Ch2cl2 Bond Angle? Molecular Geometry? Hybridization? Polar Or Nonpolar

Dichloromethane (Ch2cl2) – Bond Angle, Molecular Geometry, And Hybridization

Dichloromethane (CH2Cl2) is a chlorinated chemical extensively employed as a solvent. It is among the least harmful chlorohydrocarbons, as well as miscible in a majority of organic solvents.

The CH2Cl2 molecules have a tetrahedral form. This is because it has two chlorine atoms and hydrogen and oxygen atoms.

Bond Angle

When atoms from different parts of the universe join to exchange or share electrons with other atoms, it relies on a range of mathematical variables to establish the proper geometry that will take form. Of these parameters, bonds are paramount and play a significant part in forming geometrical bonds between molecules and atoms.

Molecular Geometry is the 3-D arrangement of the atoms which make the Molecule. It encompasses the general form of the molecules, along with their bond lengths bonds, bond angles, torsion angles, and other parameters of geometrical nature that affect its overall configuration.

In the simplest of chemistry, a molecule is made up of a central atom that is surrounded by a variety of other molecules. They are connected to the central atom via several bonds, which form the electron-electron pair to one another or from lone pairs to surrounding atoms.

The shape and the angles of bonding are defined by mutual Pauli Repulsion between the electron pairs. The more attracted the pairs of electrons are by the element they are around, the less their distance to each other.

Another aspect that affects Molecular Geometry and bond angle is the electronegativity of molecules’ ligands. The higher the electronegativity of molecules’ ligands, the more it presents their electron-bonding electron pairs, and the fewer molecules can exchange electrons with bonding atoms.

So, a molecule having more electron pairs that have been repelled has greater polarity than one with fewer electron pairs that have been repelled. Based on the relative electronegativities of elements, this variation could result in either a negative or positive charge for the Molecule.

Electronegativity refers to the capacity of an atom in an element to draw electrons from the atoms of the compound to itself. This is a significant aspect that determines the polarity of chemical bonds since it could result in the atom becoming positive or negatively charged when it is surrounded by other atoms having less electronegativity.

Similar to the size of an atom, the dimensions of an atom may influence the bond angle as well as molecular shape. The smaller atoms possess more trigonal planar, or helical geometry, than larger ones and are often associated with the VSEPR or valence shell electron pair (VSEPR) model of molecules.

Molecular Geometry

Molecular Geometry is the 3D arrangement of atoms inside the molecules. It may have a variety of shapes, such as tetrahedral, pyramidal linear, angular, and tetrahedral, according to how many atoms are located in the same place within the central atom (considering the lone pair).

Normally, electron pairs oppose each other to stabilize the molecules by moving as far as possible. This process is known as the valence shell electron pair repel or VSEPR, which is the foundation of molecular geometry.

This repulsion is crucial to comprehending the covalent Molecule’s geometry and how it affects crystal structure and the behavior of phase changes, rates and energy for chemical interaction, solubility, and more. Additionally, it has an immediate effect on the chemical Reactivity of the chemical Molecule.

The most basic instance that can be used to illustrate VSEPR could be the octahedral geometrical structure of the XeF4 Molecule, which contains five atoms bonded to one central S atom and two pairs of lone pairs. In this model, the lone pairs are located adjacent to each other on the central atom.

If you have a molecule with five bonds but no lone pair like H2O, the shape of the Molecule will be Tetrahedral. If there is a molecule with two bonds but no lone pair, like carbon dioxide, then the shape of the molecules is linear.

Every Molecule has its specific molecular shape that can be identified using various methods. A few of these methods comprise techniques for spectroscopy, such as infrared microwave, infrared, and Raman spectroscopy. Other methods include diffraction techniques like crystallography with X-rays.

Another method of determining the structure of a molecule is by looking at the state of its hybridization. A hybridization condition of carbon atoms shows how many electrons that bond are distributed throughout the atom.

This can help redistribute this energy and create an entirely new orbital that has the same or more energy. This results in a brand new geometrical model of atomic bonds that can predict the structure of molecules.

The atomic geometry created is known as”the Lewis structure. It is the primary 3D structure found in molecules and is a major influence on every aspect of its chemical properties. For example, the presence of a Lewis structure that is not correct can result in the opposite polarity, which is not favorable for chemical reactions. This is why you must draw correct Lewis shapes when drawing the Molecule.

