QQuestionChemistry
QuestionChemistry
"For the HCl molecule:
Draw the correct Lewis structure.
Select all polar covalent bonds."
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:: Determine the total number of valence electrons in the HCl molecule.
Hydrogen (H) has 1 valence electron and Chlorine (Cl) has 7 valence electrons. Thus, the HCl molecule has a total of 1 + 7 = \boxed{8} valence electrons.
Step 2:: Draw the Lewis structure for the HCl molecule.
Step 3:
Place H at the center with Chlorine (Cl) surrounding it.
Step 4:
Distribute the 8 valence electrons around the HCl molecule as pairs, ensuring that each atom has 8 electrons around it (octet rule).
Step 5:
Since Hydrogen only needs 2 electrons to complete its octet, it will share one of its electrons with Chlorine.
Step 6:
Assign a positive charge to Hydrogen and a negative charge to Chlorine to balance the sharing of electrons. The Lewis structure of the HCl molecule is: ``` H : Cl ```
Step 7:: Identify the polar covalent bonds.
A polar covalent bond is formed when the electrons are not shared equally between the two atoms due to differences in electronegativity. In this case, Chlorine is more electronegative than Hydrogen. Therefore, the shared pair of electrons is attracted more towards the Chlorine atom. The polar covalent bond in the HCl molecule is the single bond between Hydrogen and Chlorine.
Final Answer
The correct Lewis structure for the HCl molecule is: ``` H : Cl ``` The polar covalent bond in the HCl molecule is the single bond between Hydrogen and Chlorine.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students