Nonpolar Covalent Bond Electronegativity Examples
Nonpolar covalent bonds occur when two atoms share electrons equally due to similar electronegativities. In these bonds, the electrons are not pulled towards one atom more strongly than the other, resulting in a balanced distribution of charge. Let’s explore some examples of nonpolar covalent bonds and their properties.
Nitrogen (N2)
Nitrogen gas (N2) is a diatomic molecule composed of two nitrogen atoms. In this molecule, the two nitrogen atoms are connected by a nonpolar covalent bond. The electronegativity of nitrogen is similar, so the shared electrons are equally distributed between the two atoms. As a result, nitrogen gas is a nonpolar molecule.
Dinitrogen Tetroxide (N2O4)
Dinitrogen tetroxide (N2O4) is a molecular compound composed of two nitrogen atoms and four oxygen atoms. The nitrogen-nitrogen bond in N2O4 is nonpolar covalent because the electronegativity of nitrogen is similar. The oxygen atoms, on the other hand, have a higher electronegativity, resulting in polar covalent bonds between nitrogen and oxygen.
Dinitrogen Difluoride (N2F2)
Dinitrogen difluoride (N2F2) is another example of a compound with a nonpolar covalent bond. It consists of two nitrogen atoms and two fluorine atoms. Since nitrogen and fluorine have similar electronegativities, the shared electrons are evenly distributed between the atoms, making the N-N and N-F bonds nonpolar.
Nitrate Ion (NO3-)
The nitrate ion (NO3-) is a polyatomic ion composed of one nitrogen atom and three oxygen atoms. The nitrogen-oxygen bonds in the nitrate ion are polar covalent due to the difference in electronegativity. However, the overall molecule is nonpolar because the three oxygen atoms are arranged symmetrically around the central nitrogen atom, canceling out the polarity.
Boron Trifluoride (BF3)
Boron trifluoride (BF3) is a compound consisting of one boron atom and three fluorine atoms. The boron-fluorine bonds in BF3 are nonpolar covalent because boron and fluorine have similar electronegativities. The molecule itself is nonpolar due to its trigonal planar shape, which results in a symmetrical distribution of charge.
Carbon Dioxide (CO2)
Carbon dioxide (CO2) is a well-known example of a nonpolar molecule. It consists of one carbon atom and two oxygen atoms. The carbon-oxygen bonds in CO2 are polar covalent due to the difference in electronegativity. However, the molecule is nonpolar overall because the two polar bonds are arranged symmetrically, resulting in a balanced distribution of charge.
Methane (CH4)
Methane (CH4) is a hydrocarbon compound composed of one carbon atom and four hydrogen atoms. The carbon-hydrogen bonds in methane are nonpolar covalent because carbon and hydrogen have similar electronegativities. The molecule itself is nonpolar due to its tetrahedral shape, which results in a symmetrical distribution of charge.
Benzene (C6H6)
Benzene (C6H6) is an aromatic hydrocarbon consisting of six carbon atoms and six hydrogen atoms. The carbon-carbon bonds in benzene are nonpolar covalent because carbon has similar electronegativity. The molecule itself is nonpolar due to its hexagonal shape and symmetrical distribution of charge.
In summary, nonpolar covalent bonds occur when two atoms share electrons equally due to similar electronegativities. Examples of compounds with nonpolar covalent bonds include nitrogen gas, dinitrogen tetroxide, dinitrogen difluoride, nitrate ion, boron trifluoride, carbon dioxide, methane, and benzene. Understanding these examples helps us comprehend the concept of nonpolar covalent bonds and their role in molecular compounds.
Dihydrogen (H2)
Dihydrogen, commonly known as hydrogen gas, is a prime example of a nonpolar covalent bond. In this section, we will explore the nature of the dihydrogen molecule and how it exemplifies nonpolar covalent bonding.
Carbon tetrachloride (CCl4)
Carbon tetrachloride, with the chemical formula CCl4, is a molecular compound that showcases nonpolar covalent bonding. Let’s delve into the characteristics of carbon tetrachloride and understand why it is considered a nonpolar molecule.
Carbon tetrachloride consists of one carbon atom bonded to four chlorine atoms. Each chlorine atom shares one electron with the carbon atom, resulting in a total of four shared electron pairs. These shared electron pairs form covalent bonds, where electrons are shared between atoms.
In a nonpolar covalent bond, the electrons are shared equally between the atoms involved. This occurs when the atoms have similar electronegativity values, which is a measure of an atom’s ability to attract electrons towards itself. In the case of carbon tetrachloride, carbon and chlorine have comparable electronegativity values, resulting in equal sharing of electrons.