Hybridization

Hybridization involves mixing the orbitals of atoms to create new orbitals which are not exactly like their predecessors. It is utilized as a part of organic chemistry to determine the structure of molecules. It is also used to determine the electrons’ repulsion in an atom to guarantee the stability of the geometrical structure.

In most cases, hybridization occurs between the s and p orbitals of an atom’s main shell, resulting in two equivalent orbitals. The hybrid orbitals created are called the sp hybridized orbitals.

The sp3 hybridization process of the carbon atom within the CH2Cl2 structure creates a tetrahedral-shaped molecule. The geometry is determined using the valence-shelf electron pair repulsion (VSEPR) theorem.

The theory of VSEPR states that substituents or atoms surrounding an atom’s central point will be in an arrangement that reduces the repulsion between electrons in the valence shell. It also describes the molecular shape of a molecule using numbers of bond pair pairs and single pairs of atoms or substituents.

When there is a huge amount of bonding, it may be challenging to establish stoichiometry and molecules. In this instance, it is the VSEPR theory can help. It explains that substituents or atoms around the atoms in the central Molecule are likely to adopt an arrangement that reduces the repulsive forces, which could help determine the stoichiometry and the molecular structure of a crystallized compound.

It is also why the geometric tetrahedral structure is present inside the CH2Cl2 molecular. The sp3 hybridization of the central carbon atom results in an unchanging tetrahedral shape for CH2Cl2’s Molecule since there aren’t any single pair of carbon atoms on the central atom.

Since there aren’t any lone carbon atoms with a single pair and no electronic repulsion is observed between C-Cl and CH bonds, which results in the stability of a tetrahedral molecular shape within this Molecule.

The theory of molecular orbits states that all the elements of a molecule are responsible for forming molecular orbitals. They are a linear mixture of atomic orbitals. The MO diagram shows that carbon atoms possess 2s as well as 2p orbitals, which are combined with 1s orbitals from the two hydrogen atoms as well as the 2p orbitals associated with the two chlorine atoms to create eight molecular orbitals.

Polarity

Then the polarity of chemical bonds is the different electronegativity of the two atoms covalently bonded. Typically, the greater the electronegativity of an atom and the stronger the bond.

A polar bond is defined as having an exact dipole time (symbol u) that is a vector number that is the product of electric charges (Q) and the length of the bond (r). This dipole moment is normally described in the Debye unit; however, it can also be measured using an Atomic Coordinate System.

In Pauling’s electronegativity scale according to Pauling’s electronegativity scale, a truly polar bond should be able to demonstrate an electronegativity gap among the two bonded molecules of greater than 0.5 units. In the case of the C-Cl bond, it is possible to find an electronegativity variance that is 0.61 units between the carbon atom and the chlorine atom.

It is the greatest electronegativity value for a molecular, which makes it an even more polar bond than nonpolar bonds. A molecule with a higher electronegativity is more likely to have a higher intermolecular attraction to other molecules of the same size.

But this isn’t always the scenario. For instance, a CH bond is characterized by weak dipole moments because of the tiny electronegativity differences between the atoms of the bonding pair. The C-H bond’s polarity in CH4 is offset due to the non-polarity C-Cl bonds that make up the Molecule.

The molecular structure of a molecule determines what nature of the polarity it exhibits. For instance, a trihedral molecule is more polar than an octahedral molecule. In the same way, a seesaw or tri-pyramidal bipyramidal is more polar way than an octahedral.

The polarity of a chemical molecule is defined by its geometrical structure and how it binds to other molecules. Molecular geometries that are extremely symmetrical (particularly tetrahedral and planar) contain distinct bond dipole moments that are canceled, meaning there isn’t a net dipole in the molecular.

Similarly to that, molecules that aren’t symmetrical also have bond dipole moments that are unable to cancel each other, which means it is possible to have a net dipole within the molecules. Examples of such geometries are the V, trigonal pyramidal seesaw, or T-shaped molecules.

Ch2cl2 Lone Pair

CH2Cl2, dichloromethane, is a nonpolar compound commonly employed as a solvent in diverse industries. It is a tetrahedral molecule with geometry. In addition, its Lewis structure will help us to understand its properties and its behavior. In this paper, we will examine the electron pairs that are the only ones found in CH2Cl2 and their roles in the structure and its properties.

