Carbon contains four electrons in its outer shell. Therefore, it can form four covalent bonds with other atoms or molecules.

There is no 4 bond formed between carbon because of the carbon electron orbitals. It does so by forming covalent bonds with another element, in order to complete its Octet rule.

eight valence electrons

Covalent bonds include single, double, and triple bonds and are composed of sigma and pi bonding interactions where 2, 4, or 6 electrons are shared respectively.

Covalent bonds involve the sharing of electron pairs between atoms. Electron pairs shared between atoms of equal or very similar electronegativity constitute a nonpolar covalent bond (e.g., H–H or C–H), while electrons shared between atoms of unequal electronegativity constitute a polar covalent bond (e.g., H–O).

Covalent molecular structures are compounds containing molecules with covalent bonds. Covalent network structures are compounds composed of a network structure with covalent bonds between atoms throughout the material. This is the main difference between covalent molecular and covalent network.

Properties of Covalent Molecular Compounds.

• Low melting points and boiling points.
• Low enthalpies of fusion and vaporization These properties are usually one or two orders of magnitude smaller than they are for ionic compounds.
• Soft or brittle solid forms.
• Poor electrical and thermal conductivity.

Covalent (or network) solids are extended-lattice compounds, in which each atom is covalently bonded to its nearest neighbors. Because there are no delocalized electrons, covalent solids do not conduct electricity. Covalent bonds are extremely strong, so covalent solids are very hard.

Boron, Carbon and Silicon all form covalent networks. They have high melting points because they only contain strong bonds.

Covalent Network Solids are giant covalent substances like diamond, graphite and silicon dioxide (silicon(IV) oxide).

AlN is chemical formula of aluminium nitride. it is an example of covalent solid.

Ionic substances and giant covalent substances are usually brittle . They shatter when bent or hit because many strong ionic bonds or covalent bonds break at once.

Ionic compounds are formed from strong electrostatic interactions between ions, which result in higher melting points and electrical conductivity compared to covalent compounds. Covalent compounds have bonds where electrons are shared between atoms.

Metallic compounds are not brittle because the metallic bonds are non-directional (sea of electrons allow the nuclei to move). Metals like tungsten are used in light bulbs because they can conduct electricity as solids, but ionic compounds can not.

In ionic compounds, electrons are tightly held by the ions, and the ions cannot move translationally relative to each other. This explains many properties of ionic solids. They are hard and brittle, they are not malleable or ductile (i.e. cannot be shaped without cracking/breaking), and they do not conduct electricity.

Ionic bonds are stronger than metallic bonds. This is because ionic bonds are strong electrostatic forces that are formed between the positive and negative ions.

ionic bond

Covalent bond means overlapping of two electron clouds. So, in metallic bond there is actually no overlapping between any two atoms. So,we can conclude that a covalent bond is more stronger than a metallic bond.

An ionic bond is formed when one atom donates valence electrons to another atom. A covalent bond is formed when both the atoms share pairs of valence electrons. A metallic bond is formed between a cloud of free electrons and the positively charges ions in a metal.

Covalent compounds are the ones having strong intra-molecular bonds. This is because the atoms within the covalent molecules are very tightly held together. Each molecule is indeed quite separate and the force of attraction between the individual molecules in a covalent compound tends to be weak.

There are two types of atomic bonds – ionic bonds and covalent bonds. They differ in their structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and bind the atoms in a fixed orientation. This results in a positively charged ion (cation) and negatively charged ion (anion).

Types of Covalent Bonds

• Single Covalent Bond.
• Double Covalent Bond.
• Triple Covalent Bond.

ionic bonding

Ionic bonds usually occur between metal and nonmetal ions. For example, sodium (Na), a metal, and chloride (Cl), a nonmetal, form an ionic bond to make NaCl. In a covalent bond, the atoms bond by sharing electrons. Covalent bonds occur between elements that are close together on the periodic table.

So carbon forms four single bonds with four fluorine atoms in order to complete its octet and the octet of fluorine is also fulfilled. This bond is formed due to sharing of the electrons and therefore is a covalent compound.