Chemical compounds made up of components united by covalent bonds are known as covalent compounds or molecular compounds. Because nonmetallic elements have the same or similar electronegativity values, covalent bonds can only form between them. Here are some examples of covalent compounds, as well as some of their features.

Covalent Compounds Examples

 Because covalent compounds are made up entirely of nonmetals, they are easily identifiable. Alternatively, examine a table of electronegativity values. Covalent compounds are formed when the electronegativity values of the elements in a compound are same or comparable. Covalent bonds are formed when the electronegativity difference between the atoms is smaller than 2 on the Pauling scale. Ionic bonds arise when the electronegativity difference between the components is two or more.

Covalent Chemicals include the following

• O₂ stands for oxygen.
• Cl₂ is the chemical symbol for chlorine.
• Phosphorus trichloride (PCl₃)
• Ethanol (CH₃CH₂OH)
• O₃ stands for ozone.
• H₂ stands for hydrogen.
• H₂O stands for water.
• HCl stands for hydrogen chloride.
• CH₄ stands for methane.
• NH₄ stands for ammonia.
• CO₂ stands for carbon dioxide.
• Proteins
• Carbohydrates are the building blocks of life (sugars and starch)
• Lipids are a type of lipid (fats)
• Nucleic acids are the building blocks of life (DNA and RNA)

Hydrogen Is A Chemical Element (H₂)

The element hydrogen (H) is the most basic of all the elements. It only possesses one electron and requires another electron in order to attain the electrical configuration of the inert gas helium, which is its nearest neighbor. A hydrogen molecule will be formed when two hydrogen atoms bind together in a single bond, as shown in the diagram.

The Presence Of Oxygen (O₂)

It takes two electrons to completely fill the outermost (valence) shell of the element oxygen (O), which indicates that it has a valency of two. Thus, two oxygen atoms will unite and share their two valence electrons, forming a double bond between the two oxygen atoms.

Nitrogen Is a Gas That Exists In The Atmosphere (N₂)

With five valence electrons, nitrogen (N) needs three more valence electrons to complete its octet of valence electrons. The combination of two nitrogen atoms will occur. In order to make three covalent bonds, also known as a triple bond, each of the two molecules will share three electrons, resulting in the formation of a nitrogen molecule.

The Use Of Water (H₂O)

A water molecule is made up of two hydrogen (H) and one oxygen (O) atoms, which are bonded together. In comparison, oxygen has a valency of two electrons, whereas hydrogen only has one electron in its orbital. Consequently, each hydrogen atom will share its electron with the oxygen atom and form a covalent link with it. As a result, there will be two single bonds created in the process.

Carbon Dioxide (CO₂) 

A single carbon (C) atom is joined to two oxygen (O) atoms in carbon dioxide, forming the compound gas carbon dioxide. Carbon has a valency of four, whereas oxygen has a valency of two. As a result, each oxygen creates a double bond with the carbon by sharing two of its valence electrons with it. As a result, every C=O bond is a double bond.

Methane (CH₄)

Methane is made up of one carbon (C) atom and four hydrogen (H) atoms, which is the simplest chemical compound known. Carbon has a valency of four, whereas hydrogen has a valency of one. As a result, each hydrogen will share its single electron with the carbon and establish a single covalent connection with it. In methane, there will be a total of four covalent bonds, all of which will be single bonds, making up the molecule.

Ammonia (NH₃)

Nitrogen (N) contains five electrons in its outer orbital and requires three more electrons to complete its valence shell in order to be considered elemental. When it comes to nitrogen (N), hydrogen (H) will share its lone electron, and three hydrogen atoms are required to complete the outermost shell of nitrogen. Three single covalent bonds are formed as a result of this sharing of electrons.

Carbon Monoxide (CO) 

Covalent bonds between the carbon (C) and oxygen (O) atoms form the carbon monoxide molecule, which is represented by three covalent bonds. Carbon has a valency of four and will require four electrons to complete the outermost shell of the atoms in its atomic structure. Two electrons are required to complete the outermost shell of oxygen, which has a valency of two and requires two electrons. As a result, between the two atoms, a normal double bond will form as expected. Two electrons are required by carbon, which will be supplied by oxygen due to the presence of lone pairs in the gaseous state. This will result in the third covalent bond being a coordinate covalent bond as a result of the transformation.

Iodine Monobromide (IBr)

A substance with the chemical formula IBr, iodine monobromide is an interhalogen compound. When heated to near room temperature, it is a dark red solid that melts. Iodine bromide (IBr) is used in various types of iodometry, same as iodine monochloride is. It serves as a source of I+ for the system. In the ECW model, its Lewis acid characteristics are compared to those of ICl and I2 to determine their relative importance. It has the ability to form CT adducts with Lewis donors.

Conclusion

Except for s orbitals, atomic orbitals have specific directional characteristics that lead to different forms of covalent bonding in different elements. Sigma bonds are created by overlapping orbitals on two distinct atoms. Sigma bonds are created by orbitals from two distinct atoms overlapping. A bond is a single bond. They are caused by lateral overlap of p (or d) orbitals and are weaker than p orbital bonds. One and one bonds connect two atoms, while one and two bonds connect three atoms, forming a triple bond.

Methane (CH₄), carbon monoxide (CO), and iodine monobromide are examples of covalent compounds (IBr).