Lewis Structure Of Ch2cl2

In order to draw diagrams of the Lewis diagram of the structure CH2Cl2, We first have to determine all the valence electrons within the chemical Molecule. Carbon is home to four electrons in valence, and each chlorine and hydrogen element has one electron in the valence. So, the total amount of valence electrons present in CH2Cl2 is:

1(4) + 2(1) + 2(7) = 20

Then, we organize the Molecule atoms and join them using single bonds. Carbon is the atom that forms the center, and we arrange the two chlorine atoms and two hydrogen atoms in its vicinity. We get the following Skeleton structure:

H – C – Cl

|

Cl

Then, we fill in the electrons of valence around each atom, beginning at the outer atoms before then moving toward the center of the atom. Every hydrogen atom has a Valence electron, and we add two electrons (a one-on-one pair) around every hydrogen atom. Each chlorine atom contains seven electrons in the valence, which is why we have six electrons (two single pairs and bonding electrons) around each chlorine atom. Carbon has four valence electrons; therefore, we put the four electrons (two bonding electrons, two bonding electrons, but no single pairs) around the carbon atom. This results in an example of a Lewis structure:

H:

|

H – C – Cl

|

Cl:

It is important to note that the dots represent the electron pairs that are the only ones, while the lines represent the electrons that bond. The Molecule is made up of one of the molecules that has a complete outer shell of valence, except carbon, with only the number of electrons it has instead. Carbon has formal charges of +1 since it has one less electron than what it would have in the neutral atom. The chlorine atoms, however, have a formal charge of -1 since they each hold one extra electron than in a neutral atom.

Lone Pairs In Ch2cl2

• The Lewis structure in CH2Cl2 shows that every hydrogen atom has two electron pairs around it. Additionally, each chlorine atom has two unique electron pairs surrounding it. Carbon does not have single electrons surrounding it.
• The electrons that are lone pair is the result of pairs of electrons that aren’t involved in bonding and are located around one atom. The lone pairs may affect the form and polarity of molecules, and also its chemical properties and reactivity.
• In CH2Cl2, The existence of single pairs of chlorine atoms makes the Molecule polar. The two chlorine molecules are more electronegative than the hydrogen and carbon atoms. This means that they draw bonding electrons more powerfully. This causes a negative charge to form upon the chlorine atoms as well as an inverse positive charge to be formed on the hydrogen and carbon atoms.
• Additionally, the lone pair on chlorine atoms could take part in hydrogen bonding which is a form of intermolecular force that happens in the hydrogen atom that is bonded to an electronegative atom as well as a lone pair of another molecule. This makes CH2Cl2 an excellent solvent for compounds with polarity but an unsuitable one for nonpolar compounds.
• In the final analysis, it is clear that the Lewis structures of CH2Cl2 indicate that the Molecule is composed of two electron pairs that are lone around each chlorine and hydrogen atom but none around the carbon atom. They play an important impact on the structure and the properties of the Molecule, such as its polarity as well as its solubility.

FAQ’s

What is the hybridization for CH2Cl2?

Tetrahedral hybridization, often known as sp3, is the process in which one s orbital and three p orbitals from the same shell of an atom combine to generate four new equivalent orbitals in the compound CH2Cl.

Is CH2Cl2 polar or non polar?

(a) Because of the polarity difference in the C-Cl bond, the CH2Cl2 molecule is polar in nature. Due to its tetrahedral shape, the net dipole moment does not cancel out the other dipole moments.

What is the bond angle of CH2Cl2?

The electron and molecule geometries are both tetrahedral because the centre atom has four atoms and no lone pairs: The sp3-hybridization with steric number 4 corresponds to idealised bond angles of 109.5o.

Does CH2Cl2 have sp2 hybridization?

As the molecule creates all four of the compound’s bonds, the central carbon undergoes hybridization. Bonds are created by a 22 orbital electron as well as three additional 2p orbital electrons. Therefore, in CH2Cl2, the hybridization of the carbon atom is sp3.

Is CH2F2 sp3 hybridization?

We notice that the molecule contains four covalent connections. This results in a hybridization of sp3 for the central carbon atom and gives us a steric number of 4.

What is the shape and polarity of CH2Cl2?

Although individual bond dipoles do not cancel one another, dichloromethane CH2Cl2, commonly known as methylene dichloride, is a polar molecule. Tetrahedral geometry describes the molecule.

