Which Of The Following Is The Correct Lewis Structure For Diphosphorus Tetrachloride, P 2 C L 4 P_2Cl_4 P 2 ​ C L 4 ​ ?A. Cl:           Cl           |           P=P           |           Cl           ClB. Cl           |           P-P           |

Introduction

Lewis structures are a fundamental concept in chemistry, used to represent the arrangement of electrons in a molecule. In this article, we will explore the correct Lewis structure for diphosphorus tetrachloride, $P_2Cl_4$. This compound consists of two phosphorus atoms bonded to four chlorine atoms. To determine the correct Lewis structure, we need to consider the valence electrons of each atom and the bonds between them.

Valence Electrons and Bonding

Phosphorus is a member of group 15 in the periodic table, which means it has five valence electrons. Chlorine, on the other hand, is a member of group 17, with seven valence electrons. To form a bond, atoms share one or more pairs of electrons to achieve a stable electronic configuration.

Option A: Cl:           Cl           |           P=P           |           Cl           Cl

The first option suggests a double bond between the two phosphorus atoms. However, this is unlikely because phosphorus typically forms single bonds with other atoms. Additionally, the double bond would require a significant amount of energy to form, which is not consistent with the stability of the molecule.

Option B: Cl           |           P-P           |

The second option proposes a single bond between the two phosphorus atoms. This is a more plausible arrangement, as phosphorus can form single bonds with other atoms. However, we need to consider the number of valence electrons and the bonds between the phosphorus and chlorine atoms.

Valence Electrons and Bonding in $P_2Cl_4$

To determine the correct Lewis structure, we need to calculate the total number of valence electrons in $P_2Cl_4$. Each phosphorus atom contributes five valence electrons, while each chlorine atom contributes seven. Therefore, the total number of valence electrons is:

2 (phosphorus atoms) x 5 (valence electrons) = 10 4 (chlorine atoms) x 7 (valence electrons) = 28 Total valence electrons = 10 + 28 = 38

Correct Lewis Structure

To achieve a stable electronic configuration, the phosphorus atoms need to form single bonds with the chlorine atoms. The correct Lewis structure for $P_2Cl_4$ is:

Cl           |           P-Cl           |           P-Cl           |           Cl

In this structure, each phosphorus atom forms single bonds with two chlorine atoms, while each chlorine atom forms single bonds with one phosphorus atom. This arrangement satisfies the octet rule, where each atom has a full outer energy level.

Conclusion

In conclusion, the correct Lewis structure for diphosphorus tetrachloride, $P_2Cl_4$, is Cl           |           P-Cl           |           P-Cl           |           Cl. This structure takes into account the valence electrons of each atom and the bonds between them, resulting in a stable electronic configuration.

References

• Chemistry: An Atoms First Approach by Steven S. Zumdahl
• General Chemistry: Principles and Modern Applications by Linus Pauling

Further Reading

• Lewis Structures by Chemistry LibreTexts
• Valence Electrons by Chemistry LibreTexts

Glossary

• Valence Electrons: The electrons in an atom's outermost energy level, which participate in chemical bonding.
• Lewis Structure: A representation of the arrangement of electrons in a molecule.
• Octet Rule: The principle that atoms tend to gain, lose, or share electrons to achieve a full outer energy level.
  

Q: What is the molecular formula of diphosphorus tetrachloride?

A: The molecular formula of diphosphorus tetrachloride is $P_2Cl_4$.

Q: What is the correct Lewis structure for diphosphorus tetrachloride?

A: The correct Lewis structure for diphosphorus tetrachloride is Cl           |           P-Cl       ��   |           P-Cl           |           Cl.

Q: How many valence electrons does each phosphorus atom contribute to the molecule?

A: Each phosphorus atom contributes five valence electrons to the molecule.

Q: How many valence electrons does each chlorine atom contribute to the molecule?

A: Each chlorine atom contributes seven valence electrons to the molecule.

Q: What is the total number of valence electrons in diphosphorus tetrachloride?

A: The total number of valence electrons in diphosphorus tetrachloride is 38.

Q: What type of bond is formed between the phosphorus and chlorine atoms in diphosphorus tetrachloride?

A: The type of bond formed between the phosphorus and chlorine atoms in diphosphorus tetrachloride is a single bond.

Q: Why is the double bond between the two phosphorus atoms in option A unlikely?

A: The double bond between the two phosphorus atoms in option A is unlikely because phosphorus typically forms single bonds with other atoms. Additionally, the double bond would require a significant amount of energy to form, which is not consistent with the stability of the molecule.

Q: What is the significance of the octet rule in determining the Lewis structure of diphosphorus tetrachloride?

A: The octet rule is significant in determining the Lewis structure of diphosphorus tetrachloride because it states that atoms tend to gain, lose, or share electrons to achieve a full outer energy level. In the case of diphosphorus tetrachloride, the Lewis structure is determined by the arrangement of electrons that satisfies the octet rule for each atom.

Q: What are some common applications of diphosphorus tetrachloride?

A: Diphosphorus tetrachloride is a versatile compound with various applications, including:

• Synthesis of phosphorus-containing compounds: Diphosphorus tetrachloride can be used as a starting material for the synthesis of other phosphorus-containing compounds.
• Catalysis: Diphosphorus tetrachloride can act as a catalyst in certain chemical reactions.
• Materials science: Diphosphorus tetrachloride can be used to synthesize materials with unique properties.

Q: What are some safety precautions that should be taken when handling diphosphorus tetrachloride?

A: When handling diphosphorus tetrachloride, it is essential to take the following safety precautions:

• Wear protective gear: Wear gloves, goggles, and a lab coat to prevent skin and eye contact.
• Work in a well-ventilated area: Diphosphorus tetrachloride can release toxic fumes, so it is essential to work in a well-ventilated area.
• Handle with care: Diphosphorus tetrachloride is a hazardous substance, so handle it with care and avoid spills.

Q: Where can I find more information about diphosphorus tetrachloride?

A: You can find more information about diphosphorus tetrachloride in various online resources, including:

• Chemistry LibreTexts: A free online textbook that provides detailed information about diphosphorus tetrachloride.
• PubChem: A database that provides information about the chemical properties and applications of diphosphorus tetrachloride.
• Scientific journals: You can find research articles about diphosphorus tetrachloride in scientific journals such as the Journal of the American Chemical Society and the Journal of Chemical Education.