Wiktor Wise
Covalent compounds are generally poor conductors of electricity. This is because, in covalent compounds, electrons are tightly held within each molecule and cannot move freely. Even when a covalent compound is dissolved in water or melted, it does not release ions that can carry an electrical charge. This is in contrast to ionic compounds, which are good conductors of electricity when dissolved in water. The difference in conductivity between covalent and ionic compounds is a fundamental concept in understanding their distinct properties.
Characteristics and Values
| Characteristics | Values |
|---|---|
| Electrical conductivity | Poor |
| Melting and boiling points | Low |
| Physical state | Gases, liquids, or soft solids |
| Solubility in water | Variable |
| Release of ions | No |
| Free electrons | No |
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What You'll Learn
Covalent compounds are electrically neutral
The electrical neutrality of covalent compounds is related to their poor conductivity of electricity. In a solid covalent compound, the electrons are tightly bound within each molecule and cannot move freely. This is in contrast to metals, where free electrons can move and carry an electrical charge. Even when dissolved in water or melted, covalent compounds do not release ions that can carry an electrical charge. This is why substances like sugar or oil, which are covalent compounds, do not conduct electricity.
The lack of free electrons or ions in covalent compounds is the primary reason for their poor electrical conductivity. This is a fundamental distinction between ionic and covalent compounds. Ionic compounds, which are composed of electrically charged ions, are good conductors of electricity when dissolved in water. The melting of ionic compounds involves breaking ionic bonds, while the melting of covalent compounds involves disrupting the weak forces between molecules without breaking the covalent bonds.
It is important to note that not all covalent compounds are poor conductors of electricity. Some polar covalent compounds are good conductors of electricity. Additionally, the water solubility of covalent compounds varies depending on their molecular structure. However, in general, covalent compounds have lower melting and boiling points than ionic compounds due to the weaker attraction between their electrically neutral molecules. Many covalent compounds are gases or liquids at room temperature, and in their solid states, they are typically softer than ionic solids.
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They have low melting and boiling points
Covalent compounds have low melting and boiling points due to their weak intermolecular forces. They are formed when two non-metals combine and share electrons, creating a covalent bond. The strength of a covalent bond is determined by the overlap of the atomic orbitals and the sharing of the electron pair.
However, the forces between these molecules, known as intermolecular forces, are relatively weak compared to the forces within the molecules, i.e., the covalent bonds. The melting and boiling points of a substance are determined by the strength of the forces between its particles. In the case of covalent compounds, these forces are the weak intermolecular forces, not the strong covalent bonds.
When a covalent compound is heated, it is these weak intermolecular forces that are overcome to convert the substance from a solid or liquid to a gas, not the covalent bonds. This is why covalent compounds have low melting and boiling points. For example, in a sample of molecular covalent compounds like CO2, the individual molecules are held by forces such as London dispersion forces or hydrogen bonds. These are significantly weaker than the bonds within the molecules, requiring less energy to disrupt during melting or boiling.
London dispersion forces are the weakest type of intermolecular force and are present in all covalent compounds. Dipole-dipole interactions occur in polar covalent compounds, and hydrogen bonding, the strongest of the intermolecular forces, occurs in compounds containing a hydrogen atom bonded to a highly electronegative atom (nitrogen, oxygen, or fluorine). Even though hydrogen bonding is the strongest intermolecular force, it is still much weaker than a covalent bond.
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They are gases, liquids or soft solids
Covalent compounds, due to their unique structure and the nature of their bonding, often exist as gases, liquids, or soft solids. This is in contrast to ionic compounds, which tend to form hard, crystalline solids. The variety of physical states among covalent compounds can be attributed to the types of covalent bonds formed and the resulting molecular structures. Some covalent compounds have strong bonds that hold molecules tightly together, resulting in solid forms, while others have weaker intermolecular forces, leading to gaseous or liquid states. The strength of these intermolecular forces directly impacts the conductivity of these substances.
Gases, such as hydrogen chloride (HCl) or ammonia (NH3), have covalent molecules that are far apart and free to move independently. This high degree of molecular freedom means that electrons are not easily transferred between molecules, leading to poor electrical conductivity. Liquids, like water (H2O) or ethanol (C2H5OH), have molecules that are closer together and experience stronger intermolecular forces, yet they still possess a degree of molecular mobility. This results in a slightly higher ability to conduct electricity compared to gases, but it is still considered poor overall.