The equal sharing of electrons in carbon tetrachloride leads to a symmetrical distribution of charge within the molecule. This symmetry cancels out any dipole moments, which are the separation of positive and negative charges within a molecule. As a result, carbon tetrachloride has a net dipole moment of zero, making it a nonpolar molecule.
To further illustrate this, let’s take a look at the Lewis structure of carbon tetrachloride:
| Atom | Valence Electrons |
|---|---|
| Carbon | 4 |
| Chlorine | 7 |
In the Lewis structure, carbon is represented by the symbol C, and each chlorine atom is represented by the symbol Cl. The valence electrons of each atom are indicated by dots surrounding the atomic symbol.
Cl
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.
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Cl-C-Cl
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Cl
As you can see, each chlorine atom shares one electron with the carbon atom, resulting in four shared electron pairs. This equal sharing of electrons contributes to the nonpolar nature of carbon tetrachloride.
Carbon tetrachloride finds applications in various industries, including as a solvent for oils, fats, and waxes. It is also used in fire extinguishers and as a refrigerant. Understanding its nonpolar covalent bonding helps us comprehend its chemical properties and applications.
In conclusion, carbon tetrachloride is an example of a nonpolar covalent bond. Its equal sharing of electrons between carbon and chlorine atoms results in a symmetrical distribution of charge, making it a nonpolar molecule. By exploring different examples of nonpolar covalent bonds, we gain a deeper understanding of chemical bonding and its impact on molecular compounds.
Nonpolar vs Polar Covalent Bond Examples
In chemical bonding, covalent bonds are formed when atoms share electrons. These bonds can be classified as either polar or nonpolar, depending on the electronegativity of the atoms involved. In this section, we will explore some examples of nonpolar and polar covalent bonds to better understand their characteristics and properties.
Nitrogen (N2) – Nonpolar Covalent Bond
One of the most well-known examples of a nonpolar covalent bond is found in the nitrogen molecule (N2). Nitrogen gas is composed of two nitrogen atoms that are bonded together by a nonpolar covalent bond.
In a nonpolar covalent bond, the electrons are shared equally between the atoms involved. This occurs when the electronegativity difference between the atoms is very small or nonexistent. In the case of nitrogen gas, both nitrogen atoms have the same electronegativity value, resulting in equal sharing of the electrons.
The equal sharing of electrons in a nonpolar covalent bond leads to a symmetrical distribution of charge. This means that there are no partial positive or negative charges on the atoms, resulting in a molecule that is overall electrically neutral. As a result, nitrogen gas does not have any significant dipole moment and is considered a nonpolar molecule.
Water (H2O) – Polar Covalent Bond
In contrast to nonpolar covalent bonds, polar covalent bonds occur when there is an unequal sharing of electrons between the atoms involved. This unequal sharing is due to differences in electronegativity between the atoms. A classic example of a polar covalent bond can be found in the water molecule (H2O).
In water, the oxygen atom is more electronegative than the hydrogen atoms. As a result, the oxygen atom attracts the shared electrons more strongly, creating a partial negative charge (δ-) on the oxygen atom and partial positive charges (δ+) on the hydrogen atoms. This uneven distribution of charge gives rise to a dipole moment in the water molecule.
The polar nature of the covalent bond in water has important implications for its properties. For example, water exhibits a high boiling point and melting point compared to similar-sized molecules with nonpolar covalent bonds. This is due to the presence of hydrogen bonding, which is a type of intermolecular force that occurs between the δ+ hydrogen atom of one water molecule and the δ- oxygen atom of another water molecule.
The polarity of the covalent bond in water also contributes to its ability to dissolve many substances. Water is often referred to as the “universal solvent” because of its ability to dissolve a wide range of ionic and polar compounds. This is because the positive and negative ends of the water molecules can interact with the charged particles of the solute, allowing them to be surrounded and dispersed in the water.
In summary, nonpolar and polar covalent bonds differ in terms of the electronegativity of the atoms involved and the distribution of charge within the molecule. Nonpolar covalent bonds occur when there is equal sharing of electrons, resulting in a molecule with no significant dipole moment. Polar covalent bonds, on the other hand, involve an unequal sharing of electrons, leading to the presence of partial positive and negative charges and the formation of a dipole moment. Understanding the nature of these bonds is crucial in explaining the properties and behavior of different molecular compounds.
