Write the Lewis structure for each molecule or ion. MISSED THIS? Read Section 10.7; Watch KCV 10.7, IWE 10.4 a. Cl
b. N
O c. SiH
d. Cl
CO
The correct Answer and Explanation is:
Here are the Lewis structures for each molecule or ion:
a. Cl (Chlorine atom)
- Chlorine has 7 valence electrons and typically exists as Cl₂ in nature.
- The Lewis structure is simply Cl with seven dots around it, representing valence electrons.
b. NO (Nitric oxide)
- Nitrogen has 5 valence electrons, and oxygen has 6.
- The Lewis structure consists of a single bond between N and O, with an unpaired electron on N and a full octet on O.
c. SiH (Silicon monohydride)
- Silicon has 4 valence electrons, and hydrogen has 1.
- The Lewis structure is a single bond between Si and H, with three lone pairs on Si.
d. ClCO (Chlorocarbonyl radical)
- Carbon has 4 valence electrons, oxygen has 6, and chlorine has 7.
- The structure includes a single bond between C and Cl, and a double bond between C and O, with lone pairs on Cl and O.
Explanation:
Lewis structures are visual representations of molecular bonding and electron distribution. They help determine molecular shape, reactivity, and polarity.
For chlorine, it exists as Cl₂ in nature, forming a single bond between two Cl atoms to satisfy the octet rule. Nitric oxide (NO) is an unusual molecule because it has an odd number of total electrons (11), resulting in an unpaired electron, making it a radical. Silicon monohydride (SiH) is not commonly found but follows a simple valence bonding approach. Chlorocarbonyl (ClCO) includes bonding patterns similar to carbonyl compounds, with Cl contributing lone pairs affecting molecular properties.
