As a chemistry expert, I am well-versed in the intricacies of atomic bonding and the periodic table. To understand the bonding preferences of hydrogen, we must delve into the realm of atomic structure and the concept of valence electrons, which are the outermost electrons of an atom that play a crucial role in chemical bonding.

Hydrogen, being the first element in the periodic table, has a single electron in its valence shell. This single electron is what defines hydrogen's bonding behavior. According to the octet rule, which is a guideline for understanding how atoms bond to each other, atoms tend to form bonds in such a way that they have eight electrons in their valence shell, giving them the same electronic configuration as a noble gas. This is because a full valence shell is energetically favorable and stable.

However, hydrogen, with its single valence electron, does not follow the octet rule directly. Instead, it aims to achieve a stable configuration by having two electrons in its valence shell, which is known as the duet rule. This is because hydrogen is a s-block element, and its valence shell is the 1s orbital, which can hold a maximum of two electrons.

In chemical reactions, hydrogen atoms typically form one covalent bond with another atom. This is because by sharing one electron with another atom, hydrogen can complete its valence shell and achieve a stable electronic configuration. For example, when hydrogen forms a molecule with another hydrogen atom, they share a pair of electrons, resulting in a stable H2 molecule.

It's important to note that while hydrogen can form one bond to achieve stability, it can also form multiple bonds under certain conditions. For instance, in hydrides, hydrogen can form bonds with more electronegative elements, such as fluorine or oxygen, where it shares its electron with the other atom. In these cases, hydrogen can be part of a network of covalent bonds that extend across a molecule or a lattice.

Now, let's consider the reference provided, which states that "Hydrogen and chlorine can each form one covalent bond, oxygen two bonds, nitrogen three, while carbon can form four bonds." This statement is generally accurate within the context of the octet rule for elements like chlorine, oxygen, nitrogen, and carbon. However, for hydrogen, as explained, the bonding preference is to form one bond to achieve a stable configuration with two electrons in its valence shell.

In summary, hydrogen's bonding preference is to form one covalent bond to achieve a stable electronic configuration with two electrons in its valence shell. This is in line with the duet rule, which is specific to hydrogen and helium, and differs from the octet rule that applies to other elements.

read more >>

Hydrogen and chlorine can each form one covalent bond, oxygen two bonds, nitrogen three, while carbon can form four bonds.read more >>