Question

For \(\mathrm{Cl}_{2}\), is the sum of the bonding electrons and the lone pair electrons (also known as nonbonding electrons) around each \(\mathrm{Cl}\) atom consistent with the Lewis model?

Short answer

Yes, the sum of the bonding electrons and the lone pair electrons around each \(\mathrm{Cl}\) atom in the \(\mathrm{Cl}_{2}\) molecule is consistent with the Lewis model. Each Cl atom is surrounded by eight electrons, fulfilling the Lewis model's octet rule.

Step-by-step solution

Identify the Lewis Structure of each Chlorine Atom

First, assess the electronic structure of a chlorine atom. Chlorine (Cl) is in the 17th group of the periodic table, so it has seven valence electrons. A Lewis structure of an individual Chlorine atom would have seven dots representing these seven valence electrons.

Construct the Lewis Structure of They \(\mathrm{Cl}_{2}\) Molecule

The molecule \(\mathrm{Cl}_{2}\) consists of two chlorine atoms. In the molecule, these two chlorine atoms share a pair of electrons to achieve stability, enforcing the octet rule. The resulting Lewis structure of \(\mathrm{Cl}_{2}\) shows each Cl atom surrounded by eight electrons – two in the bonding pair and six in lone pairs.

Understand the Relationship to the Lewis Model

Given that in the \(\mathrm{Cl}_{2}\) molecule, each Cl atom is surrounded by eight electrons (two from shared bonding and six from lone pairs), it satisfies the Lewis model's requirement for each atom.

Key concepts

Understanding Valence Electrons

Valence electrons are the outermost electrons of an atom and play a crucial role in determining the chemical behavior of an element. They are the electrons involved in forming bonds between atoms.

• For a chlorine (Cl) atom, which is in Group 17 of the periodic table, there are seven valence electrons.
• Representing these electrons in a Lewis structure, we place dots around the atomic symbol, and for chlorine, seven dots are arranged around the 'Cl'.

Knowing the number of valence electrons helps in predicting how atoms will interact and bond to form molecules.

Exploring the Octet Rule

The octet rule is a fundamental principle in chemistry, indicating that atoms tend to gain, lose, or share electrons to achieve a stable configuration similar to that of noble gases, typically having eight electrons in their valence shell.

• In the case of the chlorine molecule (\(\mathrm{Cl}_2\)), each chlorine atom shares one valence electron with another chlorine atom, allowing both to complete their octet.
• This sharing creates a bond where each atom achieves a state of having eight valence electrons, satisfying the octet rule.

This is why understanding the octet rule is essential when discussing molecule stability and electron sharing among atoms.

Bonding Electrons in Molecules

Bonding electrons are the pairs of electrons that atoms share in a bond. These electrons define the connection between two atoms, holding them together in a molecule.

• In \(\mathrm{Cl}_2\), a pair of bonding electrons is shared between the two chlorine atoms, creating a single covalent bond.
• This covalent bond is represented as a line or by a pair of dots between the two Cl atoms in a Lewis structure.

Understanding bonding electrons helps elucidate molecular structures and the strength of the connections between different atoms.

Nonbonding Electrons or Lone Pairs

Nonbonding electrons, also known as lone pairs, are the valence electrons not involved in bonding between atoms. These electrons remain on a single atom and are shown as pairs of dots in Lewis structures.

• Each chlorine atom in \(\mathrm{Cl}_2\) possesses three pairs of nonbonding electrons, maintaining the stability of the atom while not partaking in bonding.
• In Lewis structures, these lone pairs are crucial for correctly depicting the electron arrangement around atoms.

Recognizing nonbonding electrons is vital for understanding molecular shape, bond angles, and the overall geometry of molecules.