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 the given molecules and ions:
a. Cl (Chlorine atom) Cl is a single atom with 7 valence electrons, represented as: Cl: ●●●●●●●
b. NO (Nitric oxide) N has 5 valence electrons, and O has 6, totaling 11 valence electrons. NO contains a double bond between N and O, with an unpaired electron on N:
.. N=O .
c. SiH (Silicon monohydride) Si has 4 valence electrons, and H has 1. Since SiH is an unstable radical, its structure is:
H-Si●●●
d. ClCO (Chlorocarbonyl radical) This molecule consists of Cl, C, and O with a total of 18 valence electrons. Carbon forms a double bond with oxygen and a single bond with chlorine:
Cl-C=O●●
Explanation (300 words)
Lewis structures help visualize molecular bonding and electron distribution, following the octet rule where atoms prefer 8 valence electrons (except H, which follows the duet rule).
Chlorine (Cl) exists as a single atom with 7 valence electrons, seeking one more to complete its octet. Nitric oxide (NO) is unique, having an odd number of electrons, making it a radical. This contributes to NO’s reactivity, as radicals are highly unstable.
Silicon monohydride (SiH) is another radical, as silicon has an incomplete octet with an unpaired electron. Due to this instability, SiH typically exists in highly reactive environments.
Chlorocarbonyl (ClCO) features a carbonyl group (-CO), where carbon forms a double bond with oxygen to satisfy the octet rule. The lone electron remains on carbon, making it a radical. Such structures often appear in reactive intermediates in organic and atmospheric chemistry.
Lewis structures are fundamental in predicting chemical behavior, reactivity, and molecular properties!
