How Molecular Compounds Form
Molecular compounds are created when atoms join together by sharing electrons. This process is called covalent bonding. Atoms try to achieve a full outer shell of electrons, which makes them more stable.
Here’s how it works:
Single Bonds: When two atoms share one pair of electrons, this is known as a single bond. For example, in hydrogen gas (H₂), each hydrogen atom shares one electron with the other.
Double Bonds: Sometimes, two pairs of electrons are shared between two atoms. This is called a double bond. A good example is oxygen gas (O₂), where two oxygen atoms share two pairs of electrons.
Triple Bonds: In some cases, three pairs of electrons are shared. This is called a triple bond. For instance, in nitrogen gas (N₂), each nitrogen atom shares three electrons with the other.
Unique Features of Molecular Compounds
Molecular compounds have some special characteristics:
States of Matter: They can be gases, liquids, or solids at room temperature. For example:
Melting and Boiling Points: Generally, molecular compounds melt and boil at lower temperatures compared to ionic compounds. For instance, water boils at 100°C, while table salt (sodium chloride) boils at 1465°C.
Solubility: Many molecular compounds can dissolve in organic solvents, but they don’t always mix well with water. An example is oil, which does not mix with water but dissolves in organic solvents.
Shape and Polarity of Molecular Compounds
The shape of molecular compounds depends on the number of bonds and lone pairs of electrons around the central atom. This is explained by something called VSEPR theory (Valence Shell Electron Pair Repulsion).
In summary, the way atoms bond and form their structures gives molecular compounds their special physical and chemical traits, setting them apart from ionic substances.
How Molecular Compounds Form
Molecular compounds are created when atoms join together by sharing electrons. This process is called covalent bonding. Atoms try to achieve a full outer shell of electrons, which makes them more stable.
Here’s how it works:
Single Bonds: When two atoms share one pair of electrons, this is known as a single bond. For example, in hydrogen gas (H₂), each hydrogen atom shares one electron with the other.
Double Bonds: Sometimes, two pairs of electrons are shared between two atoms. This is called a double bond. A good example is oxygen gas (O₂), where two oxygen atoms share two pairs of electrons.
Triple Bonds: In some cases, three pairs of electrons are shared. This is called a triple bond. For instance, in nitrogen gas (N₂), each nitrogen atom shares three electrons with the other.
Unique Features of Molecular Compounds
Molecular compounds have some special characteristics:
States of Matter: They can be gases, liquids, or solids at room temperature. For example:
Melting and Boiling Points: Generally, molecular compounds melt and boil at lower temperatures compared to ionic compounds. For instance, water boils at 100°C, while table salt (sodium chloride) boils at 1465°C.
Solubility: Many molecular compounds can dissolve in organic solvents, but they don’t always mix well with water. An example is oil, which does not mix with water but dissolves in organic solvents.
Shape and Polarity of Molecular Compounds
The shape of molecular compounds depends on the number of bonds and lone pairs of electrons around the central atom. This is explained by something called VSEPR theory (Valence Shell Electron Pair Repulsion).
In summary, the way atoms bond and form their structures gives molecular compounds their special physical and chemical traits, setting them apart from ionic substances.