur contributes 6 valence electrons.
Identify the central atom: In thioformaldehyde, carbon is the central atom since it can form multiple bonds.
Connect the atoms: Use single bonds to connect the central carbon atom with the hydrogen atoms and the sulfur atom.
Distribute the remaining electrons: Distribute the remaining electrons around the atoms to satisfy the octet rule. Hydrogen atoms only need 2 electrons to achieve a full outer shell, while carbon and sulfur atoms need 8 electrons.
Check for octet rule compliance: Ensure that all atoms, except hydrogen, have a complete octet of electrons. If any atom does not have an octet, form double or triple bonds as needed.
Calculate the formal charges: Calculate the formal charges on each atom to determine the most stable Lewis structure. Minimize formal charges and place any negative charges on the most electronegative atom.

Characteristics of Thioformaldehyde Lewis Structure

The Lewis structure of thioformaldehyde reveals important characteristics about the molecule’s geometry, electron distribution, and bonding. Here are some key features of the thioformaldehyde Lewis structure:

Molecular geometry: The thioformaldehyde molecule has a bent or V-shaped geometry. This is due to the presence of two bonding pairs and one lone pair of electrons around the central carbon atom. The bond angle between the hydrogen atoms is approximately 104.5 degrees.
Electron distribution: The Lewis structure shows that the carbon atom forms two sigma bonds with the hydrogen atoms and one sigma bond with the sulfur atom. Additionally, there is one lone pair of electrons on the carbon atom and three lone pairs on the sulfur atom.
Bonding: Thioformaldehyde exhibits covalent bonding, where electrons are shared between atoms to form stable bonds. The carbon-hydrogen and carbon-sulfur bonds are covalent in nature.

In summary, the Lewis structure of thioformaldehyde provides valuable insights into its molecular geometry, electron distribution, and bonding. Understanding these characteristics helps us comprehend the chemical properties and behavior of thioformaldehyde in various chemical reactions and interactions.
Conclusion

In conclusion, the IO4 Lewis structure is an important concept in chemistry that helps us understand the arrangement of atoms and electrons in a molecule. By following the octet rule and considering the formal charges, we can determine the correct Lewis structure for IO4. The IO4- ion consists of one iodine atom bonded to four oxygen atoms, with a negative charge. This structure allows us to visualize the distribution of electrons and predict the chemical behavior of IO4-. Understanding the Lewis structure of IO4 is crucial for studying its properties and reactions. It serves as a foundation for further exploration of the compound’s behavior in various chemical processes. By mastering the IO4 Lewis structure, we can gain a deeper understanding of the fascinating world of chemistry and its applications in our daily lives.

Frequently Asked Questions

What type of structure do ionic compounds have?

Ionic compounds have a crystal lattice structure, where positively charged ions (cations) are surrounded by negatively charged ions (anions) in a repeating pattern.

What is the Lewis structure of IO4-?

The Lewis structure of IO4- (iodate ion) consists of one iodine atom bonded to four oxygen atoms. The iodine atom has a formal charge of +7, while each oxygen atom has a formal charge of -1.

How to find the Lewis structure?

To find the Lewis structure of a molecule or ion, follow these steps:
1. Determine the total number of valence electrons.
2. Identify the central atom.
3. Connect the atoms with single bonds.
4. Distribute the remaining electrons as lone pairs to satisfy the octet rule.
5. Check the formal charges to ensure they are minimized.

What is the Lewis dot structure of C2H4?

The Lewis dot structure of C2H4 (ethylene) consists of two carbon atoms double bonded to each other and each carbon atom bonded to two hydrogen atoms. Each carbon atom has three lone pairs of electrons.

How does ionic bonding work?

Ionic bonding occurs between a metal and a non-metal. It involves the transfer of electrons from the metal to the non-metal, resulting in the formation of positively charged ions (cations) and negatively charged ions (anions). These oppositely charged ions are then attracted to each other, forming an ionic bond.

What is the Lewis dot structure of IO3-?

The Lewis dot structure of IO3- (iodate ion) consists of one iodine atom bonded to three oxygen atoms. The iodine atom has a formal charge of +5, while each oxygen atom has a formal charge of -1.

What is the Lewis structure of IO4+?

The Lewis structure of IO4+ (iodate ion) consists of one iodine atom bonded to four oxygen atoms. The iodine atom has a formal charge of +5, while each oxygen atom has a formal charge of -1.

What is the molecular geometry of IO4-?

The molecular geometry of IO4- (iodate ion) is tetrahedral. The central iodine atom is surrounded by four oxygen atoms, resulting in a symmetrical arrangement.

What is the bond angle in IO4-?

The bond angle in IO4- (iodate ion) is approximately 109.5 degrees. This is because the molecular geometry of IO4- is tetrahedral, and the bond angles in a tetrahedral arrangement are all equal.

What is the electron geometry of IO4+?

The electron geometry of IO4+ (iodate ion) is also tetrahedral. The central iodine atom is surrounded by four oxygen atoms, resulting in a symmetrical arrangement of electron pairs.

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Dr. Shruti Ramteke

Hello everyone, I am Dr. Shruti M Ramteke, I did my Ph.D. in chemistry. I am passionate about writing and like to share my knowledge with others . Feel free to contact me on linkedin