Final answer:
The Lewis structure for SeS2 has 4 bonds and 5 lone pairs.
Step-by-step explanation:
The Lewis structure for SeS2 consists of a central selenium (Se) atom bonded to two sulfur (S) atoms. To determine the total number of bonds and lone pairs, we need to count the number of valence electrons and distribute them accordingly. Se has 6 valence electrons, and each S has 6 valence electrons. Therefore, the total number of valence electrons in SeS2 is 6 (Se) + 6 (S) + 6 (S) = 18.
Considering that each bond requires 2 electrons, we can deduce that there are 9 bonding electrons in SeS2, which corresponds to 4.5 bonds. However, we cannot have fractional bonds, so we can say that there is a total of 4 bonds in SeS2. This leaves (18 - 8) = 10 electrons remaining.
These remaining 10 electrons form 5 lone pairs. Therefore, the Lewis structure for SeS2 has a total of 4 bonds and 5 lone pairs.