Ch2cl2 Bond Angle? Molecular Geometry? Hybridization? Polar Or Nonpolar

Dichloromethane (Ch2cl2) – Bond Angle, Molecular Geometry, And Hybridization

Dichloromethane (CH2Cl2) is a chlorinated chemical extensively employed as a solvent. It is among the least harmful chlorohydrocarbons, as well as miscible in a majority of organic solvents.

The CH2Cl2 molecules have a tetrahedral form. This is because it has two chlorine atoms and hydrogen and oxygen atoms.

Bond Angle

When atoms from different parts of the universe join to exchange or share electrons with other atoms, it relies on a range of mathematical variables to establish the proper geometry that will take form. Of these parameters, bonds are paramount and play a significant part in forming geometrical bonds between molecules and atoms.

Molecular Geometry is the 3-D arrangement of the atoms which make the Molecule. It encompasses the general form of the molecules, along with their bond lengths bonds, bond angles, torsion angles, and other parameters of geometrical nature that affect its overall configuration.

In the simplest of chemistry, a molecule is made up of a central atom that is surrounded by a variety of other molecules. They are connected to the central atom via several bonds, which form the electron-electron pair to one another or from lone pairs to surrounding atoms.

The shape and the angles of bonding are defined by mutual Pauli Repulsion between the electron pairs. The more attracted the pairs of electrons are by the element they are around, the less their distance to each other.

Another aspect that affects Molecular Geometry and bond angle is the electronegativity of molecules’ ligands. The higher the electronegativity of molecules’ ligands, the more it presents their electron-bonding electron pairs, and the fewer molecules can exchange electrons with bonding atoms.

So, a molecule having more electron pairs that have been repelled has greater polarity than one with fewer electron pairs that have been repelled. Based on the relative electronegativities of elements, this variation could result in either a negative or positive charge for the Molecule.

Electronegativity refers to the capacity of an atom in an element to draw electrons from the atoms of the compound to itself. This is a significant aspect that determines the polarity of chemical bonds since it could result in the atom becoming positive or negatively charged when it is surrounded by other atoms having less electronegativity.

Similar to the size of an atom, the dimensions of an atom may influence the bond angle as well as molecular shape. The smaller atoms possess more trigonal planar, or helical geometry, than larger ones and are often associated with the VSEPR or valence shell electron pair (VSEPR) model of molecules.

Molecular Geometry

Molecular Geometry is the 3D arrangement of atoms inside the molecules. It may have a variety of shapes, such as tetrahedral, pyramidal linear, angular, and tetrahedral, according to how many atoms are located in the same place within the central atom (considering the lone pair).

Normally, electron pairs oppose each other to stabilize the molecules by moving as far as possible. This process is known as the valence shell electron pair repel or VSEPR, which is the foundation of molecular geometry.

This repulsion is crucial to comprehending the covalent Molecule’s geometry and how it affects crystal structure and the behavior of phase changes, rates and energy for chemical interaction, solubility, and more. Additionally, it has an immediate effect on the chemical Reactivity of the chemical Molecule.

The most basic instance that can be used to illustrate VSEPR could be the octahedral geometrical structure of the XeF4 Molecule, which contains five atoms bonded to one central S atom and two pairs of lone pairs. In this model, the lone pairs are located adjacent to each other on the central atom.

If you have a molecule with five bonds but no lone pair like H2O, the shape of the Molecule will be Tetrahedral. If there is a molecule with two bonds but no lone pair, like carbon dioxide, then the shape of the molecules is linear.

Every Molecule has its specific molecular shape that can be identified using various methods. A few of these methods comprise techniques for spectroscopy, such as infrared microwave, infrared, and Raman spectroscopy. Other methods include diffraction techniques like crystallography with X-rays.

Another method of determining the structure of a molecule is by looking at the state of its hybridization. A hybridization condition of carbon atoms shows how many electrons that bond are distributed throughout the atom.

This can help redistribute this energy and create an entirely new orbital that has the same or more energy. This results in a brand new geometrical model of atomic bonds that can predict the structure of molecules.

The atomic geometry created is known as”the Lewis structure. It is the primary 3D structure found in molecules and is a major influence on every aspect of its chemical properties. For example, the presence of a Lewis structure that is not correct can result in the opposite polarity, which is not favorable for chemical reactions. This is why you must draw correct Lewis shapes when drawing the Molecule.