Nonpolar Covalent Bond Examples
In chemical bonding, covalent bonds are formed when atoms share electrons. Nonpolar covalent bonds occur when the electrons are shared equally between the atoms involved. This type of bond is commonly found in molecular compounds, diatomic molecules, and hydrocarbons. Let’s explore some examples of nonpolar covalent bonds and their properties.
Nitrogen (N2)
Nitrogen gas, represented by the formula N2, is a diatomic molecule composed of two nitrogen atoms. In this molecule, the two nitrogen atoms are bonded together by a nonpolar covalent bond. The electronegativity of nitrogen is the same for both atoms, resulting in equal sharing of electrons. As a result, nitrogen gas is a nonpolar molecule.
Dinitrogen Tetroxide (N2O4)
Dinitrogen tetroxide, with the chemical formula N2O4, is a compound composed of two nitrogen atoms and four oxygen atoms. The nitrogen atoms in N2O4 are bonded together by a nonpolar covalent bond, while the oxygen atoms are bonded to the nitrogen atoms by polar covalent bonds. This compound is often used as an oxidizer in rocket propellants.
Dinitrogen Difluoride (N2F2)
Dinitrogen difluoride, represented by the formula N2F2, is a compound composed of two nitrogen atoms and two fluorine atoms. The nitrogen atoms in N2F2 are bonded together by a nonpolar covalent bond, while the nitrogen and fluorine atoms are bonded by polar covalent bonds. This compound is a powerful oxidizing agent and is used in various chemical reactions.
Nitrate Ion (NO3-)
The nitrate ion, with the chemical formula NO3-, is an anion composed of one nitrogen atom and three oxygen atoms. The nitrogen atom in the nitrate ion is bonded to the three oxygen atoms by polar covalent bonds. However, the overall molecule is nonpolar due to its trigonal planar geometry, which cancels out the polarity of the individual bonds.
Boron Trifluoride (BF3)
Boron trifluoride, represented by the formula BF3, is a compound composed of one boron atom and three fluorine atoms. The boron atom in BF3 is bonded to the three fluorine atoms by polar covalent bonds. However, the molecule is nonpolar due to its trigonal planar geometry, which results in the cancellation of the individual bond polarities.
Carbon Dioxide (CO2)
Carbon dioxide, with the chemical formula CO2, is a compound composed of one carbon atom and two oxygen atoms. The carbon atom in CO2 is bonded to the two oxygen atoms by polar covalent bonds. However, the molecule is nonpolar due to its linear geometry, which cancels out the polarity of the individual bonds. Carbon dioxide is a greenhouse gas and plays a crucial role in the Earth’s climate.
Methane (CH4)
Methane, represented by the formula CH4, is a hydrocarbon composed of one carbon atom and four hydrogen atoms. The carbon atom in methane is bonded to the four hydrogen atoms by nonpolar covalent bonds. The electronegativity of carbon and hydrogen is similar, resulting in equal sharing of electrons and a nonpolar molecule. Methane is the primary component of natural gas and is widely used as a fuel.
Benzene (C6H6)
Benzene, with the chemical formula C6H6, is an aromatic hydrocarbon composed of six carbon atoms and six hydrogen atoms. The carbon atoms in benzene are bonded to each other by nonpolar covalent bonds, while the carbon and hydrogen atoms are bonded by nonpolar covalent bonds as well. This compound has a unique hexagonal ring structure and is widely used in the production of various chemicals and plastics.
In conclusion, nonpolar covalent bonds occur when electrons are shared equally between atoms. Examples of nonpolar covalent bonds include nitrogen gas, dinitrogen tetroxide, dinitrogen difluoride, the nitrate ion, boron trifluoride, carbon dioxide, methane, and benzene. Understanding these examples helps us comprehend the diverse nature of chemical bonding and its impact on the properties of different compounds.
Nonpolar Covalent Bond Definition Chemistry Quizlet
A nonpolar covalent bond is a type of chemical bond that occurs when two atoms share electrons equally. In this type of bond, the electronegativity difference between the two atoms is minimal, resulting in a balanced distribution of electrons. This balanced sharing of electrons leads to the formation of nonpolar molecules.
Nonpolar covalent bonds are commonly found in molecular compounds, particularly diatomic molecules and hydrocarbons. These bonds play a crucial role in determining the physical and chemical properties of substances. Let’s explore some examples of nonpolar covalent bonds and their significance.
Examples of Nonpolar Covalent Bonds
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Carbon Dioxide (CO2): Carbon dioxide is a well-known example of a nonpolar molecule. It consists of one carbon atom bonded to two oxygen atoms through double bonds. The electronegativity of carbon and oxygen is similar, resulting in equal sharing of electrons and a nonpolar covalent bond.
