use the periodic table above to predict the bonding interaction between sulfur and lithium. Explain what type of bond is formed, what happens to the electrons, and why this interaction happens
Unfortunately, I cannot see the periodic table you mentioned since our conversation is in text format. However, I can still provide you with the information you need.
Sulfur (S) is commonly found in column 16 of the periodic table, while lithium (Li) is found in column 1. Sulfur has six valence electrons, and lithium has one valence electron.
Based on their positions in the periodic table, sulfur tends to gain two electrons to achieve a stable electron configuration of eight (like a noble gas), while lithium tends to lose one electron to achieve a full outer shell of two electrons, also emulating the noble gas configuration.
When sulfur and lithium interact, it is likely that sulfur will tend to gain an electron from lithium. This is because sulfur is close to achieving stability by gaining two electrons, while lithium only has one valence electron to give away.
Thus, the resulting bond between sulfur and lithium is an ionic bond. An ionic bond is formed when one atom transfers electrons to another atom, resulting in the formation of charged particles called ions. In this case, sulfur becomes negatively charged and forms an ion (S2-), while lithium becomes positively charged and forms a lithium ion (Li+).
The attraction between the opposite charges of S2- and Li+ holds the two ions together, forming the ionic bond. This type of bond is typically strong and leads to the formation of a crystalline lattice structure, as seen in ionic compounds like lithium sulfide (Li2S).
In summary, the bonding interaction between sulfur and lithium results in an ionic bond. Sulfur gains an electron from lithium, forming a negatively charged sulfur ion (S2-), while lithium loses an electron and becomes a positively charged ion (Li+). This occurs because both elements aim to achieve a stable electron configuration resembling that of a noble gas.