Question

Explain the formation of hydrogen, oxygen and nitrogen molecules.

Short answer

Question: Explain how hydrogen, oxygen, and nitrogen molecules are formed, including the types of bonds formed and the electron configurations of the atoms involved. Answer: Hydrogen, oxygen, and nitrogen molecules are formed through the sharing of electrons between their respective atoms, creating covalent bonds. Hydrogen atoms form a single covalent bond by sharing one electron pair, oxygen atoms form a double covalent bond by sharing two electron pairs, and nitrogen atoms form a triple covalent bond by sharing three electron pairs. This process allows the atoms to achieve stability in their electron configurations: hydrogen with a 1s^2 configuration, oxygen with a 1s^2 2s^2 2p^6 configuration, and nitrogen with a 1s^2 2s^2 2p^6 configuration.

Step-by-step solution

Understanding Atomic Structures

To form molecules, we first need to understand the atomic structure of hydrogen, oxygen, and nitrogen. Hydrogen (H) has 1 electron, Oxygen (O) has 8 electrons, and Nitrogen (N) has 7 electrons. The distribution of electrons in their respective energy levels is: - Hydrogen: 1s^1 - Oxygen: 1s^2 2s^2 2p^4 - Nitrogen: 1s^2 2s^2 2p^3

Formation of Hydrogen Molecule (H2)

Hydrogen atoms bond by sharing their single electrons to form a stable covalent bond via a process called valence bond theory. This combines their 1s orbitals and results in a stable electron configuration. The hydrogen molecule (H2) is formed as follows: H + H -> H-H : H2 molecule (sharing of the two electrons) H2 has a single covalent bond, and both hydrogen atoms have a completed valence shell.

Formation of Oxygen Molecule (O2)

Oxygen atoms form a double covalent bond, in which two pairs of electrons are shared. This is necessary because oxygen atoms need two more electrons to complete their outer shell and become stable. The oxygen molecule (O2) forms as follows: O + O -> O=O : O2 molecule (sharing of four electrons, forming a double bond) O2 has a double covalent bond, and both oxygen atoms have a completed valence shell.

Formation of Nitrogen Molecule (N2)

Nitrogen atoms form a triple covalent bond by sharing three pairs of electrons between them to achieve a stable electron configuration in their outer shell. The nitrogen molecule (N2) forms as follows: N + N -> N≡N : N2 molecule (sharing of six electrons, forming a triple bond) N2 has a triple covalent bond, and both nitrogen atoms have completed valence shells. In conclusion, hydrogen, oxygen, and nitrogen molecules are formed through the sharing of electrons between their respective atoms, creating single, double, and triple covalent bonds. This allows the atoms to achieve stability in their electron configurations.

Key concepts

Atomic Structure

The atomic structure is the foundation for understanding how molecules form.
At the center of an atom lies the nucleus, consisting of protons and neutrons. Surrounding the nucleus are energy levels where electrons orbit. These electrons are arranged in a specific pattern known as the electron configuration, which plays a crucial role in the bonding between atoms to form molecules.
For instance, hydrogen (H), with its single electron in the 1s orbital, seeks to pair up that electron to achieve a more stable arrangement. Similarly, oxygen (O) and nitrogen (N) aim to complete their outermost energy levels, which significantly influences how they bond.

Covalent Bonds

Covalent bonds are the glue that hold atoms together in a molecule. They form when two atoms share one or more pairs of electrons to achieve a full valence shell, resulting in increased stability.

• Single Covalent Bond: In a hydrogen molecule (H2), two hydrogen atoms share a pair of electrons, resulting in a single covalent bond.
• Double Covalent Bond: An oxygen molecule (O2) is formed by two oxygen atoms sharing two pairs of electrons, resulting in a double covalent bond.
• Triple Covalent Bond: For a nitrogen molecule (N2), three pairs of electrons are shared, creating a triple covalent bond.

These shared electrons mean that each atom involved in the bond achieves a fuller outer shell, akin to the noble gases, which are naturally stable due to their complete valence shells.

Valence Bond Theory

Valence Bond Theory helps us understand how atoms form covalent bonds. It suggests that electrons in an atom's valence shell can be shared with others to form a bond.
When a hydrogen atom combines with another hydrogen atom, they blend their 1s orbitals, each contributing one electron to create a bonded pair. In essence, each hydrogen atom behaves as if it has two electrons, similar to helium. Oxygen and nitrogen, with more complex outer shells, use hybrid orbitals to form double and triple bonds respectively, allowing them to reach the coveted full valence shell configuration.

Electron Configuration

Electron configuration is the arrangement of electrons around an atom's nucleus. It has a significant influence on an atom's chemical properties and its ability to bond with other atoms.
For instance, hydrogen’s configuration is 1s1, which indicates one electron in the s-orbital of the first energy level. Oxygen's electron configuration is 1s2 2s2 2p4, and for nitrogen it's 1s2 2s2 2p3. These specific configurations explain why oxygen atoms form double bonds (to fill the six spaces in the p-orbital) and nitrogen atoms form triple bonds (to fill the five spaces in the p-orbital). Understanding these details ensures a grasp on why molecules form the way they do and can predict the types of bonds that will form.