Soft solids, including substances like paraffin wax (a type of hydrocarbon, C_{n}H_{2n+2}), have molecules that are held together by relatively weak intermolecular forces, which allows for some degree of molecular motion. This motion can facilitate a limited transfer of electrons, resulting in poor to moderate electrical conductivity. It is important to note that while some soft solids may exhibit higher conductivity than gases or liquids, it is still significantly lower compared to ionic compounds or metals.
The conductivity of these covalent compounds is influenced by factors such as temperature and pressure, which can alter the intermolecular forces and molecular distances. For example, increasing the temperature of a soft solid may provide enough energy to overcome the weak intermolecular forces, transforming it into a liquid with increased molecular mobility and, consequently, slightly higher electrical conductivity. However, even with these changes in physical state, the fundamental characteristic of poor electrical conductivity remains due to the inherent nature of covalent bonding.
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They lack free electrons or ions
Covalent compounds are poor conductors of electricity because they lack free electrons or ions. This is due to the nature of covalent bonding, which involves the sharing of electrons between atoms to create a stable electronic configuration. In a solid covalent compound, the electrons are held tightly within each molecule and cannot move freely.
In covalent bonding, atoms with similar electronegativities (the same affinity for electrons) share electrons because neither atom preferentially attracts or repels the shared electrons. This sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration. However, these shared electrons are not free to move and carry an electrical charge.
In contrast, ionic bonding involves the transfer of electrons from one atom to another, creating oppositely charged ions. These free electrons or ions can move and carry an electrical charge, making ionic compounds good conductors of electricity.
Even when a covalent compound is dissolved in water or melted, it does not release ions that can carry an electrical charge. This is why substances like sugar or oil, which are covalent compounds, do not conduct electricity. The lack of free electrons or ions in covalent compounds is the primary reason why they are poor conductors of electricity.
It is important to note that not all covalent compounds are completely unable to conduct electricity. Some polar covalent compounds, such as water (H2O), have a partial charge separation due to the difference in electronegativity between the atoms. This can lead to a weak conductivity of electricity, but it is still much lower compared to ionic compounds.
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They do not separate into ions
Covalent compounds are poor conductors of electricity because they lack free electrons or ions. In a solid covalent compound, the electrons are held tightly within each molecule and cannot move freely. Even when dissolved in water or melted, they do not release ions that can carry an electrical charge. This is because, in covalent bonding, electrons are shared between two or more atoms. The shared electrons mostly occupy the bonding orbital between the two nuclei, and the molecules are held together by the sharing of electrons, not by charge differences.
Ionic compounds, on the other hand, are formed when two or more ions come together and are held together by charge differences. Ionic bonds are formed by the combination of positive and negative ions, which form in numerical combinations to generate a neutral (zero-charge) molecule. The ions in an ionic compound can move and carry an electrical charge through the metal.
An example of an ionic compound is common salt or NaCl. When sodium (Na) and chlorine (Cl) are combined, the sodium atom donates its valence electron to chlorine, forming positive and negative ions. These ions are then attracted to each other due to their opposite charges, forming an ionic bond.
In contrast, a covalent compound is formed when two non-metal elements share their valence electrons to achieve a stable electron configuration. For example, when hydrogen bonds with chlorine, the hydrogen atom gets the two electrons it needs to fulfil its duet, and chlorine gets the one extra electron it needs to fulfil its octet. The shared electrons between the two atoms form a covalent bond.
Since covalent compounds do not have ions, they are classified as covalent and not as ionic. If they had ions, they would be classified as ionic compounds. Therefore, the absence of ions in covalent compounds is essential to their classification and properties, including their poor conductivity of electricity.
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Frequently asked questions
No, covalent compounds are generally poor conductors of electricity. This is because they lack free electrons or ions.
In a solid covalent compound, the electrons are tightly held within each molecule and cannot move freely. Even when dissolved in water or melted, they do not release ions to carry an electrical charge.
Sugar (C12H22O11) and oil are covalent compounds and do not conduct electricity.
