homework\n22. draw the lewis dot structure for the compound ccl4\n23. draw the lewis dot structure for the…

Explanation:

Step1: Determine valence electrons

For $CCl_4$: Carbon (C) has 4 valence - electrons and each chlorine (Cl) has 7 valence - electrons. Total valence electrons = $4+(4\times7)=32$. Place C in the center and connect it to 4 Cl atoms with single bonds. Then complete the octets of Cl atoms. For $H_2S$: Sulfur (S) has 6 valence - electrons and each hydrogen (H) has 1 valence - electron. Total valence electrons = $6+(2\times1)=8$. Place S in the center, connect it to 2 H atoms with single bonds, and then add 2 lone pairs on S to complete its octet. For $CCl_4$ (repeated, same as above). For $Si_2Br_6$: Silicon (Si) has 4 valence - electrons and each bromine (Br) has 7 valence - electrons. Total valence electrons = $(2\times4)+(6\times7)=50$. Place 2 Si atoms in the center connected by a single bond, and then connect 3 Br atoms to each Si atom with single bonds. Complete the octets of all Br atoms. For $H_2O_2$: Oxygen (O) has 6 valence - electrons and each hydrogen (H) has 1 valence - electron. Total valence electrons = $(2\times6)+(2\times1)=14$. Connect the two O atoms with a single bond, connect 1 H atom to each O atom with a single bond, and then add 2 lone pairs on each O atom.

Answer:

For $CCl_4$: C is in the center with 4 single - bonds to Cl atoms and each Cl has 3 lone pairs. For $H_2S$: S is in the center with 2 single - bonds to H atoms and 2 lone pairs on S. For $Si_2Br_6$: 2 Si atoms are connected by a single bond in the center, with 3 single - bonds from each Si to Br atoms and 3 lone pairs on each Br. For $H_2O_2$: Two O atoms are connected by a single bond, with 1 H atom bonded to each O and 2 lone pairs on each O.