Question

Which of the following elements occur naturally as diatomic molecules: He, \(\mathrm{O}, \mathrm{F}, \mathrm{I}, \mathrm{Ne} ?\)

Short answer

O, F, and I form diatomic molecules.

Step-by-step solution

Define Diatomic Molecules

Diatomic molecules are molecules composed of two atoms. In nature, some elements naturally exist as molecules made of two of their atoms bonded together, such as \({\mathrm{O}}_2\), \({\mathrm{F}}_2\), and \({\mathrm{I}}_2\).

Identify Noble Gases

Helium (He) and neon (Ne) are noble gases. Noble gases typically do not form diatomic molecules because they are chemically inert, having full valence electrons.

Assess Each Element

Going through each element: - Helium (He) is a noble gas and exists as single atoms.- Oxygen (O) naturally occurs as \({\mathrm{O}}_2\) (diatomic).- Fluorine (F) naturally occurs as \({\mathrm{F}}_2\) (diatomic).- Iodine (I) naturally occurs as \({\mathrm{I}}_2\) (diatomic).- Neon (Ne) is a noble gas and exists as single atoms.

List the Diatomic Elements

From the given elements, those that occur naturally as diatomic molecules are oxygen (O), fluorine (F), and iodine (I), which form \({\mathrm{O}}_2\), \({\mathrm{F}}_2\), and \({\mathrm{I}}_2\), respectively.

Key concepts

Noble Gases

Noble gases are a group of chemical elements with similar properties in Group 18 of the periodic table. These include helium (He) and neon (Ne), among others. True to their name, noble gases are known for their incredible stability and low reactivity. This is because they have a full set of valence electrons, making their electron configuration particularly stable. - Helium has 2 valence electrons, completely filling its outer shell. - Neon has 8 valence electrons, achieving a stable octet. As a result, noble gases do not seek out other atoms to bond with, and therefore, they do not naturally form molecules, diatomic or otherwise. Instead, they exist as individual atoms. This kind of non-reactivity is what makes them "noble," much like how noble people are traditionally seen as being set apart from others.

Chemical Bonding

Chemical bonding refers to the force that holds atoms together in molecules and compounds. There are several types of chemical bonds, including ionic, covalent, and metallic bonds, with covalent bonding being one of the most important for diatomic molecules. Covalent bonding occurs when two atoms share a pair of electrons. This sharing allows each atom to attain a full valence shell, leading to increased stability. For example: - Oxygen (O) naturally pairs with another oxygen atom through covalent bonding, creating - Fluorine (F) forms a diatomic molecule similarly, bonding covalently to create Fluorine and oxygen atoms form bonds readily because they lack full outer electron shells. These atoms tend to form diatomic molecules, thereby achieving the stable electron configurations they desire.

Molecular Structure

The molecular structure refers to the arrangement of atoms in a molecule and the chemical bonds that hold these atoms together. Diatomic molecules are a simple type of molecular structure, consisting of only two atoms. - The diatomic molecules of oxygen, fluorine, and iodine— The simplistic architecture of diatomic molecules makes them unique in how they interact with the environment. Because they are only two atoms, these molecules can have straightforward interactions, such as those seen in atmospheric oxygen ( The linear arrangement ensures that each molecule maintains balance and stability. This balance is crucial for processes such as respiration, where oxygen must be efficiently transported and consumed by organisms. The structural simplicity and efficiency of diatomic molecules make them fundamental in nature and essential to understanding molecular behavior.