I am having figuring out the Lewis Dot Structure of ICl2-? Can anyone help???
I can't begin to draw it on the board because it won't accommodate spaces; however, I found one on the web. You must scroll down about 3/4 of the page but scroll down to the trigonal bipyramidal structures and it is the third or fourth one.
http://butane.chem.uiuc.edu/cyerkes/Chem102AEFa07/Lecture_Notes_102/newLecture%2014-102.htm
Of course! I can help you with that.
To determine the Lewis dot structure of ICl2-, we need to follow a few steps:
Step 1: Calculate the total number of valence electrons in the molecule/ion.
- Iodine (I) is a Group 7A element, so it has 7 valence electrons.
- Chlorine (Cl) is a Group 7A element, so it also has 7 valence electrons.
- The minus sign (-) indicates that the ion has gained one extra electron, so we need to add one more electron to the total count.
Adding these up, we have:
1(I) + 2(Cl) + 1(extra electron) = 17 valence electrons
Step 2: Determine the central atom.
- In this case, the central atom is iodine (I) because it is less electronegative compared to chlorine (Cl).
- The central atom is usually the least electronegative element in the molecule/ion.
Step 3: Connect the outer atoms to the central atom.
- Place the chlorine (Cl) atoms around the iodine (I) atom.
- Chlorine (Cl) atoms have a single bond (represented by a line) connecting them to the iodine (I) atom.
Step 4: Distribute the remaining electrons.
- Starting with the iodine (I) atom, place the remaining valence electrons around the atoms in pairs (dots).
- Continue placing electrons until you have used all the valence electrons.
- If there are any remaining electrons, add them as lone pairs on the central atom (Iodine, in this case).
Step 5: Check the octet rule.
- Make sure all the atoms (except hydrogen) have a complete octet (8 electrons) or duet (2 electrons).
- Fill octets starting from the terminal atoms (chlorine, in this case) and then the central atom (iodine).
Following these steps, the Lewis dot structure of ICl2- is:
Cl
.:
:
Cl-I-:
I hope this helps!