Draw the Lewis structures for the following molecules and ions:
H₂S
H₂S: S is the central atom bonded to two H atoms via single bonds. The remaining electrons form two lone pairs on S to complete its octet. Structure: H : S : H
SiCl₄
SiCl₄: Si is the central atom bonded to four Cl atoms via single bonds. The remaining electrons form three lone pairs on each Cl atom to complete their octets.
BeF₂
BeF₂: Be is the central atom bonded to two F atoms via single bonds. The remaining electrons form three lone pairs on each F atom. Structure: F—Be—F
CO₃²⁻
CO₃²⁻: C is the central atom bonded to three O atoms. To complete the octet, there is one double bond and two single bonds with O atoms, with lone pairs on the oxygens.
HCOOH
HCOOH: C is the central atom bonded to one H, double bonded to one O, and single bonded to another O which is bonded to the second H. Remaining electrons form lone pairs on the O atoms.
Explanation
Following the method from the textbook, we first count the total number of valence electrons for each molecule or ion. Next, we draw the skeletal structure with single bonds. Finally, the remaining electron pairs are distributed as lone pairs or utilized for multiple bonding, ensuring that each bonded atom gets an octet of electrons. For CO₃²⁻, the representation aligns with Table 4.1, utilizing multiple bonding to satisfy the octet rule for the central carbon atom.