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Methane (CH4): Methane, the primary component of natural gas, is another example of a nonpolar molecule. It consists of one carbon atom bonded to four hydrogen atoms. The carbon-hydrogen bonds in methane are nonpolar covalent bonds due to the similar electronegativity of carbon and hydrogen.
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Nitrogen Gas (N2): Nitrogen gas, which makes up approximately 78% of Earth’s atmosphere, is composed of two nitrogen atoms bonded together by a triple bond. The electronegativity of nitrogen is the same, resulting in a nonpolar covalent bond.
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Oxygen Gas (O2): Oxygen gas, essential for respiration, consists of two oxygen atoms bonded together by a double bond. The electronegativity of oxygen is similar, leading to a nonpolar covalent bond.
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Hydrogen Gas (H2): Hydrogen gas, the lightest and most abundant element in the universe, is composed of two hydrogen atoms bonded together by a single bond. Since hydrogen has the same electronegativity, the bond formed is nonpolar covalent.
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Water (H2O): Although water is a polar molecule, it contains nonpolar covalent bonds. The oxygen atom in water is more electronegative than the hydrogen atoms, resulting in an unequal sharing of electrons and a polar molecule overall. However, the individual oxygen-hydrogen bonds are nonpolar covalent bonds.
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Carbon Tetrachloride (CCl4): Carbon tetrachloride is a nonpolar compound used as a solvent and fire extinguisher. It consists of one carbon atom bonded to four chlorine atoms. The electronegativity of carbon and chlorine is similar, leading to nonpolar covalent bonds.
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Tetrafluoromethane (CF4): Tetrafluoromethane, also known as carbon tetrafluoride, is a nonpolar gas used in various industrial applications. It consists of one carbon atom bonded to four fluorine atoms. The electronegativity of carbon and fluorine is similar, resulting in nonpolar covalent bonds.
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Ethane (C2H6): Ethane is a hydrocarbon consisting of two carbon atoms bonded to six hydrogen atoms. The carbon-carbon bond in ethane is nonpolar covalent, while the carbon-hydrogen bonds are also nonpolar covalent due to similar electronegativities.
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Ethene (C2H4): Ethene, also known as ethylene, is an important industrial chemical used in the production of plastics. It consists of two carbon atoms bonded together by a double bond and four hydrogen atoms. The carbon-carbon bond in ethene is nonpolar covalent.
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Ethyne (C2H2): Ethyne, commonly known as acetylene, is a hydrocarbon used in welding and cutting torches. It consists of two carbon atoms bonded together by a triple bond and two hydrogen atoms. The carbon-carbon bond in ethyne is nonpolar covalent.
In summary, nonpolar covalent bonds occur when two atoms share electrons equally due to similar electronegativities. These bonds are found in various molecular compounds, including diatomic molecules, hydrocarbons, and other nonpolar molecules. Understanding nonpolar covalent bonds is essential for comprehending the behavior and properties of these substances.
Nonpolar Covalent Bonding Examples
Covalent bonding is a type of chemical bonding where atoms share electrons to form molecules. In nonpolar covalent bonds, the electrons are shared equally between the atoms involved. This equal sharing of electrons leads to the formation of nonpolar molecules. Let’s explore some examples of nonpolar covalent bonds and the molecules they create.
Nitrogen (N2)
Nitrogen gas (N2) is a diatomic molecule composed of two nitrogen atoms. In this molecule, the two nitrogen atoms are bonded together by a nonpolar covalent bond. Each nitrogen atom has five valence electrons, and they share three electrons with each other to achieve a stable octet configuration. This equal sharing of electrons results in a nonpolar molecule.
Dinitrogen Tetroxide (N2O4)
Dinitrogen tetroxide (N2O4) is a molecular compound composed of two nitrogen atoms and four oxygen atoms. The nitrogen atoms are bonded to each other by a nonpolar covalent bond, while the oxygen atoms are bonded to the nitrogen atoms by polar covalent bonds. The nonpolar covalent bond between the nitrogen atoms is due to the equal sharing of electrons.
Dinitrogen Difluoride (N2F2)
Dinitrogen difluoride (N2F2) is another example of a molecule with a nonpolar covalent bond. It consists of two nitrogen atoms bonded to each other and two fluorine atoms bonded to the nitrogen atoms. The nonpolar covalent bond between the nitrogen atoms is a result of the equal sharing of electrons.