Hybridization

Hybridization involves mixing the orbitals of atoms to create new orbitals which are not exactly like their predecessors. It is utilized as a part of organic chemistry to determine the structure of molecules. It is also used to determine the electrons’ repulsion in an atom to guarantee the stability of the geometrical structure.

In most cases, hybridization occurs between the s and p orbitals of an atom’s main shell, resulting in two equivalent orbitals. The hybrid orbitals created are called the sp hybridized orbitals.

The sp3 hybridization process of the carbon atom within the CH2Cl2 structure creates a tetrahedral-shaped molecule. The geometry is determined using the valence-shelf electron pair repulsion (VSEPR) theorem.

The theory of VSEPR states that substituents or atoms surrounding an atom’s central point will be in an arrangement that reduces the repulsion between electrons in the valence shell. It also describes the molecular shape of a molecule using numbers of bond pair pairs and single pairs of atoms or substituents.

When there is a huge amount of bonding, it may be challenging to establish stoichiometry and molecules. In this instance, it is the VSEPR theory can help. It explains that substituents or atoms around the atoms in the central Molecule are likely to adopt an arrangement that reduces the repulsive forces, which could help determine the stoichiometry and the molecular structure of a crystallized compound.

It is also why the geometric tetrahedral structure is present inside the CH2Cl2 molecular. The sp3 hybridization of the central carbon atom results in an unchanging tetrahedral shape for CH2Cl2’s Molecule since there aren’t any single pair of carbon atoms on the central atom.

Since there aren’t any lone carbon atoms with a single pair and no electronic repulsion is observed between C-Cl and CH bonds, which results in the stability of a tetrahedral molecular shape within this Molecule.

The theory of molecular orbits states that all the elements of a molecule are responsible for forming molecular orbitals. They are a linear mixture of atomic orbitals. The MO diagram shows that carbon atoms possess 2s as well as 2p orbitals, which are combined with 1s orbitals from the two hydrogen atoms as well as the 2p orbitals associated with the two chlorine atoms to create eight molecular orbitals.

Polarity

Then the polarity of chemical bonds is the different electronegativity of the two atoms covalently bonded. Typically, the greater the electronegativity of an atom and the stronger the bond.

A polar bond is defined as having an exact dipole time (symbol u) that is a vector number that is the product of electric charges (Q) and the length of the bond (r). This dipole moment is normally described in the Debye unit; however, it can also be measured using an Atomic Coordinate System.

In Pauling’s electronegativity scale according to Pauling’s electronegativity scale, a truly polar bond should be able to demonstrate an electronegativity gap among the two bonded molecules of greater than 0.5 units. In the case of the C-Cl bond, it is possible to find an electronegativity variance that is 0.61 units between the carbon atom and the chlorine atom.

It is the greatest electronegativity value for a molecular, which makes it an even more polar bond than nonpolar bonds. A molecule with a higher electronegativity is more likely to have a higher intermolecular attraction to other molecules of the same size.

But this isn’t always the scenario. For instance, a CH bond is characterized by weak dipole moments because of the tiny electronegativity differences between the atoms of the bonding pair. The C-H bond’s polarity in CH4 is offset due to the non-polarity C-Cl bonds that make up the Molecule.

The molecular structure of a molecule determines what nature of the polarity it exhibits. For instance, a trihedral molecule is more polar than an octahedral molecule. In the same way, a seesaw or tri-pyramidal bipyramidal is more polar way than an octahedral.

The polarity of a chemical molecule is defined by its geometrical structure and how it binds to other molecules. Molecular geometries that are extremely symmetrical (particularly tetrahedral and planar) contain distinct bond dipole moments that are canceled, meaning there isn’t a net dipole in the molecular.

Similarly to that, molecules that aren’t symmetrical also have bond dipole moments that are unable to cancel each other, which means it is possible to have a net dipole within the molecules. Examples of such geometries are the V, trigonal pyramidal seesaw, or T-shaped molecules.

Ch2cl2 Lone Pair

CH2Cl2, dichloromethane, is a nonpolar compound commonly employed as a solvent in diverse industries. It is a tetrahedral molecule with geometry. In addition, its Lewis structure will help us to understand its properties and its behavior. In this paper, we will examine the electron pairs that are the only ones found in CH2Cl2 and their roles in the structure and its properties.

