Part B – Please use the Lewis dot structure. a) ClH b) CHN c) CH2OS d) SiH3P
The Correct Answer and Explanation is:
Here are the Lewis dot structures and explanations for each molecule:
a) ClH (Hydrogen chloride)
Lewis Structure:
rubyCopyEdit:H – Cl:
- Explanation:
Hydrogen has 1 valence electron and forms one bond. Chlorine has 7 valence electrons and needs one more to complete its octet. A single bond forms between H and Cl, with Cl keeping 6 electrons as lone pairs. This satisfies both atoms — hydrogen has 2 electrons (full shell for H), and chlorine has 8 electrons around it.
b) CHN (Assuming structure is H–C≡N)
Lewis Structure:
mathematicaCopyEditH – C ≡ N:
- Explanation:
Carbon has 4 valence electrons, hydrogen has 1, and nitrogen has 5. The most stable configuration is a linear molecule with hydrogen single-bonded to carbon and carbon triple-bonded to nitrogen. Carbon shares one pair with H and three pairs with N. Nitrogen keeps one lone pair. This arrangement satisfies the octet rule for both carbon and nitrogen, and hydrogen has its full shell of 2 electrons.
c) CH₂OS (Assuming structure is H₂C=O–S)
Lewis Structure:
mathematicaCopyEditH H
\ /
C = O
|
S:
- Explanation:
Carbon forms four bonds: two with hydrogen, one double bond with oxygen, and one single bond with sulfur. Oxygen forms a double bond with carbon and keeps two lone pairs. Sulfur forms a single bond with carbon and keeps two lone pairs (can exceed the octet). This satisfies the bonding rules for all atoms involved.
d) SiH₃P (Silicon bonded to three hydrogens and one phosphorus)
Lewis Structure:
lessCopyEdit H
|
H–Si–P:
|
H
- Explanation:
Silicon has 4 valence electrons and forms four single bonds: three with hydrogen atoms and one with phosphorus. Phosphorus has 5 valence electrons and uses one to bond with Si, keeping two lone pairs. Hydrogen atoms each form one single bond. The octet rule is satisfied for Si and P, and H has full shells.
These Lewis structures ensure each atom achieves a stable configuration using shared electron pairs and lone pairs.