Nitrate Ion (NO3-)
The nitrate ion (NO3-) is a polyatomic ion consisting of one nitrogen atom and three oxygen atoms. The nitrogen atom is bonded to the three oxygen atoms by polar covalent bonds, but the overall molecule is nonpolar due to its symmetrical shape. The equal sharing of electrons in the nitrogen-oxygen bonds contributes to the nonpolar nature of the nitrate ion.
Boron Trifluoride (BF3)
Boron trifluoride (BF3) is a molecule composed of one boron atom and three fluorine atoms. The boron atom is bonded to the three fluorine atoms by nonpolar covalent bonds. The equal sharing of electrons in these bonds results in a nonpolar molecule.
Carbon Dioxide (CO2)
Carbon dioxide (CO2) is a well-known example of a nonpolar molecule. It consists of one carbon atom bonded to two oxygen atoms. The carbon-oxygen bonds in carbon dioxide are nonpolar covalent bonds due to the equal sharing of electrons. The symmetrical linear shape of the molecule also contributes to its nonpolar nature.
Methane (CH4)
Methane (CH4) is a hydrocarbon compound composed of one carbon atom bonded to four hydrogen atoms. The carbon-hydrogen bonds in methane are nonpolar covalent bonds. The equal sharing of electrons between carbon and hydrogen atoms results in a nonpolar molecule.
Benzene (C6H6)
Benzene (C6H6) is an aromatic hydrocarbon consisting of six carbon atoms and six hydrogen atoms. The carbon-carbon bonds in benzene are nonpolar covalent bonds. The equal sharing of electrons between carbon atoms contributes to the nonpolar nature of benzene.
In conclusion, nonpolar covalent bonds occur when electrons are shared equally between atoms. This equal sharing leads to the formation of nonpolar molecules. The examples discussed above, such as nitrogen gas, carbon dioxide, and methane, illustrate the concept of nonpolar covalent bonding in various molecular compounds. Understanding these examples helps us comprehend the nature of nonpolar molecules and their significance in chemistry.
Frequently Asked Questions
What is a nonpolar covalent bond?
A nonpolar covalent bond is a type of chemical bond where two atoms share electrons equally. This occurs when the electronegativity difference between the two atoms is very small or nonexistent.
What are some examples of nonpolar covalent bonds?
Some examples of nonpolar covalent bonds include the bonds in diatomic molecules such as hydrogen gas (H2), nitrogen gas (N2), and oxygen gas (O2). Other examples include hydrocarbons like methane (CH4), ethane (C2H6), and ethyne (C2H2).
How is a nonpolar covalent bond different from a polar covalent bond?
In a nonpolar covalent bond, electrons are shared equally between the two atoms involved. On the other hand, in a polar covalent bond, there is an unequal sharing of electrons due to differences in electronegativity between the atoms.
Can you provide some examples of nonpolar covalent compounds?
Certainly! Some examples of nonpolar covalent compounds include carbon dioxide (CO2), carbon tetrachloride (CCl4), tetrafluoromethane (CF4), and water (H2O).
How does electronegativity affect nonpolar covalent bonding?
Electronegativity is the measure of an atom’s ability to attract electrons towards itself in a chemical bond. In nonpolar covalent bonding, the electronegativity difference between the atoms is very small or zero, resulting in equal sharing of electrons.
What is the definition of a nonpolar covalent bond in chemistry?
In chemistry, a nonpolar covalent bond is a type of chemical bond where two atoms share electrons equally. This type of bonding occurs when the electronegativity difference between the atoms is negligible.
What are shared electrons in a nonpolar covalent bond?
Shared electrons in a nonpolar covalent bond are the electrons that are equally shared between two atoms. These electrons are involved in the formation of the bond and contribute to the stability of the molecule.
Are all nonpolar covalent molecules hydrocarbons?
No, not all nonpolar covalent molecules are hydrocarbons. While hydrocarbons like methane, ethane, and ethyne are nonpolar covalent molecules, there are other nonpolar compounds like carbon dioxide and tetrafluoromethane that are not hydrocarbons.
How can I distinguish between polar and nonpolar covalent compounds?
One way to distinguish between polar and nonpolar covalent compounds is by considering the electronegativity difference between the atoms. If the electronegativity difference is small or nonexistent, the compound is likely nonpolar. If there is a significant electronegativity difference, the compound is likely polar.
Can you provide more examples of nonpolar covalent compounds?
Certainly! In addition to hydrocarbons and diatomic molecules, other examples of nonpolar covalent compounds include ethene (C2H4), hydrogen gas (H2), and ethyne (C2H2).
