using the lewis dot structures, predict the formula for the compound formed between lithium and chlorine.
Li.
+
.
:Cl:
..
yields
Li^+
+
.. -
:Cl:
..
That's about the best I can do on this board.
no
To predict the formula for the compound formed between lithium (Li) and chlorine (Cl) using Lewis dot structures, follow these steps:
Step 1: Determine the number of valence electrons for each element.
- Lithium is in Group 1 of the periodic table, so it has 1 valence electron.
- Chlorine is in Group 17, so it has 7 valence electrons.
Step 2: Determine the number of electrons needed to achieve stability.
- Lithium needs to lose 1 electron to achieve a stable electron configuration (it wants to have the same electron configuration as helium).
- Chlorine needs to gain 1 electron to achieve a stable electron configuration (it wants to have the same electron configuration as argon).
Step 3: Construct the Lewis dot structures for each element.
- For lithium (Li), draw one dot to represent its single valence electron.
- For chlorine (Cl), draw seven dots around the element symbol, one for each valence electron.
Li: .
Cl: :Cl:
Step 4: Combine the elements to form a compound.
- Lithium can donate its single valence electron to chlorine, which needs one electron to complete its outer shell.
- By transferring the electron from lithium to chlorine, both elements can achieve a stable electron configuration.
Step 5: Write the formula for the compound.
- Since lithium donates its electron to chlorine, the compound formed is LiCl (one lithium atom and one chlorine atom).
- The formula indicates that there is one lithium ion (Li+) and one chloride ion (Cl-) in the compound.
Therefore, the formula for the compound formed between lithium and chlorine is LiCl.
To predict the formula for the compound formed between lithium and chlorine using Lewis dot structures, we first need to determine the number of valence electrons for each element.
Lithium (Li) is in group 1 of the periodic table, so it has 1 valence electron.
Chlorine (Cl) is in group 17 of the periodic table, so it has 7 valence electrons.
The Lewis dot structure for lithium would be represented as Li•, where the dot represents the valence electron. Similarly, the Lewis dot structure for chlorine would be represented as Cl•••••••.
To form a stable compound, both lithium and chlorine need to achieve a stable electron configuration. Lithium can achieve stability by losing its 1 valence electron, while chlorine can achieve stability by gaining 1 electron.
Since lithium has only 1 valence electron and chlorine needs only 1 electron to achieve stability, one lithium atom can combine with one chlorine atom to form a compound.
To represent this, we can show the transfer of an electron from lithium to chlorine, resulting in the formation of an ionic compound. The Lewis dot structure for the compound can be represented as:
Li+ • + Cl- ••••••
The transfer of the single valence electron from lithium to chlorine allows lithium to have a stable electron configuration of 2 electrons in its outermost shell (similar to helium, the noble gas in the previous period), and chlorine achieves a stable configuration of 8 electrons in its outermost shell (similar to argon, the noble gas in the same period).
Therefore, the formula for the compound formed between lithium and chlorine is LiCl (lithium chloride), where the lithium atom loses an electron to become a Li+ ion, and the chlorine atom gains an electron to become a Cl- ion.