Atoms bond with one another to create a more stable electron configuration (inert gas configuration), to complete its octet commonly known as the octet rule, which leads to the sharing of electrons in molecular compounds. The simplest unit with the fundamental chemical characteristics of a covalent compound is a molecule. As a result, covalent bond compounds are referred to as molecular compounds to distinguish them from ionic compounds. In this article, we will study Why Are Electrons Shared In Molecular Compounds?
What are Molecular Compounds?
Molecules are groups of atoms that are bonded together and have a unique, independent existence. The building blocks of molecular compounds are molecules. Molecular compounds are created between non-metals and are held together by covalent bonds, which are chemical bonds in which atoms share one or more pairs of electrons. When the atoms in a molecular compound make covalent bonds with one another in a specific arrangement, a molecule is created. The characteristics of the molecule are different from those of the atoms that make it up.
1. Why are Electrons shared in Molecular Compounds?
A covalent bond is present in molecular compounds. Covalent bonding occurs when atoms share electrons in order to achieve a more stable electron configuration, also known as the octet rule. In covalent bonds, atoms can fill their outermost electron shells and become more stable by sharing electrons with other atoms. This type of bond is present in molecular compounds, which are made up of molecules, which in turn are made up of two or more atoms held together by covalent bonds.
1 Why a Molecular
Compound has a Covalent bond and not an Ionic Bond? A molecular compound has a covalent bond because the atoms in the compound have similar electronegativities, which means that they have a similar attraction for electrons. This means that neither atom can easily take or give away electrons to the other atom, so they have to share electrons in order to fill their outermost electron shells and become more stable.
2. Characteristics of Molecular Compounds
Many characteristics of molecular compounds can be attributed to their covalent bonds.
Many characteristics of molecular compounds can be attributed to their covalent bonds.
Molecular compounds have weak intermolecular forces.
The forces holding molecules together are typically weaker than the forces holding ions together in an ionic compound, which results in molecules having lower melting and boiling temperatures than ionic compounds.
Molecular compounds have very different properties than ionic compounds because valence electrons are shared in molecular compounds, rather than being transferred between atoms as in ionic compounds.
Many molecular compounds are easily burned, particularly those that contain carbon and hydrogen.
In comparison to most ionic compounds, many molecular compounds do not dissolve in water since they are usually nonpolar.
Molecular compounds cannot conduct electricity because they lack freely moving electrons. Instead, they act as effective insulators.
Most molecular compounds have relatively low boiling temperatures because the individual molecules of covalent compounds may be separated more readily than the ions in a crystal. The fact that many of them are liquids or gases at room temperature is explained by this characteristic.
Key Takeaways
Two or more nonmetallic elements are bound together by covalent bonds, in which atoms share pairs of valence electrons, to form covalent compounds. The smallest particle of a covalent compound that retains the properties of the compound is called a molecule.
The majority of the characteristics of covalent compounds are caused by covalent bonding. Covalent compounds can be difficult to dissolve in water and have relatively low boiling temperatures. They also cannot conduct electricity.
FAQs
1. Why do atoms share electrons in molecular compounds?
Atoms share electrons in molecular compounds in order to achieve a more stable electron configuration, also known as the octet rule. By sharing electrons, atoms can fill their outermost electron shells and become more stable.
2. How does sharing electrons lead to stability in molecular compounds?
When atoms share electrons, they can fill their outermost electron shells, which is a stable inert gas configuration. This is known as the octet rule. Atoms with full outer shells have zero tendency to react with other atoms or molecules.
3. What type of bond holds atoms together in molecular compounds?
A covalent bond holds atoms together in molecular compounds. Covalent bonding occurs when atoms share electrons in order to achieve a more stable electron configuration.
4. Why do atoms in molecular compounds form covalent bonds?
Atoms in molecular compounds form covalent bonds because they have similar electronegativities, which means that they have a similar attraction for electrons. This means that neither atom can easily take or give away electrons to the other atom, so they have to share electrons in order to fill their outermost electron shells and become more stable (satisfy their octet). This type of sharing is known as a covalent bond.
5. What is the octet rule?
The octet rule states that atoms tend to react in ways that would allow them to have eight electrons in their outermost electron shell. This is considered a very stable configuration, and it is why atoms tend to share electrons in order to achieve this configuration.
Conclusion
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