Lewis Structure Of Ch2cl2

In order to draw diagrams of the Lewis diagram of the structure CH2Cl2, We first have to determine all the valence electrons within the chemical Molecule. Carbon is home to four electrons in valence, and each chlorine and hydrogen element has one electron in the valence. So, the total amount of valence electrons present in CH2Cl2 is:

1(4) + 2(1) + 2(7) = 20

Then, we organize the Molecule atoms and join them using single bonds. Carbon is the atom that forms the center, and we arrange the two chlorine atoms and two hydrogen atoms in its vicinity. We get the following Skeleton structure:

H – C – Cl

|

Cl

Then, we fill in the electrons of valence around each atom, beginning at the outer atoms before then moving toward the center of the atom. Every hydrogen atom has a Valence electron, and we add two electrons (a one-on-one pair) around every hydrogen atom. Each chlorine atom contains seven electrons in the valence, which is why we have six electrons (two single pairs and bonding electrons) around each chlorine atom. Carbon has four valence electrons; therefore, we put the four electrons (two bonding electrons, two bonding electrons, but no single pairs) around the carbon atom. This results in an example of a Lewis structure:

H:

|

H – C – Cl

|

Cl:

It is important to note that the dots represent the electron pairs that are the only ones, while the lines represent the electrons that bond. The Molecule is made up of one of the molecules that has a complete outer shell of valence, except carbon, with only the number of electrons it has instead. Carbon has formal charges of +1 since it has one less electron than what it would have in the neutral atom. The chlorine atoms, however, have a formal charge of -1 since they each hold one extra electron than in a neutral atom.

Lone Pairs In Ch2cl2

• The Lewis structure in CH2Cl2 shows that every hydrogen atom has two electron pairs around it. Additionally, each chlorine atom has two unique electron pairs surrounding it. Carbon does not have single electrons surrounding it.
• The electrons that are lone pair is the result of pairs of electrons that aren’t involved in bonding and are located around one atom. The lone pairs may affect the form and polarity of molecules, and also its chemical properties and reactivity.
• In CH2Cl2, The existence of single pairs of chlorine atoms makes the Molecule polar. The two chlorine molecules are more electronegative than the hydrogen and carbon atoms. This means that they draw bonding electrons more powerfully. This causes a negative charge to form upon the chlorine atoms as well as an inverse positive charge to be formed on the hydrogen and carbon atoms.
• Additionally, the lone pair on chlorine atoms could take part in hydrogen bonding which is a form of intermolecular force that happens in the hydrogen atom that is bonded to an electronegative atom as well as a lone pair of another molecule. This makes CH2Cl2 an excellent solvent for compounds with polarity but an unsuitable one for nonpolar compounds.
• In the final analysis, it is clear that the Lewis structures of CH2Cl2 indicate that the Molecule is composed of two electron pairs that are lone around each chlorine and hydrogen atom but none around the carbon atom. They play an important impact on the structure and the properties of the Molecule, such as its polarity as well as its solubility.

FAQ’s

What is the hybridization for CH2Cl2?

Tetrahedral hybridization, often known as sp3, is the process in which one s orbital and three p orbitals from the same shell of an atom combine to generate four new equivalent orbitals in the compound CH2Cl.

Is CH2Cl2 polar or non polar?

(a) Because of the polarity difference in the C-Cl bond, the CH2Cl2 molecule is polar in nature. Due to its tetrahedral shape, the net dipole moment does not cancel out the other dipole moments.

What is the bond angle of CH2Cl2?

The electron and molecule geometries are both tetrahedral because the centre atom has four atoms and no lone pairs: The sp3-hybridization with steric number 4 corresponds to idealised bond angles of 109.5o.

Does CH2Cl2 have sp2 hybridization?

As the molecule creates all four of the compound’s bonds, the central carbon undergoes hybridization. Bonds are created by a 22 orbital electron as well as three additional 2p orbital electrons. Therefore, in CH2Cl2, the hybridization of the carbon atom is sp3.

Is CH2F2 sp3 hybridization?

We notice that the molecule contains four covalent connections. This results in a hybridization of sp3 for the central carbon atom and gives us a steric number of 4.

What is the shape and polarity of CH2Cl2?

Although individual bond dipoles do not cancel one another, dichloromethane CH2Cl2, commonly known as methylene dichloride, is a polar molecule. Tetrahedral geometry describes the molecule.